chem H ch. 8 3/7

molecule

a group of two or more atoms held together by chemical bonds

covalent bond

• shared valence electrons between two atoms

• non-metals or non-metal & metalloid

ionic bond

• transferred valence electrons between two atoms

• metal & non-metal

electronegativity

• measure of an atom’s ability to attract shared electrons toward itself in a chemical bond

• determines whether it’s polar or non-polar

polar covalent bond

• two atoms unequally share valence electrons, giving the 2 atoms partial charges

non-polar covalent bond

• two atoms equally share valence electrons, giving the atoms no partial charges

prefixes: 1 atom

mono

prefixes: 2 atoms

di

prefixes: 3 atoms

tri

prefixes: 4 atoms

tetra

prefixes: 5 atoms

penta

prefixes: 6 atoms

hexa

prefixes: 7 atoms

hepta

prefixes: 8 atoms

octa

prefixes: 9 atoms

nona

prefixes: 10 atoms

deca

ous

ending for when an acid ends in “ite”

ic

ending for when an acid ends in “ate”

hydroic

begining & ending for when an acid ends in “ide”

ic

ending for when an acid is monoatomic (ex: HCl —> hydrochlor acid)

single bond

weakest bond

triple bonds

highest dissociation energy

resonance structures

different ways atoms can bond together (all possible combinations)

VSEPR theory

states that 2D Lewis structures can be used to predict 3D molecular geometry fo covalent bonds

linear

• same ions on each side of the central element (180 degrees)

trigonal planar

• 3 ions of the same type (120 degrees)

bent

• 1 lone pair of electrons and two of the same element (104.5 degrees)

tetrahedral

• 4 bonds with no lone pairs and atoms are located at the 4 corners (109.5 degrees)

trigonal pyramidal

• 1 lone pair of electrons (107 degrees)