Periodic Table

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Learning Objectives

After completing this unit of study, you should be able to: An element’s location on the periodic table gives an indication of its physical and

chemical properties. Elements on the Periodic Table are arranged in order of increasing atomic number. Elements are classified as metals, nonmetals and metalloids based on their

properties and location on the periodic table. Groups 1, 2, and 13-18 have the same number of valence electrons in the group,

and therefore have similar chemical properties. Helium is the exception to this. Each group shows trends in atomic radius, ionic radius, Electronegativity, first

ionization energy, and metallic and nonmetallic properties. Each period shows trends in atomic radius, Electronegativity, first ionization energy,

and metallic and nonmetallic properties. When an element becomes an anion by gaining electrons, the radius increases. When an element becomes a cation by losing electrons, the radius decreases. Some elements exist as two or more forms in the same phase due to differences in

molecular or crystal structures, and therefore have different chemical and physical properties. These are called Allotropes. Carbon has the allotropes coal, graphite, diamond, and fullerenes. Oxygen has the allotropes O2 & O3.

The Periodic Table – A Different Way of Doing Things.

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During the Periodic Table Unit, you will be working with some of your colleagues in a cooperative group. As with many things we do, some of you will love it and some of you will not. However, this is an important skill for you to develop as you approach life after high school. Our goal is to see you work as a team, using the strengths of all your team members and building on areas that may need improvement. With this in mind, here is the layout for this unit.

1. With each new topic within the unit, you will be assigned a learning guide. You will answer the questions from the learning guide independently using your review book or other printed sources.2. I will go over the contents of the learning guide with the entire class the following day.3. You will afterwards break into assigned groups of 3-4 students to complete an activity called a ChemDo. I will collect activities from all the students, but I will select one randomly to grade. Each member of the group will receive this same grade. This means it is in the best interest of the group to work together and make sure all members understand.4. After the ChemDo has been collected, there will be a 5-10 point quiz on the information in the learning guides and Chemdo the following day. As an incentive, all groups whose members receive 100 % on the quiz will get an extra point(s), No extra points will be assigned unless all members of the group get 100% on the quiz. It is your job to let me know if this occurs.5. The test for this unit will be broken up into two parts, multiple choice and short answer. You will each complete the multiple-choice portion independently, but the group will have the opportunity to complete the short answer questions together. As before, one test will be chosen at random to grade and you will receive that grade as a group.

I look forward to this opportunity to work with all of you in a new and different way. Please contact me if you have problems with your group. While I will consider individual situations, I expect you to work professionally with all members of your group

Vocabulary3

Use your review book to write the definitions for each term listed below:

1. Chemical Property

2. Physical Property

3. Atomic Number

4. Metal

5. Nonmetal

6. Metalloid

7. Metallic Character

8. Valence Electrons

9. Atomic Radius

10. Ionic Radius

11. Electronegativity

12. First Ionization Energy

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13. Allotrope

14. Alkali Metals

15. Alkaline Earth Metals

16. Halogens

17. Noble Gases

18. Transition Metals

19. Shielding Effect

20. Period

21. Group

22. Periodic Law

23. Nuclear Charge

24. Malleable

25. Ductile

26. Luster

27. Cation

28. Anion

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Name ________________________________________Period_________________________

Date__________________________Use Review Book Pages 77-95

1. What was Dimitri Mendeleev’s method for creating the first Periodic Table?

2. What was the problem with Mendeleev’s Periodic Table?

3. How was Mosley’s Periodic Table different from Mendeleev’s?

4. Complete the chart below.***Fill in the labels for a square from the periodic table***

5. What is a period?

6. What do all elements in a period have in common?

7. How does the number of valence electrons change as you move across a period?

8. Where are metals located on the Periodic Table?

9. Where are nonmetals located on the Periodic Table?

10. Where are metalloids located on the Periodic Table?

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P 30.97376 -3

+3

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11. Which elements on the Periodic Table are liquids?

12. Which elements on the Periodic Table are solids?

13. Which elements on the Periodic Table are gases?

14. What is a group on the Periodic Table?

15. Another name for a group is ___________________________________.

16. All elements in a group have the same number of _____________________.

17. All elements in a group have similar _______________________________.

18. Complete the following Table:Symbol Name Atomic # Period GroupPb

Potassium45

Iron3 17

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19. Answer the following questions in the Review Book: Page 83: 1-4,16 Page 84: 16 Page 94: 1,11,12 Page 95: 13

Name ________________________________________ Period_________________________Date__________________________Page 80-87, 99-100 and old notes

1. Why are nonmetal ions larger than the atoms from which they form?8

Metals NonmetalsLocation on Periodic TablePhysical Properties-8 for metals-6 for nonmetals

Do they Gain or Lose Electrons?

