Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Liquids, Solids, and Intermolecular forces > Flashcards

Liquids, Solids, and Intermolecular forces Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Why are molecules attracted to each other?

A

intermolecular attractions are due to attractive forces btwn. opposite charges, such as cations and anions , - and + ends of polar molecules (H bonds especially strong).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Can nonpolar molecules ever have a charge?

A

yes, even nonpolar molecules will have a temporary charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The larger the charge the _________ the attraction.

A

stronger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

The smaller the charge the ________ the attraction.

A

weaker

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

If the bonds btwn. atoms in a molecule are very strong, how can the molecule be separated?

A

The stronger the attractions btwn. atoms or molecules the more energy is required to separate them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

When liquid is boiling what is happening?

A

energy is being added to the point where the attractions between the molecules or atoms can be broken apart.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

If a liquid has a high boiling point what can be said about the bonds btwn. the molecules or atoms that make up the liquid?

A

The higher the normal boiling point of the liquid , the stronger the intermolecular attractive forces.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How are nonpolar molecules able to sit next to polar molecules

A

Dispersion forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are dispersion forces?

A

fluctuations in the e- distribution in atoms and molecules that result in temporary dipole. The region with excess e- density has a small partial - charge and the region depleted of e- has a small partial charge of +

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Attractive forces caused by temporary dipoles

A

Dispersion or London forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Do all molecules and atoms have dispersion forces?

A

yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Temporary Dipole vs. Permanent Dipole

A

Temporary dipoles are dipoles created by random e- dispersion, and permanent dipoles are found on polar molecules and are due to a dipole moment.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens when a temporary dipole is established in one molecule?

A

it induces a dipole in all the surrounding molecules, then the dipoles may attract

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does the size of an induced dipole depend on?

A

1) Polarizability of the e-
- volume of e- cloud
- the larger the molar mass the more e-, the more e- the larger the e- cloud, the bigger the cloud is the greater its polarizability, the greater the polarizability the stronger the attraction.
2) Shape of the molecule
- more surface to surface contact, the larger the induced dipole and the stronger the attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Dipole-dipole interactions involve _________ dipoles.

A

permanent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

London dispersion involves _________ dipoles.

A

temporary

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What does solubility depend on?

A

the attractive forces of the solute and solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what does “like dissolves like mean?”

A

miscible substances will dissolve each other and immiscible substances will dissolve each other but miscible substances will not dissolve immiscible substances.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

polar substances will dissolve in _________.

A

polar solvents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what are the hydrophilic groups?

A

OH, CHO, C=O, COOH, NH2, and Cl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

nonpolar molecules dissolve in ______ solvents.

A

nonpolar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What are the hydrophobic groups?

A

C-H and C-C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Many molecules have both ________ and ________ parts.

A

hydrophilic

hydrophobic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

A dipole-dipole interaction where H is involved.

A

Hydrogen/ H bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

How does H bonding happen?

A

A very electronegative element is covalently bonded to hydrogen, it hogs the electrons which makes it more negative. The Hydrogen atom has an exposed nucleus which is positive and attracts (e- clouds) negative molecules or molecule parts.

26
Q

Which elements must be covalently bonded to H in order for a dipole-dipole to be called a “hydrogen bond?”

A

Fluorine, Nitrogen, or Oxygen

ex. O-H, N-H, F-H

27
Q

What are the requirements for an H bond?

A

H must be attached to O,F or N and H must be directly involved in the bond.

28
Q

Why are H bonds so strong?

A

Because they have a large polarity

29
Q

Do C-H bonds like to interact with water?

A

No because water is polar and C-H is nonpolar

30
Q

How many H bonds does water have when it is liquid?

A

3-4 H bonds

31
Q

How many H bonds does water have when it is solid?

A

4 H bonds

32
Q

How many possible H bonds can water have?

A

4

33
Q

What happens when you introduce an ionic substance to a polar mixture?

A

ions are attracted to dipoles of polar molecule

34
Q

What is one of the main factors that determines the solubility of an ionic compound in water?

A

the strength of the ion-dipole attraction. If there isn’t enough of an attraction ionic compound will be insoluble. I f the attraction weak in the compound it will be soluble.

35
Q

Which has more force of attraction an i0n-dipole bond or a dipole-dipole bond?

A

they have the same force of attraction

36
Q

Dispersion

A

present in all molecules

Has the lowest boiling point

temporary shift in charges causes domino effect

37
Q

Dipole-dipole

A

present only in polar molecules

second to last in strength and boiling point

38
Q

H bonding

A

Present in molecules where H is bonded to F, N or O.

middle strength wise and has midrange boiling point

39
Q

Ion-dipole

A

Present in mistures of ionic and polar compounds

Strongest and has highest boiling point

40
Q

Surface tension

A

the property of liquids that results from the tendency of liquids to minimize their surface area.

41
Q

Why do liquids form spherical drops?

A

because spherical objects have less surface area

42
Q

What are the factors that affect surface tension?

A

1) the stronger the intermolecular attractive forces the higher the surface tension will be
2) raising the temp of liquid reduces surface tension because raising the average temp of molecules will increase their movement

43
Q

Viscosity

A

the resistance of liquid to flow, this results from strong intermolecular forces

44
Q

the large the intermolecular attractions the greater the ____________.

A

viscosity

45
Q

How can one reduce the viscosity of a liquid?

A

by increasing its temperature

46
Q

Vaporization is an ______ process.

A

endothermic

47
Q

molecules in a liquid are __________.

A

constantly in motion

48
Q

when measuring temperature what is truly being measured?

A

the average kinetic energy

49
Q

What happens during vaporization?

A

some molecules have more kinetic energy than the average, if the molecules are at the surface they may have enough energy to overcome attractive forces. Because of energy surface area is larger so evaporation occurs faster. Once molecules escape attractive forces they become a vapor

50
Q

Condensation is an ___________ process.

A

exothermic

51
Q

Describe what happens during the process of condensation.

A

some molecules of the vapor will lose energy through collisions, some molecules will collide into liquid and become a part of the liquid again, some may stick together and form droplets of liquid on surrounding surfaces

52
Q

Dynamic equilibrium

A

When the rate of evaporation is equal to the rate of condensation; molecules are continually becoming vapors or droplets.

53
Q

Vapor pressure

A

the pressure exerted by the vapor when it is in dynamic equilibrium with its liquid

54
Q

The weaker the attractive forces the ____ ________ will be in vapor form.

A

more molecules

55
Q

The weaker the attractive forces the weaker the ____________.

A

vapor pressure; the higher the vapor pressure the more volatile the liquid. * depends on temp

56
Q

Boiling

A

when the temp of a liquid reaches a point where the vapor pressure is the same as the external pressure , vapor bubbles can form anywhere in the liquid (not just surface)

57
Q

Boiling point

A

the temperature required to have the vapor pressure = external pressure

58
Q

A higher elevation will cause a decrease in _________.

A

boiling point ; because less external pressure

59
Q

What is normal boiling point?

A

the temperature at which the vapor pressure of the liquid is equal to 1 atm

60
Q

the lower the external pressure the ____ the boiling point.

A

lower

61
Q

Crystalline solids

A

solids that have their particles arranged in an orderly geometric pattern

ex. salt and diamonds

62
Q

Amorphous solids

A

solids with particles that do not show a regular geometric pattern over a long range.

ex. Plastic and glass

Chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions