Give the formulas of the following salts: 𝐚. bismuthyl nitrate; b. strontium perchlorate; c. eur

Give the formulas of the following salts: 𝐚. bismuthyl...

Give the formulas of the following salts: $\mathbf{a}$. bismuthyl nitrate;
b. strontium perchlorate;
c. europium(II) sulfite;
d. iron(II) phosphate;
e. chromium(II) carbonate;
f. cesium phosphate;
g. zinc(II) perbromate;
h. potassium perbromate;
i. calcium bromite;
j. calcium borate.

Key Concepts

Ionic Compounds

Ionic compounds are composed of positively charged ions (cations) and negatively charged ions (anions) held together by electrostatic forces. The formation of these compounds depends on the attraction between oppositely charged ions, and the overall formula must reflect a balance between these charges.

Cation and Anion Nomenclature

The naming of ionic compounds follows a systematic order where the cation is named first and the anion second. For metals that can exhibit multiple oxidation states, a Roman numeral is used to indicate the specific charge of the metal ion, which is critical for deducing the correct formula.

Polyatomic Ions

Polyatomic ions are stable groups of covalently bonded atoms that carry a net charge. In ionic compounds, these ions function as the anion or sometimes the cation. Learning the common polyatomic ions and their charges aids in the construction and balancing of the formulas of salts.

Oxidation States

The oxidation state of an element in a compound indicates its degree of oxidation and is especially important for transition metals where multiple oxidation states are possible. Knowing the oxidation state helps in correctly pairing cations and anions to generate a compound with a neutral overall charge.

Charge Balancing

Charge balancing is the process of ensuring that the total positive charges equal the total negative charges in an ionic compound. This principle ensures the electrical neutrality of the compound and is essential when determining the subscripts in the chemical formula of a salt.

Transcript

00:01 Let's put everything together and write some formulas from the given names of some compounds.

00:07 We'll start with calcium -hydrogen sulfate.

00:11 From the name we know we have calcium.

00:13 We have hydrogen in the middle, and we're going to end with sulfate, s -o -4.

00:17 Sulfate has a minus -3 charge, and the plus 2 from calcium and plus 1 from hydrogen.

00:22 Even everything out, and we're good to go.

00:25 Next we have zinc phosphate, which we have zinc, and we know phosphate is p .o.

00:30 C .04.

00:32 Since phosphate has a minus three charge and zinc a plus two, we're going to need two phosphates, excuse me, two phosphates and three zincs.

00:43 Next up, iron three perchlorates.

00:45 We have iron, which from the name we know is a plus three charge and perchlorate, c .o4.

00:53 Since perchlorid is only minus one, we don't you need three of them.

00:57 Next we have cobaltic hydroxide.

01:00 Cobaltic hydroxide starts with cobalt, and we know hydroxide is oh -h -minus.

01:07 We're going to need three of those to balance charges.

01:09 We have co -o -h -3, excuse me.

01:14 Next, potassium chromate.

01:16 We have potassium, k, then chromate, c -r -o -4.

01:23 And since there's a minus charge on that, we are going to need two potassium to each.

01:31 Even us out and give us k2 -c -r -o -4.

01:36 Next we have aluminum -dihigrogen phosphate.

01:40 So we'll start with our cation aluminum...

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