1
Chem I #2
Wksts # 1-5 Packet
Valence Electron & Oxidation Number Practice
Name____________________ Period_____
Instructions: Complete the chart using your knowledge of atoms.
Element
Atomic
Symbol
Bromine
Br
Total # of
Electrons
# of Valence
Electrons
# of Electrons
Gained or Lost
Oxidation
Number
Ion
Symbol
7
1 gained
-1
Br
35
Lithium
Calcium
Sulfur
Boron
Phosphorus
Chlorine
Sodium
Hydrogen
Oxygen
Helium
Nitrogen
Magnesium
Potassium
Fluorine
2
-
Chem I - PERIODIC TRENDS WORKSHEET #3
Name________________ Period________
PART I - Directions: Label each periodic table according to the directions given.
When drawing arrows, show the increasing trend (from smallest to largest value).
1. Group #’s & Period #’s – write the numbers
of each group and period.
4. Atomic Radius – draw arrows that show the
trend for periods and groups.
Define the group # & period # for Carbon (C):
__________________________________________
Rank the following atoms from smallest to largest
Li, C, F:________________________________
2. Valence Electrons – write the number of
valence electrons about each group.
5. Ionization Energy – draw arrows that show
the trend for periods, groups and also diagonal.
Definition of Valence Electrons: _________________
___________________________________________
Rank the following atoms from lowest to highest
ionization energy Mg, Ca, Ba:__________________
3. Oxidation Numbers – write the oxidation
numbers for each group.
6. Electronegativity – draw arrows that show
the trend for periods, groups and also diagonal.
Definition of Oxidation Number: ________________
__________________________________________
Rank the following atoms from lowest to highest
electronegativity Si, P, O:______________________
PART II - Directions: Using the information from your notes, answer the following questions.
3
1. What group are the most reactive metals located?
2. What group are the most reactive nonmetals located?
3. As you go from left to right across a period, the atomic size (decreases / increases).
Why?
4. As you travel down a group, the atomic size (decreases / increases).
Why?
5. As you go from left to right across a period, the first ionization energy generally (decreases /
increases).
Why?
6. As you travel down a group, the first ionization energy generally (decreases / increases).
Why?
7. What element has the highest electronegativity?
8. What element has the lowest electronegativity?
9. Elements of Group 1 are called
10. Elements of Group 2 are called
11. Elements of Group 3-12 are called
12. As you go from left to right across the periodic table, the elements go from (metals / non-metals) to
(metals / non-metals).
13. Group 17 elements are called
14. The most reactive element in Group 17 is
15. Group 18 elements are called
16. What sublevels are filling across the Transition Elements?
17. Elements within a group have a similar number of
18. Elements across a period have the same number of
19. An element that has lost or gained an electron is called
20. As you go down a group, the elements generally become (more / less) metallic.
21. The majority of elements in the periodic table are (metals / nonmetals).
22. Elements in the periodic table are arranged according to their
23. An element with both metallic and nonmetallic properties is called a
4
Chem I - Periodicity Defined #4
Name___________________________ Period_____
1. The periodic table can be used to discover properties of elements. Name 4 trends that can be
predicted using the periodic table.




2.
Define the following:
 Ionization Energy

Electronegativity
3. The element with a high electronegativity value of 2.96 is most likely Bromine or Potassium?
Why?
4. Rank the following elements in order of increasing atomic radius: Ag, Sr, Sb, I, Rb, Te
5. Circle the element of each pair that has the highest atomic radius:
 Br or Cl
 Mg or Al
 Na or Cl
 B or Si
 Cs or Bi
 Ni or Br
 K or Sr
 P or As
5
6. Rank the following elements in order of increasing electronegativity: F, Sb, Sr, I, Rb, Fr
7. Define oxidation number.
8. Write valance electrons for each element and predict the oxidation numbers:
Element
Ca
Al
Se
O
F
Na
Mg
P
N
Cl
Valence Electrons
Oxidation Number
9. What are Group 1 elements called?
What oxidation number do they usually have?
10. What are Group 2 elements called?
What oxidation number do they usually have?
11. What are Group 17 elements called?
What oxidation number do they usually have?
12. What are Group 18 elements called?
What oxidation number do they usually have?
13. What is the group name given to elements that have the following valence shell electron
configuration?
 s2
__________________

s2p6
__________________


s2p5
___________
s1
___________
6
14. Name the three lightest members of the noble gases?
15. List the symbols of all the alkali earth metals.
16. Which alkali metal belongs to the sixth period?
17. Which halogen belongs to the fourth period?
18. What element is in the fifth period and the eleventh group?
19. Why do all the members of a group have similar properties?
20. Name the element that is classified as the most reactive metal.
21. Name the element that is classified as the most reactive nonmetal.
22. Provide 3 properties for:
a. Metals
b. Nonmetals
c. Metalloids
7
Chem I #5 – Graphing Periodicity
Name___________________ Period______
Background Information
Elements are arranged in the periodic table in the periodic table in order of increasing atomic number.
The elements are further arranged into groups and periods. The arrangement of the periodic table
reveals trends. A trend is a predictable change in a particular direction. Knowing the various trends for
elements in the periodic table enables you to make logical predictions about chemical behavior.
Purpose
 To establish trends of atomic radius
and ionization energy of representative
elements from the periodic table.
 To correlate trends of atomic radius
and ionization energy.
Procedure:
1. Use the graph paper provided to
create two separate “line graphs”.
Graph #1 should display the data for
atomic radius. Graph #2 should
display the data for ionization energy.
2. For the both graphs, on the X axis
(place the element symbol) and on the
Y axis (place the appropriate data).
3. Highlight the following - USE
COLOR
a. HIGHLIGHT YELLOW Period 3 (Na-Ar) in the
Atomic Radius Graph and the
Ionization Energy Graph
b. HIGHLIGHT PINK - Period
4
(K-Kr) in both the Atomic Radius Graph and
the Ionization Energy Graph
4. On both graphs, be sure to include the
appropriate labels, a key and title.
5. Analyze the graphs to address the
questions.
Data:
Element
Symbol
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Ga
Ge
As
Se
Br
Kr
Rb
Sr
In
Sn
Sb
Te
I
Xe
8
Atomic Radius
(in angstrons)
0.79
0.49
2.05
1.40
1.17
0.91
0.75
0.65
0.57
0.51
2.23
1.72
1.82
1.46
1.23
1.09
0.97
0.88
2.77
2.23
1.81
1.52
1.33
1.22
1.12
1.03
2.98
2.45
2.00
1.72
1.53
1.42
1.32
1.24
Ionization Energy
(in Electron Volts)
1.3598
24.587
5.392
9.322
8.298
11.26
14.5354
13.618
17.422
21.564
5.139
7.646
5.986
8.151
10.486
10.36
12.967
15.759
4.341
6.113
5.999
7.899
9.81
9.752
11.814
13.999
4.177
5.965
5.786
7.344
8.641
9.009
10.451
12.13
Analysis Questions:
1. Examine the graph carefully and describe the general trends of atomic radius for period 3. (Na
through Cl)
2. Define ionization energy:
3. Examine the graph carefully and describe general trends for ionization energy for period 3.
(Na through Cl)
4. Compare the trends for both atomic radius and ionization energy moving left to right across
period 4. (K through Kr)
5. Explain how ionization energy is related to atomic radius.
6. If an element has high ionization energy, is it likely to be Calcium or Bromine and why?
7. What would be the correlation between atomic radius and electronegativity if you to graph
them?
9
Graph #1 Title:
Graph #2 Title:
10
11