UNIT 5:
THE PERIODIC
TABLE
CHEMISTRY 2014-2015
AGENDA 11/3/14
Today’s Objectives:
- Hand back spectra labs
- Introduction to the Periodic Table
- Periodic Table Activity
HW: Finish the questions from the table
structure activity
Now: Quietly read the unit 5 learning targets,
Highlighting words you may not be familiar with
STRUCTURE OF THE
TABLE
•Using a blank Periodic Table create your own table following
the guidelines in the activity directions.
•Be sure to pay attention to what each section is called.
•Do not answer the questions for this lab yet, we will have
time at the end of the class period to work on the questions.
CRYSTAL LAKE
CENTRAL
NOBEL PRIZE
CONTEST
WE HAVE DISCOVERED
NEW ELEMENTS!!
It is your job to take the data you are given and arrange it in a
way that organizes all of the data.
You will slowly get more information as scientists discover it.
You will have to present your table to the other scientists in
the class upon your final draft, be sure to have a reason for
your setup!!
THE FIRST SET OF DATA
**The elements are named after the famous scientists who
discovered them at The University of Iowa
Element
Symbol
Mass # (Top Right)
Meekeron
Em
30.97
Bernardine
Bp
19.00
Sonntagium
Js
14.01
Baldinic
Mb
79.90
Ballentite
Kb
32.07
Kreiterite
Ck
20.18
Leonardium
Ln
35.45
Olsonium
Om
16.00
Schmiederon
Sh
74.92
Soderlous
Sd
28.09
Element
Symbol
Mass # (Top
Right)
Energy Levels
(Bottom Right)
Meekeron
Em
30.97
3
Bernardine
Bp
19.00
2
Sonntagium
Js
14.01
2
Baldinic
Mb
79.90
4
Ballentite
Kb
32.07
3
Kreiterite
Ck
20.18
2
Leonardium
Ln
35.45
3
Olsonium
Om
16.00
2
Schmiederon
Sh
74.92
4
Soderlous
Sd
28.09
3
Element
Symbol
Mass #
Energy
(Top Right) Levels
(Bottom
Right)
# protons
(Top Left)
Meekeron
Em
30.97
3
15
Bernardine
Bp
19.00
2
9
Sonntagium
Js
14.01
2
7
Baldinic
Mb
79.90
4
35
Ballentite
Kb
32.07
3
16
Kreiterite
Ck
20.18
2
10
Leonardium
Ln
35.45
3
17
Olsonium
Om
16.00
2
8
Schmiederon
Sh
74.92
4
33
Soderlous
Sd
28.09
3
14
Element
Symbol
Mass #
(Top
Right)
Energy
Levels
(Bottom
Right)
# protons
(Top Left)
Valence
electrons
(Bottom
Left)
Meekeron
Em
30.97
3
15
5
Bernardine
Bp
19.00
2
9
7
Sonntagium
Js
14.01
2
7
5
Baldinic
Mb
79.90
4
35
7
Ballentite
Kb
32.07
3
16
6
Kreiterite
Ck
20.18
2
10
8
Leonardium
Ln
35.45
3
17
7
Olsonium
Om
16.00
2
8
6
Schmiederon
Sh
74.92
4
33
5
Soderlous
Sd
28.09
3
14
4
OUR PERIODIC TABLE
Is organized so that the properties of elements repeat
themselves in each row.
Mendeleev was able to predict properties of elements before
they were discovered!!
Can you predict the properties of an element that would fit in
the hole in your periodic table??
Fake Element
Real Element
Meekeron (Em)
Phosphorus
Bernardine (Bp)
Fluorine
Sonntagium (Js)
Nitrogen
Baldinic (Mb)
Bromine
Ballentite (Kb)
Sulfur
Kreiterite (Ck)
Neon
Leonardium (Ln)
Chlorine
Olsonium (Om)
Oxygen
Schmiederon (Sh)
Arsenic
Soderlous (Sd)
Silicon
Element
Fake
Symbol
Mass #
Orbital
Shells
# protons
Valence
electrons
Phosphorus
Em
30.97
3
15
5
Fluorine
Bp
19.00
2
9
7
Nitrogen
Js
14.01
2
7
5
Bromine
Mb
79.90
4
35
7
Sulfur
Kb
32.07
3
16
6
Neon
Ck
20.18
2
10
8
Chlorine
Ln
35.45
3
17
7
Oxygen
Om
16.00
2
8
6
Arsenic
Sh
74.92
4
33
5
Silicon
Sd
28.09
3
14
4
AGENDA 11/4/14
HAPPY ELECTION DAY
Today’s Objectives:
- Recap Yesterday
- What are metals and non-metals?
