Periodic Table



Periodic Table Worksheet

Tier 1 and 2

1. Periodic means .

Examples of periodic properties:

2. What is a group (or family)? What is a period?

3. How can you determine the number of electrons in an element’s outer energy level by the group it’s in?

4. What is the octet rule?

5. Why do elements that make positive ions occur on the left side of the periodic table while those that

make negative ions occur on the right?

6. What is the common name for group 18?

Why do the elements of this group usually not form ions?

7. Complete the following table.

|Group |Common Name |Charge on Ions of this Group |

|1 | | |

|2 | | |

|13 / 3A |-------- | |

|16 / 6A |-------- | |

|17 / 7A | | |

8. Predict the charges on ions of the following atoms.

Ra As Te Cs In At Ga

9. a) In group 1, which element is the most active?

b) Metallic activity tends to (increase, decrease) as one goes down Group 1.

10. a) Which element is most active in group 17?

b) Nonmetal activity tends to (increase, decrease) as one goes down Group 17.

11. Compare and contrast ionization energy and atomic radius.

Ionization Energy Radius

Definition:

12. Choose the element in each pair that has the largest radius:

a) K or Br b) F or Br c) He or Rn d) Mg or Cl e) O or S f) Be or O

13. Choose the element in each pair that has the highest ionization energy:

a) Na or Cl b) Na or Cs c) F or I d) K or F e) Mg or S f) N or Sb

14. When elements have a large radius, they tend to have a (large, small) ionization energy. WHY???

15. Name all the elements called metalloids.

Periodic Table Scavenger Hunt

1. Which element is a metal: Ba (56) or At (85)?

2. Which period is Ca (20) in?

3. What is the number of the group N (7) is in?

4. Which element is an alkali metal: Rb (37) or Al (13)?

5. Which element is a halogen: Na (11) or Cl (17)?

6. Which element is a noble gas: Ne (10) or Br (35) or O (8)?

7. Which element is the most active nonmetal?

8. Which element is the most active metal?

9. Which element has the largest radius: Na (11) or Cs (55)?

10. Which element would be a positive ion in a compound: Sr (38) or Te (52)?

11. How many electron dots should As (33) have?

12. Which element has the highest ionization energy: K (19) or Kr (36)?

13. When Te (52) is an ion in a compound, what charge does it have?

14. How many is an octet of electrons?

15. Which element has the largest radius: Rb (37) or Xe (54)?

16. Which element has the largest ionization energy: K (19) or Cl (17)?

17. Which element has 5 valence electrons? B (5) or P (15)?

18. Which element has 18 electrons when it is an ion with a –1 charge?

19. What atomic number would an isotope of U (92) have?

20. How many neutrons does bromine-80 have?

Characteristics of Elements

Use a periodic table to help you answer the following questions.

1. a. How many protons does an atom of bromine (Br) have? a.

b. In which group number is bromine found? b.

c. What is the common name of this chemical family? c.

d. How many valence electrons does it have? d.

e. Is it a metal, a nonmetal, or a metalloid? e.

f. How does its atomic radius compare to that of chlorine (Cl)? f.

g. How does its atomic radius compare to that of arsenic (As)? g.

h. What ion is it most likely to form in compounds? h.

2. a. How many protons does an atom of argon (Ar) have? a.

b. In which group number is argon found? b.

c. What is the common name of this chemical family? c.

d. How many valence electrons does it have? d.

e. Is it a metal, a nonmetal, or a metalloid? e.

f. How does its atomic radius compare to that of krypton (Kr)? f.

g. How does its atomic radius compare to that of sulfur (S)? g.

h. What ion is it most likely to form in compounds? h.

3. a. How many protons does an atom of potassium (K) have? a.

b. In which group number is potassium found? b.

c. What is the common name of this chemical family? c.

d. How many valence electrons does it have? d.

e. Is it a metal, a nonmetal, or a metalloid? e.

f. How does its atomic radius compare to that of sodium (Na)? f.

g. How does its atomic radius compare to that of selenium (Se)? g.

h. What ion is it most likely to form in compounds? h.

Periodic Table Vocabulary

Choose the correct words from the list, then place the appropriate number in each blank.

Word List:

1. actinide series 2. alkali metal 3. alkaline earth metal 4. anion

5. atomic mass 6. atomic number 7. cation 8. family

9. group 10. halogen 11. lanthanide series 12. metal

13. metalloid 14. noble gas 15. nonmetal 16. period

17. periodic law 18. periodic table 19. inner transition metals 20. transition metal

Dmitri Mendeleev developed a chartlike arrangement of the elements called the . He stated that if the elements were listed in order of increasing , their properties repeated in a regular manner. He called this the of the elements. The arrangement used today differs from that of Mendeleev in that the elements are arranged in order of increasing . Each horizontal row of elements is called a(n) . Each vertical column is called a(n) , or , because of the resemblance between elements in the same column, a(n) .

In rows 4 through 7, there is a wide central section containing elements, each of which is called a(n) . Rows 6 and 7 also contain two other sets of elements that are listed below the main chart. These are called the and the , respectively. Each of the elements to the left of the stairstep line of the chart, is classified as a(n) . Each of the elements at the right side of the stairstep line is classified as a(n) . Each of the elements between these two main types, having some properties like one type and other properties like the other type, is called a(n) . Each of the elements in the column labeled IA or 1 is called a(n) . Each of the elements in the column labeled IIA or 2 is called a(n) . Each of the elements in column VIIA or 17 is called a(n) . Each of the elements in column VIIIA or 0 or 18 is called a(n) .

Periodicity Worksheet

Use a periodic table to help you answer the following questions.

