Question 1

What is the core charge for the calcium atom, Ca?

Accepted Answer

A)  +1 
B)  +2 
C)  +8 
D)  +10 
E)  +20 
A)  +1 
B)  +2 
C)  +8 
D)  +10 
E)  +20

Question 2

Why is the ionization energy of potassium (K) less than the ionization energy of sodium (Na)?

Accepted Answer

A)  The ionized electron in K is in a higher energy shell than the ionized electron in Na. 
B)  Because the core charge remains the same going down a group 
C)  Because K has more protons in its nucleus than Na. 
D)  Because the core charge decreases down a group 
E)  Because the ionized electron in K is in a higher energy shell AND because the core charge of K and Na are the same. 
A)  The ionized electron in K is in a higher energy shell than the ionized electron in Na. 
B)  Because the core charge remains the same going down a group 
C)  Because K has more protons in its nucleus than Na. 
D)  Because the core charge decreases down a group 
E)  Because the ionized electron in K is in a higher energy shell AND because the core charge of K and Na are the same.

Question 3

A photoelectron spectrum has three peaks. The first two are one third the size of the last one. Which atom corresponds to this spectrum?

Accepted Answer

A)  He 
B)  Be 
C)  C 
D)  O 
E)  Ne 
A)  He 
B)  Be 
C)  C 
D)  O 
E)  Ne

Question 4

What would you describe as the key result of the Rutherford experiment, in which a metal target was bombarded with  
 $\alpha$ -particles?

Accepted Answer

A)  The  $\alpha$ -particles were able to pass through the target. 
B)  The particles were found to knock electrons out of the target. 
C)  Some of the  $\alpha$ -particles were deflected through large angles. 
D)  Flashes of light were emitted when the  $\alpha$ -particles hit the ZnS screen after they passed through the target. 
E)  The experiment showed the need for better  $\alpha$ -particle detectors. 
A)  The  $\alpha$ -particles were able to pass through the target. 
B)  The particles were found to knock electrons out of the target. 
C)  Some of the  $\alpha$ -particles were deflected through large angles. 
D)  Flashes of light were emitted when the  $\alpha$ -particles hit the ZnS screen after they passed through the target. 
E)  The experiment showed the need for better  $\alpha$ -particle detectors.

Question 5

A helium-neon laser emits light with a wavelength of 6328 Å. What is the energy of a 6328 Å photon in joules?

Accepted Answer

A)  2.179 x 10-19 J 
B)  3.139 x 10-19 J 
C)  5.448 x 10-19 J 
D)  6.328 x 10-19 J 
E)  2.179 x 10-18 J 
A)  2.179 x 10-19 J 
B)  3.139 x 10-19 J 
C)  5.448 x 10-19 J 
D)  6.328 x 10-19 J 
E)  2.179 x 10-18 J

Question 6

Which of the following statements about the Bohr model is wrong?

Accepted Answer

A)  The energy of the electron is quantized. 
B)  All possible wavelengths can occur in the emission spectrum since n runs from 1 to infinity. 
C)  The angular momentum of the electron is quantized. 
D)  All quantized energies are negative. 
E)  The electron travels around the nucleus in an orbit. 
A)  The energy of the electron is quantized. 
B)  All possible wavelengths can occur in the emission spectrum since n runs from 1 to infinity. 
C)  The angular momentum of the electron is quantized. 
D)  All quantized energies are negative. 
E)  The electron travels around the nucleus in an orbit.

Question 7

Which element is represented by the following PES spectrum?

Accepted Answer

A)  Li 
B)  Mg 
C)  Ca 
D)  Be 
E)  Ne 
A)  Li 
B)  Mg 
C)  Ca 
D)  Be 
E)  Ne

Question 8

Which of the following transitions in the spectrum of the hydrogen atom results in the absorption of a photon with the largest energy?

