Unit 4
The Incredible
Periodic Table
Today…
• Turn in:
–Get out PT Basics Poster
• Our Plan:
–PT Basics Questions with group
–Introduce Personal PT Project
• Homework (Write in Planner):
–Personal PT Project
• Choose topic and how to organize
Block
A B C D F
Ave
High
Score
1 5 3 5 5 4 74 96
2 6 2 5 4 5 74 94
5 1 5 4 5 6 66 94
6 8 3 9 5 3 77 100
TOTAL
22% 14% 25% 20% 19%
Daily Challenge
• PT Basics Inquiry Activity
–Answer the questions on the
back of your PT Basics Handout
with your group.
–Turn in your poster and your
questions when finished.
Wrap Up
• As a group, come up with 3 things
that you learned today about the
Periodic Table and be prepared to
share.
Today…
• Turn in:
–Nothing
• Our Plan:
–Work on your Personal Periodic Table
–Wrap Up – Questions about project?
• Homework (Write in Planner):
–Personal PT Project – due Monday
• Don’t forget a title and key!
Wrap Up
•What questions do
you have about your
Periodic Table
project?
Today…
• Turn in:
– Periodic Table Project
• Our Plan:
– Crash Course Video
– PT Card Sort
– Alphabet Brainstorm
• Homework (Write in Planner):
– Stop the Process due NEXT class
Crash Course on the
Periodic Table
• http://www.youtube.com/watch?v=0RRVV
4Diomg
• First 5 minutes
Game Time
• In your team of 3 or 4, complete
the Periodic Table Card Sort and
complete the worksheet as a
team.
• Be sure to follow the
requirements in the instructions
for how many things you have to
list.
Activity Discussion
•
•
•
•
Where are the metals?
Where are the nonmetals?
Where are the metalloids?
What do things in a column have in
common?
• What do things in a row have in
common?
• What is the trend in size?
• What is the trend in reactivity?
Wrap Up
• Alphabet Brainstorm – as a
group of 4, come up with one
word for each letter of the
alphabet that relates to the
Periodic Table. Don’t forget to
look at the Word Wall!
Homework
• Complete p. 3 of your notes by
next class. Read your textbook to
answer the questions.
Today…
• Turn in:
– Get out Stop the Process
– Grade Reflections
• Our Plan:
– PT Puns
– Notes/Label Your PT
– Family Sort/Crossword Puzzle
– Wrap Up – Family Clicker Review
• Homework (Write in Planner):
– Family Sort/Crossword Puzzle due next class
Modern Periodic
Table
• The table is called the
“Periodic Table” because
elements have similar
properties that occur
periodically.
Periods
• Rows (left to
right) are called
periods.
• All of the
elements in a
period have the
same number
of energy levels.
Periods Relate to
Atoms
• As we increase the atomic
number, the electrons fill the
energy levels
• Energy levels are labeled K,
L, M, N, O, P, Q (or 1-7)
1. Label on your PT
Label Your PT
Energy Levels
GROUPS
• The columns (top to
bottom) of the periodic
table
GROUPS
• The elements in a group have the
same number of valence
electrons.
• Valence electrons are the
electrons found in the outermost
energy level of the atom
• They are VERY important to
bonding and reactions!
GROUPS
• Every element in the first
column (Group 1) has one
electron in its outer shell. Every
element in the second column
(Group 2) has two electrons in
its outer shell. ETC.
2. Label the group #s and
valence electrons
Label Your PT
Symbols on the PT
19
K
39.1
Atomic
Number=
number of
protons
Symbols on the PT
19
K
39.1
Symbol
Symbols on the PT
19
K
39.1
Average Atomic
Mass= average
mass of the
naturally
occurring
isotopes
Let’s Label the PT
3. Oxidation Number = charge
– Relates to how many electrons
needed to become stable
– To become stable an atom
wants 8 electrons (THE OCTET
RULE)
– “Eight is great, except for
hydrogen and helium, 2 will do”!
