S8P1. Students will examine the scientific view of the nature
of matter. a.Distinguish between atoms and molecules Page 42
Slide 2
S8P1a. Matter10/12/1 2 What is matter and how can it be
classified? Page 43 Matter is anything that has mass and takes up
space. Examples: book, toy, car, paper Non-examples: heat, light
Matter is made of tiny indivisible particles called atoms. Atoms
are the basic building blocks of all matter. For many years, people
have wondered what matter is made of including Democritus,
Lavoisier, Dalton, Thompson, Rutherford and Bohr.
Slide 3
Page 45 Democritus thought the universe was made of empty space
and tiny bits of stuff that were so small they could no longer be
divided into smaller pieces. He called these pieces atoms.
Lavoisier came up with the law of conservation of matter, which
states that matter is not created or destroyed it only changes
forms. wood + oxygen = ash + gases + water vapor Dalton developed
the atomic theory of matter. He felt that matter was too small to
be seen by the human eye and that each type of matter was made of
only one kind of atom.
Slide 4
Page 47 Thompson discovered that atoms were a ball of positive
charge embedded with negatively charged particles, called
electrons. Rutherford called the positively charged, center part of
the atom the nucleus. He named the positively charged particles in
the nucleus, protons. He concluded that the atom must be mostly
empty space in which electrons travel in random paths around the
nucleus. Chadwick, a student of Rutherfords discovered uncharged
particles in the nucleus, called neutrons.
Slide 5
Page 49 Bohr found that electrons are arranged in energy levels
in an atom. The lowest energy level is closest to the nucleus. It
can only have two electrons. Higher energy levels are farther from
the nucleus. According to Modern Atomic Theory, electrons move in a
cloud around the nucleus. Atoms are very small. It would take a
million of them combined to be the size of a pencil tip. As tiny as
atoms are, they consist of even smaller particles protons, neutrons
and electrons.
Slide 6
On page 46,neatly illustrate, color and label Rutherfords Model
of the Atom with Chadwicks contribution of the neutron. When
labeling, label and define the nucleus, electrons, protons,
neutrons. On the top half of page 48, neatly illustrate, color and
label Bohrs Model of the Atom On the bottom half of page 48, neatly
illustrate, color and label the current model of the atom.
Slide 7
Page 51 The nucleus is the small dense, positively charged
center of an atom. It contains the most of the atoms mass. The
nucleus contains protons and neutrons. Protons are positively
charged particles located inside the nucleus. Neutrons are
neutrally charged particles located inside the nucleus. Electrons
are negatively charged particles found in electron clouds outside
the nucleus.
Slide 8
On page 50 + + + + + + - - - - - -
Slide 9
Page 51 & 53 There are two kinds of pure substances:
elements and compounds. An element is matter made up of only one
kind of atom. There are over 100 known elements. About 90 of them
are found naturally on Earth and the other 20+ are synthetic
(man-made). All known elements are arranged in a chart called the
periodic table of elements. Each element on the chart has a
chemical symbol with one to three letters. The periodic table is
arranged in rows called periods and columns called groups or
families. There are 7 periods and 18 groups.
Slide 10
Page 53 Elements in the same group share similar properties.
Each element has an atomic number and an atomic mass. The atomic
mass is the average of all of the isotopes of an element. The
atomic number is ALWAYS the number of protons. It is also the
number of electrons in a neutral atom. To determine the number of
neutrons, you must subtract the atomic number from the atomic mass.
For example, Copper has an atomic number of 29 and an atomic mass
of 63. It has 29 protons, 29 electrons and 34 neutrons.
Slide 11
On page 52 Look at the periodic table and identify the group
name of the following elements: 1.Lithium 2.Xenon 3.Gold
4.Beryllium
Slide 12
Page 55 Sometimes the atomic mass of elements can change. For
example Hydrogen sometimes has an atomic number of 1, 2 or 3. This
is because the number of neutrons may vary. Isotopes are atoms of
the same element that have a different number of neutrons. When
referring to an isotope, you state the element name followed by its
atomic mass. For example: Hydrogen-1 or Hydrogen-2 or
Hydrogen-3
Slide 13
S8P1a., S8P1f., S8P1d Matter10/31/1 2 How can matter be
classified? Page 59 All forms of matter can be classified into two
groups: pure substances and mixtures. A pure substance is one
having a homogeneous composition. There are two types of pure
substances: elements and compounds. An element is matter that is
made of only one kind of atom. A compound is matter that is formed
when two or more elements join (bond) chemically. They cannot be
broken apart.
