Exam 1

2 bonding groups, 0 lone pairs

2 bonding groups, 0 lone pairs

linear, 180

3 bonding groups, 0 lone pairs

trigonal planar, 120

2 bonding groups, 1 lone pair

trigonal planar, bent, <120

4 bonding groups, 0 lone pairs

tetrahedral, 109.5

3 bonding groups, 1 lone pair

tetrahedral, trigonal pyramidal, <109.5

2 bonding groups, 2 lone pairs

tetrahedral, bent, <109.5

5 bonding groups, 0 lone pairs

trigonal bipyramidal, 120 (equatorial) and 90 (axial)

4 bonding groups, 1 lone pair

trigonal bipyramidal, seesaw, <120 (equatorial) and <90 (axial)

3 bonding groups, 2 lone pairs

trigonal bipyramidal, t-shaped, <90

2 bonding groups, 3 lone pairs

trigonal bipyramidal, linear, 180

6 bonding groups, 0 lone pairs

octahedral, octahedral, 90

5 bonding groups, 1 lone pair

octahedral, square pyramidal, <90

4 bonding groups, 2 lone pairs

octahedral, square planar, 90

Rutherford

gold foil experiment showed that an atom is mostly empty space and that electrons orbit in a mostly fixed path

Thompson

cathode ray tube showed that all atoms contain electrons

Millikan

oil drop experiment to determine charge of electron

Bohr

electrons orbit the nucleus at a certain distance and lead to discovery of orbitals and shells

double slit experiment

lead to the idea that light can behave as a wave cause an interference pattern

photoelectric effect

when light is shined onto a metal, sometimes it emits electrons

ionic bond

between a metal and a non-metal EN is greater than 1.7

covalent bond

two atoms have to share electrons completely, EN is less than 0.4

polar covalent bond

two atoms of different electronegativities share electrons, EN is between 0.4 and 1.7

Degenerate

systems that are equal in energy

Shielding

valence electrons don't feel full charge of core electrons because of electrons in between

Penetration

higher probability to be found inside the atom's core region

ground state

the lowest energy of an atom or particle

periodic trends in atomic radius

down- radius increases across- radius decreases

periodic trends in first ionization energy

down- energy decreases across- energy increases

periodic trends in electron affinity

not much of a trend among group 1A becomes more positive down and more negative to the right

first ionization energy

the energy required to remove the first electron from an atom

Z effective formula

atomic number-valence electrons

light equation

c = λv

energy of a photon equation

E=hv (frequency)

valence bond theory

the idea that covalent bonds are formed when orbitals of different atoms overlap

molecular orbitals

orbitals that apply to the entire molecule