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Chem 101 > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

Study of matter and it’s transformations

A

Chemistry

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2
Q

Anything that has mass

A

Matter

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3
Q

F=MA

A

Force=massxacceration

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4
Q

Everything around us that is made up of matter is made up from atoms

A

Atomism

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5
Q

Matter that cannot be separated by physical means

A

pure substance

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6
Q

Matter that can be separated by physical means

ex) filtration

A

mixture

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7
Q

pure substance made up of only one type of atom and cannot be separated into simpler substances

ex)H2

A

elements

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8
Q

pure substance made up of more than one type of atoms that are chemically bonded

ex)NaCl

A

compounds

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9
Q

mixture in which you can see the individual particles

can be separated by filtration

ex) sandy water, italian dressing

A

heterogeneous

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10
Q

mixture in which you cannot see the individual particles

cannot be separated by filtration

ex) coffee, soda, air

A

homogeneous

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11
Q

property that depends on the amount of substance present

ex) length, mass, volume

A

extensive properties

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12
Q

property in which the amount of substance present is not relevant

ex) color, melting point, density

A

intensive properties

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13
Q

a measurement of how tightly packed the particles in a substance are

A

density

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14
Q

why is density not an extensive property?

A

because every element spaces has a specific density

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15
Q

D=m/v

A

density=mass/volume

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16
Q

properties that can be measured without changing the substance into another

ex) intensive and extensive properties
ex) boiling point (water into steam)

A

physical properties

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17
Q

properties that can only be observed by reacting the substance with something else to create a another substance

ex) combustion, corrosion

A

chemical properties

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18
Q

the tendency of a substance to burn when reacted with oxygen

A

combustion

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19
Q

tendency of a substance to rust when reacted with oxygen

ex)Fe+O—FeO(rust)

A

corrosion

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20
Q

published the first chemistry textbook, in which he listed a series of substances that could not be broken down

A

antoine lavoisier

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21
Q

a concise explanation of widely observed phenomena that has been extensively tested

A

scientific theory

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22
Q

an approach to acquiring knowledge based on the observation of phenomena, the development of a testable hypothesis, and additional experiments that test the validity of the hypothesis

A

scientific method

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23
Q

the principle that compounds always contain the same proportions of their component elements

A

law of definite proportions

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24
Q

the principle that all samples of a particular compound have the same elemental composition

A

law of constant composition

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25
Q

a transformation of a sample of matter that does not alter the chemical identity of any substance in the sample

A

physical process

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26
Q

a tentative and testable explanation for an observation or a series of observations

A

hypothesis

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27
Q

when it is possible to have two different masses of one element react with a given mass of another element, the two masses of the first element must be a small, two whole-numbers ratio

A

law of multiple proportions

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28
Q

the conversion of one or more substances into one or more different substances

A

chemical reaction

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29
Q

a collection of atoms chemically bonded together

A

molecule

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30
Q

an atom or molecule that has a net positive or negative charge

A

ion

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31
Q

another name for a homogeneous mixture

often liquids but may also be gasses or solids

A

solution

32
Q

combinations of liquids that do not mix with or dissolve in each other

A

immiscible liquids

33
Q

a process using evaporation and condensation to separate a mixture of substances with different volatilities

A

distilation

34
Q

a measure of how readily a substance vaporizes

A

volatility

35
Q

a process for separating solid particles from a liquid or gaseous sample by passing it through a porous material that retains the solid particles

A

filtration

36
Q

a process involving a stationary and a mobile phase for separating a mixture of substances based on their different affinities for the two phases

A

chromatography

37
Q

transformation of solid directly to a gas

heat is absorbed

A

sublimation

38
Q

transformation of a gas directly into a solid

heat released

A

deposition

39
Q

transformation of a solid into a liquid

heat absorbed

A

melting

40
Q

transformation of a liquid into a solid

heat released

A

freezing

41
Q

transformation of gas to liquid

heat released

A

condensation

42
Q

transformation of liquid to gas

heat absorbed

A

vaporization

43
Q

the capacity to do work(w)

A

energy

44
Q

the exertion of a force(F) through a distance(d)

A

work(w)

45
Q

w = F x d

A

work = force x distance

46
Q

the energy stored in an object because of it position or composition

A

potential energy (PE)

47
Q

the energy of an object in motion due to its mass(m) and its speed(u)

A

kinetic energy(KE)

48
Q

the transfer of energy from one object or place to another due to the differences in temperature of the objects or places

A

heat

49
Q

the principle that energy cannot be created or destroyed but can be changed from one form to another

A

law of conservation of energy

50
Q

a chemical formula that shows how many atoms of each element are in one molecule of a pure substance

A

molecular formula

51
Q

a representation of a molecule that uses short lines between the symbols of elements to show chemical bonds between atoms

A

structural formula

52
Q

contain ions held together by attraction of opposite charges

ex) NaCl

A

ionic compounds

53
Q

a chemical formula in which the subscripts represent the simplest whole number ratio of the atoms or ions in a compound

A

empirical formula

54
Q

the standard unit of length

A

meter(m)

55
Q

the SI unit of energy

A

joule(J)

56
Q

chemical formula in which atoms appear in a pattern

ex) −CH3

A

condensed structural formulas

57
Q

chemical formula that shows the three-dimensional representations of molecules

shows bond angles

A

ball and stick models

58
Q

chemical formula that is a more accurate representation of the molecule in three dimensions

A

space filling models

59
Q

zero point on Kelvin scale

theoretically the lowest temperature possible

A

absolute zero (O K)

60
Q

the reproducibility of a measurement or the agreement between values

A

percision

61
Q

temperature scale based upon the freezing point and boiling point of water at sea level

A

celsius

62
Q

temperature scale based upon the notion that there is a lower limit to temperature, absolute zero, rather than physical properties of substances

A

kelvin scale

63
Q

how close a measured value is to the true value

A

accuracy

64
Q

all the certain digits in a measured value plus one estimated digit

tells the reader what degree of uncertainty there is in a measured value or a calculation based upon measured values

A

significant numbers

65
Q

the rule that the result of a calculation is known only as well as the least well known value used in the calculation

A

weak-link rule

66
Q

fraction in which the numerator is equivalent to the denominator but is expressed in different units making the fraction equivalent to 1

A

conversion factor

67
Q

the answer of a addition/subtraction operation of significant figures

A

can have no more decimal places that the number with the fewest decimal places used in the calculation

68
Q

the answer of a multiplication/division operation of significant figures

A

can have no more significant figures than the number used in the calculation with the fewest numbers of significant figures

69
Q

system of numbers which uses prefixes to identify different factors of 10

ex) deca=10

A

the metric system

70
Q

are assumed to have infinite significant figures

ex) 1 mi=5280 ft

A

conversion factors

71
Q

Tc

A

Tc=(Tf-32)(5/9)

72
Q

Tf

A

Tf=9/5(Tc)+32

73
Q

water boils @ 212

water freezes @ 32

A

Farenheit temperature scale

74
Q

water boils @ 100

water freezes @ 0

A

celsius (centigrade) temperature scale

75
Q

Tk

A

Tk=Tc+273

Chem 101 (2 decks)

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