Chemistry Notes on Strong Acids, Bases, and Oxidation States

A collection of flashcards summarizing key concepts of strong acids, strong bases, oxidation states, and important polyatomic ions.

Strong Acids

Seven strong acids include HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HNO₃ (nitric acid), HClO₃ (chloric acid), HClO₄ (perchloric acid), and H₂SO₄ (sulfuric acid).

Strong Bases

Strong bases include LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, and Ba(OH)₂.

Oxidation State Rules

Key oxidation state rules include: Free elements = 0; Monatomic ions = charge; Oxygen = usually -2; Hydrogen = usually +1; Fluorine = always -1; Group 1 metals = +1; Group 2 metals = +2.

Sum Rule of Oxidation States

The sum of oxidation states in a neutral compound equals 0; for a polyatomic ion, they add up to the ion's charge.

Sulfur in SO₄²⁻

In the sulfate ion (SO₄²⁻), sulfur has an oxidation state of +6.

Polyatomic Ion: Ammonium

NH₄⁺ is the ammonium ion, which carries a +1 charge.

Polyatomic Ion: Hydroxide

OH⁻ is the hydroxide ion, which carries a -1 charge.

Polyatomic Ion: Nitrate

NO₃⁻ is the nitrate ion, which carries a -1 charge.

Polyatomic Ion: Sulfate

SO₄²⁻ is the sulfate ion, which carries a -2 charge.

Polyatomic Ion: Phosphate

PO₄³⁻ is the phosphate ion, which carries a -3 charge.