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11th Grade > Intermolecular Forces and Properties > Flashcards

Intermolecular Forces and Properties Flashcards

1
Q

Types of Intermolecular Forces

A

London Dispersion Factors/Induced Dipole-Induced Dipole, Dipole-Dipole Attractions, Hydrogen Bonding, Ion-Dipole Attractions

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2
Q

Types of Intramolecular Forces

A

ionic, metallic, and covalent bonds

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3
Q

Which forces are strong? Intermolecular or Intramolecular

A

Intramolecular

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4
Q

London Dispersion Forces

A

Motion of Electrons create momentary dipoles
Occurs between all molecules and sometimes stronger than dipole-dipole forces

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5
Q

Polarizability

A

the ease with which the electron distribution in a molecule can be distorted (‘squashiness’ of the electron cloud)

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6
Q

+ Polarizability =

A

+ Dispersion Forces

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7
Q

What molecules have more polarizability?

A

Molecules with a greater molar mass have a greater # of electrons and, therefore, greater polarizability and more dispersion forces
Molecular shape also influences dispersion forces → if molecules can pack more tightly together in a long/cylindrical shape then they have greater dispersion forces than a spherical molecule

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8
Q

Dipole-Dipole Interactions

A

Attraction between the partially charged ends of polar molecules
+ polarity = stronger forces

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9
Q

Dipole-Induced Dipole Forces

A

A polar molecule induces or creates a momentary dipole in a neighboring nonpolar molecule

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10
Q

Hydrogen Bonds

A

Attraction between a hydrogen atom that is covalently bonded to a highly EN atom (N, O, F) and a nearby highly EN atom (N, O, F) in another molecule
Stronger than dipole-dipole but weaker than ion-dipole

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11
Q

Ion-Dipole Interactions

A

Attraction between an ion and a polar molecule
Increase in charge or polarity = increase in force
Smaller ions have stronger attractions with polar molecule

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12
Q

Comparing Relative Strengths of IMFs in two substances

A

If they have similar molar masses and shapes then dispersion forces are ~equal in the substances-more polar molecules have greater attraction

If they have very different molar masses, then dispersion forces are the most important attractive forces-the bigger the molecule, the greater the number of electrons, the greater the polarizability, the greater the dispersion forces

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13
Q

Ranking Strengths of Intermolecular Forces

A

Dispersion Forces, Dipole-Dipole, Hydrogen Bond, Ion Dipole Interactions

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14
Q

Vapor Pressure

A

The pressure exerted by a liquid’s vapor phase when the liquid and vapor states are in equilibrium
Increase in temp = Increase in vapor pressure

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15
Q

Volatile

A

Liquids that evaporate easily due to low IMFs

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16
Q

Increase in IMFs = increase…

A

Melting point, boiling point, surface tension, viscosity (resistance to flow), heat of vaporization (energy required to evaporate)

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17
Q

Increase in IMFs = decrease…

A

Vapor Pressure, volatility

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18
Q

Types of Solids

A

Metallic Solids, Ionic Solids, Covalent-network solids, Molecular Solids

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19
Q

Ionic Solids

A

Held together by electrostatic attraction between cations and anions held in a 3D lattice structure
High Melting and Boiling points
Brittle
Poor conductors of electricity unless they’re aqeuous

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20
Q

Molecular Solids

A

Held together by IMFs
Relatively low melting and boiling point due to the weak IMFs holding the molecules together
Poor conductors of electricity because the electrons are held tightly in covalent bonds

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21
Q

Covalent-Network Solids

A

Formed by atoms all held together in large networks by covalent bonds
Hard solids, high melting points due to being held in solid state by covalent bonds

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22
Q

Types of Covalent-Network Solids (8)

A

diamond, graphite, silicon, germanium, quartz (SiO­2), silicon carbide (SiC), boron nitride (BN), and boron carbide (BC)

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23
Q

Metallic Solids

A

Held together by delocalized ‘sea’ of collectively shared valence electrons
Great conductors of heat and electricity
Melting points vary depending on the element

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24
Q

Polymers

A

Contain long chains of atoms (usually carbon), where atoms within a chain are held together by covalent bonds but adjacent chains are held together by IMFs

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25
Q

State of matter depends on…

A

balance between the kinetic energies of the particles
the attractive forces between the particles

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26
Q

Ideal Gas Law

A

PV=nRT

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27
Q

STP

A

0 degrees Celsius, 1 atm, and 1 mole of gas occupies 22.4L

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28
Q

1atm =

A

760 mmHg=760 torr=101.3 kPa

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29
Q

Molar mass equation

A

M = dRT/p

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30
Q

Dalton’s Law of Partial Pressure

A

P total = P1 + P2 +…

31
Q

Calculating Vapor Pressure over water

A

P total = P H2O + P gas

32
Q

Mole Fraction

A

Xa (mole fraction) = na (mole of substance)/ ntotal (total moles)

33
Q

Calculating partial pressure

A

Pa (partial pressure of gas) =Xa (mole fraction)/ Ptotal (total pressure)

34
Q

Kinetic-Molecular Theory of Gas

A

Gas particles are in constant, random motion
Gas particles do not take up space (volume of particles is negligible)
Gas particles do not attract or repel each other
Average kinetic energy of gas particles remains constant (energy is conserved when collisions occur)
Average kinetic energy of gas particles is directly proportional to temperature in Kelvin

35
Q

Effusion

A

Diffusion of gas through a small hole

36
Q

Diffusion

A

Diffusion of gas from a high concentration to a low concentration

37
Q

The speed of gas is dependent on what?

