IB Chemistry HL - 2024 - Questionbank
Topic 2 All - Atomic Structure
All Questions for Topic 2 (Atomic Structure). The Nuclear Atom, Electron Configuration
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Question 1
What is the maximum number of electrons in the subshell?
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A. 6
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B. 10
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C. 2
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D. 8
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Question 2
What is the electron configuration of this orbital diagram?
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A.
-
B.
-
C.
-
D.
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Question 3
Which of the following subshells contains the highest energy?
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A.
-
B.
-
C.
-
D.
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Question 4
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
-
D.I and III only
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Question 5
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 6
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 7
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
-
D.I only
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Question 8
What is the term for the region where there is the highest probability of finding an electron?
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A. Orbital
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B. Nucleus
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C. Orbital diagram
-
D. Orbit
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Question 9
Which of the following is the correct electron configuration of a typical sodium ion?
-
A.
-
B.
-
C.
-
D.
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Question 10
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 11
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?
-
A.
-
B.
-
C.
-
D.
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Question 12
Which of the following is the correct orbital diagram for ?
-
A. B. C. D.
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Question 13
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 14
[Maximum mark: 2]
Cobalt is an important cofactor that often inhibits enzyme activity involved in cellular respiration, such as catalase.
-
Using the complete electron configuration, determine the electron configuration of [1]
-
Draw the orbital diagram of the electrons of . [1]
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Question 15
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 16
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 17
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
-
C.C and D
-
D.D and E
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Question 18
[Maximum mark: 4]
Hydrogen exhibits two emission lines, and . has a wavelength of and has a frequency of .
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Calculate the frequency of the emission line of hydrogen. [1]
-
Calculate the wavelength of the emission line of hydrogen. [1]
-
Compare the two emission lines, and using the Data Booklet, suggest which of the emission lines is most likely to be red. [2]
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Question 19
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?
-
A.A and B
-
B.B and C
-
C.C and D
-
D.D and E
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Question 20
What will happen to the frequency of moving light particles if the wavelength is doubled, assuming the velocity is constant?
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A. The frequency will be doubled
-
B. The frequency will decrease by half
-
C. The frequency will not be affected
-
D. The frequency will increase by four
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Question 21
Which of the following statement(s) is (are) true?
- I. The emission spectra are produced from a release of energy of excited electrons
II. No two electrons in one atom have the same set of quantum numbers
III. The electrons in an orbital must have an opposite spin
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A. I only
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B. II and III only
-
C. I and II only
-
D. I, II, and III
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Question 22
Mass spectrometry uses fast-moving electrons to ionize particles and determine the mass-to-charge ratio of an unknown compound.
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Using the data booklet section 1 and 2, calculate the frequency of an electron with a wavelength of [1]
-
Calculate the wavelength of an electron with a frequency of . [1]
-
State the effect of increasing the wavelength on frequency. [1]
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Question 23
Which of the following statements is incorrect?
-
A.All ions contain electrons
-
B.A few alpha particles deflected at large angles in Rutherford's Gold Foil experiment
-
C.A mass spectrometer can tell us the number of isotopes an element has
-
D.An atom can have more neutrons than protons
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Question 24
[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.
-
Calculate the number of protons of element X. [1]
-
State the nuclear symbol of the ion formed (refer to the periodic table). [2]
-
An isotope of X has a mass number of 132. Determine the number of neutrons in its atom. [2]
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Question 25
The following is a hydrogen energy level diagram.
How many different emission lines are possible?
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A.1
-
B.5
-
C.15
-
D.30
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Question 26
[Maximum mark: 8]
Deuterium is an isotope of hydrogen that contains one proton, one neutron, and one electron.
-
-
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%
-
-
-
Describe the emission spectrum of the hydrogen atom. [2]
-
Outline the difference between a continuous spectrum and a line spectrum. [1]
-
Suggest how your answer to (b)(i) shows that energy levels are quantized. [1]
-
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Question 27
[Maximum mark: 9]
Cobalt-60 is a radioactive isotope of the element cobalt that is used to treat thyroid cancer.
-
-
State the full electron configuration of cobalt and chromium. [2]
-
Explain what is special about the electron configuration of chromium. [1]
-
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.
-
-
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]
-
-
-
Define orbital. [1]
-
Sketch the shapes of an s-orbital and a p-orbital. [2]
-
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Question 28
[Maximum mark: 5]
Each element contains a different arrangement of electrons, and these electron configurations can also be represented using orbital diagrams. Determine the identity of each element described below.
-
[1]
-
[1]
-
In Period with valence electrons of [1]
-
[1]
-
An ion with +1 charge, with valence electrons of:
[1]
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Question 29
[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 30
Which of the following pairs of terms describe the shape of an s orbital and the relative energy of a d orbital?
A. | Spherical | Low |
B. | Dumbbell-shape | High |
C. | Spherical | High |
D. | Dumbbell-shape | Low |
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Question 31
Which atoms' orbital diagram does this figure represent?
-
A.
-
B.
-
C.
-
D.
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Question 32
[Maximum mark: 7]
and are the two most abundant isotopes of copper.
-
-
Define isotope. [1]
-
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]
-
-
Complete the orbital diagram for the valence electrons in a copper atom and a copper (II) ion. [2]
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Question 33
[Maximum mark: 3]
is a transition metal commonly used in wires.
