Question 1

Which of the following make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+?

Accepted Answer

A) Ca2+ and Fe3+ 
B) O2- and F 
C) F and Cl- 
D) Cl- and Ca2+ 
E) None of the above. 
A) Ca2+ and Fe3+ 
B) O2- and F 
C) F and Cl- 
D) Cl- and Ca2+ 
E) None of the above.

Question 2

Sodium ions are more reactive than sodium atoms.

Accepted Answer

A) True 
 B)False

Question 3

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

Accepted Answer

A) X has a larger electron affinity than Y does. 
B) X has a larger effective nuclear charge than Y does. 
C) X has greater metallic character than Y does. 
D) X has a larger first ionization energy than Y does. 
E) X is a poorer conductor of electricity than Y when in the solid state. 
A) X has a larger electron affinity than Y does. 
B) X has a larger effective nuclear charge than Y does. 
C) X has greater metallic character than Y does. 
D) X has a larger first ionization energy than Y does. 
E) X is a poorer conductor of electricity than Y when in the solid state.

Question 4

Which of the following is a basic oxide?

Accepted Answer

A) NO2 
B) H2O 
C) Na2O 
D) SnO 
E) SO2 
A) NO2 
B) H2O 
C) Na2O 
D) SnO 
E) SO2

Question 5

Consider the following reaction: 3Li + Z $\rarr$ Li3Z.What is a reasonable guess for the identity of element Z?

Accepted Answer

Nitrogen, or other e

Question 6

The representative elements are those with unfilled energy levels in which the "last electron" was added to

Accepted Answer

A) an s orbital. 
B) an s or p orbital. 
C) a d orbital. 
D) a p or d orbital. 
E) an f orbital. 
A) an s orbital. 
B) an s or p orbital. 
C) a d orbital. 
D) a p or d orbital. 
E) an f orbital.

Question 7

Which of the following is an acidic oxide?

Accepted Answer

A) P4O10 
B) MgO 
C) Fe2O3 
D) K2O 
E) Cr2O3 
A) P4O10 
B) MgO 
C) Fe2O3 
D) K2O 
E) Cr2O3

Question 8

The electron configuration of the outermost electrons of atoms of the halogen group is ns2np7.

Accepted Answer

A) True 
 B)False

Question 9

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Accepted Answer

A) nuclear binding energy. 
B) number of neutrons. 
C) atomic mass. 
D) atomic number. 
E) atomic size. 
A) nuclear binding energy. 
B) number of neutrons. 
C) atomic mass. 
D) atomic number. 
E) atomic size.

Question 10

Which of the following atoms has the greatest electron affinity (largest positive value)?

Accepted Answer

A) S 
B) P 
C) Ga 
D) Li 
E) Br 
A) S 
B) P 
C) Ga 
D) Li 
E) Br

Question 11

Write the ground-state electron configuration for Br-.

Accepted Answer

Question 12

Which of the following elements has the greatest metallic character?

Accepted Answer

A) Br 
B) Se 
C) Ni 
D) As 
E) Si 
A) Br 
B) Se 
C) Ni 
D) As 
E) Si

Question 13

The law of octaves was proposed by

Accepted Answer

A) G.N.Lewis. 
B) John Newlands. 
C) Dmitri Mendeleev. 
D) J.J.Thompson. 
E) Ernest Rutherford. 
A) G.N.Lewis. 
B) John Newlands. 
C) Dmitri Mendeleev. 
D) J.J.Thompson. 
E) Ernest Rutherford.

Question 14

Which of the elements listed below has the following pattern for its first six ionization energies? (I1 = first ionization energy, I2 = second ionization energy, etc.)

Accepted Answer

A) Ca 
B) Si 
C) Al 
D) Se 
E) P 
A) Ca 
B) Si 
C) Al 
D) Se 
E) P

Question 15

For phosphorus atoms, which ionization energy will show an exceptionally large increase over the previous ionization energy?

Accepted Answer

A) 2nd 
B) 3rd 
C) 4th 
D) 5th 
E) 6th 
A) 2nd 
B) 3rd 
C) 4th 
D) 5th 
E) 6th

Question 16

Which one of the following pairs are isoelectronic?

Accepted Answer

A) Mn2+ and Ar 
B) Zn2+ and Cu2+ 
C) Na+ and K+ 
D) Cl- and S 
E) K+ and Cl- 
A) Mn2+ and Ar 
B) Zn2+ and Cu2+ 
C) Na+ and K+ 
D) Cl- and S 
E) K+ and Cl-

Question 17

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l)$\rarr$ Hg+(g)+ e- is therefore

Accepted Answer

A) 1006 kJ/mol. 
B) greater than 1006 kJ/mol. 
C) less than 1006 kJ/mol. 
D) is equal to the electron affinity of mercury. 
E) is equal to the second ionization energy of mercury. 
A) 1006 kJ/mol. 
B) greater than 1006 kJ/mol. 
C) less than 1006 kJ/mol. 
D) is equal to the electron affinity of mercury. 
E) is equal to the second ionization energy of mercury.

Question 18

In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s24d105p2?

Accepted Answer

A) row 4, group 4A 
B) row 4, group 5A 
C) row 5, group 4A 
D) row 5, group 5A 
E) none of the above 
A) row 4, group 4A 
B) row 4, group 5A 
C) row 5, group 4A 
D) row 5, group 5A 
E) none of the above

Question 19

The chief contribution of physicist Henry Moseley to atomic theory was

Accepted Answer

A) the discovery of the periodic law. 
B) the determination of the charge of the proton. 
C) the measurement of the atomic numbers of the elements. 
D) the scientist who determined the electric charge of the electron. 
E) the discovery of the law of octaves. 
A) the discovery of the periodic law. 
B) the determination of the charge of the proton. 
C) the measurement of the atomic numbers of the elements. 
D) the scientist who determined the electric charge of the electron. 
E) the discovery of the law of octaves.

Exam 8: Periodic Relationships Among the Elements

Which of the following make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+?

Sodium ions are more reactive than sodium atoms.

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

Which of the following is a basic oxide?

Consider the following reaction: 3Li + Z →\rarr→ Li3Z.What is a reasonable guess for the identity of element Z?

The representative elements are those with unfilled energy levels in which the "last electron" was added to

Which of the following is an acidic oxide?

The electron configuration of the outermost electrons of atoms of the halogen group is ns2np7.

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Which of the following atoms has the greatest electron affinity (largest positive value)?

Write the ground-state electron configuration for Br-.

Which of the following elements has the greatest metallic character?

The law of octaves was proposed by

Which of the elements listed below has the following pattern for its first six ionization energies? (I1 = first ionization energy, I2 = second ionization energy, etc.)

For phosphorus atoms, which ionization energy will show an exceptionally large increase over the previous ionization energy?

Which one of the following pairs are isoelectronic?

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) →\rarr→ Hg+(g)+ e- is therefore

In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s24d105p2?

The chief contribution of physicist Henry Moseley to atomic theory was

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca²⁺, Fe³⁺?

Consider the following reaction: 3Li + Z $\rarr$ Li₃Z.What is a reasonable guess for the identity of element Z?

The electron configuration of the outermost electrons of atoms of the halogen group is ns²np⁷.

Write the ground-state electron configuration for Br^-.

Which of the elements listed below has the following pattern for its first six ionization energies? (I₁ = first ionization energy, I₂ = second ionization energy, etc.)

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) $\rarr$ Hg⁺(g)+ e^- is therefore

In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s²4d¹⁰5p²?