Question 1

Identify the location of the visible range of light.

Accepted Answer

A) between X-ray and ultraviolet 
B) between microwave and radio 
C) between gamma ray and ultraviolet 
D) between X-ray and gamma ray 
E) between ultraviolet and infrared 
A) between X-ray and ultraviolet 
B) between microwave and radio 
C) between gamma ray and ultraviolet 
D) between X-ray and gamma ray 
E) between ultraviolet and infrared

Question 2

Give the value of l for a 3p sublevel.

Accepted Answer

A) 1 
B) -4 
C) -1 
D) 2 
E) -2 
A) 1 
B) -4 
C) -1 
D) 2 
E) -2

Question 3

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

Accepted Answer

A) 7.62 × 103 kJ 
B) 2.76 × 103 kJ 
C) 1.31 × 103 kJ 
D) 3.62 × 103 kJ 
E) 5.33 × 103 kJ 
A) 7.62 × 103 kJ 
B) 2.76 × 103 kJ 
C) 1.31 × 103 kJ 
D) 3.62 × 103 kJ 
E) 5.33 × 103 kJ

Question 4

Which of the following occurs as the wavelength of a photon increases?

Accepted Answer

A) The frequency decreases. 
B) The energy increases. 
C) The speed decreases. 
D) Planck's constant decreases. 
E) None of the above occurs as the wavelength of a photon increases. 
A) The frequency decreases. 
B) The energy increases. 
C) The speed decreases. 
D) Planck's constant decreases. 
E) None of the above occurs as the wavelength of a photon increases.

Question 5

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does not contain an error.

Accepted Answer

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

Question 6

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

Accepted Answer

A) 1.46 × 1014 s-1 
B) 6.86 × 1014 s-1 
C) 4.33 × 1014 s-1 
D) 6.17 × 1014 s-1 
E) 1.62 × 1014 s-1 
A) 1.46 × 1014 s-1 
B) 6.86 × 1014 s-1 
C) 4.33 × 1014 s-1 
D) 6.17 × 1014 s-1 
E) 1.62 × 1014 s-1

Question 7

Which statement is correct about orbital?

Accepted Answer

A) An orbital can have maximum two electrons. 
B) A p orbital can have six electrons. 
C) An s orbital has no shape. 
D) All p orbitals have same orientation. 
A) An orbital can have maximum two electrons. 
B) A p orbital can have six electrons. 
C) An s orbital has no shape. 
D) All p orbitals have same orientation.

Question 8

Place the following types of electromagnetic radiation in order of increasing wavelength.
Ultraviolet light gamma rays radio waves

Accepted Answer

A) gamma rays < radio waves < ultraviolet light 
B) radio waves < ultraviolet light < gamma rays 
C) radio waves < gamma rays < ultraviolet light 
D) ultraviolet light < gamma rays < radio waves 
E) gamma rays < ultraviolet light < radio waves 
A) gamma rays < radio waves < ultraviolet light 
B) radio waves < ultraviolet light < gamma rays 
C) radio waves < gamma rays < ultraviolet light 
D) ultraviolet light < gamma rays < radio waves 
E) gamma rays < ultraviolet light < radio waves

Question 9

How many orbitals are there in the fourth shell?

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 16 
A) 3 
B) 4 
C) 6 
D) 16

Question 10

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 11

In which orbital below would an electron (on average)be farthest from the nucleus?

Accepted Answer

A) 1s 
B) 4f 
C) 3s 
D) 3d 
E) 2p 
A) 1s 
B) 4f 
C) 3s 
D) 3d 
E) 2p

Question 12

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Accepted Answer

A) +4.89 × 10-18 J 
B) +1.64 × 10-18 J 
C) -6.12 × 10-18 J 
D) +3.55 × 10-18 J 
E) -2.04 × 10-18 J 
A) +4.89 × 10-18 J 
B) +1.64 × 10-18 J 
C) -6.12 × 10-18 J 
D) +3.55 × 10-18 J 
E) -2.04 × 10-18 J

Question 13

Each of the following sets of quantum numbers is supposed to specify an orbital.Which of the following sets of quantum numbers contains an error?

Accepted Answer

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

Question 14

In which orbital below would an electron (on average)be closest to the nucleus?

Accepted Answer

A) 2p 
B) 4s 
C) 2s 
D) 5d 
E) 3p 
A) 2p 
B) 4s 
C) 2s 
D) 5d 
E) 3p

Question 15

Which of the following visible colors of light has the highest frequency?

Accepted Answer

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

Question 16

How much energy,in kJ,is required to ionize 2.78 moles of hydrogen atoms?

Accepted Answer

A) 2.74 × 103 kJ 
B) 4.72 × 103 kJ 
C) 1.66 × 103 kJ 
D) 3.65 × 103 kJ 
E) 5.89 × 103 kJ 
A) 2.74 × 103 kJ 
B) 4.72 × 103 kJ 
C) 1.66 × 103 kJ 
D) 3.65 × 103 kJ 
E) 5.89 × 103 kJ

Question 17

Which of the following statements are true?

Accepted Answer

A) The principal quantum number (n)describes the shape of an orbital. 
B) The angular momentum quantum number (l)describes 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. 
E) All of the above are true. 
A) The principal quantum number (n)describes the shape of an orbital. 
B) The angular momentum quantum number (l)describes 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. 
E) All of the above are true.

Question 18

Which of the following visible colors of light 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 19

Choose the transition (in a hydrogen atom)below that represents the absorption of the shortest wavelength photon.

Accepted Answer

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

Question 20

What is the photoelectric effect?

Accepted Answer

Many metals emit electrons whe

Identify the location of the visible range of light.

Give the value of l for a 3p sublevel.

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

Which of the following occurs as the wavelength of a photon increases?

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does not contain an error.

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

Which statement is correct about orbital?

Place the following types of electromagnetic radiation in order of increasing wavelength. Ultraviolet light gamma rays radio waves

How many orbitals are there in the fourth shell?

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

In which orbital below would an electron (on average)be farthest from the nucleus?

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Each of the following sets of quantum numbers is supposed to specify an orbital.Which of the following sets of quantum numbers contains an error?

In which orbital below would an electron (on average)be closest to the nucleus?

Which of the following visible colors of light has the highest frequency?

How much energy,in kJ,is required to ionize 2.78 moles of hydrogen atoms?

Which of the following statements are true?

Which of the following visible colors of light has the shortest wavelength?

Choose the transition (in a hydrogen atom)below that represents the absorption of the shortest wavelength photon.

What is the photoelectric effect?

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Exam 7: The Quantum-Mechanical Model of the Atom

Identify the location of the visible range of light.

Give the value of l for a 3p sublevel.

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

Which of the following occurs as the wavelength of a photon increases?

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does not contain an error.

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

Which statement is correct about orbital?

Place the following types of electromagnetic radiation in order of increasing wavelength. Ultraviolet light gamma rays radio waves

How many orbitals are there in the fourth shell?

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

In which orbital below would an electron (on average)be farthest from the nucleus?

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Each of the following sets of quantum numbers is supposed to specify an orbital.Which of the following sets of quantum numbers contains an error?

In which orbital below would an electron (on average)be closest to the nucleus?

Which of the following visible colors of light has the highest frequency?

How much energy,in kJ,is required to ionize 2.78 moles of hydrogen atoms?

Which of the following statements are true?

Which of the following visible colors of light has the shortest wavelength?

Choose the transition (in a hydrogen atom)below that represents the absorption of the shortest wavelength photon.

What is the photoelectric effect?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

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