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honors chemistry > unit 1 > Flashcards

unit 1 Flashcards

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1
Q

whats the 1st law of thermodynamics (law of conservation of mass)

A

matter, energy or charge cannot be created or destroyed

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2
Q

whats a pure substance

A

something that has the same composition and properties throughout (elements and compounds)

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3
Q

whats a element

A

substances composed of all the same atom

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4
Q

whats a compound

A

contains two or more different elements chemically combined in fixed proportions, and can be broken down by a chemical change

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5
Q

whats a mixture

A

a combination of two or more pure substances that can be separated by physical means

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6
Q

whats a homogenous mixture

A

a mixture in which different substances are blended evenly throughout (ex. glass cleaner)

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7
Q

whats a heterogenous mixture

A

a mixture in which different materials are easily distinguishable (ex. pizza)

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8
Q

whats filtration

A

seperation of a heterogenous mixture

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9
Q

whats crystallization

A

separation by different freezing points or vapor pressure (evaporation)

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10
Q

whats disilliation

A

separation based on different boiling points; different from evaporation

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11
Q

whats chromatography

A

separation based on substances affinity for a medium

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12
Q

whats accuracy in chemistry

A

how close the measurement is to the actual value

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13
Q

whats precision

A

how reproducible the measurements are

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14
Q

whats % error

A

((measured - accepted)/accepted) x 100

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15
Q

what are the two different types of energies

A

potential energy and kinetic energyw

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16
Q

what is potential energy

A

stored energy

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17
Q

what is kinetic energy

A

energy of motion

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18
Q

what are some forms of energy

A

heat, light, electricity, chemical, nuclear

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19
Q

whats the law of conservation of energy

A

energy cannot be created or destroyed

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20
Q

what is heat not and what is it actually

A

heat is not temperature, it is the energy itself

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21
Q

what is temperature

A

the amount of heat a material has

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22
Q

what is the equation to find heat energy

A

q = MCΔT

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23
Q

what is temperature a measure of

A

average kinetic energy of a material

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24
Q

what is the celsius scale based on

A

the freezing point (0c) and boiling point (100c) of water. zero degrees celsius doesnt mean zero average kinetic energy

