By LeeAnn Kruis
Chemistry
 Chemistry is stuff such as water(H20), clothes, air, and
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so on, that has states of matter.
The three states of matter is Solid, Liquid, and Gas.
Solid has fixed volume and shape that results from the
way their particles are arranged.
Liquids have fixed volumes but not a fixed shape,
because the particles are lose enough to slip past each
other.
Gas has neither a fixed volume and a fixed shape, the
particles are very spaced apart and the particles have
weak attractions and hardly touch each other.
Physical and Chemical Changes
 Physical Changes
 Physical changes are changes in which the identity of a
substance does not change.
 But the arrangement, location, and speed of the
particle may change.
 Such as in sweet ice tea; dissolving sugar in tea is a
physical change.
Chemical Change
 A chemical change is where the substances change and
new substances form.
 Such as Mercury(II) Oxide, when exposed to heat, the
mercury becomes and liquid, and the oxide becomes
oxygen gas.
Matter
 Matter is anything that has mass and volume, such as a
balloon, when blowing up the balloon the mass and
volume changes due to adding carbon dioxide, or
helium.
Mass
 Mass of an object is the quantity of matter contained
in that object.
 Such as a marble verses a ping-pong ball.
 The marble has more volume then the ping-pong ball
due the marble not having a cavity, such as the pingpong ball.
Volume
 Volume is the space the object occupies.
 An example of space is a text book, the book takes up
space due to the volume of it.
 The volume of the book can be found for multiplying
the book’s length times the width, times the height.
Measuring Mass and Volume
 How you measure mass is with the objects
gravitational pull; you usually weigh it in grams.
 How you measure volume is using liters; you usually
fill any beaker to a certain point with water, record the
height, and then add the object and record the new
height of water; and then you take the difference and
find out how much volume the object has.
Density/Weight
 The weight is defined as the force produced by gravity
acting on mass.
 An example is sand compared to dirt. The dirt will
weigh more then the sand because the dirt has a lot
more gravitational pull then the sand.
Calculating Density
 You find the mass and the volume.
 After you find those you divide them together to get
the density.
SI Units; fundamental and derived
units; metric prefixes.
 SI Units are Length(meter), Mass(kilogram),
Time(second), Thermodynamic temperature(kelvin),
Amount of substance(mole), Electric current(ampere),
and Luminous intensity(candela).
 The last two in the SI Units have very little to do with
chemistry, but the first five are very important in the
foundation of all chemical measurements.
Converting between units
 Let’s say you want to convert 0.851 liters into milliliters.
 How you would do that is you need to find how many
milliliters are in liters.(1000 ml/1L)
 You then calculate and cancel out the liters to get
0.851L*1000Ml/1L=851Ml.
Chemical and physical properties
of matter
 The physical properties of matter is how a substance
looks, and can always be determined without changing
the nature of the substance.
 You can use sucrose(sugar) as an example; Sucrose is
solid and white at room temperature, so color and
state are physical properties.
Chemical Properties
 Chemical properties can be identified y trying to
cause a chemical change, such as a rusty nail; the
reason the rusty nail is rusty is because it’s been
exposed for a long period of time to oxygen and a
chemical reaction occurs.
Atoms
 Atoms are in everything around you, air, plants, water,
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and people.
All mater is composed of 110 different kinds of atoms.
Atoms can be pure substances, copper, bromine,
carbon dioxide, each of these pure substances are
elements.
Elements can only contain one kind of atom, unless it
is a molecule.
A molecule is two atoms combined in a definite ratio.
Compounds , and Mixtures
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Compounds are pure substances that are not elements.
An example of a compound is mercury(II)oxide.
Mixtures are two or more pure substances.
Most foods we eat are mixtures.
There are two kinds of mixtures, Homogeneous and
Heterogeneous.
 Homogeneous is a mixture that has two or more pure
substances in it, but we can’t see them.
 Heterogeneous is a mixture that you are able to see the
different substances.
Measurements and Calculations in
Chemistry
 Accuracy is how close you estimated the true value to
be. Accuracy is important in chemistry because in
labs you need to be the closest possible unit to the
actual value.
Presision
 Precision is how closely several measurements that are
of the same quantity and that are made in the same
way agree with one another.
Rules for Determining
 Gather the information
 Plan your work
 Calculate
 Verify your results
Significant figures
 Significant figures are the figures used to measure or
calculate an object with certainty.
Converting
 You sometimes need to convert in chemistry, so you
need to know how to convert.
 Let’s say you want to convert 0.851 liters into milliliters.
 How you would do that is you need to find how many
milliliters are in liters.(1000 ml/1L)
 You then calculate and cancel out the liters to get
0.851L*1000Ml/1L=851Ml.(taking from slide 10)
Scientific Notation
 In scientific notation, exponents are count values; in
chemistry you use scientific notation with extremely
large numbers and extremely small numbers.
 Scientific notation has two parts; the first part is with a
number, any number, from one to ten, this may be in a
decimal form.
 The second part is to the power of ten.
 An example is 0.0910^6