Download Final Exam Class Review - Mrs. Kittrell`s Science Classes

Physical Science
EOC Review
Marilyn Pendley, Instructor, CCCMC
Modified by R. Kittrell
Jan 2015 & 5Jan2016
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Scientific Experimentation
controlled experiment
-Only one variable should be changed
at a time.
Manipulated (independent) variable –
changed by the experimenter.
Responding (dependent) variable – the
effect that is measured.
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Law vs. Theory
• Develop a law
– Law: Summarizes the outcome of several
experiments that occur repeatedly and
consistently.
– Example: The spoiled food served at lunch
makes people sick with a stomachache.
• Develop a theory
– Theory: Explanation for why a law exists.
– Example: It is the bacteria in the spoiled food
that makes people ill.
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Types of Measurements
1. Length
a. The distance from one point to another
point.
b. Base unit is the meter (m).
c. Tool is the metric ruler.
2. Volume
a. The amount of space a substance
occupies.
b. Base unit is the liter (L).
c. Tools: metric ruler for regular solids or
graduated cylinder for liquids.
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3. Mass
a. The amount of matter in a
substance.
b. Base unit - kilogram (kg).
c. Tool is the balance.
4. Weight
a. A measure of gravitational force
on an object.
b. Unit is the newton (N).
c. Tool is the scale.
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5. Time
a. How long an event takes to occur.
b. Unit is the second (s).
c. Tool is the clock (stopwatch).
6. Temperature
a. The amount of kinetic energy a
substance has.
b. SI unit is the Kelvin (K).
c. Tool is the thermometer.
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7. Density
a. How compacted the matter is in a
substance.
b. Units can be g/mL, g/cm3, kg/m3.
c. Density is a derived unit (it is made
up of other types of measurement).
d. D = m / v
e. Objects float if their density is less
than the density of the fluid they are
in.
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Who is the Father of Atomic Theory?
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Thomson’s Experiment:
• In Thomson’s model of the atom, the negative
charges are scattered throughout an atom filled with
a positively charged mass of matter.
• The “plum pudding” model
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What did this experiment prove?
Beam of Alpha-Particles were
REPELED by Positive Charges in the nucleus
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Atomic Theory:
Who’s Model
of the Atom?
Neils Bohr
The
Bohr Model
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Electron_______
Cloud is a visual model
An _________
of the most likely locations for electrons in
an atom.
www.unitedstreaming.com – Physical Science – Elements, Compounds, and Atoms
An Orbital is a region of space around the nucleus where an electron is likely to be found.
* An electron cloud is a good approximation of how
electrons behave in their orbitals.
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Lewis Dot Diagram
•An electron dot diagram uses
the symbol of the element and
dots to represent the outer level
electrons.
•Electron dot diagrams are used
also to show how the electrons
in the outer energy level are
bonded when elements combine
to form compounds.
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Atom
the smallest particle making up elements
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Atomic Structure Basics:
• Protons: positively charged
particles, weighing 1 atomic
mass unit (1.67x10-24 grams)
and located in the nucleus.
• Neutrons: neutrally charged
particles, weighing
approximately 1 atomic
mass unit and located in the
nucleus.
• Electrons: negatively
charged particles , weighing
zero atomic mass units,
located in orbitals of the
energy levels found outside
the atomic nucleus
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Atomic Number:
• The number of protons • Play the Name the
in an atom determines
Atom Game at:
what element it is.
• http://www.learner.org
• Add or subtract even
/interactives/periodic/b
one proton from an
asics_interactive.html
atom of any element
and you no longer have
the original element in
any form. Now you have
a different element!
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Drawing an Atom of Carbon
6
C
12.011
Atomic # = # of p+ and # of eCarbon has 6 p+ and 6 e-
Atomic Mass minus Atomic # = # of n0
Carbon has 6 n0
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Drawing an Atom of
Carbon
eee-
6 p+
6 n0
e-
ee19
Periodic Table Basics:
Essential Question: What are Horizontal Rows called?
Answer: PERIODS
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Electron Configuration
• The “Period” number is
equal to the number of
energy levels in an atom
• Remember:
The number of
electrons are equal to
the number of protons
in a neutral atom
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What are Groups on the Periodic Table?
Essential Question: Groups are also known as Families of Elements.
They share chemical properties. WHY?
Answer: They have the same number of outer shell electrons.
