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CHEM 139 > Chapter 1: Matter, Measurement, and Problem Solving > Flashcards

Chapter 1: Matter, Measurement, and Problem Solving Flashcards

1
Q

atoms

A

the submicroscopic particles that constitute the fundamental building blocks of ordinary matter

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2
Q

molecules

A

atoms that bind together in specific geometrical arrangments

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3
Q

chemistry

A

the science that seeks to understand the behavior of matter by studying the behavior of atoms and molecules

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4
Q

atom

A

carbon (C) is a(n) __________

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5
Q

molecule

A

water (H2O) is a(n) ___________

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6
Q

4

A

hydrogen peroxide (H2O2) is a molecule that contains ___ atoms

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7
Q

false

A

true or false - carbon monoxide (CO) and carbon dioxide (CO2) molecules are both composed of carbon and oxygen atoms and therefore must have similar properties

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8
Q

matter

A

anything that occupies space and has mass
- can be classified as solid, liquid, or gas based on what properties it exhibits

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9
Q

state

A

the physical form of matter

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10
Q

composition

A

the basic components that make up matter

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11
Q

solid matter

A
  • atoms in fixed locations (fixed shape)
  • atoms can vibrate
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12
Q

liquid matter

A
  • atoms are closely packed, but can move past one another
  • fixed volume, but not shape
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13
Q

gaseous matter

A
  • lots of space between atoms
  • no fixed volume so they are compressible
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14
Q

solid

A

in which state of matter will the molecules that compose a given substance pack the closest?

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15
Q

gas

A

in which state of matter are the molecules that compose a substance be able to be compressed because they are spaced so far apart from one another?

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16
Q

solid

A

what state of matter will not conform to the shape of the container you put it in?

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17
Q

pure substance

A

made up of only one component and its composition is invariant (no variation)

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18
Q

mixture

A

a substance composed of two or more components in proportions that can vary from one sample to another

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19
Q

element

A

a substance that cannot be chemically broken down into simpler substances
- composed of one type of atom

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20
Q

compound

A

a substance composed of two or more elements in fixed definite proportions
- ex: H2O

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21
Q

heterogeneous mixture

A

composition varies from one region of the mixture as compared to another
- ex: oil and water

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22
Q

homogeneous mixture

A
  • multiple substances are present, but are evenly distributed
  • therefore, the composition does not vary from one region of the mixture as compared to another
  • ex: tea with sugar
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23
Q

decanting

A

carefully pouring off the water into another container
- a mixture of sand and water can be separated with this method

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24
Q

distillation

A
  • a process in which a mixture is heated to boil off the more volatile liquid
  • the volatile liquid is then re-condensed in a condenser and collected in a separate flask
  • a homogeneous mixture of liquids can usually be separated by this method
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25
volatile
easily vaporizable
26
filtration
- process in which the mixture is poured through filter paper in a funnel - a mixture of an insoluble solid and a liquid can be separated by this method
27
physical changes
changes that alter only the state or appearance, but not composition - the atoms or molecules that compose a substance do not change their identity during a physical change
28
chemical changes
changes that alter the composition of matter - atoms rearrange, transforming the original substances into different substances
29
physical property
a property that a substance displays without changing its composition - the smell of gasoline - odor, taste, color, appearance, melting point, boiling point, and density
30
chemical property
a property that a substance displays only by changing its composition via a chemical change (or chemical reaction) - the flammability of gasoline - corrosiveness, acidity, and toxicity
31
energy
the capacity to do work
32
work
the action of a force through a distance
33
kinetic energy
the energy associated with the motion of an object
34
potential energy
the energy associated with the position or composition of an object
35
thermal energy
the energy associated with the temperature of an object
36
total energy
= kinetic energy + potential energy
37
law of conservation of energy
energy is always conserved in a physical or chemical change; it is neither created nor destroyed
38
unstable
systems with high potential energy are ______ and tend to change in a direction that lowers their potential energy, releasing energy into the surroundings
39
units
standard quantities used to specify measurements
40
metric system, english system
two most common unit systems
41
meter (m)
SI unit of length - slightly longer than a yard
42
mass
the quantity of matter within it
43
kilogram (kg)
SI unit of mass - = 2lb 3oz
44
weight
a measure of the gravitational pull on its matter
45
time
the measure of the duration of an event
46
second (s)
SI unit of time - defined as the period of time it takes for a specific number of radiation events of a specific transition from cesium-133
47
temperature
a measure of the average amount of kinetic energy of the atoms or molecules that compose the matter - also determines the direction of thermal energy transfer, or what we commonly call heat
48
Kelvin (K)
SI unit of temperature
49
Kelvin scale (absolute scale)
assigns 0 K (absolute zero) to the coldest temperature possible
50
absolute zero
the temperature at which molecular motion virtually stops; lower temperatures do not exist - -273°C or - 459°F
51
water boils
- 212°F - 100°C - 373 K
52
water freezes
- 32°F - 0.00°C - 273 K
53
Fahrenheit degree
5/9 the size of a Celsius degree
54
same size
the Celsius degree and the Kelvin degree are the ____ ____
55
°C = (°F-32)/1.8
Fahrenheit to Celsius
56
K = °C+273.15
Celsius to Kelvin
57
prefix multipliers
change the value of the unit by the powers of 10
58
mega (M)
multiplier: 1,000,000 (10^6)
59
kilo (k)
multiplier: 1000 (10^3)
60
deci (d)
multiplier: 0.1 (10^-1)
61
centi (c)
multiplier: 0.01 (10^-2)
62
milli (m)
multiplier: 0.001 (10^-3)
63
micro (u)
multiplier: 0.000001 (10^-6)
64
nano (n)
multiplier: 0.000000001 (10^-9)
65
giga (g)
multiplier: 1,000,000,000 (10^9)
66
derived unit
a combination of other units
67
speed
m/s - distance per unit time
68
volume
m^3 or Liter (L) - measure of space
69
density
g/cm^3 or g/mL - ratio of mass to volume
70
significant
all nonzero digits
71
significant
interior zeros (zeroes between two nonzero digits)
72
not significant
leading zeroes (zeroes to the left of the first nonzero digit)
73
significant
trailing zeroes after a decimal point
74
significant
trailing zeroes before a decimal point (and after a nonzero number)
75
ambiguous
trailing zeroes before an implied decimal point
76
significant
decimal points are placed after one or more trailing zeroes if the zeroes are to be _________
77
unlimited
exact number have an _________ number of significant figures
78
fewest significant figures
in multiplication or division, the result carries the same number of significant figures as the factor with the ________ __________ ________
79
fewest decimal places
in addition or subtraction, the result carries the same number of decimal places as the quantity with the ______ _______ ______
80
accuracy
how close the measured value is to the actual value
81
precision
how close a series of measurements are to one another or how reproducible they are
82
dimensional analysis
using units as a guide to solving problems
83
conversion factor
a fractional quantity of a unit equation with the units we are converting from on the bottom and the units we are converting to on the top
84
unit equation
a statement of two equivalent quantities, such as 1.094 yd = 1 m.

CHEM 139 (3 decks)

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