Selected Response Assessment
UNIT:
The Periodic Table, 10th-12th grade
CLEAR PURPOSE:
The purpose of this formative assessment is to evaluate students’ mastery of the learning targets
presented in the unit thus far based on the learning targets listed below. This assessment will consist of
multiple choice, true false, fill in the blank and matching questions. Each section will be worth 5 pts. This
assessment will be used by the teacher to monitor student understanding of key concepts that are needed
to move forward with the unit. The assessment will also be used as a self-evaluation tool for the students
to identify their strengths and weaknesses in the unit thus far. The learning targets listed below will also
be tested in a summative assessment at the end of the term.
STANDARDS/BENCHMARKS: (Taken from the Michigan Merit Curriculum-Chemistry)
C4.9 A Identify elements with similar chemical and physical properties using the periodic table.
C4.9c Predict general trends in atomic radius, first ionization energy, and electronegativity of the
elements using the periodic table.
CLEAR LEARNING TARGETS (knowledge and reasoning)
Learning Targets/Goals
I can identify elements on the periodic table with similar
chemical and physical properties.
I can classify an element as a metal, non-metal or metalloid
based on its position on the periodic table.
I can define atomic radius.
Knowledge
Questions
9, 11, 12, 13
1,12, 13
10, 18
I can explain the trend for atomic radius using the periodic
table.
2, 17
I can define first ionization energy.
3, 19
I can explain the trend for first ionization energy using the
periodic table.
4, 5
I can define electronegativity.
6,, 20
I can explain the trend for electronegativity using the
periodic table.
7, 8
I can compare several elements and order them from
greatest to least for each trend.
Reasoning
Questions
14, 15, 16
Directions will be read aloud to the class.
Directions: By the end of this unit you will be able to use the periodic table to identify elements, explain
how they will bond with other elements, and write the chemical formula for the newly formed compound.
Before we move on, we need to check your understanding of the terminology and concepts that will allow
you to complete the tasks mentioned above. You will be receiving a clean copy of a periodic table to use
with the assessment. The assessment has 10 multiple-choice questions, 6 matching questions and 4 fill in
the blank questions each worth 1 point for a total of 20 pts. Please remember while we are evaluating
your score on this assessment, it will not count for a grade. Please put your name, date and hour in the
upper right corner of the packet. Read the directions for each section carefully so you know exactly
how I would like the questions answered. You may write your answers directly on the assessment
packet. After each question you will find a spot to mark whether you are sure or not sure of your
answer. Please be honest in answering these, as it will help you know what areas you need to
study more. You will have 45 minutes to complete this assessment, so please take your time in
answering each question and be sure to raise you hand and ask Mrs. Lillibridge if you are unsure of what
a question is asking. Please place the assessment in the tray when you have finished and remain
silent until everyone has finished his or her assessments. Good Luck! I know you will do well!
Name:______________________________
Date:_______________________________
Hour:______________________________
Multiple-Choice : (10 pts)
Please circle the best response to the question. Don’t forget to check if you are sure or not sure of your
answer.
1. An atom has an atomic mass of 80, and 45 neutrons. What type of element is it?
A. Metal
B. Non-metal
C. Metalloid
D. Transition Metal
_____ Sure ______ Not Sure
2. As the atomic number increases across a period, what happens to the atomic radius?
A. Increases
B. Decreases
C. Stays the same
D. Doubles
_____ Sure ______ Not Sure
3. Which electron requires the least energy to remove?
A. First
B. Second
C. Third
D. Fourth
_____ Sure ______ Not Sure
4. Ionization energy generally_____________ as we move across a period and _____________ as we move
down a group.
A. Increases, increases
B. Increases, decreases
C. Decreases, increases
D. Decreases, decreases
_____ Sure ______ Not Sure
5. Which of the following periodic groups has the highest ionization energy?
A. Alkali Metals
B. Alkali Earth Metals
C. Halogens
D. Noble Gases
_____ Sure ______ Not Sure
6. What is the measure of an atoms ability to attract electrons in a chemical compound called?
A. Conductivity
B. Ionization energy
C. Luster
D. Electronegativity
_____ Sure ______ Not Sure
7. Which of the following periodic groups has the lowest electronegativity?
A. Alkali Metals
B. Alkali Earth Metals
C. Halogens
D. Noble Gases
_____ Sure ______ Not Sure
8. Electronegativity generally ____________ as we move across a period and ____________ as we move
down a group.
A. Increases, increases
B. Increases, decreases
C. Decreases, Increases
D. Decreases, decreases
_____ Sure ______ Not Sure
9. Any elements in the same column on the periodic table share physical and chemical properties,
why is this?
