CHEMISTRY
2014-2015 SCHOOL YEAR
CLASSROOM: 510
CODE: SCS21A
INSTRUCTOR: Ms. Bui
LAB ROOM: 506
PERIODIC TABLE
TRENDS
Name_______________________________________
Date: ______________________________________
Period: _____________________________________
Subject: Chemistry
Standards:
 3.1aa – The succession of elements within the same group demonstrates characteristic trends: differences in atomic radius, ionic radius,
electronegativity, first ionization energy, metallic/nonmetallic properties.
 3.1bb – The succession of elements across the same period demonstrates characteristic trends: differences in atomic radius, ionic radius,
electronegativity, first ionization energy, metallic/nonmetallic properties.
SCIENCE STARTER
1. Using the Periodic Table, provide the following information about fluorine
a. Period:
b. Group:
c. Group name:
d. Atomic Number:
e. Valence Electrons:
f. Number of Energy Levels
2. What is the Group Name for Group 1?
3. What is the name of the element located at Period 5 Group 17?
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Practice
Instruction: Complete the table below by identifying the trends for the properties listed.
Comparison
Na to Al
Atomic Radius
First Ionization Energy
Electronegativity
Metallic
Ca to Ba
Ga to Br
B to Ga
Cs to At
Instruction: Write a claim, provide evidence from the periodic table or Table S and explain your
evidence.
AIM Prompt: In a chemical reaction, which element (K or Br) loses its valence electron first?
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PERIODIC TABLE
GUIDED NOTES - TRENDS
Name_______________________________________
Date: ______________________________________
Period: _____________________________________
Subject: Chemistry
Part 1: Atomic Radius
Table 1
Symbol Atomic Number
Li
3
Be
4
B
5
C
6
Atomic Radius
130. pm
99 pm
84 pm
75 pm
1. These elements are located in Period ___________.
2. Elements located in this period have _____________ energy levels (or electron shells).
3. Based on the table above, as the atomic number increases, the atomic radius ______________.
4. Atomic Radius is an ___________ of the size of the atom or the distance from the ___________
to the edge of the atom.
5. Going across a period, electrons are added to the ____________ energy level. At the same time
____________ are being added to the nucleus. As a result, the increased concentration of
protons in the nucleus creates a higher effective nuclear charge. Thus, a ____________ force of
attraction pulls the electrons closer to the ____________________ resulting in a
_______________ atomic radius.
Table 2
Symbol Atomic Number
Li
3
Na
11
K
19
Rb
37
Atomic Radius
130. pm
160 pm
200 pm
215 pm
6. These elements are located in Group ___________.
7. Elements located in this period have _____________ valence electrons.
8. Based on the table above, as the atomic number increases, the atomic radius ______________.
9. Going down a group, the number of energy levels ______________. Each subsequent energy
level is further from the _______________. Thus, the atomic radius _____________ as the
group and energy levels increase.
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Part 2: First Ionization Energy
Table 3
Li
Atomic
Number
3
First Ionization
Energy
520. kJ/mol
Be
4
900. kJ/mol
B
5
801 kJ/mol
C
6
1086 kJ/mol
Symbol
1. These elements are located in Period ___________.
2. Based on the table above, as the atomic number increases, the first ionization energy
______________.
3. First Ionization Energy is the energy required to remove the most loosely bound (outermost)
_____________ from an atom
4. Going across a period, the atomic radius _____________making the atom smaller thereby
making the outer electrons (or ____________ electrons) closer to the _________ and more
strongly attracted to the center. Therefore, it becomes more difficult to __________ the
outermost electron
Table 4
Atomic
Symbol Number
Li
3
Na
K
Rb
First Ionization
Energy
520. kJ/mol
11
19
37
496 kJ/mol
419 kJ/mol
403 kJ/mol
1. These elements are located in Group ___________.
2. Elements located in this period have _____________ valence electrons.
3. Based on the table above, as the atomic number increases, the first ionization energy
______________.
4. Going down a group, the number of energy levels ______________. Thus, the valence
electrons are __________ away from the nucleus making it ______________ to remove the
valence electrons.
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Part 3: Electronegativity
Table 5
Li
Atomic
Number
3
Be
4
1.6
B
5
2.0
C
6
2.6
Symbol
Electronegativity
1.0
5. These elements are located in Period ___________.
6. Based on the table above, as the atomic number increases, the electronegativity
______________.
7. Electronegativity measures an atom’s tendency to attract and form bonds with ______________.
8. Going across a period, the number of valence electrons _________________thus, making the
electronegativity __________________ as the atomic number increases.
Table 6
Atomic
Symbol Number
Li
3
Na
K
Rb
11
19
37
Electronegativity
1.0
0.9
0.8
0.8
5. These elements are located in Group ___________.
6. Elements located in this period have _____________ valence electrons.
7. Based on the table above, as the atomic number increases, the number of energy levels
increases. Thus, the valence electrons are located ________________ away from the nucleus.
As a result, the ______________.
8. Going down a group, the number of energy levels ______________. Thus, the valence
electrons are __________ away from the nucleus resulting in a ______________
______________ electronegativity.
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Part 4: Metallic
1. Metallic characteristic of an element refers to how readily an atom can ________________ an
electron.
2. Going across a period from right to left, the metallic characteristic ____________________
because the attraction between the valence electrons and the nucleus is ________________.
Part 5: Identify the Trends
Instructions: Place the following terms into the correct arrow. Each arrow may holds only one
vocabulary (first ionization energy, atomic radius, metallic, electronegativity). The vocabulary
will be used twice
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