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IB Chemistry HL - 2024 - Questionbank

2.2 - Electron Configuration

Hydrogen Emission Spectra, Wavelength, Frequency, Energy, Full & Condensed Electron Configuration, Orbital Diagrams

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Question 1

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What is the maximum number of electrons in the 4p4p subshell?

  • A.\hspace{1em} 6

  • B.\hspace{1em} 10

  • C.\hspace{1em} 2

  • D.\hspace{1em} 8

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Question 2

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What is the electron configuration of this orbital diagram?

2.2-262

  • A.\hspace{1em} 1sX2 2sX2 2pX3\ce{1s^2 2s^2 2p^3}

  • B.\hspace{1em} 1sX2 2pX3 2sX2\ce{1s^2 2p^3 2s^2}

  • C.\hspace{1em} 1sX2 2sX3 2pX2\ce{1s^2 2s^3 2p^2}

  • D.\hspace{1em} 1sX2 2sX2 3sX3\ce{1s^2 2s^2 3s^3}

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Question 3

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Which of the following subshells contains the highest energy?

  • A.\hspace{1em} 2s2s

  • B.\hspace{1em} 2p2p

  • C.\hspace{1em} 2d2d

  • D.\hspace{1em} 3d3d

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Question 4

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What is the term for the region where there is the highest probability of finding an electron?

  • A.\hspace{1em} Orbital

  • B.\hspace{1em} Nucleus

  • C.\hspace{1em} Orbital diagram

  • D.\hspace{1em} Orbit

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Question 5

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Which of the following is the correct electron configuration of a typical sodium ion?

  • A.\hspace{1em} [Ne] 3sX1\ce{[Ne] 3s^1}

  • B.\hspace{1em} [Ne] 3sX2\ce{[Ne] 3s^2}

  • C.\hspace{1em} [Ne]\ce{[Ne]}

  • D.\hspace{1em} [Ne] 2sX1\ce{[Ne] 2s^1}

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Question 6

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Which of the following is the correct orbital diagram for Carbon\ce{Carbon}?

  • A.\hspace{1em}2.2-261-a
    B.\hspace{1em}2.2-261-b
    C.\hspace{1em}2.2-261-c
    D.\hspace{1em}2.2-261-d

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Question 7

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[Maximum mark: 2]

Cobalt is an important cofactor that often inhibits enzyme activity involved in cellular respiration, such as catalase.

  1. Using the complete electron configuration, determine the electron configuration of CoX2+.\ce{Co^2+}. [1]

  2. Draw the orbital diagram of the 3d\ce{3d} electrons of Co\ce{Co}. [1]

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Question 8

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The following table shows the number of subatomic particles present in five species.

SpeciesNumber of protonsNumber of neutronsNumber of electrons
A888
B8810
C9108
D101010
E101210

Which two species are isotopes of the same element?

  • A.\hspace{1em}A and B

  • B.\hspace{1em}B and C

  • C.\hspace{1em}C and D

  • D.\hspace{1em}D and E

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Question 9

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[Maximum mark: 4]

Hydrogen exhibits two emission lines, D1D1 and D2D2. D1D1 has a wavelength of 656nm656\, nm and D2D2 has a frequency of 6.17×1014s16.17\times 10^{14}s^{-1}.

  1. Calculate the frequency of the D1D1 emission line of hydrogen. [1]

  2. Calculate the wavelength of the D2D2 emission line of hydrogen. [1]

  3. 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 10

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The following table shows the number of subatomic particles present in five species.

SpeciesNumber of protonsNumber of neutronsNumber of electrons
A888
B8810
C9108
D101010
E101210

Which two species are ions?


  • A.\hspace{1em}A and B

  • B.\hspace{1em}B and C

  • C.\hspace{1em}C and D

  • D.\hspace{1em}D and E

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Question 11

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What will happen to the frequency of moving light particles if the wavelength is doubled, assuming the velocity is constant?

  • A.\hspace{1em} The frequency will be doubled

  • B.\hspace{1em} The frequency will decrease by half

  • C.\hspace{1em} The frequency will not be affected

  • D.\hspace{1em} The frequency will increase by four

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Question 12

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Which of the following statement(s) is (are) true?

  • I.\enskip 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


  • A.\hspace{1em} I only

  • B.\hspace{1em} II and III only

  • C.\hspace{1em} I and II only

  • D.\hspace{1em} I, II, and III

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Question 13

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Mass spectrometry uses fast-moving electrons to ionize particles and determine the mass-to-charge ratio of an unknown compound.