Accepted Answer

A)  n = 2 to n = 3 
B)  n = 2 to n = 4 
C)  n = 1 to n = 4 
D)  n = 3 to n = 1 
E)  n = 7 to n = 1 
A)  n = 2 to n = 3 
B)  n = 2 to n = 4 
C)  n = 1 to n = 4 
D)  n = 3 to n = 1 
E)  n = 7 to n = 1

Question 9

Which ion, Na+ or K+, is the smaller? Explain.

Accepted Answer

Na⁺. The potassium ion will hav

Question 10

Which of the following atomic orbitals doesn't exist?

Accepted Answer

A)  3f 
B)  3p 
C)  5f 
D)  5d 
E)  6s 
A)  3f 
B)  3p 
C)  5f 
D)  5d 
E)  6s

Question 11

In what group of the periodic table would an element with the following electron configuration belong?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

Accepted Answer

A)  Group IA 
B)  Group IlIA 
C)  Group VA 
D)  Group VIIA 
E)  none of the above 
A)  Group IA 
B)  Group IlIA 
C)  Group VA 
D)  Group VIIA 
E)  none of the above

Question 12

A possible set of quantum numbers for the last electron added to form a gallium atom (Z = 31) in its lowest energy state is:

Accepted Answer

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

Question 13

Which set of quantum numbers can be used to describe a 2p electron?

Accepted Answer

A)  2,1,0,-   
B)  2,0,0,   
C)  2,2,1,   
D)  3,2,1,-   
E)  3,1,0,   
A)  2,1,0,-   
B)  2,0,0,   
C)  2,2,1,   
D)  3,2,1,-   
E)  3,1,0,

Question 14

Arrange the following atoms in order of increasing first ionization energy.

Accepted Answer

A)  P < S < Cl 
B)  Cl < S < P 
C)  S < P < Cl 
D)  S < Cl < P 
E)  Cl < P < S 
A)  P < S < Cl 
B)  Cl < S < P 
C)  S < P < Cl 
D)  S < Cl < P 
E)  Cl < P < S

Question 15

Which of the following selection rules for quantum numbers is incorrectly stated?

Accepted Answer

A)  n is any integer greater than or equal to zero. 
B)  l is any integer between zero and n - 1. 
C)  ml is any integer between -/ and +/. 
D)  ms is either +   or -   . 
E)  All of the above selection rules are correctly stated. 
A)  n is any integer greater than or equal to zero. 
B)  l is any integer between zero and n - 1. 
C)  ml is any integer between -/ and +/. 
D)  ms is either +   or -   . 
E)  All of the above selection rules are correctly stated.

Question 16

Give the full electron configuration of arsenic, As.

Accepted Answer

1s² 2s² 2p⁶ 3

Question 17

Why is the first ionization energy of Br less than that of Cl?

Accepted Answer

A)  Bromine has more protons than chlorine. 
B)  Bromine has more electrons than chlorine. 
C)  The core charge on bromine is less than that on chlorine. 
D)  The outer shell electrons in bromine are farther from the nucleus than in chlorine. 
E)  none of these 
A)  Bromine has more protons than chlorine. 
B)  Bromine has more electrons than chlorine. 
C)  The core charge on bromine is less than that on chlorine. 
D)  The outer shell electrons in bromine are farther from the nucleus than in chlorine. 
E)  none of these

Question 18

Which transition in the spectrum of the hydrogen atom results in the emission of light with the longest wavelength?

Accepted Answer

A)  n = 3 to n = 2 
B)  n = 3 to n = 1 
C)  n = 5 to n = 4 
D)  n = 2 to n = 3 
E)  n = 1 to n = 3 
A)  n = 3 to n = 2 
B)  n = 3 to n = 1 
C)  n = 5 to n = 4 
D)  n = 2 to n = 3 
E)  n = 1 to n = 3

Question 19

In which of the following groups of atoms does each atom have the same number of outer shell electrons?

