DP Chemistry (last assessment 2024)

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Core » Topic 3: Periodicity

Topic 3: Periodicity

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Directly related questions

20N.2.hl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.1.sl.TZ0.8:
Which oxide will dissolve in water to give the solution with the lowest pH?

A.   $P_{4} O_{10}$

B.   ${SiO}_{2}$

C.   ${Al}_{2} O_{3}$

D.   $MgO$
20N.1.sl.TZ0.8:
Which oxide will dissolve in water to give the solution with the lowest pH?

A.   $P_{4} O_{10}$

B.   ${SiO}_{2}$

C.   ${Al}_{2} O_{3}$

D.   $MgO$
20N.2.hl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.hl.TZ0.a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.3.sl.TZ0.4b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.2.sl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.sl.TZ0.a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.3.sl.TZ0.4b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.sl.TZ0.b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
17N.1.sl.TZ0.7:
Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases
II. Melting point increases
III. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
17N.2.hl.TZ0.b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
21M.1.sl.TZ1.8: Which trend is correct, going down group 1? A. Melting point increases B. Reactivity...
17N.1.sl.TZ0.7:
Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases
II. Melting point increases
III. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.2.sl.TZ0.2a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
21M.1.sl.TZ1.8: Which trend is correct, going down group 1? A. Melting point increases B. Reactivity...
17N.2.sl.TZ0.2a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
17N.2.sl.TZ0.a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
21M.1.sl.TZ2.7: Which property increases down group 1? A. atomic radius B. electronegativity C. first...
21M.1.sl.TZ2.7: Which property increases down group 1? A. atomic radius B. electronegativity C. first...
21M.2.sl.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.1.sl.TZ2.8:
Which is a d-block element?

A. Ca

B. Cf

C. C $l$

D. Co
21M.1.sl.TZ2.8:
Which is a d-block element?

A. Ca

B. Cf

C. C $l$

D. Co
17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
21M.2.sl.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
17N.2.sl.TZ0.2c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
17N.2.sl.TZ0.2c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
17N.2.sl.TZ0.c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
21M.2.hl.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ1.c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ1.d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.a(i): Explain why Si has a smaller atomic radius than Al.
18M.1.sl.TZ1.8: Which statement is correct? A. Atomic radius decreases down group 17. B. First...
21M.2.sl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.sl.TZ2.a(i): Explain why Si has a smaller atomic radius than Al.
18M.2.sl.TZ1.2e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.2.hl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.1.sl.TZ1.8: Which statement is correct? A. Atomic radius decreases down group 17. B. First...
18M.2.hl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.hl.TZ1.d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.2e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.2.sl.TZ1.e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ2.8: Which element is in the p-block? A. Pb B. Pm C. Pt D. Pu
18M.2.hl.TZ1.2f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ1.7: Which describes the oxide of sodium, Na2O?
18M.1.sl.TZ2.8: Which element is in the p-block? A. Pb B. Pm C. Pt D. Pu
18M.1.sl.TZ1.7: Which describes the oxide of sodium, Na2O?
18M.2.hl.TZ1.2f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.2.hl.TZ1.f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ2.7: Which increase across a period from left to right?
18M.2.sl.TZ2.3b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18M.1.sl.TZ2.7: Which increase across a period from left to right?
18M.2.sl.TZ2.3b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ2.3b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18M.2.sl.TZ2.3b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ2.b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ2.b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
21N.1.hl.TZ0.6: Which ion has the largest radius? A. Na+ B. Mg2+ C. P3− D. S2−
21N.1.sl.TZ0.8: Which combination describes the acid–base nature of aluminium and phosphorus oxides?
21N.1.sl.TZ0.7: Which element has the highest metallic character in Group 14? A. C B. Si C. Ge D. Sn
21N.1.hl.TZ0.6: Which ion has the largest radius? A. Na+ B. Mg2+ C. P3− D. S2−
21N.1.sl.TZ0.7: Which element has the highest metallic character in Group 14? A. C B. Si C. Ge D. Sn
18N.2.sl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
21N.2.sl.TZ0.2: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.sl.TZ0.2: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.1.sl.TZ0.8: Which combination describes the acid–base nature of aluminium and phosphorus oxides?
18N.2.hl.TZ0.4b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.sl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.4b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.hl.TZ0.b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
22M.1.sl.TZ1.7: Which gases are acidic? I. nitrogen dioxideII. carbon dioxideIII. sulfur dioxide A. I and...
18N.2.sl.TZ0.a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
22M.1.sl.TZ2.7: Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of...
18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
22M.1.sl.TZ1.7: Which gases are acidic? I. nitrogen dioxideII. carbon dioxideIII. sulfur dioxide A. I and...
18N.2.hl.TZ0.a: Explain the decrease in atomic radius from Na to Cl.
22M.1.sl.TZ2.8: Which element is found in the 4th group, 6th period of the periodic table? A. Selenium B....
22M.1.sl.TZ2.8: Which element is found in the 4th group, 6th period of the periodic table? A. Selenium B....
22M.1.sl.TZ2.7: Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of...
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?