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Electron Configuration
• For Groups IA – VIII the
group numbers are
equal to the number of
outer shell electrons or
valence electrons
• Group “IA” has ONE
valence electron
• Group “IIA” has TWO
valence electrons; etc.
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Name that GROUP:
The Alkali Metals
IA = one outer shell electrons
therefore Oxidation state?
+1
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Name that GROUP:
The Alkali Earth Metals
IIA = two outer shell electrons
Oxidation state?
+2
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Name that GROUP:
The Noble Gases
VIIIA = eight outer shell electrons (except Helium which has 2 but is FULL)
therefore Oxidation state?
NOT!
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Name that GROUP:
The HALOGENS
The Salt Formers
VIIA = SEVEN outer shell electrons
therefore Oxidation state?
-1
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Name that GROUP:
The Transition Metals
B series = usually 2 or 3 outer shell electrons
therefore Oxidation state?
+2 or +3
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Criss-Cross Method
• Determine the charges/oxidation #’s for each
element.
• By criss-crossing the charges of the elements
you can easily write the chemical formula
• Example:
Hydrogen + Oxygen
– H + O  IONS = H+1 + O–2
– Criss cross the oxidation #
• just the numbers - not the + / - signs
– Write the numbers as subscripts
• bottom right of symbol
Criss Cross Method
This becomes
H+1
O-2
CrissCross the numbers
H2O1
Final:
H2O
• Where is the 1 in the final formula?
Criss-Cross Method
e-
This becomes
e-
H+1
O-2
CrissCross the numbers
H2O1
Final:
H2O
• Where is the 1 in the final formula?
Criss-Cross Method - -You Try it!
Mg + O
Ca + P
K+S
C+H
As + S
C+O
Criss-Cross Method
You Try
1.
2.
3.
4.
5.
6.
Mg + O
Ca + P
K+S
C+H
As + S
C+O
 Mg2O2  MgO
 Ca3P2
Just like with
Fractions in
 K2S
math the
 CH4
Numbers will
reduce!
 As2S3
 C2H4  CO2
Criss-Cross & Polyatomic Ions
• Sodium + Sulfate
– Na + SO4
– Na+1 + (SO4)-2
Do the Criss-Cross
Na2(SO4)1
Final: Na2(SO4)
Chemical Bonding:
• Three types of bonding
Game: Ionic Bonding
• Ionic
• Covalent
• Metallic
Bonding Animations and short clips
AWESOME MOVIE ON BONDING
30 minutes long
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Ionic Bonding
• Ionic Bonds: between oppositely charged atoms;
usually on opposite sides of the periodic table
(nonmetal and a metal)
• transfer electrons
• form networks, not molecules
• conduct electricity
Covalent Bonds
• Covalent Bonds: share electrons; usually
between 2 elements close on the periodic table
(2 nonmetals)
– nonpolar covalent bond: e- shared equally
– polar covalent bond: e- shared unequally
Metallic Bonding
• “sea of electrons”: electrons can “float” freely
between atoms; allows metals to conduct
electricity well
Rules for naming and
writing chemical formulas
1. Metal name comes first
2. Change the ending of the second element to
“ide”
• If you have two nonmetals, use the prefixes:
Mono – 1
Penta - 5
Di - 2
Hexa - 6
Tri - 3
Hepta - 7
Tetra – 4
Octa - 8
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Which of the following is the correct name
of a combination of sodium and iodine?
• a) sodium chloride
• b) sodium iodide
• c) sodium iodine
• d) iodine sodium
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Transition Metal Naming
• Transition metals show their charges as Roman
Numerals because they can change charge!!
FeO = Fe+2 + O-2
Iron (II) Oxide
Fe2O3 = Fe+3 + O-2
Iron (III) Oxide
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Chemical Reactions Types
• Combustion: ALWAYS has O2 as a REACTANT!
– AB + O2
AO + BO
• Single-Replacement (single-displacement):
• AX + B
A + BX
• Double-Replacement (double-displacement):
• AX + BY
AY + BX
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Types of Chemical Reactions.
