Unit 2 Study

Question 1

Electromagnetic Radiation

Answer 1

Effects electrons and how they behave and change atomic properties(seen as waves of light)

Question 2

How do lights move?

Answer 2

They oscillate until they hit their target

Question 3

Amplitude

Answer 3

Avg distance to maximum peak, λ

Question 4

Frequency

Answer 4

Distance of waves across time Hz(1/s)

Question 5

Speed of light

Answer 5

3(10^8) (s^-1)

Question 6

How to calculate Speed of light, Wavelength, Frequency

Answer 6

c=λv

Question 7

Wave Diffraction

Answer 7

Waves project through a hole instead of going straight through

Question 8

Interference patterns

Answer 8

in phase waves reinforce and expand amplitude(constructive); out of phase waves cancel each other out(destructive)

Question 9

How do interference patterns affect diffraction?

Answer 9

interfering points create concentrated spots, non overlaps create dead zones

Question 10

Photoelectric effect

Answer 10

Light ejects electrons from metal due to the right frequency of EM radiation

Question 11

Photons

Answer 11

Light comes in pockets of energy called photons, energy depends on frequency not intensity

Question 12

How to calculate energy of a photon

Answer 12

E=hv

Question 13

Plancks Constant

Answer 13

6.626 x 10^-34 js

Question 14

Emission Spectrums

Answer 14

only certain wavelengths pass through a substance(achieved by irradiating substance)

Question 15

Absorption spectrum

Answer 15

shows gaps within full light spectrum

Question 16

Bohr Model

Answer 16

fixed planetary model in which you can find the location of an electron(wrong), but stated photons being absorbed or emitted between electrons

Question 17

Energy Diagram

Answer 17

shows energy level/quantum number of electrons

Question 18

Davisson and Germer Expriment

Answer 18

inside a vacuum electron beam hit nickel and showed interference pattern, but differed when observed

Question 19

Wavelength of matter equation

Answer 19

h/mv

Question 20

Atomic Orbitals

Answer 20

show area of 90% electron probability, exist on an xyzzy axis, hold 2 electrons

Question 21

S orbitals

Answer 21

l=0 m=0, spherical

Question 22

P orbitals

Answer 22

l=1 m=-1, 0, 1, dumbell shaped, exist on each axis

Question 23

D orbitals

Answer 23

l=2 m=-2, 0, 1, 2

Question 24

degenerate orbitals

Answer 24

orbitals of the same energy level (ex 2px 2py 2pz)

Question 25

n

Answer 25

principle quantum number

Question 26

L

Answer 26

orbital quantum(n-1)

Question 27

m of f

Answer 27

angular momentum

Question 28

m of s

Answer 28

"spin quantum number" or interaction with magnetic field +1/2 or -1/2

Question 29

Pauli Exclusion Principle

Answer 29

states that no two electrons can occupy the same state(pos or neg) within an orbital

Question 30

Valence Electrons

Answer 30

Determine chemical behavior,

Question 31

ENC

Answer 31

model to understand valence electrons and shows how valence electrons are attracted to nucleus

Question 32

Z of eff

Answer 32

of protons - core electrons

Question 33

ENC trends

Answer 33

increases across a row

Question 34

Coulomb's law and ENC

Answer 34

attractive forces increase across a row and down period groups

Question 35

Atomic Radius

Answer 35

Depends on EM forces, higher ENC results in smaller radius

Question 36

Atomic Radius trends

Answer 36

decreases across a row, increases down a period

Question 37

Ions

Answer 37

atoms with non standard charge due to difference in electrons

Question 38

Cations

Answer 38

Ions removed from vlaence electrons which results in a positive charge, and shrink due to less electron repulsion

Question 39

Oxidation Numbers

Answer 39

expected charges for a group

Question 40

PEW with ions

Answer 40

less electrons lead to a decreased PEW, less PE required to change states

Question 41

Anions

Answer 41

Negative ions(added electrons) increase radii size due to increased electron repulsion

Question 42

Ionization energy

Answer 42

energy required to remove an electron from an atom in the gas phase

Question 43

Ionization energy trends

Answer 43

Increases across a period, decreases down a group, related to Z of eff, always positive

Question 44

Successive ions

Answer 44

more energy required fro each successive electron, massively increases with new orbital group

Question 45

What increases Ionization energy?

Answer 45

Larger ENC, smaller atom size, core electron shells