PLEASE DO NOT WRITE ON THIS TEST! ID: A

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Chemistry (H) - CHAPTER 5 TEST

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.

1. Use the graph bellow to answer the follwing question

Why do the 4th and 5th periods have more dots and different patterns?

a. They contain more elements, including the d block elements

c. They contain more elements, including the f block elements

b. They contain more elements, including the s and p block elements

d. They contain more elements, including the d and f block elements

ID: A

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2. Which element has an electron configuration that ends in p6?a. A c. Cb. B d. D

3. d-block elements are also known asa. alkali metals c. halogensb. alkali earth metals d. transition elements

4. An example of a halogen isa. Cs c. Brb. Pd d. Xe

5. Elements on the right side of the periodic tablea. tend to lose electrons to become negative

ionsc. tend to lose electrons to become positive

ionsb. tend to gain electrons to become negative

ionsd. tend to gain electrons to become positive

ions

6. Which of following elements has a higher IE?a. B b. O

7. Which is the most important characteristic in detemining an element’s chemical properties?a. the number of protons and neutrons in its nucleusb. which period it is found inc. the number of valence electrons it containsd. its outermost energy level

ID: A

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8. Refer to the following graph to answer the question bellow:

Alkali metals have low ionization energy becausea. their number of protons is greater than

number of neutronsc. they have valence electrons that don’t

react b. they have one valence electron d. they have a full octet shell

9. The number of valence electrons for Group 2 elements isa. 2 c. 18b. 8 d. equal to the period number

10. Which region contains the halogen family of elements?a. A c. Cb. B d. D

11. The electrons available to be gained, lost, or shared in the formation of chemical compounds are calleda. outer shell electrons c. valence electronsb. High-E electrons d. none of the answers are correct

ID: A

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12. Which region is referred to as the f-block on the diagram? a. A c. Cb. B d. D

13. Which block contains 5 orbitals?a. s c. db. p d. f

14. Which block is element Y most likely found in?Element Block Characteristics

X s Soft, shiny grey metal; highly reactive, lightweight

Y ? Gas at room temperature; has the highest electronegativity in its period

Z p Used as a semiconductor due to its electricity-conducting properties

a. s c. db. p d. f

15. Which category of elements have the property of being malleable and ductile?a. gases c. metalloidsb. metals d. nonmetals

16. Which metalloid is in the fourth period and the same group as Carbon?a. Silicon c. Tinb. Germanium d. Boron

17. Which has the larger radius?a. Cl b. Cl-

18. Which scientist first arranged elements by atomic number?a. Mendeleev c. Newlandsb. Lavoisier d. Mosely

ID: A

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19. Which of the following elements has a lower IE?a. N b. Sb

20. Which region contains elements with two valence electrons?a. A c. Cb. B d. D

21. Which region contains elements with an electron configuration that ends with p3?a. A c. Cb. B d. D

22. An anion has a _______ charge.a. positive c. neutralb. negative d. none of the answers are correct

23. Which element is the alkaline earth metal with the largest atomic number?a. Fr c. Hb. Ra d. Be

24. The element with the highest IE isa. H c. Fb. He d. Fr

ID: A

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25. Use the following graph to answer the question below:

Why is the tendency of atoms to gain electrons decreasing as you go down the periodic table?a. As an atom gets larger, any added

electrons are not close to thenucleus (and therefore theattractive force of the nucleusisn’t powerful enough)

c. As an atom gets larger, you have toadd even more electrons

b. Because you have less electrons and the less electrons you have the bigger atomic radius molecules have.

d. As you go down, there are a lowernumber of shells and a higher numberof protons

26. Which of the following elements has the smaller radius?a. Sr b. Y

27. The box for an element from the periodic table is shown. Which is the atomic mass?

a. A c. Cb. B d. D

28. Which is a transition element with five d-block electrons in energy level 4?a. Niobium (Nb) c. Manganese (Mn)b. Renium (Re) d. Technicium (Tc)

29. Which is defined as the energy required to remove an electron from an atom of an element in the gaseous state?a. ionization energy c. ionic radiusb. electronegativity d. law of octets

ID: A

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30. Which correctly describes elements in the same group?a. They have the same number of valence electrons.b. They have electrons in the same outermost energy level.c. They have the same atomic radius.d. They must be in the same state of matter.

31. Which property describes the attraction of an element to electrons in a chemical bond?a. atomic radius c. electronegativityb. ionic radius d. ionization energy

32. What is the group, period, and block in which [Rn]7s1 is found?a. Group 1, 7th period, p-block c. Group 7, 7th period, d-blockb. Group 1, 1st period, s-block d. Group 1, 7th period, s-block

33. The element with the largest atomic radius isa. H c. Frb. He d. Lr

34. Which of the following elements is a metal?a. Boron c. Magnesiumb. Nitrogen d. Carbon

35. An anion isa. a nonmetal that has gained an electron c. a metal that has gained an electronb. a nonmetal that has lost an electron d. a metal that has lost an electron

36. Which block on the periodic table contains the actinide series of elements?a. s-block c. d-blockb. p-block d. f-block

