Electronic configuration quiz

1. When sodium forms a Na⁺ ion which electron is lost?

a) 1s
b) 2p
c) 3s
d) 3p

2. The electronic configuration of Ca²⁺ is?

a) [Ar]4s⁰
b) [Ar]
c) [Ne]3p6
d) [Ne]3s²3p⁶

3. How many electrons will an aluminium atom lose when it form the aluminium ion Al³⁺?

a) 1
b) 2
c) 3
d) 4

4. The electronic configuration of the oxide ion (O^2-) is the same as the noble gas ; it is isoelectronic with it.

5. Chlorine atoms gain 1 electron to achieve the electronic configuration of:

a) [Ne]
b) [Ar]
c) [Kr]
d) [He]

6. When forming ions, transition metals lose electrons first from the sub-level and then secondly from the sub-level.

7. The electronic configuration of Fe²⁺is?

a) [Ar]4s²3d⁴
b) [Ar]3d⁶
c) [Ar]4s3d⁵
d) [Ar]3d⁴

8. When iron atoms form Fe³⁺ ions one electron is lost from the sub-level.

9. The electronic configuration of Ti²⁺ion is ?

a) [Ar]3d²
b) [Ar]4s²3d⁰
c) [Ar]4s¹3d¹
d) [Ar]3d⁴

10. Chromium has an unusual electronic configuration because it has:

a) A full d sub-shell
b) No 4s electrons
c) Only 3 electrons in the 3d sub-shell
d) A half-filled 3d sub-shell

11. The electronic configuration of Cr³⁺ is:

a) [Ar]3d³
b) [Ar]3d⁵
c) [Ar]4s¹3d⁴
d) [Ar]3d⁶

12. Atoms and ions with the same number of electrons are said to be with each other; for example ions from group one (the alkali metals) in the periodic table are isoelectronic with neon.

13. What concept developed by Wolfgang Pauli helped chemists work out the electronic configuration of atoms and ions?

a) The idea of delocalisation of electrons in atoms and ions
b) Resonance theory
c) The rule of maximum multiplicity
d) the Exclusion principle

14. Why is the Fe³⁺ ion more stable than the Fe²⁺ion?

a) It has a full 3d sub-shell
b) It has a half-filled 3d sub-shell
c) It has more 4s electrons
d) It has a stable octet of electrons

15. When non-metal atoms react they tend to electrons to achieve a noble gas configuration (ns²np⁶)