Transcript EOCT Review PPT

EOCT Review
Physics
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Section 1: Motion, Forces, and
Energy
SPS 7. Students will relate transformations and flow of
energy within a system.
SPS 8. Students will determine relationships among force,
mass, and motion.
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Speed and Velocity:
SPS 8a. Calculate velocity and acceleration.
• Speed is how fast an object is going with respect to an object.
• Velocity is a measure of the speed in a given direction.
• You can say the top speed of an airplane is 300 kilometers per hour
(kph). But its velocity is 300 kph in a northeast direction.
Calculating speed or velocity
•
•
Speed= distance/ time
velocity= distance/time; directions
Calculate the following:
1. Bob travels 300 km in 10 hrs towards the store.
2. Ashley swims 50 m in 10 seconds.
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Acceleration:
SPS 8a. Calculate velocity and acceleration
.
• Acceleration is the increase of velocity over a period of time.
• Deceleration is the decrease of velocity.
• Acceleration = final velocity- initial velocity/ time or
a = vf- vi/ t
Change in acceleration:
• Caused by a change in speed
• Caused by a change in direction
Calculate the acceleration
1. A train traveling 20 meters per second takes 10 seconds to stop.
2. A boy gains a speed of 5 m/s after running for 20 seconds.
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Newton’s Laws of Motion:
SPS 8b. Apply Newton’s 3 Laws to everyday situations by
explaining the following: inertia, relationship between force,
mass, and acceleration, and equal and opposite forces.
• Newton’s 1st Law: An object at rest stays at
rest, and an object in motion stays in motion,
with the same direction and speed unless
acted on by unbalanced force. (Also called the
Law of Inertia)
• Newton’s 2nd Law: F= ma
• Newton’s 3rd Law: For every action there is an
equal and opposite reaction. Forces are found
in pairs.
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Newton’s 1st Law
• The ladder continues to move forward even
though the truck stops.
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Newton’s 2nd Law
• F= ma
F
m a
• The force required to move the car is 50N.
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Newton’s 3rd Law
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Forces and Gravitation:
SPS 8c. Relate falling objects to gravitational force.
Gravity is the force that pulls objects toward the Earth. It is
affected by mass and distance.
• The equation for the force of gravity is F or W = mg.
Acceleration due to gravity
The acceleration due to the force of gravity on Earth is g: 9.8
m/s2 .
Weight
The weight of an object is the measurement of the force of
gravity on that object. You weigh something on
a scale, according to the force that the Earth pulls it down:
w = mg; where w is the weight in Newtons (N)
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Mass and Weight:
SPS 8d. Explain the difference between mass and weight.
• Mass is a measure of how much matter an object has.
• Weight is a measure of how strongly gravity pulls on that
matter.
• Mass is constant, but the weight may change.
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Section 2: Work and Mechanical
Advantage:
SPS 8e. Calculate amounts of work and
mechanical advantage using simple
machines.
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Simple Machines
• Machines are devices that make work easier.
• Machines do work ( W = F • d ) with just one
movement
• Compound machines require more than one
movement to do work.
• There are six simple machines: lever, pulley,
wheel and axle, inclined plane, wedge, and
screw.
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Simple Machines
• Since a machine has
parts that are in contact
with other things,
friction is produced. So
in the real world, a
machine can never be
100% efficient.
• Efficiency = Work
output/ Work input x
100%
Wheel and axle
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Mechanical Advantage
SPS 8e. Calculate amounts of work and mechanical
advantage using simple machines.
Formula for Force
• MA =Resistance force (Fr)
Effort force (Fe)
• MA= 100kg/50 kg
– MA= 2
Formula for Distance
• MA = Input distance (slope)
Output distance (height)
• MA= 12m/6m
MA= 2
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Section 3: Energy and Energy
Transformations
SPS 7. Students will relate transformations
and flow of energy within a system.
SPS 7a. Identify energy transformations
within a system (e.g. lighting of a match.)
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Energy:
SPS 7. Students will relate transformations and flow of energy within a
system.
SPS 7a. Identify energy transformations within a system (e.g. lighting of a
match.)
Types of Energy
Potential energy
Stored energy due to position
Kinetic energy
Energy of motion
Chemical Energy A form of potential energy and it is possessed by things such as
food, fuels and batteries
Thermal Energy
Heat
Mechanical Energy Sum of potential and kinetic energy in a system
Electromagnetic
The energy source required to transmit information (in the form of
Energy
waves) Some types of electromagnetic energy include: radio
waves, microwaves, infrared waves, visible light, ultraviolet light,
x-rays, and gamma rays. All electromagnetic forms of energy
travel at the speed of light which is very fast.
