Question 1

Draw the best Lewis structure for Cl3⁻.What is the formal charge on the central Cl atom?

Accepted Answer

A) -1 
B) 0 
C) +1 
D) +2 
E) -2 
A) -1 
B) 0 
C) +1 
D) +2 
E) -2

Question 2

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH4 would be expected to

Accepted Answer

A) be ionic and contain H- ions. 
B) be ionic and contain H+ ions. 
C) have polar covalent bonds with a partial negative charges on the H atoms. 
D) have polar covalent bonds with a partial positive charges on the H atoms. 
A) be ionic and contain H- ions. 
B) be ionic and contain H+ ions. 
C) have polar covalent bonds with a partial negative charges on the H atoms. 
D) have polar covalent bonds with a partial positive charges on the H atoms.

Question 3

Use Lewis theory to determine the chemical formula for the compound formed between Mg and N.

Accepted Answer

A) Mg3N2 
B) Mg2N3 
C) MgN2 
D) MgN 
A) Mg3N2 
B) Mg2N3 
C) MgN2 
D) MgN

Question 4

Place the following in order of increasing magnitude of lattice energy.
MgO LiI BaS

Accepted Answer

A) BaS < MgO < LiI 
B) LiI < BaS < MgO 
C) MgO < BaS < LiI 
D) LiI < MgO < BaS 
E) MgO < LiI < BaS 
A) BaS < MgO < LiI 
B) LiI < BaS < MgO 
C) MgO < BaS < LiI 
D) LiI < MgO < BaS 
E) MgO < LiI < BaS

Question 5

Lattice energy of NaF and CaO are -910 kJ/mol and -3414 kJ/mol respectively.Which accounts for almost four fold increase in the lattice energy of CaO?

Accepted Answer

A) the higher ionic radius of CaO compared to that of NaF 
B) the higher magnitude of ionic charge of CaO compared to that of NaF 
C) factors other than ionic radius and ionic change 
D) Ca is a group II metal in the periodic table. 
A) the higher ionic radius of CaO compared to that of NaF 
B) the higher magnitude of ionic charge of CaO compared to that of NaF 
C) factors other than ionic radius and ionic change 
D) Ca is a group II metal in the periodic table.

Question 6

Give the number of valence electrons for SF4.

Accepted Answer

A) 28 
B) 30 
C) 32 
D) 34 
A) 28 
B) 30 
C) 32 
D) 34

Question 7

Choose the bond below that is the weakest.

Accepted Answer

A) Na-Cl 
B) I-I 
C) C=N 
D) Li-F 
E) C=O 
A) Na-Cl 
B) I-I 
C) C=N 
D) Li-F 
E) C=O

Question 8

Choose the best Lewis structure for OCl2.

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 9

Use the bond energies provided to estimate ΔH°rxn for the reaction below.
C2H4(g)+ H2(g)→ C2H6(g)ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
C-C 347
C-H 414
C=C 611
C≡C 837
H-H 436

Accepted Answer

A) -128 kJ 
B) +98 kJ 
C) +700 kJ 
D) -102 kJ 
E) -166 kJ 
A) -128 kJ 
B) +98 kJ 
C) +700 kJ 
D) -102 kJ 
E) -166 kJ

Question 10

Use the bond energies provided to estimate ΔH°rxn for the reaction below.
2 Br2(l)+ C2H2(g)→ C2H2Br4(l)ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
Br-Br 193
C≡C 837
C-C 347
C-Br 276
C-H 414

Accepted Answer

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

Question 11

Define electronegativity.

Accepted Answer

The ability of an at

Question 12

Of the following elements,which has the lowest electronegativity?

Accepted Answer

A) Sr 
B) I 
C) Ba 
D) At 
A) Sr 
B) I 
C) Ba 
D) At

Question 13

Place the following in order of increasing magnitude of lattice energy.
MgO LiI CaS

Accepted Answer

A) CaS < MgO < LiI 
B) LiI < CaS < MgO 
C) MgO < CaS < LiI 
D) LiI < MgO < CaS 
E) MgO < LiI < CaS 
A) CaS < MgO < LiI 
B) LiI < CaS < MgO 
C) MgO < CaS < LiI 
D) LiI < MgO < CaS 
E) MgO < LiI < CaS

Question 14

Which is most polar?

Accepted Answer

A) HF 
B) HCl 
C) HBr 
D) HI 
A) HF 
B) HCl 
C) HBr 
D) HI

Question 15

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Accepted Answer

A) AlN 
B) MgO 
C) NaF 
D) CaS 
E) RbI 
A) AlN 
B) MgO 
C) NaF 
D) CaS 
E) RbI

Question 16

Give the number of valence electrons for XeI2.

