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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

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

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

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)

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

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

25
Q

State of matter depends on…

A

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

26
Q

Combined Gas Law

A

PV=nRT

27
Q

STP

A

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

28
Q

1atm =

A

760 mmHg=760 torr=101.3 kPa

29
Q

Molar mass equation

A

M = dRT/p

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

11th Grade (1 decks)

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