Vocabulary
Mass – measure of the amount of matter the object contains
Volume – measure of the space occupied by the object
Extrinsic/extensive property – property that depends on the amount of matter in a sample
Intrinsic/intensive property – property that depends on the type of matter in a sample, not the amount of matter
Substance – matter that has a uniform and definite composition
Physical property – a quality or condition of a substance that can be observed or measured without changing the substance’s composition
Solid – form of matter that has a definite shape and volume
Liquid – form of matter that has indefinite shape, flows, yet has a fixed volume
Gas – form of matter that takes both the shape and volume of its container
Vapor – the gaseous sate of a substance that is generally a liquid or a solid at room temperature
Physical change – some properties of a material change, but the composition of the material does not
Mixture – physical blend of two or more components
Heterogeneous mixture – a mixture in which the composition is not uniform throughout
Homogeneous mixture – a mixture in which the composition is uniform throughout
Solution phase - any part of a sample with uniform composition
Filtration – the process that separates a solid from a liquid in a heterogeneous mixture
Distillation – a liquid is boiled to produce a vapor that is then condensed into a liquid
Element – simplest form of matter that has a unique set of properties
Compound – a substance that contains two or more elements chemically combined in a fixed proportion
Chemical change – a change that produces matter with a different composition than the original matter
Chemical symbol – one or two-letter representation of an element
Periodic table – an arrangement of elements in which the elements are separated into groups based on a set of repeating properties
Period – a horizontal row of elements in the periodic table
Group – a vertical column of elements in the periodic table
Chemical property – the ability of a substance to undergo a specific chemical change
Chemical reaction – a change in which one or more reactants change into one or more products
Reactant – a substance present at the start of a reaction
Product – a substance produced in the reaction
Precipitate – a solid that forms and settles out of a liquid mixture
Law of conservation of mass – in any physical change or chemical reaction, mass is
conserved; mass is neither created nor destroyed
Identifying  a  Substance
•
Pure  substances  are  made  up  of  only  one  element  ie.  An  aluminum  can
•
Every  sample  of  a  given  substance  has  identical  intensive  properties  because   every  sample  has  the  same  composition

•
Hardness,  color,  conductivity,  and  malleability  are  examples  of  physical   properties
States  of  Matter
•
Solids     o The  shape  does  not  depend  on  the  shape  of  its  container   o Particles  packed  tightly  together,  often  in  an  orderly  arrangement   o Almost  incompressible     o Expand  only  slightly  when  heated   o Definite  shape  and  volume
•
Liquids   o Particles  in  close  contact  with  one  another  but  arrangement  is  not   rigid  or  orderly  because  the  particles  can  flow  from  one  location  to   another   o Takes  the  shape  of  the  container   o Volume  doesn’t  change   o Shape  changes   o Almost  incompressible     o Expand  slightly  when  heated
•
Gases   o Takes  shape  of  container     o Can  expand  to  fill  any  volume   o Takes  both  volume  and  shape  of  container   o Particles  much  further  apart   o Gasses  are  easily  compressed

Physical  Changes
•
Melting  is  a  physical  change  because  the  composition  doesn’t  change
•
Boil,  melt,  freeze,  split,  grind,  cut,  crush  and  condense  are  all  words  used  to   describe  physical  changes
•
However  those  words  split  up  into  two  different  categories
•
Irreversible   o Grind   o Cut   o Crush   o Split
•
Reversible     o Boil     o Melt   o Freeze   o Condense
Classifying  Mixtures
•
Heterogeneous  or  homogeneous
•
Heterogeneous   o Contents  not  evenly  distributed     o No  uniform  composition   o ie:  chicken  noodle  soup   o two  or  more  phases
•
Heterogeneous  mixture   o Substances  evenly  distributed   o Doesn’t  look  like  a  mixture   o Aka  a  solution   o Many  are  liquids   o Some  are  gases   o Single  phase   o ie:  coffee
Separating  Mixtures
•
Methods   o Filtration   o Distillation
Distinguishing  Elements  and  Compounds
•
Compounds  can  be  broken  down  elements  cannot
Breaking  Down  Compounds
•
Need  a  chemical  change
•
Heating  is  one  processes
•
There  is  no  process  that  could  break  down  carbon  because  it  is  an  element
•
Electricity  can  cause  water  to  break  down

Distinguishing  Substances  and  Mixtures
Chemical  Changes
•
Burn,  rot,  rust,  decompose,  ferment,  explode,  corrode  –  chemical  change
•
Composition  of  matter  always  changes
•
Aka  a  chemical  reaction

Conservation  of  Mass
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Mass  of  the  products  is  always  equal  to  the  mass  of  the  reactants
•
Mass  always  holds  constant  in  a  chemical  reaction
•
Mass  is  neither  created  nor  destroyed
Questions
1.
Which  of  the  following  is  an  example  of  an  intrinsic  property   a.
A  large  marker   b.
A  5lb  weight   c.
A  hollow  chocolate  bunny   d.
A  leather  basketball
2.
Which  of  the  following  is  an  example  of  an  extrinsic  property   a.
A  leather  basketball   b.
A  cotton  sock   c.
A  5lb  weight   d.
An  orange  scented  marker
3.
Which  of  the  following  is   NOT   a  physical  change   a.
The  freezing  of  ice  cubes     b.
Condensing  a  gas  into  a  smaller  container   c.
Cooking  pasta   d.
Burning  a  steak  on  the  grill
4.
Which  of  the  following  is  irreversible

a.
Melting  an  ice  cube   b.
Filing  a  nail     c.
Freezing  a  banana   d.
Boiling  soda
5.
Which  of  the  following  is  heterogeneous   a.
Coffee   b.
Oil  and  vinegar   c.
Oil     d.
Vinegar
6.
Describe  the  difference  between  a  chemical  change  and  a  physical  change.
Give  an  example  of  each.
7.
How  is  the  arrangement  of  particles  different  in  a  solid  and  a  gas?
8.
When  MgS
MgS O
!
O
!
explodes  the  products  are  Mg,  S,  and
originally  and  20g  of  Mg  after  and  21g  of   O
!
O
!
I  have?
9.
Explain  the  difference  between  intrinsic  and  extrinsic  property.
10.
Describe  how  to  break  down  a  compound.
.  If  I  have  50g  of
.  How  many  grams  of  S  do