The Periodic Table Multiple Choice



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The Periodic Table
Multiple Choice

Identify the choice that best completes the statement or answers the question.
____ 1. The two most abundant elements created in the Big Bang were:

a.

hydrogen and carbon

c.

oxygen and helium

b.

carbon and oxygen

d.

hydrogen and helium

____ 2. In the periodic table, where are the halogens located?



a.

the first column on the left

c.

the second to last column on the right

b.

all the columns in the middle

d.

the last column on the right

____ 3. Which of the following elements has the largest atomic radius?



a.

helium

c.

argon

b.

magnesium

d.

nitrogen

____ 4. Which of the following elements is the most electronegative?



a.

oxygen

c.

aluminum

b.

calcium

d.

boron

____ 5. How many electrons can fit in a p-orbital?



a.

2

c.

10

b.

6

d.

14

____ 6. What do elements K and Fe have in common?



a.

They have the same number of valence electrons.

b.

They have the same atomic radii.

c.

They belong to the same family.

d.

They belong to the same period.

____ 7. What is another name for the representative elements?



a.

Group A elements

c.

Group C elements

b.

Group B elements

d.

transition elements

____ 8. What is another name for the transition metals?



a.

noble gases

c.

Group B elements

b.

Group A elements

d.

Group C elements

____ 9. Which of the following elements is in the same period as phosphorus?



a.

carbon

c.

nitrogen

b.

magnesium

d.

oxygen

____ 10. Each period in the periodic table corresponds to ____.



a.

a principal energy level

c.

an orbital

b.

an energy sublevel

d.

a suborbital

____ 11. The modern periodic table is arranged in order of increasing atomic ____.



a.

mass

c.

number

b.

charge

d.

radius

____ 12. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?



a.

Henry Moseley

c.

John Dalton

b.

Antoine Lavoisier

d.

Dmitri Mendeleev

____ 13. Which of the following categories includes the majority of the elements?



a.

metalloids

c.

metals

b.

liquids

d.

nonmetals

____ 14. Of the elements Pt, V, Li, and Kr, which is a nonmetal?



a.

Pt

c.

Li

b.

V

d.

Kr

____ 15. To what category of elements does an element belong if it is a poor conductor of electricity?



a.

transition elements

c.

nonmetals

b.

metalloids

d.

metals

____ 16. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?



a.

In, 49 protons, 49 electrons

c.

Cs, 55 protons, 132.9 electrons

b.

Zn, 30 protons, 60 electrons

d.

F, 19 protons, 19 electrons

____ 17. The atomic number of an element is the total number of which particles in the nucleus?



a.

neutrons

c.

electrons

b.

protons

d.

protons and electrons

____ 18. What element has the electron configuration 1s2s2p3s3p?



a.

nitrogen

c.

silicon

b.

selenium

d.

silver

____ 19. Which of the following is true about the electron configurations of the noble gases?



a.

The highest occupied s and p sublevels are completely filled.

b.

The highest occupied s and p sublevels are partially filled.

c.

The electrons with the highest energy are in a d sublevel.

d.

The electrons with the highest energy are in an f sublevel.

____ 20. Elements that are characterized by the filling of p orbitals are classified as ____.



a.

groups 3A through 8A

c.

inner transition metals

b.

transition metals

d.

groups 1A and 2A

____ 21. Which of the following electron configurations is most likely to result in an element that is relatively inactive?



a.

a half-filled energy sublevel

b.

a filled energy sublevel

c.

one empty and one filled energy sublevel

d.

a filled highest occupied principal energy level

____ 22. Which subatomic particle plays the greatest part in determining the properties of an element?



a.

proton

c.

neutron

b.

electron

d.

none of the above

____ 23. Which of the following elements is a transition metal?



a.

cesium

c.

tellurium

b.

copper

d.

tin

____ 24. Which of the following groupings contains only representative elements?



a.

Cu, Co, Cd

c.

Al, Mg, Li

b.

Ni, Fe, Zn

d.

Hg, Cr, Ag

____ 25. Which of the following is true about the electron configurations of the representative elements?



a.

The highest occupied s and p sublevels are completely filled.

b.

The highest occupied s and p sublevels are partially filled.

c.

The electrons with the highest energy are in a d sublevel.

d.

The electrons with the highest energy are in an f sublevel.

____ 26. What are the Group 1A and Group 7A elements examples of?



a.

representative elements

c.

noble gases

b.

transition elements

d.

nonmetallic elements

____ 27. Of the elements Fe, Hg, U, and Te, which is a representative element?



a.

Fe

c.

U

b.

Hg

d.