Gravitational
Potential energy
Energy stored within an object due to its height above the surface
of the Earth.
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Energy Transformation
Consuming food
Chemical energy to mechanical energy
Car engine
Chemical energy to mechanical energy
Light bulb
Electrical energy to light and heat
Windmills
Energy of the wind into mechanical energy of the
blades and then into electrical energy
Solar panels
Light energy from the sun into electrical energy
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3 Methods of Heat Transfer
SPS 7b. Investigate molecular motion as it relates to thermal
energy changes in terms of conduction, convection, and
radiation.
Method of heat
transfer
Conduction
Description
Example
Heat transfer by
direct contact
Burning your hand by
touching a hot pan.
Convection
Heat transfer through Wind currents.
fluids (gas or liquid) Heating and cooling
system in our homes
and buildings.
Heat transfer through The hood of a car
open space (vacuum) getting hot on a
summer day.
Radiation
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Conduction
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Convection
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Radiation
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Insulator vs. Conductor
Insulator
Conductor
Material that does not allow
heat/charge to pass easily.
Examples: wood, plastic,
rubber, air, fiberglass,
fleece, thermal underwear
Poor conductor
Material that allows
heat/charge to pass easily.
Examples: Metals such as
copper, silver, gold,
aluminum
Poor insulator
Heat travels from a warmer material to a colder
material.
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Calculating Specific Heat
SPS 7c. Determine the heat capacity of a substance using
mass, specific heat, and temperature.
• The amount of energy needed to raise 1kg of a
substance by 1 K
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Section 4: Waves, Electricity, and
Magnetism
SPS9- Students will investigate the
properties of waves
SPS10: Students will investigate the
properties of electricity and magnetism.
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SPS9a.
Recognize that all waves transfer energy.
• A wave is a disturbance that transfers energy
through matter or through space.
• Some waves, like sound waves, must travel
through matter, these waves are called
mechanical waves.
• Other waves, like light do not require a
medium and can travel through space. These
waves are called electromagnetic waves.
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SPS9e.
Relate the speed of sound to different mediums
2 Different Types of Waves
.
Mechanical
• (requires a medium: solid,
liquid, or gas)
Electromagnetic
• (does not require a medium/
can travel in a vacuum)
• Sound waves require air
• Radio waves
(gas)
• Water waves require water • Infrared Light
(liquid)
• Earthquake (seismic waves) • Gamma rays
requires earth (solid)
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SPS9e.
Relate the speed of sound to different mediums
Wave Speed through different mediums
• Sound travels fastest in solids.
• Sounds travels slowest in gases?
Sound travels faster in solids because particles
are closer together in solids than in gases, and therefore
energy moves faster!
Gas
Liquid
Solid
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Longitudinal vs. Transverse
• Waves can be either longitudinal (compression)
or transverse.
Label the parts of the wave below.
Longitudinal
Transverse
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Relating Frequency and Wavelength:
SPS 9b. Relate frequency and wavelength to the
electromagnetic waves and mechanical waves
.
Frequency is how fast the wave is moving. If you stand in
one spot and watch a wave go by, it is the number of
crests that go by in a second.
• Waves with long wavelengths have a low frequency.
Waves with short wavelengths have a high frequency.
The higher the frequency, the more energy a wave has.
• The speed or velocity of a wave depends on the
wavelength and the frequency. The formula for wave
speed is:
• Speed = wavelength x frequency
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Frequency vs. Wavelength
• What happens to the wavelength as the
frequency decreases?
• Which wave has more energy? Why?
A.
B.
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THE ELECTROMAGNETIC SPECTRUM:
SPS 9c. Compare and contrast the characteristics of
electromagnetic and mechanical (sound waves).
• The electromagnetic spectrum is a set of electromagnetic waves in
order of wavelength and frequency.
– a long wavelength has a low frequency
Rabbits
Mate
– a short wavelength has a high frequency.
In
• What happens to frequency as you move from left to right?
Very
Wavelengths? Energy?
Unusual
X-tra
• Which wave has the longest wavelength? Shortest?
Gardens
• Which wave has the highest frequency? Lowest?
• Which wave has the most energy? Least?
