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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)