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MINE Chem BASICS Semester 1 > Exam 2: Intermolecular Forces > Flashcards

Exam 2: Intermolecular Forces Flashcards

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1
Q

Intermolecular Forces

A

force of attraction that occurs between atoms, molecules, and ions during to their proximity in space to each other

weaker than intermolecular forces (ionic, covalent, metallic bonds)

can occur between more than one atom/molecule in the same space

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2
Q

How can intermolecular forces appear stronger?

A

They can have a large number of interactions, therefore appear to be stronger

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3
Q

The closer the proximity of atoms the _______ interactions

A

more

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4
Q

Place in order from least to most intermolecular forces: Gas, Solid, Liquid

A

Gas (furthest distance between atoms/molecules)

Liquid (closer in proximity)

Solid (most intermolecular forces, tightest in proximity and distinct arrangement to maximize the intermolecular forces)

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5
Q

Intermolecular forces come about because of ______

A

charges (partial charges develop because of an unequal sharing of electrons)

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6
Q

How do you denote a partial charge?

A

lowercase delta (+ or -)

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7
Q

T/F
The magnitude of a charge (real or partial) affects the strength of the attraction

A

True

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8
Q

What is a dipole?

A

A dipole occurs when the polarity is unequally distributed (think polar covalent bonds)

pushes from + to -

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9
Q

What type of bond would you see equal sharing in?

A

non-polar covalent

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10
Q

In a molecule of H2O, which ion has what partial charge and where does it push to (which way does the arrow point)?

A

H has a + partial charge, O has a - partial charge, the arrow points FROM H and TO O

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11
Q

T/F
The distance between species affects the strength of the attraction

A

True

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12
Q

If the attractive force between two particles is strong, how does this affect the resistance to moving/breaking apart?

A

The stronger the force of attraction, the more they resist moving/breaking apart

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13
Q

Define polarity

A

The separation of electric charge along a bond due to differences in the electronegativity of the bonded atoms

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14
Q

Define an electric dipole or dipole moment

A

Electron density that is not equally shared between two atoms leading to the formation of partial charges

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15
Q

When denoting the dipole moment, which way does the arrow point?

A

towards the more electronegative atom

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16
Q

How many drops can fit on a penny?

A

more than 100 drops

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17
Q

Explain surface tension and its application of intermolecular forces

A
  • liquid’s resistance to increase its surface area
  • the stronger the intermolecular forces, the more energy required to increase the surface area
  • to minimize the surface area, liquids form spherical drops
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18
Q

If your car is freshly waxed, what happens to the water and what is this an application of?

A

the water will slide right off, this is an application of intermolecular forces in surface tension

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19
Q

What is capillary action?

A

the 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

20
Q

What is capillary action the result of?

A

it is the result of cohesive (holding the liquid molecules together) and adhesive (attraction of the outer molecules to the container’s surface) forces

21
Q

How does capillary action function within the body?

A

Helps pump blood through the body in certain areas, it happens because of the attractive forces of what is rising and the material it is rising up in to

22
Q

How is an aneurysm affected by intermolecular forces?

A

blood travels up a straight line easier, an aneurysm makes it harder for blood to move around

23
Q

What is viscosity?

A
  • the measure of a liquid’s resistance to flow
  • the amount of energy necessary to move an object through a fluid
24
Q

The _____ the viscosity, the _____ the resistance

A

higher, higher

25
Q

Explain how the size of molecules plays a role in viscosity.

A

The larger the molecule, the greater potential for more intermolecular force interactions

26
Q

The higher the viscosity, the ____ energy it requires to move itself or move something within it

A

more

27
Q

The higher the surface area, the _____ potential for intermolecular forces to occur

A

more

28
Q

How do intermolecular forces affect receptor drug binding?

A
  • efficacy
  • potency
  • toxicity (to some extent)
  • the goal is that the drug binds to just one receptor (indiscriminate binding is typically not good per FDA)
29
Q

Define phase changes

A

representation of the changes in the past of a substance with respect to temperature and pressure (energy is required to disrupt molecular interactions and thus lead to changes in states of matter)

30
Q

T/F
Phase changes break chemical bonds

A

False

31
Q

Disruption in intermolecular forces will result in what?

A

phase changes (phase changes are directly impacted by intermolecular forces, the amount of energy necessary to overcome these forces)

32
Q

“Like dissolves like” refers to what?

A

solubility

33
Q

Define solubility

A

substances with similar polarity will be soluble (solid in liquid) or miscible (liquid in liquid)

34
Q

Solubility depends on what?

A

depends on attractive forces between solute (what we are trying to dissolve) and solvent (what we are trying to dissolve it in)

35
Q

Since humans are made up of mostly of polar water, what types of drugs tend to work better?

A

polar drugs

36
Q

Van der Waals forces (London Dispersion) are what?

A

interactions arising from the formation of induces dipoles between two non-polar molecules (or portions of molecules)

weakest of the intermolecular forces

37
Q

Dipole-Dipole interactions occur in all _____ molecules

A

polar

38
Q

How strong are dipole-dipole interactions?

A

relatively strong interaction but depends on the nature of individual dipoles involved

39
Q

T/F
Hydrogen bonds are weak.

A

False

40
Q

Define hydrogen bonding.

A
  • very strong, specialized dipole-dipole interaction
  • H-bond donors (molecules providing the hydrogen)
  • H-bond acceptors (molecules that attract the hydrogen)
41
Q

Define ion-dipole interactions.

A
  • very strong interaction between a full formal charge and a dipole
  • found in drug interactions
  • polar bond that is attracted to an ion
42
Q

Describe electrostatic interactions.

A
  • ionic interactions between a cationic and anionic portion
  • effective at distances farther than other types of interactions
  • persists longer than other types of interactions
  • ion-ion interactions
43
Q

Define covalent bonds

A
  • strongest interaction
  • limited reversibility
  • not intermolecular, INTRAMOLECULAR interactions
  • difficult to break (seldom freed)
44
Q

List the bonds/forces from weakest to strongest.

A
  • van der waals
  • dipole-dipole
  • hydrogen bonding
  • ion-dipole
  • electrostatic
  • covalent (not intermolecular, INTRAMOLECULAR)
45
Q

T/F
Receptor shape helps determine if a drug compound is effective at binding.

A

True

MINE Chem BASICS Semester 1 (9 decks)

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