Accepted Answer

A)  B, C, N 
B)  K, Ca, P 
C)  C, Si, Ge 
D)  O, F, Cl 
E)  N, P, Cl 
A)  B, C, N 
B)  K, Ca, P 
C)  C, Si, Ge 
D)  O, F, Cl 
E)  N, P, Cl

Question 20

In period 6 of the periodic table, the series of elements which differ in the number of electrons contained in f orbitals

Accepted Answer

A)  begins with Cs and ends with Rn. 
B)  begins with La and ends with Hg. 
C)  begins with Tl and ends with Rn. 
D)  begins with La and ends with Rn. 
E)  begins with Ce and ends with Lu. 
A)  begins with Cs and ends with Rn. 
B)  begins with La and ends with Hg. 
C)  begins with Tl and ends with Rn. 
D)  begins with La and ends with Rn. 
E)  begins with Ce and ends with Lu.

What is the core charge for the calcium atom, Ca?

Why is the ionization energy of potassium (K) less than the ionization energy of sodium (Na)?

A photoelectron spectrum has three peaks. The first two are one third the size of the last one. Which atom corresponds to this spectrum?

What would you describe as the key result of the Rutherford experiment, in which a metal target was bombarded with $\alpha$ -particles?

A helium-neon laser emits light with a wavelength of 6328 Å. What is the energy of a 6328 Å photon in joules?

Which of the following statements about the Bohr model is wrong?

Which element is represented by the following PES spectrum?

Which of the following transitions in the spectrum of the hydrogen atom results in the absorption of a photon with the largest energy?

Which ion, Na⁺or K⁺, is the smaller? Explain.

Which of the following atomic orbitals doesn't exist?

In what group of the periodic table would an element with the following electron configuration belong? 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹

A possible set of quantum numbers for the last electron added to form a gallium atom (Z = 31) in its lowest energy state is:

Which set of quantum numbers can be used to describe a 2p electron?

Arrange the following atoms in order of increasing first ionization energy.

Which of the following selection rules for quantum numbers is incorrectly stated?

Give the full electron configuration of arsenic, As.

Why is the first ionization energy of Br less than that of Cl?

Which transition in the spectrum of the hydrogen atom results in the emission of light with the longest wavelength?

In which of the following groups of atoms does each atom have the same number of outer shell electrons?

In period 6 of the periodic table, the series of elements which differ in the number of electrons contained in f orbitals

Elements Compounds

The Mole

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Exam 3: Structure of the Atom

What is the core charge for the calcium atom, Ca?

Why is the ionization energy of potassium (K) less than the ionization energy of sodium (Na)?

A photoelectron spectrum has three peaks. The first two are one third the size of the last one. Which atom corresponds to this spectrum?

What would you describe as the key result of the Rutherford experiment, in which a metal target was bombarded with α\alphaα -particles?

A helium-neon laser emits light with a wavelength of 6328 Å. What is the energy of a 6328 Å photon in joules?

Which of the following statements about the Bohr model is wrong?

Which element is represented by the following PES spectrum?

Which of the following transitions in the spectrum of the hydrogen atom results in the absorption of a photon with the largest energy?

Which ion, Na+ or K+, is the smaller? Explain.

Which of the following atomic orbitals doesn't exist?

In what group of the periodic table would an element with the following electron configuration belong? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

A possible set of quantum numbers for the last electron added to form a gallium atom (Z = 31) in its lowest energy state is:

Which set of quantum numbers can be used to describe a 2p electron?

Arrange the following atoms in order of increasing first ionization energy.

Which of the following selection rules for quantum numbers is incorrectly stated?

Give the full electron configuration of arsenic, As.

Why is the first ionization energy of Br less than that of Cl?

Which transition in the spectrum of the hydrogen atom results in the emission of light with the longest wavelength?

In which of the following groups of atoms does each atom have the same number of outer shell electrons?

In period 6 of the periodic table, the series of elements which differ in the number of electrons contained in f orbitals

Elements Compounds

The Mole

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

What would you describe as the key result of the Rutherford experiment, in which a metal target was bombarded with $\alpha$ -particles?

Which ion, Na⁺or K⁺, is the smaller? Explain.

In what group of the periodic table would an element with the following electron configuration belong? 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