Type of
Reaction
Synthesis
Decomposition
Definition
 Equation
Two or more elements or
compounds combine to
make a more complex
substance
A + B → AB
Compounds break down
into simpler substances
AB → A + B
Single
Replacement
Occurs when one element
replaces another one in a
compound
AB + C → AC + B
Double
Replacement
Occurs when different
atoms in two different
compounds trade places
AB + CD → AC + BD
A = Red B = Blue C = Green D = Yellow
Identifying Chemical Reactions
Use colored pencils to circle the common atoms or compounds in
each equation to help you determine the type of reaction it
illustrates. Use the code below to classify each reaction.
S = Synthesis
D = Decomposition
____ P +
O2 → P4O10
____ HgO → Hg
____ Cl2 +
+
SR = Single Replacement
DR = Double Replacement
____ Mg + O2 →
O2
NaBr → NaCl + Br2
____ Al2O3
MgO
→ Al + O2
____ H2 + N2 → NH3
____ Na
____ HgO
+ Br2
→ NaBr
____ CuCl2 + H2S →
+ Cl2 → HgCl + O2
____ KClO3 →
KCl +
____ BaCl2 + Na2 SO4 →
O2
NaCl +
____ C +
____ S8 +
BaSO4
H2 →
F2 →
CuS + HCl
CH4
SF6
Acids & Bases
• The strength of an acid or base depends on how
many acid or base particles dissociate into ions
in water.
• Strong Acid/Base
- +
– 100% ions in water
– strong electrolyte
– HCl, HNO3, NaOH, LiOH
•
Weak Acid/Base
• few ions in water
• weak electrolyte
• HC2H3O2, NH3
- +
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pH Scale
• pH
– a measure of the concentration of H3O+ ions
in solution
– measured with a pH meter or an indicator
with a wide color range
Atomic Structure:
How many neutrons in
the following isotopes?
Hydrogen – 1
Helium – 4
Lithium – 6
Sodium – 22
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More Isotope stuff…
A
Mass Number
Z
Atomic Number
1
1
2
H
1
235
92
U
X
Element Symbol
3
H (D)
1
238
H (T)
U
92
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Radioactive Decay
Radioactive decay results in the emission [or release] of
either:
• an alpha particle (a),
• a negative beta particle (electron) (b-),
• a positive beta particle (positron) (b+),
• or a gamma ray (g).
In a nuclear reaction the MASS and ATOMIC NUMBER
must be the SAME on both sides of the equations
Alpha Decay
An alpha particle is identical to that of a helium nucleus.
It contains two protons and two neutrons.
A
X
Z
A-4
4
Y
He
+
Z-2
2
unstable atom
alpha particle
more stable atom
Beta Emission
A beta particle is a fast moving electron which is
emitted from the nucleus of an atom undergoing
radioactive decay.
Beta emission occurs when a neutron changes into a
proton and an electron.
A
X
Z
A
Y
+
Z+1
proton stays
in nucleus
0
e
-1
beta particle
(electron)
Gamma Decay
• When atoms decay by emitting a or b
particles to form a new atom, the nuclei
of the new atom may still have too much
energy to be completely stable. These
unstable atoms will emit gamma rays to
release that energy.
• There is no change in mass or atomic
number
A
X
Z
A
Z
X +
g
0
0
Decay Summary
Reaction
What happens?
Alpha Decay
a
Lose Helium Nucleus
Beta Decay
b-
Lose electron from nucleus
(neutron turns into proton)
Gammy Decay
g
Mass #
Atomic #
-4
-2
No change
+1
Emit high energy gamma ray No change
and either a or b particle
No
change
Test questions may involve
graphs like this one. The
Most common questions are:
"What is the half-life of this
element?"
Just remember, that at the end
of one half-life, 50% of the
element will remain. Find 50%
on the vertical axis. Follow the
blue line over to the red curve
and drop straight down to find
the answer:
The half-life of this element is 1 million years.
Another common question is:
"What percent of the material
originally present will remain
after 2 million years?"
Find 2 million years on
the bottom, horizontal
axis. Then follow the
green line up to the
red curve. Go to the left
and find the answer.
After 2 million years 25% of the original material
will remain.
Nuclear Energy Essential Questions:
• Why is it worth the
RISK??
• Tremendous
OUTPUT of
ENERGY!!
• Fission or Fusion?
•Fission! Atoms of
U-235 are split
•Use the link to see how Nuclear Fusion works:
•Fusion! Atoms are
joined or fused
together.
http://science.howstuffworks.com/fusion-reactor.htm/printable
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Heat energy:
• Direction of Energy Flow?