Do they Form Anions or Cations?

Are the ions they form larger or smaller than atom?Do they Conduct heat & electricity?

Are their Ionization Energies high or low?Are their Electronegativities high or low?Location of Most Active Elements

2. Why are metal ions smaller than the atoms from which they form?

3. In which groups are the transition metals located?

4. What are two unique characteristics of transition metals?

5. What are metalloids?

6. Where are metalloids located?

7. Noble gases are another unique group on the Periodic Table. Where are they located?

8. What makes the noble gases unique?

9. What is an allotrope?

10. What elements exist as allotropes?

11. Answer the following questions in your Review Book:Page 84: 5-29

Metals, Nonmetals, Semimetals(Metalliods)

On the periodic table below, color the metals yellow, the metalloids green, and the

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nonmetals blue:

Property METAL SEMIMETAL NONMETAL

LOCATION

LUSTER – SHINY?

CONDUCTIVE OFHEAT & ELECTRICITY?

MALLEABLE – can bend without breaking?

PHYSICAL STATE at RT?

Important examples:

GENERAL ATOMIC STRUCTURE

TENDENCY TO LOSE OR TO GAIN ELECTRONS?

# OF VALENCE ELECTRONS

Name ______________________________________ Period_________________________10

Date__________________________

Pages 85-86, 100,

1. Define/explain nuclear charge.

2. Define/explain shielding.

3. Define ionization energy.

4. As you go left to right across a period nuclear charge___________________, electrons are __________________ attracted and more/less (circle one) energy is needed to remove them.

5. As you go top to bottom down a group valence electron are ____________________ from the nucleus and it is easier/harder(circle one) to remove them

6. Define atomic radius.

7. As you move across a period on the Periodic Table, atomic radius increases / decreases. (circle one)

8. How does nuclear charge cause the atomic size to change as atomic number increases in a period on the Periodic Table?

9. Why is the shielding effect constant in the same period on the Periodic Table?

10. As you move down a group in the Periodic Table, atomic radius increases / decreases. (circle one)

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11. How does the number of occupied principal energy levels(shells) change as atomic number increases in a group on the Periodic Table?

12. How does shielding cause atomic size to change as atomic number increases in a group on the periodic table?

13. Define ion(p100).

14. Define ionic radius.

15. Metals tend to lose/gain(circle one) electrons to form an ion therefore the radius of a metallic ion is smaller/larger(circle one) than the atom.

16. Nonmetals tend to lose/gain(circle one) electrons to form an ion therefore the radius of a nonmetallic ion is smaller/larger(circle one) than the atom.

17. Define electronegativity.

18. Which element has the lowest electronegativity value?

19. Which element has the highest electronegativity value?

20. Answer the following questions in your review book:Page 91:Questions 39-42Page 93: Questions 76

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INSERT BOHR MODELS PAGE HERE!!!

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Name ________________________________________ Period_________________________Date__________________________

Use pages 87 – 90 in your Review Book.

1. Look at each group(column) in the periodic table what changes in the electron configuration as you go down the group?

2. Look at each group(column) in the periodic table what stays the same in the electron configuration as you go down the group?

3. Why do elements in the same group on the periodic table have similar chemical properties?

4. Explain how the type of element in a group may change from top to bottom.

5. How do metallic characteristics change from top to bottom in a group?

6. How do metallic characteristics change from left to right in a period?

7. Explain why Hydrogen may not be considered a member of group one.

8. What are the two oxidation states Hydrogen may have in a compound?

9. What happens to the electrons of hydrogen when it combines with oxygen to form water?

10. What is the name assigned to group 1 elements?

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11. What is the name given to group 2 elements?

12. Group 1 & 2 elements are characterized by (circle one) high/low electronegativity & ionization energy and (circle one) high/low reactivity.

13. Which group is more reactive: group 1 or group 2?

14. Which groups contains elements that progress from nonmetal -> semimetal -> metal?

15. What name is assigned to the group 17 elements?

16. Group 17 is the only group to contain what types of matter?

17. When group 17 elements combine with a metal they produce salts called ________________.

18. Group 17 elements are characterized by (circle one) high/low electronegativity & ionization energy and (circle one) high/low reactivity.

19. Since small nonpolar molecules are held in solid & liquid phases by weak forces, what happens to boiling point and melting point as the number of electrons increase?

20. Explain why groups 1, 2, & 17 are never found free (uncombined) in nature?

21. Primarily, how are they reduced to their free state?

22. What type of compound do elements in group 1 & 17 combine to form?

a. Give an example.15

b. Why do they react this way?

23. What type of compound do elements in group 2 & 17 combine to form?

a. Give an example.

b. Why do they react this way?

