Chapter 6: The Periodic Table Multiple Choice



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Chapter 6: The Periodic Table
Multiple Choice

Identify the choice that best completes the statement or answers the question.
____ 1. Which of the following elements is in the same period as phosphorus?

a.

carbon

c.

nitrogen

b.

magnesium

d.

oxygen

____ 2. Each period in the periodic table corresponds to ____.



a.

a principal energy level

c.

an orbital

b.

an energy sublevel

d.

a suborbital

____ 3. The modern periodic table is arranged in order of increasing atomic ____.



a.

mass

c.

number

b.

charge

d.

radius

____ 4. 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

____ 5. Which of the following categories includes the majority of the elements?



a.

metalloids

c.

metals

b.

liquids

d.

nonmetals

____ 6. Of the elements Pt, V, Li, and Kr, which is a nonmetal?



a.

Pt

c.

Li

b.

V

d.

Kr

____ 7. 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

____ 8. 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

____ 9. What element has the electron configuration 1s2s2p3s3p?



a.

nitrogen

c.

silicon

b.

selenium

d.

silver

____ 10. 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.

____ 11. 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

____ 12. 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

____ 13. 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

____ 14. 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

____ 15. What element in the second period has the largest atomic radius?



a.

carbon

c.

potassium

b.

lithium

d.

neon

____ 16. 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.

____ 17. 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.

____ 18. 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

____ 19. 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 because nuclear attraction increases.

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.

____ 20. 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

____ 21. What is the element with the highest electronegativity value?



a.

cesium

c.

calcium

b.

helium

d.

fluorine

____ 22. 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

____ 23. 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.

____ 24. Which of the following elements has the smallest first ionization energy?



a.

sodium

c.

potassium

b.

calcium

d.

magnesium

____ 25. 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.

Essay
26. Atomic size of elements vary in the periodic table.

(Include the following vocabulary = nuclear attraction and nuclear shielding)

A. How does the atomic size change in a period. Explain the causes for change in size within a period.

B. How does the atomic size change in a group. Explain the causes for the change in size within a group.

27. The graphs show the relationship between the electronegativities and first ionization energies for period 2 and period 3 elements.
a. Based on data for these two periods, what is the general trend between these two values?

b. Use nuclear charge and shielding effect to explain this trend.



Chapter 6: The Periodic Table

Answer Section
MULTIPLE CHOICE
1. B
2. A
3. C
4. D
5. C
6. D
7. C
8. A
9. C
10. A
11. A
12. D
13. B
14. C
15. B
16. A
17. B
18. D
19. A
20. B
21. D
22. B
23. C
24. C
25. A
ESSAY
26. 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.
27. a. electronegativitiy increases as first ionization energy increases.

b. both properties depend on the attraction between the nucleus and electrons in the highest occupied energy level. Across a period, the nuclear charge increases, but the shielding effect is constant.


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