Brainscape's Knowledge GenomeTM

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


See full index

CHEM 1310 - 2019 > Quiz 1 - Chapter 11 > Flashcards

Quiz 1 - Chapter 11 Flashcards

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

Polar vs non-polar

A

Polar: one atom is more electronegative than the other

Non-polar: electrons are shared equally, very similar electronegativity

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

Density (mass/volume) of gas, liquid and solid?

A

Least to most….

Gas, liquid, solid

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

Strength of intermolecular forces of gas, liquid and solid?

A

Least to most….

Gas, liquid, solid

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

Why is water an exception to the density rule?

A

H20(l) is more dense than H2O (s) =ice

*ice floats on water

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

Crystalline vs Amorphous Solids

A

Crystalline solid: regular ordered structure
Amorphous Solid: not predictable, no order

Ex) glass vs quartz
○ Glass is not regular or repeating arrangement of atoms
○ Quartz is regular and repeating

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

What is the energy level of the molecules in solids, liquids and gases?

A

Least to most energy….

Solid, liquid gas

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

Intermolecular vs Intramolecular Forces

A

Intra=within a molecule, shorter and stronger bonds
Inter=between two molecules or more, longer and weaker bonds
*The forces that hold condensed states together

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

Intermolecular force: Dipole-dipole

A
  • between 2 polar molecules (permanent dipoles)
  • Happens when positive end of one permanent dipole is attracted to the negative end of another permanent dipole
  • water is a special case
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Intermolecular force: Ion-induced dipoles

A
  • ion+non-polar

- induced dipole: starts out as non-polar but once ion interacts it then becomes polarized

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

Intermolecular force: Dipole-induced dipoles

A
  • polar+non-polar

- Polar compound comes closer to nonplar molecule but electrons push it away onto other side of molecule

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

Intermolecular force: Dispersions

A
  • always present
  • weakest IMF
  • based on polarizability
  • larger cloud=more dispersion force
  • instantaneous dipole of an atom induces instantaneous dipoles on neighbouring atoms which then attract one another
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Intermolecular force: Ion dipole

A
  • strongest IMF

- ion+polar

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

Intermolecular force: Hydrogen bonding

A
  • occurs in polar molecule with H atom bonded to a small electronegative atom F, O, N
  • super dipole-dipole force
  • Not a BOND, but an INTERMOLECULAR FORCE
  • Intermolecular forces span much further distances than bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Increasing dispersion force does what to electrons, polarizability, dispersion, surface area, boiling point and energy?

A
  • increase number of electrons
  • increase polarizability
  • increase dispersion
  • increase surface area
  • increase boiling point
  • more energy to break forces
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

If you have an isomer (same chemical formula but different structural arrangement and same number of electrons), which two structure, linear or branched arrangements, will have a higher boiling point?

A

Linear=large area for interaction=high boiling point

Branched=smaller area for interaction=low boiling point

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

Miscibility

A
  • Like dissolves like (Polar dissolves in other polars, non-polars dissolve in non-polars)
  • Liquids with the same polarity tend to mix without separating
  • F, O, N has a possibility for hydrogen bonding with water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Increasing hydrogen bonding does what to electrons, polarizability, dispersion, and dipole?

A
  • increasing electrons
  • increasing polarizability
  • increasing dispersion
  • decreasing dipole
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Which intermolecular force is strongest? Weakest?

A

Strongest=ion-dipole

Weakest=dispersion

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

Which element is the most electronegative in the entire periodic table?

A

Fluorine (F)

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

Surface tension

A
  • how hard it is to break the surface of a liquid
  • increase surface tension=increasing intermolecular forces
  • energy required to increase the surface area by a unit amount
  • molecules at the surface have more potential energy than those surrounded inside a liquid
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

An increasing boiling point does what to number of electrons, molecule arrangements/structures and dipoles?

A
  • increasing electrons
  • linear arrangement = higher boiling point
  • branched arrangement= lower boiling point
  • increasing dipole
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What happens to intermolecular forces if surface tension increases?

A

increasing intermolecular forces

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

What happens to intermolecular forces if viscosity increases?

A

increasing intermolecular forces

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

Is a longer chain or shorter chain tend to be more viscous?

A

longer chain tends to tangle more, so more viscous

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

Viscosity

A
  • resistance of a liquid to flow
  • stronger IMF increase viscosity
  • molecules that are longer can tangle more and tend to be more viscous
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Capillary action

A
  • ability of a liquid to flow against gravity up a narrow tube
  • a balance of cohesive and adhesive forces
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Cohesive vs adhesive forces

A

Cohesive: attraction between liquid molecules; forms a dome
ex) Hg metal with glass
Adhesive:attraction between liquid molecules and the surface of a tube (allows for upward movement); meniscus is formed
ex) water with glass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Vaporization

A

liquid to gas (endothermic: low to high energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Condensation

A

gas to liquid (exothermic: high to low energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What does an increase in temperature mean for heat and kinetic energy?

A

heat is transferred to molecules and kinetic energy increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Volatile vs nonvolatile liquids

A

Volatile: easily vaporizes, have weak intermolecular forces
Nonvolatile: don’t easily vaporize, have stronger intermolecular forces (H2O)

32
Q

If a liquid is volatile, what happens to its intermolecular forces?

A

high volatility=low intermolecular forces

33
Q

Heat of vaporization (delta vap H)

A

amount of heat required to vaporize one mole of a liquid to gas

34
Q

Vapour pressure

A
  • the pressure of a gas in dynamic equilibrium with its liquid
  • pressure at which the amount of molecules leaving and entering the container is equal
  • increasing vapour pressure lowers IMF
35
Q

If the vapour pressure increases, what happens to the boiling point and temperature?

