Question

bellringer: 1. what are the rules for naming ionic bonds? 2. what are the rules for naming covalent bonds? 3. what are the rule for naming acids? 4. h(io3) 5. h2(c2o4) 6. hi

Explanation:

Step1: Rules for naming ionic bonds

The name of the metal (cation) comes first, followed by the name of the non - metal (anion). The anion's name is modified to end in - ide. For polyatomic anions, the name of the polyatomic ion is used as is.

Step2: Rules for naming covalent bonds

Name the first element using the element's name. Name the second element with an - ide ending. Use prefixes to indicate the number of atoms of each element (mono - for 1, di - for 2, tri - for 3, etc., but mono is usually not used for the first element).

Step3: Rules for naming acids

For binary acids (compounds with hydrogen and one other non - metal), the name starts with hydro - followed by the root of the non - metal name and ends with - ic acid. For oxyacids (acids containing hydrogen, oxygen, and another element), if the polyatomic anion ends in - ate, the acid name ends in - ic acid; if the polyatomic anion ends in - ite, the acid name ends in - ous acid.

Step4: Naming H(IO3)

The polyatomic ion is iodate ($IO_3^-$). So the name is iodic acid.

Step5: Naming H2(C2O4)

The polyatomic ion is oxalate ($C_2O_4^{2 - }$). So the name is oxalic acid.

Step6: Naming HI

It is a binary acid. The name is hydroiodic acid.

Answer:

1. Name metal (cation) first, then non - metal (anion) with - ide ending for simple anions or use polyatomic ion name as is.
2. Name first element as is, second with - ide ending, use prefixes for number of atoms.
3. Binary acids: hydro - + non - metal root + - ic acid; Oxyacids: - ate in anion gives - ic acid, - ite in anion gives - ous acid.
4. Iodic acid
5. Oxalic acid
6. Hydroiodic acid