Name these compounds: (a) Ba(NO3)2 ; (b) HNO2 (c) CrO2 ; (d)...

Name these compounds: (a) $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2} ;$ (b) $\mathrm{HNO}_{2}$ (c) $\mathrm{CrO}_{2} ;$ (d) $\mathrm{KIO}_{3} ;$ (e) $\mathrm{LiCN} ;$ (f) $\mathrm{KIO} ;$ (g) $\mathrm{Fe}(\mathrm{OH})_{2}$ (h) $\mathrm{Ca}\left(\mathrm{H}_{2} \mathrm{PO}_{4}\right)_{2} ;$ (i) $\mathrm{H}_{3} \mathrm{PO}_{4} ;$ (j) $\mathrm{NaHSO}_{4} ;$ (k) $\mathrm{Na}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$; (l) $\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2} ;(\mathrm{m}) \mathrm{MgC}_{2} \mathrm{O}_{4} ;$ (n) $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$

Name these compounds: (a) $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2} ;$ (b) $\mathrm{HNO}_{2}$
(c) $\mathrm{CrO}_{2} ;$ (d) $\mathrm{KIO}_{3} ;$ (e) $\mathrm{LiCN} ;$ (f) $\mathrm{KIO} ;$ (g) $\mathrm{Fe}(\mathrm{OH})_{2}$
(h) $\mathrm{Ca}\left(\mathrm{H}_{2} \mathrm{PO}_{4}\right)_{2} ;$ (i) $\mathrm{H}_{3} \mathrm{PO}_{4} ;$ (j) $\mathrm{NaHSO}_{4} ;$ (k) $\mathrm{Na}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$;
(l) $\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2} ;(\mathrm{m}) \mathrm{MgC}_{2} \mathrm{O}_{4} ;$ (n) $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$

Key Concepts

Ionic Compound Nomenclature

This concept deals with how to name compounds that are composed of cations (positively charged ions) and anions (negatively charged ions). When naming ionic compounds, one typically names the cation first followed by the anion. The cation usually retains its elemental name, while the anion is modified to end in “-ide” for simple ions. For compounds containing polyatomic ions the full name of the ion is used.

Polyatomic Ion Nomenclature

Polyatomic ions are groups of atoms that act as a single charged entity in a compound. Their names are often derived from traditional names and usually end in “-ate” or “-ite” for oxyanions depending on the number of oxygen atoms present. Familiarity with common polyatomic ions like nitrate, nitrite, sulfate, and phosphate is critical when naming many inorganic compounds.

Oxyanion Nomenclature

Oxyanions are polyatomic ions that contain oxygen along with a central atom and one or more negative charges. Their naming involves recognizing the number of oxygen atoms attached to the central atom. Common examples include nitrate (NO3–) and nitrite (NO2–), where the suffix ‘-ate’ is used for the ion with more oxygen atoms and ‘-ite’ for the one with fewer.

Acid Nomenclature

Acid nomenclature involves naming compounds that donate protons (H+ ions) in solution. When an acid contains a polyatomic ion with oxygen, if the anion’s name ends in ‘-ate’ the corresponding acid name will be formed by replacing ‘-ate’ with ‘-ic’ and adding the word acid. If the polyatomic ion ends in ‘-ite’, the acid name is modified to end in ‘-ous’ acid. For non-oxygen containing acids, the prefix ‘hydro-’ is used followed by the root of the element and the word acid.

Oxidation State Conventions in Nomenclature

When a metal, particularly a transition metal, can exhibit multiple oxidation states, its specific oxidation state in a compound is indicated by a Roman numeral placed in parentheses immediately after the metal's name. This system avoids ambiguity in compounds where the metal's chemical behavior and the compound's reactivity depend on its oxidation state.

Transcript

00:01 So for this question, we want to name a number of compounds, and we're going to do so in a number of ways for questions like this first one.

00:11 We're going to look at what makes up the compound, and here we see this is a nitrate, and we know this is barium, so we know the name to be barium nitrate.

00:35 So we can look at b.

00:39 And if we look at the oxidation state, so we're looking here at the oxidation state of nitrogen.

00:46 If we were to calculate this out to find the oxidation state, we would find that it was positive three.

00:51 And since it is positive three, that means our ending is going to be oss, which is based on how many oxidation states of nitrogen there are.

01:02 So we know this to be nitrous acid because of that acidic.

01:11 Hydrogen.

01:13 And then for cro2, which is chromium and two oxygen, we know the oxidation state of oxygen is negative 2, and then we can calculate to find the oxidation state of chromium, and we find it to be a positive 4.

01:31 So we can find the name of c to be chromium.

01:42 Since this is a metal, we'll do 4 oxide.

01:53 And we always are going to use the roman numerals, as i did for c.

01:57 And then we can move on to look at d.

02:00 And like we did in a, look at what is made up of.

02:04 And we find this to be iodate.

02:10 So that means our name is potassium iodate.

02:24 Then we can go down and look at e first.

02:33 So for e we see a lithium, carbon, and a nitrogen.

02:38 And we know this to be cyanide...