ap chem ch. 7

thompson

plum pudding model

rutherford

sea of electrons

bohr

planetary model

wave velocity =

frequency*wavelength

emission line spectrum

shows how many times an electron transitioned from a higher to lower energy state; more lines means more energy

electromagnetic spectrum

balmer series

shows visible light

s sublevel

sphere shaped, 1 orbital

p sublevel

dumbbell shaped, 3 orbitals (px, py, pz), all the dumbbells together form a sphere

d sublevel

clover shaped, 5 orbitals, all the clovers together forms a sphere

f sublevel

flower shaped, 7 orbitals, all the flower

hund's rule

electrons fill unoccupied degenerate orbitals before pairing

pauli's exclusion principle

no two electrons can have the same 4 quantum numbers

plank's hypothesis

worked with electromagnetic waves; E = hv = plank's constant * frequency

plank's constant

6.626x10^-34

atomic spectra

produced when an electron moves from a higher to lower energy level, giving off light in the process; delta E = Ehi - Elo = hv = h*c/λ

bohr model

electrons move around the nucleus with a fixed radius, they absorb energy as as they get farther from the nucleus, and gives off energy yas it gets closer to the nucleus. this resulted in the emission spectra, which only happens as certain visible wavelengths.

wave/particle duality

- plank said waves can act like particles
- de broglie said E = hv = mc^2
- experiments can only demonstrate one of these particles at a time
- hiesnburg uncertainty principle: the momentum & position of a particle cannot be known at the same exact time. therefore, we can only refer to the probability of finding an electron in a region; we cannot specify the path

schrodinger

wave equations (ψ2) can be used to predict the region of probability for locating an electron

particle behavior

photoelectric effect (solar powered calculator)

wave behavior

refraction (changes speed in different media), defraction (bends around barriers), reflection

exceptions to the auf bau

electron promotion; an electron can be promoted from the s sublevel to the d sublevel for stability (half or full)

elements in the same group have

similar chemical properties & outer electron config

elements in the same period have

similar physical properties

coulombs law

strength of a bond

types of bonds

strong nuclear, weak nuclear, electromagnetic, gravitational

periodic trends

explained by Z effective force (how strong the nucleus is); represented by the numerator (q1 * q2)

groups trends

explained by quantum energy & shielding effect - electron penetration; represented by the denominator (r^2)

trends of the periodic table

shielding effect

the attraction between outer electrons and the nucleus decreases as the number of electrons between them and the nucleus increases, causing bonding situations

Z effective force

how strong a nucleus is; # of protons - # core electrons

ionization energy

the energy required to remove one electron from one gaseous atom

electron affinity

atoms ability to attract additional electrons; metals have a high electron affinty, non-metals have a low electron affinty

multiple ionization energies

looking at the table - remove valence electrons take less energy and removing core electrons take a lot more energy, as they are more stable. 2nd and 3rd ionization energys can give clues as to the atomic structure