DP Chemistry (first assessment 2025)

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Structure 1. Models of the particulate nature of matter » Structure 1.3—Electron configurations

Structure 1.3—Electron configurations

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Directly related questions

22N.1A.SL.TZ0.4:
Which is a possible empirical formula for a substance with M_r = 42?

A. CH

B. CH₂

C. C₃H₆

D. C₃H₈
22N.1A.SL.TZ0.4:
Which is a possible empirical formula for a substance with M_r = 42?

A. CH

B. CH₂

C. C₃H₆

D. C₃H₈

Sub sections and their related questions

Structure 1.3.1—Emission spectra. Emission spectra are produced by atoms emitting photons when electrons in excited states return to lower energy levels. Qualitatively describe the relationship between colour, wavelength, frequency and energy across the electromagnetic spectrum. Distinguish between a continuous and a line spectrum.

Structure 1.3.2—The line emission spectrum of the hydrogen atom. The line emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels, which converge at higher energies. Describe the emission spectrum of the hydrogen atom, including the relationships between the lines and energy transitions to the first, second and third energy levels.

Structure 1.3.3—The main energy level. The main energy level is given an integer number, n, and can hold a maximum of 2n2 electrons. Deduce the maximum number of electrons that can occupy each energy level.

Structure 1.3.4—Detailed model of the atom. A more detailed model of the atom describes the division of the main energy level into s, p, d and f sublevels of successively higher energies. Recognize the shape and orientation of an s atomic orbital and the three p atomic orbitals.

19N.1A.SL.TZ0.6: Which represents the shape of an s atomic orbital?
21M.1A.SL.TZ1.6: Which represents a p orbital?
21N.2.SL.TZ0.9b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.
21N.2.SL.TZ0.8b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.
19N.1A.SL.TZ0.6: Which represents the shape of an s atomic orbital?
21M.1A.SL.TZ1.6: Which represents a p orbital?
21N.2.SL.TZ0.9b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.
21N.2.SL.TZ0.b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.
21N.2.SL.TZ0.8b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.
21N.2.SL.TZ0.b(i):
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.

Structure 1.3.5—Each orbital has a defined energy state for a given electron configuration and chemical environment, and can hold two electrons of opposite spin. Sublevels contain a fixed number of orbitals, regions of space where there is a high probability of finding an electron. Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to deduce electron configurations for atoms and ions up to Z = 36.

22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen 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.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?

A. 2

B. 3

C. 6

D. 8
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe²⁺.
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1A.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
21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3⁺.
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
22M.2.SL.TZ1.a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen 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.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.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?

A. 2

B. 3

C. 6

D. 8
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe²⁺.
22M.2.SL.TZ2.a(i):
State the full electronic configuration of Fe²⁺.
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
19M.1A.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
21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3⁺.
21M.2.SL.TZ2.b(i):
State the condensed electron configurations for Cr and Cr3⁺.
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
21M.2.SL.TZ1.d(iii):
State the full electron configuration of the sulfide ion.
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
21M.2.SL.TZ1.c(ii):
State the full electron configuration of the sulfide ion.
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.

Structure 1.3.6—In an emission spectrum, the limit of convergence at higher frequency corresponds to ionization. Explain the trends and discontinuities in first ionization energy (IE) across a period and down a group. Calculate the value of the first IE from spectral data that gives the wavelength or frequency of the convergence limit.

22M.2.HL.TZ2.2b(ii): Draw an arrow, labelled X, to represent the electron transition for the ionization of a hydrogen...
19M.1A.HL.TZ1.5: Which element is represented by the first eight successive ionization energies on the...
19M.2.HL.TZ2.3c:
Explain why the first ionization energy of nitrogen is greater than both carbon and oxygen.

