Question 1

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye.The energy of one photon of this light is ________ J.

Accepted Answer

A) 1.04 × 10-31 
B) 3.79 × 10-28 
C) 3.79 × 10-19 
D) 1.04 × 10-22 
E) 2.64 × 1018 
A) 1.04 × 10-31 
B) 3.79 × 10-28 
C) 3.79 × 10-19 
D) 1.04 × 10-22 
E) 2.64 × 1018

Question 2

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Accepted Answer

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

Question 3

Identify the color that has a wavelength of 540 nm.

Accepted Answer

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

Question 4

In the electromagnetic spectrum,identify the highest energy radiation

Accepted Answer

The answer of In the electromagnetic spectrum,identify the highest energy...

Question 5

Which of the following established that an electron has wave properties?

Accepted Answer

A) diffraction 
B) spectrum of visible light 
C) photoelectric effect 
D) removal of electron from atom 
A) diffraction 
B) spectrum of visible light 
C) photoelectric effect 
D) removal of electron from atom

Question 6

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 7

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

Accepted Answer

A) 3.37 × 1019 photons 
B) 3.06 × 1030 photons 
C) 1.80 × 1024 photons 
D) 4.03 × 1028 photons 
E) 2.48 × 1025 photons 
A) 3.37 × 1019 photons 
B) 3.06 × 1030 photons 
C) 1.80 × 1024 photons 
D) 4.03 × 1028 photons 
E) 2.48 × 1025 photons

Question 8

Match the following.
-n = 1 to n = 2

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 9

Which of the following has both particle and wave properties?

Accepted Answer

A) electron 
B) light 
C) matter 
D) all of the above 
A) electron 
B) light 
C) matter 
D) all of the above

Question 10

Which of the following quantum numbers describes the orientation of an orbital?

Accepted Answer

A) magnetic quantum number 
B) principal quantum number 
C) angular momentum quantum number 
D) spin quantum number 
E) Schrödinger quantum number 
A) magnetic quantum number 
B) principal quantum number 
C) angular momentum quantum number 
D) spin quantum number 
E) Schrödinger quantum number

Question 11

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.

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 12

How many orbitals are contained in the third principal level (n = 3)of a given atom?

Accepted Answer

A) 9 
B) 3 
C) 18 
D) 7 
E) 5 
A) 9 
B) 3 
C) 18 
D) 7 
E) 5

Question 13

How many subshells are there in the shell with n = 4?

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 18 
A) 3 
B) 4 
C) 6 
D) 18

Question 14

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10-33 m.

Accepted Answer

A) 45.2 m/s 
B) 11.3 m/s 
C) 22.1 m/s 
D) 38.8 m/s 
E) 52.9 m/s 
A) 45.2 m/s 
B) 11.3 m/s 
C) 22.1 m/s 
D) 38.8 m/s 
E) 52.9 m/s

Question 15

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Accepted Answer

A) 4.85 × 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) 4.85 × 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 16

Designate the correct quantum numbers for 2s orbital?

Accepted Answer

A) n = 2,l = 1,m = 0,s = + or -1/2 
B) n = 2,l = 0,m = 0,s = + or -1/2 
C) n = 2,l = 0,m = +1,s = + or -1/2 
D) n = 1,l = 0,m = 0,s = + or -1/2 
A) n = 2,l = 1,m = 0,s = + or -1/2 
B) n = 2,l = 0,m = 0,s = + or -1/2 
C) n = 2,l = 0,m = +1,s = + or -1/2 
D) n = 1,l = 0,m = 0,s = + or -1/2

Question 17

How many sublevels are contained in the second shell (n = 2)of a given atom?

Accepted Answer

A) 1 
B) 2 
C) 9 
D) 4 
E) 3 
A) 1 
B) 2 
C) 9 
D) 4 
E) 3

Question 18

Place the following types of electromagnetic radiation in order of increasing wavelength.
Visible light gamma rays microwaves

Accepted Answer

A) gamma rays < microwaves < visible light 
B) microwaves < visible light < gamma rays 
C) microwaves < gamma rays < visible light 
D) visible light < gamma rays < microwaves 
E) gamma rays < visible light < microwaves 
A) gamma rays < microwaves < visible light 
B) microwaves < visible light < gamma rays 
C) microwaves < gamma rays < visible light 
D) visible light < gamma rays < microwaves 
E) gamma rays < visible light < microwaves

Question 19

Calculate the wavelength of an electron (m = 9.11 × 10-28 g)moving at 3.66 × 106 m/s.

Accepted Answer

A) 1.99 × 10-10 m 
B) 5.03 × 10-10 m 
C) 1.81 × 10-10 m 
D) 5.52 × 10-9 m 
E) 2.76 × 10-9 m 
A) 1.99 × 10-10 m 
B) 5.03 × 10-10 m 
C) 1.81 × 10-10 m 
D) 5.52 × 10-9 m 
E) 2.76 × 10-9 m

Question 20

Describe the shape of a p orbital.

Accepted Answer

A) a ball 
B) two balls 
C) three balls 
D) four balls 
A) a ball 
B) two balls 
C) three balls 
D) four balls

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye.The energy of one photon of this light is ________ J.

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Identify the color that has a wavelength of 540 nm.

In the electromagnetic spectrum,identify the highest energy radiation

Which of the following established that an electron has wave properties?

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

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

Match the following. -n = 1 to n = 2

Which of the following has both particle and wave properties?

Which of the following quantum numbers describes the orientation of an orbital?

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.

How many orbitals are contained in the third principal level (n = 3)of a given atom?

How many subshells are there in the shell with n = 4?

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10^-33 m.

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Designate the correct quantum numbers for 2s orbital?

How many sublevels are contained in the second shell (n = 2)of a given atom?

Place the following types of electromagnetic radiation in order of increasing wavelength. Visible light gamma rays microwaves

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g)moving at 3.66 × 10⁶ m/s.

Describe the shape of a p orbital.

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Exam 7: The Quantum-Mechanical Model of the Atom

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye.The energy of one photon of this light is ________ J.

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Identify the color that has a wavelength of 540 nm.

In the electromagnetic spectrum,identify the highest energy radiation

Which of the following established that an electron has wave properties?

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

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

Match the following. -n = 1 to n = 2

Which of the following has both particle and wave properties?

Which of the following quantum numbers describes the orientation of an orbital?

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.

How many orbitals are contained in the third principal level (n = 3)of a given atom?

How many subshells are there in the shell with n = 4?

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10-33 m.

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Designate the correct quantum numbers for 2s orbital?

How many sublevels are contained in the second shell (n = 2)of a given atom?

Place the following types of electromagnetic radiation in order of increasing wavelength. Visible light gamma rays microwaves

Calculate the wavelength of an electron (m = 9.11 × 10-28 g)moving at 3.66 × 106 m/s.

Describe the shape of a p orbital.

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

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.

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10^-33 m.

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g)moving at 3.66 × 10⁶ m/s.