Accepted Answer

A) 22 
B) 20 
C) 18 
D) 24 
A) 22 
B) 20 
C) 18 
D) 24

Question 17

The iodine atom in I2 would be expected to have a

Accepted Answer

A) charge of 1-. 
B) partial charge δ-. 
C) partial charge δ+. 
D) charge of 0. 
A) charge of 1-. 
B) partial charge δ-. 
C) partial charge δ+. 
D) charge of 0.

Question 18

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

Accepted Answer

A) MgBr 
B) Mg2Br3 
C) Mg3Br2 
D) MgBr2 
E) Mg2Br 
A) MgBr 
B) Mg2Br3 
C) Mg3Br2 
D) MgBr2 
E) Mg2Br

Question 19

Which of the following elements can form compounds with an expanded octet?

Accepted Answer

A) N 
B) Br 
C) F 
D) Be 
E) None of the above can form compounds with an expanded octet. 
A) N 
B) Br 
C) F 
D) Be 
E) None of the above can form compounds with an expanded octet.

Question 20

Place the following in order of decreasing magnitude of lattice energy.
NaF RbBr KCl

Accepted Answer

A) RbBr > NaF > KCl 
B) NaF > KCl > RbBr 
C) KCl > NaF > RbBr 
D) NaF > RbBr > KCl 
E) RbBr > KCl > NaF 
A) RbBr > NaF > KCl 
B) NaF > KCl > RbBr 
C) KCl > NaF > RbBr 
D) NaF > RbBr > KCl 
E) RbBr > KCl > NaF

Draw the best Lewis structure for Cl₃⁻.What is the formal charge on the central Cl atom?

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH₄ would be expected to

Use Lewis theory to determine the chemical formula for the compound formed between Mg and N.

Place the following in order of increasing magnitude of lattice energy. MgO LiI BaS

Lattice energy of NaF and CaO are -910 kJ/mol and -3414 kJ/mol respectively.Which accounts for almost four fold increase in the lattice energy of CaO?

Give the number of valence electrons for SF₄.

Choose the bond below that is the weakest.

Choose the best Lewis structure for OCl₂.

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. C₂H₄(g)+ H₂(g)→ C₂H₆(g)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. 2 Br₂(l)+ C₂H₂(g)→ C₂H₂Br₄(l)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

Define electronegativity.

Of the following elements,which has the lowest electronegativity?

Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS

Which is most polar?

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Give the number of valence electrons for XeI₂.

The iodine atom in I₂ would be expected to have a

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

Which of the following elements can form compounds with an expanded octet?

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

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Exam 9: Chemical Bonding I: Lewis Theory

Draw the best Lewis structure for Cl3⁻.What is the formal charge on the central Cl atom?

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH4 would be expected to

Use Lewis theory to determine the chemical formula for the compound formed between Mg and N.

Place the following in order of increasing magnitude of lattice energy. MgO LiI BaS

Lattice energy of NaF and CaO are -910 kJ/mol and -3414 kJ/mol respectively.Which accounts for almost four fold increase in the lattice energy of CaO?

Give the number of valence electrons for SF4.

Choose the bond below that is the weakest.

Choose the best Lewis structure for OCl2.

Use the bond energies provided to estimate ΔH°rxn for the reaction below. C2H4(g)+ H2(g)→ C2H6(g)ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

Use the bond energies provided to estimate ΔH°rxn for the reaction below. 2 Br2(l)+ C2H2(g)→ C2H2Br4(l)ΔH°rxn = ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

Define electronegativity.

Of the following elements,which has the lowest electronegativity?

Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS

Which is most polar?

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Give the number of valence electrons for XeI2.

The iodine atom in I2 would be expected to have a

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

Which of the following elements can form compounds with an expanded octet?

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

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Draw the best Lewis structure for Cl₃⁻.What is the formal charge on the central Cl atom?

The electronegativity is 2.1 for H and 1.9 for Pb.Based on these electronegativities PbH₄ would be expected to

Give the number of valence electrons for SF₄.

Choose the best Lewis structure for OCl₂.

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. C₂H₄(g)+ H₂(g)→ C₂H₆(g)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 C≡C 837 H-H 436

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. 2 Br₂(l)+ C₂H₂(g)→ C₂H₂Br₄(l)ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Br-Br 193 C≡C 837 C-C 347 C-Br 276 C-H 414

Give the number of valence electrons for XeI₂.

The iodine atom in I₂ would be expected to have a