Question 1

Arrange P,S,and O in order of increasing atomic radius.

Accepted Answer

A) S < O < P 
B) P < S < O 
C) O < S < P 
D) O < P < S 
E) The answer cannot be determined from the data given. 
A) S < O < P 
B) P < S < O 
C) O < S < P 
D) O < P < S 
E) The answer cannot be determined from the data given.

Question 2

An aluminum ion,Al3+,has

Accepted Answer

A) 13 protons and 13 electrons. 
B) 27 protons and 24 electrons. 
C) 16 protons and 13 electrons. 
D) 13 protons and 10 electrons. 
E) 10 protons and 13 electrons. 
A) 13 protons and 13 electrons. 
B) 27 protons and 24 electrons. 
C) 16 protons and 13 electrons. 
D) 13 protons and 10 electrons. 
E) 10 protons and 13 electrons.

Question 3

What is the electron configuration for Fr?

Accepted Answer

A) [Xe]6s1 
B) [Rn]7s1 
C) [Rn]7s2 
D) [Xe]6s2 
E) [Kr]6s1 
A) [Xe]6s1 
B) [Rn]7s1 
C) [Rn]7s2 
D) [Xe]6s2 
E) [Kr]6s1

Question 4

In Mendeleev's version of the periodic table,the elements were arranged in order of increasing atomic number.

Accepted Answer

A) True 
 B)False

Question 5

How does atomic radius change as you move across the periodic table?

Accepted Answer

A) Atomic radius decreases moving from left to right across a period and increases from top to bottom. 
B) Atomic radius increases moving left to right across a period and decreases from top to bottom. 
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D) Atomic radius increases diagonally across the periodic table. 
E) None of the answers is correct. 
A) Atomic radius decreases moving from left to right across a period and increases from top to bottom. 
B) Atomic radius increases moving left to right across a period and decreases from top to bottom. 
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D) Atomic radius increases diagonally across the periodic table. 
E) None of the answers is correct.

Question 6

Which element would be expected to have properties similar to calcium?

Accepted Answer

A) Ba 
B) K 
C) Sc 
D) Na 
E) Rb 
A) Ba 
B) K 
C) Sc 
D) Na 
E) Rb

Question 7

Which of these 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 8

Which of these pairs consists of isoelectronic species?

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 9

Which of these atoms has the smallest radius?

Accepted Answer

A) Al 
B) P 
C) As 
D) Te 
E) Na 
A) Al 
B) P 
C) As 
D) Te 
E) Na

Question 10

Explain how the elements in Group 4A differ from one another.

Accepted Answer

C is a nonmetal; Si

Question 11

Explain why hydrogen is placed in Group 1A even though it really belongs in a group by itself.

Accepted Answer

Hydrogen is typically placed a

Question 12

Which one of these ions is not isoelectronic with Kr?

Accepted Answer

A) As3+ 
B) Se2- 
C) Rb+ 
D) Sr2+ 
E) Br- 
A) As3+ 
B) Se2- 
C) Rb+ 
D) Sr2+ 
E) Br-

Question 13

Which species have the most similar atomic radii?

Accepted Answer

A) S2- and Cl- 
B) Ar and As 
C) Rb+ and K+ 
D) I- and Br - 
E) Br and Cs 
A) S2- and Cl- 
B) Ar and As 
C) Rb+ and K+ 
D) I- and Br - 
E) Br and Cs

Question 14

The energy states of atoms containing more than one electron arise from nucleus-electron and electronelectron interactions.Which of the following statements correctly describes these effects?

Accepted Answer

A) Larger nuclear charge lowers energy; more electrons in an orbital lowers energy. 
B) Larger nuclear charge lowers energy; more electrons in an orbital increases energy. 
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D) Smaller nuclear charge lowers energy; more electrons in an orbital increases energy. 
E) None of these statements is generally correct. 
A) Larger nuclear charge lowers energy; more electrons in an orbital lowers energy. 
B) Larger nuclear charge lowers energy; more electrons in an orbital increases energy. 
C) Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D) Smaller nuclear charge lowers energy; more electrons in an orbital increases energy. 
E) None of these statements is generally correct.

Question 15

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Accepted Answer

A) True 
 B)False

Question 16

Which one of the following equations correctly represents the process relating to the ionization energy of X?

Accepted Answer

A) X(s)→ X+(g)+ e- 
B) X2(g)→ X+(g)+ X-(g) 
C) X(g)+ e- → X-(g) 
D) X-(g)→ X(g)+ e- 
E) X(g)→ X+(g)+ e- 
A) X(s)→ X+(g)+ e- 
B) X2(g)→ X+(g)+ X-(g) 
C) X(g)+ e- → X-(g) 
D) X-(g)→ X(g)+ e- 
E) X(g)→ X+(g)+ e-

Question 17

Consider the element with the electron configuration [Kr]5s24d7.This element is

Accepted Answer

A) a halogen. 
B) a transition metal. 
C) a nonmetal. 
D) an actinide element. 
E) a noble gas. 
A) a halogen. 
B) a transition metal. 
C) a nonmetal. 
D) an actinide element. 
E) a noble gas.

Question 18

Explain how the elements in Group 6A differ from one another.

Accepted Answer

O,S,and Se are nonme

Question 19

The elements in a column of the periodic table are known as

Accepted Answer

A) metalloids. 
B) a period. 
C) noble gases. 
D) a group. 
E) nonmetals. 
A) metalloids. 
B) a period. 
C) noble gases. 
D) a group. 
E) nonmetals.

Question 20

The general electron configuration for noble gas atoms is

Accepted Answer

A) ns2np6. 
B) ns2np5. 
C) ns2np4. 
D) ns2np3. 
E) ns2. 
A) ns2np6. 
B) ns2np5. 
C) ns2np4. 
D) ns2np3. 
E) ns2.

Exam 7: Electron Configuration and the Periodic Table

Arrange P,S,and O in order of increasing atomic radius.

An aluminum ion,Al3+,has

What is the electron configuration for Fr?

In Mendeleev's version of the periodic table,the elements were arranged in order of increasing atomic number.

How does atomic radius change as you move across the periodic table?

Which element would be expected to have properties similar to calcium?

Which of these elements has the greatest metallic character?

Which of these pairs consists of isoelectronic species?

Which of these atoms has the smallest radius?

Explain how the elements in Group 4A differ from one another.

Explain why hydrogen is placed in Group 1A even though it really belongs in a group by itself.

Which one of these ions is not isoelectronic with Kr?

Which species have the most similar atomic radii?

The energy states of atoms containing more than one electron arise from nucleus-electron and electronelectron interactions.Which of the following statements correctly describes these effects?

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Which one of the following equations correctly represents the process relating to the ionization energy of X?

Consider the element with the electron configuration [Kr]5s24d7.This element is

Explain how the elements in Group 6A differ from one another.

The elements in a column of the periodic table are known as

The general electron configuration for noble gas atoms is

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

An aluminum ion,Al³⁺,has

Consider the element with the electron configuration [Kr]5s²4d⁷.This element is