So I have to draw a couple of lewis structures for; (b) (CH 3 ) 2 S (c) KOCl

For b I did H-C-C-S-H (Remaining Hs connected above and below C) and for c) I did [K]^+ O-Cl. Are either of the right?

For (CH3)2S see https://www.youtube.com/watch?v=g_z4roJO1fY

For KOCl see https://www.google.com/search?q=lewis+structure+KClO&client=firefox-b-1&tbm=isch&tbo=u&source=univ&sa=X&ved=0ahUKEwj8wc3I6enYAhVDjK0KHZr-AOIQsAQILA&biw=918&bih=474

Let's go through the Lewis structures you have drawn and check if they are correct.

For (b) (CH3)2S (dimethyl sulfide), you have correctly identified the central atom as sulfur (S). However, the actual structure would look like this:

H H
| |
H-C-C-S-C-C-H
| |
H H

In the Lewis structure, there should be four total bonds around the sulfur atom and each hydrogen atom should be connected directly to a carbon atom.

Now, moving on to (c) KOCl, you have correctly indicated potassium cation (K+) and chloride anion (Cl-) in the Lewis structure. However, you missed the oxygen atom (O). The correct Lewis structure for KOCl would look like this:

K+
/
O
\
Cl-

In this structure, the oxygen atom is bonded to the chlorine atom (O-Cl bond) and the potassium atom forms a separate bond with oxygen.

I hope this clarifies the correct Lewis structures for (b) (CH3)2S and (c) KOCl.

To draw Lewis structures, you need to consider the valence electrons of each atom and then distribute them around the atoms in a way that satisfies the octet rule. Let's go through each compound and draw the Lewis structures:

(b) (CH3)2S:
To draw the Lewis structure for (CH3)2S, you need to consider the valence electrons of each atom. Carbon (C) has 4 valence electrons, hydrogen (H) has 1 valence electron, and sulfur (S) has 6 valence electrons.

1. Start by connecting the carbon (C) and sulfur (S) atoms with a single bond.

H-C-C-S-H

2. Add the remaining hydrogen (H) atoms around each carbon (C) atom.

H H
|
H-C-C-S-H
|
H H

3. Distribute the valence electrons around the atoms, starting with the outer atoms. In this case, distribute the remaining electrons around the hydrogen (H) atoms first and then the remaining electrons around the central carbon (C) and sulfur (S) atoms.

H H
|
H-C-C-S-H
|
H H

The structure should show a total of 8 valence electrons around each hydrogen (H) atom, and 8 valence electrons around the carbon (C) and sulfur (S) atoms.

(c) KOCl:
To draw the Lewis structure for KOCl, you need to consider the valence electrons of each atom. Potassium (K) has 1 valence electron, oxygen (O) has 6 valence electrons, and chlorine (Cl) has 7 valence electrons.

1. Start by connecting the potassium (K) and chlorine (Cl) atoms with a single bond.

[K]-O-Cl

2. Distribute the valence electrons around the atoms, starting with the outer atoms. In this case, distribute the remaining electrons around the oxygen (O) atom first and then the remaining electrons around the central potassium (K) and chlorine (Cl) atoms.

[K]^+ O-Cl

The structure should show a total of 8 valence electrons around the oxygen (O) atom, and the potassium (K) atom should have a +1 charge, while the chlorine (Cl) atom should have a -1 charge.

In summary, your Lewis structures for (CH3)2S and KOCl are correct based on the valence electrons and connectivity of the atoms.