The 4 Modern States of Matter
Animation
Tutorial
 Matter can take four states:
The states of matter and  Solid
their properties can be
○ Solid is the state in which
defined and explained by
matter maintains a fixed
volume and shape.
the motion of particles,
(atoms and molecules). The  Liquid
○ liquid is the state in which
explanation is called
matter maintains a fixed
Kinetic Molecular Theory.
volume but adapts to the
shape of its container
 Gas
○ Gas is the state in which
matter expands to occupy
whatever volume is available.
 Plasma
○ Plasma can be considered
highly ionized particles that
have distinct properties, so
that it is usually considered as
a different phase or state of
matter
Definitions from wikipedia
Another animation
Changing States of Matter
The three states of matter that are most
often studied are gas, liquid, and solid.
A fourth state of matter, plasma, which is
much hotter (more energetic) than gas is
included here.
Notice that plasma can only be formed
from a gas which is ionized (changed
into charged particles).
To make a change from one state of matter
requires a change in energy.
For example, the change form the
liquid state to a gas is called
vaporization.
The amount of energy (heat) needed
to make this change is called the
enthalpy (heat) of vaporization.
Since the gas state of matter is hotter than
is the liquid state, enthalpy of vaporization is
the amount of heat that must be added to
the liquid for it to change into a gas.
Slide by: J. Levasseur ©
Phase Change Animation
•Name the four states of matter?
•What states of matter are fluid,
can flow?
•Which state of matter has the
strongest bonds between particles?
•Which states of matter have no
bonds between particles?
•Which state of matter is the most
energetic?
•Which state of matter has the least
amount of heat?
•What is enthalpy?
•How are temperature, energy and
state of matter related?
•Define: sublimation, deposition,
melting, freezing, evaporation,
condensation, ionization,
deionization.
Movie
http://scienceprojectideasforkids.com/2009/states-of-matterenthalpy/ by J VanCleave
Kinetic Molecular
Theory
• The Kinetic-Molecular
•What("the
is kinetic
Theory
theory of
Molecular
Theory?
moving
molecules)
•How does Kinetic
• The
Kinetic Molecular
Molecular
theory
Theorythe
is based
on of
the
explain
behavior
idea that
particles of
gases?
matter
are is
always
• What
the in
relationship
motion. between a
gases’ volume, theory
• Kinetic-molecular
pressure an
can be used to explain
temperature?
the
properties of solids,
•Why is more energy
liquids and
gases
in
required
to turn
liquid
terms
of the
energy
water into
a gas
than
particles
and the(Hforces
other molecules
2S
thatfor
actexample)?
between them.
Assumptions of Kinetic Molecular Theory
1.
2.
3.
4.
5.
6.
Gases are composed of a large number of particles that
behave like hard, spherical objects in a state of constant,
random motion.
These particles move in a straight line until they collide with
another particle or the walls of the container.
These particles are much smaller than the distance between
particles. Most of the volume of a gas is therefore empty
space.
There is no force of attraction between gas particles or
between the particles and the walls of the container.
Collisions between gas particles or collisions with the walls of
the container are perfectly elastic. None of the energy of a
gas particle is lost when it collides with another particle or
with the walls of the container.
The average kinetic energy of a collection of gas particles
depends on the temperature of the gas and nothing else.
Solid
Liquid
Gas
Animation
Tutorial
Video Part 1 on Atoms
Video Part 2 on Atoms
Atomic Structure and
Nuclear Chemistry
Springfield Central High School
Chemistry
Slide by: J. Levasseur ©
John Levasseur
levasseurj@sps.springfield.ma.us
centralscience.net
MA State Frameworks
2. Atomic Structure and Nuclear Chemistry
• Central Concepts:
– Atomic models are used to explain atoms and help us understand the interaction of
elements and compounds observed on a macroscopic scale.
– Nuclear chemistry deals with radioactivity, nuclear processes, and nuclear properties.
