Question 1

Which of the following statements is TRUE?

Accepted Answer

A)  The principal quantum number (n) describes the shape of an orbital. 
B)  The angular momentum quantum number (l) describes the the size and energy associated with an orbital. 
C)  The magnetic quantum number (ml) describes the orientation of the orbital. 
D)  An orbital is the path that an electron follows during its movement in an atom. 
A)  The principal quantum number (n) describes the shape of an orbital. 
B)  The angular momentum quantum number (l) describes the the size and energy associated with an orbital. 
C)  The magnetic quantum number (ml) describes the orientation of the orbital. 
D)  An orbital is the path that an electron follows during its movement in an atom.

Question 2

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 ×   J. Thus, a laser that emits   of energy in a pulse of light at this wavelength produces ________ photons in each pulse.

Accepted Answer

A)  1.5 ×   
B)  1.2 × 10-23 
C)  3.2 ×   
D)  3.1 ×   
E)  6.5 ×   
A)  1.5 ×   
B)  1.2 × 10-23 
C)  3.2 ×   
D)  3.1 ×   
E)  6.5 ×

Question 3

Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays

Accepted Answer

A)  microwaves < visible light < X-rays 
B)  X-rays < visible light < microwaves 
C)  microwaves < X-rays < visible light 
D)  X-rays < microwaves < visible light 
E)  visible light < X-rays < microwaves 
A)  microwaves < visible light < X-rays 
B)  X-rays < visible light < microwaves 
C)  microwaves < X-rays < visible light 
D)  X-rays < microwaves < visible light 
E)  visible light < X-rays < microwaves

Question 4

Which of the following transitions represent the emission of a photon with the largest energy?

Accepted Answer

A)  n = 2 to n = 1 
B)  n = 3 to n = 1 
C)  n = 6 to n = 3 
D)  n = 1 to n = 4 
E)  n = 2 to n = 5 
A)  n = 2 to n = 1 
B)  n = 3 to n = 1 
C)  n = 6 to n = 3 
D)  n = 1 to n = 4 
E)  n = 2 to n = 5

Question 5

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?

Accepted Answer

A)  2s → 3p 
B)  2p → 6d 
C)  6p → 4s 
D)  7f → 5d 
A)  2s → 3p 
B)  2p → 6d 
C)  6p → 4s 
D)  7f → 5d

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

Give the number of core electrons for Br-.

Accepted Answer

A)  35 
B)  18 
C)  30 
D)  40 
E)  28 
A)  35 
B)  18 
C)  30 
D)  40 
E)  28

Question 8

Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

Accepted Answer

A)  3.19 × 10-20 J 
B)  4.18 × 10-20 J 
C)  -6.06 × 10-20 J 
D)  -7.80 × 10-20 J 
E)  -8.62 × 10-20 J 
A)  3.19 × 10-20 J 
B)  4.18 × 10-20 J 
C)  -6.06 × 10-20 J 
D)  -7.80 × 10-20 J 
E)  -8.62 × 10-20 J

Question 9

What is the maximum number of s orbitals that are possible in the same level?

Accepted Answer

A)  1 
B)  3 
C)  7 
D)  5 
E)  9 
A)  1 
B)  3 
C)  7 
D)  5 
E)  9

Question 10

How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?

Accepted Answer

A)  183 kJ 
B)  303 kJ 
C)  394 kJ 
D)  548 kJ 
E)  254 kJ 
A)  183 kJ 
B)  303 kJ 
C)  394 kJ 
D)  548 kJ 
E)  254 kJ

Question 11

Identify the set of four quantum numbers that could represent the electron lost to form the Rb ION from the Rb atom.

Accepted Answer

A)  n = 6, l = 0, ml = 0, ms = -   
B)  n = 4, l = 1, ml = 1, ms = -   
C)  n = 5, l = 1, ml = 0, ms = +   
D)  n = 4, l = 1, ml = 0, ms = -   
E)  n = 5, l = 0, ml = 0, ms = +   
A)  n = 6, l = 0, ml = 0, ms = -   
B)  n = 4, l = 1, ml = 1, ms = -   
C)  n = 5, l = 1, ml = 0, ms = +   
D)  n = 4, l = 1, ml = 0, ms = -   
E)  n = 5, l = 0, ml = 0, ms = +

Question 12

Electromagnetic radiation with a wavelength of 585 nm appears as yellow light to the human eye. The energy of one photon of this light is ________ J.

