Characteristics of
Matter
Mrs. Kuhn
Chemistry
Center for Creative Arts
Scientific Method
 State the problem and observe. Observations
may be either qualitative (describing physically
observed phenomena) or quantitative
(involving numerical measurements).
 Propose an explanation (aka hypothesis).
 Perform experiments to test hypothesis.
Results and conclusions may lead to further
experimentation.
States of Matter
 All matter has two distinct characteristics:
mass and volume.
 Solids: definite shape and volume. Particles
are closely packed and only vibrate in fixed
positions.
 Liquids: indefinite shape and definite volume.
Particles in liquid are free to move.
 Gases: No definite shape or volume. Particles
are free to move and expand to fill container.
Properties of Matter
Physical Properties
Hardness
Color and Odor
Density
Boiling/Melting Point
Solubility
Chemical Properties
Flammability
Acidity
Basicity
Reactivity
Vocabulary
 Think/Pair/Share: First individually
and then with one or two tablemates,
differentiate between mixtures,
solutions, pure compounds, and
pure elements.
 Also discuss this: what is the
difference between a physical and a
chemical change?
Physical Changes
 Involve altering shape, size, or state
without changing chemical composition.
 SOLIDLIQUID _______________
 GASLIQUID
_______________
 SOLIDGAS
_______________
 LIQUIDSOLID _______________
 GASSOLID
_______________
 LIQUIDGAS
_______________
Chemical Changes
 In chemical changes or reactions, the
atoms of a substance are rearranged.
The chemical composition of the new
substance differs from the original.
 Examples?
Heat Transfer
 When physical or chemical changes produce or absorb
heat, the amount of heat involved is calculated using
the specific heat capacity of the substance.
∆H = m x c x ∆T
∆H = amount of heat change
m = mass of substance
c = specific heat capacity
∆T = change in temperature in Celsius (determined by
subtracting the final temp from the initial temp)
Common Heat Capacities
Aluminum
Brass
.91 J/gC
.377 J/gC
Copper
.39 J/gC
Iron
Nickel
.46 J/gC
.54 J/gC
Tin
.21 J/gC
Silver
.24 J/gC
Water
4.184 J/gC
Specific Heat Capacity
Sample Problems
1. What quantity of energy is required to
raise the temperature of 10 grams of
water from 15°C to 50°C?
2. A 5.0 gram sample of an iron nail
requires 37.75J of energy to change its
temperature from 25°C to 32.5°C. Is the
nail made of pure iron? Explain.
Density
 Density is another attribute of matter.
Density describes the relationship
between a substance’s mass and its
volume.
 Density = mass/volume
 d = m/v d = g/cm3 d = g/mL
Density practice
 What is the density of an object if its mass is
124 grams and its volume is 130 mLs?
 What is the density of a rectangular object if its
dimensions are 3cm x 4 cm x 2 cm and its
mass is 10.0 g? (Remember:
v= l x w x h)
Common Densities
Water
1.0000 g/cm3
Air
0.00123 g/cm3
Helium
0.000178 g/cm3
Densities of Common Metals

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



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Aluminum 2.71 g/cm3
Brass 8.5 g/cm3
Gold 19.3 g/cm3
Iron 7.85 g/cm3
Lead 11.3 g/cm3
Nickel 8.8 g/cm3
Platinum 21.4 g/cm3
Silver 10.5 g/cm3
Tin 7.28 g/cm3
Titanium 4.5 g/cm3
Lab Write-Up Format
 Title (This will be the title of the lab)
 Purpose: (This may be called objective or goal; it is the
learning purpose of the lab.)
 Procedure: (These are directions for performing the
lab. It is VERY important that you put these directions
in your own words.)
 Safety concerns: (As you read the lab, note the
solutions and situations that may be dangerous.
Record those safety issues here and leave three
additional lines for safety concerns that I address
before the lab.)
 Data: (Draw the data table in your lab here.
Eventually, you will create your own data tables.)
 Problem Solving: (Completed AFTER you have
finished the lab.
Reflection Questions
(Select one of the prompts below and respond in a oneparagraph reflection of your lab experience. )
1. What are my strengths and weaknesses as a lab
partner?
 2. What skills do I need to work on to achieve better
lab results?
 3. What parts of the procedure did I find confusing and
how did I figure out what to do?
 4. What distracted me in this lab and how could I avoid
that distraction in the future?
 5. How did this lab tie in to what I am currently learning
in Chemistry class?
 6. What are three "resolutions" I could make for future
lab activities?
Lab Safety Activity
 Take out your Lab Safety Contract.
 Each table will be given a group of safety rules
on this sheet. For the rules assigned to you,
record your responses to these questions:
 Which ones are confusing or do not make sense to
you?
 Which rule are you most likely to use in every day
life (it’s just common sense)?
 Which rule do you think your peers are mostly like to
break/forget?
 Breaking which rule would be most likely to cause
an injury?