chemistry x English - glossary, names and terminology

The chemistry nomenclature has to be memorized. A system of rules mostly determined by the IUPAC.

polyatomic ions

Polyatomic ions are some atoms grouped together, and they have some charge on it.

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I hear you asking. Yes, it hurts, but remember some of them please.

Ion Name	Formula	Charge
Ammonium	$\mathrm{N}{\mathrm{H}}_4{}^{+}$	+1
Hydroxide	$\mathrm{OH}{}^{-}$	-1
Nitrate	$\mathrm{N}{\mathrm{O}}_3{}^{-}$	-1
Nitrite	$\mathrm{N}{\mathrm{O}}_2{}^{-}$	-1
Carbonate	$\mathrm{C}{\mathrm{O}}_3{}^{2-}$	-2
Sulfate	$\mathrm{S}{\mathrm{O}}_4{}^{2-}$	-2
Sulfite	$\mathrm{S}{\mathrm{O}}_3{}^{2-}$	-2
Phosphate	$\mathrm{P}{\mathrm{O}}_4{}^{3-}$	-3
Phosphite	$\mathrm{P}{\mathrm{O}}_3{}^{3-}$	-3
Bicarbonate	$\mathrm{HC}{\mathrm{O}}_3{}^{-}$	-1
Perchlorate	$\mathrm{Cl}{\mathrm{O}}_4{}^{-}$	-1
Chlorate	$\mathrm{Cl}{\mathrm{O}}_3{}^{-}$	-1
Chlorite	$\mathrm{Cl}{\mathrm{O}}_2{}^{-}$	-1
Hypochlorite	$\mathrm{ClO}{}^{-}$	-1
Acetate	${\mathrm{C}}_2{\mathrm{H}}_3{\mathrm{O}}_2{}^{-}$ or $\mathrm{C}{\mathrm{H}}_3\mathrm{COO}{}^{-}$	-1
Cyanide	$\mathrm{CN}{}^{-}$	-1
Chromate	$\mathrm{Cr}{\mathrm{O}}_4{}^{2-}$	-2
Dichromate	$\mathrm{C}{\mathrm{r}}_2{\mathrm{O}}_7{}^{2-}$	-2
Permanganate	$\mathrm{Mn}{\mathrm{O}}_4{}^{-}$	-1

covalent compounds

Covalent compounds are two nonmetal elements bonded.

• The element order is C-P-N-H-S-I-Br-Cl-O-F, which is mostly sorted by increasing electronegativity.
• Prefixes to show the amount of the element, mono- prefix needed for the second element if singular.
• Change the ending of the second element to -ide.

Examples.

• $\mathrm{CO}$, 1 carbon + 1 oxygen = carbon monoxide
• ${\mathrm{P}}_2{\mathrm{O}}_5$, 2 Phosphorus + 5 Oxygen = diphosphorus pentoxide

ionic compounds

Ionic compounds have one metal and one nonmetal.

• Name the metal cation first (a cat has paw-sitive charge), then the nonmetal anion second.
• Change the ending of the nonmetal to -ide.

Examples.

• $\mathrm{NaCl}$, sodium + chlorine = sodium chloride
• $\mathrm{MgO}$, magnesium + oxygen = magnesium oxide

acids

An acid molecule donates protons (aka ${\mathrm{H}}^{+}$ atoms) to a base molecule.

binary acids

A binary acid is hydrogens bonded to a nonmetal.

• The name of the acid is hydro-nonmetal-acid.

Examples.

• $\mathrm{HCl}$, hydrogen + chlorine = hydrochloric acid
• $\mathrm{HBr}$, hydrogen + bromine = hydrobromic acid
• ${\mathrm{H}}_2\mathrm{S}$, 2 hydrogen + sulfur = hydrosulfuric acid

oxyacids

An oxyacid is hydrogens bonded to a polyatomic ion that has oxygen.

• If polyatomic ends in -ate, make the ending -ic acid.
• If polyatomic ends in -ite, make the ending -ous acid.

Examples.

• $\mathrm{HN}{\mathrm{O}}_3$: Contains the Nitrate ion ($\mathrm{N}{\mathrm{O}}_3{}^{-}$). Nitrate $\to$ Nitric acid
• $\mathrm{HN}{\mathrm{O}}_2$: Contains the Nitrite ion ($\mathrm{N}{\mathrm{O}}_2{}^{-}$). Nitrite $\to$ Nitrous acid
• ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$: Contains the Sulfate ion ($\mathrm{S}{\mathrm{O}}_4{}^{2-}$). Sulfate $\to$ Sulfuric acid
• ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_3$: Contains the Sulfite ion ($\mathrm{S}{\mathrm{O}}_3{}^{2-}$). Sulfite $\to$ Sulfurous acid
• ${\mathrm{H}}_3\mathrm{P}{\mathrm{O}}_4$: Contains the Phosphate ion ($\mathrm{P}{\mathrm{O}}_4{}^{3-}$). Phosphate $\to$ Phosphoric acid

special names

• Water: ${\mathrm{H}}_2\mathrm{O}$
• Ammonia: $\mathrm{N}{\mathrm{H}}_3$
• Methane: $\mathrm{C}{\mathrm{H}}_4$
• Acetic Acid (the acid in vinegar): $\mathrm{C}{\mathrm{H}}_3\mathrm{COOH}$ (or $\mathrm{H}{\mathrm{C}}_2{\mathrm{H}}_3{\mathrm{O}}_2$)
• Hydrogen Peroxide: ${\mathrm{H}}_2{\mathrm{O}}_2$
• Nitrous Oxide (Laughing Gas): ${\mathrm{N}}_2\mathrm{O}$
• Table Salt (or Common Salt): $\mathrm{NaCl}$
• Baking Soda (or Sodium Bicarbonate): $\mathrm{NaHC}{\mathrm{O}}_3$
• Benzene: ${\mathrm{C}}_6{\mathrm{H}}_6$
• Formaldehyde: $\mathrm{C}{\mathrm{H}}_2\mathrm{O}$ (often written as $\mathrm{HCHO}$)
• Glucose: ${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6$