A. [Ne] 3s² 3p²

B. [Ne] 3s² 3p⁴

C. [Ne] 3s² 3p⁶ 3d³ 4s²

D. [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵
22M.1.hl.TZ2.6: Which are the most reactive elements of the alkali metals and halogens? A. Lithium and...
22M.1.hl.TZ2.5: What is the correct order for increasing first ionization energy? A. Na < Mg < Al B. Na...
22M.1.hl.TZ2.6: Which are the most reactive elements of the alkali metals and halogens? A. Lithium and...
22M.1.hl.TZ2.5: What is the correct order for increasing first ionization energy? A. Na < Mg < Al B. Na...
22M.2.hl.TZ1.1a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?

A. [Ne] 3s² 3p²

B. [Ne] 3s² 3p⁴

C. [Ne] 3s² 3p⁶ 3d³ 4s²

D. [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵
22M.2.sl.TZ1.3f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.1a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.1a(ii): State the block of the periodic table in which magnesium is located.
22M.2.hl.TZ1.a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.hl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ1.3f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ1.f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.5d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.5d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ1.1a(ii): State the block of the periodic table in which magnesium is located.
22M.2.sl.TZ1.a(ii): State the block of the periodic table in which magnesium is located.
22M.2.hl.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ2.1d: Describe two observations that indicate the reaction of lithium with water is exothermic.
22M.2.sl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ2.2a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22M.2.sl.TZ2.1d: Describe two observations that indicate the reaction of lithium with water is exothermic.
22M.2.sl.TZ2.2a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22M.2.sl.TZ2.a:
Explain why the first ionization energy of calcium is greater than that of potassium.
19M.2.hl.TZ1.3b:
Outline why the alkali metals (group 1) have similar chemical properties.
22M.2.sl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ2.d: Describe two observations that indicate the reaction of lithium with water is exothermic.
19M.2.hl.TZ2.3b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.3b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ1.3e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ2.b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.4e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.2.hl.TZ1.3e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ1.e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ1.3b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ1.b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ2.e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.3.hl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.hl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.hl.TZ1.b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.hl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.3.hl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.3.hl.TZ1.b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.2.hl.TZ2.4e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.2.sl.TZ1.3a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.1.hl.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.hl.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.hl.TZ1.7: Which series represents atoms in order of decreasing atomic radius? A. N > C > Be >...
19M.1.hl.TZ1.7: Which series represents atoms in order of decreasing atomic radius? A. N > C > Be >...
19M.2.sl.TZ1.3a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.sl.TZ2.4a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.2.sl.TZ2.4a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.2.sl.TZ2.a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.2.sl.TZ2.3c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.3c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ1.a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.1.sl.TZ1.8: What are typical characteristics of metals?
19M.1.sl.TZ2.8: How do the following properties change down Group 17 of the periodic table?
19M.1.sl.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.sl.TZ1.8: What are typical characteristics of metals?
19M.1.sl.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.sl.TZ2.8: How do the following properties change down Group 17 of the periodic table?
22N.2.sl.TZ0.2d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
19M.1.sl.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?

A. Highest energy levels occupied

B. Energy sub-levels occupied

C. Orbitals occupied

D. Valence electrons
19M.1.sl.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?

A. Highest energy levels occupied

B. Energy sub-levels occupied

C. Orbitals occupied

D. Valence electrons
19N.1.sl.TZ0.8: Which is an f-block element? A. Sc B. Sm C. Sn D. Sr
19N.1.sl.TZ0.8: Which is an f-block element? A. Sc B. Sm C. Sn D. Sr
19N.2.sl.TZ0.6b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.2.sl.TZ0.6b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.2.sl.TZ0.b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.1.sl.TZ0.7: Which property shows a general increase from left to right across period 2, Li to F? A. Melting...
19N.1.sl.TZ0.7: Which property shows a general increase from left to right across period 2, Li to F? A. Melting...
22N.2.sl.TZ0.2d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
17N.1.sl.TZ0.8: Which oxide dissolves in water to give a solution with a pH below 7? A. MgO B. Li2O C. CaO D....
22N.1.sl.TZ0.7:
Which elements are considered to be metalloids?

