DP Chemistry (first assessment 2025)

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Structure 2. Models of bonding and structure » Structure 2.1—The ionic model

Structure 2.1—The ionic model

Description

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Directly related questions

20N.2.SL.TZ0.3a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.3a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.3a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.3a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.3a:
Outline the two distinct phases of this composite.
20N.2.SL.TZ0.a:
Outline the two distinct phases of this composite.

Sub sections and their related questions

Structure 2.1.1—When metal atoms lose electrons, they form positive ions called cations. When non-metal atoms gain electrons, they form negative ions called anions. Predict the charge of an ion from the electron configuration of the atom.

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.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
21M.2.SL.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.TZ1.1c(i): Describe the bonding in this type of solid.
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.
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.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
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.g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
21M.2.SL.TZ2.a(ii): Explain the decrease in radius from Na to Na+.
21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
21M.2.SL.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.d(i): Describe the bonding in this type of solid.
21M.2.SL.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.TZ1.1c(i): Describe the bonding in this type of solid.
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(i): Describe the bonding in this type of solid.
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.

[N/A]

None

Structure 2.1.2—The ionic bond is formed by electrostatic attractions between oppositely charged ions. Deduce the formula and name of an ionic compound from its component ions, including polyatomic ions. Binary ionic compounds are named with the cation first, followed by the anion. The anion adopts the suffix “ide”. Interconvert names and formulas of binary ionic compounds.

22M.1A.SL.TZ1.9: A compound consists of the ions Ca2+ and PO43–. What are the name and formula of the compound?
19M.2.SL.TZ2.5b(iii):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
21N.1A.SL.TZ0.11: Which compound contains both ionic and covalent bonds? A. CH3COONa B. CH3COOH C. K2O D. ...
19M.2.SL.TZ2.5d(i):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
21M.1A.HL.TZ2.11:
What is the formula of the compound formed from Ca²⁺ and PO₄³⁻?

A. CaPO₄

B. Ca₃(PO₄)₂

C. Ca₂(PO₄)₃

D. Ca(PO₄)₂
21M.2.SL.TZ1.1d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
21M.2.SL.TZ1.1c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
20N.1A.SL.TZ0.9:
Which formula is correct?

A.   ${NH}_{4} {PO}_{4}$

B.   ${({NH}_{4})}_{2} {PO}_{4}$

C.   ${({NH}_{4})}_{3} {PO}_{4}$

D.   ${({NH}_{4})}_{3} {({PO}_{4})}_{2}$
22M.1A.SL.TZ2.10: What is the type of bonding in a compound that has high boiling and melting points, poor...
21N.1A.SL.TZ0.20: Which ions are present in an aqueous solution of Na2CO3? I. HCO3−II. OH−III. CO32− A. I and...
22M.1A.SL.TZ1.9: A compound consists of the ions Ca2+ and PO43–. What are the name and formula of the compound?
19M.2.SL.TZ2.5b(iii):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
19M.2.SL.TZ2.b(iii):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
21N.1A.SL.TZ0.11: Which compound contains both ionic and covalent bonds? A. CH3COONa B. CH3COOH C. K2O D. ...
19M.2.SL.TZ2.5d(i):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
19M.2.SL.TZ2.d(i):
Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:
21M.1A.HL.TZ2.11:
What is the formula of the compound formed from Ca²⁺ and PO₄³⁻?

A. CaPO₄

B. Ca₃(PO₄)₂

C. Ca₂(PO₄)₃

D. Ca(PO₄)₂
21M.2.SL.TZ1.1d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
21M.2.SL.TZ1.d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
21M.2.SL.TZ1.1c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
21M.2.SL.TZ1.c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
20N.1A.SL.TZ0.9:
Which formula is correct?

A.   ${NH}_{4} {PO}_{4}$

B.   ${({NH}_{4})}_{2} {PO}_{4}$

C.   ${({NH}_{4})}_{3} {PO}_{4}$

D.   ${({NH}_{4})}_{3} {({PO}_{4})}_{2}$
22M.1A.SL.TZ2.10: What is the type of bonding in a compound that has high boiling and melting points, poor...
21N.1A.SL.TZ0.20: Which ions are present in an aqueous solution of Na2CO3? I. HCO3−II. OH−III. CO32− A. I and...

[N/A]

None

Structure 2.1.3—Ionic compounds exist as three-dimensional lattice structures, represented by empirical formulas. Explain the physical properties of ionic compounds to include volatility, electrical conductivity and solubility.

19M.1A.SL.TZ2.16:
Which equation represents lattice enthalpy?

A. NaCl (g) → Na⁺ (g) + Cl⁻ (g)

B. NaCl (s) → Na⁺ (g) + Cl⁻ (g)

C. NaCl (s) → Na⁺ (aq) + Cl⁻ (aq)

D. NaCl (s) → Na⁺ (s) + Cl⁻ (s)
22M.1A.SL.TZ1.10: What is the explanation for the high melting point of sodium chloride? A. The covalent bond...
19N.1A.SL.TZ0.9: Which is correct for all solid ionic compounds? A. High volatility B. Poor electrical...
21N.1A.SL.TZ0.10: Which combination would create the strongest ionic bond?
19M.1A.SL.TZ1.11: Which describes an ionic compound?
21M.1A.SL.TZ1.11: Which substance is most likely to be ionic?
21M.1A.SL.TZ1.10:
Which compound contains both ionic and covalent bonds?

A. $MgO$

B. ${CH}_{2} {Cl}_{2}$

C. ${CH}_{3} COOH$

D. $NaOH$
21M.1A.SL.TZ1.17:
Which substance has the highest lattice enthalpy?

A.   $KCl$

B.   ${CaCl}_{2}$

C.   $KF$

D.   ${CaF}_{2}$
19M.1A.SL.TZ2.16:
Which equation represents lattice enthalpy?

A. NaCl (g) → Na⁺ (g) + Cl⁻ (g)

B. NaCl (s) → Na⁺ (g) + Cl⁻ (g)

C. NaCl (s) → Na⁺ (aq) + Cl⁻ (aq)

D. NaCl (s) → Na⁺ (s) + Cl⁻ (s)
22M.1A.SL.TZ1.10: What is the explanation for the high melting point of sodium chloride? A. The covalent bond...
19N.1A.SL.TZ0.9: Which is correct for all solid ionic compounds? A. High volatility B. Poor electrical...
21N.1A.SL.TZ0.10: Which combination would create the strongest ionic bond?
19M.1A.SL.TZ1.11: Which describes an ionic compound?
21M.1A.SL.TZ1.11: Which substance is most likely to be ionic?
21M.1A.SL.TZ1.10:
Which compound contains both ionic and covalent bonds?

A. $MgO$

B. ${CH}_{2} {Cl}_{2}$

C. ${CH}_{3} COOH$

D. $NaOH$
21M.1A.SL.TZ1.17:
Which substance has the highest lattice enthalpy?

A.   $KCl$

B.   ${CaCl}_{2}$

C.   $KF$

D.   ${CaF}_{2}$