Download 6 The Periodic Tableааааааааааааааааааааааааа__ /__ pts First

2
6 The Periodic Table __ /__ pts Anticipatory Response
1. Elements in the same row & column behave similarly? Y N 2. Alkalis are in column 1? Y N 3. Metalloids are on the stair Steps of the table? Y N 4. Metals are on the right? Y N 5. A family, group, or column Are the same thing? Y N Anticipatory Response 1.Elements are bigger toward The right side of a row? Y N 2. Elements get bigger as you Move down a column? Y N 3. It’s harder to remove an electron from metals? Y N 4. Metals have higher ionization Energies than non‐metals? Y N 5. Shielding remains constant In a row or energy level? Y N Summary Section: 2
First Last Name___Per__ Cornell Question & Ans
Directions: Make 5 questions
& answers that are different
than the Anticipatory Response
1. 2. 3. 4. 5. 3
PERIODIC TRENDS
3
Name:________________
Week of:__9/26/2016_____
Weekly Warm-Ups
Monday
Tuesday
Wednesday
Period:____
Name:________________
Thursday
Friday
Week of:__9/26/2016_____
Period:____
Name:________________
Week of:__10/03/2016_____
Weekly Warm-Ups
Monday
Tuesday
Wednesday
Period:____
Name:________________
Thursday
Friday
Week of:__10/03/2016_____
Period:____
05_CTR_ch06 7/9/04 3:27 PM Page 131
6
Name ___________________________
6.1
Date ___________________
Class __________________
ORGANIZING THE ELEMENTS
Section Review
Objectives
• Explain how elements are organized in a periodic table
• Compare early and modern periodic tables
• Identify three broad classes of elements
Vocabulary
•
•
•
•
periodic law
metals
nonmetals
metalloids
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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Chemists used the
of elements to sort them into groups.
The periodic table organizes the elements into vertical
and horizontal
3
4
2. _______________________
. The table is
3. _______________________
constructed so that elements that have similar chemical properties
4. _______________________
are in the same
5
in order of increasing
2
1. _______________________
.
6
when cut. Most nonmetals are
have a high luster, or sheen,
5. _______________________
7
6. _______________________
at room temperature.
Elements with properties that are similar to those of metals
7. _______________________
8
8. _______________________
and nonmetals are called
. Across the periodic table,
the properties of elements become
10
9
metallic and
nonmetallic.
9. _______________________
10. _______________________
6
↑
Chapter 6 The Periodic Table
131
05_CTR_ch06 7/9/04 3:27 PM Page 132
Name ___________________________
7
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 10. In his periodic table, Mendeleev arranged the elements in order of
atomic number.
________ 11. There are six periods in a periodic table.
________ 12. Most of the elements in the periodic table are metals.
________ 13. The elements within a period have similar properties.
Part C Matching
Match each description in Column B to the correct term in Column A
Column A
Column B
________ 14. metals
a. a vertical column of elements in the periodic table
________ 15. periods
b. good conductors of heat and electric current
________ 16. group
c. poor conductors of heat and electric current
________ 17. nonmetals
d. have properties that are similar to those of metals and
nonmetals
________ 18. metalloids
e. the horizontal rows of the periodic table
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Part D Questions and Problems
Answer the following questions in the space provided.
19. List the elements of Group 5A. Tell whether each is a metal, nonmetal, or
metalloid.
20. List three properties of metals.
21. Name two elements that have similar properties to those of chlorine.
132
Core Teaching Resources
7
↑
05_CTR_ch06 7/9/04 3:27 PM Page 133
Name ___________________________
6.2
8
Date ___________________
Class __________________
CLASSIFYING THE ELEMENTS
Section Review
Objectives
• Describe the information in a periodic table
• Classify elements based on electron configuration
• Distinguish representative elements and transition metals
Vocabulary
• alkali metals
• alkaline earth metals
• halogens
• noble gases
• representative elements
• transition metals
• inner transition metals
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
The periodic table displays the symbols and
1
of
1.
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the elements along with information about the structures of their
2
. The Group 1A elements are called
4
Group 2A elements are called
through 7A are called the
6
are
, and the
2A and 3A, there are
7
8
5
3
2.
, and the
3.
. The elements in Groups 1A
4.
. The nonmetals of Group 7A
5.
make up Group 8A. Between Groups
6.
in periods 4 through 7 and
9
in periods 6 and 7.
7.
8.
The atoms of the noble gas elements have their highest occupied 9.
s and
10
sublevels filled. The highest occupied s and p
sublevels of the representative elements are
11
.
10.
11.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 12. Group A elements are representative elements.