A. They have the same number of protons.
B. The have the same atomic radius.
C. They have the same atomic mass.
D. They have the same number of valence electrons.
_____ Sure ______ Not Sure
10. How do you calculate an atoms atomic radius?
A. It is the same as the atomic mass.
B. Number of electrons minus the charge.
C. Number of protons plus number of neutrons.
D. Distance between 2 nuclei of the same atom divided by 2.
_____ Sure ______ Not Sure
Matching: (6pts)
There are two portions to the matching section. For questions 11-13 please match the statement from
column 1 with the best choice from column 2. Some choices from column 2 may not be used. Don’t forget
to check if you are sure or not sure of your answer.
Column 1
Column 2
11. _______ Group 17 on the periodic table.
_____ Sure
_____ Not Sure
12. ______ Elements that are shiny and conduct
electricity found in groups 1 – 12 on the
periodic table.
_____ Sure
A. Metals
B. Halogens
C. Non-metals
D. Noble Gases
E. Metalloids
_____ Not Sure
13. ______ Elements that are dull, and do not
conduct electricity found in groups
_____ Sure
_____ Not Sure
For questions 14-16 order the elements listed below from greatest to lease for each trend. You may write
the corresponding letter for each element in the blanks provided. Don’t forget to check if you are sure or not
sure of your answer.
A. Oxygen
B. Cesium
C. Phosphorus
14. Electronegativity: ___________ > ____________> ____________
______ Sure
______ Not Sure
15. Atomic Radius: ____________> _____________> ______________
______ Sure
______ Not Sure
16. First Ionization Energy: __________>____________>______________
______ Sure
______ Not Sure
Fill in the Blank: (4pts)
Please write the answer in the blanks provided. Don’t forget to check if you are sure or not sure of your
answer.
17. The atomic radius ________________ as we move _______________a group because additional electrons
occupy shells further from the nucleus.
______ Sure ______ Not Sure
18. The ______________________________ of an element is a measure of the size of its atoms, the distance from
the nucleus to the valence shell electrons.
______ Sure ______ Not Sure
19. The energy required to remove one electron from a neutral atom of an element is
the____________________________________________.
______ Sure
______ Not Sure
20. _________________________ results from the strength of an atom’s desire to achieve a full valence shell and
the attraction caused by the protons in the nucleus.
______ Sure
______ Not Sure
Self-Assessment Portion:
This is where you will look at how well you did for each learning target. Fill in the table below by marking
how many questions you got right, how many questions your got wrong, and what questions you were
sure and not sure of. If you got even 1 wrong for any of the learning targets, you need to complete the
corrective worksheet for that target.
Learning
Targets/Goals
I can identify
elements on the
periodic table with
similar chemical and
physical properties.
I can classify an
element as a metal,
non-metal or
metalloid based on its
position on the
periodic table.
I can define atomic
radius.
Questions
Total #
Right
Total #
Wrong
# Sure
# Not Sure
Corrective
worksheet #
9, 11, 12, 13
#1
1,12, 13
#1
10, 18
#2
I can explain the
trend for atomic
radius using the
periodic table.
2, 17
#2
I can define first
ionization energy.
3, 19
#2
I can explain the
trend for first
ionization energy
using the periodic
table.
4, 5
#2
I can define
electronegativity.
6,, 20
#2
I can explain the
trend for
electronegativity
using the periodic
table.
7, 8
#2
I can compare several
elements and order
them from greatest to
least for each trend.
14, 15, 16
#3
** If you got 100% on the assessment please complete the enrichment activity.
Answer Key
1. B
2. B
3. A
4. B
5. C
6. D
7. A
8. B
9. D
10. D
11. B
12. A
13. C
14. A>B>C
15. B>C>A
16. A>B>C
17. Increase, Down
18. Atomic Radius
19. First Ionization Energy
20. Electronegativity
Accommodations for diverse learners:
Several students in this class are ESL students or labeled LD. These students will be allowed to take their
test separate from the rest of the class in their special education teacher’s classroom. The students may
take the test on paper and have the questions read to them orally by their teacher, or they may take it on
the computer through exam view. Exam view allows students to see only one question at a time and they
can chose to have the computer read it to them orally if they like. These students will also be given time
and a half to complete this assessment.
Corrective #1
Student Worksheet: Periodic Organization
A Periodic Advertisement Project Worksheet
Use your notes to answer the following questions.
1. Why are the elements placed in specific places on the Periodic Table?
____________________________________________________
2. Periods are ______ that run from left to right.
3. Elements in the same period have the same number of _____________________.
4. Every element in the first period has _____ shell for its __________. Every element in the second period has _____
shells for its __________. See the pattern?
5. Groups are _______ that run from top to bottom.
6. The elements of a group have the same number of ____________ in their __________ shell.
7. Every element in group one has _____ electron in its outer shell. Every element in group two has _____ electrons in
its outer shell.
