Question

Which of the following electron configurations gives the correct arrangement of the four valence electrons of the carbon atom in the molecule methane (CH4)? (the 4 is on the bottom not on top )

A) 2s^2 2p^2
B)2s^1 2p^1 3s^1
C)2s^1 2p^2 3s^1
D)2s^1 2p^3

Answer 1

Answer:

D) $2s^12p^3$

Explanation:

Carbon.

The electronic configuration is -  

$1s^22s^22p^2$

Thus, 2s orbital is fully filled and p orbital can singly filled 3 electrons. Thus, Carbon has 2 singly occupied orbitals.

But in methane, $CH_4$ it forms 4 bonds. So, 1 electron each from 2s orbital jumps to the next orbital in the p subshell.

Thus, the configuration is:-

$1s^22s^22p^2$

Thus, the valence electron configuration is:-

$2s^12p^3$

Answer 2

The valence electronic configuration of carbon in methane has been

$\rm 2s^1\;2p^3$. Thus, the correct option has been D.

Methane has been the simplest hydrocarbon with 1 carbon and 4 hydrogen atoms. The carbon has 6 electrons, and 4 valence electrons in 2 shells.

The electronic configuration of carbon valence electrons has been:

$\rm 2s^2\;2p^2$

Since. p subshell has been able to occupy 6 electrons and there has 4 hydrogen bonds with the carbon atom, the electron in 2s subshell has been jumped to 2p orbitals, and having the electronic configuration:

$\rm 2s^1\;2p^3$.

Thus, the correct option has been D.

For more information about the valence electrons, refer to the link:

https://brainly.com/question/14989344