Label Your PT
Let’s Label the PT
4. Multivalent= elements with 2
or more possible charges
+1 only = Ag
+1, +2 = Cu, Hg
+2, +3 = Cr, Ni, Fe, Co
+2, +4 = Pb, Sn
Label Your PT
Let’s Label the PT
5. Diatomic Molecules
– Atoms that exist in nature as pairs
– Only diatomic when ALONE!
H2, O2, Cl2, I2, N2, F2, Br2
Label Your PT
Let’s Label the PT
6. Metals, Nonmetals, & Metalloids
Type
Location
Properties
Metals
Left-side PT
(80% of elements)
Shiny, malleable, ductile, good
conductor of heat & electricity
Nonmetals
Upper Right
Corner
Colorless, gases @ room
temp, Poor conductors
Metalloids
Stair-Step Line
Properties of both metals
& nonmetals,
semiconductors
Label Your PT
Groups
• Group 1: Alkali
Metals
–Most reactive
metals
–Do not occur in
nature
–Very soft
–Explode in Water
Groups
• Group 2:
Alkaline Earth
Elements
–Very reactive
–Not found in
nature
Groups
• Group 3-10: Transition
Metals
–Unreactive – used in
coins and jewelry
–Electrons they use to
bond are in more
than one energy
level(MULTIVALENT)
–Iron, Cobalt, and
Nickel are Magnetic
Groups
• Metalloids
–On the stair-step line
–Properties of metals &
non-metals
–Semiconductors
Groups
• Group 17: Halogens
–Most reactive non-metals
–Exist as all three states of
matter at room temperature
–Compounds with them are
called “salts”
Groups
• Group 18: Noble Gases
–Contain 8 electrons in
outer shell (oxidation # 0) =
stable
–Unreactive
Groups
• 57-71: Lanthanides
• 89-103: Actinides
–Most are synthetic, or manmade
–Actually in Period 6 & 7
–Actinides are Radioactive
Assignment Time…
• Complete the
Family Sort
and the
Crossword
Puzzle. It is
due next class!
Wrap Up
• Family Clicker Review
Today…
• Turn in:
– Crossword/Family Sort – basket
• Our Plan:
– Crash Course Review
– Clicker Review
– Notes – Trends
– Periodic Trends War
• Homework (Write in Planner):
– Nothing
Quick Crash Course Review
• 5 – 7 minutes
• http://www.youtube.com/watch?v=0RRVV
4Diomg
Periodic Trends
•Activity Series of
Metals - Reactivity
increases right to left
and top to bottom
•Most reactive = Fr
Why?
• The further to the left and
down you go, the easier it is
for electrons to be given or
taken away
Periodic Trends
• Activity Series of
Nonmetals - Reactivity
increases left to right and
bottom to top
• EXACT OPPOSITE
• Most Reactive = F
Why?
• The farther right and up you
go, the stronger the element
can “grab” other electrons
or bond
Atomic Radii
• Calculated by finding
1/2 the distance
between the 2 nuclei
of 2 atoms of the
element when joined
Period Trend
• Atomic Radius DECREASES as
you go left to right across a period
• Why?
– Determined by the strength of the attraction
between the nucleus and the outermost
electrons (protons “suck” the electrons in)
– Stronger the attraction, smaller the size of atom
– More Protons = More Nuclear Attractive Force
Group Trend
• Atomic Radius INCREASES as you
go down a group
• Why?
–There is a significant jump in the
size of the nucleus (protons &
neutrons) as well as the number of
electron energy levels
Ions
• An atom or group of atoms with a
positive or negative charge.
• Form when electrons are
transferred between atoms
–Cation – positive charge (Ca+2)
–Anion – negative charge (N-3)
Ionization Energy
• Energy required to
remove an electron from
the neutral atom to form
a positively charged ion
(cation)
Period Trend
• Ionization Energy INCREASES as you
go from left to right across a period
• Metals (left) WANT to get rid of their
electrons, therefore it doesn’t take
much energy to ionize
• Non-metals (right) DO NOT WANT to
give away electrons, therefore it takes
more energy to ionize
Group Trend
• Ionization Energy DECREASES as you go
down a group
• Why?
