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Core Chem 1A - Term 1 > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

1
Q

Name the group 1 elements in order down the group

A

H, Li, Na, K, Rb, Cs, Fr

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2
Q

Name the group 2 elements in order down the group

A

Be, Mg, Ca, Sr, Ba, Ra

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3
Q

Name the group 3 elements in order down the group

A

Sc, Y

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4
Q

Name the group 4 elements in order down the group

A

Ti, Zr, Hf, Rf

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5
Q

Name the group 5 elements in order down the group

A

V, Nb, Ta, Db

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6
Q

Name the group 6 elements in order down the group

A

Cr, Mo, W, Sg

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7
Q

Name the group 7 elements in order down the group

A

Mn, Tc, Re, Bh

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8
Q

Name the group 8 elements in order down the group

A

Fe, Ru, Os, Hs

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9
Q

Name the group 9 elements in order down the group

A

Co, Rh, Ir, Mt

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10
Q

Name the group 10 elements in order down the group

A

Ni, Pd, Pt, Ds

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11
Q

Name the group 11 elements in order down the group

A

Cu, Ag, Au, Rg

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12
Q

Name the group 12 elements in order down the group

A

Zn, Cd, Hg, Cn

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13
Q

Name the group 13 elements in order down the group

A

B, Al, Ga, In, Ti, Uut

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14
Q

Name the group 14 elements in order down the group

A

C, Si, Ge, Sn, Pb, Fl

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15
Q

Name the group 15 elements in order down the group

A

N, P, As, Sb, Bi, Uup

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16
Q

Name the group 16 elements in order down the group

A

O, S, Se, Te, Po, Lv

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17
Q

Name the group 17 elements in order down the group

A

F, Cl, Br, I, At, Uus

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18
Q

Name the group 18 elements in order down the group

A

He, Ne, Ar, Kr, Xe, Rn, Uuo

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19
Q

Define ‘quantize’

A

To restrict a physical quantity to one of a fixed set of numbers

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20
Q

What is the experimental evidence for electrons behaving as both a particle and a wave?

A

The photoelectric effect - Many metals emit electrons when light shines on them. Increasing intensity of light increased number of electron emitted, but not their kinetic energy - So electrons can behave as particles

Davisson and Germer (1925): - Fired electrons at nickel - Electrons diffracted not just reflected - Diffraction is a property of waves

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21
Q

What is the De Broglie relation?

A

wavelength = h / mv

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22
Q

Kinetic energy =

A

Curvature = 2nd derivative

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23
Q

What is the typical bond length in a molecule?

A

100 pm

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24
Q

A very small wavelength means…

A

No diffraction

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25
Q

What is the potential energy of an electron confined to a 1D box?

A

0 inside the box, infinity at the walls

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26
Q

What is the wavefunction, ψ?

A

Wave height at point x

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27
Q

When you put an electron in a box…

A

It behaves as a wave

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28
Q

ψn(x) =

A

Csin(nπx / L)

L = length of box

n = quantum number

C = normaliation constant, value needed to make the integral of this 1

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29
Q

Energy of a wave, E =

A

n2h2 / 8mL2

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30
Q

What is a node?

A

Locus where the wavefunction is 0

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31
Q

What is ψ2?

A

The probability of finding the electron at that point

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32
Q

ψn,m(x,y) =

A

2/L sin(nπx/L) sin(mπy/L)

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33
Q

2D: En,m =

A

(n2 + m2)h2 / 8mL2

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34
Q

Quantum number n =

A

Orbital size quantum number - principle quantum number

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35
Q

Quantum number l =

A

Orbital shape quantum number - orbital angular momentum quantum number

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36
Q

Quantum number ml =

A

Orbital orientation quantum number - magnetic quantum number

37
Q

Orbital is another word for…

A

Hydrogen wavefunction, ψ

38
Q

What does it mean to say that the electron can behave as a wave as long as it’s a standing wave?

A

The wave must be continuous, and there must be an integral number of waves around the ring

39
Q

2πr =

40
Q

What is the radial wavefunction?

A
  • Depends on radius, r - Quantum number n= 1,2,3,4…infinity - Uses symbol ψ(r)
41
Q

What is the angular wavefunction?

A
  • Depends on θ, ϕ - Quantum numbers l (0,1…n-1) and m (-l,….,+l) - Uses the symbol ψ(θ,ϕ)
42
Q

What is needed to give a wavefunction in spherical polar coordinates?

