IB Chemistry SL - 2024 - Questionbank
2.1 - The Nuclear Atom
Atomic Structure, Subatomic Particles, Isotopes, Atomic Number, Mass Number, Mass Spectra Analysis
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Question 1
The atom of an element Q has an atomic number of 27 and a mass number of 60. Which of the following statements is true about the subatomic particles of the atom of element Q?
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I. Atom of element Q has 27 electrons and 60 protons II. Atom of element Q has 27 protons and 27 electrons III. Atom of element Q has 27 electrons and 60 neutrons IV. Atom of element Q has 27 protons and 33 neutrons
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A. I and IV only
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B.II and IV only
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C.II and III only
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D.I and III only
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Question 2
Which of the following is most likely to be the diameter of a carbon nucleus, if the diameter of a particular carbon atom is measured as 140 pm?
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A. 12 amu
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B. 0.0012 mm
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C. 0.001 nm
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D. 0.005 pm
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Question 3
In Rutherford’s gold foil experiment, some alpha particles bounced back towards the source. Which of the following statements best explains this result?
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A. The atom consists mainly of empty space.
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B. The atom has a positively charged center.
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C. The atom consists of negative particles around the center.
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D. The atom has a neutrally charged core.
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Question 4
Which of the following statements is not true?
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I. Electrons have greater mass than protons and neutrons II. Protons and neutrons are in the nucleus III. Protons and electrons are charged subatomic particles IV. Electrons are located outside the nucleus
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A.I and III only
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B.II and IV only
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C.II only
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D.I only
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Question 5
The nuclear symbol for an isotope of iodine is . Which of the following is correct?
Atomic Number | Mass Number | Number of protons | Number of neutrons | Number of electrons | |
---|---|---|---|---|---|
A. | 53 | 125 | 53 | 72 | 53 |
B. | 53 | 125 | 72 | 53 | 53 |
C. | 125 | 53 | 53 | 72 | 72 |
D. | 125 | 53 | 53 | 53 | 72 |
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Question 6
A mass spectrometer was used to determine that the relative ratio by mass of N:O
in a molecule containing nitrogen and oxygen is 7:16. What is the most likely molecule?
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A.
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B.
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C.
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D.
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Question 7
Which of the following is not a physical property of an isotope of an element with fewer neutrons in its atom?
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A. Lower mass
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B. Faster rate of diffusion
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C. Higher density
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D. Lower melting and boiling points
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Question 8
The isotopes of carbon and :
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I. have the same atomic number II. have the same physical properties III. have the same chemical properties
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A.I and III only
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B.I and II only
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C.II and III only
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D.I, II and III
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Question 9
How many electrons are there in ?
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A. 17
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B. 18
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C. 35
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D. 36
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Question 10
The following table shows the number of subatomic particles present in five species.
Species | Number of protons | Number of neutrons | Number of electrons |
---|---|---|---|
A | 8 | 8 | 8 |
B | 8 | 8 | 10 |
C | 9 | 10 | 8 |
D | 10 | 10 | 10 |
E | 10 | 12 | 10 |
Which two species are isotopes of the same element?
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A.A and B
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B.B and C
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C.C and D
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D.D and E
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Question 11
The following table shows the number of subatomic particles present in five species.
Species | Number of protons | Number of neutrons | Number of electrons |
---|---|---|---|
A | 8 | 8 | 8 |
B | 8 | 8 | 10 |
C | 9 | 10 | 8 |
D | 10 | 10 | 10 |
E | 10 | 12 | 10 |
Which species are ions?
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A.A and B
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B.B and C
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C.C and D
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D.D and E
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Question 12
Which of the following statements is incorrect?
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A.All ions contain electrons
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B.A few alpha particles deflected at large angles in Rutherford's Gold Foil experiment
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C.A mass spectrometer can tell us the number of isotopes an element has
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D.An atom can have more neutrons than protons
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Question 13
[Maximum mark: 5]
The atom of element X has a mass number of 127 and has 74 neutrons. The ion derived from X has 54 electrons.
