Question 1

Only two electrons,with opposing spins,are allowed in each orbital.What is this known as?

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 2

Which of the following colours of electromagnetic radiation has the shortest wavelength?

Accepted Answer

A) blue 
B) violet 
C) orange 
D) green 
E) yellow 
A) blue 
B) violet 
C) orange 
D) green 
E) yellow

Question 3

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 
1.76 × 103 kJ mol-1.

Accepted Answer

A) 147 nm 
B) 68.0 nm 
C) 113 nm 
D) 885 nm 
E) 387 nm 
A) 147 nm 
B) 68.0 nm 
C) 113 nm 
D) 885 nm 
E) 387 nm

Question 4

Identify the ground-state electron configuration for Mg2+.

Accepted Answer

A) 1s22s22p63s2 
B) 1s22s22p6 
C) 1s22s22p63s23p2 
D) 1s22s22p63s23p6 
E) 1s22s22p63s1 
A) 1s22s22p63s2 
B) 1s22s22p6 
C) 1s22s22p63s23p2 
D) 1s22s22p63s23p6 
E) 1s22s22p63s1

Question 5

Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.

Accepted Answer

A) 2.20 × 1014 s-1 
B) 1.98 × 1014 s-1 
C) 4.55 × 1014 s-1 
D) 5.05 × 1014 s-1 
E) 3.32 × 1014 s-1 
A) 2.20 × 1014 s-1 
B) 1.98 × 1014 s-1 
C) 4.55 × 1014 s-1 
D) 5.05 × 1014 s-1 
E) 3.32 × 1014 s-1

Question 6

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410 nm.

Accepted Answer

A) 4.84 × 10-19 J 
B) 2.06 × 10-19 J 
C) 1.23 × 10-19 J 
D) 8.13 × 10-19 J 
E) 5.27 × 10-19 J 
A) 4.84 × 10-19 J 
B) 2.06 × 10-19 J 
C) 1.23 × 10-19 J 
D) 8.13 × 10-19 J 
E) 5.27 × 10-19 J

Question 7

Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.

Accepted Answer

A) 2.19 × 1014 s-1 
B) 5.59 × 1014 s-1 
C) 4.57 × 1014 s-1 
D) 1.79 × 1014 s-1 
E) 3.28 × 1014 s-1 
A) 2.19 × 1014 s-1 
B) 5.59 × 1014 s-1 
C) 4.57 × 1014 s-1 
D) 1.79 × 1014 s-1 
E) 3.28 × 1014 s-1

Question 8

Give the electron configuration for O.

Accepted Answer

A) 1s22s22p4 
B) 1s22p4 
C) 1s22s22p3 
D) 1s22s22p5 
E) 1s22s22p2 
A) 1s22s22p4 
B) 1s22p4 
C) 1s22s22p3 
D) 1s22s22p5 
E) 1s22s22p2

Question 9

Choose the orbital diagram that represents the ground state of N.

Accepted Answer

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

Question 10

If two electrons in the same atom have the same value of l,they are

Accepted Answer

A) in the same sublevel,but not necessarily in the same level. 
B) in the same level,but in different sublevels. 
C) in the same orbital. 
D) in different levels and in different shaped orbitals. 
E) None of the above. 
A) in the same sublevel,but not necessarily in the same level. 
B) in the same level,but in different sublevels. 
C) in the same orbital. 
D) in different levels and in different shaped orbitals. 
E) None of the above.

Question 11

The de Broglie wavelength of an electron with a velocity of 9.00 × $10 ^ { 6 }$ m s-1 is ________ m.The mass of the electron is 9.11 × $10 ^ { - 28 }$ g.

Accepted Answer

A) 1.24 × 1010 
B) 1.24 × 1013 
C) 8.08 × 10-17 
D) 8.08 × 10-14 
E) 8.08 × 10-11 
A) 1.24 × 1010 
B) 1.24 × 1013 
C) 8.08 × 10-17 
D) 8.08 × 10-14 
E) 8.08 × 10-11

Question 12

Identify the colour of a flame test for potassium.

Accepted Answer

A) violet 
B) red 
C) white 
D) yellow 
E) blue 
A) violet 
B) red 
C) white 
D) yellow 
E) blue

Question 13

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

Accepted Answer

A) +3.03 × 10-19 J 
B) -1.82 × 10-19 J 
C) +5.51 × 10-19 J 
D) -3.03 × 10-19 J 
E) +2.69 × 10-19 J 
A) +3.03 × 10-19 J 
B) -1.82 × 10-19 J 
C) +5.51 × 10-19 J 
D) -3.03 × 10-19 J 
E) +2.69 × 10-19 J

Question 14

Why don't we observe the wavelength of everyday macroscopic objects?

