Chemical bonding

Chemical bonding study terms

covalent bond

A chemical bond formed when two atoms share electrons

ionc bond

The attraction between oppositely charged ions; bond in which electrons are transferred

Bohr Model

More detailed model of atom showing protons, neutrons, and electrons in different energy levels

Lewis structure

A more simple representation of atoms that only show and elements symbol, valence electrons, and bonds

Single bond

a covalent bond in which two atoms share one pair of electrons (two total)

Double bond

A chemical bond formed when atoms share two pairs of electrons (four total)

Triple bond

The strongest and shortest covalent bond

Ionic properties

high melting points, soluble in water, no odor, usually solid, hard, conducts electricity in solution

Soluble

capable of being dissolved

covalent properties

lower melting points, solid liquid or gas, softer, doesn't conduct electricity

polar covalent bond

A covalent bond in which electrons are not shared equally

nonpolar covalent bond

a covalent bond in which the electrons are shared equally by the two atoms, or the molecular shape balances the direction of the charge.

H2O

Example of a molecule that has polar covalent bonds

O2

Example of a nonpolar covalent double bond

N2

Example of a nonpolar molecule that has triple bonds

CO2

This molecule is nonpolar due to its shape

valence electrons

The electrons in the outermost energy level of an atom that influence how an element will react with other substances. Elements of the same group have the same number of valence electrons.

Electronegativity

How strongly an atom attracts electrons. Same trend as ionization energy where Fr is the lowest, and Fluorine has the hightest.

Metallic elements

Can for ionic bonds with nonmetal, or metallic bond with other metals

Nonmetals

Can form ionic bonds with metals, or covalent bonds with other nonmetals

1:1

Bond ratio with elements from groups 1 & 7 form an ionic compound (also 2 & 6)

1:2

Bond ratio with elements from groups 1 & 6 form an ionic compound (also 2 & 7)

+1

Charge of group 1 ions

+2

Charge of group 2 ions

-1

Charge of group 7 ions

-2

Charge of group 2 ions

Group 7 elements

Need one single bond

Group 6 elements

Need two single bonds, or one double bond

Group 5 elements

Need three single bonds, or one triple bond

Organic compounds

contain carbon and hydrogen atoms

Metallic bonds

the forces of attraction between the free-floating valence electrons and the positively charged metal ions

Carbon

Forms the central chain in organic molecules; C needs 4 bonds to become stable