Chm Unit 1.2 Final Review

Chm Unit 1.2 Final Review

Mr. Mendoza

Chm.1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties.

• Chm.1.2.1 Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds.

• Chm.1.2.2 Infer the type of bond and chemical formula formed between atoms.

• Chm.1.2.3 Compare inter- and intra- particle forces.

• Chm.1.2.4 Interpret the name and formula of compounds using IUPAC convention.

• Chm.1.2.5 Compare the properties of ionic, covalent, metallic, and network compounds.

Chm.1.2.1

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

Lewis Dots

Bonds

Lewis Dot Structures

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

Covalent

Nonmetal to Nonmetal

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

Metallic

Metal to Metal

Sea of electrons

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

luster.

Ionic

Metal and Nonmetal

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

either in molten state or in aqueous solution.

Chm.1.2.2

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

EN

Name that bond looking at the PT

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

Name that bond looking at the PT

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.

Chm.1.2.3

Compare inter- and intra- particle forces.

IMF

Bonds

IMF

Forces that exist between molecules.

intermolecular forces are weaker than ionic, covalent or metallic bonds

Dipole Dipole

Hydrogen Bond

London Dispersion

Bond Length

Single Bonds long strong

Double Bonds- are stronger than single bonds

Triple bonds-shorter than double bonds

Chm.1.2.4

Interpret the name and formula of compounds using IUPAC convention.

Binary compounds of two nonmetals

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

Binary compounds of metal/nonmetal

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).

Examples

NaCl- Sodium chloride

AlBr₃-Aluminum Bromide

Ca₃P_2-Calcium phosphide

Ternary compounds (polyatomic ions)

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

Examples

Ca(NO₃)₂-Calcium nitrate

Mg(BrO₃)₂-Magenisum Bromate

K₃PO₄-Potassium phosphate

Acids

HCl- Hydrochloric Acid

HNO_3-Nitric Acid

H₂SO_4-Sulfuric Acid

HC₂H₃O₂- Acetic Acid

(CH₃COOH)-Acetic Acid

Chm.1.2.5

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

VSEPR Theory

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