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Honors Chemistry > First Test > Flashcards

First Test Flashcards

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1
Q

standard significant figures rules :

A 
leading 0 = no
sandwich 0 = yes 
tailing if there's a decimal = yes 
trailing if there's no decimal = no 
0 before other significant numbers = no
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2
Q

addition & subtraction significant figures rules :

A

answer should contain as many decimal places with the LEAST amount of places

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3
Q

multiplication & division significant figures rules :

A

only contain as many significant figures as the least number of them in the equation

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4
Q

calorimetry & heat

A

the process for the measurement of the heat into or out of a system of chemical and physical process; measured in joule (J)

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5
Q

calorimeter

A

device used to measure absorption or release of thermal energy

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6
Q

what is being measured when using a calorimeter

A

temperature change induced on a measured mass of water

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7
Q

law of conservation of energy

A

the amount of energy released by a process must be equal to the amount of energy absorbed by the rest of the system

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8
Q

heat capacity

A

the amount of heat needed to increase the temperature of an object exactly 1 degree Celsius

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9
Q

heat capacity for 100g of air

A

101 J/g C

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10
Q

heat capacity for 100g of water

A

41.79 J/g C

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11
Q

specifit heat capacity

A

the amount of heat it takes to raise the temperature of exactly 1 gram of the substance by 1 C

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12
Q

heating curve straight line rules :

A
  • temp is constant
  • heat & potential energy is constant
  • bonds are breaking
  • equilibrium is being achieved
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13
Q

heating curve slanted line rules :

A
  • increase in temp

- kinetic energy is going up

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14
Q

matter =

A

physical material of the universe that has define mass & volume

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15
Q

pure substance =

A
  • contain the same composition of material throughout; each piece has the same chemical makeup
  • can’t be separated by physical means
  • has a formula
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16
Q

element =

A
  • simplest form of matter
  • made of 1 atom
  • can’t be broken down chemically
  • 2 types: normal and diatomic (atoms in pairs)
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17
Q

compounds =

A
  • 2 elements chemically combined
  • always fixed ratio
  • has at least 2 or more chemical symbols
  • doesn’t protein their chemical properties alone
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18
Q

5 ways to break down compounds chemically:

A
  • reations
  • smelting
  • combustions
  • electrolysis
  • cracking
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19
Q

mixtures =

A
  • composed of 2 or more distinct substances
  • can be broken down physically
  • not chemically combined
  • composition can vary
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20
Q

homogeneous mixture

A
  • same throughout

- uniformly dispersed

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21
Q

aqueous =

A

water solution

transparent

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22
Q

alloy =

A

mixture of metals that aren’t chemically combined

ex. steel (iron and carbon)

23
Q

heterogeneous mixture =

A
  • isn’t uniformly dispersed
  • particles are too large
  • composition varies
24
Q

filtration =

A
  • solid is recovered from mixture

- draining

25
Q

vaporization =

A

-transition from liquid to gas

26
Q

distillation

A

boiling point

27
Q

chromatography

A

difference in solubility

28
Q

2 types of energy =

A
  • kinetic

- potential

29
Q

measuring potential energy =

A

has to be converted to kinetic and used to measure by calorimeter

30
Q

kinetic energy =

A

energy of motion contained by anything that moves

31
Q

temperature =

A
  • measure of average kinetic energy passed by the particles of an object
  • measures how fast or slow the particles are moving
32
Q

difference in kelvin and celsius

A

k = c +273

33
Q

0 point on kelvin scale =

A

absolute 0; particles have stopped moving

34
Q

thermal energy movement

A

from hot to cold

35
Q

endothermic =

A

heat travels into an object; object is getting hotter

36
Q

exothermic =

A

object is getting colder; heat travels out of object

37
Q

heat energy of substance depending =

A
  • amount of material
  • identity of material
  • change in temp
38
Q

heat =

A

how energy is transferred & the movement of thermal energy

39
Q

intermolecular attractive forces =

A
  • attractive forces between molecules

- the strength of said forces determine what phase of matter substances are in at a given temp

40
Q

substances with weak forces =

A

tend to be a gas at room temp

41
Q

substances with strong attractive forces =

A

tend to be a solid at room temp

42
Q

phases of matter =

A

stages of attraction

43
Q

ideal gasses =

A

-made of molecules of low imf’s allowing molecules to fly past each other

44
Q

liquids imf’s =

A
  • stronger attractive forces

- particles moving past each other but stay together

45
Q

solids imf’s =

A
  • strong attractive forces which hold the particles to vibrate
  • can’t move relative to each other
46
Q

phase of substance depending =

A

temperature and pressure

47
Q

force and pressure =

A 
force= how hard you push 
pressure= how spread out the push is
48
Q

pressure measure =

A
  • atmospheres (atm)
  • kilopascals (kPa)
  • torricelli (torr)
  • millimeters of mercury (mm Hg)
49
Q

standard pressure =

A

1 atm = 101.325 kPa = 760 torr = 760 mm Hg

50
Q

standard temperature

A

273 k = 0 C

51
Q

phase change involving particles moving FARTHER apart =

A

energy must be absorbed in order to overcome the attractive forces between them

52
Q

phase change involving the particles moving CLOSER together =

A

energy must be RELEASED to pull the particles closer together

53
Q

phase equilibrium =

A
  • condition where the rates of opposing changes are equal

- during phase change, both phases exist at equilibrium

Honors Chemistry (3 decks)

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