Question 1

Which of the following elements will form a cation with a +2 charge?

Accepted Answer

A)  Si 
B)  Sr 
C)  Ga 
D)  Cs 
E)  S 
A)  Si 
B)  Sr 
C)  Ga 
D)  Cs 
E)  S

Question 2

Elements in the same period of the periodic table have similar valence shell electron configurations.

Accepted Answer

A) True 
 B)False

Question 3

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Accepted Answer

A)  n = 2 l = 1 ml = -1 ms = +½ 
B)  n = 3 l = 0 ml = 0 ms = -½ 
C)  n = 3 l = 2 ml = -2 ms = -½ 
D)  n = 4 l = 0 ml = 0 ms = -½ 
E)  n = 4 l = 2 ml = 1 ms = +½ 
A)  n = 2 l = 1 ml = -1 ms = +½ 
B)  n = 3 l = 0 ml = 0 ms = -½ 
C)  n = 3 l = 2 ml = -2 ms = -½ 
D)  n = 4 l = 0 ml = 0 ms = -½ 
E)  n = 4 l = 2 ml = 1 ms = +½

Question 4

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Accepted Answer

A) True 
 B)False

Question 5

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Accepted Answer

A) True 
 B)False

Question 6

Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

Accepted Answer

A)  A2- > B- > C > D+ > E2+ 
B)  E2+ > D+ > C > B- > A2- 
C)  A2- > B- > C + 2+ 
D)  A2- -  D+ > E2+ 
E)  None of these choices are correct. 
A)  A2- > B- > C > D+ > E2+ 
B)  E2+ > D+ > C > B- > A2- 
C)  A2- > B- > C + 2+ 
D)  A2- -  D+ > E2+ 
E)  None of these choices are correct.

Question 7

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Accepted Answer

A)  X(g) → X+(g) + e- 
B)  X+(g) → X+(aq) 
C)  X+(g) + e- → X(g) 
D)  X(g) + e- → X-(g) 
E)  X+(g) + Y-(g) → XY(s) 
A)  X(g) → X+(g) + e- 
B)  X+(g) → X+(aq) 
C)  X+(g) + e- → X(g) 
D)  X(g) + e- → X-(g) 
E)  X+(g) + Y-(g) → XY(s)

Question 8

Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

Accepted Answer

A)  3d 
B)  4s 
C)  4p 
D)  4d 
E)  5s 
A)  3d 
B)  4s 
C)  4p 
D)  4d 
E)  5s

Question 9

Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

Accepted Answer

A) True 
 B)False

Question 10

Which of the following elements has the largest first ionization energy?

Accepted Answer

A)  Na 
B)  Cl 
C)  Ca 
D)  Te 
E)  Br 
A)  Na 
B)  Cl 
C)  Ca 
D)  Te 
E)  Br

Question 11

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Accepted Answer

A)  the first valence electron is removed. 
B)  the second valence electron is removed. 
C)  the eighth electron of is removed. 
D)  the first core electron is removed. 
E)  the last valence electron is removed. 
A)  the first valence electron is removed. 
B)  the second valence electron is removed. 
C)  the eighth electron of is removed. 
D)  the first core electron is removed. 
E)  the last valence electron is removed.

Question 12

Which of the following electron configurations is impossible?

Accepted Answer

A)  1s22s22p63s23p4 
B)  1s22s22p53s13p4 
C)  1s22s22p63s23p63d104s2 
D)  1s22s22p63s33p4 
E)  1s12s22p63s23p4 
A)  1s22s22p63s23p4 
B)  1s22s22p53s13p4 
C)  1s22s22p63s23p63d104s2 
D)  1s22s22p63s33p4 
E)  1s12s22p63s23p4

Question 13

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471
IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

Accepted Answer

A)  Li 
B)  B 
C)  O 
D)  Ne 
E)  None of these choices are correct. 
A)  Li 
B)  B 
C)  O 
D)  Ne 
E)  None of these choices are correct.

Question 14

A negative electron affinity implies that the atom repels an approaching electron.

Accepted Answer

A) True 
 B)False

Question 15

Bigger atoms generally have smaller ionization energies.

Accepted Answer

A) True 
 B)False

Question 16

Which of the following elements has the greatest atomic radius?

Accepted Answer

A)  Li 
B)  Ne 
C)  Rb 
D)  Sr 
E)  Xe 
A)  Li 
B)  Ne 
C)  Rb 
D)  Sr 
E)  Xe

Question 17

Which of the following has the most negative electron affinity?

Accepted Answer

A)  H 
B)  Li 
C)  Na 
D)  K 
E)  Rb 
A)  H 
B)  Li 
C)  Na 
D)  K 
E)  Rb

Question 18

Which of the following elements has the largest second ionization energy (IE2)?

Accepted Answer

A)  Li 
B)  B 
C)  O 
D)  F 
E)  Na 
A)  Li 
B)  B 
C)  O 
D)  F 
E)  Na

Question 19

Which of the following fourth-period elements has the smallest atomic radius?

Accepted Answer

A)  K 
B)  Ti 
C)  Cu 
D)  Ge 
E)  Kr 
A)  K 
B)  Ti 
C)  Cu 
D)  Ge 
E)  Kr

Question 20

According to the exclusion principle, two is the maximum number of electrons in an atom which can share the same four quantum numbers.

Accepted Answer

A) True 
 B)False

Exam 8: Electron Configuration and Chemical Periodicity

Which of the following elements will form a cation with a +2 charge?

Elements in the same period of the periodic table have similar valence shell electron configurations.

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

Which of the following elements has the largest first ionization energy?

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Which of the following electron configurations is impossible?

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471 IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

A negative electron affinity implies that the atom repels an approaching electron.

Bigger atoms generally have smaller ionization energies.

Which of the following elements has the greatest atomic radius?

Which of the following has the most negative electron affinity?

Which of the following elements has the largest second ionization energy (IE2)?

Which of the following fourth-period elements has the smallest atomic radius?

According to the exclusion principle, two is the maximum number of electrons in an atom which can share the same four quantum numbers.

Keys to Studying Chemistry Definitions, Units, and Problem Solving

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

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

Periodic Patterns in the Main-Group Elements

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Consider the set of isoelectronic atoms and ions A^2-, B^-, C, D⁺, and E²⁺. Which arrangement of relative radii is correct?

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE₁, 1314 IE₂, 3389 IE₃, 5298 IE₄, 7471 IE₅, 10992 IE₆, 13329 IE₇, 71345 IE₈, 84087

Which of the following elements has the largest second ionization energy (IE₂)?