Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

AP Chem > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

What are two-atom molecules called?

A

Diatomic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Matter consists of __ __. The world we know is called the __ world. World of atoms and molecules is called the __ world. Substances result from about __ different atoms

A

Individual atomsMacroscopicMicroscopic100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Steps in the scientific method (3)

A

1) making observations (qualitative: no numbers, quantitative: number & a unit)2) formulating hypotheses (possible explanation for an observation)3) performing experiments (carried out to test whether a hypothesis is valid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the 2 fundamental concepts in chemistry?

A

1) matter is composed of various types of atoms2) one substance changes to another by reorganizing the way the atoms are attached to each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define theory

A

A set of assumptions put forth to explain the observed behavior of matter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define model

A

Usually involve assumptions about the behavior of individual atoms or molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Theories are a set of __ __ that help focus our questions

A

Tested hypotheses

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

An __ is something that is witnessed and can be recorded; a __ is an interpretation, a possible explanation of why nature behaves in a particular way

A

ObservationTheory

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define natural law

A

Statement that expresses generally observed behavior

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Define law of conservation of mass

A

Mass is neither created nor destroyed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

A __ summarizes what happens, a __ (__) is an attempt to explain why it happens

A

LawTheory (model)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

__ stated an __ is anything that cannot be broken down into simpler substances

A

BoyleElement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Who’s the father of modern chemistry?

A

Lavoisier

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

A measurement (__ observation) always consists of two parts: a __ & a __

A

QuantitativeNumberUnit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Physical quantity: massName of unit:Abbreviation:

A

Name of unit: kilogramAbbreviation: kg

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Physical quantity: lengthName of unit:Abbreviation:

A

Name of unit: meterAbbreviation: m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Physical quantity: time Name of unit:Abbreviation:

A

Name of unit: secondAbbreviation: s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Physical quantity: temperature Name of unit:Abbreviation:

A

Name of unit: kelvinAbbreviation: K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Physical quantity: electric currentName of unit:Abbreviation:

A

Name of unit: ampere Abbreviation: A

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Physical quantity: amount of substanceName of unit:Abbreviation:

A

Name of unit: moleAbbreviation: mol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Physical quantity: luminous intensity Name of unit:Abbreviation:

A

Name of unit: candelaAbbreviation: cd

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

1 liter = (1 __)^3 = (10 __)^3 = 1000 __^3 = 1000 __

A

dmcmcmmL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

1 cm^3 = 1 __1 m^3 = 1000 __

A

mLL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Common types of lab equipment used to measure liquid volume (4)