I. Gallium

II. Germanium

III. Arsenic

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
22N.1.sl.TZ0.7:
Which elements are considered to be metalloids?

I. Gallium

II. Germanium

III. Arsenic

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
22N.2.sl.TZ0.d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
18N.1.sl.TZ0.7: Which oxides produce an acidic solution when added to water? I. Al2O3 and SiO2 II. P4O6...
17N.1.sl.TZ0.8: Which oxide dissolves in water to give a solution with a pH below 7? A. MgO B. Li2O C. CaO D....
18N.1.sl.TZ0.7: Which oxides produce an acidic solution when added to water? I. Al2O3 and SiO2 II. P4O6...
17N.1.hl.TZ0.7:
Which electron configuration is that of a transition metal atom in the ground state?

A. [Ne]3s²3p⁶4s¹

B. [Ar]3d⁹

C. 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

D. [Ar]4s¹3d⁵
17N.1.hl.TZ0.7:
Which electron configuration is that of a transition metal atom in the ground state?

A. [Ne]3s²3p⁶4s¹

B. [Ar]3d⁹

C. 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

D. [Ar]4s¹3d⁵
22N.1.sl.TZ0.8: Which property of elements increases down a group but decreases across a period? A. Atomic...
18N.1.sl.TZ0.8: Which species will require the least energy for the removal of one electron? A. Na+ B. ...
18N.1.sl.TZ0.8: Which species will require the least energy for the removal of one electron? A. Na+ B. ...
22N.1.sl.TZ0.8: Which property of elements increases down a group but decreases across a period? A. Atomic...
19M.1.hl.TZ2.7: How do the following properties change down Group 17 of the periodic table?
18N.2.sl.TZ0.4b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
19M.3.sl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
18N.2.sl.TZ0.4b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.sl.TZ0.b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
19M.1.hl.TZ2.7: How do the following properties change down Group 17 of the periodic table?
19M.3.sl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
20N.1.hl.TZ0.6: What is the correct trend going down groups 1 and 17? A. Melting points increase B. Boiling...
20N.1.sl.TZ0.7:
Which of the following shows a general increase across period 3 from $Na$ to $Cl$ ?

A. Ionic radius

B. Atomic radius

C. Ionization energy

D. Melting point
19M.3.sl.TZ1.b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.sl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
20N.1.sl.TZ0.7:
Which of the following shows a general increase across period 3 from $Na$ to $Cl$ ?

A. Ionic radius

B. Atomic radius

C. Ionization energy

D. Melting point
20N.1.hl.TZ0.6: What is the correct trend going down groups 1 and 17? A. Melting points increase B. Boiling...
19M.3.sl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
20N.3.hl.TZ0.4c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
19M.3.sl.TZ1.b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
21M.1.sl.TZ1.7: Which species has the same electron configuration as argon? A. Br− B. Ca2+ C. Al3+ D. Si4+
20N.3.hl.TZ0.4c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.hl.TZ0.c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
21M.1.sl.TZ1.7: Which species has the same electron configuration as argon? A. Br− B. Ca2+ C. Al3+ D. Si4+
21M.2.sl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
20N.2.sl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
21M.2.hl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.sl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.sl.TZ1.b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.hl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21N.2.hl.TZ0.2a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
20N.2.sl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
21M.2.hl.TZ1.b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
23M.1.SL.TZ1.7: What is the correct labelling of the blocks of the periodic table?
22M.2.sl.TZ1.1a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
21N.2.hl.TZ0.2a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.hl.TZ0.a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
23M.1.SL.TZ1.7: What is the correct labelling of the blocks of the periodic table?
23M.1.HL.TZ2.7: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
23M.1.SL.TZ2.8: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
22M.2.sl.TZ1.1a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
23M.2.HL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ1.a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ1.a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.1.HL.TZ2.7: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
23M.1.SL.TZ2.8: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
23M.2.HL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.HL.TZ2.a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ2.a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.

Sub sections and their related questions

3.1 Periodic table

17N.1.hl.TZ0.7:
Which electron configuration is that of a transition metal atom in the ground state?