  1. Using the data booklet section 1 and 2, calculate the frequency of an electron with a wavelength of 1.68m.1.68\, m. [1]

  2. Calculate the wavelength of an electron with a frequency of 2.00×108s12.00 \times 10^8 \,s^{-1}. [1]

  3. State the effect of increasing the wavelength on frequency. [1]

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Question 14

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Which of the following statements is incorrect?

  • A.\hspace{1em}All ions contain electrons

  • B.\hspace{1em}A few alpha particles deflected at large angles in Rutherford's Gold Foil experiment

  • C.\hspace{1em}A mass spectrometer can tell us the number of isotopes an element has

  • D.\hspace{1em}An atom can have more neutrons than protons

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Question 15

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The following is a hydrogen energy level diagram.

CH0682

How many different emission lines are possible?

  • A.\hspace{1em}1

  • B.\hspace{1em}5

  • C.\hspace{1em}15

  • D.\hspace{1em}30

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Question 16

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[Maximum mark: 8]

Deuterium is an isotope of hydrogen that contains one proton, one neutron, and one electron.

    1. Complete the following table. [2]

      ProtonsNeutronsElectrons
      Relative charge
      Relative mass~11836\dfrac{1}{1836}
      Location


    2. Using the following data, calculate the relative atomic mass of hydrogen correct to five decimal places, showing your work. [2]

      IsotopeRelative abundance
      Hydrogen-199.98%
      Deuterium0.012%
      Hydrogen-30.008%


    1. Describe the emission spectrum of the hydrogen atom. [2]

    2. Outline the difference between a continuous spectrum and a line spectrum. [1]

    3. Suggest how your answer to (b)(i) shows that energy levels are quantized. [1]

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Question 17

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[Maximum mark: 9]

Cobalt-60 is a radioactive isotope of the element cobalt that is used to treat thyroid cancer.

    1. State the full electron configuration of cobalt and chromium. [2]

    2. Explain what is special about the electron configuration of chromium. [1]

    3. State the atomic symbol notation for the cobalt-60 isotope. [1]

One atom of cobalt-60 undergoes beta decay, releasing an electron and energy with a frequency of 7.65×1019Hz7.65\times10^{19} Hz to form nickel-60.

    1. Using section 1 of the data booklet, calculate the wavelength of energy released from beta decay. [1]

    2. 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]

    1. Define orbital. [1]

    2. Sketch the shapes of an s-orbital and a p-orbital. [2]

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Question 18

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[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. 1sX2 2sX2 2pX6 3sX2 3pX6 4sX1\ce{1s^2 2s^2 2p^6 3s^2 3p^6 4s^1} [1]

  2. [Ne] 3sX2 3pX6\ce{[Ne] 3s^2 3p^6} [1]

  3. In Period 33 with valence electrons of 3sX2\ce{3s^2} [1]

  4. \mbox{}2.2-263d [1]

  5. An ion with +1 charge, with valence electrons of:
    \mbox{}2.2-263e [1]

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Question 19

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Which of the following pairs of terms describe the shape of an s orbital and the relative energy of a d orbital?


Shape of s orbital\enskip\textbf{Shape of s orbital}\enskipRelative energy of d orbital\enskip \textbf{Relative energy of d orbital}\enskip
\hspace{1em}A.\hspace{1em}SphericalLow
\hspace{1em}B.\hspace{1em}Dumbbell-shapeHigh
\hspace{1em}C.\hspace{1em}SphericalHigh
\hspace{1em}D.\hspace{1em}Dumbbell-shapeLow

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Question 20

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Which atoms' orbital diagram does this figure represent?

2.2-260

  • A.\hspace{1em} C\ce{C}

  • B.\hspace{1em} O\ce{O}

  • C.\hspace{1em} N\ce{N}

  • D.\hspace{1em} F\ce{F}

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Question 21

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[Maximum mark: 7]

X63X2263Cu\ce{^{63}_{}Cu} and X65X2265Cu\ce{^{65}_{}Cu} are the two most abundant isotopes of copper.

    1. Define isotope. [1]

    2. Determine the correct numbers of subatomic particles to complete the following table. [1]

      Copper-63Copper-65
      Number of protons
      Number of electrons
      Number of neutrons


    3. Calculate the relative abundances of X63X2263Cu\ce{^{63}_{}Cu} and X65X2265Cu\ce{^{65}_{}Cu} using section 6 (Section 7- 2025 Syllabus) of the data booklet. [3]

  1. Complete the orbital diagram for the valence electrons in a copper atom and a copper (II) ion. [2]

    CH0684b

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Question 22

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[Maximum mark: 3]

Cu\ce{Cu} is a transition metal commonly used in wires.