8
↑
Chapter 6 The Periodic Table
133
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Name ___________________________
9
Date ___________________
Class __________________
________ 13. Chlorine has the electron configuration 1s22s22p63s23p7.
________ 14. The element in Group 4A, period 3, is gallium.
________ 15. There is a relationship between the electron configurations of elements
and their chemical and physical properties.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. nonmetals of Group 7A
________ 17. inner transition metal
b. an element in which the highest occupied s and p
sublevels are filled
________ 18. representative element
c. Group 2A elements
________ 19. transition metal
d. an element whose highest occupied s sublevel and a
nearby d sublevel contain electrons
________ 20. noble gas
e. an element whose highest occupied s sublevel and a
nearby f sublevel generally contain electrons
________ 21. alkaline earth metals
f. Group 1A elements
________ 22. halogens
g. an element whose highest occupied s or p sublevels
are partially filled
Part D Questions and Problems
Answer the following in the space provided.
23. List the electron configurations for the highest occupied energy level of the
elements in period 3 from left to right.
24. List the elements of Group 6A. Tell whether each is a solid, liquid, or gas at room
temperature and whether it is a metal, nonmetal, or metalloid.
134
Core Teaching Resources
9
↑
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________ 16. alkali metals
05_CTR_ch06 7/9/04 3:27 PM Page 135
Name ___________________________
10
Date ___________________
Class __________________
PERIODIC TRENDS
6.3
Section Review
Objectives
• Describe trends among elements for atomic size
• Explain how ions form
• Describe and explain periodic trends for first ionization energy, ionic size, and
electronegativity
Vocabulary
• atomic radius
• ion
• cation
• anion
• ionization energy
• electronegativity
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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Atomic radii generally
in a period. Atomic size
2
as you move from left to right
with atomic number within a
group because there are more occupied
3
3.
4
The energy required to remove an electron from an atom is
.
4.
5.
energy. This quantity generally
6
as you
6.
move left to right across a period. Ions form when
7
are
7.
than the
7.
known as
5
2.
and an
increased shielding effect, despite an increase in nuclear
1.
8
transferred between atoms. Cations are always
atoms from which they form. The ability of an atom to attract
electrons when it is in a compound is called
value
10
9
, and this
as you move from left to right across a period.
8.
9.
10.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. Compounds are composed of particles called ions.
10
↑
Chapter 6 The Periodic Table
135
05_CTR_ch06 7/9/04 3:27 PM Page 136
11
Name ___________________________
Date ___________________
Class __________________
________ 12. Removing one electron from an atom results in the formation of a
positive ion with a 1 charge.
________ 13. An anion has more electrons than protons.
________ 14. Elements with a high electronegativity value tend to form positive ions.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 15. ion
a. half the distance between the nuclei of two atoms of the
same element when the atoms are joined
________ 16. ionization energy
b. a negatively charged ion
________ 17. electronegativity
c. the energy required to remove an electron from an atom
in its gaseous state
________ 18. atomic radius
d. an atom or group of atoms that has a positive or negative
charge
________ 19. cation
e. a positively charged ion
________ 20. anion
f. the ability of an atom of an element to attract electrons
when the atom is in a compound
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Part D Questions and Problems
Answer the following in the space provided.
21. For the following pairs of atoms, tell which one of each pair has the largest
ionic radius.
a. Al, B
b. S, O
c. Br, Cl
d. Na, Al
e. O, F
22. Indicate which element of the following pairs is the most electronegative.
a. calcium, gallium
b. lithium, oxygen
c. chlorine, sulfur
d. bromine, arsenic
136
Core Teaching Resources
11
↑
05_CTR_ch06 7/9/04 3:27 PM Page 142
Name ___________________________
6
12
Date ___________________
Class __________________
THE PERIODIC TABLE
Chapter Quiz
Fill in the word(s) that will make each statement true.
1. In the modern periodic table, when elements are arranged
1.
1
according to their atomic
, there is a periodic repetition
of properties.
6.1
2.
6.1
3
3. The elements in any
in the periodic table have
similar physical and chemical properties.
3.
6.1
4
4. Oxygen and sulfur, Group 6A elements, have
electrons in their highest occupied energy level.
4.
6.2
5. For the inner transition elements, electrons are added to an
5
f sublevel with a principal energy level that is
than
the period number.
5.
6.2
2. There are
2
periods in the periodic table.
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
6.3
________ 7. For Group 3A elements, there is a relatively small increase in
ionization energy between the second and third ionization energies.
6.3
________ 8. Anions are smaller than the neutral atoms from which they are
formed.