-
Determine the complete electron configuration of . [1]
-
State the condensed electron configuration of [1]
-
Determine whether the electron configuration of follows the usual rules of electron configuration. [1]
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Question 34
[Maximum mark: 4]
John is sitting on a beach on a warm summer evening watching the reddish sky () while his brother, Eric, is playing with his laser beam with a frequency of .
-
Calculate the frequency of the radiation from the red sky. [1]
-
Calculate the wavelength of the laser beam of Eric. [1]
-
Compare the wavelength of the laser beam with the wavelength of the radiation of the red sky. [1]
-
Deduce the colour of the laser beam of Eric. [1]
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Question 35
What is the smallest amount of energy an electron can release?
-
A. 0.31
-
B. 0.54
-
C. 10.19
-
D. 13.59
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Question 36
[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 |
-
State the definition of an isotope. [1]
-
Outline the concept of relative abundance. [1]
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Question 37
[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 |
-
Calculate the relative atomic mass of the element. [2]
-
Identify the element. [1]
-
The atom of the element can form an ion with a charge of 4+. Determine the number of electrons in the ion. [1]
-
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 38
[Maximum mark: 10]
Copper(II) chloride can exist as an anhydrous solid or hydrate.
-
A sample of copper(II) chloride hydrate was heated on a watch glass until the blue solid changed completely to brown, and the following data was recorded:
Mass of watch glass () Mass of copper(II) chloride hydrate () Mass of anhydrous copper(II) chloride + watch glass (1st heating, 5 min) Mass of anhydrous copper(II) chloride + watch glass (2nd heating, 5 min) Mass of anhydrous copper(II) chloride + watch glass (3rd heating, 2 min) Suggest a reason why the sample was heated for a second 5 minute increment showing a mass change. [1]
-
Calculate the mass of anhydrous copper(II) chloride. Do not include the calculations of uncertainties in your work. [1]
-
Calculate the mass of water in the hydrated copper(II) chloride sample. Do not include the calculations of uncertainties in your work. [1]
-
Calculate the percent uncertainty on the mass of water in the copper(II) chloride sample. [2]
-
Determine the chemical formula for the copper(II) chloride hydrate from the experimental data. [3]
-
State the chemical name of the copper(II) chloride hydrate from this experiment. [1]
-
State the core electron configuration for copper. [1]
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Question 39
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 |
-
A. 39.00
-
B. 40.00
-
C. 39.39
-
D. 40.50
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Question 40
Which electron transition in the hydrogen atom emission spectrum emits radiation with the highest frequency?
-
A.
-
B.
-
C.
-
D.
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Question 41
[Maximum mark: 15]
Copper(II) chloride can exist as an anhydrous solid or hydrate.
-
A sample of copper(II) chloride hydrate was heated on a watch glass until the blue solid changed completely to brown, and the following data was recorded:
Masses Value Mass of watch glass () Mass of copper(II) chloride hydrate () Mass of anhydrous copper(II) chloride + watch glass (1st heating, 5 min) Mass of anhydrous copper(II) chloride + watch glass (2nd heating, 5 min) Mass of anhydrous copper(II) chloride + watch glass (3rd heating, 2 min) Suggest a reason why the sample was heated for a second 5 min increment showing a mass change. [1]
-
Calculate the mass of anhydrous copper(II) chloride. Do not include the calculations of uncertainties in your work. [1]
-
Calculate the mass of water in the hydrated copper(II) chloride sample.Do not include the calculations of uncertainties in your work. [1]
-
Calculate the percent uncertainty on the mass of water in the copper(II) chloride sample. [2]
-
Determine the chemical formula for the copper(II) chloride hydrate from the experimental data. [3]
-
State the chemical name of the copper(II) chloride hydrate from this experiment. [1]
-
State the core electron configuration for copper. [1]
-
Copper is known to exist in complex ions. One such complex ion is . State the molecular geometry around the central metal ion and the type of bonding that exists between the and the ligands. [2]
-
When reacts with ammonia, , the color changes from light to dark blue. Explain the cause of this color change using Sections 3 and 15 of the data booklet. [3]
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Question 42
[Maximum mark: 12]
Spectral analysis of molecules can be useful in identifying structure.
-
Determine the empirical formula of a molecule with the following percent composition by mass. [2]
Element by mass C H O -
State the molecular formula for this molecule if the mass spectrum indicates a molecular ion at . [1]
-
State the index of hydrogen deficiency for this molecule. [1]
-
An infrared spectrum was obtained for this molecule. Use Section 26 of the Data Booklet to identify two possible molecular structures consistent with the spectrum below. [2]
[Source: Created with the NIST Chemistry WebBook - https:// webbook.nist.gov]
-
Explain why the infrared spectrum alone is not useful in confirming the identity of this molecule. [2]
-
The following data was collected from an NMR spectrum of the molecule. Using Section 27 of the Data Booklet, explain how this data can distinguish between the molecules suggested in (d), stating the confirmed identity of the molecule. [2]
Chemical shift () Integration 2.40 4 1.06 6 -
Predict, with a reason, the spin-spin coupling that would be observed for the NMR signal at 1.06 . [2]
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