Te

____ 28. How does atomic radius change from top to bottom in a group in the periodic table?



a.

It tends to decrease.

c.

It first increases, then decreases.

b.

It tends to increase.

d.

It first decreases, then increases.

____ 29. How does atomic radius change from left to right across a period in the periodic table?



a.

It tends to decrease.

c.

It first increases, then decreases.

b.

It tends to increase.

d.

It first decreases, then increases.

____ 30. What causes the shielding effect to remain constant across a period?



a.

Electrons are added to the same principal energy level.

b.

Electrons are added to different principal energy levels.

c.

The charge on the nucleus is constant.

d.

The atomic radius increases.

____ 31. Atomic size generally ____.



a.

increases as you move from left to right across a period

b.

decreases as you move from top to bottom within a group

c.

remains constant within a period

d.

decreases as you move from left to right across a period

____ 32. What element in the second period has the largest atomic radius?



a.

carbon

c.

potassium

b.

lithium

d.

neon

____ 33. Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?



a.

more shielding of the electrons by the highest occupied energy level

b.

an increase in size of the nucleus

c.

an increase in number of protons

d.

fewer electrons in the highest occupied energy level

____ 34. Which of the following elements has the smallest atomic radius?



a.

sulfur

c.

selenium

b.

chlorine

d.

bromine

____ 35. What is the charge of a cation?



a.

a positive charge

b.

no charge

c.

a negative charge

d.

The charge depends on the size of the nucleus.

____ 36. Which of the following statements is true about ions?



a.

Cations form when an atom gains electrons.

b.

Cations form when an atom loses electrons.

c.

Anions form when an atom gains protons.

d.

Anions form when an atom loses protons.

____ 37. The metals in Groups 1A, 2A, and 3A ____.



a.

gain electrons when they form ions

c.

all have ions with a 1 charge

b.

all form ions with a negative charge

d.

lose electrons when they form ions

____ 38. Which of the following statements is NOT true about ions?



a.

Cations are positively charged ions.

b.

Anions are common among nonmetals.

c.

Charges for ions are written as numbers followed by a plus or minus sign.

d.

When a cation forms, more electrons are transferred to it.

____ 39. Why is the second ionization energy greater than the first ionization energy?



a.

It is more difficult to remove a second electron from an atom.

b.

The size of atoms increases down a group.

c.

The size of anions decreases across a period.

d.

The nuclear attraction from protons in the nucleus decreases.

____ 40. In which of the following sets are the charges given correctly for all the ions?



a.

Na, Mg, Al

c.

Rb, Ba, P

b.

K, Sr, O

d.

N, O, F

____ 41. In which of the following groups of ions are the charges all shown correctly?



a.

Li, O, S

c.

K, F, Mg

b.

Ca, Al, Br

d.

Na, I, Rb

____ 42. What is the element with the lowest electronegativity value?



a.

cesium

c.

calcium

b.

helium

d.

fluorine

____ 43. What is the element with the highest electronegativity value?



a.

cesium

c.

calcium

b.

helium

d.

fluorine

____ 44. Which of the following elements has the smallest ionic radius?



a.

Li

c.

O

b.

K

d.

S

____ 45. What is the energy required to remove an electron from an atom in the gaseous state called?



a.

nuclear energy

c.

shielding energy

b.

ionization energy

d.

electronegative energy

____ 46. For Group 2A metals, which electron is the most difficult to remove?



a.

the first

b.

the second

c.

the third

d.

All the electrons are equally difficult to remove.

____ 47. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?



a.

increase in atomic size

b.

increase in size of the nucleus

c.

increase in number of protons

d.

fewer electrons in the highest occupied energy level

____ 48. Which of the following elements has the smallest first ionization energy?



a.

sodium

c.

potassium

b.

calcium

d.

magnesium

____ 49. Which of the following elements has the lowest electronegativity?



a.

lithium

c.

bromine

b.

carbon

d.

fluorine

____ 50. Which statement is true about electronegativity?



a.

Electronegativity is the ability of an anion to attract another anion.

b.

Electronegativity generally increases as you move from top to bottom within a group.

c.

Electronegativity generally is higher for metals than for nonmetals.

d.

Electronegativity generally increases from left to right across a period.

____ 51. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.



a.

lower

c.

the same

b.

higher

d.

unpredictable

____ 52. Which of the following decreases with increasing atomic number in Group 2A?



a.

shielding effect

c.

ionization energy

b.

ionic size

d.

number of electrons

____ 53. Which of the following statements correctly compares the relative size of an ion to its neutral atom?



a.

The radius of an anion is greater than the radius of its neutral atom.

b.

The radius of an anion is identical to the radius of its neutral atom.

c.