– Nuclear reactions produce tremendous amounts of energy and lead to the formation
of elements.
•
•
•
•
•
•
•
2.1 Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of atom), and understand how each discovery leads to
modern theory.
2.2 Describe Rutherford’s “gold foil” experiment that led to the discovery of the nuclear
atom. Identify the major components (protons, neutrons, and electrons) of the nuclear atom
and explain how they interact.
2.3 Interpret and apply the laws of conservation of mass, constant composition (definite
proportions), and multiple proportions.
2.4 Write the electron configurations for the first twenty elements of the periodic table.
2.5 Identify the three main types of radioactive decay (alpha, beta, and gamma) and compare
their properties (composition, mass, charge, and penetrating power).
2.6 Describe the process of radioactive decay by using nuclear equations, and explain the
concept of half-life for an isotope (for example, C-14 is a powerful tool in determining the age of
objects).
2.7 Compare and contrast nuclear fission and nuclear fusion.
Slide by: J. Levasseur ©
The Atom •
The Basic Model of an Atom
– Atoms- tiny units of mass that take up space; these
units determine the properties of matter. These
tiny units have no net charge having equal positive
protons and negative electrons.
– The atom consists of two regions.
1.
The nucleus
•
•
2.
Protons
Neutrons
Energy levels (electron clouds)
• Electrons
• Specific amounts of energy
Slide by: J. Levasseur ©
Animation
Tutorial
Animation
The Atom’s Nucleus
• Protons are positively charged
subatomic particles found in the
nucleus
Protons are positively
charged subatomic
particles found in the
nucleus
– The number of protons in an atom will
 Neutrons have no net
charge and allow the
determine what type of element.
positively charged protons
– The atomic number of an element is the
to be tightly packed into
number of protons in that element’s atoms’ the nucleus
nuclei
• Neutrons are particles with no net
charge and found in the nucleus
Slide by: J. Levasseur ©

•What are atoms?
•What are protons, neutrons
and electrons?
•What is he nucleus of an
atom?
•What makes one kind of
atom, (element) different
from another?
•What is the “Strong Force,
and why is the Strong Force
an example of E=mc2?
The Atom’s Electrons (e-)
• Electrons are negatively
charged subatomic particle
found in discrete energy levels
around the atom’s nucleus .
– Electrons are found in the outer
regions surrounding the nucleus
called energy levels also known
as energy shells.
• The outermost energy level is
called the valence level.
– The electrons found in the
valence level is called the
valence electron.
– The number of valence electrons
determine the chemical
reactions of the element.
– How an atom behaves when it
encounters other atoms is
determined by valence
electrons.
Slide by: J. Levasseur ©
•What are electrons?
•What is the valence level in an
atom?
•How do electrons determine the
behavior of groups of the periodic
table?
•How many valence electrons
does each of the following atoms
have: Na, B, Si, Sb, Br, Kr, K, C, He
• Avogadro’s Number
Knowing the Animation
mole
– • Avogadro’s
number
isfor
thechemicals
number
The Mole
isvalue
a counting
word ofis
• The Mole
particles
exactly
mole
of axpure
with ainvalue
of one
about
6.02
1023
the
key
to
– The mole is the SI unit for amount of
• substance.
Think of other
counting words
understanding
so in
23
substance.
– 6.022
1415 × 10many
English
other values
– A mole (abbreviated mol) is the amount
– Pair = 2 that you can measure
of a substance that contains as many
– Dozen = for
12 in a lab.
particles as there are atoms in exactly 12
– Gross = 144
g of carbon-12.
– Grand = 1000
– There are 6.022 1415 × 1023 atoms
– Mole = 6.02 x 1023
in exactly 12 g of carbon-12.
What –isThere
a Mole?
are approximately 6.02 x 1023 • 6.02 x 1023 (mole) is such an
• The Mole
important number it was given a
carbon atoms in 12 grams of carbon
– The mole is the SI unit
for
name, Avogadro’s Number
23
• So a Mole is 6.02 x 10 particles, (atoms,
amount of substance.
