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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
What is group 1?
Alkali metals
26
What is group 2?
Alkali earth metals
27
What is group 3?
Al
28
What is group 7?
Halogens
29
What is group 6?
Chalcogens
30
What is group 5?
N + P
31
What are the properties of ionic compounds?
High melting points Solid at RTP Hard + brittle crystalline solids Soluble in H2O
32
What happens if you have a larger ion?
Weaker attraction = lower lattice energy
33
What happens if you have a higher charge on ion?
Stronger attraction = higher lattice energy
34
What is Lewis Theory of covalent compounds?
Atoms achieve octet by sharing e- A bond consists of a shared pair of e-
35
What are e- called that are not shared? | Lewis Theory - covalent
Lone pairs
36
How is the shape of a molecule explained?
Electrostatic repulsion between bonding pairs + lone pairs
37
What pattern do atoms in the first period tend to follow?
``` 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
What is formal charge?
No. of valence e- - (no. of L.P + 1/2 no. of bonding e-)
39
What is it hen one atom has a single unpaired e-?
A free radical
40
What is Kekule structure?
Bonding e- drawn as lines + L.P not shown
41
What happens in covalent bonding of 2 different atoms?
Covalent bond where 2 e- are shared unequally
42
What do polar covalent bonds have?
Dipoles
43
Why is a bond polar?
When one atom is more electronegative than another atom
44
What is electronegativity?
The ability of an atom to pull bonding e- towards itself
45
What is the most electronegative element?
Fluorine
46
What is the least electronegative element?
Caesium
47
What is the electronegativity difference of purely covalent bond?
NONE
48
What is the electronegativity difference of non-polar covalent bond?
0.1-0.4
49
What is the electronegativity difference of polar covalent bond?
0.5-1.9
50
What is the size of the dipole indicated by?
Dipole moment
51
How do you calculate dipole moment?
Magnitude of charge on atom X distance between 2 charges
52
For complex molecules what does dipole moment depend on?
Dipole moments of all bonds in molecule + geometry of molecule
53
For molecules with only 1 covalent bond, what is the dipole moment?
Just dipole moment of that bond
54
What are the colours of electrostatic potential maps?
Blue > green > yellow > orange > red Blue = most positive electrostatic potential red = most negative electrostatic potential
55
Describe p-orbitals
Dumbbell shaped | Nodal plane that cuts dumbbell into 2 lobes
56
What do the +/- signs denote in the p-orbital?
Phase of lobe | NOT charge
57
How many degenerate (same charge) p-orbitals is there?
3 | Symmetry around x, y + z axes
58
What are each of the p orbitals respective to the other two?
Perpendicular
59
What is the energy of 2p orbital compared to energy of 2s orbital?
Bigger | = farther away from nucleus
60
Why do atoms combine to form molecules?
Their total energy is lowered in the process
61
What are the 2 main theories to describe covalent bond?
``` Molecular orbital (MO) Valence-bond ```
62
What does MO involve?
Orbitals | BUT NOT atoms + bonds
63
In MO, what are molecules made up from?
Nuclei + e- | Nuclei are held together by molecular orbitals
64
What is MO?
e- distribution with e- density over the whole molecule
65
What is the only molecule that MO can be used to solve completely?
H2+
66
What is 1 rule for MO?
You must get the same number of MOs as starting AOs
67
What happens in an addition of wave functions? | MO
Bonding molecular orbital
68
What happens in subtraction of wave functions?
Anti-bonding molecular orbital
69
What does antibonding mean?
That it is a higher energy
70
What do bonding MO have?
High e- density on line between nuclei
71
How can 2p orbitals combine? | MO
Side on or end on
72
What does side on overlap lead to? | MO
Pi bonds
73
What is stronger a pi bond or sigma bond?
Sigma bond
74
What is the shape of 2 groups?
Linear
75
What is the shape of 3 groups?
Trigonal planar
76
What is the shape of 4 groups?
Tetrahedral
77
What is the bond angle for linear?
180 degrees
78
What is the bond angle for trigonal planar?
120 degrees
79
What is the bond angle for tetrahedral?
109.5 degrees
80
What is the hybridisation of linear (180 degrees)?
sp
81
What is the hybridisation of trigonal planar (120 degrees)?
sp2
82
What is the hybridisation of tetrahedral (109.5 degrees)?
sp3

Medicinal Chemistry (19 decks)

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