A

increasing boiling point and increasing temperature

36
Q

If volume of a cylinder is increased, what happens to the pressure and gas molecules?

A

pressure falls, more gas vaporizes and pressure is restored to equilibrium

37
Q

If volume of a cylinder is decreased, what happens to the pressure and gas molecules?

A

pressure rises, more gas condenses and pressure is restored to equilibrium

38
Q

Boiling point

A

the temperature where the vapour pressure equals the external pressure

39
Q

Normal boiling point vs standard boiling point

A

normal boiling point: temperature where the vapour pressure is 1 atm
standard boiling point: temperature where the vapour pressure is 1 bar

40
Q

Sublimation

A

the transition of a substance from solid to gas (endothermic, low to high energy)

41
Q

Deposition

A

transition of a substance from gas to solid (exothermic, high to low energy)

42
Q

Melting or fusion

A

transition of a substance from a solid to a liquid (endothermic, low to high energy)

43
Q

Heat of fusion (delta fus H)

A

amount of heat required to melt 1 mol of solid

44
Q

Freezing

A

transition of a substance from a liquid to a solid (exothermic, high to low energy)

45
Q

Heat capacity

A

How much heat can be absorbed by the substance

46
Q

What is the 1st Law of Thermodynamics?

A

Energy can be neither created nor destroyed, only transformed.

47
Q

Phase diagrams

A
  • map the state/phase of a substance as a function of pressure and temperature
  • have major regions that are labelled with respective state
  • lines and curves represent a set of temperatures and pressures where the substances are in equilibrium
48
Q

Triple point

A
  • represents the temperature and pressure where all 3 states are in equilibrium
  • in the center of phase diagram where all three equilibriums of each state meets
49
Q

Where are the fusion curve, vaporization curve and sublimation curve in the phase diagram?

A

Fusion curve: equilibrium between solid and liquid
Vaporization curve: equilibrium between liquid and gas
Sublimation curve: equilibrium between solid and gas

50
Q

What must happen to pressure and temperature in order for a solid to form?

A

high pressure, low temperature

51
Q

What must happen to pressure and temperature in order for a gas to form?

A

low pressure, high temperature

52
Q

Critical point or supercritical fluid

A
  • have a liquid and a gas at the same time at the highest possible (critical) temperature and (critical) pressure
  • located at the top end of the curve in the phase diagram
  • a superficial fluid has properties of both a liquid and a gas
  • makes it an amazing solvent
53
Q

Polarity

A

Difference in electronegativity in a molecule and permanent dipole

54
Q

What is the distance between two atoms in a crystal? Why can X-ray radiation be used to study crystals?

A

10^2 pm

X-ray radiation has wavelengths in this range

55
Q

When x-ray interacts with crystals what are the results?

A

Crystals are ordered so interference and diffraction patterns result. Diffraction pattern can then be used to relate distances between atoms of crystal.
Light parts= constructed interference
Dark parts=deconstructive interference

56
Q

Crystalline lattice

A

Regular arrangement of atoms/ions in a crystalline solid

57
Q

Unit cell

A

Small collection of atoms/ions/molecules that can be repeated over and over again to reproduce a 3D structure

58
Q

Coordination number

A

Number of atoms touching the central atom

59
Q

Simple cubic lattice

A

Coordination number: 6

Atoms per unit cell: (1/8 corners of each atom* 8 corners total=) 1

60
Q

Body-centred cubic

A

Coordination number: 8

Atoms per unit cell: 2

61
Q

Face-centred cubic

A

Coordination number: 12

Atoms per unit cell: 4

62
Q

List the cubic cells from least so most efficient in packing.

A

Simple cubic = 52%
Body-centred = 68%
Face-centred = 74%

63
Q

Simple cubic edge length

A

2r

64
Q

Body-centred cubic edge length

A

4r/root3

65
Q

Face-centred cubic edge length

A

(2root2)r

66
Q

What are the 2 closest-packed systems?

A

1) hexagonal closest packing

2) cubic closest packing

67
Q

Hexagonal closest packing (HCP): alternating layers, packing efficiency and coordination number.

A
  • 2 alternating layers slightly to the side (in between empty spaces)
  • ABABAB
  • 74% packing efficiency
  • coordination number=12
  • not simple cubic
68
Q

Cubic closest packing (CCP): alternating layers and coordination number

A
  • 3 alternating layers slightly to the side (in between empty spaces, top and bottom layers are different orientations)
  • ABCABCABC
  • coordination number=12
  • same as face-centred cubic!
69
Q

Name the types of crystalline solids.

A

1) molecular solids
2) ionic solids
3) atomic solids

70
Q

Crystalline solid: molecular solids

A
  • Composite units are molecules
  • Low melting point
  • ex) ice
71
Q

Crystalline solids: ionic solids

A
  • Composite units are formula units (cations and anions)
  • High melting points
  • Ex) Table salt
72
Q

Crystalline solids: Atomic solids

A
  • composite units are atoms

- types: nonbonding, metallic and network covalent

73
Q

Crystalline solids: Atomic solids: Nonbonding

A
  • held together by dispersion force
  • low melting points
  • Ex) solid xenon
74
Q

Crystalline solids: Atomic solids: Metallic

A
  • Held together by metallic bonds
  • Variable melting points
  • Ex) gold
75
Q

Crystalline solids: Atomic solids: Network covalent

A
  • held together by covalent bonds
  • high melting points
  • ex) quartz

CHEM 1310 - 2019 (2 decks)

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