Draw the Lewis structures for each of the following, determine the shape of the molecules.

a. H2S
b. CN3-
c. CCl4
d.NH4
e.PO4-
f.PCL3
f.SF6

and explain how do you determine the shape of it

same song, second verse.

To draw the Lewis structures and determine the shape of the molecules, we need to follow these steps:

1. Count the total number of valence electrons for each atom in the molecule. Valence electrons are the electrons in the outermost energy level of an atom.
- Hydrogen (H) has 1 valence electron.
- Oxygen (O) has 6 valence electrons.
- Nitrogen (N) has 5 valence electrons.
- Carbon (C) has 4 valence electrons.
- Sulfur (S) has 6 valence electrons.
- Chlorine (Cl) has 7 valence electrons.
- Fluorine (F) has 7 valence electrons.
- Phosphorus (P) has 5 valence electrons.

2. Determine the total number of valence electrons in the molecule by adding up the valence electrons of all the atoms.
For anions (negative ions) like CN3- and PO4-, add an additional electron for each negative charge.

3. Determine the central atom. The central atom is usually the least electronegative atom that can form multiple bonds. In some cases, like in NH4+, there is no central atom.

4. Connect the central atom to the surrounding atoms using single bonds. Fill the octet of each atom except hydrogen by placing lone pairs. If there are remaining electrons, place them on the central atom as lone pairs.

5. Determine the shape of the molecule using the VSEPR theory (Valence Shell Electron Pair Repulsion Theory).

- In the VSEPR theory, electron pairs around the central atom repel each other and try to maximize the distance between them. The shape is determined by the number of electron pairs around the central atom.

- Two electron pairs arrange themselves in a linear shape, with a bond angle of 180 degrees (e.g., H2S).

- Three electron pairs arrange themselves in a trigonal planar shape, with a bond angle of 120 degrees (e.g., CCl4).

- Four electron pairs arrange themselves in a tetrahedral shape, with a bond angle of approximately 109.5 degrees (e.g., NH4+).

- Five electron pairs arrange themselves in a trigonal bipyramidal shape, with bond angles of 90 and 120 degrees (e.g., PO4-).

- Six electron pairs arrange themselves in an octahedral shape, with bond angles of 90 degrees (e.g., SF6).

Now, let's draw the Lewis structures and determine the shapes of the molecules you mentioned.

a. H2S:
- Hydrogen (H) has 1 valence electron.
- Sulfur (S) has 6 valence electrons.
Total valence electrons = 2 + 6 = 8
Lewis structure: H-S-H
Shape: Linear

b. CN3-:
- Carbon (C) has 4 valence electrons.
- Nitrogen (N) has 5 valence electrons.
- An additional electron for the negative charge.
Total valence electrons = 4 + 3(5) + 1 = 20
Lewis structure: C≡N-N-N
Shape: Linear

c. CCl4:
- Carbon (C) has 4 valence electrons.
- Chlorine (Cl) has 7 valence electrons.
Total valence electrons = 4 + 4(7) = 32
Lewis structure: Cl-C-Cl-Cl-Cl
Shape: Tetrahedral

d. NH4+:
- Nitrogen (N) has 5 valence electrons.
- An additional electron for the positive charge.
Total valence electrons = 5 + 4(1) - 1 = 8
Lewis structure: H-H-H-NH3
Shape: Tetrahedral

e. PO4-:
- Phosphorus (P) has 5 valence electrons.
- An additional electron for the negative charge.
Total valence electrons = 5 + 4(6) + 1 = 32
Lewis structure: O-P(=O)(-O)-O
Shape: Trigonal Bipyramidal

f. PCl3:
- Phosphorus (P) has 5 valence electrons.
- Chlorine (Cl) has 7 valence electrons.
Total valence electrons = 5 + 3(7) = 26
Lewis structure: Cl-P-Cl-Cl
Shape: Trigonal Pyramidal

g. SF6:
- Sulfur (S) has 6 valence electrons.
- Fluorine (F) has 7 valence electrons.
Total valence electrons = 6 + 6(7) = 48
Lewis structure: F-S-F-F-F-F-F
Shape: Octahedral

Remember that the Lewis structures and shapes are approximations based on the rules we followed. Some molecules may have multiple resonance or isomer possibilities.