Quiz 9

*picture* is the lewis electron diagram of __________ a. O2+ b. O- c. O d. O2- e. O+

O2-

Identify the correct Lewis electron diagram for CO 2. *picture*

a.

How many electrons should a Ca atom lose to satisfy the octet rule? a. 2 b. 8 c. 1 d. 3 e. 4

a. 2

Which of the following ions contain an octet of valence electrons? a. F- b. Ba+ c. O- d. Na2+ e. N2-

a. F-

Which of the following molecules is not linear in shape? a. PCl3 b. CO2 c. BeH2 d. O2 e. NO

a. PCl3

Which of the following bonds is formed when electrons are shared between atoms? a. covalent bond b. ionic bond c. metallic bond d. dipole interaction e. valence bond

a. covalent bond

Which of the following is used to represent the Na atom using the Lewis electron dot diagram?

b. Na *

What is the energy change for this reaction? (Refer to Table 9.2 in the text.) a. -4.00 kJ/mol b. -183 kJ/mol c. -129 kJ/mol d. -477 kJ/mol e. 477 kJ/mol

b. -183 kJ/mol

Atoms like to have _____ electrons in their valence shell to remain stable. a. 3 b. 8 c. 5 d. 4 e. 6

b. 8

Which of the following molecules is likely to have a trigonal planar electron group distribution? a. NO b. BF3 c. CO2 d. H2O e. NO2

b. BF3

Which of the following occurs when Ca reacts with Cl 2 to form CaCl 2? a. Ca gains two electrons to become Ca2+ b. Ca loses two electrons to become Ca2+ c. Cl atoms loses 2 electrons each to become Cl2- d. Cl2 gains two electrons to become Cl22+ e. Cl2 loses two electrons to become Cl22-

b. Ca loses two electrons to become Ca2+

_____ is a scale for judging how much atoms of any element attract electrons. a. Electron affinity b. Electronegetavity c. Magnetivity d. Electron density e. Reactivity

b. Electronegetavity

Atoms like to have _____ electrons in their valence shell to remain stable. a. CO2 b. F2 c. O2 d. NaCl e. N2

b. F2

Which of the following bonds is most likely ionic? a. H-Br b. Li-F c. P-H d. H-I e. C-C

b. Li-F

Which of the following molecules will have a trigonal pyramidal molecular structure? a. CH4 b. PCl3 c. NaCl d. NO2 e. CaCl2

b. PCl3

Two hydrogen atoms share electrons to form a stable compound. This type of a bond is called a(n)_____ bond. a. ionic b. covalent c. hydrogen d. dipole e. metallic

b. covalent

What column of the periodic table has Lewis electron dot diagrams that have four electrons in them? a. the column headed by nitrogen b. the column headed by carbon c. the column headed by fluorine d. the column headed by oxygen e. the column headed by boron

b. the column headed by carbon

Identify the molecule with a tetrahedral molecular structure. a. PCl3 b. CH2O c. CH4 d. NOF e. NH3

c. CH4

In the molecule CO 2, how many electrons are shared by C and the two O atoms? a. 5 b. 6 c. 4 d. 8 e. 10

d. 8

NaCl remains stable due to the attraction between the Na + and Cl - ions. This attraction is called a(n)_____. a. chemical bond b. dipole attraction c. metallic bond d. ionic bond e. covalent bond

d. Ionic bond

A(n) _____ is a representation of the valence electrons of an atom that uses dots around the symbol of the element. a. molecular electron geometry b. molecular electron graph c. structural electron formula d. Lewis electron dot diagram e. orbital electron diagram

d. Lewis dot diagram

If the electronegativity of a bond formed between two atoms is 0.15, it is likely to be a(n)_____ bond. a. likely ionic b. slightly ionic c. nonpolar covalent d. slightly polar covalent e. definitely polar covalent

d. slightly polar covalent

Diatomic molecules are linear because _____. a. electron-deficient molecules cannot be formed of only two electron groups b. they form odd-electron molecules around the central atom c. bonds in such compounds have a polarity of less than 0.4 d. there are only two atoms in the molecule e. only polar covalent bonds are formed in such molecules

d. there are only two atoms in the molecule

*picture* is the Lewis electron diagram for _____. a. BF4 b. BF42+ c. BF4+ d. BF42- e. BF4-

e. BF4-

For a chlorine atom to complete an octet, it must _____ a. lose an electron b. gain five electrons c. lose two electrons d. gain two electrons e. gain an electron

e. gain an electron