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Name: _____________________________________ Period : ________Chemistry – Chapter 14 – Chemical Periodicity

State/District Chemistry Standards Addressed:SC 2.2 Describe the arrangements of electrons in atoms using various theories and models.SC 2.4 Explain Chemical Periodicity and the classification of elementsSC 6.0 Demonstrate that the scientific process applies to all areas of science

Objectives: Students will be able to: Describe how the periodic table can be used to predict the properties of elements Give the outer shell configuration for each of the groups on the periodic table Give the names of groups 1,2,7 and 8 Identify the s, p, d and f blocks on the periodic table Write the electron configuration, orbital notation and electron dot structure using only the periodic table and

also be able to do this using shorthand notation for electron configuration. Define nuclear charge, electronegativity, and ionization energy Explain the reason for the trends in atomic size, nuclear charge, electronegativity and ionization energy as you

go down a group or across a period on the periodic table. Explain the sizes of atoms compared to their ions.

Textbook Pages 391- 396

PART I1. Who told the elements where to go? ____________________________2. What particle is most important in determining the physical and chemical properties of an element?_____________________3. How is the modern periodic table arranged?

4. What is meant by the term group or family on the periodic table and what do elements in the samegroup have in common?

5. How many groups are there? ___________6. What is the name of the following groups?

Group 1 __________________________________Group 2___________________________________Group 17 _________________________________Group 18 _________________________________Groups 3 – 12 ____________________________The groups starting with elements 57 and 89 ____________________________________Groups 1,2 and 13 – 18 _____________________________________________________

7. How many periods are there? ___________8. What does each period on the periodic table represent?________________________________Using Fig 14.5 pg 395, and your Energy Level Diagram to answer the following:9. What is the electron configuration for only the last electron to fill for each of the following groups?

Group 1: _______ Group 2: _______ Group 13: _______ Group 14: _______

Group 15: _______ Group 16: _______ Group 17: _______ Group 18: _______

10. What groups comprise the s electron block? ______ Which main level does the s sublevel start with? ___11. What groups comprise the p electron block? ______Which main level does the p sublevel start with? ___12. What groups comprise the d electron block? _________ Which main level does the d start with? ______

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13. What is the name of given to the elements that make up the f electron block ____________________14. Which main level does the f start with? ______15. What is the maximum number of s electrons in any period? _______16. What is the maximum number of p electrons in any period? _______17. What is the maximum number of d electrons in any period? _______18. What is the maximum number of f electrons in any period? _______19. What are valence electrons? _________________________________20. What is the octet rule?

21. Fill in the following table for each group.Group#

Configuration ofouter shell only

ValenceElectrons

Electronsgained or lostto form octet

Chargeon theion

Cation (+)orAnion (-)

121314151617183-12

Using the information in the above table answer the following:22. How does the group number relate to the number of valence electrons?

23. Why do elements in the same group have similar properties?

24. Why don’t elements in the same group have exactly the same properties?

25. Which group of elements is most stable and why?

26. Which are the only sublevels (s, p, d, f) that can occupy the outermost shell? __________ What does thissay about the maximum number of electrons that can be outer shell (valence) electrons?

27. Where are the elements that want to gain electrons located on the periodic table, and what is this groupof elements called?___________________________

28. Where are the elements that want to lose electrons located on the periodic table and what is this group ofelements called? __________________________________

29. What is an ion?

30. What is a cation?

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31. What is an anion?

PART II1. USING ONLY YOUR PERIODIC TABLE WRITE THE ELECTRON CONFIGURATION FORELEMENT 118. (From now on you will not be able to use your order of filling sheet)

2. Using only your periodic table write the electron configuration for the following elements and give theelement’s name with correct spelling.

Mg:

N:

S:

Ra:

Br:

Zn:

O:

Pb:

3. Only valence electrons are involved in chemical reactions so it is only necessary to know the outer shellconfiguration. Therefore, we use what is called the shorthand notation. To do shorthand notation you firstfind the noble gas (also known as inert gas) that has an atomic number just before the element you haveselected. Put brackets around this noble gas then continue writing the electron configuration.

Name Shorthandnotation

ValenceElectrons

Electronsgained orlost

Charge onion

Metal orNonmetal

MgPbNaFAsIUSnRaAlCFeSe

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PART III

1. Write the complete electron configuration for Lithium. Then draw a diagram of the atom showing the howmany protons in the nucleus and how many electrons are in each of the main levels around the atom.

2. Do the same instructions described in #1 for Sodium.

3. Do the same instructions described in #1 for Potassium.

4. What is the name of this group? __________________________5. How are the elements in this group the same?6. How are they different?7. How does the size of atoms compare as you go down this group?8. Why is this?

9. Would you expect this to be true for other groups in the periodic table? Why?

10. What general rule could you write concerning the size of atoms as you go down a group and the reasonfor this?

See Fig 14.8 pg 399 to verify that your rule is correctIonization energy – The energy needed to remove a valence electron from an atomElectronegativity – A measure of how strongly an atom will pull away electrons from another atom11. As you go down a group would you expect the ionization energy to increase or decrease and explain

why.

12. As you go down a group would you expect the electronegativity to increase or decrease and explainwhy.

13. The smaller the atom the larger/smaller the ionization energy. Why?

14. The smaller the atom the larger/smaller the electronegativity. Why?

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PART IV

1. Write the complete electron configuration for Sodium. Then draw a diagram of the atom showing the howmany protons in the nucleus and how many electrons are in each of the main levels around the atom.

