Chemistry Chapter 6 - Atomic Theory II/Periodic Trends

neils bohr

made bohr model of atom

particle theory

newton (relfection/refraction)

wave theory

huygens (diffraction)

what is light? (today)

wave/particle duality

james clerk maxwell

discovered electromagnetic radiation

heinrich hertz

created first radio transmitter and receiver

relationship between wavelength and frequency

inverse relationship

energy and frequency relationship

if one increases so does the other

wavelength

distance from wave to wave

crest

peak of the wave

trough

lowest part of the wave

max planck

energy comes in fixed amounts called quanta

quantum is what

bundle/packet/particle of energy

what is quantum light energy?

photon

einstein

light behaves as particle photoelectric effect

lyman series

n = 1, uv

balmer series

n = 2, vis/uv

paschen series

n=3, IR (infrared)

brackett

n=4, IR (infrared)

probability of finding electron outside nucleus

90%

louis de broglie (1924)

light behaves like particle and wave

werner heisenberg

heisenberg uncertainty principle. cannot know the exact position and momentum of an electron at the same time

erwin schrodinger

wave equation. solutions to wave equation yields quantum numbers.

4 quantum numbers

n = principle lvl. l = sublevel (house) . m = orbital (room). s = spin

s p d f values

1 3 5 7

how many electrons can s orbital hold

2 electrons

p orbital shape

dumbell or figure 8

s orbital shape

sphere

if the electrons are in the same room what is the spin?

opposite spin

stern and gerlach

experimented and discovered spin

pauli exclusion principle

no two electrons can exist in exactly the same quantum state

what are the four subshells

s p d f

what quantum num represents subshell

l

number of orbitals formula

n²

max electron formula

2n²

maximum number of electron in a orbital?

always 2

orbital can be seen as

room, has 2 electrons

electron configuration exception (chromium)

chromium = [Ar] 4s²3d⁴ —→ [Ar] 4s¹3d⁵

electron configuration exception (copper)

copper = [Ar] 4s²3d⁹ —→ [Ar] 4s¹3d¹⁰

electron configuration exception (silver)

silver = [Kr] 5s¹4d¹⁰

electron configuration exception (gold)

gold = [Xe] 6s¹4f¹⁴5d¹⁰

where are valence electrons found

outermost s and p shell

electron configurations of transition metal cations lose electron for valence first

Fe = [Ar] 4s²3d⁶, Fe²⁺ = [Ar] 3d⁶, Fe³⁺ = [Ar] 3d⁵

isoelectronic

want to become like noble gas

atomic radi periodic trend

right to left up to down

chemical reactivity

francium right to left up to down chlorine down to up left to right

as z_eff increases atomic radius ____

decreases

FOR NEUTRAL ATOMS zeff = ____

num of valence electrons

positive to ___ (cations get smaller) negative to ___ (anions get bigger)

lose gain

as zeff increase ionic radius ________

decreases

why do atoms get larger when they gain electrons?

more electron repulsion

shielding effect

larger atom more shielding e- therefore easier to remove last electron

electromagnetic radiation meaning

light behaves as a wave

maxwell’s theory was experimentally verified by ______ using a ________

hertz, spark apperatus

what color on the visible light scale has the lowest wavelength?

violet

what color on the visible light scale has the lowest frequency?

red

frequency units

1/s, s^-1, Hz

what is quantum theory?

light behaves as particle

long wavelength, low freq, low energy electromagnetic spectrum order

radio microwave ir visible uv x-ray

short wavelength, high freq, high energy electromagnetic spectrum order

x-ray uv visible ir microwave radio

quantum level letter

n

n = 1 is known as ______ _____. all others are _______ states

ground state, excited

momentum equals

mass x velocity

for standing waves, each orbit corresponds to a __ _______ wavelenght

de brogili

wave function equals

ψ psi

wave equation can only be solved for _ electron system

1

ψ² equals

probability of finding an electron in a region of space

schrodinger wave equation incorperates ____ and ________ nature of matter

wave, particle

solution to wave equation yields what

quantum numbers

principle quantum number (n) represents

average distance from nucleus

for sublevel (l) l = ______

0 1 2 3

hunds rule is

each orbital is filled with only one electron before the pair up

paramagnetic =

unpaired electron

diamagnetic =

all paired electron

dimitri mendelev organized elements by increase ______ ____

atomic mass

ionization energy general trend

increases up and to the right

electron affinity general trend

increases up and to the right

which group has the lowest IE?

alkali metals

which group has the highest IE?

nobel gas

IE exceptions group 3

group 3 has lower ionization energy than group 2

IE exception group 6

group 6 has lower ionization energy than group 5

half filled subshells are relativley ______

stable

the more ________ the EA, the ____ easily an atom accepts an electron.

positive more

what group has the highest EA

halogens

fluorine has ____ IE and ____ EA

high high