Download Valence Electrons - Warren County Public Schools

Periodic Table: 4.23.14
Infinite Campus Update:
•“Where do chemical elements come from” article (18pts.)
•Periodic Table Worksheet (10pts.)
•Periodic Table Basics Worksheet (15pts.)
•Electron Configuration Exams (30pts.)
Homework:
•Review electron properties and arrangement notes, review
exam tomorrow.
Periodic Table Objectives
Objectives:
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
•I can distinguish between metallic and non-metallic
properties.
•I can graph and interpret periodic trends.
•I can understand how the periodic table was organized by
Mendeleev and Moseley.
Periodic Table and Valence Electrons
Due:
 E- arrangement and Chemical Reactivity Wksht.
Objectives:
 I can establish a relationship between the periodic
table and valence electrons.

I can establish a relationship between the periodic
table and chemical reactivity.
Periodic Table Objectives
Objectives:
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
•I can predict the charge for an element (ion) to reach
maximum stability.
•I can distinguish between metallic and non-metallic
properties.
•I can understand how the periodic table was organized by
Mendeleev and Moseley.
•I can graph and interpret periodic trends.
•I can illustrate valence electrons using Lewis Dot structures.
Bell Ringer: Periodic Table
1. a. What period and group is sulfur on?
b. What element is in period 6; group 2 ?
2. Give an example of an element from the following
groups:
Noble Gases, Transitional, Alkali, Halogens, Alkaline Earth
3. Circle the elements below that are representative: ,
Na, Cr, Ag, Kr, C, Sn
4. a. What are valence electrons?
b. Determine how many valence electrons each element
below has:
a. H
b. Se c. Sr d. Zn
Bell Ringer: Periodic Table
1. a. What period and group is sulfur on?
b. What element is in period 6; group 2 ?
2. Give an example of an element from the following
groups:
Noble Gases, Transitional, Alkali, Halogens, Alkaline Earth
3. Circle the elements below that are representative: ,
Na, Cr, Ag, Kr, C, Sn
4. a. What are valence electrons?
b. Determine how many valence electrons each element
below has:
a. H
b. Se c. Sr d. Zn
Periodic Table: Organization of Elements
•Groups: Represent columns on periodic table.
•Periods: Represent rows on the periodic table.
Periodic Table and Groups
Transitional Groups:
 Short groups.
Representative Groups:
 Tall groups
Periodic Table and Valence Electrons
Objectives:
 I can establish a relationship between the periodic
table and valence electrons.

