Chapter 3 Test

Question 1

Rutherford’s Contribution

Answer 1

• Electrons move in space randomly around the nucleus, beehive model
• e- account for the volume of atom
• nucleus accounts for mass of atom

Question 2

Rydberg’s Equation

Answer 2

• En = -RH/n^2
• RH is a constant value
• Calculates energy of e- in an energy level

Question 3

Electromagnetic spectrum concepts

Answer 3

• Radio, micro, infrared, UV, X-Ray, Gamma
• Longer wavelength (lambda) = lower frequency (nu) = lower energy
• Energy is proportional to frequency
• Frequency is inversely proportional to wavelength
• c = λv (c is speed of light, given)

Question 4

Visible length spectrum concepts

Answer 4

• (Red) 700nm to 400 nm (Violet)
• Colours of the rainbow from the least to most energetic: ROYGBIV

Question 5

Discontinuous spectrum

Answer 5

• Quantum: fixed amount of energy
• Energy quantized to specific levels…
• Separation and gaps
• Compare to a staircase

Question 6

Continuous spectrum

Answer 6

• All wavelengths of light are represented
• No gaps
• Compare to a ramp

Question 7

Emmision spectrum

Answer 7

• Spectrum of frequency of EM Radiatoin due to e- moving from high to low energy levels
• e- releases quantum energy as light as it moves down (6 to 1, 5 to 1, …)

Question 8

Emission series

Answer 8

• Different series depending on final energy level value
• Represented through emmision line spectrums for elements
• Lyman series: E(n) to E(n=1) - UV
• Balmer series: E(n) to E(n=2) - Visible
• Paschen series: E(n) to E(n=3) - Infrared Radiation
• Brackett series: E(n) to E(n=4) - Infrared Radiation
  high E –> low E
  Little BAbies Paint BRains

Question 9

Emmission Line Spectrum

Answer 9

• Ladder of energies
• Each element has own signature

Question 10

What are the four quantum numbers?

Answer 10

1. Principle quantum number, n
2. Angular momentum momentum quantum number, l
3. Magnetic quantum number, ml
4. Magnetic spin quantum number, ms

Question 11

Orbit model

Answer 11

• e- travel around nucleus in 2d pathway
• fixed distance
• No evidence exists

Question 12

Orbital model

Answer 12

• Region of probability where e- can be found
• 95% probability to find e-
• Can hold maximum 2 e-
• Different orbitals exist for different energy states, described by quantum numbers

Question 13

Principle quantum number

Answer 13

• Represented by n
• Represents energy level of e-
• Distance between e- and nucleus
• greater n = greater energy

Question 14

Angular momentum quantum number

Answer 14

• Represented by l
• Represents types and shapes of orbitals within each quantum level
• Restriction l<n
• s, p, d, f orbitals! s=0, p=1, d=2, f=3
• s orbitals: 1 spherical orbital (2e- max)
• p orbitals: 3 degenerate perpendicular/dumbbell orbitals (6e- max)
  *d orbitals: 5 degenerate diffuse orbitals (10e- max)
• f orbitals: 7 degenerate fundamental orbitals (14e- max)
• Relative energy of orbitals: s<p<d<f

Question 15

Magnetic quantum number

Answer 15

• Represented by ml
• Indicates 3D orientation/specific plane the e- in an orbital is found in
• Restriction: -l<=ml<=l
• s orbitals have 1 ml = 0
• p orbitals have 3 ml = -1, 0, 1 (x,y,z)
  etc.

Question 16

Magnetic spin quantum number

Answer 16

• Represented by ms
• Direction of e- spin
• Can either be ms = 1/2 (up) or ms = -1/2 (down)
• Each orbital can hold max 2 electrons w/ opposite spin

Question 17

Afbau principle

Answer 17

• e- will fill lowest energy levels before higher ones are filled
• ex: 4s is filled first because it has less energy than 3d
• FOLLOW PERIODIC TABLE TO MAKE DIAGRAM!

Question 18

Pauli exclusion principle

Answer 18

• each orbital holds a max of two e- w opposite spin
• connects with ms
• 2e- of the same spin in one orbital cannot be true

Question 19

Hund’s rule

Answer 19

• When there are degenerate orbitals in a sublevel (ml), electrons will half fill each orbital before pairing up
• e= dont want to be together unless they have to!

Question 19

Electron configuration for ions

Answer 19

• Cation/+: electrons are lost from outermost shell/highest n value from highest energy orbital
• Anions/-: electrons are gained to nearest orbitals that are nolt yet full

Question 20

Paramagnetic

Answer 20

• Elements with unpaired electrons
• attracted to a magnetic field

Question 21

Diamagnetic

Answer 21

• Elements with paired electrons
• Repelled by a magnetic field

Question 22

Ground state

Answer 22

• Valence electrons are found in order we would predict
• 1s2,2s2,2p6, etc
• close to the nucleus as possible

Question 23

Excited state

Answer 23

• Electron configuration is out of order and unpredicted
• energy levels further from the nucleus
• Look for a gap while following periodic table

Question 24

Exceptions to the electron configurations

Answer 24

* Group 6: Chromium (Cr), Molybdenum (Mo) * Group 11: Copper (Cu), Silver (Ag), Gold (Au) * d orbitals become filled (10e-) or half filled (5e-) * s2 orbitals become s1 (loses an e- to a d orbital)