Electrons

Question 1

Organization of the Electron Cloud

Answer 1

Principal Energy Level (P.E.L.)
Sublevels
Orbitals
Electrons
Different spins

Question 2

Pauli Exclusion Principle

Answer 2

No two electrons can have the same location
No two electrons can have the same set of quantum numbers (electrons adress)

(n, L, m, s)
n = P.E.L.
L = Sublevel
m = Orbital
s = Spin

Question 3

P.E.L. (n)

Answer 3

Main energy levels
Distance from the nucleus
Labeled with numbers
Ex. n=1, n=2….n=7
Further the distance the higher the energy

Question 4

Sublevels (L)

Answer 4

The # of sublevels is equal to the P.E.L. number
Ex. 1st P.E.L. has 1 sublevel, etc
Max of 4 sublevels
Labeled with letters (s, p, d, f)

Question 5

s Sublevel

Answer 5

Lowest in energy
Has 1 orbital (sphere shaped)
Holds up to 2 electrons

Question 6

p Sublevel

Answer 6

Higher in energy than s sublevel
Has 3 orbitals (each is dumbbell shaped)
Holds up to 6 electrons

Question 7

d Sublevel

Answer 7

Higher in energy than both s and p sublevels
Has 5 orbitals (each is a complex and different shape)
Holds up to 10 electrons

Question 8

f Sublevel

Answer 8

Highest in energy
Has 7 orbitals (each have complex shape)
Holds up to 14 electrons
Only used in P.E.L. #4-7

Question 9

Aufbau Principle

Answer 9

Lowest energy sublevel is the 1st to be filled with orbitals

Question 10

1st P.E.L.

Answer 10

s sublevel
1 orbital
2 electrons

Question 11

2nd P.E.L.

Answer 11

s, and p sublevels
1, and 3 orbitals (4 overall)
2, and 6 electrons (8 overall)

Question 12

3rd P.E.L.

Answer 12

s, p, and d sublevels
1, 3, and 5 orbitals (9 overall)
2, 6, and 10 electrons (18 overall)

Question 13

4th P.E.L.

Answer 13

s, p, d, and f sublevels
1, 3, 5, and 7 orbitals (16 overall)
2, 6, 10, and 14 electrons (32 overall)

Question 14

Electron Configurations

Answer 14

Sorting ALL the sublevels and electrons of an atom from lowest energy to highest energy.

Question 15

Valence Electrons

Answer 15

Outermost electrons (located in the LAST energy shell)
Ex. Carbon (C) = 1s^2 2s^2 2p^2
|______|—> valence energy level
Valence electron amount measured by the last two in the electron configuration (2s^2 2p^2) In the ex. above there are 4 valence electrons

Question 16

Octet Rule

Answer 16

ALL* elements want 8 valence electrons
Elements with 8 valence electrons are the most stable

• there are only 4 elements that do not want 8 valence electrons (hydrogen, beryllium, helium, boron)

Question 17

Hund’s Rule

Answer 17

Fill empty orbitals first

Question 18

Excited / Base States

Answer 18

1. Electrons absorb energy (heat OR electricity) and jump to a higher energy level AWAY from the nucleus
2. Electrons that have moved to higher energy levels are described as “Excited State Electrons”
3. These unstable electrons can not maintain the excited state and immediately return to the lowest energy level possible and is called “The Base State”

When an electron returns to its base state it will emit or give off the same amount of energy it had absorbed, and an Electromagnetic Wave (E.M. Wave) is produced

Question 19

Wavelength and Frequency

Answer 19

Wavelength -
Distance from crest -> crest, OR trough -> trough
Measured in meters OR nanometers

Frequency -
Symbol = f
Measured in hertz (Hz), the # of wavelengths that pass a given point in a unit of time

Relationship -
Shorter the wavelength = higher the frequency (inverse)
Higher the frequency = higher the energy (direct)

Question 20

Electromagnetic Spectrum

Answer 20

A family of waves all caused by vibrations of electrons

Question 21

Energy of a Wave

Answer 21

E = H * f
H = Planck’s constant (6.63 * 10^-34 J/s)
Measured in joules (J)

Question 22

Spectroscopy

Answer 22

“The study of the emission of electromagnetic waves”

Question 23

Continuous Spectrum

Answer 23

All wavelengths inside a certain range
Make up the visible light spectrum (ROYGBIV)

Question 24

Bright Line Spectrum

Answer 24

Various bright colors representing individual wavelengths