Deck 9: Covalent Bonding and Molecules

Question 1

Ozone has the formula O₃. Which statement is CORRECT concerning ozone?

A) One oxygen atom has a +1 formal charge while another has a -1 formal charge. The third one is neutral.
B) All three atoms are neutral.
C) Two atoms have a -1 formal charge, and the third oxygen atom has a +1 formal charge.
D) Two atoms have a +1 formal charge, and the third oxygen atom has a -1 formal charge.

Answer 1

One oxygen atom has a +1 formal charge while another has a -1 formal charge. The third one is neutral.

Question 2

A ClO₂^- ion has _____ valence electrons.

A) 16
B) 18
C) 20
D) 22

Answer 2

20

Question 3

Which compound has 24 valence electrons?

A) C₃H₆O
B) C₂H₆O
C) CO₂
D) HCN

Answer 3

C₃H₆O

Question 4

What is the formal charge on the oxygen atom in this structure?

A) +1
B) +2
C) -1
D) -2

Question 5

Which Lewis structure BEST describes the carbonate ion?

A) a
B) b
C) c
D) d

Question 6

How many atoms in this molecule have a trigonal planar geometry?

A) one
B) two
C) three
D) four

Question 7

Which statement is CORRECT concerning the cyanide ion?

A) The carbon atom has a tetrahedral geometry, and the nitrogen atom has a liner geometry.
B) The carbon atom has a trigonal planar geometry, and the nitrogen atom has a liner geometry.
C) Both atoms have a linear geometry.
D) Both atoms have a trigonal planar geometry.

Question 8

What is the electronic geometry around the oxygen atoms in CO₂?

A) trigonal planar
B) linear
C) tetrahedral
D) bent

Question 9

Which Lewis structure, although acceptable, LEAST describes the carbonate ion?

A) a
B) b
C) c
D) d

Question 10

A oxygen atom with one bond and three lone pairs has a charge of:

A) +1.
B) +2.
C) -1.
D) -2.

Question 11

In this Lewis structure, which atom does NOT have a complete valence?

A) H
B) B
C) C
D) Cl

Question 12

What is the formal charge on the nitrogen atom in this structure?

A) +1
B) +2
C) -1
D) -3

Question 13

A neutral carbon atom has _____ valence electrons.

A) two
B) four
C) five
D) eight

Question 14

Which molecule does NOT have a lone pair on the central atom?

A) NH₃
B) SF₂
C) PCl₃
D) CO₂

Question 15

Which compound has an expanded octet around the central atom?

A) NH₃
B) PCl₃
C) SF₆
D) CF₄

Question 16

A neutral sulfur atom has _____ valence electrons.

A) two
B) four
C) six
D) eight

Question 17

The Lewis structure of the cyanide ion is shown here. How many valence electrons are in this ion?

A) 11
B) 10
C) 8
D) 7

Question 18

How many atoms in this molecule have a tetrahedral geometry?

A) one
B) two
C) three
D) four

Question 19

A phosphorus atom with four bonds has a charge of:

A) +1.
B) +2.
C) -1.
D) -2.

Question 20

What is the electronic geometry around the central atom in CO₂?

A) trigonal planar
B) linear
C) tetrahedral
D) bent

Question 21

Based on the Pauling electronegativities, an Fr-F bond is:

A) ionic.
B) covalent.
C) polar ionic.
D) polar covalent.

Question 22

Which molecule will have the STRONGEST attraction to another molecule of its own kind?

A) a
B) b
C) c
D) d

Question 23

Based on the Pauling electronegativities, a P-Cl bond is:

A) ionic.
B) covalent.
C) polar ionic.
D) polar covalent.

Question 24

Which atom is the MOST electronegative?

A) Ca
B) Sr
C) Ba
D) Be

Question 25

Which structure BEST describes the polarity of an H-O bond?

A) a
B) b
C) c

Question 26

Which atom is the MOST electronegative?

A) Li
B) C
C) P
D) O

Question 27

Based on the Pauling electronegativities, a C-H bond is:

A) ionic.
B) covalent.
C) polar ionic.
D) polar covalent.

Question 28

Which molecule has a NET DIPOLE?

A) a
B) b
C) c
D) d

Question 29

What is the correct ELECTRONIC GEOMETRY and MOLECULAR GEOMETRY around the central nitrogen in NO₂^-? (Hint: You may need to draw the molecule.)

A) tetrahedral, trigonal pyramidal
B) tetrahedral, tetrahedral
C) linear, linear
D) trigonal planar, bent

Question 30

Which molecule(s) is/are likely to be a gas at room temperature due to a lack of attraction to another molecule of its own kind?

A) a, b, and c
B) a, c, and d
C) b
D) c and d