Accepted Answer

A)  2.94 ×   
B)  1.16 × 10-31 
C)  1.16 × 10-22 
D)  3.40 ×   
E)  3.40 ×   
A)  2.94 ×   
B)  1.16 × 10-31 
C)  1.16 × 10-22 
D)  3.40 ×   
E)  3.40 ×

Question 13

Choose the paramagnetic species from below.

Accepted Answer

A)  Ag 
B)  Ca 
C)  O2- 
D)  Cd2+ 
E)  Zn 
A)  Ag 
B)  Ca 
C)  O2- 
D)  Cd2+ 
E)  Zn

Question 14

Determine the end (final) value of n in a hydrogen atom transition if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.

Accepted Answer

A)  3 
B)  1 
C)  4 
D)  6 
E)  7 
A)  3 
B)  1 
C)  4 
D)  6 
E)  7

Question 15

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

Accepted Answer

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

Question 16

Identify the colour that has a wavelength of 700 nm.

Accepted Answer

A)  blue 
B)  green 
C)  red 
D)  yellow 
A)  blue 
B)  green 
C)  red 
D)  yellow

Question 17

Which of the following types of electromagnetic radiation has the lowest frequency?

Accepted Answer

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

Question 18

The attraction and repulsion between chanrged particles are described by ________.

Accepted Answer

A)  Coulomb's law 
B)  the Pauli exclusion principle 
C)  Hund's rule 
D)  the aufbau principle 
A)  Coulomb's law 
B)  the Pauli exclusion principle 
C)  Hund's rule 
D)  the aufbau principle

Question 19

Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.

Accepted Answer

A)  3.09 × 10-19 J 
B)  6.14 × 10-19 J 
C)  3.24 × 10-19 J 
D)  1.63 × 10-19 J 
E)  5.11 × 10-19 J 
A)  3.09 × 10-19 J 
B)  6.14 × 10-19 J 
C)  3.24 × 10-19 J 
D)  1.63 × 10-19 J 
E)  5.11 × 10-19 J

Question 20

Choose the ground-state electron configuration for Zn2⁺.

Accepted Answer

A)  [Ar]4s23d8 
B)  [Ar]3d10 
C)  [Ar]4s23d6 
D)  [Ar] 
E)  [Ar]3d8 
A)  [Ar]4s23d8 
B)  [Ar]3d10 
C)  [Ar]4s23d6 
D)  [Ar] 
E)  [Ar]3d8

Exam 7: The Quantum-Mechanical Model of the Atom

Which of the following statements is TRUE?

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 × J. Thus, a laser that emits of energy in a pulse of light at this wavelength produces ________ photons in each pulse.

Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays

Which of the following transitions represent the emission of a photon with the largest energy?

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?

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

Give the number of core electrons for Br-.

Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

What is the maximum number of s orbitals that are possible in the same level?

How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?

Identify the set of four quantum numbers that could represent the electron lost to form the Rb ION from the Rb atom.

Electromagnetic radiation with a wavelength of 585 nm appears as yellow light to the human eye. The energy of one photon of this light is ________ J.

Choose the paramagnetic species from below.

Determine the end (final) value of n in a hydrogen atom transition if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.

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

Identify the colour that has a wavelength of 700 nm.

Which of the following types of electromagnetic radiation has the lowest frequency?

The attraction and repulsion between chanrged particles are described by ________.

Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.

Choose the ground-state electron configuration for Zn2⁺.

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

Give the number of core electrons for Br^-.

Determine the end (final) value of n in a hydrogen atom transition if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 10¹⁴ Hz.

Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 10¹⁴ Hz.

Choose the ground-state electron configuration for Zn²⁺.