The compound's name is zinc perchlorate. With the addition of a fourth oxygen atom to the molecule, chlorate , we follow the polyatomic ion naming rules and add a per- to the molecule's name, giving us perchlorate. When bonded ionically to a zinc cation , the resulting ionic compound is called zinc perchlorate.

 is the correct formula because, following IUPAC acid naming rules, when combining a hydrogen cation with an anion that consists of only one element (in this case iodide), one drops the -ide ending, adds an -ic ending and adds a hydro- prefix. Other examples would be hydrochloric acid  and hydrofluoric acid .

While the student's description of the location and size of the sidechains is correct, he/she failed to recognize the longest parent chain, it being the eight-carbon string which encompasses what he/she named isopropyl- and pentyl-. The resulting octane molecule has four methyl- substituents at the 2, 3, 4, and 5 positions. 

While it is tempting to think that butane and isobutane, because of their structural differences would have different numbers of of hydrogens, they are in fact constitutional isomers, and have the same molecular formula. Both butane and isobutane have four carbons and ten hydrogens, although butane's carbons and hydrogen's are arranged

 and isobutane's are arranged 

A good rule of thumb for the formulas of simple hydrocarbons is:

Because the ion,  , is correctly referred to as both bicarbonate and hydrogen carbonate, the correct names for the compound in question are both potassium bicarbonate and potassium hydrogen carbonate.

Because the polyatomic ion from which the acid, , is derived is perchlorate, , the resulting acid is named perchloric acid. The naming protocol is to use the -ic suffix for acids derived from polyatomic ions ending in -ate, while using the -ous suffix for acids derived from polyatomic ions ending in -ite.

All of the incorrect options have prefixes or suffixes associated with polyatomic ions "hypo," "per," "ite," and "ate". Since  is not an ion (it does not have a charge), it must just be a covalent compound. Therefore, use the prefixes reserved for covalent compounds to name it.

The name of this compound is iron (II) oxide. First, notice how the chemical formula  contains one metal and one nonmetal, so we know that we are not going to be using prefixes such as "mono" because those are used for covalent compounds. Secondly, notice that iron is a transition metal, which means that we have to specify the charge it has, in roman numerals. Iron must have a positive two charge to balance out the negative two charge oxygen will have.

This is an ionic compound, we know that because we see a metal bound to a nonmetal. To name ionic compounds, first write the name of the metal, or cation: magnesium. Next, we have the polyatomic ion arsenate . Thus our answer is: magnesium arsenate. Since magnesium is not a transition metal, we do not need to indicate its charge with Roman numerals. If arsenate was part of a series of oxyanions (anions that contain oxygen), we use the prefix "per" to indicate more oxygens, however this is not the case.

To name this compound, it's important to first notice what the formal charge would be on each of the constituent ions. We know that the formal charge of a hydroxide ion is . Since there are three of these, and because we know the compound is neutral, the iron constituent must have a charge of . Therefore, this compound is correctly called iron (III) hydroxide.

It's also important to note that there are alternate names for iron (II) and iron (III). Iron (II) is sometimes referred to as "ferrous" while iron (III) is sometimes referred to as "ferric." An easy way to remember this is to note that "ferrous" has an "O" in it and so does the word "lower" (lower as in the lower charge of the +2 iron). Moreover, the term "ferric" has an "I" in it and so does the word "higher" (higher as in the higher charge of +3 iron).