6.3
________ 9. Atoms with low electronegativity values tend to form positive ions.
6.3
________ 10. As a group, alkali metals have the highest electronegativities.
6.3
142
Core Teaching Resources
12
↑
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________ 6. The atomic radius of an element in period 3 is larger that the
atomic radius of an element in period 2.
Name:_____________________________ Date:__________ Period: ________ Answer the following questions while watching the BrainPop video on the Periodic Table 1) How are elements categorized in the Period Table? 2) How are elements listed on the Period Table? 3) Period are ​vertical​ or ​horizontal​ (circle one) on the Periodic Table. 4) Groups are ​vertical​ or ​horizontal​ (circle one) on the Periodic Table 5) Why would Group 1 bond with Group 17 6) Write the characteristics of the following categories: Alkali Metals ­ Alkali Earth Metals ­ Transition ­ Poor ­ Semimetals ­ Non­Metals ­ Nobel Gases 13
Name
Date
Period
Questions About The Periodic Table
1.
2.
3.
4.
5.
6.
7.
Which of the following is a NOBLE GAS?
a.
Oxygen
b.
Nitrogen
c.
Hydrogen
d.
Helium
e.
all of the above are noble gasses
Sodium and Magnesium are both…
a.
alkali metals
b.
alkaline earth metals
c.
metals
d.
non-metals
e.
semi-metals
The family (column) at the far right side of the periodic table are called…
a.
the metallic gasses
b.
the alkaline earth gasses
c.
the noble gasses
d.
the smelly gasses
e.
all of the above
A row in the periodic table (across from left to right) is called a…
a.
period
b.
family
c.
group
d.
semi-family
e.
none of the above
A semi-metal is the same thing as a …..
a.
metal
b.
non-metal
c.
metalloid
d.
semi-non-metal
e.
both a and b above
MALLEABLE means…
a.
breaks easily
b.
is made of non-metals
c.
a mixture of metals
d.
can be bent or pounded into shapes
e.
can be found in a MALL
DUCTILE means …
a.
that a substance is brittle
b.
that a substance easily breaks
c.
that a substance bends
d.
that a substance can be pulled into wires
e.
all of the above
13
14
8.
9.
10.
Cesium is ….
a.
an alkaline earth metal
b.
an alkali metal
c.
a non-metal
d.
a semi-metal
e.
both a and b above
Barium is …
a.
an alkaline earth metal
b.
an alkali metal
c.
a non-metal
d.
a semi-metal
e.
both c and d above
Two or more metals mixed together are called an…
a.
alloy
b.
metal soup
c.
non-metal
d.
metalloid
e.
semi-non-metalloid
CIRCLE True or False on the problems below
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
T
T
T
T
T
T
T
T
T
T
F
F
F
F
F
F
F
F
F
F
An atomic number tells us the number of neutrons in an atom.
Protons are located in the nucleus of an atom
Uranium is a metal
Most elements are non-metals
Metals do not conduct electricity
metalloids are found along the “zig-zag” on the periodic table
metals tend to have very low melting points
There are no metals that are a liquid at room temperature
Calcium is a white powder non-metal found in bones.
All metals conduct electricity.
MATCH THE FOLLOWING ON THE LEFT WITH THE CHOICES ON THE RIGHT
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
Argon
Silicon
Uranium
Antimony
Oxygen
Potassium
Iron
Chlorine
Boron
Mercury
a.
b.
c.
14
metal
non-metal
semi-metal
05_CTR_ch06 7/9/04 3:27 PM Page 137
Name ___________________________
6
15
Date ___________________
Class __________________
THE PERIODIC TABLE
Practice Problems
In your notebook, solve the following problems.
SECTION 6.1 ORGANIZING THE ELEMENTS
1. Which element listed below should have chemical properties similar to
fluorine (F)?
a. Li
b. Si
c. Br
d. Ne
2. Identify each element as a metal, metalloid, or nonmetal.
a. fluorine
b. germanium
c. zinc
d. phosphorus
e. lithium
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3. Which of the following is not a transition metal?
a. magnesium
b. titanium
c. chromium
d. mercury
4. Name two elements that have properties similar to those of the element
potassium.
5. Elements in the periodic table can be divided into three broad classes based
on their general characteristics. What are these classes and how do they
differ?
15
↑
Chapter 6 The Periodic Table
137
05_CTR_ch06 7/9/04 3:27 PM Page 138
Name ___________________________
16
Date ___________________
Class __________________
SECTION 6.2 CLASSIFYING THE ELEMENTS
1. Use the periodic table to write the electron configuration for silicon. Explain
your thinking.