– Avogadro was a famous
molecules, formula units, protons, ect)
– A mole (abbreviated mol)
Italian chemist
• Avogadro’s Number
is the amount of a
23 is often
–
So,
6.02
x
10
•substance
Avogadro’s
the number of
thatnumber
containsis as
referred to as Avogadro’s
particles
in
exactly
one
mole
of
a
pure
many particles as there
Number.
substance.
are atoms in exactly 12 g
• Like 3.14 is often referred to
•of carbon-12.
6.022 1415 × 1023
as Pi
What is a Mole?
Animation
Central Concepts
Atomic Mass & Molar Mass
• Atomic Mass
– When you look at a Periodic Table, the
numbers under the element symbols are
the relative atomic weights.
Tutorial
Slide by: J. Levasseur ©
• For example, notice helium and neon,
it shows that neon is basically 5 times
heavier (20.1797/4.00260). If we
compare helium to carbon, we see that
carbon is about 3 times heavier
(12.0107/4.00260)
– These are relative weights, but if we
count out a mole of these atoms, then
these numbers is the weight in grams . In
other words, a mole of sulfur weighs
32.066 grams
• Molar Mass
– The mass of one mole of a pure
substance is called the molar mass of that
substance.
– Molar mass is usually written in units of
g/mol.
– The molar mass of an element is
numerically equal to the atomic mass of
the element in atomic mass units.
Solving a Grams per Mole Problem with
the This per that triangle
.
If you have 880 grams of
Calcium (Ca), how many
moles of Calcium do you
have?
 What is the “This”?
 What is the “That”?
 What is the “This per That”?
 How do you find the molar
mass of Ca?
880
This
grams
40
This per That
g/mol
22
That
?
mol
We know the “This” is 880 grams
 We can look up Calcium on the periodic table and find out
the molar mass is 40 g/mol
 So we can solve for the number of moles.

Solving a Grams per Mole Problem with
the This per that triangle
.
If you have 883.5 grams of
Cobalt (Co), how many moles
of Cobalt do you have?
 What is the “This”?
 What is the “That”?
 What is the “This per That”?
 How do you find the molar mass
of Co?
883.5
This
grams
58.9
g/mol
This per That
That
1
? 5 mol
We know the “This” is 883.5 grams
 We can look up the molar mass of Co and find out the it is
58.9 g/mol
 So we can solve for the number of moles.
How many moles of cobalt (Co) are in 353.4 grams of cobalt?
How many moles of Indium (In) are in 430.5 grams of In?
 What is the mass of 10 moles of cobalt ?
What is the mass of 7.5 moles of Indium?

Slide by: J. Levasseur ©
Next Problem: Grams per mole
5.3
• You have a sample of .66 moles of Potassium (K), how much should your
sample weigh?
What is the mass of
• What is the “This” in our Problem?
2.5 moles of Na?
• What is the “That” in our Problem?
How many moles of
• What is the “This per That”?
carbon are there in 66
grams of carbon?
What is the mass of
3 moles of oxygen,
This
(careful HONClBrIF)?
This
per
That
That
.
• Democritus 400 B.C.
