Question 1

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 C

Question 2

Which statement is correct?

Accepted Answer

A) The probability of finding an electron near the nucleus is very high. 
B) The probability of finding an electron near the nucleus is very low. 
C) An electron can be located all the time within an orbital. 
D) An orbital is a circular path around which electrons revolve round the nucleus. 
A) The probability of finding an electron near the nucleus is very high. 
B) The probability of finding an electron near the nucleus is very low. 
C) An electron can be located all the time within an orbital. 
D) An orbital is a circular path around which electrons revolve round the nucleus. A

Question 3

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

Question 4

What value of l is represented by a d orbital?

Accepted Answer

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

Question 5

Calculate the energy of the green light emitted,per photon,by a mercury lamp with a frequency of 5.49 × 1014 Hz.

Accepted Answer

A) 2.75 × 10-19 J 
B) 3.64 × 10-19 J 
C) 5.46 × 10-19 J 
D) 1.83 × 10-19 J 
E) 4.68 × 10-19 J 
A) 2.75 × 10-19 J 
B) 3.64 × 10-19 J 
C) 5.46 × 10-19 J 
D) 1.83 × 10-19 J 
E) 4.68 × 10-19 J

Question 6

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of
6.88 × 1014 Hz.

Accepted Answer

A) 229 nm 
B) 436 nm 
C) 206 nm 
D) 485 nm 
E) 675 nm 
A) 229 nm 
B) 436 nm 
C) 206 nm 
D) 485 nm 
E) 675 nm

Question 7

Describe how a neon light works.

Accepted Answer

A neon sign contains glass tub

Question 8

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 9

Which of the following statements is true?

Accepted Answer

A) The emission spectrum of a particular element is always the same and can be used to identify the element. 
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. 
C) The uncertainty principle states that we can never know both the exact location and speed of an electron. 
D) An orbital is the volume in which we are most likely to find an electron. 
E) All of the above are true. 
A) The emission spectrum of a particular element is always the same and can be used to identify the element. 
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. 
C) The uncertainty principle states that we can never know both the exact location and speed of an electron. 
D) An orbital is the volume in which we are most likely to find an electron. 
E) All of the above are true.

Question 10

How many different values of l are possible in the third principal level?

Accepted Answer

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

Question 11

What are the possible values of l if n = 6?

Accepted Answer

A) 6 
B) 0,1,2,3,4,or 5 
C) -4,-3,-2,-1,0,+1,+2,+3,or +4 
D) -5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5 
A) 6 
B) 0,1,2,3,4,or 5 
C) -4,-3,-2,-1,0,+1,+2,+3,or +4 
D) -5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5

Question 12

Give the principal level for a 2p sublevel.

Accepted Answer

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

Question 13

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom?

Accepted Answer

A) 656.3 nm 
B) 486.2 nm 
C) 364.6 nm 
D) 2.057 × 10-3 nm 
A) 656.3 nm 
B) 486.2 nm 
C) 364.6 nm 
D) 2.057 × 10-3 nm

Question 14

What is the maximum number of f orbitals that are possible?

Accepted Answer

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

Question 15

For n = 3,what are the possible sublevels?

Accepted Answer

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

Question 16

Match the following.
-n = 3 to n = 1

Accepted Answer

A) 103 nm 
B) 657 nm 
C) 7460 nm 
D) 122 nm 
E) 1280 nm 
A) 103 nm 
B) 657 nm 
C) 7460 nm 
D) 122 nm 
E) 1280 nm

Question 17

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Accepted Answer

The energies of atoms are quantized.When

Question 18

Calculate the wavelength (in nm)of the red light emitted by a neon sign with a frequency of
4.74 × 1014 Hz.

Accepted Answer

A) 633 nm 
B) 158 nm 
C) 142 nm 
D) 704 nm 
E) 466 nm 
A) 633 nm 
B) 158 nm 
C) 142 nm 
D) 704 nm 
E) 466 nm

Question 19

Which of the following transitions (in a hydrogen atom)represent emission of the longest wavelength photon?

Accepted Answer

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

Question 20

X-rays pass through many substances that block visible light and are therefore used to image bones and internal organs.Which of the following is a correct statement about X-rays?

Accepted Answer

A) X-rays have lower energy than visible light. 
B) X-rays have lower frequency than visible light. 
C) X-rays have shorter wavelength than visible light. 
D) X-rays have longer wavelength than visible light. 
A) X-rays have lower energy than visible light. 
B) X-rays have lower frequency than visible light. 
C) X-rays have shorter wavelength than visible light. 
D) X-rays have longer wavelength than visible light.

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

Which statement is correct?

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.

What value of l is represented by a d orbital?

Calculate the energy of the green light emitted,per photon,by a mercury lamp with a frequency of 5.49 × 10¹⁴ Hz.

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 10¹⁴Hz.

Describe how a neon light works.

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

Which of the following statements is true?

How many different values of l are possible in the third principal level?

What are the possible values of l if n = 6?

Give the principal level for a 2p sublevel.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom?

What is the maximum number of f orbitals that are possible?

For n = 3,what are the possible sublevels?

Match the following. -n = 3 to n = 1

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Calculate the wavelength (in nm)of the red light emitted by a neon sign with a frequency of 4.74 × 10¹⁴Hz.

Which of the following transitions (in a hydrogen atom)represent emission of the longest wavelength photon?

X-rays pass through many substances that block visible light and are therefore used to image bones and internal organs.Which of the following is a correct statement about X-rays?

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Molecules, Compounds and Chemical Equations

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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

Liquids, Solids, and Intermolecular Forces

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Exam 7: The Quantum-Mechanical Model of the Atom

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

Which statement is correct?

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.

What value of l is represented by a d orbital?

Calculate the energy of the green light emitted,per photon,by a mercury lamp with a frequency of 5.49 × 1014 Hz.

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Describe how a neon light works.

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

Which of the following statements is true?

How many different values of l are possible in the third principal level?

What are the possible values of l if n = 6?

Give the principal level for a 2p sublevel.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom?

What is the maximum number of f orbitals that are possible?

For n = 3,what are the possible sublevels?

Match the following. -n = 3 to n = 1

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Calculate the wavelength (in nm)of the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.

Which of the following transitions (in a hydrogen atom)represent emission of the longest wavelength photon?

X-rays pass through many substances that block visible light and are therefore used to image bones and internal organs.Which of the following is a correct statement about X-rays?

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 green light emitted,per photon,by a mercury lamp with a frequency of 5.49 × 10¹⁴ Hz.

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 10¹⁴Hz.

Calculate the wavelength (in nm)of the red light emitted by a neon sign with a frequency of 4.74 × 10¹⁴Hz.