Naming Compounds

TM + NM

  • NM charge = -1 -> NM subscript = roman numeral

  • F, Cl, Br, I

    • same goes for TM + Poly Ion

For charges > -1....

  1. Charge value x NM subscript = total neg charge

  2. l total neg charge l ÷ # metal atoms(subscript) = ROMAN NUMERAL

ex. Mn2O3

  1. O has -2

  2. -2 x 3 = -6

  3. ∣−6∣ ÷ 2 = 3

  4. Therefore, Mn2O3 is Manganese (III) oxide

ex. Fe(OH)3

  1. OH has - neg, so…

  2. Fe(OH)3 is Iron (III) Hydroxide

ex. Ag2Cr2O7

  1. Cr2O7 has -2

  2. -2 × 1 = -2

  3. I-2I ÷ 2 = 1

  4. Therefore, Ag2Cr2O7 is Silver (I) Dichromate

M + NM

M + NM: Ionic - transfer of e-

  • Write metal/cation FIRST

    • both for formula + compound name

  • nm/anion last! Ends w/ -ide

    anion charge + cation charge = 0 ← NEUTRAL!

ex. NaCl

  1.     Sodium = m → +1

  2. Chlorine = nm → -1

  3. Therefore, the name is Sodium Chloride

ex. Fe2(SO4)3

  1. Iron = m → charge tbd

  2. Sulfate = nm (poly ion!) → -2

    2.1 -2 × 3 = -6

  3. I-6I ÷ 2 = 3

  4. Therefore, the name is Iron (III) Sulfate

NM + NM

NM + NM: Covalent - share of e-

  • Less electronegative is first (Based on PT)

  • Most eletroneg last (based on PT); ends w/ -ide

USE PREFIXES!! (study flashcard set)

Acids

Acid - contains H and another element; usually a NM

  1. Start w/ Hydro-

  2. add root of nm

    1. drop n-e -ine or -gen

  3. end w/ “-ic acid”

ex. HCL

  1. Hydro…

  2. Hydrochlor…

  3. Hydrochloric acid

Acids can also contain an POLY ION!!

  • Ion ending dictates acid name

    • -ate = ic acid

    • -ite = ous acid

      • Take the name of poly ion and replace -ate → ic / -ite → ous

        ex. HNO3 → nitrate → nitric acid

ex. H2SO3

  1. SO3 = sulfite ← OUS!

Sulfurous acid!

ex. H3PO4

  1. PO4 = phosphate ← IC!

Phosphoric acid

HOWEVER… for HCN is an exception and follows H + NM