electrons (ew) and light

Question 1

Heisenberg’s uncertainty principle

Answer 1

we can’t pinpoint exactly where an electron is or how fast it’s moving but we can predict with >90% certainty the probability the region where the electron might be

Question 2

energy levels

Answer 2

1, 2, 3, 4, etc.
- describes the average distance of an electron from the nucleus
- energy increases as you move farther away from nucleus
- within each energy level, electrons occupy sublevels (spdf)
- energy levels and types of sublevels match

Question 3

What is the max number of electrons in each energy level?

Answer 3

1. -2
2. 8
3. 18
4. 32

Question 4

Aufbau principle

Answer 4

electrons occupy orbitals that need the least amount of energy first

Question 5

Pauli exclusion principle

Answer 5

orbitals can hold at most 2 electrons and they must have opposite spins

Question 6

Hund’s rule

Answer 6

in a sublevel with more than 1 orbital, put 1e- into each orbital before putting 2e- into any one orbital to minimize -/- repusion between electrons (take your own seat on a bus before you have to share a seat)

Question 7

Where are the spdf blocks on the periodic table?

Answer 7

• s is He and groups 1 and 2
• d is 3-12
• p is 13-18
• f is rare earth metals

Question 8

electromagnetic spectrum

Answer 8

contains all types of light waves

Question 9

light equations

Answer 9

c=wavelength x frequency (c is 3 x 10^8)

energy=frequency x planck’s constant
(planck’s constant is 6.626 x 10^-34)