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Calculate the number of protons of element X. [1]
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State the nuclear symbol of the ion formed (refer to the periodic table). [2]
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An isotope of X has a mass number of 132. Determine the number of neutrons in its atom. [2]
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Question 14
The following is a hydrogen energy level diagram.
How many different emission lines are possible?
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A.1
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B.5
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C.15
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D.30
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Question 15
[Maximum mark: 8]
Deuterium is an isotope of hydrogen that contains one proton, one neutron, and one electron.
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Complete the following table. [2]
Protons Neutrons Electrons Relative charge Relative mass ~ Location -
Using the following data, calculate the relative atomic mass of hydrogen correct to five decimal places, showing your work. [2]
Isotope Relative abundance Hydrogen-1 99.98% Deuterium 0.012% Hydrogen-3 0.008%
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Describe the emission spectrum of the hydrogen atom. [2]
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Outline the difference between a continuous spectrum and a line spectrum. [1]
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Suggest how your answer to (b)(i) shows that energy levels are quantized. [1]
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Question 16
[Maximum mark: 9]
Cobalt-60 is a radioactive isotope of the element cobalt that is used to treat thyroid cancer.
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State the full electron configuration of cobalt and chromium. [2]
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Explain what is special about the electron configuration of chromium. [1]
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State the atomic symbol notation for the cobalt-60 isotope. [1]
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One atom of cobalt-60 undergoes beta decay, releasing an electron and energy with a frequency of to form nickel-60.
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Using section 1 of the data booklet, calculate the wavelength of energy released from beta decay. [1]
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Using section 3 (Section 5- 2025 Syllabus) of the data booklet and your answer to (b) (i), deduce the type of electromagnetic radiation emitted. [1]
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Define orbital. [1]
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Sketch the shapes of an s-orbital and a p-orbital. [2]
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Question 17
[Maximum mark: 5]
Complete the following table:
Nuclear Symbol | Number of protons | Number of neutrons | Number of electrons |
---|---|---|---|
62 | |||
81 | 120 | ||
26 | |||
46 | |||
16 | 16 | 18 |
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Question 18
[Maximum mark: 7]
and are the two most abundant isotopes of copper.
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Define isotope. [1]
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Determine the correct numbers of subatomic particles to complete the following table. [1]
Copper-63 Copper-65 Number of protons Number of electrons Number of neutrons -
Calculate the relative abundances of and using section 6 (Section 7- 2025 Syllabus) of the data booklet. [3]
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Complete the orbital diagram for the valence electrons in a copper atom and a copper (II) ion. [2]
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Question 19
What is the smallest amount of energy an electron can release?
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A. 0.31
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B. 0.54
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C. 10.19
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D. 13.59
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Question 20
[Maximum mark: 5]
Lithium is a low-density alkali metal that reacts vigorously with water.
- Given the below data and referring to the periodic table, calculate the relative abundances of the isotopes of lithium. [3]
Isotope | Atomic Mass |
---|---|
6.015 | |
7.016 |
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State the definition of an isotope. [1]
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Outline the concept of relative abundance. [1]
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Question 21
[Maximum mark: 5]
Element Y has 4 stable isotopes. The table below shows the relative abundance and atomic masses of these isotopes.
Isotope | Percent abundance | Atomic mass |
---|---|---|
1 | 1.40 % | 203.97 |
2 | 24.10 % | 205.97 |
3 | 22.10 % | 206.98 |
4 | 52.40 % | 207.98 |
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Calculate the relative atomic mass of the element. [2]
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Identify the element. [1]
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The atom of the element can form an ion with a charge of 4+. Determine the number of electrons in the ion. [1]
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Determine the nuclear symbol of another corresponding ion of element Y given the numbers of subatomic particles: electrons = 80; neutrons = 122. [1]
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Question 22
What is the relative atomic mass, , of an unknown element found in a meteorite with the isotopic abundance shown below?
Isoptope | Abundance% |
---|---|
80.0 | |
1.00 | |
19.0 |
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A. 39.00
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B. 40.00
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C. 39.39
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D. 40.50
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