Download Periodicity Group Project

Periodicity Group Project:
You will be working with your lab table to complete this assignment by creating and leading a 10 minute
instructional class on your topic. Each lab table will be assigned a different topic. Topics and the order of
presentations will be:
Coulombic Attraction
Shielding
Atomic Radius
Ionization Energy
Electronegativity
Electron Affinity
Ionic Radius – (no trends – compare atom to cation and atom to anion) – this is for classes with 13 lab
groups)
Directions: Complete the questions for your topic and design a class instructional presentation that is under 10
minutes. Instruction must include visuals and a student handout/worksheet and answer key. All presentations
must include a clever way to help someone remember the trend and why the trend happens along with
anomalies.
Rubric: Total 105
_____ 3 pts
1. Student contributed to team success as determined anonymously by team members
with a 1-3 ranking and explanation.
_____5 pts
2. Pre presentation worksheet completed by team (1submittal per team)
_____ 5 pts
3. Student worksheet with accurate key (1 submittal per team; evening prior to
presentation, so that copies may be made.)
_____5 pts
4. Class presentation and worksheet never refer to octet rule or achieving Noble gas configuration.
_____5 pts
5. Class presentation included visuals
_____ 4pts
6. Each student contributed equally in the class instruction.
_____10pts
7. Student presentation includes having class students engage in activity/worksheet to
learn the material (Note, the whole presentation including student worksheet should not take more than 10
min, so worksheets must include big idea – takeaway with trends and comparisons of elements to apply trends.
_____ 10 pts 7. Presenters checked student work to ensure content knowledge correct and worksheet complete to
serve as a study guide.
_____ 3 pts
8. Average of anonymous class evaluation of presentation in terms of how well the student learned the
material form their presentation: 1 poor; 2 good; 3 excellent
_____ 55 pts
Post Activity Questions - each person must submit
Coulombic Attraction Team members
_____________________,_________________,_______________,________________,______________
1. Define Coulombic Attraction in your own words:
2. Why does F have higher Coulombic Attraction than Li?
3. Why does I have Iower Coulombic Attraction than F?-
4. Explain differences in Coulombic Attraction in terms of the following diagrams
Protons at the
nucleus
Electrons in
orbit
(Helium atom)
5. Draw Bohr models using atomic radius to show relative size, showing Coulombic Attraction for Li, Be,
and F and explain what is happening and the trend we observe
6. Describe the Coulombic Attraction trends we observe on the periodic table
7. Fill in the blanks: Coulombic Attraction – The force of attraction between oppositely charged particles
such as__________ and _____________. Two main trends for Coulombic Attraction between the
nucleus and the valence electrons. If two elements are not in the same family, but are in the same
horizontal period, then the number of __________________ in the nucleus is the dominant factor. As
we move across and down the periodic table the number of ______ increases. The more protons in
the nucleus, the ____________the force of Coulombic Attraction.
As a team, create your class presentation, presentation visuals, and student worksheet and answer key.
The worksheet should include 2 questions each comparing 4 elements with drawings.
Shielding Team members
_____________________,_________________,_______________,________________,______________
1. Define Shielding in your own words:
2. Draw Nobel gas configurations for Li and F. Circle the core electrons with one color and the valance
electrons with another color. Label the core and the valance electrons with a legend.
3. Which electrons are creating the shield: core or valence electrons?
4. When comparing Li and F, are the core electrons the same or different?
5. What shielding trend do we observe as we go across the periodic table?
6. Draw Nobel gas configurations for F and I. Circle the core electrons with one color and the valance
electrons with another color. Label the core and the valance electrons with a legend.
7. Which electrons are creating the shield: core or valence electrons?
8. When comparing F and I, are the core electrons the same or different? Hint: Write the Noble gas
configurations
9. What shielding trend do we observe as we go down the periodic table?
10. The more completed Energy Levels (solar system rings on Bohr’s model) that atoms have, the
farther away the valence electron(s) are from the protons in the nucleus, the _______the Shielding
will be. If two elements are in the same period, electrons are added to the same energy level, thus
the shielding remains the _____________. When elements are in the same group and you go down
the periodic table, both Coulombic attraction and Shielding are increasing, but shielding has the
greater effect, therefore the net pull on the electrons is reduced. For example, consider Li and Na,
who has more Coulombic Attraction?________. Who has more Shielding?_____Whose electrons
feel the greater pull? _____. Right, Li because the effect of Shielding is greater than effect of
Coulombic Attraction.
