Name ____________________________________ Date_____________ Period_______
Study Guide for Matter and Change
Describe what makes up matter and explain how matter can be
identified and categorized by its properties and changes.
a. Name and describe 2 requirements for matter.
(1)
Matter must have mass. (Mass is the amount of matter present)
(2)
Matter must have volume (Volume is how much space the matter
takes up
b. Compare and contrast atom, element, and compound. Give 1 example of
each.
An atom is the smallest unit of matter. An example of one atom of
carbon could be written as “C”, the symbol for carbon.
An element is composed of atoms of only one type. Any substance on
the period table is an example of an element (Sulfur, Oxygen, Carbon,
Fluroine, Plutonium, Gold)
A compound is composed of two or more different elements chemically
combined. H2O, CH4, NaCl, CO2 are all examples of compounds.
c. What is a property and how is it used?
A property is a characteristic or description, which is used to describe
matter.
d. Explain the difference between extensive and intensive properties. Give 2
examples of each.
Extensive properties are properties that depend on the amount of matter
present. Examples are mass, volume, length, and energy.
Intensive properties are properties that do NOT depend on the amount of
matter present. Examples are color, odor, density, conductivity,
malleability, ductility.
e. Compare and contrast physical and chemical properties. Give 1 example
of each.
Physical properties are properties which can be observed without altering
the chemical composition or identity of the substance. Examples are
color, shape, texture, odor, density, magnetism.
Chemical properties are properties that describe a substance’s ability to
undergo a chemical change which alters its composition or identity.
Examples are flammability, reactivity, oxidation state, toxicity, chemical
stability, solubility.
f. Describe chemical and physical changes. Give 1 example of each.
A physical change is a change that does not involve a change in the
identity of a substance. State changes are always physical changes.
Examples are ice melting, water freezing, grinding spices, cutting paper,
salt or sugar dissolving in water, shaping iron in a forge.
A chemical change results in the change of the identity or composition of
a substance due to undergoing a chemical reaction. Examples are
brownies baking, silver tarnishing, metal rusting, baking soda and vinegar
combining (bubbles released), wood burning. The indicators of a
chemical change are a change in color, taste, or odor, a change in heat or
light, the release of a gas(bubbles), or the formation of a precipitate
(solid) from two or more liquids.
g. What is a change of state?
h. Name the process of transfer between each of the following states of
matter.
(1) solid liquid
melting
i.
(2) liquid  gas
evaporation
(3) gas  liquid
condensation
(4) liquid  solid
freezing
Define reactant and product. Which side of the arrow does each go on?
A reactant is the substance(s) that react in a chemical reaction. They are
placed on the left of the arrow.
A product is the substance(s) that is formed in a chemical reaction. They
are placed on the right of the arrow.
In an equation where we made brownies from flour, cocoa, eggs, water,
etc., the ingredients are the reactants and would go on the left. The
brownies are the product and would go on the right of the arrow.
___________________________________________________
j. What are the two types of pure substances?
Elements and compounds. They are considered pure substances because
all their particles are identical
k. What is the difference between an element and a compound?
An element is composed of only one type of atom. Compounds are
composed of two or more different elements chemically bonded
together.
l.
What is the difference between a molecule and a compound?
A molecule is any two atoms bonded together. They can be the same
type of element or different, so long as there are at least two atoms
chemically bonded together.
A compound is two or more different elements chemically bonded
together. The key for it to be a compound is that there must be at least
two atoms of DIFFERENT elements bonded together. Therefore, all
compounds are composed of molecules.
m. What are the two types of mixtures? Give an example of each type.
A homogeneous mixture is a mixture in which the particles look uniform
throughout. You can’t see the particles and tell them apart by looking at
them. Examples of homogeneous mixtures are air, grape juice, salt water,
sugar water, koolaid, windex, etc. They are also called “solutions”.
Heterogeneous mixtures are mixtures in which the particles are different
in composition. You can see the differences in the particles. Examples
are dirt, granite countertops, orange juice, skittles and starburst in a
bowl, blood, milk.
n.
What do subscripts tell us in a chemical formula?
Subscripts tell us how many atoms of an element are present. Example:
the compound H2O contains 2 atoms of hydrogen and 1 atom of oxygen.
The compound CH4 contains one atom of carbon and 4 atoms of
hydrogen.
o.
Define independent and dependent variable. Which axis is each graphed
on?
An independent variable is the variable that is not dependent on another
variable in an experiment. The independent variable can be manipulated
or varied by the scientist in order to test how the dependent variable
changes based on the independent variable’s value. When time is listed
as a variable, it is USUALLY the independent variable. The independent
variable is graphed on the X (horizontal) axis.
A dependent variable changes in response to the independent variable.
We say its value is DEPENDENT on the value of the independent variable
It is graphed on the Y (vertical) axis.
p.
Can mixtures be separated by physical means? What about elements?
Compounds?
Mixtures can be separated by physical means (magnetism, evaporating,
picking out particles, centrifuging, or being filtered. Elements and
compounds cannot.
q.
Can compounds be separated using chemical means? What about
elements?
Compounds can be separated by chemical means. Elements cannot.
r.
Describe the kinetic energy levels, and the shape and volume
characteristics of solids, liquids, gases, and plasma.
Solids have very low kinetic energy. They have a fixed volume and fixed
shape, and are not compressible.
Liquids have a low kinetic energy. They have a fixed volume, but no fixed
shape. They will take the shape of whatever container they are in. They
are not compressible.
Gases have a high kinetic energy. They have no fixed volume and no
fixed shape. They will expand to fill the volume and shape of their
container. They are compressible.
Plasma has a very high kinetic energy, so much that the particles are
tearing themselves apart. They have no fixed volume and no fixed shape.
Stars are made of plasma.
s. Explain the difference between monatomic and diatomic elements. Draw
an example of each.
Monatomic elements are elements that prefer to exist in a single,
unbonded state. Examples of monatomic elements are carbon, sulfur,
iron, and lead. A drawn example would look like this:
Diatomic elements are elements that prefer to exist in a paired state, in
which they are bonded to another atom of the same element. Examples
of diatomic elements are oxygen, nitrogen, fluorine, and hydrogen. They
are usually written with subscripts such as: O2, N2, F2, H2. A drawn
example would look like this:
t.
Ex.
Be able to classify substances into solids, liquids, and gases based on
given properties.
Formaldehyde
Density = 0.8153 g/cm3
Particles can slip past one another.
Not compressible.
liquid
Boron
Density = 2.46 g/cm3
Particles arranged in tight, orderly structure
Not compressible.
solid
Hydrogen Sulfide
Density = 0.00136 g/cm3
Compressible.
Particles can move about freely within their container.
gas
Word problems as demonstrated on Tuesday (10/9) and
Wednesday (10/10) Powerpoint. See website for the
powerpoint and view the examples given.
Identify mixtures/ compounds/elements from given diagrams of particles
(see website: colored bead activity 2 on 9/28 and 10/1, and examples
given on Tuesday (10/9) and Wednesday (10/10) handout (on front of
flow chart).
Be able to graph data like on your matter, classification, and properties
homework, and your Activity 3 noodle mini-lab (on 9/28 and 10/1).