- Begin analyzing the Periodic Table
Now: Take out your homework from last night
OUR ROADMAP TO THE CHEMICAL WORLD
•Where are the transition metals located?
•Where are the metalloids located?
•Where are the Non-metals located?
•Where are the Metals located?
Important Properties of…
Metals:
Non-Metals:
STRUCTURE AND REGIONS
Metals
•
Largest region – left of staircase
•
Solids (except Hg)
•
Conduct heat/electricity
•
Luster
•
Ductile (stretchable)
•
Malleable (able to be flattened)
STRUCTURE AND REGIONS
• Non-metals
– Right of staircase
– Solids, liquids,
gases
– Low conductivity
(heat and
electricity)
– Low luster
– Brittle solids
STRUCTURE AND REGIONS
Metalloids/Semi-Metals
•On staircase
•Share properties of
metals and nonmetals
•Semi-conductors
SOME VOCAB YOU NEED TO KNOW
Family/Group
Period
BLAST FROM THE
PAST!!!
Write the electron configuration for:
• Li
• Na
• K
• Do you notice a trend?
• As you go down a family/group, each element gains an energy
level.
AGENDA 11/5/14
Today’s Objectives:
- Review P.T. Basics
- Learn the Trends of the Periodic Table
HW: Complete note review of periodic trends
Now: Discuss with your neighbors about the answer
to yesterday’s homework question!
THE SHIELDING EFFECT
The ability/tendency of lower energy
level electrons to “shield” outer
electrons from the pull/attraction of
protons in the nucleus.
Which would show a greater
“Shielding Effect”?
GREATER SHIELDING
Having a greater shielding effect means that the outer
electrons are not as attracted to the nucleus.
Remember our holding hand demo…
ATOMIC
SIZE/RADII
ATOMS INCREASE IN SIZE AS YOU GO FROM TOP TO BOTTOM WITHIN A
FAMILY/GROUP BECAUSE . . .
“Bottom” elements have electrons in higher
principal energy levels ---> greater distance
from the nucleus ---> more levels means
larger atom!
Plus, each successive element in a group
exhibits a greater shielding effect!! Outer
electrons feel only a weak pull from the
nucleus!
ATOMS DECREASE IN SIZE AS YOU GO FROM LEFT TO RIGHT ACROSS A
PERIOD BECAUSE . . .
From left to right, successive elements
have more protons & electrons.
However, the “extra” electrons do not
occupy higher energy levels, so there is
no additional shielding effect. With the
“extra” protons, all electrons are pulled
closer to the nucleus!
ATOMIC RADIUS
Greatest Atomic
Radius! (Francium)
Smallest Atomic
Radius! (Helium)
Let’s Recap
What are some properties of Metals?
What are some properties of Non-Metals?
What causes the changes in atomic size within a FAMILY?
What causes the changes in atomic size in a PERIOD?
AGENDA 11/6/14
Today’s Objectives:
- Review P.T. Basics
- Discuss Ions
- Ionization Energy
HW: Forming Ions Homework
Now: Find a partner for an activity
Let’s Recap
What are some properties of Metals?
What are some properties of Non-Metals?
What causes the changes in atomic size within a FAMILY?
What causes the changes in atomic size in a PERIOD?
P.T. REVIEW
2. Vertical columns of elements are called groups/families.
Horizontal rows are called __________.
3. True or False: Elements in the same row tend to have very similar
chemical properties.
4. What is the chemical symbol for the halogen in Period
4?
5. An element’s outermost electrons are found in the 5 th
energy level. The Lewis dot structure for the element
shows four dots. Give the chemical symbol for this
element.
6. Of the elements that have 2 valence electrons, which
has the lowest atomic mass? What family is this
element a part of?
P.T. REVIEW
2. Vertical columns of elements are called groups/families.
Horizontal rows are called periods.
3. True or False: Elements in the same row tend to have very
similar chemical properties. False! Elements in the same
column have very similar chemical properties!
4. What is the chemical symbol for the halogen in Period 4? Br
5. An element’s outermost electrons are found in the 5 th energy
level. The Lewis structure for the element shows four dots.
Give the chemical symbol for this element. Sn
6. Of the elements that typically form ions with a +2 charge, which
has the lowest atomic mass? What family is this element a
part of? Be; part of Alkali Earth metals
REACTIVITY
METAL REACTIVITY
•Metals react by losing electrons.
•Would it be easier to lose an electron
from a smaller or larger atom??
• Think about the shielding effect.
REACTIVITY INCREASES AS YOU GO
DOWN A GROUP OF METALS. WHY?
