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Chemistry Lecture > Exam Three > Flashcards

Exam Three Flashcards

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1
Q

Pi/Sigma bonds within a double bond:

A

one pi bond and one sigma

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2
Q

Pi/Sigma bonds within a triple bond:

A

two pi bonds and one sigma

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3
Q

Which elements can have an expanded octet (provide example for each.

A
  1. phosphorus (PCl5)
  2. sulfur (SF6)
  3. chlorine (ClF3)
  4. sulfate ion
  5. sulfate oxides
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4
Q

What compounds can have a deficient octet?

A
  1. BeCl2
    * *central atom has 2 sigma bonds
  2. BF3
    * *central atom has 3 sigma bonds
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5
Q

What compound have a weird octet?

A

NO2

**due to lone electron

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6
Q

Class of a linear geometry:

A

AX2 or AX2E3

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7
Q

Example of linear geometry (3):

A

BeF2, HCN, CO2

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8
Q

Ideal bond angle of a linear geometry:

A

180

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9
Q

Class of trigonal planar:

A

AX3

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10
Q

Ideal bond angle of trigonal planar:

A

about 120

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11
Q

Class of bent:

A

AX2E or AX2E2

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12
Q

What do lone pairs do to the bond angle?

A

causes deviation, angle will be less than the ideal value

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13
Q

Tetrahedral electron group arrangement can have how many shapes?

A

3

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14
Q

Class of tetrahedral:

A

AX4

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15
Q

Class of trigonal pyramidal:

A

AX3E

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16
Q

Ideal bond angle of tetrahedral arrangments:

A

about 109.5

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17
Q

Trigonal bipyramidal electron group arrangement can have how many shapes?

A

4

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18
Q

Class of trigonal bipyramidal:

A

AX5

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19
Q

Class of seesaw:

A

AX4E

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20
Q

Class of t-shape:

A

AX3E2

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21
Q

Ideal bond angle of trigonal bipyramidal arrangments:

A

about 120 and 90

  • *t-shaped is 90
  • *linear is 180
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22
Q

Octahedral electron group arrangement can have how many shapes?

A

3

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23
Q

Class of octahedral:

A

AX6

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24
Q

Class of square pyramidal:

A

AX5E

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25
Q

Class of square planar:

A

AX4E2

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26
Q

Ideal bond angle of octahedral arrangement:

A

about 90

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27
Q

Period(s) […] can form more than four bonds.

A

3-6

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28
Q

Formal charge:

A

valence - sticks - dots

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29
Q

As you go L to R across the periodic table, the atomic size…

A

decreases

**nucleus to electron attraction (Zeff)

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30
Q

As you go down the periodic table, the atomic size…

A

increases

**adding more orbitals

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31
Q

Down a group […] dominates due to […].

Across a period […] dominates because […] remains the same and electrons pull closer to […]..

A

n (quantum number); electron shielding;

Zeff (effective nuclear charge); electron shielding; the nucleus

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32
Q

What is electron shielding? How does this affect the periodic trend?

A

inner layers of electrons shield the outer electrons

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33
Q

Down a transition series, atomic size […] from Period 4 to 5 and […] from 5 to 6.

A

increases slightly; none

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34
Q

Across a transition series, atomic size […] through the first two or three elements.

A

shrinks

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35
Q

After the first 2/3 elements in the transition series, the atomic size…

A

remains constant

36
Q

Size of V (23) compared to Zn (30):

A

same

**transition metals going across a series remain constant

37
Q

Atoms with a low IE tend to form […] while those with a high IE tend to form […] (except for […]).

A

cations; anions; noble gases

38
Q

Ionization energy:

A

requirement to completely remove 1 mol of electrons from 1 mol of atoms/ions

39
Q

Ionization energy is to overcome the […].

A

electrostatic attraction

40
Q

As size decreases, it takes […] energy to remove an electron.

A

more

41
Q

Electronegativity is inversely related to […]. So across the periodic table, EN […] while down the table, EN […].

A

atomic size; increases; decreases

42
Q

Pauli exclusion principle:

A

no two electrons in the same atom can have the same four quantum numbers

43
Q

Consequence of exclusion principle:

A

an atomic orbital can hold a max of two electrons, which must have opposing spins

**unique value of ms

44
Q

A higher nuclear charge (Z) increases […] and this lowers […] which stabilizes the atom.