As a team, create your class presentation, presentation visuals, and student worksheet and answer key.
The worksheet should include 2 questions each comparing 3 elements with Noble gas configurations.
Atomic Radius Team members
_____________________,_________________,_______________,________________,______________
1. Define Atomic Radius in your own words:
2. Fill in the following table:
Li
Be
B
C
N
O
F
Noble Gas
configuration
Atomic
Radius
3. What do we notice about the electron configurations as we move across a period? (What remains
constant? What changes?)
4. What trend in atomic radius do you see as you go across the periodic table?
5. Explain how Coulombic Attraction and Shielding influence atomic radius. (You must address both in
your explanation.)
6. Fill in the following table:
Element
Noble gas configuration
Atomic Radius
Li
Na
K
Rb
Cs
Fr
7. What trend in atomic radius do you see as you go down the periodic table

What do we notice about the electron configurations as we move down a group? What remains
constant? What changes?)
8. Explain how Coulombic Attraction and Shielding influence atomic radius. (You must address both in
your explanation.)
As a team, create your class presentation, presentation visuals, and student worksheet and answer key.
The worksheet and or presentation should include questions that compare the following: H and Cs; S and F; Li.
Si, and Te; Na and Cl. Worksheet should include drawings showing relative atomic radius and require students
to write the Noble gas configurations.
Ionization Energy Team members
_____________________,_________________,_______________,________________,______________
1. Define ionization energy in your own words:
2. Fill in the following table:
Li
Be
B
C
N
O
F
Noble Gas
configuration
The first ion
that forms
when an
electron is
lost
Ionization
energy, IE1
3. What do we notice about the electron configurations as we move across a period? (What remains
constant? What changes?)
4. What trend in ionization energy do you see as you go across the periodic table
5. What anomalies did you observe? Between what 2 atoms do they occur?
6. How can the anomalies be explained? Hint: Draw electron orbital diagrams for each.
7. Be able to write an equation to show the first, second and third ionizations of an element.
a. Compare IE1 to IE2 to IE3
b. Why is there a large increase in IE3 for Mg?
8. Fill in the following table:
Element
Noble gas configuration
Ion when the first
electron is lost
Ionization Energy, IE1
Li
Na
K
Rb
Cs
Fr
9. What do we notice about the electron configurations as we move down the periodic table? (What
remains constant? What changes?)
10. What trend in ionization energy do you see as you go down the periodic table? Explain this in terms of
Coulombic Attraction and Shielding.
As a team, create your class presentation, presentation visuals, and student worksheet and answer key. The
worksheet should include 2 questions each comparing 4 elements with noble gas configurations
/drawings/charts. Worksheet should provide drawings showing relative atomic radius and require students to
write the Noble gas configurations. Worksheet should include these pairs: Li and F; Mg and P; C and Ge, O and
Se.
Electronegativity Team members
_____________________,_________________,_______________,________________,______________
1. Define electronegativity in your own words:
2.
Fill in the following table:
Li
Be
B
C
N
O
F
Noble Gas
configuration
Electronegativity
3. What do we notice about the electron configurations as we move across a period? (What remains
constant? What changes?)
4. What trend in electronegativity do you see as you go across the periodic table? Account for this in terms
of Coulombic Attraction and Shielding.
5. Fill in the following table:
Element
Noble gas configuration
Electronegativity
Li
Na
K
Rb
Cs
Fr
6. What do we notice about the electron configurations as we move down the periodic table? (What
remains constant? What changes?)
7. What trend in electronegativity do you see as you go down the periodic table
8. Explain why the trend occurs in terms of Coulombic attraction and Shielding.
9. Fill in the blanks : Electronegativity reflects an atom’s ability to _______________ electrons involved in
a covalent bond. Coavlent bonds are formed between two ___________. The higher the EN value, the
____________ the ability of the atom to pull electrons in a covalent bond towards its nucleus. The
lower the EN value, the ____________ the ability of the atom to pull electrons in a coavalent bond
towards its nucleus.
As a team, create your class presentation, presentation visuals, and student worksheet and answer
key.The worksheet should include 2 questions each comparing 4 elements with noble gas configurations
/drawings/charts. Worksheet should provide drawings showing relative atomic radius and require
students to write the Noble gas configurations. Worksheet should include C-F; F-I; N-O; O-Se; and Cl-O
as a challenge question.
Electron Affinity Team members
_____________________,_________________,_______________,________________,______________
1. Define electron affinity in your own words:
2. Fill in the following table:
Li
Be
B
C
N
O
F
Noble Gas
configuration
Ion it forms
when
accepting
one electron
Electron
Affinity
3. What do we notice about the electron configurations as we move across a period? (What remains
constant? What changes?)
