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Chemistry > Module 4: Intermolecular Forces > Flashcards

Module 4: Intermolecular Forces Flashcards

Test 2

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1
Q

What is intermolecular forces?

A

Attractions that occur BETWEEN atoms, molecules, and ions due to their proximity

Not covalently bonded

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2
Q

What are INTRAmolecular forces?

A

Covalent bonds

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3
Q

What does a bond tell you?

A

How the drug is interacting with the receptor

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4
Q

Blue =

A

Nitrogen

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5
Q

Yellow =

A

Sulfur

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6
Q

red =

A

oxygen

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7
Q

black =

A

carbon

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8
Q

Is O2 an intermolecular or intramolecular force?

A

INTRAmolecular

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9
Q

Are 2 H2O molecules intermolecular or intramolecular?

A

Intermolecular

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10
Q

T/F: Intermolecular forces are stronger than intramolecular forces

A

F

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11
Q

Why do intermolecular forces APPEAR stronger?

A

Normally d/t the larger number of interactions

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12
Q

There has to be a ________ to have an intermolecular force

A

closeness

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13
Q

What are partial charges?

A

Not an actual charge

d/t unequal sharing of electrons

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14
Q

What does Delta + mean?

A

Partial positive charge (No or less electrons)

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14
Q

What does Delta - mean?

A

Partial negative charge (More electrons)

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15
Q

What happens when there is a partial negative and a partial positive charge in a molecule?

A

A dipole-dipole bond is formed

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16
Q

What is a dipole polar bond? vs a non polar?

A

polar: Unequal sharing of electrons

non polar: equal sharing of electrons

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17
Q

How does the arrow point in the dipole dipole bonds?

A

Towards the more electronegative

Towards the Delta (-)

Towards more electrons

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18
Q

T/F: If the distance is wide there can still be intermolecular forces

A

F

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19
Q

The distance between intermolecular forces is very ______

A

small

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20
Q

The _______ the atoms the ________ the bond

A

closer

stronger

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21
Q

T/F: The stronger the attractive forces between particles, the more they resist moving.

A

T

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22
Q

Name your nonpolar bonds

A

C–C
C–H

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23
Q

Name your polar bonds

A

C–O
C–N
C–S
C–F
C–Cl
C–Br
C–I
H–O
H–N
H–S
P–O

24
Q

What is the electronegativity of a nonpolar bond?

A

if the difference in electronegativity is < 0.5 between bonded atoms

25
Q

What is the electronegativity of a polar bond?

A

if the difference in electronegativity is greater than 1 between bonded atoms

26
Q

T/F: Strong intermolecular forces will not break apart?

A

F

27
Q

Where does the partial negative charge reside?

A

the more electronegative atom

28
Q

What is surface tension?

A

Liquid’s resistance to increase its surface area

29
Q

How does surface tension relate to intermolecular forces?

A

The stronger the intermolecular forces the more energy required to increase surface area

30
Q

How many drops of water can you put on a penny?

A

Over 100

d/t surface tension

31
Q

What is capillary action?

A

Spontaneous rising of a liquid in a narrow tube or the movement of a liquid up a piece of paper against the pull of gravity

32
Q

What is capillary action due to?

A

cohesive and adhesive forces

33
Q

What is viscosity?

A

Measure of a liquid’s resistance to flow

thickness of liquid

34
Q

Increased viscosity means a liquid doesn’t pour as ______

A

easily

35
Q

With _______ viscosity you increase the amount of energy needed to get through the fluid.

A

increased

36
Q

increased hemaocrit =

A

increased viscosity

37
Q

T/F: The bigger the atom the more potential for more intermolecular force interactions

A

T

38
Q

T/F: Drugs bind receptors through intermolecular forces rather than chemical bonds

A

T

39
Q

The way the drug binds to the receptor determines what?

A

Efficacy, potency, toxicity

40
Q

T/F: Phase changes to different phases of matter are not affected by intermolecular forces?

A

F

They are directly impacted by them

41
Q

What does the phase change graph show?

A

The changes in the different phases of matter with respect to temperature and pressure

42
Q

_______ is required to disrupt molecular interactions and lead to changes in the state of matter

A

energy

43
Q

T/F: Changes is phases (state of matter) break chemical bonds

A

F

They do not break chemical bonds

44
Q

When you _______ the temperature you add more energy

A

increase

45
Q

Substances with ________ polarity will be soluble

A

Similar

46
Q

______ dissolves _______

A

Like dissolves like

47
Q

What are the weakest to strongest bonds?

A

Van der Waals Forces
Dipole-Dipole Interactions
Hydrogen Bonding
Ion-Dipole
Electrostatic Interactions
Covalent Bonds

48
Q

What are the bonds from strongest to weakest?

A

Covalent Bonds
Electrostatic Interactions
Ion-Dipole
Hydrogen Bonding
Dipole-Dipole Interactions
Van der Waals Forces

49
Q

What is Van der Waals Forces?

A

non polar dipole

Easily broken

weakest intermolecular forces

50
Q

What is another name for Van der Waals?

A

London Dispersion

51
Q

Describe Dipole-Dipole interactions

A

Polar Dipole

Relatively strong

52
Q

Describe Hydrogen bonding

A

Strong and specialized dipole-dipole bond

Between hydrogen donor and hydrogrn acceptors

53
Q

What is a hydrogen donor?

A

Molecule providing the H

**Molecule with a H

54
Q

What is a hydrogen acceptor?

A

Molecule that attracts the hydrogen

N, O, F

55
Q

Describe Ion-Dipole

A

a very strong interaction between a full formal charge and a dipole

56
Q

The partial charge in O in water dissolving a dissociated Na molecule is considered?

A

Ion-Dipole

57
Q

Describe Electrostatic interactions

A

Between the cationic and anionic portion of 2 NON METALS

2 non metals that have actual formal charges

Can exist at larger distances
Can hold alot longer
occur less often

58
Q

Describe Covalent bonds

A

Strongest
Limited reversibility
Seldom formed
INTRAmolecular forces

Chemistry (13 decks)

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