AP Chemistry Chapter 1: Matter & Measurement
Chemistry –
Matter –
A property is a characteristic that distinguishes one type of matter from another.
All matter is made up of about _________ elements
Elements come in pieces called ______________
Atoms can combine to form __________________
States of Matter
Solid
- Fixed shape and volume
- particles close together - rigid structure
- particles vibrate only – no movement
Liquid
- fixed volume - takes shape of container
- particles farther apart than solid
- little order - particles can move around
Gas
- takes volume and shape of container
- particles are far apart
- random motion of particles
Classification of Matter
Law of Constant Composition / Law of Definite Proportions
A compound is always__________________________________________________
Water is always H2O and is always 11% hydrogen and 89% oxygen by mass. There are
other compounds containing hydrogen and oxygen (hydrogen peroxide - H2O2), but if
they don’t have these properties then they aren’t water!
Properties:
• Physical Properties: Measured without changing the identity and composition of
the substance.
– Examples: Color, Odor, Hardness, Melting/Boiling Points, Density
• Chemical Properties: Measured by reacting (changing) the substance to form a
new substance
– Examples: Flammability, Reaction to water or another substance
Extensive – ______________________________________________________
Examples: mass and volume
Intensive – ________________________________________________________
Examples: temperature, density, boiling point
Changes/Reactions:
Physical changes – The physical appearance may change but
___________________________________________ (it has to stay the same stuff)
- ______________________ (solid  liquid  gas) __________________
Chemical changes/reactions – One substance _________________________
Nuclear Changes – A new substance is formed by changes in the atoms themselves – not
just by rearranging the atoms like in chemical changes.
Endothermic - ____________________________________
Example: Boiling water
Exothermic - _____________________________________
Example: Burning a candle
Scientific Method:
1.)
2.) Hypothesis – a preliminary (before any testing) __________________________
based on observation.
The hypothesis is then tested by experimentation and 1 of 3 things happens:
1)
Hypothesis is totally wrong - hypothesis is thrown out
2)
Hypothesis is partially correct - modify hypothesis and retest
3)
Hypothesis passes repeated experiments
3.) The hypothesis leads to a ________________ after it passes many repeated
experiments
Theory - ____________________________________________ _________
(supported by experimental evidence)
Law - generalization _________________________________________________
______________
• A LAW tells you what happens; a THEORY tells you why it happens.
Measurement
FUNDAMENTAL QUANTITY
SI SYSTEM
• Mass
kilogram (kg)
• Distance
meter (m)
• Temperature
Kelvin (K)
• Time
second (s or sec)
• Amount
mole (mol)
ENGLISH SYSTEM
oz, lb, ton
in, ft, yd, mi
°F
sec, min, hr, day
DERIVED QUANTITY (derived from the fundamental quantities above)
• Area (distance)2
m2
in2, ft2
• Volume (distance)3
m3, L
in3, yd3
• Velocity (distance/time) m/s
mi/hr
• Density (mass/volume) g/L
lb/in3
*See table 1.5 for metric prefixes (know pico through mega!)
Temperature Scales:
There are 3 commonly used temperature scales in science. They are the Fahrenheit scale,
the Celsius or centigrade scale and the Kelvin or absolute scale.
Conversions between Temperature Scales
• Celsius to Kelvin conversion:
• Kelvin to Celsius conversion:
• Fahrenheit to Celsius conversion:
• Celsius to Fahrenheit conversion:
Uncertainty:
Accuracy Precision –
Percentage Error:
Significant Digits:
- All scientific measurements contain one digit which is an estimate.
- Any digit in a measurement which is the result of measurement is called a significant
digit.
The following rules apply to determining the number of significant digits in a measured
quantity:
All nonzero digits are significant
Zeros between nonzero digits are significant
Zeros to the left of the first nonzero digit in a measurement less than 1 are
not significant
Zeros on the end of a measurement to the right of a decimal point are
significant
Zeros at the end of a measurement left of the decimal point are not
significant unless a line is present above the zero or there is a decimal
point after the number.
Rounding
Rules for rounding off numbers:
• If the digit to be dropped is less than 5, it and all following digits are dropped.
• If the digit to be dropped is greater than or equal to 5, it and all following digits
are dropped and the preceding digit is increased by 1
Adding & Subtracting
The resulting answer can be no more precise than the least precise measurement added or
subtracted. (PLACE VALUE RULE)
5.42 cm
0.012 cm
85063 mL
 6450 mL
 4.6 cm
Multiplication & Division
The resulting answer should have the same number of significant digits as are in the
measurement which has the smallest number of significant digits in it. (COUNTING
RULE)
5.26400m x 0.00012m 
4500.2m

2.125 sec
Dimensional Analysis (Factor Label)
A problem solving method using a series of multiplications and divisions
Multiply by fractions called “conversion factors”
ALL conversion factors are equal to 1
Conversion factors can be made from:
English - English relationships (1 foot = 12 inches)
Metric – Metric relationships (1 km = 1 x 103 m)
English – Metric relationships (1.00 in = 2.54 cm)
Steps of Dimensional Analysis
1) Put the given AND the given unit on the left
2) Arrange conversion factors (fractions) to cancel ALL units EXCEPT the required
unit
For fractional units (m/sec)– work one unit at a time
For units to powers (m3) – take the ENTIRE conversion factor to that power