8. Hydrogen is special because it can act like two groups, _________ and __________.
9. Hydrogen sometimes is ________ an electron and sometimes it has an ______ electron.
10. Although helium has only _____ electrons in its outer shell, it is grouped with elements that have an octet, or _____
electrons.
11. The group 2 elements on this table are called __________ metals. They each have two electrons in their outer shell.
1
2
3
4
5
Key: O Alkali metals
Groups O Halogens
6
7
8
9
10
11 12 13 14 15
O Alkaline Earth metals
O Noble gases
16
O Transition metals
17 18
O Other
12. On this periodic table, color and label the 6 element groups listed for this piece of the Periodic Table on p.27 of your
notebook.
13. Alkali Metals:
a. What is the group number? ______
b. Are these metals reactive? ______
c. Do these metals occur freely in nature? _____
d. How many electrons are in their outer shell? _____
e. What are the three characteristics of ALL metals? ____________________
___________________________________________________________
f. Are these metals soft or hard? __________
g. Name the two most reactive elements in this group? ________ and ________
h. What happens when they are exposed to water? ____________________
14. Alkaline Earth Metals :
a. What is the group number? ______
b. Are these metals reactive? ______
c. Do these metals occur freely in nature? _____
d. How many electrons are in their outer shell? (Hint: it's the same as their oxidation
number or group number.) ___________
15. Transition Metals :
a. How many elements are in this group? ______
b. What are the group numbers? ______ through ______
c. What are valence electrons? _______________________________
d. Because the valence electrons are present in more that one __________
transition metals often exhibit several common ___________________.
16. Other Metals:
a. How many elements are in this group? ______
b. What are the group numbers? ______ through ______
c. How are these other metals similar to the transition metals? _______________
d. How are these other metals different to the transition metals?_____________
e. List three physical properties of these other metals. ______________________
f. . What are the common ions of the metals? Positive or Negative
17. Metalloids:
a. On your periodic table, draw the black stair-step line that distinguishes metals from nonmetals.
b. On your periodic table, use your pencil to lightly shade the nine elements that share a full side with the stair-step
line. These are the metalloids. Ask your teacher if you need help before you begin.
c. Metalloids have properties of both __________ and __________.
d. Define semiconductor. _________________________________________
e. Name two metalloids that are semi-conductors. __________ and __________
f. This property makes metalloids useful in __________ .
18. Nonmetals:
a. What are the group numbers? __________ through __________
b. List four characteristics of ALL nonmetals. __________________________
__________________________________________________________
c. What three states of matter do nonmetals exist in at room temperature?
_____________, ____________ and _____________
d. What are the common ions of the nonmetals? Positive or Negative
19. Halogens:
a. What is the halogen group number? _____
b. Are halogens metals or nonmetals? __________
c. The term "halogen" means ____________________ and compounds containing halogens are called ________.
d. How many electrons are in their outer shell? __________
e. What is their most common ion? __________
f. What states of matter do halogens exist in at room temperature? ___________
20. Noble Gases:
a. What is the group number? _____
b. Why were these gases considered to be inert or stable? _________________
___________________________________________________________
c. What common ions do they form? _____
21.Rare Earth Elements:
a. On your periodic table, label the Lanthanide and Actinide series with your pencil.
b. How many Rare Earth elements are there? _____
c. Define trans-uranium. __________________________________________
d. The Rare Earth metals are found in group _____ and periods _____ and _____.
Corrective #2
Periodic Trends Activity Alternative Assignment
1. Examine Figure 6.19 on Page 175. Why are the ions of the top 3 elements in group 5A
larger than the ions of the top 3 elements in Group 4A?
2. The elements in group 4A can become either +4 or -4 (even though the Ionic Radius
Chart shows only +4.) If the chart showed the -4 ion of Carbon or Silicon, describe what
you would expect them to look like. How large would they be compared to their neutral
atoms?
3. Examine the Electronegativity Chart (Table 16.2, Page 177) Which of the elements in
each of the following sets attracts electrons the strongest?
Arsenic Nitrogen, Phosphorus
Antimony, Indium, Tin
Calcium, Germanium, Oxygen
4. Examine the Ionization Energy Chart (Table 6.1 on Page 173) What do the elements
with the lowest first ionization energies (about 500 kJ/mol or less) have in common?
5. Examine the Ionization Energy Chart (Table 6.1 on Page 173 and the Electronegativity
Chart (Table 16.2, Page 177). What is the First Ionization energy for the element with
the highest electronegativity?
6. Examine the Ionization Energy Chart (Table 6.1 on Page 173) . Why is the 3rd ionization
energy for Beryllium so much higher than its 2ndionization energy?
