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Modeling Chemistry Unit 11 Packet Page | 1
Name: _____________________
Period: ______
Unit 11 Packet: Periodic Table and Bonding
Packet Contents Sheet (this sheet)
Group and Period Trends- WHY?
With Table of Ionization Energies on the back
Unit 11 Worksheet 1- Ionization Energy
Unit 11 Worksheet 2- Periodic Trends
Periodic Trends Graph (two sided)
Atomic Radii and 1st Ionization Energy Practice w/s
Unit 11 Worksheet 3- Using I.E.
Lewis Dot Diagrams
Unit 11 Worksheet 5- Lewis Structures w/ Valence Electrons on
back
Shapes of Molecules
Polarity Notes/ Polarity of Molecules Practice
Unit 11 Review- two pages
DO NOT, under any circumstances, throw this away!
This packet MUST be saved for the final exam.
Modeling Chemistry Unit 11 Packet Page | 2
Unit 10 – Structure of the Atom - Objectives
Students can analyze data to explain the trends of atomic radii, ion size, ionization
energy, and electronegativity as seen on the periodic table. They will also
understand the role of valence electrons in bonding and can diagram bonding using
Lewis Dot structures and valence shapes.
Scale Score Comment
Score 4 Without any major errors, students can independently: Students can analyze data to compare and contrast the trends of atomic
radii, ion size, ionization energy, and electronegativity as seen on the
periodic table. They will also understand the role of valence electrons in
bonding and can diagram bonding using Lewis Dot structures and valence
shapes.
Score 3 Without any major errors, students can independently: Students can analyze data to explain the trends of atomic radii, ion size,
ionization energy, and electronegativity as seen on the periodic table. They
will also understand the role of valence electrons in bonding and can
diagram bonding using Lewis Dot structures and valence shapes.
Score 2 With one or two major errors, students can independently: Students can describe the trends of atomic radii, ion size, ionization energy,
and electronegativity as seen on the periodic table. They will also
understand the role of valence electrons in bonding and can diagram
bonding using Lewis Dot structures and valence shapes.
Score 1 With help from the teacher, students can: Students can analyze data to explain the trends of atomic radii, ion size,
ionization energy, and electronegativity as seen on the periodic table. They
will also understand the role of valence electrons in bonding and can
diagram bonding using Lewis Dot structures and valence shapes.
Score 0 Even with the teachers help, students show no understanding or ability: Students can analyze data to explain the trends of atomic radii, ion size,
ionization energy, and electronegativity as seen on the periodic table. They
will also understand the role of valence electrons in bonding and can
diagram bonding using Lewis Dot structures and valence shapes.
Modeling Chemistry Unit 11 Packet Page | 3
Group and Period Trends: Why? Bohr Diagrams It is helpful to look at Bohr diagrams of atoms up a group and across a period to understand why the
periodic trends exist. Please draw a Bohr diagram of each of the following atoms in the box indicated
and use the drawings along with the Group and Period Trends Why? activity to determine why the
periodic trends are what they are.
H
Li
B N F
Na
K
Modeling Chemistry Unit 11 Packet Page | 4
HH
eL
iB
eB
CN
OF
Ne
Na
Mg
Al
Si
PS
Cl
Ar
KC
aZ->
12
34
56
78
910
11
12
13
14
15
16
17
18
19
20
1st
13.6
24.6
5.3
99.3
28.3
11.3
14.5
13.6
17.4
21.6
5.1
47.6
55.9
98.1
510.5
10.4
13
15.8
4.3
46.1
1
2n
d54.4
75.6
18.2
25.2
24.4
29.6
35.1
35
41
47.3
15
18.8
16.3
19.8
23.3
23.8
27.6
31.6
11.9
3rd
122
154
37.9
47.9
47.4
54.9
62.7
63.5
71.6
80.1
28.4
33.5
30.2
34.8
39.6
40.7
45.8
50.9
4th
218
259
64.5
77.5
77.4
87.1
97.1
98.9
109
120
45.1
51.4
47.2
53.5
59.8
60.9
67.3
5th
340
392
97.9
114
114
126
138
141
154
167
65
72.6
67.8
75
82.7
84.5
6th
490
552
138
157
158
172
187
190
205
220
88.1
97
91
99.4
109
7th
667
739
185
207
209
225
242
247
264
281
114
124
118
127
8th
871
954
239
264
266
285
304
310
329
348
143
155
147
9th
1103
1196
300
328
330
351
372
380
400
422
176
189
10th
1362
1465
368
399
401
424
448
456
479
504
211
11th
1649
1762
442
476
479
505
529
539
565
592
12th
1963
2086
523
561
564
592
618
629
657
13th
2304
2437
611
652
657
686
715
727
14th
2673
2817
707
750
756
787
818
15th
3070
3224
809
855
861
895
16th
3494
3658
918
968
974
17th
3946
4120
1033
1087
18th
4426
4611
1158
19th
4934
5129
20th
5470
Modeling Chemistry Unit 11 Packet Page | 5
Name
Date Pd
Chemistry – Unit 11 Worksheet 1 Ionization energy
Plot graphs of successive ionization energies for B, Si, and Ca.
