Nomenclature

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Nomenclature
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• Chemical Formula type of notation made with
  numbers and chemical symbols
• indicates the composition of a compound
• indicates the number of atoms in one molecule
• Molecule - Bonded collection of two or more atoms
  of the same element or different elements
• - monatomic molecule one atom molecules
• - diatomic molecule two atom molecules (seven)
  MEMORIZE
• Br, I, N, Cl, H, O, F

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Nonmetals
METALS

• Metals
• Location Left side of Periodic Table
• Properties Ductile drawn into wires
• Malleable hammered into sheets
• Metallic Luster shine
• Good Conductors of Heat and Electricity
• Nonmetals
• Location Right side of Periodic Table
• Properties Brittle
• Lack Luster not shiny
• Poor Conductors of Heat and Electricity
• Semi-metals
• Location Along Stair-step
• Properties Have properties of metals and
  nonmetals
• also called METALLOIDS Si, Ge, As, Sb,
  Te, Po, At

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Naming

• 1. Ionic Compounds Formed from a metal and a
  non-metal
• When a metallic element combines chemically with
  a non-metallic element to form an ionic compound
  one or more electrons are transferred from each
  atom of the metal to one or more atoms of the
  nonmetal
• charged atom ion
• net charge on compound 0
• Na1 Cl-1 ? NaCl
• Loses Gains compound
• electron electron NO CHARGE
• Cation positive ion metal
• Anion negative ion - nonmetal
• Ions Formed

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Rules for writing formulas for Ionic Compounds

• Binary compound compound formed by two elements
• Tertiary compound - compound formed by more than
  two elements
• Polyatomic ion groups of atoms of more than one
  element that carries a charge
• bound tightly together
• dont break apart during a chemical reaction,
  function as a unit
• 1. Write the symbols cation first, anion
  second
• 2. Determine the charge on the atoms of each
  element
• 3. Select subscripts that make the lowest ratio
• TOTAL POSITIVE CHARGE TOTAL NEGATIVE CHARGE
• When using subscripts with polyatomic ions, the
  formula for the ion is placed in parentheses and
  the subscript is placed outside the parenthesis

Na
1
O
-2
Al
3
S
-2
K
1
SO4-2
Examples Sodium Oxide Aluminum Sulfide
Potassium Sulfate Ammonium Phosphate
Na2O
Al2S3
K2SO4
NH41
PO4-3
(NH4)3PO4
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Naming Ionic Compounds

• Name the Cation first Name of the metal
• the anion is the name of the nonmetal altered by
  adding the suffix -ide to the root word
• chlorine ? chloride
• fluorine ? fluoride
• sulfur ? sulfide
• oxygen ? oxide
• phosphorus ? phosphide
• etc
• Polyatomic name is not altered
• Some metals can form more than one kind of ion
  (Type II)
• Fe, Cu, Co, Sn, Pb, Hg
• Stock System name the metal followed by a roman
  numeral in parenthesis. The Roman numeral tells
  the charge.
• Exception Mercury (I) Hg22
• Examples

I, II, III, IV, V, VI,
NaCl KNO3 MgBr2 CuO Li2SO4 Cu2O K3N Sn
S2

sodium chloride

potassium nitrate

magnesium bromide

copper (II) oxide

lithium sulfate

copper (I) oxide

potassium nitride

tin (IV) sulfide
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Molecular Compounds

• 2. Molecular Compounds (molecules) compounds
  made from two nonmetals
• - electrons are shared by two atoms
• Naming Molecular
• Prefixes (MEMORIZE)
• Mono-1 tetra-4 hepta-7 deca-10
• di-2 penta-5 octa-8
• tri-3 hexa-6 non-9
• prefixes are used with both the first named and
  second named element. Exception mono- is not
  used on the first word
• second word ends in ide
• If a two syllable prefix ends in a vowel, the
  vowel is dropped before the prefix is attached to
  a word beginning with a vowel

monooxide
Writing molecular formulas Translate prefixes
Examples
N2O dihydrogen monoxide Si8O5 tetrasulfur
hexachloride NH3 carbon monoxide P3I10 carbo
n dioxide

Dinitrogen monoxide

H2O

Octasilicon pentoxide

S4Cl6

Nitrogen trihydride

CO

Triphosphorus deciodide

CO2
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Naming Acids

• Acid - has one or more H1 ions attached to an
  anion Second Word is Acid
• If the anion doesnt contain oxygen, the acid is
  named with the prefix hydro- and the suffix ic
  attached to the root
• When the anion contains oxygen, the suffix ic or
  -ous is added
• -ate becomes ic
• -ite becomes ous
• Writing formulas for acids
• Balance charges between H1 and anion.
• Examples

HCl hydroiodic acid HClO3 hydronitric
acid HClO4 nitric acid HClO2 nitrous
acid HClO sulfuric acid

Hydrochloric acid

HI

Chloric acid

H3N

Perchloric acid

HNO3

Chlorous acid

HNO2

hypochlorous acid

H2SO4