Chapter U5.15, Problem 4E

Interpretation Introduction

Interpretation:

Shell models for lithium and oxygen atoms to show the transfer of electrons during oxidation needs to be explained.

Concept introduction:

Metal elements contain one, two, or three electrons in their outermost shells. Having such a small number of electrons in the valence shell makes it more likely that metal atoms will lose electrons, forming cations that have a charge of +1, +2, or +3. Metal atoms form ionic bonds with nonmetal atoms via electron transfer.

Answer to Problem 4E

The below shell diagram shows the transfer of electrons from lithium to oxygen

Explanation of Solution

The shell model of Li atom is shown below:

The atomic number of Li is 3. Its electron configuration is $1s^{2}2s^{1}or2,1$. The electron configuration of O is $1s^{2}2s^{2}2p^4\text{ or 2, 6 }$. So, oxygen needs two electrons to fill its octet. Therefore, each Li transfers one electron that means two Li transfers 2 electrons to oxygen. The shell model shows two lithium atoms being oxidized and produces 2 ${\text{Li}}^{\text{+}}$ ions.

Conclusion

In an oxidation reaction, an atom transfers electrons to oxygen or another atom.