ap chem ch. 7

plum pudding model

sea of electrons

planetary model

frequency*wavelength

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

shows visible light

sphere shaped, 1 orbital

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

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

flower shaped, 7 orbitals, all the flower

electrons fill unoccupied degenerate orbitals before pairing

no two electrons can have the same 4 quantum numbers

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

6.626x10^-34

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

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.

• 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

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

photoelectric effect (solar powered calculator)

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

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

similar chemical properties & outer electron config

similar physical properties

strength of a bond

strong nuclear, weak nuclear, electromagnetic, gravitational

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

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

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

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

the energy required to remove one electron from one gaseous atom

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

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