A. [Ne]3s²3p⁶4s¹

B. [Ar]3d⁹

C. 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

D. [Ar]4s¹3d⁵
18M.1.sl.TZ2.8: Which element is in the p-block? A. Pb B. Pm C. Pt D. Pu
19M.3.hl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.1.hl.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.hl.TZ2.7: How do the following properties change down Group 17 of the periodic table?
19M.3.sl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.1.sl.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.sl.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?

A. Highest energy levels occupied

B. Energy sub-levels occupied

C. Orbitals occupied

D. Valence electrons
19N.1.sl.TZ0.8: Which is an f-block element? A. Sc B. Sm C. Sn D. Sr
20N.3.sl.TZ0.4b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.hl.TZ0.4c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
21M.1.sl.TZ1.7: Which species has the same electron configuration as argon? A. Br− B. Ca2+ C. Al3+ D. Si4+
21M.1.sl.TZ2.8:
Which is a d-block element?

A. Ca

B. Cf

C. C $l$

D. Co
21M.2.sl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.hl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
22M.1.sl.TZ2.8: Which element is found in the 4th group, 6th period of the periodic table? A. Selenium B....
22M.2.sl.TZ1.1a(ii): State the block of the periodic table in which magnesium is located.
22N.1.sl.TZ0.7:
Which elements are considered to be metalloids?

I. Gallium

II. Germanium

III. Arsenic

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
23M.2.HL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.1.SL.TZ1.7: What is the correct labelling of the blocks of the periodic table?
19M.3.hl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.hl.TZ1.b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.1.hl.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.hl.TZ2.7: How do the following properties change down Group 17 of the periodic table?
19M.3.sl.TZ1.1b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.3.sl.TZ1.b(ii):
Suggest, with a reason, whether the lanthanoids or actinoids of the f-block would have the higher density.
19M.1.sl.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1.sl.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?

A. Highest energy levels occupied

B. Energy sub-levels occupied

C. Orbitals occupied

D. Valence electrons
19N.1.sl.TZ0.8: Which is an f-block element? A. Sc B. Sm C. Sn D. Sr
20N.3.sl.TZ0.4b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.sl.TZ0.b(iv):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.hl.TZ0.4c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
20N.3.hl.TZ0.c(iii):
Suggest a gas which should be continuously passed over the molten magnesium in the electrolytic cell.
21M.1.sl.TZ1.7: Which species has the same electron configuration as argon? A. Br− B. Ca2+ C. Al3+ D. Si4+
21M.1.sl.TZ2.8:
Which is a d-block element?

A. Ca

B. Cf

C. C $l$

D. Co
21M.2.sl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.sl.TZ1.b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.hl.TZ1.1b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
21M.2.hl.TZ1.b:
Justify why sulfur is classified as a non-metal by giving two of its chemical properties.
22M.1.sl.TZ2.8: Which element is found in the 4th group, 6th period of the periodic table? A. Selenium B....
22M.2.sl.TZ1.1a(ii): State the block of the periodic table in which magnesium is located.
22M.2.sl.TZ1.a(ii): State the block of the periodic table in which magnesium is located.
22N.1.sl.TZ0.7:
Which elements are considered to be metalloids?

I. Gallium

II. Germanium

III. Arsenic

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.1.hl.TZ0.7:
Which electron configuration is that of a transition metal atom in the ground state?

A. [Ne]3s²3p⁶4s¹

B. [Ar]3d⁹

C. 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

D. [Ar]4s¹3d⁵
23M.2.HL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ1.a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.HL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.HL.TZ2.a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ1.4a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ1.a:
State the oxidation state of sulfur in copper (II) sulfate.
23M.2.SL.TZ2.4a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.2.SL.TZ2.a:
Bismuth has atomic number 83. Deduce two pieces of information about the electron configuration of bismuth from its position on the periodic table.
23M.1.SL.TZ1.7: What is the correct labelling of the blocks of the periodic table?
18M.1.sl.TZ2.8: Which element is in the p-block? A. Pb B. Pm C. Pt D. Pu

