Question 1

In gaseous BeCl2, Be does not obey the octet rule; in solid BeCl2, it does.

Accepted Answer

A) True 
 B)False

Question 2

Which of the following ions and atoms has the greatest radius?

Accepted Answer

A)  Se2¯ 
B)  Br¯ 
C)  Rb+ 
D)  Sr2+ 
E)  Kr 
A)  Se2¯ 
B)  Br¯ 
C)  Rb+ 
D)  Sr2+ 
E)  Kr

Question 3

Salts of group 1A metals are generally more soluble than those of group 2A metals.

Accepted Answer

A) True 
 B)False

Question 4

Select the element with the highest first ionization energy.

Accepted Answer

A)  Mg 
B)  Ca 
C)  Ba 
D)  Ra 
E)  K 
A)  Mg 
B)  Ca 
C)  Ba 
D)  Ra 
E)  K

Question 5

According to the phase diagram of carbon, what pressure and temperature conditions, if any, are needed in order for diamond to be the stable phase?

Accepted Answer

A)  low pressure, low temperature 
B)  low pressure, high temperature 
C)  high pressure, low temperature 
D)  high pressure, high temperature 
E)  Actually, diamond is not stable under any conditions. 
A)  low pressure, low temperature 
B)  low pressure, high temperature 
C)  high pressure, low temperature 
D)  high pressure, high temperature 
E)  Actually, diamond is not stable under any conditions.

Question 6

Predict the products for the following set of reactants. 
PCl3(l) + H2O(l) $\rightarrow$

Accepted Answer

A)  H3PO3(aq) + HCl(aq) 
B)  H3PO4(aq) + Cl2(g) 
C)  PH3(g) + HCl(aq) + O2(g) 
D)  P2O5(s) + HCl(aq) 
E)  PCl5(l) + PH3(g) + O2(g) 
A)  H3PO3(aq) + HCl(aq) 
B)  H3PO4(aq) + Cl2(g) 
C)  PH3(g) + HCl(aq) + O2(g) 
D)  P2O5(s) + HCl(aq) 
E)  PCl5(l) + PH3(g) + O2(g)

Question 7

Predict the product(s) for the reaction of the following set of reactants. 
Ca(s) + H2(g) $\rightarrow$

Accepted Answer

A)  CaH(s) 
B)  CaH2(s) 
C)  Ca2H3(s) 
D)  Ca3H2(s) 
E)  None of these choices is correct. 
A)  CaH(s) 
B)  CaH2(s) 
C)  Ca2H3(s) 
D)  Ca3H2(s) 
E)  None of these choices is correct.

Question 8

Hydrogen forms metallic (interstitial) hydrides with the d and f transition elements. Which of the following statements is correct?

Accepted Answer

A)  These substances have distinct stoichiometric formulas like ionic hydrides. 
B)  Hydrogen forms bonds with the metals by donating its electron to the valence band of the metal. 
C)  Hydrogen molecules and atoms occupy holes within the crystal structure of the metal. 
D)  These substances are useful catalysts. 
E)  These hydrides are stabilized by hydrogen bonding forces. 
A)  These substances have distinct stoichiometric formulas like ionic hydrides. 
B)  Hydrogen forms bonds with the metals by donating its electron to the valence band of the metal. 
C)  Hydrogen molecules and atoms occupy holes within the crystal structure of the metal. 
D)  These substances are useful catalysts. 
E)  These hydrides are stabilized by hydrogen bonding forces.

Question 9

Which of the following has the most allotropes?