2. Do the same instructions described in #1 for Aluminum.

3. Do the same instructions described in #1 for Chlorine.

4. These elements are all in the same __________________________5. How are the atoms of these elements the same?___________________________6. The effective nuclear charge is determined by adding up the electrons in an atom except the valence

electrons, and then subtracting this number from the number of protons in the nucleus. The formula is:Effective Nuclear Charge = Protons - Non-valence electrons

The higher the effective nuclear charge the stronger the nucleus attracts the electrons around an atom.7. Calculate the effective nuclear charge for Na _____ Mg _____ Al _____ S______ Cl ______

Which nucleus of the above atoms would attract its electrons more strongly? ________The effective nuclear charge turns out to be the same as what other value? _____________________

8. What is the effective nuclear charge for Mg _____ Ca_____ Sr______How does nuclear charge change when you go down a group? ________________________Then what factor causes the size to increase as you go down a group? _____________________

9. How does the size of atoms compare as you go across the period left to right? __________________10. Why is this?

11. Would you expect this to be true for other periods in the periodic table? Why?

10. What general rule could you write concerning the size of atoms as you go across a period and the reasonfor this?

See Fig 14.8 pg 399 to verify that your rule is correct

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Ionization energy – The energy needed to remove a valence electron from an atomElectronegativity – A measure of how strongly an atom will pull away electrons from another atom11. As you go across a period left to right would you expect the ionization energy to increase or decreasebased on the size of the atom? Explain why.

12. As you go across a period left to right would you expect the electronegativity to increase or decreasebased on the size of the atom? Explain why.

13. The higher effective nuclear charge that an atom has the larger/smaller the ionization energy.Circle the correct answer and explain your answer.

14. The higher effective nuclear charge that an atom has the larger/smaller the electronegativity.Circle the correct answer and explain your answer.

SUMMARY: (Nobel gases (also known as inert gases) are not included in these trends because they havestable shells and do not want to gain or lose electrons.)15. The atomic size increases as you go up/down and left/right on the periodic table.16. The electronegativity increases as you go up/down and left/right on the periodic table.17. The ionization energy increases as you go up/down and left/right on the periodic table.18. The element with the highest electronegativity is ___________19. The element with the lowest ionization energy is ___________20. The smallest atom is ________21. The largest atom is _________

DRAW ARROWS SHOWING THE TRENDS FOR ATOMIC SIZE, IONIZATION ENERGY ANDELECTRONEGATIVY ON YOUR BLANK PERIODIC TABLE.Circle the correct word in italics in the following passages:22. Metals are located on the left/right side of the periodic table. Metals have (1 to3) or ( 5 to 7) valenceelectrons. They lose/gain electrons to become like a stable noble gas. When they lose/gain electrons theyform a _____________ charged ion called a(n) _____________________.

23. The most reactive metal would be one that would gain/lose electrons most easily so it would have ahigh/low ionization energy and a high/low electronegativity. It would also be a small/large atom. Based onthis trend the most active metals would be at the left/right and top/bottom of the periodic table. The mostreactive metal would be the element _____________________.

24. Nonmetals are located on the left/right side of the periodic table. Nonmetals have (1 to3) or ( 5 to 7)valence electrons. They lose/gain electrons to become like a stable noble gas. When they lose/gain electronsthey form a _____________ charged ion called a(n) _____________________.

25. The most reactive nonmetal would be one that would gain/lose electrons most easily so it would have ahigh/low electronegativity and a high/low ionization energy. It would also be a small/large atom. Based onthis trend the most active nonmetals would be at the left/right and top/bottom of the periodic table. The mostreactive nonmetal would be the element _____________________.

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Part V1. Write the complete electron configuration for Magnesium. Then draw a diagram of the atom showing thehow many protons in the nucleus and how many electrons are in each of the main levels around the atom.

2. Write the complete electron configuration for a Magnesium cation that has lost its two valence electrons.Draw a diagram of the atom showing the how many protons in the nucleus and how many electrons are ineach of the main levels around the Magnesium cation.

3. How many protons are in the nucleus of the Magnesium cation? ________4. How many electrons are around the nucleus of the Magnesium cation? ________5. What would be the charge on the Magnesium cation? __________6. Would the Magnesium cation be larger or smaller than the Magnesium atom _____________.7. Explain how you came up with your answer for #6 above.

8. A third ionization would involve removing a third electron from a Magnesium atom, which mainlevel would it be removed from? _______. Why would it take significantly more ionization energy toremove this third electron?

9. Write the complete electron configuration for Nitrogen. Then draw a diagram of the atom showing thehow many protons in the nucleus and how many electrons are in each of the main levels around the atom.

10. Write the complete electron configuration for a Nitrogen anion that has gained three valence electrons.Draw a diagram of the atom showing the how many protons in the nucleus and how many electrons are ineach of the main levels around the Nitrogen anion.

11. How many protons are in the nucleus of the Nitrogen anion? ________12. How many electrons are around the nucleus of the Nitrogen anion? ________13. What would be the charge on the Nitrogen anion? __________14. Would the Nitrogen anion be larger or smaller than the Nitrogen atom _____________.15. Explain how you came up with your answer for #14 above.

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16. Nonmetals want to gain/lose electrons forming anions/cations with a +/- charge. Since the anion/cationhas gained/lost electrons it will be larger/smaller that the atom from which it was formed. Write the electronconfiguration for an oxygen anion and give the charge on this anion.

17. Metals want to gain/lose electrons forming anions/cations with a +/- charge. Since the anion/cation hasgained/lost electrons it will be larger/smaller that the atom from which it was formed. Write the electronconfiguration for an aluminum cation and give the charge on this cation?