Question 1

Who was the first chemist to recognize patterns in chemical properties of the elements?

Accepted Answer

A) Bohr 
B) Dobereiner 
C) Meyer 
D) Mendeleev 
E) Newlands 
A) Bohr 
B) Dobereiner 
C) Meyer 
D) Mendeleev 
E) Newlands B

Question 2

An atom of which of the following elements has the highest fourth ionization energy?

Accepted Answer

A) Al 
B) Se 
C) Si 
D) Ga 
E) As 
A) Al 
B) Se 
C) Si 
D) Ga 
E) As A

Question 3

Fe has ____ that is(are)unpaired in its d orbitals.

Accepted Answer

A) 2 electrons 
B) 3 electrons 
C) 1 electron 
D) 4 electrons 
E) none of these 
A) 2 electrons 
B) 3 electrons 
C) 1 electron 
D) 4 electrons 
E) none of these D

Question 4

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is

Accepted Answer

A) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that oxygen has one doubly occupied 2p orbital and nitrogen does not. 
B) consistent with the general trend relating changes in ionization energy across a period from left to right because it is harder to take an electron from an oxygen atom than from a nitrogen atom. 
C) consistent with the general trend relating changes in ionization energy across a period from left to right because it is easier to take an electron from an oxygen atom than from a nitrogen atom. 
D) incorrect. 
E) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that the oxygen atom has two doubly occupied 2p orbitals and nitrogen has only one. 
A) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that oxygen has one doubly occupied 2p orbital and nitrogen does not. 
B) consistent with the general trend relating changes in ionization energy across a period from left to right because it is harder to take an electron from an oxygen atom than from a nitrogen atom. 
C) consistent with the general trend relating changes in ionization energy across a period from left to right because it is easier to take an electron from an oxygen atom than from a nitrogen atom. 
D) incorrect. 
E) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that the oxygen atom has two doubly occupied 2p orbitals and nitrogen has only one.

Question 5

Rank the following ions in order of increasing first ionization energy: O2-,Mg2+,F-,Na+.

Accepted Answer

A) Mg2+ + - 2- 
B) Mg2+ 2- + - 
C) O2- - 2+ + 
D) O2- - + 2+ 
E) O2- 2+ - + 
A) Mg2+ + - 2- 
B) Mg2+ 2- + - 
C) O2- - 2+ + 
D) O2- - + 2+ 
E) O2- 2+ - +

Question 6

Which element is found in the s-block of the periodic table?

Accepted Answer

A) Ra 
B) Ar 
C) Db 
D) Np 
E) none of the above 
A) Ra 
B) Ar 
C) Db 
D) Np 
E) none of the above

Question 7

An atom of which of the following elements has the smallest first ionization energy?

Accepted Answer

A) Rb 
B) Si 
C) F 
D) P 
E) Ca 
A) Rb 
B) Si 
C) F 
D) P 
E) Ca

Question 8

Which of the following have one or more filled d subshells in their ground state electron configuration?

Accepted Answer

A) Br 
B) H 
C) Ti 
D) Cr 
E) P 
A) Br 
B) H 
C) Ti 
D) Cr 
E) P

Question 9

The change in energy for which of the following processes represents the first ionization energy of iodine?

Accepted Answer

A) I(g)→ I2+(g)+ 2e- 
B) I(g)+ e - → I-(g) 
C) 2I-(g)→ I2(s)+ 2e- 
D) I(g)→ I+(g)+ e- 
E) I-(g)→ I+(g)+ 2e- 
A) I(g)→ I2+(g)+ 2e- 
B) I(g)+ e - → I-(g) 
C) 2I-(g)→ I2(s)+ 2e- 
D) I(g)→ I+(g)+ e- 
E) I-(g)→ I+(g)+ 2e-

Question 10

What is the ground-state electron configuration of terbium (Tb)?

Accepted Answer

A) 1s22s22p63s23p63d104s24p64d105s25p65d96s2 
B) 1s22s22p63s23p63d104s24p64d104f145s25p3 
C) 1s22s22p63s23p63d104s24p64d105s25p65d106s1 
D) 1s22s22p63s23p63d104s24p64d94f105s25p66s2 
E) 1s22s22p63s23p63d104s24p64d104f95s25p66s2 
A) 1s22s22p63s23p63d104s24p64d105s25p65d96s2 
B) 1s22s22p63s23p63d104s24p64d104f145s25p3 
C) 1s22s22p63s23p63d104s24p64d105s25p65d106s1 
D) 1s22s22p63s23p63d104s24p64d94f105s25p66s2 
E) 1s22s22p63s23p63d104s24p64d104f95s25p66s2

Question 11

Sodium and potassium have similar chemical and physical properties.This is best explained by the fact that both elements

Accepted Answer

A) have the same ground-state valence-electron configuration. 
B) have low relative atomic weights. 
C) are in Period 1 of the periodic table. 
D) have relatively low first ionization energies. 
E) are active metals. 
A) have the same ground-state valence-electron configuration. 
B) have low relative atomic weights. 
C) are in Period 1 of the periodic table. 
D) have relatively low first ionization energies. 
E) are active metals.

Question 12

Which of the following orbital diagrams violates the Pauli exclusion principle?
1s 2s 2p

Accepted Answer

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

Question 13

How many valence electrons does an arsenic atom have?