1. Compare the graphs – what are the common features? What are the
differences?
2. Group the electrons for each element based on ionization energies. How many
electrons are in each group? You can change the scale of the vertical axis to
better differentiate between groups.
3. Is there a maximum number of electrons that can fit in each group? If so,
what is it?
4. Plot graphs of successive ionization energies for a few more atoms. Does the
evidence support your answer to #3?
5. Summarize the patterns you found in the table of successive ionization
energies.
Modeling Chemistry Unit 11 Packet Page | 6
Name
Date Pd
Chemistry – Unit 11 – Worksheet 2 Periodic trends
1. Using the data in the table of ionization energies, plot the first ionization energy
(IE1) vs. the atomic number (Z) for the first 20 elements.
2. Using the data in the table on the 2nd sheet in the workbook, plot the atomic
radius (in nm) vs. the atomic number.
Conclusion 1. Examine the graph of 1st ionization energy vs atomic number. Can a periodic
trend be observed? If so, describe the trend.
2. Which group (or chemical family) has the highest ionization energies? Which
group has the lowest?
3. Examine the graph of atomic radius vs atomic number. Can a periodic trend be
observed? If so, describe the trend.
4. For a given period (a row in the Periodic Table), which group (a column in the
table) appears to have the largest atomic radii? Which group has the smallest?
5. What appears to be the relationship between trends in IE and atomic radii?
Modeling Chemistry Unit 11 Packet Page | 7
Extension Draw energy well diagrams for B, N, F and Na, Use these diagrams to explain the
trend in 1st ionization energy as you move across a period. Explain why IE1 for sodium is so much lower than it is for fluorine.
Now, use these diagrams to explain the trend in atomic radii as you move across a
period. Explain why fluorine is smaller than oxygen, yet sodium is not smaller yet than fluorine.
Modeling Chemistry Unit 11 Packet Page | 10
Atomic Radii and 1st Ionization Energy Practice
1. Define atomic radius.
2. Define 1st ionization energy.
3. What is the trend for atomic radii and 1st ionization energy as you go up a group and across a
period?
4. Why does the trend up a group for atomic radii exist?
5. Why does the trend across a period for atomic radii exist?
6. Why does the trend up a group for 1st ionization energy exist?
7. Why does the trend across a period for 1st ionization energy exist?
Atomic Radii 1st Ionization
Energy
Modeling Chemistry Unit 11 Packet Page | 11
8. Arrange the following elements in order of increasing atomic size: Nitrogen, Fluorine ,
Lithium, Carbon
9. Arrange the following elements in order of increasing ionization energy
a. B, N, Li
b. Mg, Na , Cl
c. Li, O, B, F
10. In each of the following pairs of elements, circle the element that is the largest.
a. Br, F
b. Na, K
c. Ne, Be
d. Ca, As
11. Which group has the highest ionization energy? Why?
12. Which group has the lowest ionization energy? Why?
13. In the space following each element below, list the charge of the ion it will form.
a. Be_________ b. Cl___________ c. Ne________ d. S_________
Modeling Chemistry Unit 11 Packet Page | 12
Name
Date Pd
Chemistry – Unit 11 Worksheet 3
Element
name
#
valence
electrons
First
ionization
energy
(eV)
Attraction
to the
nucleus:
Weak (<
7.8) Strong
(> 10)
Can it
become
a
positive
ion?
