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CHEM1110 > FINAL - SECTION 1 > Flashcards

FINAL - SECTION 1 Flashcards

1
Q

zA Z P

A

A = atomic mass
Z = atomic symbol
P = number of protons

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2
Q

Frequency (v)

A

Number of cycles per second (s-1)

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3
Q

Wavelength (λ)

A

Distance wave travels in 1 cycle (nm)

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4
Q

Amplitude

A

Height of crest of wave

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5
Q

Relationship between frequency and wavelength

A

Inversely proportional (small freq = big wavelength, big freq = small wavelength)

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6
Q

Rank electromagnetic spectrum from lowest energy (big wavelength) to high energy (small wavelength)

A
  1. Radio (10^5-10^-1)
  2. Microwave (10^-1-10^-3)
  3. Infrared (10^-3-10^-6)
  4. Visible light (10^-6-10^-7)
  5. UV (10^-7-10^-9)
  6. X ray (10^-9-10^-11)
  7. Gamma ray (10^-11-10^-15)
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7
Q

Which ER has longest wavelength (small freq)

A

Radio

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8
Q

Which ER has smallest wavelength (largest freq)

A

Gamma ray

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9
Q

Rank visible light from low energy (big wavelength) to high energy (small frequency)

A
  • Red
  • Orange
  • Yellow
  • Green
    -Blue
  • Violet
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10
Q

Relationship between visible light and color

A

Amplitude determines brightness, frequency/wavelength determines color

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11
Q

Important equations (5)

A
  • c = λv
  • λ = c/v
  • v = c/λ
  • E = hc/λ
  • λ = hc/Ephoton
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12
Q

Conversion of nm to m

A

nm x 1m/10^9nm

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13
Q

Conversion of m to nm

A

m x 10^9nm/1m

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14
Q

KE

A

Ephoton - Binding energy

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15
Q

Energy of electron

A

En = -2.179x10^-18 J (z^2/n^2)
Z is atomic number
n is orbital

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16
Q

Excitation

A

Energy is absorbed and electron gain enough energy to move to higher orbital

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17
Q

Relaxation

A

Energy emitted (released) and electron moves to lower orbital

18
Q

Ground state

A

n=1 (lowest level)

19
Q

Excited state

A

n >= 2 (higher level)

20
Q

Difference in energy level

A
  • Used then question is asking when n=5 goes to n=3
    (-2.179x10^-18 J)(z^2/n^2f-z^2/n^2i)
21
Q

DeBroglie equation

A
  • λ = h/mv (velocity)
  • Finds wavelength from mass of electron and velocity, so end unit should be m/nm
22
Q

Heisenberg uncertainty principle

A

States that we do not know the speed and position of particles with exact accuracy

23
Q

3 types of quantum numbers

A
  • Describe orbitals in terms of their property
  • Principal quantum number (n)
  • Angular momentum quantum number (l)
  • Magnetic quantum number (ml)
24
Q

Principle quantum number (n)

A
  • Size and orbital energy
  • n is integer
  • Larger n = larger orbital (far from nucleus)
25
Q

Angular momentum number (l)

A
  • Orbital shape
  • Dependant on n, is every shape from 0 to n-1
26
Q

Relationship of l with orbital subshell

A
  • l = 0: s
  • l = 1: p
  • l = 2: d
  • l = 3: f
  • l = 4: d
27
Q

Magnetic quantum number (ml)

A
  • Orientation of orbital
  • Integer from -l to 0 to +1 (DO EVERY l)
  • Number of ml = number of orbitals
28
Q

s orbital

A

Spherical in shape, as n increases the size of s orbital increase

29
Q

Spherical node

A

Round nodes found on 2s orbitals and up

30
Q

Angular (planar) node

A

Nodes at nucleus of p orbitals and up

31
Q

Node

A

Areas of 0 electron density (n-1)

32
Q

p orbital

A

First occur in n=2, there is 3 with different orientations

33
Q

d orbital

A

First occur in n=3, there is 5 with different orientations

34
Q

Draw the orbitals

A

Ok

35
Q

Spin orientation quantum number (ms)

A

If electron configuration has arrow UP = +1/2, if arrow down = -1/2

36
Q

3 rules for electron configuration

A
  • Aufbau principle
  • Pauli exclusion principle
  • Hunds rule
37
Q

Aufbau principle

A

Electrons occupy lower energy orbitals first before going higher

38
Q

Pauli exclusion principle

A

2 electrons in orbitals must have different spins

39
Q

Hunds rule

A

Electrons will fill singly before pairing

40
Q

Periodic table blocks

A
  • s block: alkali earth + alkali metal
  • p block: basic metal + metalloid + nonmetal + halogen + noble gas
  • d block: transition metal
  • f block: lanthanoid + actinide
41
Q

Diamagnetic atom

A

All paired electrons

42
Q

Paramagnetic atom

A

Unpaired electrons

CHEM1110 (18 decks)

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