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Topic 2: Atomic Structure
For both SL and HL students
1. [1 mark]
Which quantities are different between two species represented by the notation Te52128 and I53128−?
A. The number of protons only
A. The number of protons only
B. The number of protons and electrons only
C. The number of protons and neutrons only
D. The number of protons, neutrons and electrons
2. [1 mark]
What is the relative atomic mass of a sample of chlorine containing 70 % of the 35Cl isotope and 30 % of the 37Cl isotope?
A. 35.4
A. 35.4
B. 35.5
C. 35.6
D. 35.7
3. [1 mark]
Naturally occurring gallium consists of the isotopes 71Ga and 69Ga. What is the approximate percentage abundance of 69Ga?
Mr (Ga) = 69.72.
A. 40 %
B. 50 %
C. 60 %
D. 75 %
4. [1 mark]
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
5. [1 mark]
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
6. [1 mark]
Which experimental results support the theory that electrons exist in discrete energy levels?
A. 1H NMR
B. X-ray diffraction pattern
C. Emission spectra
D. IR spectra
7. [1 mark]
What is the relative atomic mass of an element with the following mass spectrum?
A. 23
B. 24
C. 25
D. 28
8. [1 mark]
State the ground-state electron configuration for copper.
9a. [1 mark]
Consider the following reaction:
Cu2+ (aq) + Fe (s) → Fe2+ (aq) + Cu (s)
State the ground-state electron configuration for Fe2+.
9b. [1 mark]
The mass spectrum for copper is shown:
Show how a relative atomic mass of copper of 63.62 can be obtained from this mass spectrum
10a. [1 mark]
When heated in air, magnesium ribbon reacts with oxygen to form magnesium oxide.
Write a balanced equation for the reaction that occurs.
10b. [1 mark]
State the block of the periodic table in which magnesium is located.
10c. [1 mark]
Identify a metal, in the same period as magnesium, that does not form a basic oxide.
10d. [1 mark]
Most nitride ions are 14N3–.
State the number of subatomic particles in this ion.
Protons.....................................................................................
Neutrons.......................................................................................
Electrons.......................................................................................
11a. [1 mark]
Ammonia, NH3, is industrially important for the manufacture of fertilizers, explosives and plastics.
Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
12a. [2 marks]
Electrons are arranged in energy levels around the nucleus of an atom.
Explain why the first ionization energy of calcium is greater than that of potassium.
12b. [2 marks]
The diagram represents possible electron energy levels in a hydrogen atom.
All models have limitations. Suggest two limitations to this model of the electron energy levels
12c. [1 mark]
Draw an arrow, labelled X, to represent the electron transition for the ionization of a hydrogen atom in the ground state.
12d. [1 mark]
Draw an arrow, labelled Z, to represent the lowest energy electron transition in the visible spectrum.
13. [1 mark]
How many p-orbitals are occupied in a phosphorus atom?
A. 2
B. 3
C. 5
D. 6
14. [1 mark]
Which represents a p orbital?
15. [1 mark]
What is represented by “2−” in X2-ZA?
A. loss of electron
B. gain of electron
C. loss of proton
D. gain of proton
16. [1 mark]
How are emission spectra formed?
A. Photons are absorbed when promoted electrons return to a lower energy level.
B. Photons are absorbed when electrons are promoted to a higher energy level.
C. Photons are emitted when electrons are promoted to a higher energy level.
D. Photons are emitted when promoted electrons return to a lower energy level.
17a. [2 marks]
Fast moving helium nuclei (4He2+) were fired at a thin piece of gold foil with most passing undeflected but a few deviating largely from their path. The diagram illustrates this historic experiment.
Suggest what can be concluded about the gold atom from this experiment.
17b. [2 marks]
Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.
Sketch diagrams of 1s, 2s and 2p.
17c. [1 mark]
State the full electron configuration of the sulfide ion.
18. [2 marks]
State the number of protons, neutrons and electrons in each species.
19. [2 marks]
State the condensed electron configurations for Cr and Cr3+.
20. [1 mark]
What is the relative atomic mass, Ar, of an element with this mass spectrum?
A. 24.0
B. 24.3
C. 24.9
D. 25.0
21. [1 mark]
What is the maximum number of electrons that can occupy the 4th main energy level in an atom?
A. 8
B. 14
C. 18
D. 32
22. [1 mark]
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
23. [1 mark]
Which transition in the hydrogen atom emits visible light?
A. n = 1 to n = 2
B. n = 2 to n = 3
C. n = 2 to n = 1
D. n = 3 to n = 2
24. [1 mark]
Which statements are correct for the emission spectrum of hydrogen?
I. The lines converge at higher frequencies.
II. Electron transitions to n = 2 are responsible for lines in the visible region.
III. Lines are produced when electrons move from lower to higher energy levels.
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
25. [1 mark]
Which statement about 56Fe3+ and 54Fe2+ is correct?
A. Both have the same numbers of protons and electrons.
B. Both have the same number of protons.
C. Both have the same number of neutrons.
D. Both have the same numbers of protons and neutrons.
26. [1 mark]
What is the number of protons and the number of neutrons in 131I?
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