4. What trend in electron affinity do you see as you go across the periodic table? Explain this in terms of
Coulombic Attraction and Sheilding.
5. Fill in the following table:
Element
Noble gas configuration
Ion it forms when
accepting one electron
Electron affinity
Li
Na
K
Rb
Cs
Fr
6. What do we notice about the electron affinity as we move down the periodic table? (What remains
constant? What changes?)
7. What trend in electron affinity do you see as you go down the periodic table? Explain this in terms of
Coulombic Attraction and Shielding.
As a team, create your class presentation, presentation visuals, and student worksheet and answer key. The
worksheet should include 2 questions each comparing 4 elements with noble gas configurations
/drawings/charts. Worksheet should include comparisons of Li and F; C and O; N and As; F and I.
Ionic Radius Team members
_____________________,_________________,_______________,________________,______________
1. Define what ionic radius refers to in your own words:
2. Fill in the following table:
Li
Be
B
C
N
O
Ion it forms
Atomic radius
Ionic Radius
3. Can you accurately predict which elements will likely form cations? Explain Why.
4. Can you accurately predict which elements will likely form anions? Explain Why.
F
5. Fill in the following table:
Element Noble gas configuration
Ion it forms
Atomic radius
Ionic Radius
Li
Na
K
Rb
Cs
Fr
6. What is the trend between atomic radius and ionic radius for cations? Why? Explain why without
mentioning octets or achieving Noble Gas configuration.
7. What is the trend between atomic radius and ionic radius for anions? Why? Explain why without
mentioning octets or achieving Noble Gas configuration.
8. Does this hold true for all ions?
As a team, create your class presentation, presentation visuals, and student worksheet and answer key. The
worksheet should include 2 questions each comparing 2 elements that form cations and 2 elements that form
anions with drawings/charts. Specifically, compare Cl and Cl- and Na and Na+ showing the relative size of the
ionic radius and ask for an explanation why the ionic radi are what they are.
Post Activity Questions:
Name: _________________________
Honors Chemistry: The Periodic Table and Periodicity
Directions: Answer each of the following questions. You need not use complete sentences.
1.
Who first published the classification of the elements that is the basis of our periodic table today?
2.
By what property did Mendeleev arrange the elements?
3.
By what property did Moseley suggest that the periodic table be arranged?
4.
What is a period? How many are there in the periodic table?
5.
What is a group (also called a family)? How many are there in the periodic table?
6.
State the number of valence electrons in an atom of:
a. sulfur
7.
10.
d. arsenic
b. Na and Li
c. Na and Cu
d. Na and Ne
Which of the following pairs of elements belong to the same group?
a. H and He
9.
c. chlorine
Which of the following pairs of elements belong to the same period?
a. Na and Cl
8.
b. calcium
b. Li and Be
c. C and Pb
d. Ga and Ge
How does an element’s period number relate to the number of the energy level of its valence
electrons?
What are the transition elements?
11.
Would you expect strontium to be, chemically, more similar to calcium or rubidium and WHY?
12.
In going from top to bottom of any group, each element has ______ more occupied energy level(s)
than the element above it.
13.
What are the Group 1 elements called?
14.
What are the Group 2 elements called?
15.
What are the Group 17 elements called?
16.
What are the Group 18 elements called?
17.
Which alkali metal belongs to the sixth period?
18.
Which halogen belongs to the fourth period?
19.
What element is in the fifth period and the eleventh group?
20.
Why do all the members of a group have similar properties?
21.
What do we mean by “atomic radius?” How is atomic radius actually measured? Why don’t we
measure from nucleus to outer electron?
22.
Within a group, what happens to the atomic radius as you go down the column?
23.
Explain your answer to Question 22 in terms of Coulobmic Attraction and Shielding: Why does the
atomic radius change?
24.
What is coulombic attraction?
25.
Within a period, what happens to the atomic radius as the atomic number increases?
26.
Explain your answer to Question 25 in terms of Coulobmic Attraction and Shielding: Why does the
atomic radius change?
27.
What two factors determine the net effect of coulombic attraction?
28.
What is the shielding effect?
29.
How are the shielding effect and the size of the atomic radius related?
30.
How are neutral atoms converted into cations?
31.
How are neutral atoms converted into anions?
32.
Metals usually form what type of ions?
33.
Nonmetals usually form what type of ions?
34.
