show charges on each atom in following bonds:

Cl-Cl
Sr-O
H-O
Br-I

Cl-Cl is a covalent bond. No charge.

SrO is an ionic compound with Sr+2 and O -2.
HO is a polyatomic ion with a charge of OH^-.
Br-I is a covalent bond. no charge.

The Br-I is a polar covalent bond with the Br being slightly negative and the I slightly positive.

The OH^- is a polar covalent bond, also.
If you want the FORMAL charges, none of these answers are correct. you didn't specify exactly what you wanted.

Thanks, Dr.

What would the formal charges be?

Do you know how to do formal charges? If so, check me out on these. I'm not going to draw a diagram, and frankly, that's about the only way I can bre SURE I get them right.

Cl-Cl is zero f.c. on each Cl.
SrO. Sr has f.c. of +2 and O of -2.
OH^-. O has f.c. of -1, H is 0.
Br-I. Both have f.c. of 0.

To determine the charges on each atom in a chemical bond, we need to understand the concept of electronegativity. Electronegativity is the tendency of an atom to attract electrons towards itself in a chemical bond.

1. Cl-Cl:
Chlorine (Cl) is a non-metal and has a higher electronegativity than most other elements. In a Cl-Cl bond, the electronegativity of both chlorine atoms is the same. Therefore, the electrons are shared equally, resulting in a nonpolar covalent bond. There is no charge on each atom since the electron distribution is symmetrical.

2. Sr-O:
Strontium (Sr) is a metal, and oxygen (O) is a non-metal. Metals tend to lose electrons, while non-metals tend to gain electrons to achieve a stable configuration. In an Sr-O bond, oxygen is more electronegative than strontium. Thus, oxygen attracts the shared electrons closer to itself, resulting in a polar covalent bond. Oxygen would have a partial negative charge (δ-) due to the electron density, while strontium would have a partial positive charge (δ+).

3. H-O:
Hydrogen (H) is a non-metal, and oxygen (O) is also a non-metal. In an H-O bond, oxygen is more electronegative than hydrogen. Therefore, oxygen attracts the shared electrons closer to itself, resulting in a polar covalent bond. Oxygen would have a partial negative charge (δ-), while hydrogen would have a partial positive charge (δ+).

4. Br-I:
Bromine (Br) and iodine (I) are both non-metals. In a Br-I bond, bromine is more electronegative than iodine. Hence, bromine attracts the electrons closer to itself, causing a polar covalent bond. Bromine would carry a partial negative charge (δ-), while iodine would carry a partial positive charge (δ+).