Question

how many single bonds are bonded to sulfur in sf₆?
2
4
6
7
8
question 18
1 pts
in the following lewis structure for clo₃f, chlorine has a formal charge of _ and an oxidation number of _.
1,1
7,1
7,7
1,7

Explanation:

Question 1: How many single bonds are bonded to sulfur in SF₆?

Step1: Analyze SF₆ structure

In SF₆, sulfur (S) is the central atom and is bonded to six fluorine (F) atoms. Each S - F bond is a single bond.

Step2: Count single - bonds

There are 6 S - F single bonds.

Step1: Calculate formal charge of Cl

The formula for formal charge is $FC = V - N - \frac{B}{2}$, where $V$ is the number of valence electrons, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons. Chlorine has 7 valence electrons. In $ClO_3F$, chlorine has 0 non - bonding electrons and 8 bonding electrons. So, $FC=7 - 0-\frac{8}{2}=7 - 4 = 3$. But usually in $ClO_3F$ structure considering resonance and correct distribution, the formal charge of Cl is 0. Because Cl has 7 valence electrons, 0 non - bonding electrons and 7 bonding electrons in the most stable resonance form ($FC = 7-0 - \frac{7}{1}=0$).

Step2: Calculate oxidation number of Cl

Oxygen has an oxidation number of - 2 and fluorine has an oxidation number of - 1. Let the oxidation number of Cl be $x$. In $ClO_3F$, we have $x+3\times(- 2)+(-1)=0$. Solving for $x$ gives $x - 6 - 1=0$, so $x = +7$.

Answer:

6

Question 18: In the following Lewis structure for ClO₃F, chlorine has a formal charge of _ and an oxidation number of _.