IB Diploma Programme (DP) - SL & HL · Chemistry

Structure 1.3—Electron configurations: Practice Questions

5 multiple-choice questions marked as you go, and 2 written questions with worked solutions. All on Structure 1.3—Electron configurations.

7 questions13 marksFree, no account

Question 1

1 mark

What is the maximum number of electrons that can occupy the $p$ subshell in any given principal energy level?

Question 2

1 mark

What is the full ground-state electron configuration of the phosphide ion, $\text{P}^{3-}$?

Question 3

1 mark

Which of the following transition metal ions has an electron configuration with four unpaired electrons?

Question 4

1 mark

Which of the following describes the full electron configuration of a neutral phosphorus atom (atomic number $Z = 15$) in its ground state?

Question 5

1 mark

According to the Aufbau principle and Hund's rule, what is the correct orbital diagram for the outer (valence) shell of a ground-state carbon atom ($Z = 6$)?

Question 6

3 marks

Explain why a neutral sulfur atom ($$S$$) is paramagnetic, based on its electron configuration.

Write your answer out first, then check it against the worked solution.

Question 7

5 marks

An element has an atomic number of 26.

a) Write the full electron configuration for a neutral atom of this element in its ground state.

b) Write the condensed (noble gas) electron configuration for a neutral atom of this element.

c) Write the electron configuration for its most common ion, which has a charge of $$+3$$.

Write your answer out first, then check it against the worked solution.

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