• F
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Wave Interactions:
SPS 9d. Students will investigate the phenomenon of
reflection, refraction, diffraction, and interference.
• When a wave hits a piece of matter, the wave
can be absorbed or it can be reflected.
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Wave Interaction
Reflection
• The bouncing back after a
wave strikes an object that
it cannot pass through.
Refraction
• The bending of waves due
to a change in speed.
• Examples include prisms,
lenses like glasses and
contacts, and a mirage.
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Wave Interaction
Diffraction
Interference
• The bending of waves
around a barrier. When it
encounters a barrier, the
wave can go around it.
• Examples include sound
waves bending to come
around a corner, or
underneath a door
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Doppler Effect
SPS 9f. Explain the Doppler Effect in terms of everyday
interactions.
• Who hears a higher pitched sound? Why?
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Electricity
Electricity & Magnetism:
SPS10: Students will investigate the
properties of electricity and magnetism
SPS10a. Investigate static electricity in terms
of friction, induction, and conduction.
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Static Electricity
• Static - some of the outer electrons are held very
loosely.
• They can move from one atom to another.
• An atom that loses electrons has more protons
than electrons. It is positively charged- cation
• An atom that gains electrons has more electrons
than protons. It has a negative charge- anion.
• A charged atom is called an "ion."
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Static Electricity
• Static electricity is the imbalance of positive
and negative charges.
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Current Electricity:
SPS10b Explain the flow of electrons in
terms of alternating and direct current;
the relationship between voltage,
resistance and current; simple, series,
and parallel circuits
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Electricity
• To make "something" (refrigerator, light,
computer, radio controlled car, sewing
machine......) turn on we need:
– an appropriate source of electricity (battery/outlet),
– metal wires insulated with plastic,
– a switch
– and the “thing”.
• We connect them in a distinct sequence for the
thing to work.
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Source of Energy
• In the case of DC (Direct Current – (battery)
current flows in one direction only), it has a
limited life than is unusable so we throw it
away.
• -In the case of AC (alternating Current – (wall
plug) current flows back and forth (changes
direction)) the power company provides the
electricity, it is far closer to limitless as an
energy source.
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Electric Current
• The flow of electrons is called a current, an electric
current
V
• Current flows from high to low energy.
• The formula for calculating voltage is:
R I
– V=RxI
•
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Circuits
Series Circuits
• The current must flow
through one device to get to
the next device. This means
that the rate of current flow
through all devices is the
same.
• 1 loop
Parallel Circuits
• In a parallel circuit each
device is directly connected
to the power source. This
means that each device
receives the same voltage.
• 2+ loops
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Series Circuit vs. Parallel Circuits
Series
1. Has a single loop for electrons
to travel round
2. Components are connected
one after another
3. Current has to travel through
all components
Parallel
1. Has two or more paths for
electrons to flow down
2. Current is shared between
the branches
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Magnetism
SPS 10c: Investigate applications of
magnetism and/or its relationship to the
movement of electrical charge as it relates
to electromagnets; simple motors; and
permanent magnets.
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Magnetism
SPS 10c: Investigate applications of magnetism and/or its
relationship to the movement of electrical charge as it relates to
electromagnets; simple motors; and permanent magnets.
• Magnetism is a universal force like gravity.
• A magnet always has two poles - north and
south.
• Like poles repel each other and opposite poles
attract.
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Temporary Magnet vs.
Permanent Magnet
Temporary Magnet
• Has magnetic properties for
a short time.
• Ex: electromagnet
Permanent Magnet
• A magnet that maintains its
magnetic properties forever.
• Ex: magnetite and
lodestone
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Electromagnetism
• Electricity can produce a magnetic field and magnetism can
produce an electric current.
• An electromagnet is a temporary magnet.
• As long as there is a current flowing, a magnetic field is present.
• A simple electromagnet consists of a
– battery,
– copper wire
– iron nail
• The strength of the electromagnet depends on:
– the number of turns in the wire coil
– and the size of the iron core
– The amount of voltage.
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Electrical Machines
Motor
• Converts electric energy to
mechanical energy
• Ex: battery, drill
Generator
• Converts mechanical energy
to electrical energy
• Ex: windmill, turbine
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EOCT Review
Chemistry
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Section 5: Properties of Matter
SPS2. Students will explore the nature of matter, its
classifications, and its system for naming types of matter.
SPS 5. Students will compare and contrast the phases of matter
as they relate to atomic and molecular motion.