Slide 14
On page 58 Identify whether each of the following are elements
or compounds in the table below. H H 2 0 Ca Na NaCl CO 2 Co Fe 2 S
OH CH 4 NaOH CO SiO 2 ElementCompounds
Slide 15
Page 61 A molecule is the smallest unit of a compound that has
all the properties of the compound. The makeup of a molecule is
shown in a chemical formula. A chemical formula uses chemical
symbols and subscripts to identify the number and types of atoms of
each element that make up a compound. A subscript is a small number
written to the right and slightly below a chemical symbol to tell
the number of atoms of that element is in the substance. The
chemical formula for water is H 2 0. This means one molecule of
water has 2 Hydrogen atoms and 1 Oxygen atom.
Slide 16
On page 60 Determine the number of atoms of each element
present in each of the following compounds. 1.CO 2.CO 2 3.H 2 O 2
4.NaCl 5.NaOH 6.C 12 H 22 O 11 7.FeS 2 8.Fe 2 O 3 9.C 2 O 10.Na 2 O
11.CH 4
Slide 17
Page 63 Elements can combine in different ways to form either
compounds or mixtures. A mixture forms when two or more substances
combine without joining chemically. They are not bonded together.
Because they are not bonded chemically, the parts of a mixture
retain their own individual identities and properties and can be
separated. A mixture that is unevenly mixed is called a
heterogeneous mixture. Ex. Trailmix. A mixture that is mixed evenly
is called a homogeneous mixture. Ex. Kool-Aid Summary: EQ- How can
matter be classified?
Slide 18
On page 62 Identify whether each of the following are
heterogeneous or homogeneous mixtures in the table below. Vegetable
soup Chex Mix coffee cake batter chocolate chip cookie milk salt
water pizza spaghetti & meatballs cereal in milk taco salad
Heterogeneous MixtureHomogeneous Mixture
Slide 19
S8P1a., S8P1f., S8P1d States of Matter 11/2/12 Water can be
found in solid, liquid and gas forms, how does that happen? Page 65
A state of matter is the physical form in which matter exists.
There are four states (phases) of matter : solid, liquid, gas and
plasma. Matter often changes state when heat is added or taken
away. A solid is a substance with a definite shape and a definite
volume. The particles in a solid are packed closely together and
maintain a rigid form without a container. They vibrate slowly
against one another.
Slide 20
Page 67 A liquid is a substance with a definite volume, but not
a definite shape. The particles in a liquid move faster and freely
past one another, but are still close to one another. Liquids take
the shape of the container they are in. A gas is a substance that
does not have a definite shape or a definite volume. Gas particles
move very fast and bounce off of one another. Gases fill the
container they are in.
Slide 21
Page 69 The transformation of matter from one state to another
is called a phase transition. Phase transitions occur at precise
points when the energy of motion in the atom is too much or too
little for the atom to remain at that state. Summary: EQ-Water can
be found in solid, liquid and gas forms. How does that happen?
Phase TransitionDescription Melting (add heat)Solid to Liquid
Evaporation (heat added)Liquid to Gas Sublimation (heat added)Solid
to Gas (skipping Liquid) Condensation (heat removed)Gas to Liquid
Freezing (heat removed)Liquid to Solid Deposition (heat removed)Gas
to Solid (skipping Liquid)
Slide 22
On page 64 Identify whether each of the following are solids,
liquids or gases in the table below. Milk toy car helium hydrogen
water ice steam sugar salt pepsi oxygen SolidLiquidGas
Slide 23
On page 66 The freezing point and melting point are the same
temperature.
Slide 24
On page 68 The following processes are phase transitions. Make
the table below and identify what they are. Phase Transition Water
droplets coat your cold soda can on a hot day. A cloud releases
rain. Solid dry ice steams in air. Glaciers floating in the ocean
are shrinking. Morning dew disappears from the grass by midday. A
cloud releases snow.
Slide 25
S8CS1, S8CS2, S8CS5, S8CS9 and S8P3 Scientific Method 11/27/12
How does the design and construction of a bridge affect its
durability and ability to withstand weight? Page 71 Bridge #Design
/ DescriptionMaximum Weight Failure Description 1 2 3 4 5 6 7 8
9
S8P1d. Properties of Matter 12/3/12 What are the various
properties of matter and how can I distinguish between physical and
chemical properties of matter? Page 75 A property is a
characteristic of matter. A physical property is a characteristic
that can be observed or measured without changing the identity of a
substance. Examples: density (mass/volume), electrical
conductivity, hardness, pH, state of matter and luster A chemical
property is a characteristic that describes how a substance will
interact with other substances during a chemical reaction.
Examples: reactivity, the ability to burn and rust Summary: What
are the various properties of matter and how can I distinguish
between physical and chemical properties of matter?
