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Chemistry 101 > States of Matter > Flashcards

States of Matter Flashcards

1
Q

Physical Properties of Gases

A
  1. Highly Compressible
  2. Infinately Miscible
  3. Theramlly Expendable
  4. Low Density

Gases exert pressure on its environment because the molecules are in constant motion

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2
Q

Boyle’s Law

A

At constant temperature, pressure is inversly proportional to volume

P1V1 = P2V2

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3
Q

Charle’s Law

A

At constant presssure, volume is direcly proportional to temperature

V1/T1 = V2/T2

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4
Q

Avagadro’s Law

A

At constant pressure and temperature, volume is directly proportional to the nember of moles

V1/n1 = V2/n2

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5
Q

Ideal Gas Law

A

PV = nRT

Note: only applies for ideal gases
* Calculations for real gases must be accomidated for particle volume and interparticle attraction

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6
Q

Dalton’s Law of Partial Pressure

A

In a mixture of non-reacting gases, the total pressure is the sum of the partial pressure of the individual gases

P(a) +P(b) = P(total)

or

P(total) = n(total) x (RT/V)

or mole fraction

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7
Q

Mole Fraction

Gases

A

An alternative way to express Dalton’s law of partial pressure.

X(a) = P(a)/(P(total))

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8
Q

Kinetic Molar Theory of Gases (Name the 5 rules)

A

A model of an ideal gas developed to explain the behaviour of real gases

Gases are made up of particles with no defined volume
* The particle size is so small compared to the distance seperating them that their volume is considered to be neglible

Particles are in continuous, random motion
* They have kinetic energy

Particles move independantly and experience no interparticle forces
* No attraction/repulsion
* They don’t have potential energy

Particles colide with eachother and with the walls of the container
* Colisions are elastic (no net loss of energy)

The average kinetic energy is the same for all gases at a given temperature
* Kenetic energy is proportional to temperature

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9
Q

What is the calculation of pressure in one dimension? What about 3?

A

1D. P = F/A

3D. P = (2/3)x((n(N(a)(1/2)mu^2)/V)

u^2 = Mean of the square to the speeds
m = Mass of the particles
N(a) = Avagadro’s number

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10
Q

What’s the requirement to be an ideal gas? What happens if the gas is above or below that value?

A

(PV)/(nRT) = 1

If above, the effect of particle volume dominates

If below, the effect of interparticle attractions predominates

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11
Q

What are the two things that can happen in gasses that make them fail to comply with ideal gas law?

A

They can experience weak interparticle attraction

They can occupy a finite volume

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12
Q

Van der Waals Equation

A

The equation that takes into accunt the interparticel attraction and the volume occupied by gas particles

P = (nRT)/(V-nb) - a(n/V)^2

b = Correction to volume
a = Correction to interparticle attraction

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13
Q

When is ideal gas behaviour oberved?

A

At low pressures and at high temperatures

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14
Q

Sublimation

A

The transfer from a solid to a gas

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15
Q

Deposition

A

The transfer from a gas to a solid

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16
Q

True or False

The transfer from a solid to a liquid is an exothermic reaction

A

False

It’s Endothermic
(Melting ice in water makes the water colder)

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17
Q

What are the commercial uses of supercritical (SC) fluids?

A
  • Caffine is extracted with it
  • Fat is reduced with it
  • Used in dry cleaning
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18
Q

What do you get under the combination fo the critical temperature (T(c)) and the critical pressure (P(c))?

A

A supercritical fluid
* This is very useful

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19
Q

Properties of Solids

A
  1. Molecules do not have the freedom of movement
  2. A solid keeps its shape no matter what the shapre of its container is
  3. The particles of a solid are very close together and interparticle forces ar every strong
  4. Density is a very improtant property
20
Q

Properties of Liquids

A
  1. Lack of rigidity and of compressibility
  2. Take the shape of the container they occupy
  3. Viscosity of a liquid can be measured
  4. Density is higher than that of a gas
21
Q

Types of intermolecular forces

A
  1. Ion-Dipole (P)
  2. Dipole-Dipole (P)
  3. H-bond (P)
  4. Induced Dipole (T)
  5. Dipole-induced dipole (T)
  6. London dispersion (T)

P = Permanant
T = Temporary

22
Q

Hydrogen bonding

A

A hydrogen bond results when a H that is covalently bonded to a more electronegative atom (N, O, F) interacts withat an electornegative atome of aanother molecule
* ONLY APPLIES TO N, O, AND F
* This is another type of dipole-dipole bond, just stronger