SPS 5a. Compare and contrast the atomic/molecular motion of
solids, liquids, gases and plasmas.
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Physical Properties and Changes
Physical Property
Characteristic that can be
observed or measured using the
5 senses.
Physical Change
Change in the form of
matter but not in identity.
Density
Shape
Color
Odor
Texture
Viscosity
Conductivity
Malleability
Hardness
Melting and Boiling Points
Phase changes
(melting, freezing)
Beating an egg
Stirring milk
Bending wire
Folding a paper
Crushing sugar
Dissolving
Slicing a tomato
Boiling water
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Density
• Density is a measure of
the amount of mass in a
certain volume.
• The heavier an object,
the more dense it is.
• This physical property is
often used to identify
and classify substances.
• It is measured in g/cm3.
m
d v
• SAMPLE PROBLEM:
What is the density of a
billiard ball that has a
volume of 100 cm3 and
a mass of 250 g?
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Chemical Properties and Changes
Chemical Property
Way a substance reacts with
another substance to produce a
new substance
Reactivity
Flammability
Combustion
Fermentation
Oxidation
Corrosion
Chemical Change
Occurs when a substance
reacts and forms one or more
new substances
Baking a cake
Mixing baking soda and vinegar
Burning a candle
Iron rusting
Making wine
Milk souring
Banana ripening/rotting
Digestion
Breathing
Evidence of chemical change:
1. change in color
2. production of a gas
3. formation of precipitate 55
States (Phases) of Matter:
SPS 5a. Compare and contrast the atomic/molecular motion
of solids, liquids, gases and plasmas.
Common
States of
Matter
Volume Shape Molecular
Attraction
Examples
Solids
yes
yes
strong
Gold, silver,
carbon
Liquids
yes
no
medium
Gases
no
no
weak
Mercury,
bromine
Nitrogen,
hydrogen,
oxyygen
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States of Matter
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Phase Change
• Label the phase changes below. Tell which
reactions are endothermic and which are
exothermic.
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Gas Laws
Factors that affect Gas
Pressure
1. Temperature
a) Increase in temperature
increases pressure.
2. Volume
a) Decrease in volume
increases pressure
3. Number of particles
a) Increase in the number of
particles increases
pressure.
3 Gas Laws
1. Charles’s Law (pressure)
2. Boyle’s Law (temperature)
3. Gay- Lusaac (volume)
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Gas Laws
SPS 5b. Relate temperature, pressure, and volume of gases
to the behavior of gases
.
Charles Law- When Pressure is constant,
temperature and volume are directly
proportional.
Boyle’s Law
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Gas Laws
SPS 5b. Relate temperature, pressure, and volume of gases
to the behavior of gases
.
Boyle’s Law- When Temperature is constant,
pressure and volume are inversely (opposite)
proportional.
Boyle’s Law
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Gas Laws
SPS 5b. Relate temperature, pressure, and volume of gases
to the behavior of gases
.
Gay Lusaac’s Law- When volume is constant,
pressure and temperature are directly
proportional.
Boyle’s Law
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Section 6: Atomic Theory and the
Periodic Table
SPS1. Students will investigate our current understanding of the
atom.
a. Examine the structure of the atom in terms of
• proton, electron, and neutron locations.
• atomic mass and atomic number.
• atoms with different numbers of neutrons (isotopes).
• explain the relationship of the proton number to the
element’s identity.
b. Compare and contrast ionic and covalent bonds in terms of
electron movement.
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Structure of the Atom
SPS1. Students will investigate our current understanding of
the atom..
• All matter is made up of atoms.
Subatomic Particle Charge
Location
Size
Proton (p+)
1+
Nucleus
Equal to size
of neutron
Neutron (n)
0
Nucleus
Equal to size
of proton
Electron (e-)
1-
Outside nucleus Smallest
subatomic
particle
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SPS1. Students will investigate our current understanding of the
atom.
a. Examine the structure of the atom in terms of
proton, electron, and neutron locations.
• Protons (+) equals Electrons (-)
• charge) and protons (+ charge) to make the atom
electrically neutral.
Protons(+)
Electrons (-)
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a. Examine the structure of the atom in terms of
atomic mass and atomic number.
• The atomic number of an element is what
distinguishes it from all other elements.
• The atomic number is the number of protons
there are in the nucleus.
• Hydrogen's atomic number is 1.
• Helium's atomic number is 2.
