Determine the number of bonding electrons and the number of nonbonding electrons in the structure of SeCl2 and SiO2.

8,8

To determine the number of bonding electrons in a molecule, we need to count the total number of valence electrons of the atoms in the molecule and then subtract the number of valence electrons used in the bonds. Nonbonding electrons are the remaining valence electrons after the bonding electrons have been determined.

1. SeCl2:
- Selenium (Se) is in Group 16 of the periodic table and has 6 valence electrons.
- Chlorine (Cl) is in Group 17 of the periodic table and has 7 valence electrons.

The total number of valence electrons in SeCl2 is calculated by adding the valence electrons of Se and both Cl atoms:
6 (Se) + 2(7) (2 Cl) = 20 valence electrons

To determine the number of bonding electrons, we need to draw the Lewis structure for SeCl2:

Cl-Se-Cl

The Se atom forms a single bond with each Cl atom, sharing two electrons with each chlorine. Therefore, there are a total of 4 bonding electrons.

To determine the number of nonbonding electrons, we subtract the number of bonding electrons from the total valence electrons:
20 - 4 = 16 nonbonding electrons.

Therefore, the structure of SeCl2 has 4 bonding electrons and 16 nonbonding electrons.

2. SiO2:
- Silicon (Si) is in Group 14 of the periodic table and has 4 valence electrons.
- Oxygen (O) is in Group 16 of the periodic table and has 6 valence electrons.

The total number of valence electrons in SiO2 is calculated by adding the valence electrons of Si and 2 O atoms:
4 (Si) + 2(6) (2 O) = 16 valence electrons

To determine the number of bonding electrons, we need to draw the Lewis structure for SiO2:

O=Si=O

The Si atom forms a double bond with each O atom, sharing 4 electrons with each oxygen. Therefore, there are a total of 8 bonding electrons.

To determine the number of nonbonding electrons, we subtract the number of bonding electrons from the total valence electrons:
16 - 8 = 8 nonbonding electrons.

Therefore, the structure of SiO2 has 8 bonding electrons and 8 nonbonding electrons.

To determine the number of bonding electrons and the number of nonbonding electrons in the structures of SeCl2 and SiO2, we need to know the Lewis structures of these molecules.

1. SeCl2:
To draw the Lewis structure of SeCl2, we first need to determine the total number of valence electrons.

For selenium (Se), it is in Group 6A and has 6 valence electrons.
For chlorine (Cl), it is in Group 7A and has 7 valence electrons.

So, the total number of valence electrons in SeCl2 is:
1(Se) + 2(Cl) = 1(6) + 2(7) = 20

Next, we draw the Lewis structure as follows:
- Place the Se atom in the center.
- Attach two Cl atoms to the Se atom with a single bond.
- Distribute the remaining electrons around the atoms to fulfill the octet rule.
- Place any remaining electrons on the central atom (Se) as nonbonding electrons.

The Lewis structure of SeCl2 would look like this:

Cl Se Cl
. :
. :

In this structure, the Se atom forms two bonds with the Cl atoms. Each bond consists of two electrons, so the total number of bonding electrons is 2 × 2 = 4. There are no nonbonding electrons (also known as lone pairs) on the Se atom.

2. SiO2:
For SiO2, we similarly need to determine the total number of valence electrons.

For silicon (Si), it is in Group 4A and has 4 valence electrons.
For oxygen (O), it is in Group 6A and has 6 valence electrons.

So, the total number of valence electrons in SiO2 is:
1(Si) + 2(O) = 1(4) + 2(6) = 16

Next, we draw the Lewis structure as follows:
- Place the Si atom in the center.
- Attach two O atoms to the Si atom with double bonds.
- Distribute the remaining electrons around the atoms to fulfill the octet rule.
- Place any remaining electrons on the central atom (Si) as nonbonding electrons.

The Lewis structure of SiO2 would look like this:

O Si O
.. :
.. :

In this structure, the Si atom forms two double bonds with the O atoms. Each bond consists of two electrons, so the total number of bonding electrons is 2 × 2 = 4. There are no nonbonding electrons (lone pairs) on the Si atom.

To summarize:
- In the structure of SeCl2, there are 4 bonding electrons and 0 nonbonding electrons.
- In the structure of SiO2, there are also 4 bonding electrons and 0 nonbonding electrons.

4,4