A.P. Chemistry: Notes on Chapter 1
Quantitative data: numerical data
Qualitative data: descriptive information
States of Matter: solid (fixed volume and shape), liquid (fixed volume, takes shape of
container), gas (takes volume and shape of container). State is determined by temperature and
pressure.
Kinetic Molecular Theory of Matter:
1) Solids – particles are packed closely together in a regular array and vibrate in position
2) Liquids – particles are randomly arranged and are fluid (can move past each other)
3) Gas – particles are far apart and move rapidly and randomly
4) The higher the temperature, the faster particles move
Classification of
Matter
Heterogeneous
Matter
Matter
Solution
Homogeneous
Matter
Compound
Pure
Substance
Element
Properties and examples of Mixtures: Homogeneous (Solutions) v. Heterogeneous
(Suspensions and Colloids) mixtures. Mixtures can be separated by physical means (filtration,
evaporation). In heterogeneous mixtures particles can be seen and exhibit the Tyndall effect.
Pure substance: cannot be separated into other substances by physical means
Element: Substance composed of only one type of matter
Atom: smallest part of an element that still retains its properties
Compound: pure substance composed of two or more elements. The properties of elements are
lost when they bond to form a compound (e.g. compare properties of C, H, and O with properties
of C12H22O11). Compounds have a definite percent composition by mass while solutions do not.
Some compounds are composed of ions (charged atoms or groups of atoms) while others are
composed of molecules (discrete units with the chemical characteristics of the compound).
Physical property: properties that can be observed and measured without changing the
composition of the substance. They include:
Color
State
Melting and boiling points
Density (D=M/V)
Conductivity
Magnetic properties
Crystal shape
Malleability (ease with which a solid can be deformed)
Ductility (ease with which a solid can be drawn into a wire)
Viscosity (susceptibility of a liquid to flow)
Heat of vaporization (heat energy required to change a liquid to a vapor)
Heat of fusion (heat energy required to change a solid to a liquid)
Solubility (amount of substance that can dissolve in a given mass of a solute)
Temperature: average kinetic energy of molecular motion of an object
Heat: energy of molecule motion
Heat is spontaneously transferred from hotter to cooler objects
Density is dependent on temperature. Explain why laboratory glassware is calibrated to
measure volume at specified temperatures
Extensive properties (depend on the amount of matter present, e.g. mass and volume) v.
Intensive properties (don’t vary with the amount of matter present, e.g. density and boiling
point)
Physical change (a change in physical properties; the identity of the substance is preserved)
Chemical change (a new arrangement of atoms results in new substances with different
properties; start with reactants and end with products)
Units of Measurement – SI System
Base Units
kg – mass
m – length
s – time
K – temp
mole – amount of substance
ampere – electric current
Prefixes
kilo = 1000
deci = 0.1
centi = 0.01
milli = 0.001
micro = 10-6
nano = 10-9
Derived Units
1L = 1 dm3
1 mL = 1 cm3
Temperature Scales
C scale was developed based on the melting and boiling temperatures of water
F scale was developed so that 0 was the lowest temperature possible at that time (late 1600’s).
This was the freezing point of a solution of water saturated with salt. 100oF was human body
temperature.
K scale – 0 was set as the temperature at which all heat is absent (molecular motion ceases)
T (K) = T (C) + 273.15
Precision (how close measurements of the same quantity are to one another) v. Accuracy (how
close measurements are to the accepted value)
Accuracy is expressed as percent error =
𝑎𝑐𝑐𝑒𝑝𝑡𝑒𝑑−𝑒𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙
𝑎𝑐𝑐𝑒𝑝𝑡𝑒𝑑
𝑥 100%
Precision is expressed as an average or standard deviation
Scientific notation – review, know how to use EE key on calculator –
Do NOT use the x 10^ method on your calculator!!
Significant figures: a calculated result can be no more precise than the least precise
measurement; the final digit of a measurement is uncertain or estimated. Constants should be
rounded to one more significant figure than the values given in the data. When using your
calculator, round only at the end of a series of calculations OR when switching from addition /
subtraction to multiplication / division since the sig fig rules are different. Know the sig fig rules
and how to use them!!
1. Zeros between nonzero digits are significant
2. Zeros to the right on a nonzero number and to the right of a decimal point are significant
3. Zeros that are placeholders (to the right of a nonzero number without a decimal point or
to the left of a number) are NOT significant
When adding or subtracting, the number of decimal places in the answer is the same as the
number of decimal places in the number with the fewest digits after the decimal.
When multiplying or dividing, the answer has the same number of sig figs as the quantity
with the fewest sig figs.
Conversion Factors – review how to use conversion factors in calculations