24. Explain why group 18 elements were once called the inert gas group.

25. What is the trend in boiling point and melting point as you go down group 18?

26. What are the exceptions to this “naming”?

27.In your review book, answer the following questions:Page 91: Questions 31-38Page 93: Questions 82-85

Trends in Reactivity on the Periodic Table

You have learned that trends occur in the physical & chemical properties of elements both horizontally & vertically on the periodic table. In this lab demonstration you will observe trends down groups 1 & 2, and the trends across periods 3 & 4.

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1 2 13 14 15 16 17 18IA IIA VII IA

1 II IA IVA VA VIA VIIA2 F3 Na Mg 3 4 5 6 7 8 9 10 11 124 K Ca567 Fr

Observations:

1) Complete the following data table by making observations about the physical appearance of the metals shown by the instructor. Include luster(shine), hardness or softness, reaction with air.

Physical properties of group IA & IIA metalsIA (1) IIA (2)

Na Mg

K Ca

2) Observe the reactions of each metal as the instructor places it in water. Record the observations below.

Reactivity of group IA (1) & IIA (2) metals in waterIA (1) IIA (2)

Na Mg

K Ca

Analysis:

1) Within group IA (1), which element is more reactive?

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2) Within group IIA (2), which element is more reactive?

3) If this trend hold true for the other elements on the periodic table, what is the trend as you go down (top to bottom) any group?

4) Across period 3, which element is more reactive: Sodium or Magnesium?

5) Across period 4, which element is more reactive: Potassium or Calcium?

6) If this trend hold true for the other elements on the periodic table, what is the trend as you go across (left to right) any group?

7) Based on your answers to #3 & #6, identify the most reactive metal on the periodic table.

8) Identify the category of elements (Metal, Metalliod, Nonmetal, or Noble Gas) of the elements on the periodic table shown on the front with the following shadings:

a.) c.)

b.) d.)

Trends in Reactivity

The number of valence electrons are important because they are the electrons that are involved in

____________________________________________________________________.

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Each unpaired electron (single dot in the Lewis dot structures) is a _______________________________________.

*When determining similar reactivity & trends, elements within the same ________________________________

will react ____________________________________, due ________________________________________________________________.

For example: Na reacts with Cl to form NaCl, PREDICT the compound formed by reacting K with Cl:

Example: Mg reacts with Cl to form MgCl2, PREDICT the compound formed by reacting Ca with Cl:

Name ________________________________________ Period_________________________Date__________________________

Use pages 87 – 90 in your Review Book.

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1. What are the metals in group one called?

2. What are the metals in group two called?

3. Group one and two metal easily gain/lose (circle one) electrons and they are never/always(circle one) found free in their atomic state in nature.

4. What type of bonds do group 1 and 2 metals typically form to achieve a stable octet (8 valence electrons).

5. Elements in group one and two have low / high ionization energy (circle one) and low / high electronegativity (circle one).

6. Elements in group one form ions with a ________ charge and elements in group two form ions with a __________ charge.

7. How does reactivity change from top to bottom in Group 1 and 2?

8. What is the most reactive metal?

9. How does metallic character change from top to bottom in groups 14, 15, and 16?

10. List the nonmetals in groups 14, 15, and 16.

11. List the metalloids in groups 14, 15, and 16.

12. List the metals in groups 14, 15, and 16.

13. What are the elements in group 17 called?

14. What is special about group 17 in terms of states of matter at room temperature?

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15. Which is the most reactive member of group 17?

16. What are the elements in group 18 called?

17. What was group 18 former name?

18. Why was group 18 given this old name?

19. Why do elements in the same group or family have similar chemical properties?

20. Answer the following questions on your review book:p. 90 # 31, 33, 34, 39, 42-50, 53-57, 59-63, 68-69, 72

Predicting Periodic Trends in Atomic & Physical Properties

1.) Use the data in the portion of the Periodic Table shown in Chart 1 to predict the properties of elements X,Y,Z, which occupy the blank squares in the table. Base your predictions on the properties of neighboring elements, and the apparent trends that occur as you go across a period or down a group. Use group number to predict the number of valence electrons and the common oxidation state. Place your answers in Table 1. The properties which you will predict are shown in the code square below:

2.) Look up the theoretical values in reference table S. Calculate the percent error between your predicted value and the theoretical value.Chart 1Key:

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Atomic Number

Symbol

Atomic Radius

Density Ionization EnergyMelting Point Electronegativity

1 2 13 14 15 163 4 5 6 7

2 Li 155 Be 112 B 98 C 91 N 91 O 650.534 520 1.848 900 2.340 801 3.5 1402 0.001 140

20.001

1314

454 1.0 1551 1.6 2573 2.0 3820 2.6 63 3.1 55 3.511 12 13 14 15 16

3 Na 190 Mg 160 Al 143 Si 132 P 128 S 1270.971 496 1.738 736 2.698 578 2.369 787 1.820 101

22.07 100

0371 0.9 922 1.3 934 1.6 1683 1.9 317 2.2 386 2.619 20 31 32 33 34

4 K 235 Ca 197 Ga 141 X As

139 Z

0.862 419 1.550 590 5.907 579 5.780 944337 0.8 112 1.0 303 1.8 1090 2.237 38 49 50 51 52

