1.
"sea of electrons": the constantly moving electrons that give properties to all electons in metals
2.
104.5º: the bent bond angle with 2 lone pairs on central
3.
107º: trigonal pyramidal bond angle
4.
109.5º: tetrahedral bond angle
5.
120º: trigonal planar bond angle
6.
120º: bent bond angle with 1 lone pair on central
7.
180º: linear bond angle
8.
anion: a negatively charged ion
9.
bond energy: energy required to break a chemical bond and form a neutral isolated atom.
10.
bond length: average distance between the two atoms at their lowest potential energy
11.
cation: a positively charged ion
12.
chemical bond: mutual electrical attraction between the nuclei and valence electrons of different atoms that bond them together
13.
chemical formula: indicates the relative numbers
14.
coordinate covalent bond: bond formed from electrons of a given atom
15.
covalent: nonmetal+metalloid
16.
covalent: nonmetal+nonmetal
17.
covalent bond: sharing of electrons
18.
crystal lattice: 3D arrangement of ions held together by electromagnetic attraction forces
19.
diatomic: two atoms will join together
20.
diatomic molecules: 2 atoms of the same element creating a molecule
21.
dipole-dipole: when two dipoles can connect inter-molecularly
22.
dispersion force: weakest intermolecular force that holds nonpolar molecules together
23.
electronegativity: a measure of an atoms ability to attract electrons in a chemical bond
24.
formula unit: the smallest part of an ionicly bonded compound with the properties of that compound
25.
hybrid orbital: orbitals of equal energies produced by the combination of 2 or more orbitals on the same atom
26.
hybridization: mixing of 2 or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies
27.
hydrogen bond: the strongest bond when hydrogen is attracted to nitrogen, oxygen or flourine
28.
intermolecular forces: forces between molecules
29.
Intra-molecular forces: forces between atoms
30.
ionic: metal+nonmetal
31.
ionic: 1.7 and higher
32.
ionic bond: the transfer of electrons
33.
ionic bonding: electrons transferred when positive and negative ions form neutral compounds
34.
lattice energy: energy released when ionic compounds form
35.
lone pairs: electrons not involved with a bond
36.
metallic: metal+metal
37.
metallic bonding: bonding between atoms of metal
38.
metallic bonds: forces between atoms of the same metal
39.
molecular compound: chemical compound whose simplest units are molecules
40.
molecule: a neutral group of atoms that are held together by covalent bonds; smallest part of a covalently bonded compound with the properties of that compound
41.
non polar covalent: 0 to .3 range
42.
nonpolar covalent bond: sharing equally; bonding electrons share equally by the bonded atoms; balanced distribution of electrical charges
43.
octet rule: compounds form so that each each atom, either by gaining, sharing, or losing electrons, has an octet in its S and P shells of the highest energy level (not including H and He)
44.
polar covalent: .31 to 1.69
45.
polar covalent bond: sharing unequally; bonded atoms have an unequal attraction for the shared electron
46.
polyatomic ion: a group of covalently bonded atoms with a charge
47.
resonance structure: molecules or ions that con not be shown with a lewis structure because electrons are always moving