I can establish a relationship between the periodic
table and chemical reactivity.
Valence Electron Worksheet
Lewis Dot Structures
•Illustrates
valence electrons
for an atom.
Place electrons (dots) around
the elements symbol using
cardinal direction.
Element
Na
Mg
Do NOT pair electrons
up until you have to.
•
S
# of
valence
electrons
Lewis Dot
Structure
Periodic Table: Arrangement
Valence Electrons:
•Electrons on the highest energy level of an atom.
•Determines chemical stability of an atom.
Common Periodic Table Groups
Periodic Groups
Alkali Metals
Alkaline-Earth
Metals
Transitional
Metals
Halogens
Noble Gases
(Inert Gases)
Group #
Valence
Electrons
Chemical Reactivity
(Yes or No)
Common Periodic Table Groups
Periodic Groups
Alkali Metals
Alkaline-Earth
Metals
Group #
Valence
Electrons
1
1ve-
2
Chemical Reactivity
(Yes or No)
Yes, chemically reactive because they only
has 1 ve-. Most reactive metallic group.
2ve-
Yes , chemically reactive because they only
have 2 ve-.
Yes, chemically reactive because they only
have 2 ve-.
Transitional
Metals
3-12
2 ve-
Halogens
17
7ve-
Yes, chemically reactive because they only
have 7ve-. Most reactive non-metallic
group.
Noble Gases
(Inert Gases)
18
8ve-
No, not chemically reactive because they
have the maximum number of ve-.
Most noble elements = 8 ve.
Exception: He = 2ve.
Chemical Stability
Octet Rule:
 Atoms will gain, lose, or share valence electrons
to reach maximum stability.
What is maximum stability for most atoms?
 8 valence electrons (ve-)
 Exceptions: H and He max. stability = 2 ve-
How do atoms achieve stability ?
 Atoms chemically bond with other atoms.
 Formation of diverse compounds in nature.
Periodic Table Lab: Valence Electrons
Purpose: To establish a pattern with valence electrons and
groups on the periodic table.
Hypothesis: What do you think the relationship is between
valence electrons and elements in the same group?
Lab
grps
A
B
C
D
grp 1 grp 2
veve-
grp 3-12 grp 13
veve-
grp 14
ve-
grp 15
ve-
grp 16
ve-
grp17 grp18
veve-
Periodic Table: 4.24.14
Objectives:
•Electron Properties and Arrangement Corrections
•I can predict chemical reactivity for an element based on
its number of valence electrons and location on periodic
table.
• I can distinguish between metallic and non-metallic
properties.
Periodic Table Lab: Valence Electrons
Lab
grps
grp 1 grp 2
veve-
grp 3-12 grp 13
veve-
grp 14
ve-
grp 15
ve-
grp 16
ve-
grp17 grp18
veve-
A
B
C
D
What can be concluded from the data table?
Common Periodic Table Groups
Periodic Groups
Alkali Metals
Alkaline-Earth
Metals
Transitional
Metals
Halogens
Noble Gases
(Inert Gases)
Group #
Valence
Electrons
Chemical Reactivity
(Yes or No)
Common Periodic Table Groups
Periodic Groups
Alkali Metals
Alkaline-Earth
Metals
Group #
Valence
Electrons
1
1ve-
2
Chemical Reactivity
(Yes or No)
Yes, chemically reactive because they only
has 1 ve-. Most reactive metallic group.
2ve-
Yes , chemically reactive because they only
have 2 ve-.
Yes, chemically reactive because they only
have 2 ve-.
Transitional
Metals
3-12
2 ve-
Halogens
17
7ve-
Yes, chemically reactive because they only
have 7ve-. Most reactive non-metallic
group.
Noble Gases
(Inert Gases)
18
8ve-
No, not chemically reactive because they
have the maximum number of ve-.
Most noble elements = 8 ve.
Exception: He = 2ve.
Chemical Stability
Octet Rule:
 Atoms will gain, lose, or share valence electrons
to reach maximum stability.
What is maximum stability for most atoms?
 8 valence electrons (ve-)
 Exceptions: H and He max. stability = 2 ve-
How do atoms achieve stability ?
 Atoms chemically bond with other atoms.
 Formation of diverse compounds in nature.
Chemical Stability: Octet Rule
1.
Will metals tend to gain or lose valence electrons to
reach maximum stability?
Will non-metals tend to gain or lose valence electrons to
www.teacherfurse.com
reach maximum stability?
http://www.green-planet-solar-energy.com/the-element-chlorine.html
Chemical Stability: Octet Rule
Metals will lose ve- to reach stability.
 Form a cation (+ charged)

www.teacherfurse.com
Non-metals will gain ve- to reach stability.
 Form an anion (- charged)

http://www.green-planet-solar-energy.com/the-element-chlorine.html
Chemical Stability
Each of the elements below are neutral.
 Determine if chemically stable by identifying what
group it is in. (# of valence electrons)
 If not stable, predict what charge it must have to
reach stability.
a. Sodium
b. Oxygen
c. Argon
d. Phosphorus
e. Chromium
Chemical Stability-Key
Determine what type of charge each element below
would form to reach maximum stability.
a.
b.
c.
d.
e.
Sodium Na1+
Oxygen O2Argon
Ar
Phosphorus p3Chromium Cr2+
Metallic vs. Non-metallic Properties











Low luster
High luster
low density
High density
High melting point
Low melting point
Ductility
Primary gases at room temp.
Primary solids at room temp.
Alkaline earth group
stability










