Given that S is the central atom, draw a Lewis structure of OSF4 in which the formal charges of all atoms are zero

We can't draw pictures on the board.

S is the central atom.
Place 4 F atoms attached to S. Place 8 electrons around each F.
Place a O= to S with four additional electrons around O.
40 electrons total.

To draw the Lewis structure of OSF4 with zero formal charges, follow these steps:

Step 1: Determine the total number of valence electrons.
The central atom is sulfur (S), which is in Group 6A, so it has 6 valence electrons. Each oxygen (O) atom has 6 valence electrons, and the fluorine (F) atoms have 7 valence electrons each. The total number of valence electrons for OSF4 is:

(6 from S) + (4 × 6 from O) + (4 × 7 from F) = 6 + 24 + 28 = 58 electrons

Step 2: Connect the atoms using single bonds.
Since S is the central atom, it should be bonded to each O atom and each F atom. Start by drawing a skeletal structure with S in the center and one O and one F atom bonded to it.

F O
| |
S

Step 3: Add the remaining valence electrons as lone pairs.
Place the remaining valence electrons around each atom to satisfy the octet rule, except for hydrogen, which can only accommodate 2 electrons.

Starting with sulfur (S), add 4 lone pairs (8 electrons) around it.

F O
| |
S :O:



Step 4: Distribute the remaining electrons to fulfill the octet rule.
Distribute the remaining valence electrons around the oxygen and fluorine atoms until each atom has an octet.

F O
| |
S :O:

F O
| |
S=O

F=O

Step 5: Make sure the central atom has an octet.
If the central atom (S) does not have an octet, try moving lone pairs from surrounding atoms to form double or triple bonds.

In this case, move a lone pair from an outer oxygen (O) atom and form a double bond with sulfur (S).

F O
| |
S=O

This arrangement gives each atom an octet, and all atoms have zero formal charges.

So, the final Lewis structure for OSF4 with zero formal charges is:

F O
| |
S=O

To draw the Lewis structure of OSF4 with zero formal charges, we need to follow a step-by-step process. Here's how you can do it:

Step 1: Determine the total number of valence electrons.
In OSF4, Oxygen (O) has 6 valence electrons, Sulfur (S) has 6 valence electrons, and Fluorine (F) has 7 valence electrons. Since there are four fluorine atoms, we multiply 7 by 4 to get a total of 28 valence electrons for fluorine.

Therefore, the total number of valence electrons for OSF4 is:
6 (Oxygen) + 6 (Sulfur) + 28 (4 x Fluorine) = 40 valence electrons.

Step 2: Determine the central atom.
In this case, the central atom is Sulfur (S) since it is less electronegative than Oxygen (O) and can accommodate more bonded atoms.

Step 3: Build the initial Lewis structure.
Place the Sulfur (S) atom in the center and connect it to the four Fluorine (F) atoms with single bonds. This gives you a structure with S as the central atom and four F atoms bonded to it. The remaining electrons are placed on the outer atoms, which is Fluorine (F).

F
|
F--S--F
|
F

Step 4: Accounting for the remaining electrons.
We've used 6 electrons for the bonds, so we have 40 - 6 = 34 electrons remaining.

Step 5: Distribute the remaining electrons.
To distribute the remaining electrons, we place them as lone pairs on the outer atoms, which is Fluorine (F). Starting with the first Fluorine atom, place 6 electrons on each Fluorine until all remaining electrons are distributed.

F
/ \
F-S-F F
\ /
F

Step 6: Check for octet rule and formal charges.
Check if all the atoms have satisfied the octet rule (except hydrogen) by counting the number of electrons around each atom. Oxygen and the Fluorine atoms should have eight electrons (full octets), and Sulfur should have 12 electrons (expanded octet).

In this case, Sulfur (S) has 12 electrons, Oxygen (O) has 8 electrons, and Fluorine (F) atoms have 8 electrons each.

Step 7: Check for formal charges.
To check for formal charges, we need to calculate the difference between the number of valence electrons an atom brought from its neutral state and the number of electrons it actually possesses.

The formal charge formula is:
Formal Charge = Valence electrons - Unshared electrons - (1/2)Shared electrons

Calculating the formal charges for each atom in OSF4:

Sulfur (S):
Valence electrons = 6
Unshared electrons = 4 (2 lone pairs)
Shared electrons = 4 (2 bonds x 2 electrons)
Formal Charge = 6 - 4 - (1/2) * 4 = 6 - 4 - 2 = 0

Oxygen (O):
Valence electrons = 6
Unshared electrons = 6 (3 lone pairs)
Shared electrons = 2 (1 bond x 2 electrons)
Formal Charge = 6 - 6 - (1/2) * 2 = 6 - 6 - 1 = -1

Fluorine (F):
Valence electrons = 7
Unshared electrons = 2 (1 lone pair)
Shared electrons = 2 (1 bond x 2 electrons)
Formal Charge = 7 - 2 - (1/2) * 2 = 7 - 2 - 1 = +4

After assigning the formal charges, we can see that the Sulfur (S) atom has a formal charge of zero, which means that all atoms in the OSF4 Lewis structure have a formal charge of zero and we have achieved a structure with zero formal charges.

Final Lewis Structure of OSF4 with Zero Formal Charges:
F
/ \
F-S-F F
\ /
F

So, this is the correct Lewis structure of OSF4 with zero formal charges.