  1. Determine the complete electron configuration of Cu\ce{Cu}. [1]

  2. State the condensed electron configuration of CuX+.\ce{Cu+}. [1]

  3. Determine whether the electron configuration of Cu\ce{Cu} follows the usual rules of electron configuration. [1]

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Question 23

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[Maximum mark: 4]

John is sitting on a beach on a warm summer evening watching the reddish sky (λ=650nm\lambda=650\, nm) while his brother, Eric, is playing with his laser beam with a frequency of 4.60×1014s14.60 \times 10^{14}\,s^{-1}.

  1. Calculate the frequency of the radiation from the red sky. [1]

  2. Calculate the wavelength of the laser beam of Eric. [1]

  3. Compare the wavelength of the laser beam with the wavelength of the radiation of the red sky. [1]

  4. Deduce the colour of the laser beam of Eric. [1]

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Question 24

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What is the smallest amount of energy an electron can release?

2-682-683

  • A. \hspace{1em} 0.31 eVeV

  • B. \hspace{1em} 0.54 eVeV

  • C. \hspace{1em} 10.19 eVeV

  • D. \hspace{1em} 13.59 eVeV

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Question 25

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[Maximum mark: 10]

Copper(II) chloride can exist as an anhydrous solid or hydrate.

  1. A 1.78 g1.78\ g 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 (gg)24.57±0.0124.57 \pm 0.01
    Mass of copper(II) chloride hydrate (gg)1.78±0.011.78 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (1st heating, 5 min)26.03±0.0126.03 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (2nd heating, 5 min)25.99±0.0125.99 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (3rd heating, 2 min)25.99±0.0125.99 \pm 0.01

    Suggest a reason why the sample was heated for a second 5 minute increment showing a mass change. [1]

  2. Calculate the mass of anhydrous copper(II) chloride. Do not include the calculations of uncertainties in your work. [1]

  3. Calculate the mass of water in the hydrated copper(II) chloride sample. Do not include the calculations of uncertainties in your work. [1]

  4. Calculate the percent uncertainty on the mass of water in the copper(II) chloride sample. [2]

  5. Determine the chemical formula for the copper(II) chloride hydrate from the experimental data. [3]

  6. State the chemical name of the copper(II) chloride hydrate from this experiment. [1]

  7. State the core electron configuration for copper. [1]

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Question 26

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Which electron transition in the hydrogen atom emission spectrum emits radiation with the highest frequency?


  • A. \hspace{1em} n=1  n=7n=1\ \rightarrow\ n=7

  • B. \hspace{1em} n=7  n=1n=7\ \rightarrow\ n=1

  • C. \hspace{1em} n=5  n=2n=5\ \rightarrow\ n=2

  • D. \hspace{1em} n=4  n=3n=4\ \rightarrow\ n=3

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Question 27

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[Maximum mark: 15]

Copper(II) chloride can exist as an anhydrous solid or hydrate.

  1. A 1.78 g1.78\ g 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:

    MassesValue
    Mass of watch glass (gg)24.57±0.0124.57 \pm 0.01
    Mass of copper(II) chloride hydrate (gg)1.78±0.011.78 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (1st heating, 5 min)26.03±0.0126.03 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (2nd heating, 5 min)25.99±0.0125.99 \pm 0.01
    Mass of anhydrous copper(II) chloride + watch glass (3rd heating, 2 min)25.99±0.0125.99 \pm 0.01

    Suggest a reason why the sample was heated for a second 5 min increment showing a mass change. [1]

  2. Calculate the mass of anhydrous copper(II) chloride. Do not include the calculations of uncertainties in your work. [1]

  3. Calculate the mass of water in the hydrated copper(II) chloride sample.Do not include the calculations of uncertainties in your work. [1]

  4. Calculate the percent uncertainty on the mass of water in the copper(II) chloride sample. [2]

  5. Determine the chemical formula for the copper(II) chloride hydrate from the experimental data. [3]

  6. State the chemical name of the copper(II) chloride hydrate from this experiment. [1]

  7. State the core electron configuration for copper. [1]

  8. Copper is known to exist in complex ions. One such complex ion is [Cu(HX2O)X6]X2+\ce{[Cu(H2O)6]^{2+}}. State the molecular geometry around the central metal ion and the type of bonding that exists between the CuX2+\ce{Cu^{2+}} and the ligands. [2]

  9. When [Cu(HX2O)X6]X2+\ce{[Cu(H2O)6]^{2+}} reacts with ammonia, NHX3\ce{NH3}, 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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