Brittle
Malleable
Conductors of heat and
electricity
Insulators of heat and
electricity
Transitional group
Noble gases
Halogens
Valence electrons
Alkali group
Groups have similar
Metallic vs. Non-metallic Properties
Periodic Table: 11.17.14
Objectives:
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic
properties.
•
•I
can graph and interpret periodic trends.
Periodic Table: Bell Ringer
Classify the following as either metallic (M) or nonmetallic (NM)
insulator of heat
high density ductility anion
2. Give an example of a metal, non-metal, and
metalloid from the periodic table.
3. Determine if the following neutral elements needs
to become ions to reach maximum stability. If so,
determine what charge they would have.
a. Al
b. Br
c. Ne
d. Au
1.
Metals, Non-metals, Metalloids
Metalloids:
 Exhibits metallic and non-metallic properties
 Depends upon what it is bonding with.
 Most touch the staircase
Size of an Ion
Use the diagrams below to determine what happens
to the size of a neutral atom(parent atom) when it
becomes an ion.
Size of a Cation
Why is the cation smaller than its parent atom (neutral)?
Size of an Anion
Why is an anion larger than its parent atom?
Size of Ions
a.
Circle the atom that is larger in size.
Ca or Ca2+
b.
S or S2-
1.
Circle the atom that is smaller in size.
a. Al or Al3+
2.
b. N or N 3-
Periodic Trend: Electronegativity

Establish a relationship between the
periodic table and electronegativity.
Periodic Table: 11.18.14
Objectives:
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic
properties.
•
•I
can distinguish between the size of neutral and charged
atoms.
•I
can graph and interpret periodic trends.
Periodic Trend: Electronegativity
Across a Period:
Down a Group:
mmsphyschem.com
Electronegativity and Chemical Bonding
•Do metals or non-metals have a greater electronegativity
value?
Periodic Table: 11.20.14
Infinite Campus:
• Periodic Table Quiz (11pts.)
• Elecronegativity Graph (10pts.)
Objectives:
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
• I can distinguish between metallic and non-metallic
properties.
•I can distinguish between the size of neutral and charged
atoms.
•I can graph and interpret periodic trends.
Homework:
• Complete Periodic Table Review-Test tomorrow
Periodic Table Quiz
Periodic Trends: Atomic Radius
Across a Period
Atomic Number vs. Atomic
Radius
200
atomic raidus (pm)
180
160
140
120
Down a Group
100
80
60
40
20
0
1
2
3
4
5
6
7
8
9
10 11 12 13 14 15 16 17 18
atomic number
Periodic Table : Atomic Radius
Explain how this picture illustrates ionic bonding?
Chemical Bonding Properties Lab
History of the Periodic Table
Dmitri Mendeleev:
• Russian chemist and teacher
•When organized elements into groups
by similar chemical properties,
he observed the periods increasing in
atomic mass. (1869)
• His organization system was
successful at predicting undiscovered
elements.
•Do you observe any inconsistencies
with his organization system?
History of Periodic Table
Henry Moseley:
•British Physicists
•Tweaked Mendeleev’s periodic table.
•When elements were placed in groups
by chemical properties, the periods
consistently increased by atomic
number. (1913)
•Current organization of elements on
the periodic table.
Periodic Table: 4.30.14
Objectives:
•Periodic Table Exam
•I can predict chemical reactivity for an element based on its
number of valence electrons and location on periodic table.
• I can distinguish between metallic and non-metallic
properties.
•I can graph and interpret periodic trends.
•I can understand how the periodic table was organized by
Mendeleev and Moseley.
•I can illustrate chemical bonding using Lewis Dot Structures.
Lewis Dot Structures
Lewis Dot Structures:
•Illustrates
valence electrons
for an atom.
Place electrons (dots) around
the elements symbol using
cardinal directions.
Element
Na
Mg
Si
S
Do NOT pair electrons
up until you have to.
•
He
# of
valence
electrons
Lewis Dot
Structure
Ionic Bonding (Lewis Dot Transfer)
Metal
(Lewis
Dot)
Non-metal
(Lewis Dot)
Ionic Bonding
(Lewis Dot Transfer)
Chemical
Formula