– Nothing exists but atoms and empty space,
everything else is opinion
– Atoms Indivisible geometric shapes
• Dalton 1830
History of the
Atomic Theory
– Daltons Atomic Theory
– Ball and Hook Model
• Thompson 1906
– Discovery of subatomic particles: electron and
protons
– Plum Pudding Model from Thompson
• Rutherford 1909
– Electrons orbiting the nucleus like planets around a
star
– Discovery of atomic nucleus
Democritus
– Dense positive nucleus surrounded by negative
electron Rutherford
– Did not obey laws of physics
Dalton
Thompson
• Bohr 1913
– Electron movement by quantum rather than
classical physics
– Electrons have discrete energy levels
– Only works for hydrogen
• Modern Quantum (or orbital) Model 1924
– Schrödinger and Heisenberg
– Electron can not be located
– Estimated location of electron based on
probabilities
1909
Rutherford
Slide by: J. Levasseur ©
Bohr
Schrödinger/
Heisenberg
History of the Atomic Theory: Dalton
• John Dalton’s recognition of atoms
and his Atomic Theory are an
explanation of three Laws in
Chemistry


– 1. The Law of Conservation of Mass
– 2. The Law of Definite Proportions
– 3. The Law of Multiple Proportions
Dalton’s Atomic Theory can be summarized in
5 points:
1.
2.
3.
4.
5.
All matter is made of atoms
Atoms are neither created nor destroyed
Atoms of the same element are identical
Atoms of different elements differ in mass,
shape, size and properties
Chemical reactions involve the rearrangement
in the combinations of atoms in substances
•Dalton’s Atomic Model pictured
atoms as balls and hooks that
can grasp onto or release one
another
•What are the 5 points of
Dalton's Atomic Theory?
Since the time of Dalton new discoveries have shown that Dalton was not
completely correct; however his atomic theory is the foundation of our modern
understanding of atoms.
Discovery of the Law of Conservation of Mass
5.1
• Antoine-Laurent de Lavoisier was a Paris tax
collector who had a passion for scientific
discovery.
– Lavoisier was appointed to the King’s Academy for
science.
– Lavoisier and his wife Marie worked together .
– The Lavoisiers’ great discovery was based on the
fact that rusting iron gains mass rather than losses
mass.
• Lavoisier showed that when water is passed
through a heated rifle barrel some of the
water disappears; however, the mass of the
lost water can be accounted for by the
increased mass of the rifle barrel and the
mass of a new gas that appears, (hydrogen).
• Lavoisier stated that no mass is lost or gained
in chemical reactions, the Law of
Conservation of Mass.
Lavoisier’s conclusion
was that mass is
neither gained nor
lost in a chemical
reaction.
This is known as the
Law of Conservation
of Mass.
The Law of Conservation of Mass
• The Law of Conservation of Mass
• States that mass is neither created
nor destroyed in any ordinary
chemical reaction.
• Or more simply, the mass of
substances produced (products) by
a chemical reaction is always equal
to the mass of the reacting
substances (reactants).
• The law of conservation of mass:
– Lavoisier: No mass is gained or lost in
a chemical reaction
– After Dalton: Atoms are neither
created, nor destroyed, during any
chemical reaction
Example:
5.1
The Law of Conservation of Mass
says that no matter is created or
destroyed in chemical reaction.
From this we know that:
1. All chemical equations MUST
have the same number of
atoms of the different reactant
elements as atoms in the
products.
2. The mass of the reactants
MUST equal the mass of the
products.
This law is the basis of balancing
chemical equations.
– 4g Hydrogen 32g oxygen  36g
water (H2O)
– 1.00g carbon + 5.34g sulfur  6.34g
carbon disulphide
– 2.00g carbon + 10.68g sulfur 
12.68g carbon disulphide
http://www.mi.mun.ca/users/edurnfor/1100/atomic structure/
Discovery of Electron
&
Thomson Atomic Model
• The discovery of the first subatomic particle, the
electron, came from experiments on the effects of
electricity in a cathode ray tube done by J.J.
Thomson.
• A cathode ray tube is a glass tube containing a gas.
• When a paddle wheel was placed in a cathode ray
tube, the wheel spun and rolled from cathode to
anode Thomson hypothesized that a stream of
particles with mass were originating at the cathode
and moving toward the anode caused the glow.
• When exposed to a magnetic field, the cathode ray
was deflected in the same manner as an electric
current, which has a negative charge.
• Thomson based his plum pudding model of the
atom on these findings.
