Chemistry 104

Front 1

Octet Rule

Back 1

Tendency of atoms to attain a stable electron configuration of eight valence electrons.

Front 2

Ionic Bonds

Back 2

Occur when the valence electrons of atoms of a metal are transferred to atoms of nonmetals.

Example: NaCl

Front 3

Covalent Bonds

Back 3

Form when atoms of nonmetals share valence electrons.

Example: water

Front 4

Ions

Back 4

Have electrical charges and form when atoms lose or gain electrons to form a stable configuration.

Front 5

Polyatomic Ion

Back 5

A group of covalently bonded atoms that has an overall ionic charge.

Front 6

Molecular Compound

Back 6

Contains two or more nonmetals that form covalent bonds in where valence electrons are shared by nonmetal atoms to achieve stability, thus forming a molecule.

Front 7

Prefixes used in naming molecular compounds:

Back 7

1)mono 2)di

3)tri 4)tetra

5)penta 6)hexa

7)hepta 8)octa

9)nona 10)deca

Front 8

Which elements exist as diatomic molecules?

Back 8

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine.

Front 9

Ions in the body:

Back 9

Sodium, potassium, calcium, magnesium, and chloride ions are present in the body.

Front 10

Double and Triple Bonds:

Back 10

Form when the number of valence electrons is not enough to complete the octets of all the atoms in the molecule. One or more lone pairs of electrons from the atoms attached to the central atom are shared with the central atom.

Front 11

Double Bond

Back 11

Occurs when two pairs of electrons are shared.

Front 12

Triple Bond

Back 12

Three pairs of electrons are shared.

Front 13

Electronegativity

Back 13

Electronegativity of an atom is its ability to attract the shared electrons in a chemical bond. Nonmetals have a higher electronegativities than do metals, because nonmetals have a greater attraction for electrons than metals.