If yes –
how
many
electrons
can be
easily
lost?
Can it
become
a
negative
ion?
If yes –
how
many
additional
electrons
can it pull
strongly?
What
ion will
be
formed?
Lithium
Sodium 1 5.1 Weak Yes 1 No – Na+
Potassium
Fluorine
Chlorine 7 13.0 Strong No – Yes 1 Cl-
Bromine 11.8
Iodine 10.5
Helium 2 24.6 Strong No – Yes 0 –
Neon
Argon
Krypton 14.0
Carbon 4 11.3 Strong No – Yes 4 C
4-
(rare)
Silicon 4 8.2 Intermediate No – No – –
Germanium 7.9
Tin 7.3 Sn
2+,
Sn4+
Lead 7.4 Pb
2+,
Pb4+
Modeling Chemistry Unit 11 Packet Page | 13
Element
name
#
valence
electrons
First
ionization
energy
(eV)
Attraction
to the
nucleus:
Weak (<
7.8)
Strong (>
10)
Can it
become
a
positive
ion?
If yes –
how
many
electrons
can be
easily
lost?
Can it
become
a
negative
ion?
If yes –
how
many
additional
electrons
can it
pull?
What
ion will
be
formed?
Beryllium
Magnesium Mg2+
Calcium
Strontium 5.7
Oxygen
Sulfur S2-
Selenium 9.8
Tellurium 9.0
Boron
Aluminum
Gallium 6.0
Nitrogen
Phosphorus
Arsenic 9.8
Antimony 8.6
Bismuth 7.4 Bi3+
Modeling Chemistry Unit 11 Packet Page | 16
Name
Date Pd
Chemistry – Unit 11 Worksheet 5 Lewis structures
Sketch Lewis dot diagrams for the following molecules.
1. CH4 2. H2O
3. NF3 4. H2O2
5. C2H6 6. C2H4
7. C2H2 8. HCN
9. CH3OCH3 10. CH3CH2OH
11. CH3COOH 12. CH2O2
Modeling Chemistry Unit 11 Packet Page | 21
Chemistry – Unit 11 Review
Periodic Trends 1. Arrange the following elements in order of decreasing atomic size (from largest to
smallest): sulfur, chlorine, aluminum, and sodium. Why does this trend exist? 2. Arrange the following elements in order of increasing first ionization energy (from
smallest to largest), and explain why this trend exists. a. Be, Mg, Sr b. Bi, Cs, Ba
3. In each of the following pairs of elements, identify the element that is the most
electronegative, and explain why this trend exists. a. chlorine, fluorine b. carbon, nitrogen
4. In each of the following pairs of elements, identify the atom or ion that is the largest
in size and explain why. a. Li or Li+ b. F or F¯
5. List the charge of the ion that each element below will form.
a. Al b. B c. Ar d. S e. I f. Mg
Modeling Chemistry Unit 11 Packet Page | 22
6. Sketch the trends up a group and across a period for the following: a. Atomic Radius b. Ionization Energy c. Electronegativity
7. What happens to the size of the ion compared to the neutral atom when an atom
loses electrons to form an ion?
Valence Model and Structural Formulas 8. Nitrogen has how many valence electrons?
a. –3
b. 2
c. 5
d. +4
9. What is a valence electron?
10. Draw the structural formulas for the following compounds:
a. C2O2
b. CH3OCH3
c. HCN
Modeling Chemistry Unit 11 Packet Page | 23
Lewis Model Compare and contrast ionic and covalent bonds in terms of:
a. What happens to electrons
b. Shape
What type of bond do the following Lewis Dot Structures Represent?
Draw Lewis Dot Structures to show what happens to electrons when the following
elements form ionic compounds (Hint: Write the formula first) Ca + Br
Mg + O
Draw Lewis Dot Structures to show what happens to electrons in the following covalent
bonds:
F2
N2
CO2
VSEPR and Polarity Draw, name the VSPER shapes and identify as polar or nonpolar the following compounds: NH3 CHCl3 CO2
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