Animation
Animation 2
J.J. Thomson used what tool to discover what
part of the atom?
http://science.jrank.org/pages/620/Atomic-Models-Discovery-electron.html
E. Rutherford and the Gold Foil Experiment
•Rutherford’s new
Note:model
In thehad
gold
atomic
the
foil experiment
negatively
charged
electrons
indefinitely
Rutherford
showed
orbiting
thenucleus
positivelyis
that the
charged nucleus.
a small,
dense and
Know
• positively
According tocharged
the
Rutherford’s
classical
laws of physics
mass in
the center
the experiment
electrons should fall
of the
atom.
into the
nucleus.
Slide by: J. Levasseur ©
• Ernest Rutherford discovered that atoms have a
solid nucleus in 1909
– Rutherford shot alpha particles at gold foil and
discovered some alpha particles bounced back
• He concluded that the alpha particles were hitting a
solid nucleus
• Rutherford postulated a new atomic model
– A model he knew was not correct since it
violated basic laws of physics.
• A new explanation of motion had to made to
explain what was happening inside atoms.
Movie
– The new explanation is called quantum mechanics
Animation
History of the Atomic Theory: Bohr Model
• Niels Bohr concluded in 1913 that electrons
inside atoms are “quantized”
– Quantized means that the electrons have discrete
fixed energy levels.
• This differed from Rutherford because Rutherford
did not see how an orbiting negative electron would
not fall into a positive nucleus based on Newton's
Laws.
• Bohr applied Max Planck’s idea that energy moves in
tiny but discrete bundles at a time
– One bundle is a quanta
• Bohr initially recognized 6 energy levels but as
measuring instruments improved 4 energy levels
were agreed on, the outer three having sublevels.
– Like Rutherford’s, Bohr’s atomic model resembled
the planets’ orbit around the sun.
• However, Bohr’s rings around the nucleus show
levels of energy not pathways of the electrons.
Animation
The Bohr Atomic Model has
four energy levels where
electrons travel about the
nucleus only in these energy
levels or their sublevels;
however, the model does
not state locations of where
electrons are rather the
model shows electron
energy levels.
Color, Light and Energy
• Gas put in tubes then electrified
glows with beautiful colors.
• What is happening?
– The electricity is exciting the electrons in the
atoms of the gas.
– The electrons absorb a certain amount of
energy then jump to higher energy levels; this
is a quantum leap.
– The electrons are most stable in a lower state
closer to the nucleus, so the electron will give
off the same amount of energy that they
absorbed then drop back to a ground state.
– The different elements will glow different
colors because the different elements have
different electron configuration.
• Each electron configuration means a different
amount of energy will be absorbed then
released as a light photon
• Different colors actually represent different
amounts of energy
– Each gas will glow a different color since the
different elements have differing electron
configurations.
The Bohr Model Explains Line Spectra
Energy and Orbitals of Bohr
Model
• The energy levels and the
sublevels correspond to
the energy represented in
the line spectra
• The Bohr model explains
the phenomenon of line
spectra rather than
continuous color because
the difference in energy
between the energy
levels determines color of
light emitted when an
electron moves from one
energy level to another.
Animation
You GOT to see this periodic Table animated
with the spdf levels again and showing the
line spectra for various elements AGAIN
How are the electrons moving around the nucleus?
• Nobody really knows.
– In fact, it's more than that - current theory says that
it is impossible to know.
• If you have planets in orbit around the sun, it is
possible to plot out an orbit for them in
mathematical terms.
• You can't predict locations of electrons.
– To plot an orbit, you need to know, amongst other
things, exactly where the electron is, what direction
it is heading in, and how fast it is going.
• The Heisenberg Uncertainty Principle says you can't
know with certainty both where an electron is and
where it is going next.
• If we can't know these essential facts, then we have
no idea what the electrons are actually doing in the
atom. All we can know about them is:
– Their energy
– Where they most likely are.
