Mr. Glimme's Things to Memorize Reference Sheet

Vocabulary practice flashcards covering polyatomic ions, solubility rules, oxidation rules, periodic trends, molecular geometries, and chemical formulas from Mr. Glimme's review notes.

Mercury(I) Ion

$$Hg_2^{2+}$$

Mercury(II) Ion

$$Hg^{2+}$$

Ammonium

$$NH_4^+$$

Nitrate

$$NO_3^-$$

Nitrite

$$NO_2^-$$

Sulfate

$$SO_4^{2-}$$

Sulfite

$$SO_3^{2-}$$

Hydroxide

$$OH^-$$

Carbonate

$$CO_3^{2-}$$

Cyanide

$$CN^-$$

Ethanoate

$$C_2H_3O_2^-$$

Phosphate

$$PO_4^{3-}$$

Permanganate

$$MnO_4^-$$

Peroxide

$$O_2^{2-}$$

Dichromate

$$Cr_2O_7^{2-}$$

Chromate

$$CrO_4^{2-}$$

Hydrogen sulfate

$$HSO_4^-$$

Hydrogen phosphate

$$HPO_4^{2-}$$

Dihydrogen phosphate

$$H_2PO_4^-$$

Hydrogen Carbonate

$$HCO_3^-$$

Hypochlorite

$$ClO^-$$

Chlorate

$$ClO_3^-$$

Chlorite

$$ClO_2^-$$

Perchlorate

$$ClO_4^-$$

Solubility Rule 1 (Nitrates)

Most nitrates are soluble.

Solubility Rule 2 (Alkali Metals & Ammonium)

Most alkali metals and ammonium compounds are soluble.

Solubility Rule 3 (Halogen Salts)

Most chloride/halogen salts are soluble, except with $Ag^+$, $Pb^{2+}$, $Hg_2^{2+}$. Most fluoride salts are only slightly soluble.

Solubility Rule 4 (Sulfate Salts)

Most sulfate salts are soluble, except with $Ba^{2+}$, $Pb^{2+}$, $Hg_2^{2+}$, and $Ca^{2+}$.

Solubility Rule 5 (Hydroxides)

Most hydroxide salts are only slightly soluble except with $Na^+$ and $K^+$.

Solubility Rule 6 (Insoluble Salts)

Most sulfide, carbonate, chromate, and phosphate salts are only slightly soluble.

Oxidation State Rule: Elemental Form

Atoms in their elemental form are given oxidation values of $0$.

Oxidation State Rule: Monatomic Ions

Monatomic ions have the same oxidation value as their charge.

Oxidation State Rule: Fluorine

Fluorine is always given an oxidation value of $-1$.

Oxidation State Rule: Oxygen

Oxygen is usually $-2$, except in peroxide compounds when it is $-1$.

Oxidation State Rule: Hydrogen

Hydrogen is usually $+1$, except in metal hydrides when it is $-1$.

Ionization Energy Trend

Increases left to right, and bottom to top, driven by increasing $p^+$ vs. increasing $e^-$ shielding.

Atomic Radius Trend

Increases right to left, and top to bottom.

Electronegativity Trend

Increases left to right, and bottom to top, with noble gases excepted.

Strong Acids

Hydrochloric ($HCl$), Perchlorate ($HClO_4$), Nitric ($HNO_3$), Hydrobromic ($HBr$), Hydroiodic ($HI$), and Sulfuric ($H_2SO_4$).

Strong Bases

Hydroxides with alkali metals.

Diatomic Elements

H, O, N, F, I, Cl, Br

Alcohol Group Structure

$$X-OH$$

Amine Group Structure

$$X-NH_2$$

Tetrahedral Molecular Geometry

4 bonds, 0 pairs; bond angle ~$109.5^\text{o}$.

Trigonal Pyramidal Molecular Geometry

3 bonds, 1 pair; bond angle ~$107.5^\text{o}$.

Bent Molecular Geometry

2 bonds, 2 pairs; bond angle ~$104.5^\text{o}$.

Covalent Prefixes (1-8)

1-mono, 2-di, 3-tri, 4-tetra, 5-penta, 6-hexa, 7-septa, 8-octa.