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Chemistry > Unit Six > Flashcards

Unit Six Flashcards

(63 cards)

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1
Q

Liquid

A

Medium packed particles, medium motion

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2
Q

Gas

A

Loosely packed particles, high motion

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3
Q

Temperature

A

A measure of the average kinetic energy particles of a substance have

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4
Q

Heat

A

Transfer of kinetic energy from a hotter object to a cooler one

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5
Q

Melting

A

Solid to liquid

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6
Q

Freezing

A

Liquid to solid

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7
Q

Vaporization

A

Liquid to gas

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8
Q

Condensation

A

Gas to liquid

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9
Q

Sublimation

A

Gas to solid

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10
Q

Deposition

A

Solid to gas

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11
Q

Fahrenheit to Celsius

A

F = 1.8 C + 32

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12
Q

Celsius to Fahrenheit

A

C = (F - 32)/1.8

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13
Q

Celsius and Kelvin

A

K = C + 273

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14
Q

Pressure conversions

A

1 atm = 14.7 psi = 101 kPa = 7.60x10^2 mm Hg (torr)

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15
Q

STP

A

Standard temperature and pressure, 1 atm and 273 K

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16
Q

Intramolecular forces

A

Hold the atoms of a molecule together

Ex. Ionic bonds, polar covalent bonds, nonpolar covalent bonds

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17
Q

Intermolecular forces

A

Hold molecules of a substance together

Ex. Dipole-dipole, hydrogen bonding, dispersion forces

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18
Q

Dispersion forces

A

Weak forces resulting from temporary shifts in electron densities, stronger for larger particles
In nonpolar molecules, bigger molecules = bigger force
Weakest type of intermolecular bonds

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19
Q

Dipole-dipole forces

A

Attraction between oppositely charged region of polar molecules
Polar covalent
Middle strength

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20
Q

Hydrogen bonds

A

Dipole-dipole attraction occurring between molecules containing hydrogen boned to fluorine, oxygen, or nitrogen
Strongest because greatest difference in electronegativity
Polar covalent
Strongest type

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21
Q

Are hydrogen bonds or ionic bonds stronger

A

Ionic because hydrogen is partial charges and ionic is full charges

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22
Q

Liquid density

A

Denser than gases

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23
Q

Liquid compression

A

Cannot compress a liquid (definite volume)

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24
Q

Liquid fluidity

A

Particles in a liquid do not have fixed locations

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25
Liquid viscosity
A measure of resistance of a liquid to flow
26
Factors affecting viscosity
Stronger intermolecular forces mean greater viscosity Larger and longer molecules will form more viscous solutions Viscosity decreases with temperature
27
Surface tension
Energy required to increase the surface area of a liquid Because intermolecular forces at the center of the liquid experience balanced attractions on all sides while molecules at the surface are only pulled inward, thus creating a taught surface
28
Cohesion
Attraction between identical molecules
29
Adhesion
Attraction between different molecules
30
Capillary action
What happens when the adhesion forces overcome the cohesion forces
31
Solid
Closely packed particles, low motion
32
Special properties of water due to hydrogen bonding
High melting and boiling point (takes more energy to line up or separate hydrogen bonds) Surface tension and capillary action (strength of hydrogen bonds pulls them to the center of the liquid and towards one another and their container) Solid water is less dense than liquid water (when cooled hydrogen bonds align in a spacious crystal pattern that makes the ice less dense than the water bc of liquid molecules) Universal solvent (neutral, no net charge, can dissolve most things)
33
Crystalline solids
Atoms, ions, or molecules in an orderly, geometric structure
34
Molecular solid
Covalent substance, break down easily, soft, low melting points, water, sugar, dry ice
35
Covalent network solid
Crystal structure, carbon, silica
36
Ionic solid
Soluble, high melting points, salts
37
Metallic solid
Orderly atoms, ductile, malleable, any metal
38
Allotropes
``` Multiple different forms of the same state Ex carbon (diamond, graphite, etc) ```
39
Amorphous solids
Solid where particles are not arranged in a repeating pattern Ex obsidian, glass rubber
40
Properties of gases
Gases are fluids Gases are highly compressible Gases completely fill containers Gases have lower densities than liquid and solids
41
KMT
Kinetic molecular theory, describes the motion of particles Gas molecules are in constant, random motion Gas molecules are separated by huge distance relative to the size of the molecules themselves Gas molecules have no attractive/repulsive forces Gases are made of molecules that have mass Molecules undergo elastic collisions
42
Relationship between temperature and kinetic energy
Temperature and energy of molecules are directly proportional If temperature increases the kinetic energy increases
43
Boyle's law
P1V1 = P2V2, inverse relationship
44
Charles law
V1/T1 = V2/T2, direct relationship
45
Gay-Lussac law
P1/T1 = P2/T2, direct relationship
46
Avogadro law
22.4 L = 1 mole gas
47
Combined gas law
P1V1/T1 = P2V2/T2
48
Ideal gas law
``` PV = nRT P = pressure in atm V = volume in liters n = moles R = 0.08205 if atm, 8.31 if kPa T = temperature in kelvin ```
49
Ideal gas
Gases that behave according to the assumptions of kinetic molecular theory
50
Assumptions made for ideal gases
No intermolecular forces | Individual molecules have no volume
51
Conditions where real gases behave ideally
High temperature and low pressure
52
Diffusion
Gas particles will travel from an area of high concentration to an area of low concentration until they are evenly distributed
53
Effusion
Passage of a gas through a small hole/opening in a barrier
54
Graham's law of effusion
Gases that have larger molar masses move more slowly than lighter gases
55
Avogadro's hypothesis
Equal volumes of gases at the same temperature and pressure contain equal number of particles
56
Other things about Avogadro's hypothesis
Due mainly to the large amount of empty space between particles From this, scientists have determined that one mole of gas = 22.4 L at STP
57
Dalton's law of partial pressure
The total pressure for a mixture of gases is equal to the sum of the pressures of the individual gases in the mixture Ptotal = P1 + P2 + Px
58
On a phase diagram, the top third is
Solid
59
On a phase diagram, the middle third is
Liquid
60
On a phase diagram, the bottom third is
Gas
61
Triple point
The temperature and pressure where all three phases of matter could exist Where the three lines converge and meet at a single point
62
Critical point
Pressure and temperature above which distinct gas and liquid phases don't exist
63
Density formula
D = m/v

Chemistry (12 decks)

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