Question

consider the four models of the carbon (c), oxygen (o), nitrogen (n), and hydrogen (h) atoms shown above. count the number of unpaired electrons in the outer shells of each of the four atoms. then, drag and drop the correct number of unpaired electrons to match it with the name of each atom.

when a covalent bond forms, an unpaired electron in one atoms outer shell takes up a physical position near an unpaired electron in the outer shell of another atom. this forms a covalent bond. the two electrons are now shared by the two atoms—their negative charges are attracted to the positive charges on both nuclei. this makes both atoms more stable.

did you fully understand the concept covered in this section?

Explanation:

Step1: Determine oxygen's unpaired electrons

Oxygen has electron - configuration $1s^{2}2s^{2}2p^{4}$. In the $2p$ sub - shell, there are 4 electrons. According to Hund's rule, 2 of the $2p$ electrons are unpaired. So oxygen has 2 unpaired electrons.

Step2: Determine hydrogen's unpaired electrons

Hydrogen has an electron - configuration of $1s^{1}$. There is 1 electron in its outer shell, so it has 1 unpaired electron.

Step3: Determine carbon's unpaired electrons

Carbon has an electron - configuration of $1s^{2}2s^{2}2p^{2}$. In the $2p$ sub - shell, there are 2 electrons which are unpaired according to Hund's rule. So carbon has 2 unpaired electrons.

Answer:

Oxygen: 2 unpaired electrons
Hydrogen: 1 unpaired electron
Carbon: 2 unpaired electrons