Atomic Number
1
H
Hydrogen
1.0079
Atomic Number
2
He
Helium
4
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a. Examine the structure of the atom in terms of
atomic mass and atomic number.
• The mass number is the number of neutrons
added to the number of protons.
• In other words, the total number of particles
in the nucleus.
Mass Number
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SPS1. Students will investigate our current understanding of
the atom.
-atoms with different numbers of neutrons (isotopes).
• Isotopes are atoms of the same element that have different
numbers of neutrons and different mass numbers.
• To distinguish one isotope from another, the isotopes are
referred by their mass numbers.
hydrogen
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Section 7: Periodic Table
SPS4. Students will investigate the
arrangement of the Periodic Table.
a. Determine the trends of the following:
• Number of valence electrons
• Location of metals, nonmetals, and metalloids
• Phases at room temperature
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Periodic Table
• The Periodic Table is organized into
– Rows (periods)
– Columns (groups)
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Periods- Total of 7
Each row in the table of elements is a period.
•
•
•
•
•
•
•
Elements in period 1 have one energy level.
Elements in period 2 have two energy levels.
Elements in period 3 have three energy levels.
Elements in period 4 have four energy levels.
Elements in period 5 have five energy levels.
Elements in period 6 have six energy levels.
Elements in period 7 have seven energy levels.
Horizontally Into Periods
There are 18 GROUPS
Vertically into Groups
Groups
Each column in the periodic table is called a
group.
• The elements in a group have the same number of
valence electrons.
• Therefore members of a group in the periodic table
have similar chemical properties.
Vertically into Groups
•
•
•
•
•
•
•
•
Elements in group 1 have one valence electron.
Elements in group 2 have two valence electrons.
Elements in group 13 have three valence electrons.
Elements in group 14 have four valence electrons.
Elements in group 15 have five valence electrons.
Elements in group 16 have six valence electrons.
Elements in group 17 have seven valence electrons.
Elements in group 18 have eight valence electrons;
except Helium (2).
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The Periodic Law
Atomic Mass
Atomic Mass Units
The mass of an atom in grams is extremely small.
In order to have a convenient way to compare the
masses of atoms, scientists chose one isotope to
serve as a standard.
• Scientists assigned 12 atomic mass units to the
carbon-12 atom, which has 6 protons and 6
neutrons.
• An atomic mass unit (amu) is defined as one
twelfth the mass of a carbon-12 atom.
Atomic Mass
There are four pieces of information for each element.
1. Atomic number
2. Element symbol
3. Element name
4. Atomic mass
Classes of Elements
What categories are used to classify elements on
the periodic table?
Elements are classified as metals, nonmetals, and
metalloids.
• Elements to the left of the blue stair case line
are metals.
• Elements to the right of the staircase line are
nonmetals
• Elements along the staircase line are
metalloids/semi-conductors.
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Classes of Elements
Metals
The majority of the elements on the periodic
table are classified as metals. Metals are
elements that are good conductors of electric
current and heat.
• Except for mercury (liquid), metals are solids at
room temperature.
• Most metals are malleable.
• Many metals are ductile; that is, they can be drawn
into thin wires.
Classes of Elements
The metals in groups 3 through 12 are called transition
metals. Transition metals are elements that form a
bridge between the elements on the left and right sides
of the table.
• Transition elements, such as copper and silver, were among
the first elements discovered.
• One property of many transition metals is their ability to
form compounds with distinctive colors.
Classes of Elements
Nonmetals
Nonmetals generally have properties opposite to
those of metals.
• Nonmetals are elements that are poor conductors
of heat and electric current.
• Nonmetals have low boiling points–many nonmetals
are gases at room temperature.
• Nonmetals that are solids at room temperature
tend to be brittle. If they are hit with a hammer,
they shatter or crumble.
Classes of Elements
Metalloids
Metalloid elements are located on the periodic table
between metals and nonmetals.
• Metalloids are elements with properties that fall
between those of metals and nonmetals.
• For example, a metalloid’s ability to conduct electric
current varies with temperature. Silicon (Si) and
germanium (Ge) are good insulators at low
temperatures and good conductors at high
temperatures.
Group Names
• Some groups have specific names
–
–
–
–
–
Group 1- alkali metals (most reactive metals)
Group 2- alkaline earth metals
Groups 3-12- transition metals
Group 17- halogens (most reactive nonmetals)
Group 18- noble gases (unreactive)
• Group 1 and Group 17 are the most reactive
elements.
• Group 18, the noble gases, are unreactive.
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