3.2 Periodic trends

17N.1.sl.TZ0.7:
Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases
II. Melting point increases
III. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.1.sl.TZ0.8: Which oxide dissolves in water to give a solution with a pH below 7? A. MgO B. Li2O C. CaO D....
17N.2.sl.TZ0.2a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.2c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
18M.2.hl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.hl.TZ1.2f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ1.7: Which describes the oxide of sodium, Na2O?
18M.1.sl.TZ1.8: Which statement is correct? A. Atomic radius decreases down group 17. B. First...
18M.2.sl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.2e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ2.7: Which increase across a period from left to right?
18M.2.sl.TZ2.3b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ2.3b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18N.1.sl.TZ0.7: Which oxides produce an acidic solution when added to water? I. Al2O3 and SiO2 II. P4O6...
18N.1.sl.TZ0.8: Which species will require the least energy for the removal of one electron? A. Na+ B. ...
18N.2.sl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.sl.TZ0.4b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.4b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
19M.2.hl.TZ1.3b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ1.3e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ2.3b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.4e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.3.hl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.hl.TZ1.7: Which series represents atoms in order of decreasing atomic radius? A. N > C > Be >...
19M.2.sl.TZ1.3a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.sl.TZ2.3c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.4a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.3.sl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.sl.TZ1.8: What are typical characteristics of metals?
19M.1.sl.TZ2.8: How do the following properties change down Group 17 of the periodic table?
19N.2.sl.TZ0.6b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.1.sl.TZ0.7: Which property shows a general increase from left to right across period 2, Li to F? A. Melting...
20N.1.sl.TZ0.7:
Which of the following shows a general increase across period 3 from $Na$ to $Cl$ ?

A. Ionic radius

B. Atomic radius

C. Ionization energy

D. Melting point
20N.1.sl.TZ0.8:
Which oxide will dissolve in water to give the solution with the lowest pH?

A.   $P_{4} O_{10}$

B.   ${SiO}_{2}$

C.   ${Al}_{2} O_{3}$

D.   $MgO$
20N.1.hl.TZ0.6: What is the correct trend going down groups 1 and 17? A. Melting points increase B. Boiling...
20N.2.sl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.hl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
21M.1.sl.TZ1.8: Which trend is correct, going down group 1? A. Melting point increases B. Reactivity...
21M.1.sl.TZ2.7: Which property increases down group 1? A. atomic radius B. electronegativity C. first...
21M.2.sl.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21N.1.sl.TZ0.7: Which element has the highest metallic character in Group 14? A. C B. Si C. Ge D. Sn
21N.1.sl.TZ0.8: Which combination describes the acid–base nature of aluminium and phosphorus oxides?
21N.1.hl.TZ0.6: Which ion has the largest radius? A. Na+ B. Mg2+ C. P3− D. S2−
21N.2.sl.TZ0.2: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.hl.TZ0.2a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
22M.1.sl.TZ1.7: Which gases are acidic? I. nitrogen dioxideII. carbon dioxideIII. sulfur dioxide A. I and...
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?

A. [Ne] 3s² 3p²

B. [Ne] 3s² 3p⁴

C. [Ne] 3s² 3p⁶ 3d³ 4s²

D. [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵
22M.1.sl.TZ2.7: Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of...
22M.1.hl.TZ2.5: What is the correct order for increasing first ionization energy? A. Na < Mg < Al B. Na...
22M.1.hl.TZ2.6: Which are the most reactive elements of the alkali metals and halogens? A. Lithium and...
22M.2.sl.TZ1.1a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ1.3f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.1a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.hl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.5d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ2.1d: Describe two observations that indicate the reaction of lithium with water is exothermic.
22M.2.sl.TZ2.2a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22N.1.sl.TZ0.8: Which property of elements increases down a group but decreases across a period? A. Atomic...
22N.2.sl.TZ0.2d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
23M.1.HL.TZ2.7: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
23M.1.SL.TZ2.8: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
19M.2.hl.TZ1.3b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ1.3e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ1.b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ1.e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ2.3b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.4e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.2.hl.TZ2.e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.3.hl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.3.hl.TZ1.b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.hl.TZ1.7: Which series represents atoms in order of decreasing atomic radius? A. N > C > Be >...
19M.2.sl.TZ1.3a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.sl.TZ1.a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.sl.TZ2.3c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.4a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.2.sl.TZ2.a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.3.sl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.3.sl.TZ1.b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.sl.TZ1.8: What are typical characteristics of metals?
19M.1.sl.TZ2.8: How do the following properties change down Group 17 of the periodic table?
19N.2.sl.TZ0.6b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.2.sl.TZ0.b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.1.sl.TZ0.7: Which property shows a general increase from left to right across period 2, Li to F? A. Melting...
20N.1.sl.TZ0.7:
Which of the following shows a general increase across period 3 from $Na$ to $Cl$ ?

