Question 1

How many valence electrons does an atom of Na possess?

Accepted Answer

A)  1 
B)  3 
C)  4 
D)  7 
E)  0 
A)  1 
B)  3 
C)  4 
D)  7 
E)  0

Question 2

Place the following elements in order of decreasing atomic radius. Xe Cs Ne

Accepted Answer

A)  Ne > Xe > Cs 
B)  Xe > Cs > Ne 
C)  Ne > Cs > Xe 
D)  Cs > Xe > Ne 
E)  Cs > Ne > Xe 
A)  Ne > Xe > Cs 
B)  Xe > Cs > Ne 
C)  Ne > Cs > Xe 
D)  Cs > Xe > Ne 
E)  Cs > Ne > Xe

Question 3

Give the number of core electrons for Mg2+.

Accepted Answer

Question 4

Place the following in order of increasing atomic radius. Sr Li Ca

Accepted Answer

A)  Sr < Ca < Li 
B)  Li < Sr < Ca 
C)  Ca < Sr < Li 
D)  Sr < Li < Ca 
E)  Li < Ca < Sr 
A)  Sr < Ca < Li 
B)  Li < Sr < Ca 
C)  Ca < Sr < Li 
D)  Sr < Li < Ca 
E)  Li < Ca < Sr

Question 5

Place the following in order of increasing radius. I- Mg2+ K+

Accepted Answer

A)  I- + 2+ 
B)  Mg2+ + - 
C)  K+ - 2+ 
D)  I- 2+ + 
E)  K+ 2+ - 
A)  I- + 2+ 
B)  Mg2+ + - 
C)  K+ - 2+ 
D)  I- 2+ + 
E)  K+ 2+ -

Question 6

How many valence electrons does a neutral lanthanide atom have?

Accepted Answer

A)  4 
B)  3 
C)  6 
D)  64 
E)  14 
A)  4 
B)  3 
C)  6 
D)  64 
E)  14

Question 7

Electrons filling up the orbitals from low to high is known as (the)

Accepted Answer

A)  Pauli exclusion principle. 
B)  Hund's rule. 
C)  Aufbau principle. 
D)  Heisenberg uncertainty principle. 
A)  Pauli exclusion principle. 
B)  Hund's rule. 
C)  Aufbau principle. 
D)  Heisenberg uncertainty principle.

Question 8

Of the following,which element has the highest first ionization energy?

Accepted Answer

A)  aluminum 
B)  magnesium 
C)  silicon 
D)  sodium 
A)  aluminum 
B)  magnesium 
C)  silicon 
D)  sodium

Question 9

Place the following elements in order of increasing atomic radius. S Te O

Accepted Answer

A)  Te < S < O 
B)  S < O < Te 
C)  O < S < Te 
D)  O < Te < S 
E)  Te < O < S 
A)  Te < S < O 
B)  S < O < Te 
C)  O < S < Te 
D)  O < Te < S 
E)  Te < O < S

Question 10

Place the following in order of decreasing metallic character. Si S P Cl

Accepted Answer

A)  S > P > Cl > Si 
B)  Cl > S > P > Si 
C)  Si > P > S > Cl 
D)  Cl > P > S > Si 
E)  P > Si > S > Cl 
A)  S > P > Cl > Si 
B)  Cl > S > P > Si 
C)  Si > P > S > Cl 
D)  Cl > P > S > Si 
E)  P > Si > S > Cl

Question 11

Which reaction below represents the electron affinity of Li?

Accepted Answer

A)  Li(g) + e⁻ → Li⁻(g) 
B)  Li(g) → Li⁺(g) + e⁻ 
C)  Li(g) + e⁻ → Li⁺(g) 
D)  Li⁺(g) → Li(g) + e⁻ 
E)  Li⁺(g) + e⁻ → Li(g) 
A)  Li(g) + e⁻ → Li⁻(g) 
B)  Li(g) → Li⁺(g) + e⁻ 
C)  Li(g) + e⁻ → Li⁺(g) 
D)  Li⁺(g) → Li(g) + e⁻ 
E)  Li⁺(g) + e⁻ → Li(g)

Question 12

Of the following,which atom has the largest atomic radius?