– Shielding Effect - Caused by an
increasing number of electrons between
the outer level and the nucleus
– Blocks the attraction of the nucleus for
the electrons
– Causes large atoms to lose their
electrons more freely
Ionization Energy
•Ionization energy
relates to activity of
metals & non-metals
• The highest ionization energy = the
most active non-metal (Fluorine)
• The lowest ionization energy = the
most active metal (Francium)
Ionization Energy
• As each electron is
removed, the ionization
energy increases
• Large jumps of energy
indicate a removal of an
electron from a new shell
Example
• For Na the IE for each
successive electron are 496
kJ/mol, 4562 kJ/mole, 4912
kJ/mol, and 5544 kJ/mol.
How many valence
electrons does Na have?
Example
496 kJ/mol
4562 kJ/mol
4912 kJ/mol
5544 kJ/mol
Large jump in
energy here,
therefore there is
only one valence
electron
Ionic Size
• Cations are always SMALLER
than the atoms from which
they form
• Anions are always LARGER
than the atoms from which
they form
Ionic Size
Electronegativity
• Ability of an
atom to
attract
electrons
when it
makes a
compound
Electronegativity
• Discovered
by Linus
Pauling
• He won the
Nobel Prize
for his work
Period Trend
• Electronegativity INCREASES as you
go left to right across a period
• WHY?
– Elements on the left side have 1-2 valence
electrons that they would rather give away than
“grab” another element’s electrons, so they
have low electronegativity
– Elements on the right side only need a few
electrons so they want to “grab” another atom’s
electrons giving them a high electronegativity
Group Trend
• Electronegativity DECREASES as
you go down a group
• Why?
– Elements near the top of the PT have few electrons
to begin with so they have a stronger desire to
acquire more electrons (higher electronegativity)
– Elements near the bottom have so many electrons
already, that gaining or losing an electron is no big
deal (lower electronegativity)
Summary of Trends
Periodic Trends Music Video
• http://www.youtube.com/watch?v=MGTKV
aZcq8Y&feature=related
Periodic Trends War
• You will play “War” with your face partner.
1. Deal out all of the cards so that each of you have
half. Keep the cards in a pile face down.
2. Each player will play their top card. The element that
is greatest for that trend wins both cards. After
going through your deck mix them up and then
continue play. Every 3 minutes we will switch
trends.
3. The game ends when one person runs out of cards.
If that doesn’t happen in the time allotted, the winner
is the person with the most cards at the end.
Trends War
• Atomic Radius
• Electronegativity
• Ionization Energy
• Valence Electrons (if tie play
next card and winner gets all)
• Reactivity (if it is a metal and a
nonmetal the metal wins)
Today…
• Turn in:
– Grab a clicker and pull out your lab
• Our Plan:
– PT Worksheet Race
– Periodic Trends Lab
– Test Review
– Clicker Review
– Exit Slip
• Homework (Write in Planner):
– Test Review Due next class
– TEST NEXT CLASS
Alkali Metals in Water
Cesium & Rubidium Bathtub
Wrap Up – write on sticky note
or index card and give to Mrs. C
on your way out…
On the Periodic Table, observe the locations
of the following elements:
Li, Ca, Co, Cl, Br, Cs
1.
2.
3.
4.
Which element is the most reactive metal?
Which element is the most reactive nonmetal?
Which element is the biggest?
Which element has the greatest
electronegativity?
5. Which element has the smallest ionization
energy?
The Answers
1.Cs
2.Cl
3.Cs
4.Cl
5.Cs
Today…
• Turn in:
– Get out test review to check
• Our Plan:
– Station Review
– Questions on Test Review
– Unit 4 Test
– Fill out Goal Sheet (except test)
– Sodium Party Reading/Video
• Homework (Write in Planner):
– Sodium Party Reading (due next class)
Sodium Party Video
• http://periodictable.com/Stories/011.2/inde
x.html