• HOT toward COLD
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States of Matter
• Watch what happens to molecules when
heated by doing cool virtual experiments.
• Click on the icon below to get started:
60
Change of Phase
FIRST DO THIS Temperature Experiment By Clicking Here!
Phase
change
Phase
change
To Understand this Graph
CLICK HERE
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Chemical or Physical Change?
Chemical Change
Physical Change
• New substances formed
with new properties
• No new substances
formed
• Examples:
• Examples:
• Rusting
• Gas forming during a
reaction (bubbles)
• A precipitant forming
during a reaction
• Ice melting
• Water evaporating
• Dry ice subliming
into Carbon dioxide
• Salt or sugar
dissolving in water
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CLASSIFICATION OF MATTER
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ELEMENTS
• contain only one type of atom
• building blocks of matter
• 115 known elements today, 90 which
occur naturally
• Found on periodic table
– The first letter is always capitalized, the
second letter is always lower case
• Fluorine is F, not f
• Cobalt is Co, not CO (which is carbon monoxide)
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Compounds
Compounds - 2 or more elements
chemically combined to form a new
substance with new properties
Properties – The way a chemical
substance looks and behaves
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Types of Matter:
Review basics about classifying matter by following the link below.
Watch the video clips!
Make sure you scroll all the way down to the chart to test your knowledge!
www.kentchemistry.com/links/Matter/ClassifiyingMatter.htm
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Mixtures and Pure Substances
– A mixture has unlike parts and a composition
that varies from sample to sample
• A heterogeneous mixture has physically distinct
parts with different properties.
• A homogeneous mixture is the same throughout
the sample
– Pure substances are substances with a fixed
composition
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Matter
comes in 3
phases
Solid
Gas
Liquid
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Solid
Definite
Shape
Definite
Volume
69
Liquid
Indefinite Shape
– takes the shape
of the container
Definite
Volume
70
Gas
Indefinite
Shape – takes
the shape of the
container.
Indefinite
Volume – can
expand and can be
compressed.
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Plasma
•
•
•
•
•
Plasma: a high energy gaseous state of matter.
It is very unstable.
Particles are moving extremely fast, free energy
Most abundant phase of matter
Only present under extremely hot/energetic
situations
• Example: Sun
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CHANGES IN STATE
• Melting: Solid to liquid
• Boiling: Liquid to gas
• Sublimation: Solid to gas
– The above three require input of energy
• Condensation: Gas to liquid
• Freezing: Liquid to solid
• Deposition: Gas to solid
– The above three release energy
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PHYSICAL PROPERTIES
• Characterize the physical state and physical
behavior of a substance {appearance, smell, feel}
• Each substance has unique physical properties
• Examples
– Sulfur appears as a yellow powder
– The boiling point of water is 100 oC
– Carbon monoxide is odorless
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Solubility
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Where is Magnetism Concentrated?
Magnetism is strongest at the
POLES
79
Magnetic Domains :
Not aligned:
Magnetic domains
are ALIGNED in a
permanent
magnet :
80
What happens if you cut a magnet in half?
81
Electricity and Magnetism:
Electromagnetism
82
Get in line!
83
Electromagnets:
• What Happens if you
increase the number
of coils in an
electromagnet?
• The magnet gets
STRONGER!
84
Induction charging of two metal spheres:
85
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Potential Energy:
PEgrav = mass • g • height
Too hard to remember? Use the Reference Table!
87
Answer key:
A: PE = 40 J (since the same mass is
elevated to 4/5-ths height of the
top stair)
B: PE = 30 J (since the same mass is
elevated to 3/5-ths height of the
top stair)
C: PE = 20 J (since the same mass is
elevated to 2/5-ths height of the
top stair)
D: PE = 10 J (since the same mass is
elevated to 1/5-ths height of the
top stair)
E and F: PE = 0 J (since the same
mass is at the same zero height
position as shown for the bottom
stair
Note since
PEgrav = m *• g • h
Doubling of the height
will result in a
doubling of the
gravitational
potential energy.
• A tripling of the
height will result in a
tripling of the
gravitational
potential energy.
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Physics Portion
• Make a given table that lists the information
you are given. BE SURE to include the item
you are to find!
• USE the Reference sheet! Find the equation
that fits what you have.
• Put the item you need to find on one side of
the equals sign.
• Add the other numbers and punch in the
calculator.
• Double check the answer from the calculator!
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