What is ionization energy?
35.
What is the equation that illustrates ionization energy, and what does each symbol represent?
36.
What do we mean by the first, second, and third ionization energies for a particular atom?
37.
Why does each successive ionization require more energy than the previous one?
38.
What is the general trend of ionization energy as you go from left to right across the periodic table?
39.
What is the general trend of ionization energy as you go down a group on the periodic table?
40.
Which of these elements has the highest first ionization energy: Sn, As, or S?
41.
When an atom becomes an anion, what happens to its radius?
42.
When an atom becomes a cation, what happens to its radius?
43.
For each of the following pairs, circle the atom or ion having the larger radius.
a. S or O
c. Na or K+
b. Ca or Ca2+
d. F or F1–
44.
For each of the following pairs, identify the smaller ion.
C4+ or C4–
45.
Where, generally, are the metals located on the periodic table?
46.
Where, generally, are the nonmetals located on the periodic table?
47.
List three physical properties of metals.
48.
List three physical properties of nonmetals.
49.
What kinds of properties do metalloids have?
50.
What is electronegativity?
51.
Who determined the scale of electronegativity most often used today?
52.
List the following atoms in order of increasing electronegativity: C, Se, F
53.
List the following atoms in order of decreasing electronegativity: Si, Sl, O
54.
What is the general trend of electronegativity as you go down the periodic table?
55.
What is the general trend of electronegativity as you go left to right across the periodic table?
KEY
Chemistry: The Periodic Table and Periodicity
Directions: Answer each of the following questions. You need not use complete sentences.
1.
Who first published the classification of the elements that is the basis of our periodic table today?
DMITRI MENDELEEV
2.
By what property did Mendeleev arrange the elements?
ATOMIC MASS
3.
By what property did Moseley suggest that the periodic table be arranged?
ATOMIC NUMBER
4.
What is the periodic law?
THE PROPERTIES OF THE ELEMENTS REPEAT PERIODICALLY
5.
What is a period? How many are there in the periodic table?
A HORIZONTAL ROW IN THE PERIODIC TABLE; 7
6.
What is a group (also called a family)? How many are there in the periodic table?
A VERTICAL COLUMN IN THE PERIODIC TABLE; 18
7.
State the number of valence electrons in an atom of:
a. sulfur
6
8.
10.
c. chlorine
d. arsenic
7
5
Give the names and chemical symbols for the elements that correspond to these atomic numbers:
a. 10
Ne, NEON
9.
b. calcium
2
b. 18
Ar, ARGON
c. 36
Kr, KRYPTON
d. 90
Th; THORIUM
List, by number, both the period and group of each of these elements.
Symbol
Period
Group
a. beryllium
Be
2
2
b. iron
Fe
4
8
c. lead
Pb
6
14
Which of the following pairs of elements belong to the same period?
a. Na and Cl
11.
b. Na and Li
c. Na and Cu
d. Na and Ne
Which of the following pairs of elements belong to the same group?
a. H and He
b. Li and Be
c. C and Pb
d. Ga and Ge
12.
How does an element’s period number relate to the number of the energy level of its valence
electrons?
PERIOD NUMBER = ENERGY LEVEL OF VALENCE ELECTRONS
13.
What are the transition elements?
GROUPS 3-12
14.
In what type of orbitals are the actinide and lanthanide electrons found?
f-ORBITALS
15.
Would you expect strontium to be, chemically, more similar to calcium or rubidium and WHY?
Ca; BOTH Ca AND Sr HAVE TWO VALENCE ELECTRONS
16.
What are the coinage elements?
GROUP 11; Cu, Ag, Au
17.
What is the heaviest noble gas? What is the heaviest alkaline earth metal?
RADON (Rn); RADIUM (Ra)
18.
In going from top to bottom of any group, each element has ONE more occupied energy level(s) than
the element above it.
19.
What are the Group 1 elements called?
ALKALI METALS
20.
What are the Group 2 elements called?
ALKALINE EARTH METALS
21.
What are the Group 17 elements called?
HALOGENS
22.
What are the Group 18 elements called?
NOBLE GASES
23.
What is the name given to the group of elements that have the following valence shell electron
configurations?
a. s2
b. s2p6
c. s2p5
d. s1
ALKALINE EARTH METALS NOBLE GASES HALOGENS
ALKALI METALS
24.
List the three lightest members of the noble gases.
He, Ne, Ar
25.
List all of the alkali metals.
Li, Na, K, Rb, Cs, Fr
26.
Which alkali metal belongs to the sixth period?
