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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
a transformation of a sample of matter that does not alter the chemical identity of any substance in the sample
physical process
26
a tentative and testable explanation for an observation or a series of observations
hypothesis
27
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
law of multiple proportions
28
the conversion of one or more substances into one or more different substances
chemical reaction
29
a collection of atoms chemically bonded together
molecule
30
an atom or molecule that has a net positive or negative charge
ion
31
another name for a homogeneous mixture often liquids but may also be gasses or solids
solution
32
combinations of liquids that do not mix with or dissolve in each other
immiscible liquids
33
a process using evaporation and condensation to separate a mixture of substances with different volatilities
distilation
34
a measure of how readily a substance vaporizes
volatility
35
a process for separating solid particles from a liquid or gaseous sample by passing it through a porous material that retains the solid particles
filtration
36
a process involving a stationary and a mobile phase for separating a mixture of substances based on their different affinities for the two phases
chromatography
37
transformation of solid directly to a gas heat is absorbed
sublimation
38
transformation of a gas directly into a solid heat released
deposition
39
transformation of a solid into a liquid heat absorbed
melting
40
transformation of a liquid into a solid heat released
freezing
41
transformation of gas to liquid heat released
condensation
42
transformation of liquid to gas heat absorbed
vaporization
43
the capacity to do work(w)
energy
44
the exertion of a force(F) through a distance(d)
work(w)
45
w = F x d
work = force x distance
46
the energy stored in an object because of it position or composition
potential energy (PE)
47
the energy of an object in motion due to its mass(m) and its speed(u)
kinetic energy(KE)
48
the transfer of energy from one object or place to another due to the differences in temperature of the objects or places
heat
49
the principle that energy cannot be created or destroyed but can be changed from one form to another
law of conservation of energy
50
a chemical formula that shows how many atoms of each element are in one molecule of a pure substance
molecular formula
51
a representation of a molecule that uses short lines between the symbols of elements to show chemical bonds between atoms
structural formula
52
contain ions held together by attraction of opposite charges ex) NaCl
ionic compounds
53
a chemical formula in which the subscripts represent the simplest whole number ratio of the atoms or ions in a compound
empirical formula
54
the standard unit of length
meter(m)
55
the SI unit of energy
joule(J)
56
chemical formula in which atoms appear in a pattern ex) −CH3
condensed structural formulas
57
chemical formula that shows the three-dimensional representations of molecules shows bond angles
ball and stick models
58
chemical formula that is a more accurate representation of the molecule in three dimensions
space filling models
59
zero point on Kelvin scale theoretically the lowest temperature possible
absolute zero (O K)
60
the reproducibility of a measurement or the agreement between values
percision
61
temperature scale based upon the freezing point and boiling point of water at sea level
celsius
62
temperature scale based upon the notion that there is a lower limit to temperature, absolute zero, rather than physical properties of substances
kelvin scale
63
how close a measured value is to the true value
accuracy
64
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
significant numbers
65
the rule that the result of a calculation is known only as well as the least well known value used in the calculation
weak-link rule
66
fraction in which the numerator is equivalent to the denominator but is expressed in different units making the fraction equivalent to 1
conversion factor
67
the answer of a addition/subtraction operation of significant figures
can have no more decimal places that the number with the fewest decimal places used in the calculation
68
the answer of a multiplication/division operation of significant figures
can have no more significant figures than the number used in the calculation with the fewest numbers of significant figures
69
system of numbers which uses prefixes to identify different factors of 10 ex) deca=10
the metric system
70
are assumed to have infinite significant figures ex) 1 mi=5280 ft
conversion factors
71
Tc
Tc=(Tf-32)(5/9)
72
Tf
Tf=9/5(Tc)+32
73
water boils @ 212 water freezes @ 32
Farenheit temperature scale
74
water boils @ 100 water freezes @ 0
celsius (centigrade) temperature scale
75
Tk
Tk=Tc+273

Chem 101 (2 decks)

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