The radius of a cation is greater than the radius of its neutral atom.

d.

The radius of a cation is identical to the radius of its neutral atom.

____ 54. Which of the following factors contributes to the increase in ionization energy from left to right across a period?



a.

an increase in the shielding effect

b.

an increase in the size of the nucleus

c.

an increase in the number of protons

d.

fewer electrons in the highest occupied energy level

____ 55. As you move from left to right across the second period of the periodic table ____.



a.

ionization energy increases

c.

electronegativity decreases

b.

atomic radii increase

d.

atomic mass decreases

____ 56. Of the following elements, which one has the smallest first ionization energy?



a.

boron

c.

aluminum

b.

carbon

d.

silicon



Numeric Response
57. How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
58. How many electrons are present in the d sublevel of a neutral atom of nickel?
59. What is the usual charge on an ion from Group 7A?
Matching
Match each item with the correct statement below.

a.

macronutrients

d.

atomic radius

b.

trace amount

e.

electronegativity

c.

periodic

f.

ionization energy

____ 60. A/An __________________ event is an event that is repeated at regular intervals.


____ 61. Sodium, calcium and phosphorus are __________________ because they are needed in large quantities in your body.
____ 62. The __________________ is the energy required to remove an electron from an atom.
____ 63. When a substance is present in extremely small quantities, we say it is present in a/an __________________.
____ 64. The distance between the nucleus of an atom and its “outer edge” is called the __________________.
____ 65. An atom’s ability to attract electrons from other atoms is referred to as __________________.
Match each item with the correct statement below.

a.

electronegativity

f.

periodic law

b.

ionization energy

g.

cation

c.

atomic radius

h.

period

d.

metal

i.

group

e.

transition metal

j.

electrons

____ 66. horizontal row in the periodic table


____ 67. vertical column in the periodic table
____ 68. A repetition of properties occurs when elements are arranged in order of increasing atomic number.
____ 69. type of element that is a good conductor of heat and electric current
____ 70. type of element characterized by the presence of electrons in the d orbital
____ 71. one-half the distance between the nuclei of two atoms when the atoms are joined
____ 72. type of ion formed by Group 2A elements
____ 73. subatomic particles that are transferred to form positive and negative ions
____ 74. ability of an atom to attract electrons when the atom is in a compound
____ 75. energy required to remove an electron from an atom
Problem
Write the full electron configuration for the following element.
76. Oxygen (O)
77. Nickel (Ni)
78. Magnesium (Mg)
79. Aluminum (Al)
80. Phosphorus (P)
81. Bromine (Br)
Essay
82. Describe the trends in the atomic size of elements within groups and across periods in the periodic table. Provide examples.
83. Explain how ions form. Provide examples.
84. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the atoms from which they are formed. Explain why this is so.

The Periodic Table

Answer Section
MULTIPLE CHOICE
1. ANS: D PTS: 1 DIF: Easy REF: Section 6.1
2. ANS: C PTS: 1 DIF: Easy REF: Section 6.1
3. ANS: B PTS: 1 DIF: Easy REF: Section 6.1
4. ANS: A PTS: 1 DIF: Easy REF: Section 6.1
5. ANS: B PTS: 1 DIF: Easy REF: Section 6.2
6. ANS: D PTS: 1 DIF: Easy REF: Section 6.2
7. ANS: A PTS: 1 DIF: L1 REF: p. 164