5 Y Sr 215 In 166 Sn

162 Sb

159 Te 132

2.540 549 7.310 558 7.310 709 6.69 944 4.930

1008

1042 1.0 429 1.8 505 1.8 904 2.1 387 2.755 56 81 82 83

6 Cs 267 Ba 222 Tl 171 Pb

171 Bi 170

1.873 376 3.594 503 11.85 589 11.350 589 9.747 703302 0.8 1002 0.9 577 2.0 601 2.0 545 2.0

Table 1: Predicted Value of Unknown Atomic and Physical Properties:Identity of

Unknown X

Identity of Unknown Y

Identity of Unknown Z

Property Predicted Actual % Error Predicted Actual % Error Predicted Actual % Error# Valence ElectronsOxidation

State

Density

Melting PointAtomic radius

IonizationEnergy

Electronegativity

Review: Periodic Trends

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Review: The Periodic Table

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I. _____________________________ developed the first periodic table in 1869. He organized the elements by

increasing _________________________________________________.

Modern Periodic Law states that _______________________________________________________________________________

_______________________________________________________________________________________________________________________

Define Perioidicity: ____________________________________________________________________________________________

* example: eating breakfast every morning,

high & low tides, receiving a magazine every month.

* On the axis provided show what the perioidicity of a trend looks like:

II.

a.) Horizontal rows on the periodic table are called _____________________________.

b.) Vertical columns on the periodic table are called ________________________________.

c.) The the group number indicates the number of ___________________________.

d.) Elements in the same vertical ________________ have similar chemical properties because they have the

same number of _______________________________________.

1.) If Na & Cl react to form NaCl, predict the compound formed by K & F: _________________________

2.) If Mg & Cl react to form MgCl2, predict the compound formed by Sr & Cl: _______________________

3.) If Al & O react to form Al2O3, predict the compound formed by B & S: __________________________

4.) If C & O react to form CO2, predict the compound formed by Si & Se: __________________________

e.) Use your notes to complete the following table:

Name Group Number(s) Representativ

e

Properties

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Elements

ALKALI METALS

ALKALINE

EARTH METALS

TRANSITION

METALS

HALOGENS

NOBLE GAS

SEMIMETALS

(METALLOIDS)

f.) Compare the properties of metals & nonmetals:

METALS NONMETALS

g.) Classify the following as metal, nonmetal or semimetal:

_______ Carbon _______ Silicon _______Iodine _________Sodium _______ Iron

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h.) Rank the following from least reactive to most reactive: Cesium, Francium, Lithium, Potassium, Sodium

__________ __________ __________ __________ _________

i.) Rank the following from least reactive to most reactive: Calcium, Cobalt, Copper, Chromium, Potassium

__________ __________ __________ __________ _________

j.) Which metal is a liquid at room temperature __________________ , which nonmetal _________________?

k.) Which group of elements makes colored solutions? _______________________________

l.) Metals gain/lose electrons, forming positive/negative ions. The ionic radius is bigger/smaller than

the atomic radius.

m.) Nonmetals gain/lose electrons, forming positive/negative ions. The ionic radius is bigger/smaller

than the atomic radius.

III Complete the following table indicating increase or decrease or remain the same:

TREND LEFT TO RIGHT TOP TO BOTTOM

Atomic number

Atomic mass

Atomic radius

Ionization energy

Electronegativity

# of valence electrons

# of energy levels

Nuclear charge

IV. Answer the following questions based on the electron configuration: 2-8-18-6

a) How many electrons are in an atom?_________________________

b) Identify the element name: ________________________________

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c) How many valence electrons are in this atom? _________________

d) How many principle energy levels are in this atom? ________________

e) How many electrons are in the second principle energy level? _________________

f) In which period is this element located? _____________________

V. You have learned how to predict unknown properties of unknown elements by averaging values across a

row & down a group. Show all work below to predict the unknown properties of element "A":

Key:

14 Si2.4 188118 1680

31 Ga5.89 138134 303

? A? ?? ?

33 As5.72 226134 1087

50 Sn7.3 169134 505

Answers: Atomic Number "A" ______________

Density "A" ______________ Ionization Energy "A" ________________

Atomic radius "A" ______________ Melting Point "A" ________________

Real Symbol of "A" ______________

Work Area:

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Atomic Number

Density Ionization energy

Atomic Radius Melting Point

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