SHIELDING EFFECT! LOWER ELEMENTS HAVE
ELECTRONS FURTHER FROM THE NUCLEUS WHICH ARE
LESS FIRMLY HELD AND THEREFORE MORE EASILY
LOST.
REACTIVITY DECREASES AS YOU GO
LEFT TO RIGHT IN A ROW OF METALS.
WHY?
Successive elements have more protons, but no “new” energy
levels for electrons. “Extra” protons hold the electrons more
tightly (helps that there’s no added shielding effect!).
TREND #2: REACTIVITY
THE MOST REACTIVE METALS TEND TO BE
LOCATED IN THE LOWER LEFT HAND
CORNER OF THE PERIODIC TABLE. WHY?
METALS REACT BY LOSING ELECTRONS. THE EASIER
IT IS TO LOSE ELECTRONS, THE MORE REACTIVE THE
METAL.
REACTIVITY OF METALS
Most Reactive
Metal!! (Francium)
THE MOST REACTIVE
METALS
https://www.youtube.com/watch?v=m55kgyApYrY
AGENDA 11/6/14
Today’s Objectives:
- Review P.T. Basics
- Discuss Ions
- Ionization Energy
HW: Forming Ions Homework
Now: Find a partner for an activity
One answers, one explains…
WHICH HAS THE SMALLER ATOMIC
RADIUS?
NA OR S ??
One answers, one explains…
WHICH EXHIBITS THE GREATER
SHIELDING EFFECT?
F OR I ??
One answers, one explains…
WHICH IS THE LARGER PARTICLE:
N OR A S ???
One answers, one explains…
WHICH IS THE MOST REACTIVE:
RB OR SR ???
One answers, one explains…
WHICH HAS 2 VALENCE ELECTRONS:
HE OR CA ???
IONIZATION
ENERGY
The ability for an atom to gain or lose an electron.
The ability for an atom to become an ion.
METALS V. NON-METALS
•Metals
• Lose electrons in order to become an ion
•Non-metals
• Gain electrons in order to become an ion
Would a smaller atom or a larger atom be able to attract an
electron better?
Would a smaller atom or a larger atom be able to release an
atom easier?
Generally, ionization energy decreases from
top to bottom within a family because….
SHIELDING INCREASES SO THE ELECTRONS ARE
ATTRACTED LESS STRONGLY!
Generally, ionization energy increases from
left to right across a period because….
EXTRA PROTONS IN NUCLEUS ATTRACT THE VALENCE
ELECTRONS MORE STRONGLY!
IONIZATION ENERGY
Highest
I.E.
(Helium)
AGENDA 11/7/14
Today’s Objectives:
- Electronegativity Trend
- Review all other trends
- Reactivity Demo
COLLECT FORMING IONS
HW: Trends Packet
Now:Take out your Forming Ions Homework
ELECTRONEGATIVITY
The ability for an atom to attract an electron.
Can a smaller or larger atom attract an electron better?
Think about shielding effect.
Generally, electronegativity tends to
decrease from top to bottom in a group
because….
AS THE SIZE OF THE ATOM INCREASES, THE PULL OF
THE NUCLEUS IS LESS STRONG
Generally, electronegativity tends to
increase from left to right in a row
because….
THE ARE MORE PROTONS IN THE NUCLEUS BUT THE
SAME NUMBER OF ENERGY LEVELS.
ELECTRONEGATIVITY
Highest
Electronegativity
(Fluorine)
Note: Noble gases will
not attract extra
electrons!!
AGENDA 11/10/14
Today’s Objectives:
- Review the periodic trends
- White board review activity
- Periodic Table History Web Quest
HW: Unit 5 Review Packet due Wednesday
Now: Take out your homework from this weekend
BECOME THE EXPERT
1. You and your table will select a trend to become the
expert on.
2. It is your job to study this trend from your notes and
prepare a 2-3 minute presentation on your trend to the
class.
3. You may use a whiteboard to organize your presentation.
4. Your presentation should include:
1. Definition of the trend
2. How the trend changes on the PT
3. How does the shielding effect or atomic size relate to your
trend.
4. What is an example question that could be asked on a
test about your trend?
The trends are…
1. Reactivity of Metals
2. Ionization Energy
3. Electronegativity
4. Atomic Radius
5. Shielding Effect
DURING PRESENTATIONS…
1. Add to your notes from in class.
2. Think about questions you might have
about this trend for the group.
3. Work out the problems on a separate
sheet of paper to turn in for credit.
HISTORY OF THE
PERIODIC TABLE
•Work in groups to answer the questions about each
scientist.
•This document will serve as your notes for this portion of
the unit.
•You are accountable to your classmates!
ACC CHEM 3/13/14
Today’s Objectives:
- Study for test tomorrow
H.W. Study for test tomorrow