Accepted Answer

A)  carbon 
B)  sulfur 
C)  oxygen 
D)  selenium 
E)  nitrogen 
A)  carbon 
B)  sulfur 
C)  oxygen 
D)  selenium 
E)  nitrogen

Question 10

Predict the products for the following set of reactants. 
Cl2(g) + I¯(aq) $\rightarrow$

Accepted Answer

A)  ICl 
B)  ICl2 
C)  ICl3 
D)  I2 + Cl¯ 
E)  I + Cl2¯ 
A)  ICl 
B)  ICl2 
C)  ICl3 
D)  I2 + Cl¯ 
E)  I + Cl2¯

Question 11

Predict the products for the following set of reactants. 
H2O(l) + ClF5(l) $\rightarrow$

Accepted Answer

A)  HClO2(aq) + HF(aq) 
B)  HClO3(aq) + HF(aq) 
C)  HClO(aq) + HF(aq) 
D)  HCl(aq) + HF(aq) 
E)  HClO(aq) + HFO(aq) 
A)  HClO2(aq) + HF(aq) 
B)  HClO3(aq) + HF(aq) 
C)  HClO(aq) + HF(aq) 
D)  HCl(aq) + HF(aq) 
E)  HClO(aq) + HFO(aq)

Question 12

Predict the products for the following set of reactants. 
Cs(s) + Br2(l) $\rightarrow$

Accepted Answer

A)  CsBr(s) 
B)  CsBr2(s) 
C)  CsBr(l) 
D)  CsBr2(l) 
E)  Cs2Br(s) 
A)  CsBr(s) 
B)  CsBr2(s) 
C)  CsBr(l) 
D)  CsBr2(l) 
E)  Cs2Br(s)

Question 13

The Haber process is the first step in the manufacture of sulfuric acid.

Accepted Answer

A) True 
 B)False

Question 14

Boron has 3 valence electrons. Which of the following processes is involved in boron's achieving a complete outer shell?

Accepted Answer

A)  formation of a B3+ cation 
B)  formation of bridge bonds 
C)  formation of  $\pi$-bonds using its d-orbitals 
D)  formation of  $\pi$-bonds using sp3-orbitals 
E)  None of these choices is correct. 
A)  formation of a B3+ cation 
B)  formation of bridge bonds 
C)  formation of  $\pi$-bonds using its d-orbitals 
D)  formation of  $\pi$-bonds using sp3-orbitals 
E)  None of these choices is correct.

Question 15

The chemical that ranks first in production among all industrial chemicals is

Accepted Answer

A)  NH3, ammonia. 
B)  H3PO4, phosphoric acid. 
C)  NaOH, sodium hydroxide. 
D)  Na2CO3, sodium carbonate. 
E)  H2SO4, sulfuric acid. 
A)  NH3, ammonia. 
B)  H3PO4, phosphoric acid. 
C)  NaOH, sodium hydroxide. 
D)  Na2CO3, sodium carbonate. 
E)  H2SO4, sulfuric acid.

Question 16

Hydrogen fluoride is used

Accepted Answer

A)  in the manufacture of steel. 
B)  in the synthesis of cryolite for aluminum production. 
C)  as an oxidizing agent. 
D)  as a disinfectant. 
E)  as a mouthwash. 
A)  in the manufacture of steel. 
B)  in the synthesis of cryolite for aluminum production. 
C)  as an oxidizing agent. 
D)  as a disinfectant. 
E)  as a mouthwash.

Question 17

Which of the following pairs of elements will form the longest single bond?

Accepted Answer

A)  C, F 
B)  C, N 
C)  C, S 
D)  C, O 
E)  C, H 
A)  C, F 
B)  C, N 
C)  C, S 
D)  C, O 
E)  C, H

Question 18

The strongest elemental oxidizing agents are found in the _________ _________ region of the periodic table while the strongest reducing agents are found in the ________ ________ region of the periodic table.

Accepted Answer

A)  upper left, lower right 
B)  upper right, lower left 
C)  lower left, upper right 
D)  lower right, upper left 
E)  transition element, main group 
A)  upper left, lower right 
B)  upper right, lower left 
C)  lower left, upper right 
D)  lower right, upper left 
E)  transition element, main group

Question 19

Most of the alkali metal salts are soluble in water while many alkaline earth salts have very low solubilities. Why is this so?

