EP 4 Sample Exam Questions Midterm 1 ch 6

ep 4 review

Matching

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


____ 1. horizontal row in the periodic table

____ 2. vertical column in the periodic table

____ 3. A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____ 4. type of element that is a good conductor of heat and electric current

____ 5. type of element characterized by the presence of electrons in the d orbital

____ 6. one-half the distance between the nuclei of two atoms when the atoms are joined

____ 7. type of ion formed by Group 2A elements

____ 8. subatomic particles that are transferred to form positive and negative ions

____ 9. ability of an atom to attract electrons when the atom is in a compound

____ 10. energy required to remove an electron from an atom

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

____ 11. 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


____ 12. 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


____ 13. What is the element with the lowest electronegativity value?
a. cesium c. calcium
b. helium d. fluorine


____ 14. Which of the following elements has the smallest first ionization energy?
a. sodium c. potassium
b. calcium d. magnesium


____ 15. Which of the following elements has the lowest electronegativity?
a. lithium c. bromine
b. carbon d. fluorine


____ 16. 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.


____ 17. 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


____ 18. 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


____ 19. 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


____ 20. Of the following elements, which one has the smallest first ionization energy?
a. boron c. aluminum
b. carbon d. silicon


Short Answer

21. Which group of elements in the periodic table is known as the alkali metals?

22. Which group in the periodic table is known as the noble gases?

23. An element has an atomic number of 80. How many protons and electrons are in an atom of the element?

24. About what percent of elements is classified as metals?

25. What is the electron configuration of oxygen?

26. What is the electron configuration of sulfur?

27. The s and p sublevels of an atom of an element in period 3 are filled with electrons. Which orbitals are filled in this atom?

28. From which orbital in a lithium atom is an electron transferred to form Li ?

29. What orbital is filled when iodine gains an electron to become a negative ion?

30. In which group in the periodic table do the elements have the highest electronegativity values?

ep 4 review
Answer Section

MATCHING

1. ANS: H DIF: L1 REF: p. 157 OBJ: 6.1.1

2. ANS: I DIF: L1 REF: p. 157 OBJ: 6.1.1

3. ANS: F DIF: L1 REF: p. 157 OBJ: 6.1.1

4. ANS: D DIF: L1 REF: p. 158 OBJ: 6.1.3

5. ANS: E DIF: L1 REF: p. 166 OBJ: 6.2.2

6. ANS: C DIF: L1 REF: p. 170 OBJ: 6.3.1

7. ANS: G DIF: L1 REF: p. 172 OBJ: 6.3.2

8. ANS: J DIF: L1 REF: p. 172 OBJ: 6.3.2

9. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

10. ANS: B DIF: L1 REF: p. 173 OBJ: 6.3.3

MULTIPLE CHOICE

11. ANS: B DIF: L3 REF: p. 162, p. 163, p. 172
OBJ: 6.3.2

12. ANS: B DIF: L3 REF: p. 162, p. 163, p. 172
OBJ: 6.3.2

13. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

14. ANS: C DIF: L2 REF: p. 173 OBJ: 6.3.3

15. ANS: A DIF: L2 REF: p. 177 OBJ: 6.3.3

16. ANS: D DIF: L2 REF: p. 177 OBJ: 6.3.3

17. ANS: B DIF: L2 REF: p. 177, p. 178
OBJ: 6.3.3

18. ANS: C DIF: L3 REF: p. 174 OBJ: 6.3.3

19. ANS: A DIF: L3 REF: p. 178 OBJ: 6.2.1, 6.3.3

20. ANS: C DIF: L3 REF: p. 173 OBJ: 6.3.3

SHORT ANSWER

21. ANS:
1A

DIF: L1 REF: p. 161 OBJ: 6.1.1

22. ANS:
8A

DIF: L1 REF: p. 164 OBJ: 6.1.1

23. ANS:
80 protons, 80 electrons

DIF: L1 REF: p. 157 OBJ: 6.2.1

24. ANS:
80%

DIF: L2 REF: p. 158 OBJ: 6.1.3, 6.2.1

25. ANS:
1s 2s 2p

DIF: L2 REF: p. 162, p. 166 OBJ: 6.2.2

26. ANS:
1s 2s 2p 3s 3p

DIF: L2 REF: p. 166 OBJ: 6.2.2

27. ANS:
1s, 2s, 2p

DIF: L3 REF: p. 166 OBJ: 6.2.2

28. ANS:
2s

DIF: L2 REF: p. 164, p. 172 OBJ: 6.3.2

29. ANS:
5p

DIF: L3 REF: p. 166 OBJ: 6.2.2, 6.3.2

30. ANS:
7A

DIF: L2 REF: p. 177 OBJ: 6.3.3