Nitrogen and carbon:

Nitrogen and oxygen:
19N.1A.HL.TZ0.5: Which shows the first ionization energies of successive elements across period 2, from left to...
21M.1A.HL.TZ2.5: The first eight successive ionization energies for an element are shown. In which group is the...
22M.2.HL.TZ2.2b(ii): Draw an arrow, labelled X, to represent the electron transition for the ionization of a hydrogen...
22M.2.HL.TZ2.b(ii): Draw an arrow, labelled X, to represent the electron transition for the ionization of a hydrogen...
19M.1A.HL.TZ1.5: Which element is represented by the first eight successive ionization energies on the...
19M.2.HL.TZ2.3c:
Explain why the first ionization energy of nitrogen is greater than both carbon and oxygen.

Nitrogen and carbon:

Nitrogen and oxygen:
19M.2.HL.TZ2.c:
Explain why the first ionization energy of nitrogen is greater than both carbon and oxygen.

Nitrogen and carbon:

Nitrogen and oxygen:
19N.1A.HL.TZ0.5: Which shows the first ionization energies of successive elements across period 2, from left to...
21M.1A.HL.TZ2.5: The first eight successive ionization energies for an element are shown. In which group is the...

Structure 1.3.7—Successive ionization energy (IE) data for an element give information about its electron configuration. Deduce the group of an element from its successive ionization data.

22M.1A.HL.TZ1.5:
The graph shows the first six ionization energies of an element.

^{[Ionization energies of the elements (data page) Available at:}https://en.wikipedia.org/wiki/Ionization_energies_of_the_
^{elements_(data_page) Text is available under the Creative Commons Attribution-ShareAlike License 3.0 (CC BY-SA}
^{3.0) https://creativecommons.org/licenses/by-sa/3.0/deed.en.]}

In which group is the element?

A. 13

B. 14

C. 15

D. 16
22M.2.HL.TZ2.5a(ii): Explain why there is a large increase from the 8th to the 9th ionization energy of iron.
21M.2.HL.TZ1.1c: Sketch the first eight successive ionisation energies of sulfur.
20N.1A.HL.TZ0.5: Which element is in group 13?
21N.1A.HL.TZ0.5: Which statement explains why the second ionization energy of aluminium is higher than the first...
22N.1A.HL.TZ0.4:
Successive ionization energies of an element, X, are shown.

What energy, in kJ mol⁻¹, is required for element X to reach its most stable oxidation state in ionic compounds?

A.  740

B.  1450

C.  2190

D.  7730
22N.1A.SL.TZ0.4:
Which is a possible empirical formula for a substance with M_r = 42?

A. CH

B. CH₂

C. C₃H₆

D. C₃H₈
22M.1A.HL.TZ1.5:
The graph shows the first six ionization energies of an element.

^{[Ionization energies of the elements (data page) Available at:}https://en.wikipedia.org/wiki/Ionization_energies_of_the_
^{elements_(data_page) Text is available under the Creative Commons Attribution-ShareAlike License 3.0 (CC BY-SA}
^{3.0) https://creativecommons.org/licenses/by-sa/3.0/deed.en.]}

In which group is the element?

A. 13

B. 14

C. 15

D. 16
22M.2.HL.TZ2.5a(ii): Explain why there is a large increase from the 8th to the 9th ionization energy of iron.
22M.2.HL.TZ2.a(ii): Explain why there is a large increase from the 8th to the 9th ionization energy of iron.
21M.2.HL.TZ1.1c: Sketch the first eight successive ionisation energies of sulfur.
21M.2.HL.TZ1.c: Sketch the first eight successive ionisation energies of sulfur.
20N.1A.HL.TZ0.5: Which element is in group 13?
21N.1A.HL.TZ0.5: Which statement explains why the second ionization energy of aluminium is higher than the first...
22N.1A.HL.TZ0.4:
Successive ionization energies of an element, X, are shown.

What energy, in kJ mol⁻¹, is required for element X to reach its most stable oxidation state in ionic compounds?

A.  740

B.  1450

C.  2190

D.  7730
22N.1A.SL.TZ0.4:
Which is a possible empirical formula for a substance with M_r = 42?

A. CH

B. CH₂

C. C₃H₆

D. C₃H₈