OBJ: 6.1.1 STA: GOAL 3.01.c


8. ANS: C PTS: 1 DIF: L1 REF: p. 166

OBJ: 6.1.1 STA: GOAL 3.01.c


9. ANS: B PTS: 1 DIF: L1 REF: p. 162 | p. 163

OBJ: 6.1.1 STA: GOAL 3.01.b


10. ANS: A PTS: 1 DIF: L2 REF: p. 157

OBJ: 6.1.1 STA: GOAL 3.01.b


11. ANS: C PTS: 1 DIF: L2 REF: p. 157

OBJ: 6.1.1 STA: GOAL 3.01.b


12. ANS: D PTS: 1 DIF: L1 REF: p. 156

OBJ: 6.1.2 STA: GOAL 3.01


13. ANS: C PTS: 1 DIF: L1 REF: p. 158

OBJ: 6.1.3 STA: GOAL 3.01.c


14. ANS: D PTS: 1 DIF: L2 REF: p. 158

OBJ: 6.1.3 STA: GOAL 3.01.c


15. ANS: C PTS: 1 DIF: L3 REF: p. 160

OBJ: 6.1.3 STA: GOAL 3.01.c


16. ANS: A PTS: 1 DIF: L1 REF: p. 162 | p. 163

OBJ: 6.2.1 STA: GOAL 3.01.c


17. ANS: A PTS: 1 DIF: L2 REF: p. 157

OBJ: 6.2.1 STA: GOAL 2.02.c


18. ANS: C PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.2 STA: GOAL 3.01.d


19. ANS: A PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.2 STA: GOAL 3.01.d


20. ANS: A PTS: 1 DIF: L2 REF: p. 166

OBJ: 6.2.2 STA: GOAL 3.01.d


21. ANS: D PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.2 STA: GOAL 3.01.d


22. ANS: B PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.2 STA: GOAL 3.01.d


23. ANS: B PTS: 1 DIF: L1 REF: p. 166

OBJ: 6.2.3 STA: GOAL 3.01.c


24. ANS: C PTS: 1 DIF: L1 REF: p. 164 | p. 166

OBJ: 6.2.3 STA: GOAL 3.01.c


25. ANS: B PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.2 | 6.2.3 STA: GOAL 3.01.c | GOAL 3.01.d


26. ANS: A PTS: 1 DIF: L2 REF: p. 164

OBJ: 6.2.3 STA: GOAL 3.01.c


27. ANS: D PTS: 1 DIF: L3 REF: p. 162 | p. 163 | p. 164

OBJ: 6.2.3 STA: GOAL 3.01.c


28. ANS: B PTS: 1 DIF: L1 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.f


29. ANS: A PTS: 1 DIF: L2 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.f


30. ANS: A PTS: 1 DIF: L2 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.d


31. ANS: D PTS: 1 DIF: L2 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.c


32. ANS: B PTS: 1 DIF: L2 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.f


33. ANS: A PTS: 1 DIF: L3 REF: p. 171

OBJ: 6.3.1 STA: GOAL 3.01.d


34. ANS: B PTS: 1 DIF: L3 REF: p. 171 | p. 175

OBJ: 6.3.1 STA: GOAL 3.01.f


35. ANS: A PTS: 1 DIF: L1 REF: p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


36. ANS: B PTS: 1 DIF: L2 REF: p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


37. ANS: D PTS: 1 DIF: L2 REF: p. 162 | p. 163 | p. 172 | p. 176

OBJ: 6.3.2 STA: GOAL 3.01.e


38. ANS: D PTS: 1 DIF: L2 REF: p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


39. ANS: A PTS: 1 DIF: L2 REF: p. 173

OBJ: 6.3.2 STA: GOAL 3.01.e


40. ANS: B PTS: 1 DIF: L3 REF: p. 162 | p. 163 | p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


41. ANS: B PTS: 1 DIF: L3 REF: p. 162 | p. 163 | p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


42. ANS: A PTS: 1 DIF: L1 REF: p. 177

OBJ: 6.3.3 STA: GOAL 3.01.g


43. ANS: D PTS: 1 DIF: L1 REF: p. 177

OBJ: 6.3.3 STA: GOAL 3.01.g


44. ANS: A PTS: 1 DIF: L2 REF: p. 175

OBJ: 6.3.3 STA: GOAL 3.01.f


45. ANS: B PTS: 1 DIF: L2 REF: p. 173

OBJ: 6.3.3 STA: GOAL 3.01.e


46. ANS: C PTS: 1 DIF: L2 REF: p. 173

OBJ: 6.3.3 STA: GOAL 3.01.d


47. ANS: A PTS: 1 DIF: L2 REF: p. 174

OBJ: 6.3.1 | 6.3.3 STA: GOAL 3.01.d


48. ANS: C PTS: 1 DIF: L2 REF: p. 173

OBJ: 6.3.3 STA: GOAL 3.01.d


49. ANS: A PTS: 1 DIF: L2 REF: p. 177

OBJ: 6.3.3 STA: GOAL 3.01.g


50. ANS: D PTS: 1 DIF: L2 REF: p. 177

OBJ: 6.3.3 STA: GOAL 3.01.g


51. ANS: B PTS: 1 DIF: L2 REF: p. 177 | p. 178

