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Medicinal Chemistry > Molecular Shape & Bonding > Flashcards

Molecular Shape & Bonding Flashcards

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1
Q

What are the characteristics of an ionic bond?

A

e- transferred

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2
Q

What are the characteristics of a covalent bond?

A

e- shared

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3
Q

What are the characteristics of a metallic bond?

A

e- pooled

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4
Q

Why do chemical bonds form?

A

They lower potential energy between charged particles that constitute atoms

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5
Q

What is pure covalent?

A

e- shared equally

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6
Q

What is polar covalent?

A

e- shared unequally

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7
Q

What is ionic bond?

A

e- transferred

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8
Q

Why does the metal lose e-?

A

Low ionisation energy of metals

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9
Q

Why does the non-metal gain e-?

A

Have high e- affinity

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10
Q

What is ions held together by?

A

Electrostatic attraction

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11
Q

What are the properties of ionic bonds?

A

Ionisation energy to form cation = endothermic
Acceptance of e- by non-metal = exothermic
Heat of formation for ionic compound = exothermic

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12
Q

Why is there energy differences in formation of ionic bond?

A

Forming crystal lattice

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13
Q

Is electrostatic attraction non-directional?

A

YES

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14
Q

What does it mean that electrostatic attraction is non-directional?

A

NO ionic molecule

= chemical formula = empirical formula = ratio of ions based on charge

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15
Q

What does Lewis Theory use?

A

Valence e-

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16
Q

Why are valence e- used in bonding?

A

Held most loosely

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17
Q

What do elements in the same column have the same properties?

A

Have same number of valence e-

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18
Q

What does Lewis Theory state?

A

e- are transferred from one atom to another atom = ions

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19
Q

What is the octet rule?

A

Rule of 8

Represents very stable configuration

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20
Q

How can represent valence e-?

A

Dot or crosses

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21
Q

What is the configuration?

A

1s2 2s2 2p6 3s2 3p6 3d10 4s2

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22
Q

What energy is required to remove e-?

A

Ionisation energy

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23
Q

What are elements with low ionisation energies?

A

Electropositive

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24
Q

What are elements that readily acquire e-?

A

Electronegative

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25
Q

What is group 1?

A

Alkali metals

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26
Q

What is group 2?

A

Alkali earth metals

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27
Q

What is group 3?

A

Al

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28
Q

What is group 7?

A

Halogens

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29
Q

What is group 6?

A

Chalcogens

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30
Q

What is group 5?

A

N + P

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31
Q

What are the properties of ionic compounds?

A

High melting points
Solid at RTP
Hard + brittle crystalline solids
Soluble in H2O

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32
Q

What happens if you have a larger ion?

A

Weaker attraction = lower lattice energy

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33
Q

What happens if you have a higher charge on ion?

A

Stronger attraction = higher lattice energy

34
Q

What is Lewis Theory of covalent compounds?

A

Atoms achieve octet by sharing e-
A bond consists of a
shared pair of e-

35
Q

What are e- called that are not shared?

Lewis Theory - covalent

A

Lone pairs

36
Q

How is the shape of a molecule explained?

A

Electrostatic repulsion between bonding pairs + lone pairs

37
Q

What pattern do atoms in the first period tend to follow?

A 
C = 4 bonds + no L.P
N = 3 bonds + 1 L.P
O = 2 bonds + 2 L.P
H = 1 bond + no L.P
Halogens = 1 bond + 3 L.P
38
Q

What is formal charge?

A

No. of valence e- - (no. of L.P + 1/2 no. of bonding e-)

39
Q

What is it hen one atom has a single unpaired e-?

A

A free radical

40
Q

What is Kekule structure?

A

Bonding e- drawn as lines + L.P not shown

41
Q

What happens in covalent bonding of 2 different atoms?

A

Covalent bond where 2 e- are shared unequally

42
Q

What do polar covalent bonds have?

A

Dipoles

43
Q

Why is a bond polar?

A

When one atom is more electronegative than another atom

44
Q

What is electronegativity?

A

The ability of an atom to pull bonding e- towards itself

45
Q

What is the most electronegative element?

A

Fluorine

46
Q

What is the least electronegative element?

A

Caesium

47
Q

What is the electronegativity difference of purely covalent bond?

A

NONE

48
Q

What is the electronegativity difference of non-polar covalent bond?

A

0.1-0.4

49
Q

What is the electronegativity difference of polar covalent bond?

A

0.5-1.9

50
Q

What is the size of the dipole indicated by?

A

Dipole moment

51
Q

How do you calculate dipole moment?

A

Magnitude of charge on atom X distance between 2 charges

52
Q

For complex molecules what does dipole moment depend on?

A

Dipole moments of all bonds in molecule + geometry of molecule

53
Q

For molecules with only 1 covalent bond, what is the dipole moment?

A

Just dipole moment of that bond

54
Q

What are the colours of electrostatic potential maps?

A

Blue > green > yellow > orange > red
Blue = most positive electrostatic potential
red = most negative electrostatic potential

55
Q

Describe p-orbitals

A

Dumbbell shaped

Nodal plane that cuts dumbbell into 2 lobes

56
Q

What do the +/- signs denote in the p-orbital?

A

Phase of lobe

NOT charge

57
Q

How many degenerate (same charge) p-orbitals is there?

A

3

Symmetry around x, y + z axes

58
Q

What are each of the p orbitals respective to the other two?

A

Perpendicular

59
Q

What is the energy of 2p orbital compared to energy of 2s orbital?

A

Bigger

= farther away from nucleus

60
Q

Why do atoms combine to form molecules?

A

Their total energy is lowered in the process

61
Q

What are the 2 main theories to describe covalent bond?

A 
Molecular orbital (MO)
Valence-bond
62
Q

What does MO involve?

A

Orbitals

BUT NOT atoms + bonds

63
Q

In MO, what are molecules made up from?

A

Nuclei + e-

Nuclei are held together by molecular orbitals

64
Q

What is MO?

A

e- distribution with e- density over the whole molecule

65
Q

What is the only molecule that MO can be used to solve completely?

A

H2+

66
Q

What is 1 rule for MO?

A

You must get the same number of MOs as starting AOs

67
Q

What happens in an addition of wave functions?

MO

A

Bonding molecular orbital

68
Q

What happens in subtraction of wave functions?

A

Anti-bonding molecular orbital

69
Q

What does antibonding mean?

A

That it is a higher energy

70
Q

What do bonding MO have?

A

High e- density on line between nuclei

71
Q

How can 2p orbitals combine?

MO

A

Side on or end on

72
Q

What does side on overlap lead to?

MO

A

Pi bonds

73
Q

What is stronger a pi bond or sigma bond?

A

Sigma bond

74
Q

What is the shape of 2 groups?

A

Linear

75
Q

What is the shape of 3 groups?

A

Trigonal planar

76
Q

What is the shape of 4 groups?

A

Tetrahedral

77
Q

What is the bond angle for linear?

A

180 degrees

78
Q

What is the bond angle for trigonal planar?

A

120 degrees

79
Q

What is the bond angle for tetrahedral?

A

109.5 degrees

80
Q

What is the hybridisation of linear (180 degrees)?

A

sp

81
Q

What is the hybridisation of trigonal planar (120 degrees)?

A

sp2

82
Q

What is the hybridisation of tetrahedral (109.5 degrees)?

A

sp3

Medicinal Chemistry (19 decks)

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