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25
what is the kelvin scale
0K = the absolute 0, where all kinetic energy has ceased.
26
whats the formula to convert C to K
K = C + 273
27
whats specific heat
its a physical property of matter, and is how a material response to the addition or loss of heat, in joules per gram Celsius its the amount of heat energy that is required to raise 1g of a substance by 1c
28
what is freezing and what is the nature of it
liquid to solid, exothermic
29
what is melting and what is the nature of it
solid to liquid, endothermic
30
what is condensation and what is the nature of it
gas to liquid, exothermic
31
what is vaporization and what is the nature of it
liquid to gas, endothermic
32
what is sublimation, and what is the nature of it
solid to gas, skipping the liquid intermediate phase. it is endothermic
33
what is deposition, and what is the nature of it
gas to solid, skipping the liquid intermediate phase. it is exothermic.
34
what is the heat of fusion (Hf)
the amount of heat energy (in J) required for a material to change from solid to liquid (melting). its equal to the temperature of where it starts to flatline
35
what is the heat of vaporization (Hv)
the amount of heat energy (in J) required for a material to change from liquid to gas (boiling). its equal to the temperature of where it starts to flatline.
36
what phases is the material at the heat of fusions
solid and liquid
37
what phase is the material at the heat of vaporization
liquid and gas
38
what is the added heat energy being used for in a slanted part of a heat graph
to increase the average kinetic energy
39
what is the added heat energy being used for in a flat part of a heat graph
to break the bonds of a substance, and change phases. average kinetic energy stays the same.
40
whats an exothermic reaction
when energy is released, in phase changes such as freezing and condensation
41
whats an endothermic reaction
when energy is absorbed, in phase changes such as melting and boiling
42
what does a catalyst do
speeds up the reaction without being used up or changed
43
what is chemical energy
chemical energy is stored potential energy in a chemical bond, which hold compounds together.
44
what happens when bonds are broken and new bonds are formed
the amount of energy that is stored changes
45
what happens if there is a change in y value
change in average kinetic energy
46
what happens if there is no change in y value
change in potential energy
47
whats enthalpy (heat of reaction)
the amount of heat energy absorbed or released during a chemical change. known as ΔH (heat of products - heat of reactants)
48
how to identify a a exothermic reaction and what does the ΔH look like
if the products have less energy then the reactants. the extra energy is released into the surroundings. The ΔH would be negative
49
how to identify a endothermic reaction and what does the ΔH look like
if the products have more energy then the reactants. the extra energy is absorbed from surroundings. The ΔH would be positive
50
what is the potential energy in a exothermic reaction for the reactants and products
reactant potential energy is higher then the potential energy of the products
51
what is the potential energy in a endothermic reaction for the reactants and products
reactant potential energy is lower then the potential energy of the products
52
what is activation energy (Ea)
the energy required to initiate a chemical reaction.
53
what does the activation energy (Ea) ensure?
it ensures that when molecules collide, they have enough energy for a effective collision (for them to react and become products)
54
how does Ea change with a catalyst
it decreases
55
how does catalyst effect ΔH
it doesn't
56
what is an example of a catalyst
an enzyme
57
what's kinetic molecular theory
KMT for an ideal gas states that: 1. they are in random, constant, straight-line motion 2. they are separated by great distances relative to their size (but the gas particles themselves have negligible volume) 3. they have neither attractive nor repelling forces between them 4. have collisions that may result in a transfer of energy between gas particles, but the total energy of the system remains constant. 5. the collisions are perfectly elastic
58
whats ideal gas concept
model to explain the behavior of gases. gases are closest to behaving as an ideal gas at low pressures and high temperatures
59
what happens when molecules collide
they can bounce apart or react to form something new
60
whats collision theory
if particles collide with the proper energy and orientation, a chemical reaction (change) can occur
61
what does kinetic molecular theory describe
the relationship of pressure, volume, temperature, velocity, frequency and force of collision among gas molecules
62
whats pressure
a forced exerted on a specific area (force divided by area)
63
how do gases exert pressure
by colliding with other gas molecules or their container. if there is no collisions, there is no pressure, and this is known as a vacumn
64
what is the kinetic-molecular view of gas pressure
gas pressure comes from the force of molecular collisions anything that increases the # of collisions will increase the pressure
65
what are all the units for pressure
pascals (pa) at sea level: 101.3 kPa mmHg (millimeter of mercury) at sea level: 760 mmHg Torr (torr) at sea level: 760 Torr atmospheres (atm) at sea level: 1 atm
66
what is vapor pressure
pressure of vaporizing liquid exerted by liquid
67
how does boiling occur in terms of vapor pressure
atmospheric pressure pushes down on the liquid, keeping the molecules in the liquid if VP = atmospheric pressure, liquid molecules can escape out of the liquid and boiling will occur
68
what happens if you increase temperature
there will be an increase in energy, which will allow for boiling
69
what happens if you increase elevation
atmospheric pressure will decrease, therefore allowing for less energy to be needed to trigger boiling.
70
what happens to boiling point if you increase vapor pressure (VP)
boiling point decreases
71
what happens to ΔT as VP increases
ΔT increases
72
what happens to ΔT as BP increases
ΔT decreases
73
whats volume
the amount of space a gas occupiesw
74
whats velocity
how fast the particles are moving (speed)
75
what does increasing temperature do in terms of velocity
it increases the velocity of the particles
76
what does increasing weight do in terms of velocity
it decreases the velocity
77
whats STEVEN
same temp = equal volume, equal # of particles
78
whats avogadro hypothesis
STEVEN equal volumes of gas at the same temperature and pressure contain and equal number of particles (STEVEN)
79
whats boyle's law
the pressure will increase as volume decreases if temperature is constant (ex. a piston) P1V1 = P2V2
80
whats charles's law
the volume will increase as temperature increases if the pressure is constant (ex. a hot air balloon) V1/T1 = V2/T2
81
why does charles law happen
it happens because the container must get bigger for the pressure to stay the same. increase in temp = increase in collisions with container wall if the walls are flexible, they'll get pushed back, and the gas expands
82
whats the combined gas law formula
(P1)(V1)/T1 = (P2)(V2)/T2
83
whats the combined gas law
when there is a change in temperature and pressure. this doesn't match
84
what is the standard temperature
0c or 273K
85
what is the standard pressure
1atm/101.3kPa/760torr/760mmHg
86
how do you seperate a homogeneous solution
distillation, chromatography, crystillization

honors chemistry (6 decks)

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