do not, under any circumstances, throw this away! this

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.


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,




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,





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


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


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.


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?


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.


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


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_________


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+


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+


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


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


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


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

do not, under any circumstances, throw this away! this

Documents