Chm Unit 1.2 Final Review

Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds.

Lewis Dots

Bonds

used to show how the electrons are arranged around individual atoms in a molecule

Nonmetal to Nonmetal

low MP, low BP, poor electrical conductivity, polar nature

Metal to Metal

Sea of electrons

high MP, high BP, high conductivity, malleability, ductility, and

luster.

Metal and Nonmetal

high MP, high BP, brittle, and high electrical conductivity

either in molten state or in aqueous solution.

Infer the type of bond and chemical formula formed between atoms.

EN

A bond is predominately ionic by the location of the atoms on the Periodic Table (metals combined with nonmetals) or
when  $\Delta$   EN > 1.7

A bond is predominately covalent by the location of the atoms on the Periodic Table (nonmetals combined with nonmetals)
or when  $\Delta$  EN < 1.7.

Compare inter- and intra- particle forces.

IMF

Bonds

Forces that exist between molecules.

intermolecular forces are weaker than ionic, covalent or metallic bonds

Dipole Dipole

Hydrogen Bond

London Dispersion

Single Bonds long strong

Double Bonds- are stronger than single bonds

Triple bonds-shorter than double bonds

Interpret the name and formula of compounds using IUPAC convention.

The first element is given its element name; the second is given its root (hydr, bor, carb, ox, fluor, etc.) followed by ide

HF- Hydrogen Fluoride

NO₂- Nitrogen Dioxide

P₂O₅-Phosphorous Pentoxide

Metals combine with nonmetals to give ionic compounds. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide).

Name the cation first (specifying the charge, if necessary), then the polyatomic ion as listed in the table above (or as derived from the rules which were given).

Do NOT use prefixes to indicate how many of each element is present

Ca(NO₃)₂-Calcium nitrate

Mg(BrO₃)₂-Magenisum Bromate

K₃PO₄-Potassium phosphate

HCl- Hydrochloric Acid

HNO_3-Nitric Acid

H₂SO_4-Sulfuric Acid

HC₂H₃O₂- Acetic Acid

(CH₃COOH)-Acetic Acid

Compare the properties of ionic, covalent, metallic, and network compounds.

Valence Shell Electron Pair Repulsion Theory: can be used to predict the shapes of many molecules and polyatomic ions