•
Any particular electron will be found in a
region of space known as an orbital.
– Each individual orbital can hold 2 electrons
http://www.chemguide.co.uk/atoms/properties/atomorbs.html
Slide by: J. Levasseur ©
Electron Orbitals and the Periodic Table
•
An atomic orbital is a
mathematical function
that describes the wavelike behavior of
electrons in an atom.
• An atomic orbital can
be used to calculate the
probability of finding
any electron of an atom
in any specific region
around the atom's
nucleus.
These functions may
serve as threedimensional graph of
an electron’s likely
location.
• The structure of the
Periodic table can be
understood based on
atomic orbitals
Slide by: J. Levasseur ©
.
http://en.wikipedia.org/wiki/Atomic_orbital
Animation
Atomic Orbitals: The order of filling orbitals
• Electrons fill low energy orbitals (closer
to the nucleus) before they fill higher
energy ones.
Movie
– Where there is a choice between
orbitals of equal energy, they fill the
orbitals singly as far as possible.
Electrons stay as far as they can from
each other.
Helium 1s2
One of the amazing phenomenon with
electron energy levels is that the 3p high
energy sublevel of the third energy level is
more energetic than the 4s low energy
sublevel of the fourth energy level.
This pattern repeats itself and can be seen
on the Periodic Table.
Slide by: J. Levasseur ©
http://www.chemguide.co.uk/atoms/properties/atomorbs.html
Periodic Table, Orbitals & Electron
Configuration
Animation
Slide by: J. Levasseur ©
Practice Writing Electron Configuration Notation
What elements
• 1s1 have the Noble Gas
• Hydrogen........
configurations:
• Helium…......... • 1s• 2[Ar] 4s1
2
• 1s• 2[Kr]
2s2 5p
• Beryllium…..
Does P3- have2 a stable
(noble gas
22p3
•
1s
2s
• Nitrogen...…
configuration?
2
3
– [He] 2s 2p
• Silicon……….
• Sulfur…………
• Argon…….…
•
•
•
1s22s22p63s23p2
– [Ne] 3s23p2
1s22s22p63s23p4
– [Ne] 3s23p4
1s22s22p63s23p6
• Potassium……… • 1s22s22p63s23p64s1
– [Ar] 4s1
• Calcium….
•
1s22s22p63s23p64s2
– [Ar] 4s2
Slide by: J. Levasseur ©
.
Animation
Slide by: J. Levasseur ©
Tutorial
• Radioactivity is the
spontaneous
breakdown of an
atom’s nucleus. This
breakdown of atomic
nuclei releases
certain particles and
energy.
• The breakdown of the
nucleus can change
the atomic mass of an
atom; producing
isotopes.
• The breakdown of an
atom’s nucleus can
also cause
transmutation of the
element.
–One element
becomes another
due to a change in
the atomic number
(the number of
protons)
The Three Radioactive Emissions & Their Penetrating Power
•
Alpha Particles are the largest in size of the
emissions, and consequently has the least
penetrating power.
– Alpha particles are the size of a helium atom's
nucleus.
– Alpha radiation: Is easily stopped by paper, foil, or a
few centimeters of air.
• Beta Particles are smaller, and therefore have more
penetrating power and danger, than alpha radiation.
– Beta particles are the size of an electron, extremely
small.
– Beta radiation is stopped by sheet metal, dense
wood, or heavy clothing.
• Gamma Radiation does not have a "size" because it
is energy and not matter, (matter has mass and
volume, ie. size). Gamma radiation is the most
penetrating and most dangerous radiation.
– Gamma rays pass through most substances easily.
– Blocking gamma radiations takes many centimeters
Animation
of lead or a think wall of concrete.
Slide by: J. Levasseur ©
Animation
Movie
Nuclear Fission and Nuclear Fusion
Fission Animation
Fusion Animation
Fission Reaction
What are alpha
•Nuclear fission is the splitting of a massive nucleus into photons in
the form of gamma rays, free neutrons, and other subatomic particles. decay, beta decay
and gamma decay?