A

nucleus-electron attraction; sublevel energy

45
Q

Nuclear charge stabilizes the atom and make is difficult to….

A

remove an electron

** harder to remove electron from Li2+ compared to H

46
Q

Effective nuclear charge is due to…

A

shielding

47
Q

Hund’s rule:

A

when orbitals of equal energy are available, the electron configuration of lowest energy has the max number of unpaired electrons with parallel spins

48
Q

Which electron configurations are exclusions to Aufbau’s principle? What occurs? Are these still stable?

A

copper and chromium

to fill d sublevel, an electron from the s sublevel is taken

these are stable (low in energy)

49
Q

Quantum number “n” represents:

A

principle energy level; the number matches the outermost s and p sublevels

50
Q

Ionization generally […] across a period and […] down a group.

A

increases; decreases

51
Q

Two exceptions to the IE trend:

A
  1. Group 3 (B and Al) dips because they easily remove an electron to conform to a stable configuration
  2. Group 6 (O and S) dips because they easily to obtain half filled orbital
52
Q

Electron affinity:

A

energy release/required when an electron is added to a neural atom

53
Q

The first electron affinities are […].

A

negative

54
Q

EA across the periodic table […], down the periodic table […].

A

increases; decreases

55
Q

Species with unpaired electrons exhibits…

A

paramagnetism

56
Q

Paramagnetism:

A

attracted by an external magnetic field

57
Q

Species with all of its electrons paired exhibits…

A

diamagnetism

58
Q

Diamagnetism:

A

not attracted (slightly repelled) by the magnetic field

59
Q

Heisenberg’s uncertainty principle:

A

impossible to know simultaneously the position and momentum of a particle

60
Q

Lyman is […] when H transmission goes to […].

A

UV radiation; n=1

61
Q

Balmer is […] when H transmission goes to […].

A

visible; n=2

62
Q

Paschen is […] when H transmission goes to […].

A

infrared; n=3

63
Q

Wavelength of Lyman series:

A

90 to 125

64
Q

Wavelength of Balmer series:

A

400 to 660

65
Q

Wavelength of Paschen series:

A

1200 to 1900

66
Q

Albert Einstein contribution:

A

proposed that light itself is particulate, quantized into tiny “bundles” of energy

**later called photons

67
Q

Rydberg equation:

A

predicts position and wavelength of any line in a given series

68
Q

De Broglie contribution:

A

if energy is particle-like, perhaps matter is wavelike

69
Q

De Broglie equation:

A
  1. wavelength = h/(mu)
  2. wavelength = h/p
  • *h = planks constant
  • *m = mass
  • *u = speed
  • *p = momentum
70
Q

Plank:

A

energy is quantized

71
Q

Bohr:

A

energy of atoms is quantized; photon is emitted when electron changes orbit

72
Q

Davisson/Gemer:

A

electron beam is diffracted by metal crystal (helps de Broglie)

73
Q

Compton:

A

photon’s wavelength increases (momentum decreases) after colliding with electron

74
Q

Einstein/de Broglie:

A

mass and energy are equivalent: particles have wavelength and photons have momentum (help Compton)

75
Q

Quantum number “l” represents:

A

angular momentum/shape of the orbital

76
Q

Magnetic quantum number (ml):

A

orientation; is the total number of orbitals in that energy level

77
Q

If l = 0, ml will be…

A

0

78
Q

If l = 1, ml will be…

A

-1, 0, 1

79
Q

If l = 2, ml will be…

A

-2, -1, 0, 1, 2

80
Q

If l = 3, ml will be…

A

-3, -2, -1, 0, 1, 2, 3

81
Q

What does ms represent:

A

spin of electron (+,- 1/2)

82
Q

Isoelectronic series:

A

given ions have the same number of electrons (noble gas configuration)

83
Q

Ions without a noble gas configuration create:

A

1, pseudo-noble gas configuration

2. inert pair configuration

84
Q

Pseudo-noble gas configuration:

A

empties out its highest energy level

85
Q

Inert pair configuration:

A

metal atoms loses just its np electrons (stable with just ns)

86
Q

Isoelectric series and atomic radius:

A

radius increases from right to left and down a period

Chemistry Lecture (7 decks)

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