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Organic Chemistry Lab (Serena) > Quiz 2 - Intermolecular Forces > Flashcards

Quiz 2 - Intermolecular Forces Flashcards

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1
Q

Intermolecular Forces are attractive forces _________ molecules.

A

Between

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2
Q

Intramolecular Forces are forces _________ ________ _________ in a molecule.

A

Holding atoms together

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3
Q

How many kcal does it take to vaporize 1 mole of water using INTERmolecular Forces?

A

10 kcal

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4
Q

How many kcal does it take to vaporize 1 mole of O-H bonds in water using INTRAmolecular Forces?

A

110 kcal

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5
Q

Generally Intermolecular Forces are much __________ than Intramolecular forces.

A

WEAKER

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6
Q

Intramolecular Forces are mainly ______.

A

Bonds

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7
Q

What are different ways of measuring Intermolecular Forces?

A
  • Boiling Point
  • Melting Point
  • ΔHvap
  • ΔHfus
  • ΔHsub
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8
Q

What are the 2 things that generate Intermolecular Forces?

A

I) Partial Charge

II) Charge Interactions

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9
Q

Formal Charges = …

A

Stronger Interactions

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10
Q

Partial Charges = …

A

Weaker Interactions

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11
Q

What is an example of a Ion-Dipole Interaction?

A

The hydration of Sodium and Chloride ions in water

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12
Q

Ex. Ion-Dipole Interaction (Sodium & Chloride ions in H2O)
Waters behave as _________ surrounding a central _________ or _________ _____.

A

Ligands; metal; halogen ion

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13
Q

What are the weak Intermolecular Forces?

A
  • Dipole-Dipole
  • Dipole-Induced Dipole
  • Instantaneous Dipole-Induced Dipole (London Forces)
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14
Q

Weak Intermolecular Forces are also called…

A

Van der Waals Forces

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15
Q

Boiling points for non-polar molecules that are considered London Forces have boiling points that increase when…

A

The more electronegative molecule has a lower boiling point, whereas a less electronegative molecule has a higher boiling point

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16
Q

__________ species give rise to London Dispersion Forces.

A

Polarizable

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17
Q

London Dispersion Interactions operate in all molecules but are the only ___________ ____________ that occur between ___________ molecules.

A

Intermolecular Interactions; non-polar

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18
Q

London Forces are also called…

A

Instantaneous Dipole-Induced Dipole Interactions

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19
Q

London Forces are interactions resulting when a molecule establishes an __________ _________ as a result of ________ __________ produced in a molecule based of _________ _________ _________.

A

Instantaneous dipole; charge separation; random electron motion

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20
Q

What happens when a London Force molecule gets near another molecule?

A

When this molecule is near another molecule it can induce a dipole in the 2nd molecule

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21
Q

The arrangement of the dipoles in London Forces will produce an…

A

Attractive Interaction (+/-)

22
Q

The larger the molecules, the _________ the number of electrons that can be involved in dispersion interactions.

A

GREATER

23
Q

Generally, as the molecular weight increases the strength of London Dispersion Forces _________.

A

INCREASES

24
Q

_________ _________ is important in determining the magnitude of London Dispersion Forces.

A

Molecular Shape

25
Q

Explain London Dispersion Forces in a fairly spherical shape

A

There is less surface area for dispersion forces to operate when the molecules are in contact

26
Q

Explain London Dispersion Forces in an extended structure

A

Extended structure allows for more contact points for dispersion forces to operate

27
Q

For Hydrogen Bonding to occur, H must be on an __________ _______ such as ___, ___ or ___.

A

Electronegative atom; O; N or F

28
Q

For Hydrogen Bonding to occur you need a __________ Bond.

A

Hydrogen

29
Q

For Hydrogen Bonding to occur, the other terminus of the hydrogen bond must be an __________ ________ such as ___, ___ or ___.

A

Electronegative atom; O: N or F

30
Q

Hydrogen Bonds are very ____________.

A

Directional

31
Q

Hydrogen Bonds align along ______ _______ and ___________ ______.

A

X-H bonds; non-bonded pairs

32
Q

Hydrogen Bonds are typically _________ than other dipole-dipole attractions.

A

STRONGER

33
Q

Why are Hydrogen Bonds typically stronger?

A

Because the small size of H allows less distances between the charges

34
Q

How to determine the H of Hydrogen Bond Donors?

A

Look for the H’s on the O’s (alcohols/acids) or N’s (amines/amides) to account for the # of HBDs

35
Q

How to determine the H of Hydrogen Bond Acceptors?

A

THe # of non-bonded pairs on the N’s and O’s which can interact with HBD’s

36
Q

How do Non-Bonded Lone Pairs affect Hydrogen Bond Acceptors?

A

Non-bonded lone pairs participate in resonance so they make Hydrogen Bond Acceptor’s availability almost 0

37
Q

Are Non-Bonded Lone Pairs counted as Hydrogen Bond Acceptor sites?

A

No they are not

38
Q

If you have a primary amide or aniline, the lone pair on the amide “N” _____ participate in hydrogen bonding.

A

CAN

39
Q

Lone pairs on “N” on amides attached to aromatic rings are _____ likely to hydrogen bond.

A

Less

40
Q

Why do lone pairs on “N” on amides attached to aromatic rings have a lesser likelihood of hydrogen bonding?

A

Because there is significantly greater interaction between the amide functional group and the aromatic ring

41
Q

Polar compounds dissolve in _________ solvents.

A

Polar

42
Q

Non-polar compounds dissolve in ___________ solvents.

A

Non-polar

43
Q

Solubility depends on ___________ ___________ between polar surfaces or non-polar surfaces, both of ________ and __________.

A

Complementary interactions; solvent; solute

44
Q

NaCl dissolves in _________.

A

Water

45
Q

NaCl does not dissolve in _____________.

A

CH3(CH2)3CH3

46
Q

T/F CH3(CH2)3CH3 and water mix well and do not form layers

A

False; they do not mix with each other and they form 2 layers

47
Q

CH3OH through CH3CH2CH2OH = …

A

Mixes with water in all proportions

48
Q

CH3CH2CH2CH2OH = …

A

Slightly soluble in water

49
Q

CH3CH2CH2CH2CH2OH = …

A

Essentially insoluble

50
Q

What is the 4 1/2 Carbon Rule?

A

Rule that exemplifies the big transition in solubility between 4C and 5C compounds

Organic Chemistry Lab (Serena) (7 decks)

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