Types of Chemical Bonds and Properties

Front

Ionic Bond

Back

Metal and Nonmetal

Transfer electrons

Very strong (forms crystals)

High melting and boiling points

Electronegativity difference greater than 1.7

dissolves in polar

Conducts electricity when dissolved

Example: Salt

Front

Polar Covalent Bond

Back

2 or more nonmetals

Lower melting and boiling point than ionic but higher than nonpolar

Unequal sharing of electrons

dissolves in polar

Electronegativity difference 0.3-1.7

Example: Water (H2O), Sugar

Front

Nonpolar covalent bond

Back

2 or more nonmetals

equal sharing of electrons

very low melting and boiling points

dissolves in nonpolar

electronegativity difference 0-0.3

Examples: diatomic molecules, oil, wax, grease

Front

Oxidation Number (Charge)

Back

determine by the number of electrons lost or gained.

Positive charge indicating losing electrons.

Negative charge indicating gaining electrons.

Front

Cation

Back

Ion with a positive charge.

Formed by losing valence electrons.

Charge is equal to the number of electrons lost.

+1 = lose 1 e-

+2 = lose 2 e-

+3 = lose 3 e-

When naming, write the name exactly as it appears on the periodic table

Front

Anion

Back

Ion with a negative charge. Charge determined by the number of electrons gained.

-1 = 1 e- gained

-2 = 2 e- gained

-3 = 3 e- gained

Named by changing the ending to -ide

Front

Diatomic molecules

Back

There are 7 on the periodic table: N2, O2, F2, Cl2, Br2, I2, and H2. They are nonpolar covalent.

Front

Transition metals

Back

Found in the middle of the periodic table.

The d block elements.

Have multiple oxidation numbers and therefore must have roman numerals when named.

Front

Electronegativity

Back

ability to attract electrons

Used to determine bond type by calculating the difference in the value between the atoms

Front

Roman Numerals

Back

Used when naming a transition metal because they have multiple oxidation states