2. Use the periodic table to write the electron configuration for iodine. Explain
your thinking.
3. Which group of elements is characterized by an s2p3 configuration?
4. Name the element that matches the following description.
a. one that has 5 electrons in the third energy level
b. one with an electron configuration that ends in 4s24p5
c. the Group 6A element in period 4
5. Identify the elements that have electron configurations that end as follows.
a. 2s22p4
b. 4s2
c. 3d104s2
6. What is the common characteristic of the electron configurations of the
elements Ne and Ar? In which group would you find them?
7. Why would you expect lithium (Li) and sulfur (S) to have different chemical and
physical properties?
8. What characterizes the electron configurations of transition metals such as
silver (Ag) and iron (Fe)?
SECTION 6.3 PERIODIC TRENDS
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1. Explain why a magnesium atom is smaller than atoms of both sodium and
calcium.
2. Predict the size of the astatine (At) atom compared to that of tellurium (Te).
Explain your prediction.
3. Would you expect a Cl ion to be larger or smaller than an Mg2 ion? Explain.
4. Which effect on atomic size is more significant, an increase in nuclear charge
across a period or an increase in occupied energy levels within a group?
Explain.
5. Explain why the sulfide ion (S2) is larger than the chloride ion (Cl).
6. Compare the first ionization energy of sodium to that of potassium.
7. Compare the first ionization energy lithium to that of beryllium.
8. Is the electronegativity of barium larger or smaller than that of strontium?
Explain.
9. What is the most likely ion for magnesium to form? Explain.
10. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity.
138
Core Teaching Resources
16
↑
18
Image 1
___________________________
First Name, Last ________
Period
SCORE: ___/10 pt
6 Periodicity Formative Assessment 3
Write True or False in the blank.
1.
Image 1, shows Electronegativity an increase from the left to the right. This is due to
more electrons in the nucleus which can pull on electrons harder.
2.
Image 1, shows Ionic Sizes and Shielding to increase from top to bottom of the
Periodic Table. This is because there are more energy levels.
3.
Below in Graph 1, one can observe that atomic radii decreases as we move from
LEFT to RIGHT with in a period or row because of greater proton pull.
4.
In Graph 1, one can observe that atomic radii increase as we move down a column
Or family because there are more energy levels.
5.
In Graph 2, one can observe that ionization energy increases as we move from
Left to right with in a period or row because of more protons pulling electrons.
6.
In Graph 2, one can observe that ionization energy decreases as we move down a
Column or family because of a great atomic radius.
7.
Image 1 Which metal is smallest because of the least amount of energy levels &
more relative protons or nuclear charge?
A.
Li
B.
Be
C.
Na
D.
Ca
8.
Which metal has the lowest ionization energy because of relatively few protons for
its’ energy level and yet the most energy levels?
A.
Rb
B.
Cs
C.
Sr
D.
Ba
9.
Which nonmetal has the highest electro-negativity because of the smallest atomic
radius more protons or nuclear charge?
A.
O
B.
N
C.
S
D.
P
10.
Which nonmetal has the smallest radii because of the most protons (nuclear charge)?
A.
O
B.
N
C.
S
D.
P
Graph 1
Graph 2
18
20
___________________________
First Name, Last ________
Period
SCORE: ___/10 pts
s1
d1
p1
Periodic Table Formative Assessment 1
1.
Which does not fit in because 2 elements do not behave similarly?
a.
groups
b.
family
c.
period
d.
column
2.
Which element is in group 2 and period 4?
a.
Be
b.
Ca
c.
Ti
d.
none correct
Which does not fit in?
a.
family
b.
period
c.
row
d.
energy level
Which is an alkali earth metal?
a.
K
b.
Mg
c.
Sc
d.
Ge
e. Br
Which is a transition metal?
a.
K
b.
Mg
c.
Sc
d.
Ge
e. Br
Which is a metalloid?
a.
K
b.
Mg
c.
Sc
d.
Ge
e. Br
Which in a nonmetal?
a.
K
b.
Mg
c.
Sc
d.
Ge
e. Br
3.
4.
5.
6.
7.
8.
9.
10.
Where are the metals compared to the stair steps?
a.
right
b.
left
c.
on the steps
Where are the inner transition metals?
a.
between the metals & nonmetals
b.
between alkali earth & transitions
Which electron configuration is a noble gas?
a.
1s22s22p6 3s23p6
b.
1s22s22p6 3s23p5
c.
1s2 2s22p6
d.
1s1
e.
more than 1 correct
20
b.
d.
d.
none correct
right of the stair step
none correct