Accepted Answer

Due to the large mass of macro

Question 15

Electromagnetic radiation with a wavelength of 471 nm appears as blue light to the human eye.The energy of one photon of this light is 4.22 × $10 ^ { - 19 }$ J.Thus,a laser that emits $1.3 \times 10 ^ { - 2 } \mathrm {~J}$ of energy in a pulse of light at this wavelength produces ________ photons in each pulse.

Accepted Answer

A) 1.5 × $10 ^ { 19 }$ 
B) 1.2 × 10-23 
C) 3.2 × $10 ^ { - 17 }$ 
D) 3.1 × $10 ^ { 16 }$ 
E) 6.5 × $10 ^ { 13 }$ 
A) 1.5 × $10 ^ { 19 }$ 
B) 1.2 × 10-23 
C) 3.2 × $10 ^ { - 17 }$ 
D) 3.1 × $10 ^ { 16 }$ 
E) 6.5 × $10 ^ { 13 }$

Question 16

Describe how a neon light works.

Accepted Answer

A neon sign contains glass tub

Question 17

Determine the end (final)value of n in a hydrogen atom transition if the electron starts in n = 4 and the atom emits a photon of light with a wavelength of 486 nm.

Accepted Answer

A) 1 
B) 5 
C) 3 
D) 4 
E) 2 
A) 1 
B) 5 
C) 3 
D) 4 
E) 2

Question 18

Identify the colour of a flame test for sodium.

Accepted Answer

A) violet 
B) red 
C) white 
D) yellow 
E) blue 
A) violet 
B) red 
C) white 
D) yellow 
E) blue

Question 19

Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves

Accepted Answer

A) radio waves > microwaves > ultraviolet light 
B) ultraviolet light > microwaves > radio waves 
C) radio waves > ultraviolet light > microwaves 
D) ultraviolet light > radio waves > microwaves 
E) microwaves > radio waves > ultraviolet light 
A) radio waves > microwaves > ultraviolet light 
B) ultraviolet light > microwaves > radio waves 
C) radio waves > ultraviolet light > microwaves 
D) ultraviolet light > radio waves > microwaves 
E) microwaves > radio waves > ultraviolet light

Question 20

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy for an atom of hydrogen,making the assumption that ionization is the transition from n = 1 to n = ∞.

Accepted Answer

A) -2.18 × 10-18 J 
B) +2 .18 × 10-18 J 
C) +4.59 × 10-18 J 
D) -4.59 × 10-18 J 
E) +4.36 × 10-18 J 
A) -2.18 × 10-18 J 
B) +2 .18 × 10-18 J 
C) +4.59 × 10-18 J 
D) -4.59 × 10-18 J 
E) +4.36 × 10-18 J

Exam 7: The Quantum-Mechanical Model of the Atom

Only two electrons,with opposing spins,are allowed in each orbital.What is this known as?

Which of the following colours of electromagnetic radiation has the shortest wavelength?

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 103 kJ mol-1.

Identify the ground-state electron configuration for Mg2+.

Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410 nm.

Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.

Give the electron configuration for O.

Choose the orbital diagram that represents the ground state of N.

If two electrons in the same atom have the same value of l,they are

The de Broglie wavelength of an electron with a velocity of 9.00 × 10610 ^ { 6 }106 m s-1 is ________ m.The mass of the electron is 9.11 × 10−2810 ^ { - 28 }10−28 g.

Identify the colour of a flame test for potassium.

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

Why don't we observe the wavelength of everyday macroscopic objects?

Describe how a neon light works.

Determine the end (final)value of n in a hydrogen atom transition if the electron starts in n = 4 and the atom emits a photon of light with a wavelength of 486 nm.

Identify the colour of a flame test for sodium.

Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy for an atom of hydrogen,making the assumption that ionization is the transition from n = 1 to n = ∞.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 10³ kJ mol^-1.

Identify the ground-state electron configuration for Mg²⁺.

The de Broglie wavelength of an electron with a velocity of 9.00 × $10 ^ { 6 }$ m s^-1 is ________ m.The mass of the electron is 9.11 × $10 ^ { - 28 }$ g.