Accepted Answer

A)  Li 
B)  F 
C)  Na 
D)  Cl 
A)  Li 
B)  F 
C)  Na 
D)  Cl

Question 13

Why do successive ionization energies increase?

Accepted Answer

After removing the first electron,the sp

Question 14

Which of the following species will have the highest ionization energy?

Accepted Answer

A)  Fr+ 
B)  Xe 
C)  Cl- 
D)  S2- 
E)  As3- 
A)  Fr+ 
B)  Xe 
C)  Cl- 
D)  S2- 
E)  As3-

Question 15

Give the set of four quantum numbers that could represent the electron gained to form the Br ION from the Br atom.

Accepted Answer

A)  n = 4, l = 1, ml = 1, ms = +   
B)  n = 4, l = 0, ml = 1, ms = -   
C)  n = 4, l = 1, ml = 1, ms = -   
D)  n = 3, l = 2, ml = -2, ms = -   
E)  n = 5, l = 1, ml = -1, ms = -   
A)  n = 4, l = 1, ml = 1, ms = +   
B)  n = 4, l = 0, ml = 1, ms = -   
C)  n = 4, l = 1, ml = 1, ms = -   
D)  n = 3, l = 2, ml = -2, ms = -   
E)  n = 5, l = 1, ml = -1, ms = -

Question 16

Which element has the ground-state electron configuration [Xe]6s2?

Accepted Answer

A)  Re 
B)  Ir 
C)  Eu 
D)  Gd 
A)  Re 
B)  Ir 
C)  Eu 
D)  Gd

Question 17

How many unpaired electrons are there in the ground state of Cl?

Accepted Answer

A)  0 
B)  4 
C)  3 
D)  2 
E)  1 
A)  0 
B)  4 
C)  3 
D)  2 
E)  1

Question 18

Choose the diamagnetic species from below.

Accepted Answer

A)  Sn2⁺ 
B)  Br 
C)  As 
D)  Cr 
E)  None of the above is diamagnetic. 
A)  Sn2⁺ 
B)  Br 
C)  As 
D)  Cr 
E)  None of the above is diamagnetic.

Question 19

Choose the valence orbital diagram that represents the ground state of Sr2⁺.

Accepted Answer

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

Question 20

Place the following in order of decreasing radius. Se Cl- Te2-

Accepted Answer

A)  Cl- > Te2- > Se 
B)  Cl- > Se > Te2- 
C)  Se > Te2- > Cl- 
D)  Se > Cl- > Te2- 
E)  Te2- > Cl- > Se 
A)  Cl- > Te2- > Se 
B)  Cl- > Se > Te2- 
C)  Se > Te2- > Cl- 
D)  Se > Cl- > Te2- 
E)  Te2- > Cl- > Se

Exam 8: Periodic Properties of the Elements

How many valence electrons does an atom of Na possess?

Place the following elements in order of decreasing atomic radius. Xe Cs Ne

Give the number of core electrons for Mg2+.

Place the following in order of increasing atomic radius. Sr Li Ca

Place the following in order of increasing radius. I- Mg2+ K+

How many valence electrons does a neutral lanthanide atom have?

Electrons filling up the orbitals from low to high is known as (the)

Of the following,which element has the highest first ionization energy?

Place the following elements in order of increasing atomic radius. S Te O

Place the following in order of decreasing metallic character. Si S P Cl

Which reaction below represents the electron affinity of Li?

Of the following,which atom has the largest atomic radius?

Why do successive ionization energies increase?

Which of the following species will have the highest ionization energy?

Give the set of four quantum numbers that could represent the electron gained to form the Br ION from the Br atom.

Which element has the ground-state electron configuration [Xe]6s2?

How many unpaired electrons are there in the ground state of Cl?

Choose the diamagnetic species from below.

Choose the valence orbital diagram that represents the ground state of Sr2⁺.

Place the following in order of decreasing radius. Se Cl- Te2-

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Give the number of core electrons for Mg²⁺.

Place the following in order of increasing radius. I^- Mg²⁺ K⁺

Which element has the ground-state electron configuration [Xe]6s²?

Choose the valence orbital diagram that represents the ground state of Sr²^⁺.

Place the following in order of decreasing radius. Se Cl^- Te^2-