Cs
27.
Which halogen belongs to the fourth period?
Br
28.
What element is in the fifth period and the eleventh group?
Ag
29.
Why do all the members of a group have similar properties?
THEY HAVE THE SAME NUMBER OF VALENCE ELECTRONS
30.
What do we mean by the “atomic radius?” THE SIZE OF A NEUTRAL ATOM
31.
Within a group, what happens to the atomic radius as you go down the column?
INCREASES
32.
Explain your answer to Question 31: Why does the atomic radius change?
ELEMENT BELOW HAS ONE MORE ENERGY LEVEL THAN ELEMENT ABOVE
33.
What is coulombic attraction?
ATTRACTION OF (+) AND (–) CHARGES
34.
Within a period, what happens to the atomic radius as the atomic number increases?
DECREASES
35.
Explain your answer to Question 34: Why does the atomic radius change?
NO ADDITIONAL ENERGY LEVELS, BUT MORE (+) AND (–) CHARGES = MORE PULL
36.
What two factors determine the strength of coulombic attraction?
AMOUNT OF CHARGE; DISTANCE BETWEEN CHARGES
37.
What is the shielding effect? KERNEL ELECTRONS “SHIELD” VALENCE ELECTRONS FROM
ATTRACTIVE FORCE OF THE NUCLEUS; CAUSED BY KERNEL
AND VALENCE ELECTRONS REPELLING EACH OTHER
38.
How are the shielding effect and the size of the atomic radius related?
AS RADIUS INCREASES, SHIELDING EFFECT INCREASES
(MORE SHELLS OF KERNEL e– TO REPEL VALENCE e–)
39.
How are neutral atoms converted into cations?
anions?
LOSE ELECTRONS
40.
ACQUIRE ELECTRONS
Metals usually form what type of ions?
CATIONS
41.
How are neutral atoms converted into
Nonmetals usually form what type of ions?
ANIONS
What is ionization energy?
THE ENERGY REQUIRED TO REMOVE AN ELECTRON FROM AN ATOM
42.
What is the equation that illustrates ionization energy, and what does each symbol represent?
M (g) + ionization energy  M1+(g) + e–
43.
What do we mean by the first, second, and third ionization energies for a particular atom?
ENERGY REQ’D TO REMOVE THE 1ST, 2ND, AND 3RD ELECTRONS
44.
Why does each successive ionization require more energy than the previous one?
(+) NUCLEUS HOLDS ON TIGHTER TO THE FEWER REMAINING ELECTRONS
45.
What is the general trend of ionization energy as you go from left to right across the periodic table?
INCREASES
46.
What is the general trend of ionization energy as you go down a group on the periodic table?
47.
DECREASES
Which of these elements has the highest first ionization energy: Sn, As, or S?
S
48.
When an atom becomes an anion, what happens to its radius?
BECOMES LARGER
49.
When an atom becomes a cation, what happens to its radius?
BECOMES SMALLER
50.
For each of the following pairs, circle the atom or ion having the larger radius.
a. S or O
c. Na1+ or K1+
b. Ca or Ca2+
d. Na or K
e. S2– or O2–
f. F or F1–
51.
52.
For each of the following pairs, identify the smaller ion.
a. K1+ or Ca2+
c. C4+ or C4–
e. O2– or F1–
b. F1– or Cl1–
d. S2– or F1–
f. Fe2+ or Fe3+
Where, generally, are the metals located on the periodic table?
ON THE LEFT
53.
Where, generally, are the nonmetals located on the periodic table?
ON THE RIGHT
54.
A.
B.
C.
55.
List some properties of metals.
GOOD CONDUCTORS; MALLEABLE; DUCTILE; LUSTROUS SOLIDS
List some properties of nonmetals.
GOOD INSULATORS; DULL, BRITTLE SOLIDS (OR GASES)
What kinds of properties do metalloids have?
PROPERTIES OF BOTH METALS AND NONMETALS
What is electronegativity?
THE TENDENCY FOR AN ATOM TO ATTRACT ELECTRONS TO ITSELF
56.
Who determined the scale of electronegativity most often used today?
LINUS PAULING
57.
List the following atoms in order of increasing electronegativity: O, Al, Ca
Ca < Al < O
58.
List the following atoms in order of decreasing electronegativity: Cl, K, Cu
Cl > Cu > K
59.
What is the general trend of electronegativity as you go down the periodic table?
DECREASES
60.
What is the general trend of electronegativity as you go left to right across the periodic table?
INCREASES