A

Radius, r

Colatitude (angle down from z axis), θ

Azimuth (angle east from x-z plane), ϕ

43
Q

What quantum numbers give a 1s wavefunction?

A

n=1, l=0, ml =0 (s means l = 0)

44
Q

Radial distribution function =

A

4πr2ψ2

The probability of finding the electrons in all directions at that radius

45
Q

How many radial nodes does an ns wavefunction have?

46
Q

How many radial nodes does an np wavefunction have?

47
Q

How many radial nodes does an nd wavefunction have?

48
Q

Total wavefunction =

A

ψ(r)ψ(θ,ϕ)

49
Q

Angular wavefunctions for all s wavefunctions are…

50
Q

What is the boundary surface?

A

A representation of the angular wavefunction that contains 90% of the electron density

51
Q

What does it mean for 2 energy states to be degenerate?

A

They have the same energy

52
Q

What is the Pauli Exclusion Principle?

A

No two electrons in an atom or ion can have all their quantum numbers the same

53
Q

What is Hand’s rule of maximum spin multiplicity?

A

Lowest energy = Maximum number of parallel spins

54
Q

For hydrogen, orbital energy is proportional to

55
Q

For atoms other than hydrogen, orbital energy is proportional to

56
Q

Order of repulsion of pairs of electrons (strongest to weakest)

A

Lone pair - Lone pair

Lone pair - Bonding pair

Bonding pair - Bonding pair

57
Q

Shape of molecule with 2 electron pairs

58
Q

Shape of molecule with 3 electron pairs

A

Trigonal planar

59
Q

Shape of molecule with 4 electron pairs

A

Tetrahedral

60
Q

Shape of molecule with 5 electron pairs

A

Trigonal bipyramid

61
Q

Shape of molecule with 6 electron pairs

A

Octahedral

62
Q

Shape of molecule with 7 electron pairs

A

Pentagonal bipyramid

63
Q

For a trigonal bipyramid, which is the larger site?

A

Equatorial

64
Q

For a pentagonal bipyramid, which is the larger site?

65
Q

What is Bent’s rule? (VSEPR)

A

The smaller atom goes to the smaller site

66
Q

Why do we need to create orbital hybrids?

A

Because for overlap we need singly occupied orbitals

67
Q

What hybridisation does forming a linear molecule require?

68
Q

What hybridisation does forming a trignal planar molecule require?

A

sp2

  • Taking s, px and py produces 3 hybrids at 120o in the xy plane
69
Q

What hybridisation does forming a tetrahedral molecule require?

A

sp3

  • Taking s, px, py and pz produces 4 hybrids directed at the vertices of the tetrahedron
70
Q

The antibondig orbital is denoted by…

A

σu* or πg*

71
Q

The bonding orbital is denoted by…

A

σg or πu

72
Q

Bond order =

A

(no. of bonding electrons - no. of antbonding electrons) / 2

73
Q

What does paramagnetic mean?

A

A material is paramagnetic if it attracted to a magnet because of unpaired electrons

74
Q

What does diamagnetic mean?

A

A material is diamagnetic if it is repelled by a magnet because of paired electrons

75
Q

Molecular orbitals are…

A

Linear combinations of atomic orbitals

76
Q

Magnetic moment, χ =

A

diamagnetic - paramagnetic

77
Q

For diatomic molecules with p orbitals, σu* =

A

1 /√2 [pz(a) + pz(b)]

78
Q

For diatomic molecules with p orbitals, σg =

A

1/√2 [pz(a) - pz(b)]

79
Q

For diatomic molecules with p orbitals, πu =

A

1/√2 [px(a) + px(b)]

80
Q

For diatomic molecules with p orbitals, πg* =

A

1/√2 [px(a) - px(b)]

81
Q

Bond order will correlate with…

A

Bond length and bond strength

82
Q

J in SI base units

83
Q

What is excitation energy?

A

The energy required to move an atom to its next energy level

84
Q

1 mile =

85
Q

Which is more penetrating, 2p or 2s?

86
Q

If an orbital is more penetrating, it feels…

A

A higher Zeff

87
Q

What is penetration?

A

The attraction an orbital feels towards the nucleus

88
Q

How to show if an orbital has a higher Zeff than another

A

Sketch the radial distribution functions, whichever has a local maximum closest to the nucelus feels a higher Zeff

89
Q

State and explain for which elements sp switching occurs

A

B,C and N

2p orbitals are not involved with elements before B, after N, the energy gap between 2s and 2p is too large

Core Chem 1A - Term 1 (6 decks)

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