U3 Chem H. - Fung

a particle that holds a quantum of light/electromagnetic radiation

Single unit of energy (quanta is the plural form)

1. height of wave from origin to peak (m)

2. distance from crest to crest (m)

3. how fast the wave oscillates (Hz)

long-wavelength = low frequency

short-wavelength = high frequency

inversely proportional

smaller mass = longer waves (more observable)

bigger mass = shorter waves (less observable)

1. form of electromagnetic radiation

2. moving through space (when energy is being transmitted)

3. interacting with matter (can only be absorbed by electrons in quanta)

wavelike behavior of particles

1. continuous

2. discrete

it’s impossible to know the position and moment of particles exactly

n = 1

when electron absorbs energy and moves up an energy level

a light-hitting metal experiment that proved that electrons can only absorb specific amounts of energy, aka, quanta, aka, photons of light

1. x 10^-3

2. x 10³

3. x ^10^6

4. x10^9

1. Hz

2. m

3. J

E = 1.78 × 10^-27 J

5.50 × 10^14 Hz

Don’t forget units!

E = 4.1 × 10^-19 J

Wavelength = 4.87 × 10^-7 m

don’t foget units!!

5.0 × 10^ 22 photons

Frequency

distribution of electrons among orbitals

an electron absorbs a certain quanta of energy → moves into a certain higher energy level

an electron loses certain quanta of energy and emits light → moves down energy levels

orbital where the electron is located (its sublevel)

1. Electrons have orbits (clear, determined paths) dictated by quanta

2. Treats the election as a wave: Electrons have orbitals— where the electron is most likely to be based on its principal energy level— but can vary in shape by sublevels (s, p, d, etc)

the energy change of the electron

Aufbau: Electrons occupy lowest levels first (Aufbau, like ‘A’ B C)

Pauli Exclusion:: Orbitals can hold at most 2 electrons, only if they spin in opposite directions (Pauli, like “pair”)

Hund’s: Single electrons fill up as many orbitals in a level as possible before doubling up

1. Find your element on the table (K = Potassium)

2. Go through all the elements before your element and write down their orbital + amnt of elecs in that orbital, aka, how many elements in that group

a: 1s²+2s²+2p^6+3s²+3p^6+4s^1

1. Find your element on the table (K = Potassium)

2. Go up one row and all the way to column 18 to find your noble gas and box it [Ar]

3. After your noble gas, continue the configuration until you reach your element

   • continue config by adding each orbital for each element (K, after Ar, is s1) (you can know what sublevel is each element based on where it is on the periodic table)

a: [Ar] 4s1