A

Molar mass and temperature
High temp = faster particle
Small molar mass = faster particle

38
Q

Graham’s Law of Effusion

A

r1/r2 = square root (molar mass of 2/molar mass of 1)

39
Q

Deviation from ideal gas law

A

High pressure and low temperature
At low pressures the volume is small relative to the space between the particles so it is negligible. But at high pressures the idea gas law predicts a volume to low because it doesn’t account for the volume of the particles. At high temperatures, the particles move to faster for there to be any attraction. But at low temperatures, the attraction impacts the pressure so the ideal gas law predicts a too large pressure.

40
Q

PARTICLES will deviate the most if…

A

Particles have the potential to have greater IMFs (more important)
Large particles

41
Q

Molarity =

A

mols solute/L

41
Q

Homogeneous vs. Heterogeneous mixtures

A

Homogeneous mixtures are uniform in physical appearance while Heterogeneous mixtures are not

42
Q

When can dispersion forces be greater than dipole-dipole forces?

A

When the molecule has a big molar mass which leads to more electrons which leads to more polarizability which leads to more Dispersion forces

43
Q

Increase in temperature =

A

Increase in vapor pressure

44
Q

Using mole fraction to calculate partial pressure

A

Pa=XaPtotal or Xa=Pa/ptotal

45
Q

When creating or analyzing particulate models, pay attention to…

A

Size of ions, Orientation of solute and solvent particles, and relative number of particles

46
Q

Chromatography

A

Used to separate components in a solution due to relative attraction forces among the components in the mobile (solvent) and stationary (paper) phases
In this, the solvent is usually polar and the paper is usually nonpolar

47
Q

What are the three types of chromatography?

A

paper, thin-layer, and column chromatography

48
Q

Polar components in a solution in chromatography will…

A

interact less with the stationary phase and will travel further by interacting more readily with the polar mobile phase

49
Q

Less polar components of the solution in chromatography will.

A

interact more with the stationary phase and will not travel as far (by interacting more readily with the nonpolar stationary phase

50
Q

Distillation

A

Used to separating components in a solution due to different strengths of intermolecular forces and therefore different boiling points

51
Q

Distillate

A

The substance that boils at a lower temperature that vaporizes and condenses into another container

52
Q

Substances with similar IMFs will tend…

A

To be more soluble (or miscible)

53
Q

What dissolves in what? (Ionic compounds, polar molecules, Nonpolar molecules)

A

Ionic compounds dissolves better in polar solvents (ion-dipole forces)
Polar molecules dissolves better in polar solvents (dipole-dipole forces)
Nonpolar molecules will dissolve better in Nonpolar molecules (LDFs)

54
Q

Interactions in a solution

A

Solute-solute Interactions, solvent-solvent Interactions, and solvent-solute interactions

55
Q

Solutions form when…

A

solvent-solute interactions are greater than the SUM of the solute-solute and solvent-solvent interactions

56
Q

Hydration

A

When a solvent is dissolving in water

57
Q

Spectroscopy

A

Matter can absorb or emit radiation in different regions of the electromagnetic radiation spectrum, and those regions are associated with molecular motion and electronic transitions

58
Q

Types of Spectroscopy

A

X-ray: Highest; Removes core electrons; tells us binding energy (helps identify the element) due to measuring how tightly e- are held; known as photoelectron spectroscopy
Ultraviolet: High; Excites valence electrons and trasitions in energy levels; tells us the identity of a molecule or element; Visible Spectroscopy
Visible Light: Medium; Excites valence electrons; identifies the concentration of a molecule; Visible spectroscopy
Infrared: Low; Changes/Transitions the vibrations in the bonds; tells us the types of bonds/atoms/functional groups; vibrational spectroscopy
Microwaves: Quite low; changes/transitions the rotations of the atoms in the bonds; tells us the location of hydrogen atoms within a molecules; rotational spectroscopy

59
Q

Electromagnetic Radiation

A

Light

60
Q

Speed of Light

A

3.00 * 10^8 m/s

61
Q

Frequency

A

Number of cycles/waves that pass a given point in 1 second
Symbols: f or nu (v thing)
Units: s^-1 or Hz

62
Q

Wavelength

A

Distance from 1 peak to the next
Symbol: lambda (tent thing)
Units: meters

63
Q

C=

A

frequency times wavelength

64
Q

Planck’s Idea

A

Energy can be released or absorbed in specific amounts called quanta

65
Q

A quantum of energy

A

Smallest amount of energy that can be emitted/absorbed

66
Q

Planck’s Constant (h(

A

6.626 * 10^-34 Js

67
Q

E=

A

hv

68
Q

Spectrometer

A

Measures the amount of light absorbed by a sample by comparing the intensity of light emitted from a light source with the intensity of the light emerging from the example

69
Q

Beer’s Law

A

Relates amount of light absorbed to the concentration of the substance absorbing the light

70
Q

Dynamic Equilibrium

A

Condition in which two opposing processes occurring simultaneously at equal rates

71
Q

A=

A

Ebc
A= measured absorbance
E (thing) = molar absorptivity constant (how intense a sample absorbs light of a particular wavelength)
b= path length (distance light is traveling when it goes through the sample)
c= concentration

72
Q

Normal Boiling Points

A

Boiling point at 1 atm

73
Q

Mean free path

A

Average distance traveled by a molecule between collisions

11th Grade (5 decks)

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