Accepted Answer

A) 5 
B) 6 
C) 7 
D) 2 
E) 33 
A) 5 
B) 6 
C) 7 
D) 2 
E) 33

Question 14

The statement that "the lowest-energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as

Accepted Answer

A) the aufbau principle. 
B) Hund's rule. 
C) the Pauli exclusion principle. 
D) Heisenberg uncertainty principle. 
E) the quantum model. 
A) the aufbau principle. 
B) Hund's rule. 
C) the Pauli exclusion principle. 
D) Heisenberg uncertainty principle. 
E) the quantum model.

Question 15

Which of the following statements concerning the periodic table is incorrect?

Accepted Answer

A) The elements in a given group or family have similar chemical properties. 
B) The chemical characteristics of the elements are periodic functions of their atomic numbers. 
C) All the elements are arranged in order of increasing atomic weight. 
D) Mendeleev left spaces in his periodic table for undiscovered elements. 
E) Mendeleev received most of the credit for the early development of the periodic table. 
A) The elements in a given group or family have similar chemical properties. 
B) The chemical characteristics of the elements are periodic functions of their atomic numbers. 
C) All the elements are arranged in order of increasing atomic weight. 
D) Mendeleev left spaces in his periodic table for undiscovered elements. 
E) Mendeleev received most of the credit for the early development of the periodic table.

Question 16

Which of the following statements is incorrect?

Accepted Answer

A) Stern and Gerlach discovered electron spin by passing silver atoms through a magnetic field. 
B) Hund's rule states that electrons are placed in the orbitals of a subshell in such a way as to give a maximum number of unpaired electrons. 
C) The Pauli exclusion principle states that each electron in an atom must have its own unique set of quantum numbers. 
D) Valence electrons consist of those electrons not contained within a noble-gas core or a pseudo-noble-gas core. 
E) The building-up principle states that electrons are added to atoms in order of increasing principal quantum number. 
A) Stern and Gerlach discovered electron spin by passing silver atoms through a magnetic field. 
B) Hund's rule states that electrons are placed in the orbitals of a subshell in such a way as to give a maximum number of unpaired electrons. 
C) The Pauli exclusion principle states that each electron in an atom must have its own unique set of quantum numbers. 
D) Valence electrons consist of those electrons not contained within a noble-gas core or a pseudo-noble-gas core. 
E) The building-up principle states that electrons are added to atoms in order of increasing principal quantum number.

Question 17

A section of the periodic table with all identification features removed is shown below.
V
W
X
Y
Z
Which element has the smallest atomic radius?

Accepted Answer

A) W 
B) Y 
C) X 
D) Z 
E) V 
A) W 
B) Y 
C) X 
D) Z 
E) V

Question 18

Which of the following electron configurations corresponds to the ground state of an atom of a transition element?

Accepted Answer

A) 1s22s22p5 
B) 1s22s22p63s23p63d104s24p2 
C) 1s22s22p63s23p63d74s2 
D) 1s22s22p63s23p64s2 
E) 1s22s22p63s23p1 
A) 1s22s22p5 
B) 1s22s22p63s23p63d104s24p2 
C) 1s22s22p63s23p63d74s2 
D) 1s22s22p63s23p64s2 
E) 1s22s22p63s23p1

Question 19

What is the maximum number of electrons in an atom that have the set of quantum numbers n= 2 and l= 1?

Accepted Answer

A) 10 
B) 2 
C) 14 
D) 18 
E) 6 
A) 10 
B) 2 
C) 14 
D) 18 
E) 6

Question 20

If the electron could have a third spin state (that is,   ,-  
,and 0),what would be the ground-state electron configuration of carbon?

Accepted Answer

A) 1s22s4 
B) 1s22s32p1 
C) 1s32s3 
D) 1s22s22p2 
E) 1s32s22p1 
A) 1s22s4 
B) 1s22s32p1 
C) 1s32s3 
D) 1s22s22p2 
E) 1s32s22p1

Exam 8: Electron Configurations and Periodicity

Who was the first chemist to recognize patterns in chemical properties of the elements?

An atom of which of the following elements has the highest fourth ionization energy?

Fe has ____ that is(are)unpaired in its d orbitals.

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is

Rank the following ions in order of increasing first ionization energy: O2-,Mg2+,F-,Na+.

Which element is found in the s-block of the periodic table?

An atom of which of the following elements has the smallest first ionization energy?

Which of the following have one or more filled d subshells in their ground state electron configuration?

The change in energy for which of the following processes represents the first ionization energy of iodine?

What is the ground-state electron configuration of terbium (Tb)?

Sodium and potassium have similar chemical and physical properties.This is best explained by the fact that both elements

Which of the following orbital diagrams violates the Pauli exclusion principle? 1s 2s 2p

How many valence electrons does an arsenic atom have?

The statement that "the lowest-energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as

Which of the following statements concerning the periodic table is incorrect?

Which of the following statements is incorrect?

A section of the periodic table with all identification features removed is shown below. V W X Y Z Which element has the smallest atomic radius?

Which of the following electron configurations corresponds to the ground state of an atom of a transition element?

What is the maximum number of electrons in an atom that have the set of quantum numbers n= 2 and l= 1?

If the electron could have a third spin state (that is, ,- ,and 0),what would be the ground-state electron configuration of carbon?

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Solutions

Rates of Reaction

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

Organic Chemistry

Polymer Materials: Synthetic and Biological

Filters

Rank the following ions in order of increasing first ionization energy: O^2-,Mg²⁺,F^-,Na⁺.