A

Graduated cylinder, pipet, buret, volumetric flask

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Volume measurements are read at the bottom of the liquid curve called the __. __ & __ are not the same
MeniscusMass Weight
26
Define mass
A measure of the resistance of an object to a change in its state of motion (the quantity of matter in an object)
27
Define weight. Weight varies with the strength of the __ __
The force exerted on an object by gravity. Gravitational field
28
Prefix: megaSymbol:Meaning:
Symbol: MMeaning: 10^6
29
Prefix: kiloSymbol:Meaning:
Symbol: kMeaning: 10^3
30
Prefix: hectoSymbol:Meaning:
Symbol: hMeaning: 10^2
31
Prefix: deka Symbol:Meaning:
Symbol: daMeaning: 10^1
32
Prefix: deciSymbol:Meaning:
Symbol: dMeaning: 10^-1
33
Prefix: centiSymbol:Meaning:
Symbol: cMeaning: 10^-2
34
Prefix: milliSymbol:Meaning:
Symbol: mMeaning: 10^-3
35
Prefix: microSymbol:Meaning:
Symbol: uMeaning: 10^-6
36
Prefix: nanoSymbol:Meaning:
Symbol: nMeaning: 10^-9
37
Define certain digits. Define uncertain digit
Remain the same no matter who's measuring.Estimated #.
38
Report measurements by recording all the __ digits plus the first __ digit
CertainUncertain
39
A measurement always has some degree of __ which depends on the __ device
Uncertainty Measuring
40
Define uncertainty
Characteristic that any measurement involves estimates and cannot be exactly reproduced (uncertainty in the last number is assumed to be +/- 1 unless otherwise indicated)
41
Define significant figures
The certain digits and the first uncertain digit of a measurement
42
Two terms often used to describe the reliability of measurements are __ and __
PrecisionAccuracy
43
Define accuracy
The agreement of a particular value with the true value
44
Define precision
The degree of agreement among several measurements of the same quantity; the reproducibility of a measurement
45
Define random error (intermediate error)
An error that has an equal probability of being high or low (occurs in estimating the value of the last digit in a measurement)
46
Define systematic error (determinate error)
An error that always occurs in the same direction
47
In quantitative work, __ is often used as an indication of accuracy (assume the __ of precise measurements is accurate; only valid when there are no __ __)
PrecisionAverageSystematic errors
48
Rules for counting significant figures (5)
1) nonzero integers are always significant 2) zeros preceding all nonzero digits are not significant3) zeros between nonzero digits are always significant 4) all zeros after nonzero digits are significant only when there's a decimal point5) exact numbers have an infinite # of sig figs and do not limit the # of sig figs in a calculation
49
Define exponential notation
Expresses a # as N • 10^M, a convenient method for representing a very large or very small number and for easily indicating the number of significant figures
50
For multiplication/division, the # of sig figs in the result is the same as the # in the __ __ measurement used in the calculation
Least precise
51
For addition or subtraction, the result has the same number of __ __ as the __ __ measurement used in the calculation
Decimal placesLeast precise
52
Rules for rounding (2)
1) in a series of calculations, carry the extra digits through to the final result, then round2) if the digit to be removed: a) is less than 5, the preceding digit remains the same, b) is equal to or greater than 5, the preceding digit is increased by 1
53
When rounding, use only the first number to the __ of the last sig fig
Right
54
Define the unit factor method (dimensional analysis)
An equivalence statement between units used for converting from one unit to another
55
Define unit factor
Converting an equivalence statement into a fraction
56
Converting from one unit to another (3)
1) use the equivalence statement that relates the two units 2) derive the appropriate unit factor by looking at the direction of the required change to cancel unwanted units3) multiply the quantity to be converted by the unit factor to give the quantity with the desired units
57
Three systems for measuring temperature
Celsius scaleKelvin scaleFahrenheit scale
58
The __ & __ scales both have the same size of the temperature unit (degree)
CelsiusKelvin
59
Temp kelvin = temp celsius _ 273.15Temp celsius = temp kelvin _ 273.15
+-
60
_*F = _*C & _*F = _*C(*F - 32*F) • (5*C/9*F) = __(*C • (9*F/5*C)) + 32*F = __
9*F = 5*C & -40*F = -40*CTemperature celsius Temperature Fahrenheit
61
Define density
Property of matter representing mass of substance per unit volume of the substance Density = mass / volume (g/cm^3)
62
Define matter
Anything occupying space and having mass; the material of the universe
63
Matter exists in what 3 states
Solid LiquidGas
64
Define states
The 3 different forms in which matter can exist (solid, liquid, gas)
65
Define solid
Rigid, has a fixed volume and fixed shape
66
Define liquid
Has a definite volume but no specific shape, it takes the shape of its container
67
Define gas
No fixed volume and no fixed shape, takes on the shape and volume of its container
68
Solids & liquids: __ compressibleGases: __ compressible, easy to decrease __
SlightlyHighly Volume
69
Define mixture
Has variable composition of pure substances, is homogeneous or heterogeneous
70
Define heterogenous
Having visibly distinguishable parts, can usually be separated into 2 or more homogeneous mixtures or pure substances
71
Define homogeneous
Having visibly indistinguishable parts
72
Define solution
A homogeneous mixture
73
Define pure substance
Substance with constant composition
74
Define physical change
Change in the form of a substance, not in its chemical composition; chemical bonds are not broken in a physical change (can separate mixtures into pure compounds)
75
__ can be separated by methods involving only physical changes
Mixtures
76
Define distillation
A method for separating the components of a liquid mixture that depends on differences in the ease of vaporization of the components
77
Define volatility
How readily substances become gases; the ease with which a substance can be changed to its vapor
78
Define simple distillation
Mixture is heated, most volatile component vaporizes at the lowest temperature, and the vapor passes through a cooled tube (condenser) where it condenses back into its liquid state
79
When a mixture contains several volatile components, one-step distillation doesn't give a __ __ in the receiving flask
Pure substance
80
Define filtration
A method for separating the components of a mixture containing a solid & a liquid (mixture poured onto mesh filter paper which passes the liquid and leaves the solid behind
81
Define chromatography
The general name for a series of methods for separating mixtures by employing a system with two phases (states) of matter: a mobile phase & stationary phase
82
Stationary phase: __Mobile phase: either __ or __
SolidLiquid or gas
83
Component with a high affinity: mobile phase- __ __, stationary phase- __ __
Moves quicklyMoves slowly
84
Define paper chromatography
Uses a strip of porous paper for the stationary phase, drop of mixture to be separated is placed on the paper, paper dipped into a liquid (mobile phase) that travels up the paper; often used by biochemists
85
Pure substances contain __ (combinations of __) or __ __
CompoundsElementsFree elements
86
Define compound
A substance with constant composition that can be broken down into elements by chemical processes
87
Define chemical change
The change of substance into other substances with different properties and different composition through a reorganization of the atoms; a chemical reaction
88
Define element
Substance that cannot be decomposed into simpler substances by chemical or physical means

AP Chem (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions