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Pharmaceutical Chemistry > molecular structure > Flashcards

molecular structure Flashcards

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1
Q

bond length (d)

A

nuclear separation distance (nm)

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2
Q

bond energy

A

energy required to break the bond (kJ mol⁻¹)

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3
Q

How many electrons form one chemical bond?

A

2

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4
Q

When atoms are the same, how do nuclei share electrons?

A

equally

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5
Q

When atoms are different, how do nuclei share electrons?

A

unequally

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6
Q

What does the unequal sharing of electrons result in?

A

polar covalent bond

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7
Q

dipole moment, µ =

A

charge, Q (C) x distance between charge, d (m)

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8
Q

What is the most electronegative element?

A

fluorine

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9
Q

What is the most electropositive element?

A

caesium

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10
Q

The smaller the atoms, the ? the bond.

A

shorter

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11
Q

The more electrons in a bond, the ? a bond.

A

shorter

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12
Q

The larger the electronegativity difference between the bonded atoms the ? the bond.

A

shorter

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13
Q

As bonds become shorter, the ? bond energy increases.

A

more

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14
Q

The more electrons in a bond, the ? bond energy increases.

A

more

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15
Q

The larger the electronegativity difference between the bonded atoms, the ? bond energy increases.

A

more

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16
Q

What structure do ionic compound form?

A

ionic lattices

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17
Q

Do ionic lattices have low or high melting points?

A

high

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18
Q

valence electrons

A

electrons in the highest atomic orbital

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19
Q

Lewis structure

A

visual representation of the valence electrons in a molecule

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20
Q

Is the central atom in a molecule often the most electronegative or electropositive?

A

electropositive

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21
Q

octet

A

set of 4 electrons associated with an atom

22
Q

VESPR

A

1) Valence
2) Electron
3) Shell
4) Pair
5) Repulsion

23
Q

2 electron pairs

A

linear

24
Q

3 electron pairs

A

trigonal planar

25
Q

4 electron pairs

A

tetrahedral

26
Q

5 electron pairs

A

trigonal bipyramidal

27
Q

6 electron pairs

A

octahedral

28
Q

What is the linear bond angle?

A

180°

29
Q

What is the trigonal planar bond angle?

A

120°

30
Q

What is the tetrahedral bond angle?

A

109.5°

31
Q

3 bonded pairs + 1 lone pair

A

trigonal pyramidal

32
Q

What is the trigonal pyramidal bond angle?

A

107°

33
Q

2 bonded pairs + 2 lone pairs

A

bent

34
Q

What is the bent bond angle?

A

105°

35
Q

What is the trigonal bipyramidal bond angle?

A

90° + 120°

36
Q

4 bonded pairs + 1 lone pair

A

seesaw

37
Q

What is the seesaw bond angle?

A

120°

38
Q

3 bonded pairs + 2 lone pairs

A

t-shaped

39
Q

What is the t-shaped bond angle?

A

90°

40
Q

2 bonded pairs + 3 lone pairs

A

linear

41
Q

What is the octahedral bond angle?

A

90°

42
Q

5 bonded pairs + 1 lone pair

A

square pyramidal

43
Q

What is the square pyramidal bond angle?

A

90°

44
Q

4 bonded pairs + 2 lone pairs

A

square planar

45
Q

What is the square planar bond angle?

A

90°

46
Q

valence bond theory

A

electrons are localised in bonds between 2 atoms / localised on a single atom, usually in pairs

47
Q

What are the conventions of the orbital overlap model?

A

1) each electron is assigned to a specific orbital
2) no 2 electrons have identical descriptions
3) the electrons obey the aufbau principal
4) only the valence orbitals are needed to describe bonding

48
Q

sigma (σ) bond

A

1) end-to-end overlap of atomic orbitals

2) single bond

49
Q

pi (π) bond

A

1) parallel overlap of atomic orbitals

2) double bond

50
Q

triple (σ) bond

A

1 σ bond + 2 π bonds

51
Q

What does hybridisation of atomic orbitals form?

A

hybrid orbitals

Pharmaceutical Chemistry (6 decks)

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