23
Q

What are the types of temporary dipoles

A

Thes occur in atoms that have the same, or very similar electronegativities

  1. Ion-induced dipole
  2. Dipole-induced dipole
  3. Induced dipole-induced dipole (london dispersion)
24
Q

What are the characteristics of London Dispersion

A
  1. Creates an instantaneous intermolecular (or interparticle) attraction that is short-lived and weak
  2. The higher the atomic mass (molar mass), the higher the probability for the formation of instant dipoles of larger magnitude
  3. They are not strong enough to lead the formation of liquid in low molecular weight compounds at room temperature
25
What factors impoact the strength of London Dispersion in a molecule
* Molar mass * Shape * More surface area = stronger LDF
26
What are the factors to consider when deciding about the intensity of intermolecular forces
**Comparing non-polar compounds** * Molar mass * Molecular Shape **Comparing polar and non-polar compounds with *comparible molar masses*** * Polar substances have higher IMF **When comparing polar compounds** * Presence of H-bonding
27
Surface tension
The resistance of a liquid to go flat on a surface (increase surface area) * High surface area = Strong IMF * The stronger the IMF, the higher the surface tension
28
Capillarity vs Wetting
**Capillarity** - The spontaneous rising or decsent of a liquid in a capillary tube **Wetting** - The ability of a liquid to maintain contact with a surface Both involve the competition of cohesive and adhesive forces
29
Cohesive vs Adhesivse Forces
**Cohesive Forces** * The IMF betwen the molecules of a liquid **Adhesivse Forces** * The forces of attraction between molecules of a liquid and the particles presant on the surface of the container If **adhisive is stronger than cohisive**, the liquid rises and forms concave meniscius If **cohisive is stronger than adhesive**, the liquid descends and forms a convex meniscius
30
Viscosity
The resistance of a liquid to flow * High viscosity = high IMF * Raising temperature lowers viscosity Note: in engine oils this is a very important trait Eg. 5W-3o vs 10W-3o Higher W = higher viscosity o refers to risistance to thinning
31
Vapor Pressure of liquids
The Equilibrium of the vapor above the liquid. It results from the evaporation of the liquid. * The stronger the IMF in the liquid, the higher the boiling point, the lower the vapor pressure
32
What are the two general catagories of solids
**Crystaline Solids** * Characterizeed by a highly ordered assemply of their components **Amorphous Solids** * Characterized by a random assemply of their components
33
What are the types of crystaline solids
**Discrete molecular solids** * **Non-polar** * Soft * Low melting point * Does not conduct * **Polar Hydrogen bonded** * Soft * Low to moderate melting points * Poor Conductors **Extended Structures** * **Ionic** * Hard & brittle * High melting point * Non-conductors in solid, good conductors in liquid * **Giant Covalent** * Very Hard * High melting point * Poor conductor * **Metalic** * Soft to hardish * Usually high melting point * Ductile
34
What are the types if cubic lattices? What are their coordination numbers?
Simple Cubic (or primative) * CN = 6 Body-Centered Cubic (BCC) * CN = 8 Face-Centered Cubic (FCC) * CN = 12 CN = Coordination number = The number of neighbors that a central particle is in contact with in a crystaline structure
35
Square-packing vs close-packing | Crystals
Square packed structure * Each atom has 4 closest neigbors Close-packed strucure * Each atom has 6 closest neighbors
36
What are the types of close packing?
**Packing leading to hexagonal close packing** * Atoms of the 3rd layer sit on the tetrahedral holes *which means directly on top of atoms in layer A* **Packaging leading to cubic close packing** * ABC ABC type arrangement * Atoms of the 2nd layer (layer B) are surrounged by 6 atoms in the same layer, 3 atoms in layer A and 3 atoms in layer C
37
Formation of alloys
Atoms of a metal occupy the intersitces (holes) of another metal * Increases mechanical strength * 2nd metal contributes additional valence electrons to metallic bonding
38
Density of metallic solids
Information required to calculate density of metallic solids * Number of atoms in a unit cell (Net attoms) * Length of the unit cell * Volume of the unit cell Density = mass/volume
39
Are alcohols soluble in water?
4C and 5C alcohols have borderline solubility in water, Alcohols of 6C and more are soluble
40
What’s the magic ratio for molecular weight to take precedence over polarity in determining boiling point
The non polar molecule must move a M (g/mol) **3 times larger** than the polar molecule
41
# True or false Metals and metal alloy solids always have extended structure
True The atoms are held together by the "sea" of delocalized electrons
42
Diamond vs Graphite structure
Each carbon in diamond is bonded to 4 other carbons * No free electrons sp3 In graphite, carbon atoms are layered, each charbon is bonded to 3 other carbons * Sheets stack on top of eachother and are held together by Van der Waals forces
43
Graphite vs Bucky Ball vs Carbon Nanotubes Structure
**Graphite** * Carbon bonded to three other carbons in a 2D sheet * Many layers * Extended structure **Bucky Ball** * Molecular sturcture * Same bonding as in graphite **Carbon Nanotubes** * Same structure as a single sheet of graphite, just in a roll
44
What force dominates when (PV)/(RT) < 1
**Interparticle attraction** At low pressures, heavy molecules fall here "a" is correction to pressure
45
What force dominates when (PV)/(RT) > 1
**Particle volume** This is the lighter gases * At higher pressures, heavy gases also fall here "b" is correction to volume
46
How do you find density of air
D = MP/RT

Chemistry 101 (6 decks)

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