Download unit 1 introduction to matter

NAME:_______________________
4.3 What is ionization energy?
DATE:____________
AHS Instructor Ms. Kasia Room 109/110
UNIT 4 THE PERIODIC TABLE
4.3 What is ionization energy?
AIM:
DO NOW: Take our your Chemistry Reference Tables. Turn to the Periodic Table of Elements (Page 8).
1. What is the trend for atomic radius as you move from left to right on the period?
2. What causes this trend?
ACTIVITY
Directions: Using Table S, order the following from least first ionization energy to greatest first
ionization energy.
Se
S
Te O
P
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Least
Greatest
What do you notice?
Al
Si
Cl
Na Ar Mg P
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Least
Greatest
What do you notice?
IONIZATION ENERGY
TERM
IONIZATION
ENERGY
DEFINITION
WHY?
GOING ACROSS
PERIOD
GOING DOWN
THE GROUP
Directions: Indicate the trend as you move UP A GROUP and as you move ACROSS A PERIOD.
NAME:_____________________________
4.3 What is ionization energy?
DATE:________
AHS Instructor Ms. Kasia Room 109
UNIT 4 THE PERIODIC TABLE
4.3 What is ionization energy?
Directions: Answer each question below to the best of your ability. Ask if you have questions.
1. Order from LEAST IONIZATION ENERGY to GREATEST IONIZATION ENERGY.
a. Sr
Sn
I
Rb
Sn
Xe
Te
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b. Ra
Ba
Sr
Ca
Mg
Be
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c. F
Cl
Br
I
At
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d. Mn
Sc
Ti
Cr
Co
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2. Which general trend is found in Period 2 on the Periodic Table
as the elements are considered in order of increasing atomic
number?
(1) Decreasing atomic mass
(2) Decreasing electronegativity
(3) Increasing atomic radius
(4) Increasing first ionization energy
Explain how you found your
answer
3. As the elements are considered from top to bottom in Group 15
of the Periodic Table, the ionization energy
(1) Decreases
(2) Increases
(3) Remains the same
Explain how you found your
answer
4. Which trends are observed when the elements in Period 3 on the
Periodic Table are considered in order of increasing atomic
number?
(1) The atomic radius decreases, and the first ionization energy
generally increases.
(2) The atomic radius decreases, and the first ionization energy
generally decreases.
(3) The atomic radius increases, and the first ionization energy
generally increases.
(4) The atomic radius increases, and the first ionization energy
generally decreases.
Explain how you found your
answer
5. As one proceeds from left to right across Period 3 of the Periodic
Table, there is a decrease in
(1) Ionization energy
(2) Metallic characteristics
(3) Electronegativity
(4) Valance electrons
6. If the elements are considered from top to bottom in Group 17,
the number of electrons in the outermost shell will
(1) Decrease
(2) Increase
(3) Remain the same
Explain how you found your
answer
Explain how you found your
answer
7. As we move across a period on the periodic table, the ionization energy_________________________
8. As we move down a group on the periodic table, the ionization energy_________________________
9. Circle the element in each pair with the higher ionization energy. USE YOUR KNOWLEDGE OF
THE TRENDS!
1
Li
Na
2
Sc
Ti
3
Pd
Ag
4
Al
Si
5
Cl
Br
10. Circle the atom in each pair that has the largest atomic radius
1
Al
B
2
S
O
3
Br
Cl
4
Na
Al
5
O
F
11. Why does fluorine (F) have a higher ionization energy than iodine (I)
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