honors chemistry chemical bonding review

ionic bonding or electrovalent bonding

an electrostatic attraction between oppositely charged ions, an actual transfer of electrons

compounds ionic bonding occurs in

metal and nonmetal, or polyatomic ions

cation

positive ion

elements that become cations

metals

anion

negative ion

elements that become anions

nonmetals

properties of ionic compounds

-high melting point crystalline solid

-usually white, except compounds of transition metals

-brittle

-electrolyte

electrolyte

compounds that don't conduct electricity as solids, but do conduct when melted or dissolved in water

requirement for conducting electricity

charged particles that are free to move around

covalent bonding

a sharing of valence electrons

compounds covalent bonding occur in

two or more nonmetals

product of covalent bonding

molecule

single covalent bond

two atoms share one pair of valence electrons (weakest)

double covalent bond

two atoms share two pairs of valence electrons

triple covalent bond

two atoms share three pairs of valence electrons (strongest)

coordinate covalent bond

one atom donates a pair of electrons for the bond and the other atom mooches

nonpolar covalent bond

a bond in which the electrons are shared equally

polar covalent bond

a bond in which the electrons are shared unequally

macromolecule or network solid

a covalent bond that is an entire crystal lattice instead of just a molecule

properties of covalent bonds

-low melting and boiling points

-at room temperature, they are gases, liquids or low melting point solids

-do not conduct electricity as solids, when melted or when dissolved in water

metallic bonding

the mutual attraction within a metal for each other's loosely held valence electrons

compounds covalent bonding occur in

metals or alloys (blends of metals)

delocalized electrons

loose valence electrons moving through a sea or cloud

properties of metallic bonds (metals)

-malleable

-ductile

-lustrous

-high melting point crystalline solids

-high tensile strength

-good conductors of heat and electricity

intramolecular force

a force inside one molecule (all covalent bonds, stronger)

intermolecular force or van der

Waal

attractions between neutral molecules to make liquids or solids (weaker)

polar molecule (dipole)

molecules that don't have an even distribution of electrical charge

nonpolar molecule

molecules that have an even distribution of electrical charge

dipole-dipole interaction

bond between polar molecules

hydrogen bonding

a type of dipole-dipole interaction, the attraction between hydrogen in one molecule with a highly electronegative element (NOF, strongest)

London force or dispersion force

bond between nonpolar molecules (weakest)

instantaneous dipoles

electrons moving in a molecule that get off balance so one end of the molecule and the other is negative

intermolecular force associated with a nonpolar covalent bond

London bond

intermolecular force associated with a polar covalent bond

dipole-dipole bond

isoelectronic

two elements that have the same electron configuration

elements that metals become isoelectronic to

the noble gas before it on the periodic table

elements that nonmetals become isoelectronic to

the noble gas after it on the periodic table

electronegativity differences for nonpolar covalent bonds

0-0.49

electronegativity differences for polar covalent bonds

0.5-1.69

electronegativity differences for ionic bonds

1.7 or greater