OBJ: 6.3.3 STA: GOAL 3.01.g


52. ANS: C PTS: 1 DIF: L2 REF: p. 178

OBJ: 6.3.1 | 6.3.3 STA: GOAL 3.01.e


53. ANS: A PTS: 1 DIF: L2 REF: p. 172 | p. 176

OBJ: 6.3.3 STA: GOAL 3.01.e


54. ANS: C PTS: 1 DIF: L3 REF: p. 174

OBJ: 6.3.3 STA: GOAL 3.01.e


55. ANS: A PTS: 1 DIF: L3 REF: p. 178

OBJ: 6.2.1 | 6.3.3 STA: GOAL 3.01.e


56. ANS: C PTS: 1 DIF: L3 REF: p. 173

OBJ: 6.3.3 STA: GOAL 3.01.e


NUMERIC RESPONSE
57. ANS: 5

PTS: 1 DIF: L2 REF: p. 164 OBJ: 6.2.2

STA: GOAL 3.01.d
58. ANS: 8

PTS: 1 DIF: L2 REF: p. 166 OBJ: 6.2.2 | 6.2.3

STA: GOAL 3.01.d
59. ANS: 1

PTS: 1 DIF: L2 REF: p. 172 OBJ: 6.3.2

STA: GOAL 3.01.d
MATCHING
60. ANS: C PTS: 1 DIF: Easy REF: Section 6.1
61. ANS: A PTS: 1 DIF: Easy REF: Section 6.1
62. ANS: F PTS: 1 DIF: Easy REF: Section 6.1
63. ANS: B PTS: 1 DIF: Easy REF: Section 6.1
64. ANS: D PTS: 1 DIF: Easy REF: Section 6.1
65. ANS: E PTS: 1 DIF: Easy REF: Section 6.1
66. ANS: H PTS: 1 DIF: L1 REF: p. 157

OBJ: 6.1.1 STA: GOAL 3.01.b


67. ANS: I PTS: 1 DIF: L1 REF: p. 157

OBJ: 6.1.1 STA: GOAL 3.01.a


68. ANS: F PTS: 1 DIF: L1 REF: p. 157

OBJ: 6.1.1 STA: GOAL 3.01


69. ANS: D PTS: 1 DIF: L1 REF: p. 158

OBJ: 6.1.3 STA: GOAL 3.01.c


70. ANS: E PTS: 1 DIF: L1 REF: p. 166

OBJ: 6.2.2 STA: GOAL 3.01.c


71. ANS: C PTS: 1 DIF: L1 REF: p. 170

OBJ: 6.3.1 STA: GOAL 3.01.f


72. ANS: G PTS: 1 DIF: L1 REF: p. 172

OBJ: 6.3.2 STA: GOAL 3.01.e


73. ANS: J PTS: 1 DIF: L1 REF: p. 172

OBJ: 6.3.2 STA: GOAL 2.02.a


74. ANS: A PTS: 1 DIF: L1 REF: p. 177

OBJ: 6.3.3 STA: GOAL 3.01.g


75. ANS: B PTS: 1 DIF: L1 REF: p. 173

OBJ: 6.3.3 STA: GOAL 3.01.e


PROBLEM
76. ANS:

1s22s22p4

PTS: 2 DIF: Average REF: Section 6.2
77. ANS:

1s22s22p63s23p63d84s2

PTS: 3 DIF: Challenging REF: Section 6.2
78. ANS:

1s22s22p63s2

PTS: 2 DIF: Average REF: Section 6.2
79. ANS:

1s22s22p63s23p1

PTS: 2 DIF: Average REF: Section 6.2
80. ANS:

1s22s22p63s23p3

PTS: 2 DIF: Average REF: Section 6.2
81. ANS:

1s22s22p63s23p63d104s24p5

PTS: 3 DIF: Challenging REF: Section 6.2
ESSAY
82. ANS:

Atomic size increases with increasing atomic number within a group. For example, sodium atoms are larger than lithium atoms, and potassium atoms are larger than sodium atoms. Atomic size decreases with increasing atomic number across a period. For example, lithium atoms are larger than beryllium atoms, and beryllium atoms are larger than boron atoms.

PTS: 1 DIF: L2 REF: p. 171 OBJ: 6.3.1

STA: GOAL 2.02.c


83. ANS:

Ions form when electrons are transferred among atoms. For example, a group 1A element, such as potassium, tends to transfer one electron to other atoms, causing it to form a net positive charge, in this case K. Such ions with net positive charges are called cations. Ions with net negative charges are anions. Nonmetal atoms, such as chlorine, tend to accept electrons from other atoms. Chlorine tends to gain a single electron, forming the anion Cl.

PTS: 1 DIF: L2 REF: p. 172 OBJ: 6.3.2

STA: GOAL 3.01.e


84. ANS:

When an electron is added to an atom, the attraction of the nucleus for any one electron decreases and the size of the ion’s radius increases. When an electron is removed from an atom, there is an increase in the nuclear attraction experienced by the remaining electrons. Consequently, the remaining electrons are drawn closer to the nucleus.



PTS: 1 DIF: L3 REF: p. 176 OBJ: 6.3.3

STA: GOAL 3.01.e


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