7. What is the trend in atomic radii as you go from Li to Na to K? From He to Ne to Ar?
What is the general trend in atomic radii as you descend any group?
8. What is the general trend in first ionization energy as you go across a period?
Down a family (e.g. alkaline earth metals)?
9. Which family of elements tends to lose its electrons?
10. Which family of elements tends to hold onto its electrons the tightest?
11. If a Na atom were to ionize, would it be bigger, smaller or the same size as its atom?
Explain why using your knowledge of atomic structure. (Hint – draw a diagram) .
12. If a chlorine atom were to ionize, would the chloride ion be bigger, smaller or the same size as its
atom? Explain why using your knowledge of atomic structure.
Corrective #3
Periodicity Worksheet
Use a periodic table to help you answer the following questions.
1. Which element in the second period has the greatest atomic radius?
2. Which of the group IIIA (13) elements is the largest?
3. Of the halogens, which has the smallest radius?
4. Which of the alkaline earth metals is the largest?
5. Which of the transition metals has the smallest atomic radius?
6. Which of the noble gases is the smallest?
7. The atomic radius of which element is the largest?
8. Do alkali metals generally make anions or cations?
9. Which of the elements which have their valence electrons in the second
energy level is the largest?
10. Which of the metalloids has the smallest atomic radius?
11. Which of the rare earth elements is the smallest?
12. Which of the transition metals in the fifth period is the largest?
13. Are metal ions larger or smaller than the neutral atoms they came from?
14. Are cations larger or smaller than the neutral atoms they came from?
15. Are ions of alkali metals larger or smaller than ions of alkaline earth
metals from the same period?
16. Which element in the second period has the greatest first ionization
energy?
17. Which of the group IIIA (13) elements has the largest ionization
energy?
18. Of the halogens, which has the smallest electronegativity?
19. Which of the alkaline earth metals has the smallest electronegativity?
20. Which of the transition metals has the largest ionization energy?
21. Which of the noble gases has the smallest ionization energy?
22. Which of the group IVB (14) metals is the least active?
23. Which of the halogens is the most active?
24. Which of the semi-metals that have their valence electrons in the fourth
energy level has the largest ionization energy?
25. Which of the period three elements has the largest electronegativity?
26. Which of the inner transition elements of the seventh period is the
easiest to ionize?
27. Which of the transition metals in the fifth period has the largest EN?
28. Which of the group four metals has the largest ionization energy?
29. Which of the non-metals in the third period is the most active?
30. As atomic size increases, what happens to the ionization energy of the
Enrichment:
A Periodic Table Logic Problem
Purpose: In this activity you will work to use a set of clues to identify a set of unknown elements in
a periodic table. The elements are the elements with atomic numbers 1-20 and 31-36. A letter of the
alphabet is used to represent each unknown element. The letter designation is not related to an element’s
chemical symbol. Each clue refers to a property of an element or a relationship an element has to other
elements in the periodic table. Along with logic and knowledge of properties, you will use the periodic
trends to solve the puzzle.
Procedure: Use the following trend clues to place the elements in their proper places on the provided
periodic table. Try to identify the elements with direct clues first. For example, B is a direct clue because
it identifies only one element.
Sloppy Copy 1:
Group
Group
1
2
Group
13
Group
14
Group
15
Group
16
Clues:
A – Has one of the highest electronegativities on the table.
B – Has one electron in a 3p orbital.
C – Has five electrons in the 4thenergy level.
D – Forms the smallest 2+ ion.
E – Tends to gain one electron.
F – Electron configuration is 1s2 2s2 2p6 3s2 3p3
G – The most electronegative element.
H – An ion of this element with a 2+ charge has 18 electrons.
I – Its second ionization energy is large compared to its first ionization energy.
J – Its highest occupied energy level is full.
Group
17
Group
18
K – This nonmetal is likely to form an ion with a 3- charge.
L – Has the highest 1st ionization energy in the table.
M – Has the smallest atomic radius in the 3rd period.
N – Is the smallest atom in its family.
O – The first element with an electron in the 2nd energy level. P – The only nonmetal in a group of highly
reactive metals.
Q – Has eight fewer protons than its “groupmate” H.
R – The most likely element of the ones included to lose an electron.
S – A metalloid in period 4.
T – Its ionic radius is larger than its atomic radius.
U – The ion with a 2- charge that it forms has 18 electrons.
V – Atomic number is 34.
W – Metalloid that forms an anion with a 3+ charge.
X – Has characteristics of both a metal and a nonmetal.
Y – Has a lower 1st ionization energy than S.
Z – Has a 1st ionization energy that is higher than T but lower than M.
Final Copy
Group
1
Group
2
Group
13
Group
14
Group
15
Group
16
Group
17
Group
18