Term | Definition |
these bind together to make molecules | atoms |
chemical bonds | intramolecular strong bond |
intermolecular forces | weaker force |
Octet Rule | atoms tend to bond with other atoms until it has 8 electrons in outermost shell to become stable like Nobles |
What the octet rule doesn't apply to | Hydrogen |
Ionic Bonding | e- transferred from atom with low IE to atom with high electron affinity; electrostatic forces |
Covalent Bonding | electrons are shared btwn 2 atoms; can be single double or triple |
Polar Covalent Bonding | partially covalent and partially ionic bonding |
Cation | loses e- and becomes |
Anion | gains e- and becomes |
Bond Order | number of shared electrons between atoms (1,2,3 for single double triple) |
Bond Length | avg distance btwn the 2 nuclei of atoms involved; the more e- shared, the shorter the BL |
Bond E | E required to separate 2 atoms |
bonding electrons | shared e- of covalent bond |
nonbonding electrons | e- not involved in covalent bond |
lone e- pairs | unshared e- pairs |
Lewis Structure | chemical symbol of an element surrounded by dots, each representing a valence e- |
Steps to Lewis Structure | 1. draw skeletal structure, least electronegative in middle, halogens and hydrogen on ends
2. Count up the valence electrons
3. complete octets
4. Shared e- are lines, lone pairs are dots |
Formal Charges | V-1/2bonding-nonbonding; or if it is missing a valence e- then +1 and vice versa |
Resonance | two or more nonidentical Lewis structures for a molecule |
Resonance Hybrid | the actual molecule is a mix of the resonance structures |
Polar Covalent Bond | like HCL and H2O, partially ionic character |
NonPolar Covalent Bond | H2, Cl2, O2 |
Lewis Acid | can accept electrons to form covalent bond |
Lewis Base | can donate lone pair of electrons to form covalent bond |
VSEPR determines | geometry of molecules |
Linear | 2 regions of electron density, 180 degrees |
Trigonal Planar | 3 regions of electron density, 120 degrees |
Tetrahedral | 4 regions of electron density, 109.5 degrees |
Trigonal Bipyramidal | 5 regions of electron density, 180-120-90 degrees |
Octahedral | 6 regions of electron density, 180-90 degrees |
Axial | elements up and down |
Equitorial | elements on "equator" of molecules surrounding central atom |
1 lone pair on a trigonal planar molecule | bent shape |
1 lone pair on tetrahedral molecule | trigonal pyramid |
2 lone pairs on tetrahedral molecule | bent shape |
1 lone pair on trigonal bipyramid | Seesaw shape |
2 lone pairs on trigonal bipyramid | T-shape |
3 lone pairs on trigonal bipyramid | linear |
1 lone pair on octahedral | square pyramid |
2 lone pairs on octahedral | square planar |
3 lone pairs on octahedral | T-shape |
4 lone pairs on octahedral | linear |
A polar bonding molecule must have what to be polar | net dipole moment or else it is nonpolar |
l = 0, 1, 2, 3 | s, p, d, f |
m | +l to -l |
s | sphere shape |
p | peanut shape |
when orbitals have same sign | bonding orbitals |
when orbitals have opposite signs | nonbonding orbitals |
when orbitals overlap head to head | sigma bond |
when orbitals overlap parallel | pi bond |
Dipole-Dipole Interaction | when 2 polar molecules come into close contact with each other; pos of one close to neg of other |
H-Bonding | F O N; strongest |
Dispersion Forces | short-lived dipoles; large molecules have greater forces, also London Force |