Accepted Answer

A)  The alkali metal cations are smaller than the alkaline earth cations and are more easily hydrated. 
B)  The alkali metals have lower ionization energies than alkaline earth elements. 
C)  The alkaline earth salts have much greater lattice energies than the alkali metal salts. 
D)  The alkaline earth metals have greater heats of atomization than the alkali metals. 
E)  Alkaline earth cations have very low heats of hydration. 
A)  The alkali metal cations are smaller than the alkaline earth cations and are more easily hydrated. 
B)  The alkali metals have lower ionization energies than alkaline earth elements. 
C)  The alkaline earth salts have much greater lattice energies than the alkali metal salts. 
D)  The alkaline earth metals have greater heats of atomization than the alkali metals. 
E)  Alkaline earth cations have very low heats of hydration.

Question 20

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. The ionic radius for Na+ is 102 pm and for Cl¯ is 181 pm. In going from Na to Cl in Period 3, why does the atomic radius decrease while the ionic radius increases?

Accepted Answer

A)  The inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. 
B)  The inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. 
C)  The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. 
D)  The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. 
E)  Monatomic ions are bigger than the atoms from which they are formed. 
A)  The inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. 
B)  The inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. 
C)  The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. 
D)  The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. 
E)  Monatomic ions are bigger than the atoms from which they are formed.

Exam 14: Periodic Patterns in the Main-Group Elements

In gaseous BeCl2, Be does not obey the octet rule; in solid BeCl2, it does.

Which of the following ions and atoms has the greatest radius?

Salts of group 1A metals are generally more soluble than those of group 2A metals.

Select the element with the highest first ionization energy.

According to the phase diagram of carbon, what pressure and temperature conditions, if any, are needed in order for diamond to be the stable phase?

Predict the products for the following set of reactants. PCl3(l) + H2O(l) →\rightarrow→

Predict the product(s) for the reaction of the following set of reactants. Ca(s) + H2(g) →\rightarrow→

Hydrogen forms metallic (interstitial) hydrides with the d and f transition elements. Which of the following statements is correct?

Which of the following has the most allotropes?

Predict the products for the following set of reactants. Cl2(g) + I¯(aq) →\rightarrow→

Predict the products for the following set of reactants. H2O(l) + ClF5(l) →\rightarrow→

Predict the products for the following set of reactants. Cs(s) + Br2(l) →\rightarrow→

The Haber process is the first step in the manufacture of sulfuric acid.

Boron has 3 valence electrons. Which of the following processes is involved in boron's achieving a complete outer shell?

The chemical that ranks first in production among all industrial chemicals is

Hydrogen fluoride is used

Which of the following pairs of elements will form the longest single bond?

The strongest elemental oxidizing agents are found in the _________ _________ region of the periodic table while the strongest reducing agents are found in the ________ ________ region of the periodic table.

Most of the alkali metal salts are soluble in water while many alkaline earth salts have very low solubilities. Why is this so?

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. The ionic radius for Na+ is 102 pm and for Cl¯ is 181 pm. In going from Na to Cl in Period 3, why does the atomic radius decrease while the ionic radius increases?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

In gaseous BeCl₂, Be does not obey the octet rule; in solid BeCl₂, it does.

Predict the products for the following set of reactants. PCl₃(l) + H₂O(l) $\rightarrow$

Predict the product(s) for the reaction of the following set of reactants. Ca(s) + H₂(g) $\rightarrow$

Predict the products for the following set of reactants. Cl₂(g) + I¯(aq) $\rightarrow$

Predict the products for the following set of reactants. H₂O(l) + ClF₅(l) $\rightarrow$

Predict the products for the following set of reactants. Cs(s) + Br₂(l) $\rightarrow$

The strongest elemental oxidizing agents are found in the _____ _ region of the periodic table while the strongest reducing agents are found in the ____ region of the periodic table.

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. The ionic radius for Na⁺ is 102 pm and for Cl¯ is 181 pm. In going from Na to Cl in Period 3, why does the atomic radius decrease while the ionic radius increases?