1. Which element in the second period has the greatest atomic radius?

2. Which of the group IIIA (13) elements is the largest?

3. Of the halogens, which has the smallest radius?

4. Which of the alkaline earth metals is the largest?

5. Which of the transition metals has the smallest atomic radius?

6. Which of the noble gases is the smallest?

7. The atomic radius of which element is the largest?

8. Do alkali metals generally make anions or cations?

9. Which of the elements which have their valence electrons in the second

energy level is the largest?

10. Which of the metalloids has the smallest atomic radius?

11. Which of the rare earth elements is the smallest?

12. Which of the transition metals in the fifth period is the largest?

13. Are metal ions larger or smaller than the neutral atoms they came from?

14. Are cations larger or smaller than the neutral atoms they came from?

15. Are ions of alkali metals larger or smaller than ions of alkaline earth

metals from the same period?

16. Which element in the second period has the greatest first ionization

energy?

17. Which of the group IIIA (13) elements has the largest ionization

energy?

18. Of the halogens, which has the smallest electronegativity?

19. Which of the alkaline earth metals has the smallest electronegativity?

20. Which of the transition metals has the largest ionization energy?

21. Which of the noble gases has the smallest ionization energy?

22. Which of the group IVB (14) metals is the least active?

23. Which of the halogens is the most active?

24. Which of the semi-metals that have their valence electrons in the fourth

energy level has the largest ionization energy?

25. Which of the period three elements has the largest electronegativity?

26. Which of the inner transition elements of the seventh period is the

easiest to ionize?

27. Which of the transition metals in the fifth period has the largest EN?

28. Which of the group four metals has the largest ionization energy?

29. Which of the non-metals in the third period is the most active?

30. As atomic size increases, what happens to the ionization energy of the

atom?

Tier 3

Periodic Puzzles:

In each of the following puzzles, each element represented has been assigned a RANDOM letter. (I.e., H is not hydrogen, S is not sulfur, etc.) Your job is to figure out where in the periodic table each element belongs based on the properties in the clues below and place it in the periodic table at the bottom of the page.

Puzzle #1: Elements that are in the same group are: AYHES, QDKLU, WVRT, JBIF, PNGX, OMCZ

Clues:

|Element T has an oxidation number of -2 (it needs 2 more electrons to |Element U has a larger atomic radius than element Q. |

|become stable). | |

|Element U does not follow the periodic trends like the other group A |Element M is more electronegative than element O. |

|elements do. | |

|Element Y is the most metallic element on this chart. |Element Z has the most metallic character in its group. |

|Element G is the most electronegative element. |Element C has the smallest atomic radius in its group. |

|Element J is one of 2 metalloids in the same group on this chart. |Element E is placed in the same group as the other elements, but it does not |

| |have properties that are similar to other elements with one valence electron. |

|Element S has a larger atomic radius than element H and a smaller atomic |Element D is used in a type of sign. |

|radius than element A. | |

|Element V has the lowest ionization energy in its group. |Element X is less metallic than element P. |

|Element B is usually a gas. |Element F has the lowest electronegativity value in its group. |

|Element L is the heaviest element in its group on this chart. |Element K is “misplaced” because it only has 2 electrons in its outermost energy|

| |level, not an octet. |

|Element I has less metallic character than element F. |Element R is more electronegative than element B. |

|Element N has the lowest ionization energy in its group. |Element T loses electrons easier than element W. |

|IA | | | | |VIIIA |

| |IIA |VA |VIA |VIIA | |

| | | | | | |

| | | | | | |

| | | | | | |

| | | | | | |

Puzzle #2: The following elements belong together in families (groups): ZRD, SIFP, JXBE, LHT, QKA, WOV, YMC, and GUN

|The element N has 4 valence electrons. |V is a liquid, whereas W is a gas at room temperature. (Generally, elements |

| |at the top of the table have the lowest boiling points.) |

|A has atomic number of 8. |The compound IW is less stable than FW. (Alkali metals with more energy |

| |levels form more stable compounds.) |

|X is a noble gas. |J has 2 protons. |

|I is an alkali metal. |Z has the lowest atomic mass in its group. |

|M has 5 valence electrons. |The electronegativity of O is the largest in the periodic table. |

|H is an alkaline earth metal. |The density of S is 0.53 and that of I is 0.97. (Metals with more energy |

| |levels are usually denser.) |

|W is a halogen. |R has an outer electron configuration of 3s23p1. |

|The ionization energy of T is greater than that of L but less than that of H.|P2A and NA2 are produced when a candle burns. (The products of a combustion |

| |reaction are H2O and CO2.) |

|Y is less metallic than M. (More metallic elements have more energy levels.)|E contains 10 protons. |

|Q’s atomic radius is greater than that of K. |The electrons of C are distributed over 4 energy levels. |

|Element U has 3 energy levels of electrons. |The electron configuration of X is the same as that of the ion Cl-. |

IA | | | | | | |VIIIA | | |IIA |IIIA |IVA |VA |VIA |VIIA | | | | | | | | | | | | | | | | | | | | | | | | | | | | | |

Tier 1

1. Repeating on a certain pattern. Electronegativity.

3. Determine the S and P electrons.

5. It is easier for the elements on the left to lose fewer electrons than gain more.

9. Francium. Increase

13. Cl, Na, S, S, F, N

15. B, Si, Ge, As, Te, Sb, Po

1. Ba

3. 5

5. Cl

7. F

9. Cs

11. 5

13. -2

15. Rb

17. P

19. 92

1. 35, 7, halogens, 7, non, Bigger, smaller, -1

1. Li

3. F

5. Zn

7. Fr

9. Ra

11. Lu

13. Smaller

15. Bigger

17. B

19. Ra

21. Rn

23. F

25. Cl

27. Cd

29. Cl

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