General Chemistry 1 Practice Questions (Set 9)

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1) Which of the following represents the Lewis structure for N?

2) Give the complete electronic configuration for Br-.
A) 1s22s22p63s23p64s24p6
B) 1s22s22p63s23p64s24d104p6
C) 1s22s22p63s23p64s23d104p6
D) 1s22s22p63s23p64s23d104p5
E) 1s22s2p63s2p64s23d104p6

3) Give the complete electronic configuration for Ca2+.
A) 1s22s22p63s24p6
B) 1s22s22p63s23p6
C) 1s22s22p63s23p5
D) 1s22s23p64s25p6
E) 1s22s2p63s2p6

4) Which of the following statements is TRUE?
A) An ionic bond is much stronger than most covalent bonds.
B) An ionic bond is formed through the sharing of electrons.
C) Ionic compounds at room temperature typically conduct electricity.
D) Once dissolved in water, ionic compounds rarely conduct electricity.
E) None of the above is true.

5) Use Lewis theory to determine the chemical formula for the compound formed between Al and O.
A) Al3O2
B) Al2O3
C) AlO2
D) Al2O
E) AlO

6) Identify the shortest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) All of the above bonds are the same length.

7) Identify the weakest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) All of the above bonds are the same strength.

8) Identify the strongest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) All of the above bonds are the same strength.

9) Identify the number of bonding pairs and lone pairs of electrons in water.
A) 1 bonding pair and 1 lone pair
B) 1 bonding pair and 2 lone pairs
C) 2 bonding pairs and 2 lone pairs
D) 2 bonding pairs and 1 lone pair
E) 3 bonding pairs and 2 lone pairs

10) Define electronegativity.
A) the ability of an atom to repel neutrons in a chemical bond
B) the ability of an atom to repel electrons in a chemical bond
C) the ability of an atom to attract protons to itself in a chemical bond
D) the ability of an atom to attract neutrons to itself in a chemical bond
E) the ability of an atom to attract electrons to itself in a chemical bond

11) Choose the best Lewis structure for CH2Cl2.

12) Choose the best Lewis structure for BF3.

13) Define bond energy.
A) energy required to form 1 mole of the bond in the solid phase
B) energy required to form 1 mole of the bond in the gas phase
C) energy required to break 1 mole of the bond in the liquid phase
D) energy required to break 1 mole of the bond in the gas phase
E) energy required to break 1 mole of the bond in the solid phase

14) A reaction is exothermic when
A) weak bonds break and strong bonds form.
B) strong bonds break and weak bonds form.
C) weak bonds break and weak bonds form.
D) strong bonds break and strong bonds form.

15) Which compound has the longest carbon-carbon bond length?
A) CH3CH3
B) CH2CH2
C) HCCH
D) All bond lengths are the same.

16) Which compound has the shortest carbon-carbon bond length?
A) CH3CH3
B) CH2CH2
C) HCCH
D) All bond lengths are the same.
17) Which compound has the highest carbon-carbon bond strength?
A) CH3CH3
B) CH2CH2
C) HCCH
D) All bond strengths are the same.

18) Use the bond energies provided to estimate ?H°rxn for the reaction below.
Use the bond energies provided to estimate ?H°rxn for the reaction below.

PCl3(g) + Cl2(g) ? PCl5(l) ?H°rxn = ?

Bond Bond Energy (kJ/mol)
Cl-Cl 243
P-Cl 331
A) -243 kJ
B) -419 kJ
C) -662 kJ
D) -67 kJ
E) -905 kJ

19) Use the bond energies provided to estimate ?H°rxn for the reaction below.

2 Br2(l) + C2H2(g) ? C2H2Br4(l) ?H°rxn = ?

Bond Bond Energy (kJ/mol)
Br-Br 193
C?C 837
C-C 347
C-Br 276
C-H 414

A) +407 kJ
B) -324 kJ
C) -228 kJ
D) +573 kJ
E) -648 kJ

20) Identify an ionic bond.
A) Electrons are pooled.
B) Electrons are shared.
C) Electrons are transferred.
D) Neutrons are gained.

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