37. What element is the group 14 element in period 4a. C c. Geb. Si d. Ti

38. A cation has a _______ charge.a. positive c. neutralb. negative d. none of the answers are correct

39. Which has the larger radius?a. Mg b. Mg+2

ID: A

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40. Which of the following properties is most helpful for chemist to determine what kind of bond atoms make?a. ionization energy c. electron affinityb. electronegativity d. valence electrons

41. According to ____ periodic table, the physical and chemical properties of elements are periodic functions of their atomic weights.a. Dmitri Mendeleev’s c. Henry Moseley’sb. John Newlands’ d. Lothar Meyer’s

42. The elements with atomic numbers from 58 through 71 in the periodic table are the a. s-block elements c. d-block elementsb. p-block elements d. f-block elements

43. An element has an outer E-level of 5s1, which element is it?a. K c. Rbb. Ca d. Sr

44. Refer to the following graph to answer the question bellow:

Reading from the graph above would you expect Ga to see an increase or decrease in ionization energy comapred to Caa. decrese because it has less unpaired

electrons in the p shellsc. increase as it has more unpaired electrons

in the p shellb. increase because it has less unpaired

electrons in the p shellsd. decrease as it is going down the perioidic

group

45. The electron configuration of an element is [Ar]2d104s24p5. This element is in the ___ period.a. 2nd c. 5thb. 4th d. 10th

ID: A

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46. In which pair is the one on the left larger than the one on the right?a. Na, Rb c. Br, Br-b. S, Mg d. K, K+

47. An example of an alkali metal isa. Li c. Fb. Sr d. Ar

48. Na+ Mg+2 Al+3 P-3 S-2 Cl-

The bar chart shows the relative radii of the ions of the elements in period 3. Why is the radii of the second set of ions bigger than the group of ions on the left of the chart?

a. atomic number increases across period 3 c. the number of neutrons increases exponentially as we travel accross period 3

b. atomic mass increases across period 3 but the number of neutrons causes electron shielding to go down

d. the first three elemetns lost electrons to become ions while the last three elemetns gained electrons to become ions.

49. Place these five elements in order of electronegativity, with the HIGHEST electronegativity FIRST.

a. B, D, C, A, E c. A, E, C, D, Bb. B, D, C, E, A d. E, C, D, B, A

ID: A

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50. Which is the correct electron dot diagram for the element Silicon (Si)?

a. Diagram A c. Diagram Cb. Diagram B d. Diagram D

ID: A

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Chemistry (H) - CHAPTER 5 TESTAnswer Section

MULTIPLE CHOICE

1. ANS: A PTS: 1 2. ANS: D PTS: 1 NAT: UCP.2 3. ANS: D PTS: 1 4. ANS: C PTS: 1 5. ANS: B PTS: 1 6. ANS: B PTS: 1 7. ANS: C PTS: 1 NAT: B.1 | B.2 8. ANS: B PTS: 1 9. ANS: A PTS: 1 10. ANS: C PTS: 1 NAT: UCP.2 | B.2 11. ANS: C PTS: 1 12. ANS: B PTS: 1 NAT: UCP.2 13. ANS: A PTS: 1 NAT: B.1 | B.2 14. ANS: B PTS: 1 NAT: UCP.2 | B.2 15. ANS: B PTS: 1 NAT: B.1 | B.2 16. ANS: B PTS: 1 NAT: B.1 | B.2 17. ANS: B PTS: 1 18. ANS: D PTS: 1 NAT: B.1 | G.3 19. ANS: B PTS: 1 20. ANS: A PTS: 1 NAT: UCP.2 | B.1 | B.2 21. ANS: C PTS: 1 NAT: UCP.2 | B.1 | B.2 22. ANS: B PTS: 1 23. ANS: B PTS: 1 24. ANS: C PTS: 1 25. ANS: A PTS: 1 26. ANS: B PTS: 1 27. ANS: D PTS: 1 NAT: B.1 | B.2 28. ANS: C PTS: 1 NAT: B.1 | B.2 29. ANS: A PTS: 1 NAT: UCP.2 30. ANS: A PTS: 1 NAT: B.1 | B.2 31. ANS: C PTS: 1 NAT: B.1 | B.2 32. ANS: D PTS: 1 33. ANS: C PTS: 1 34. ANS: C PTS: 1 NAT: G.3 | B.1 | UCP.1

KEY: Metals MSC: 1 35. ANS: A PTS: 1 36. ANS: D PTS: 1 NAT: UCP.2 | B.1 | B.2 37. ANS: C PTS: 1 38. ANS: A PTS: 1 39. ANS: A PTS: 1

ID: A

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40. ANS: B PTS: 1 41. ANS: A PTS: 1 NAT: G.3 | B.1 | UCP.1

KEY: Periodic properties MSC: 1 42. ANS: D PTS: 1 43. ANS: C PTS: 1 44. ANS: A PTS: 1 45. ANS: B PTS: 1 46. ANS: D PTS: 1 NAT: B.1 | B.6 47. ANS: A PTS: 1 48. ANS: D PTS: 1 49. ANS: B PTS: 1 50. ANS: A PTS: 1