In a typical nuclear reaction involving 235U and a neutron:
If an atom gains a
235 U + n  236 U
92
92
proton but loses no
followed by
236 U  144 Ba + 89 Kr + 3n + 177 MeV
mass, what decay
92
56
36
Fusion
•Nuclear fusion is the reaction in which two or more nuclei combine
together to form a new element with higher atomic number (more
protons in the nucleus).
•The energy released in fusion is related to E = mc 2.
An example is: Deuterium–Tritium reaction. Deuterium and
Tritium are both isotopes of hydrogen.
2 Deuterium + 3 Tritium  4 He + 1 n + 17.6 MeV
1
1
2
0
Slide by: J. Levasseur ©
occurred?
 If an atom loses
two protons and
drops 4 amu, what
decay occurred?
What is the
difference between
fission and fusion?
Movie
Half-Life
Animation
• Half-life is closely related to the
property of Radioactive Decay.
• Half-life represents the time taken
for half the atoms in a radioactive
substances to undergo decay and
change into another nuclear form
– Either a radioactive daughter
product or a stable form.
– Half-life is the time taken for
the breakdown (decay) of a
radioactive sample by half.
– The commonly given the
symbol for Half-life is:
t ½.
Thallium-201 has a half-life of 73 hours. If
Actinium-226
a half-life
of3.66
29 hours.
An isotopehas
ofhas
cesium
(cesium-137)
has aifIf
Radon-224
a
half-life
of
days,
4.0
mg
ofofthallium-201
disintegrates
over
a
100
mg
actinium-226
disintegrates
over
half-life
30
years.
If
1.0
g
of
cesium-137
you
haveofa6.0
50 days
gramand
sample
of Radon-224
period
2
hours,
how
many
a
period
of
58
hours,
how
many
mg
of
disintegrates
over
a
period
of
90
years,
how much
radon-224
will
be
remaining
in
mg actinium-226
of gthallium-201
remain?
willwill
remain?
how many
of 7.32
cesium-137
would
remain?
days?
Slide by: J. Levasseur ©
http://www.ionactive.co.uk/glossary/HalfLife.html
Periodicity
.
Click on circle for
interactive Periodic Table
Springfield Central High School
John Levasseur
Chemistry
levasseurj@sps.springfield.ma.us
centralscience.net
Slide by: J. Levasseur ©
MA State Frameworks
.
3. Periodicity
• Central Concepts:
•
•
•
•
– Repeating (periodic) patterns of physical and chemical properties occur
among elements that define families with similar properties.
– The periodic table displays the repeating patterns, which are related to the
atoms’ outermost electrons.
3.1 Explain the relationship of an element’s position on the periodic table to its
atomic number.
– Identify families (groups) and periods on the periodic table.
3.2 Use the periodic table to identify the three classes of elements: metals,
nonmetals, and metalloids.
3.3 Relate the position of an element on the periodic table to its electron
configuration and compare its reactivity to the reactivity of other elements in the
table.
3.4 Identify trends on the periodic table (ionization energy, electronegativity,
and relative sizes of atoms and ions).
Slide by: J. Levasseur ©
Periodic Table
Internet Tutorial by Karl Loren
•How many protons
does an atom of Zinc
have?
•How many electrons
does an atom of
Sodium have?
•How many neutrons
does an atom of
potassium have?
Animation
Movie
Do you remember how to read the Periodic
Table?
– Each element has an atomic number
based on the number of protons in an
atom of that element
– The elements are arranged by
increasing atomic number
• The horizontal rows of the Periodic table
are known as the periods.
– The horizontal rows of the periodic
Table increase in mass with every
element as you move from left to right.
• Groups on the Periodic Table, (aka Families)
are the vertical columns
– Groups of elements share similar
properties because they share the same
valence electron number
3.1