Slide 29
page 74 Create a two-column table and classify each of the
terms below as either a physical property or a chemical property.
reacts with base to form water Boiling point density Taste reacts
with an acid color flammability melting point luster reacts to
oxygen solubility hardness odor reacts with water to form gas
Physical PropertyChemical Property
Slide 30
S8P1.d & S8P1.e Changes in Matter 12/3/12 What types of
changes can matter undergo? What happens to matter when it
undergoes changes? Page 77 Matter can change. The types of changes
matter undergoes are classified into two groups: physical changes
and chemical changes. A physical change alters the physical
properties of a substance without changing the identity of the
substance. Physical changes cause a change in properties such as
volume, mass, or state of matter. Many physical changes can be
reversed. Examples: melting, evaporating, freezing, cutting A
chemical change occurs when a substance is changed into a new
substance with different properties. During a chemical change, the
identity of a substance is changed. Examples: burning, rusting,
baking, combusting
Slide 31
Page 79 A chemical reaction is the process by which new
substances are formed during a chemical change. Some signs that
indicate a chemical reaction has occurred include the forming of
gases, a change in color, the release of heat, or the emission of
light. Another sign of a chemical reaction is the formation of a
precipitate. A precipitate is a solid that forms from a chemical
reaction that takes place in a solution. It is very difficult or
impossible to reverse the effects of a chemical change. Summary: EQ
- What types of changes can matter undergo? What happens to matter
when it undergoes changes?
Slide 32
page 76 Create a two-column table and classify each of the
descriptions below as either a physical change or a chemical
change. Iron rusts sodium hydroxide dissolves in water milk goes
sour a match ignites and burns an ice cube melts to form a puddle
of water icicles form at the edge of a roof chocolate bar melts in
the sun water is heated and changed into steam vinegar and baking
soda react acid on limestone produces carbon dioxide gas wood and
leaves rot a tea kettle begins to whistle Physical ChangeChemical
Change
Slide 33
page 78 PHYSICAL OR CHEMICAL CHANGE? YES PHYSICAL CHANGE NO
CHEMICAL CHANGE QUESTION: AFTER THE CHANGE IS IT THE SAME
SUBSTANCE? EVIDENCE OF A CHEMICAL CHANGE BUBBLING TURNS CLOUDY
TEMPERATURE CHANGES EXOTHERMIC ENERGY IS EXITING - GETS HOTTER
ENDOTHERMIC ENERGY IS ENTERING GETS COOLER COLOR CHANGE CHANGE IN
SMELL OR TASTE
Slide 34
S8P1g. Conservation of Matter 12/4/12 During a change in
matter, how does the amount of matter compare before and after it
changes? Page 81 The law of conservation of matter states that,
during a chemical reaction, matter cannot be created or destroyed.
Even though the matter may change from one form to another, the
same number of atoms exist before and after the changes take place.
Reactant the substances there before a reaction occurs. Product the
substances there after the reaction takes place. MASS OF REACTANT =
MASS OF PRODUCT
Slide 35
UNDERSTANDING CHEMICAL REACTIONS & THE LAW OF CONSERVATION
OF MATTER 2H 2 + O 2 2H 2 0 Reactants Products A coefficient shows
the number of molecules. 2H2 means 2 hydrogen molecules for a total
of 4 hydrogen atoms. A subscript shows how many atoms are in a
formula. In O2, the 2 means 2 atoms of oxygen. 4K + O 2 2K 2 0 25g
+ 5g 30g If 25g of Potassium is reacted with 5g of Oxygen, how much
Potassium Oxide is produced? Page 83
Slide 36
page 80 Write the questions and answer each. How many different
elements are present? N 2 CaF 2 CO 2 NaSO 3 CaCO 3 SiO 2 How many
molecules are present? 2H 2 O 5Be 2 Br 8CO 2 3NaCl O 2 MgS How many
total atoms are present? 2H 2 O 2Be 2 Br 7CO 2 6NaCl 4O 2 2MgS
Using this reaction, answer the following questions. Li 2 O + MgCl
2 2LiCl + MgO Name the first reactant. Circle the second reactant.
Underline the first product. Name the second product. How many Mg
atoms are on the reactant side? the product side? How many Chlorine
atoms are on the reactant side? the product side?
Slide 37
page 82 Write each chemical reaction (and question) and
determine the missing value? 2Mg + O 2 2Mg0 23g + ?g 38g 2KCl + Li
2 O K 2 O + 2LiCl 21g + 4g ?g + 12g If 23g of Magnesium is reacted
with Oxygen to produce 38 g of Magnesium Oxide, how much Oxygen was
used in the reaction? Using the numbers provided, determine how
much K 2 O is produced in the reaction.