A. Ionic radius

B. Atomic radius

C. Ionization energy

D. Melting point
20N.1.sl.TZ0.8:
Which oxide will dissolve in water to give the solution with the lowest pH?

A.   $P_{4} O_{10}$

B.   ${SiO}_{2}$

C.   ${Al}_{2} O_{3}$

D.   $MgO$
20N.1.hl.TZ0.6: What is the correct trend going down groups 1 and 17? A. Melting points increase B. Boiling...
20N.2.sl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.sl.TZ0.a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.hl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.hl.TZ0.a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
21M.1.sl.TZ1.8: Which trend is correct, going down group 1? A. Melting point increases B. Reactivity...
21M.1.sl.TZ2.7: Which property increases down group 1? A. atomic radius B. electronegativity C. first...
21M.2.sl.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ1.c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ1.d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.sl.TZ2.a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.a(i): Explain why Si has a smaller atomic radius than Al.
21N.1.sl.TZ0.7: Which element has the highest metallic character in Group 14? A. C B. Si C. Ge D. Sn
21N.1.sl.TZ0.8: Which combination describes the acid–base nature of aluminium and phosphorus oxides?
21N.1.hl.TZ0.6: Which ion has the largest radius? A. Na+ B. Mg2+ C. P3− D. S2−
21N.2.sl.TZ0.2: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.hl.TZ0.2a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.hl.TZ0.a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
22M.1.sl.TZ1.7: Which gases are acidic? I. nitrogen dioxideII. carbon dioxideIII. sulfur dioxide A. I and...
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?

A. [Ne] 3s² 3p²

B. [Ne] 3s² 3p⁴

C. [Ne] 3s² 3p⁶ 3d³ 4s²

D. [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵
22M.1.sl.TZ2.7: Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of...
22M.1.hl.TZ2.5: What is the correct order for increasing first ionization energy? A. Na < Mg < Al B. Na...
22M.1.hl.TZ2.6: Which are the most reactive elements of the alkali metals and halogens? A. Lithium and...
22M.2.sl.TZ1.1a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ1.a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.sl.TZ1.3f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ1.f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.1a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.hl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.hl.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.5d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ2.1d: Describe two observations that indicate the reaction of lithium with water is exothermic.
22M.2.sl.TZ2.d: Describe two observations that indicate the reaction of lithium with water is exothermic.
22M.2.sl.TZ2.2a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22M.2.sl.TZ2.a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22N.1.sl.TZ0.8: Which property of elements increases down a group but decreases across a period? A. Atomic...
22N.2.sl.TZ0.2d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
22N.2.sl.TZ0.d: State, giving a reason, whether carbon or nitrogen is the most electronegative element.
17N.1.sl.TZ0.7:
Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases
II. Melting point increases
III. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.1.sl.TZ0.8: Which oxide dissolves in water to give a solution with a pH below 7? A. MgO B. Li2O C. CaO D....
17N.2.sl.TZ0.2a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.2c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
17N.2.sl.TZ0.a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
17N.2.sl.TZ0.b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
17N.2.hl.TZ0.b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
18M.2.hl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.hl.TZ1.2f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.2.hl.TZ1.d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.hl.TZ1.f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
23M.1.HL.TZ2.7: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
23M.1.SL.TZ2.8: Which properties increase down the group 1 alkali metals? atomic radii melting point reactivity...
18M.1.sl.TZ1.7: Which describes the oxide of sodium, Na2O?
18M.1.sl.TZ1.8: Which statement is correct? A. Atomic radius decreases down group 17. B. First...
18M.2.sl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.2e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.2.sl.TZ1.d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.sl.TZ1.e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ2.7: Which increase across a period from left to right?
18M.2.sl.TZ2.3b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ2.3b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18M.2.sl.TZ2.b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
18M.2.sl.TZ2.b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18N.1.sl.TZ0.7: Which oxides produce an acidic solution when added to water? I. Al2O3 and SiO2 II. P4O6...
18N.1.sl.TZ0.8: Which species will require the least energy for the removal of one electron? A. Na+ B. ...
18N.2.sl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.sl.TZ0.4b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.sl.TZ0.a: Explain the decrease in atomic radius from Na to Cl.
18N.2.sl.TZ0.b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.4b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.2.hl.TZ0.a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.