Question 1

Contact lenses can focus light due to the ___________ of the waves.

Accepted Answer

A) diffraction 
B) reflection 
C) refraction 
D) dispersion 
E) interference 
A) diffraction 
B) reflection 
C) refraction 
D) dispersion 
E) interference

Question 2

Use the Rydberg equation to calculate the wavelength,in nm,of the least energetic (longest wavelength)line in the visible series (n1 = 2)of the spectrum of atomic hydrogen.

Accepted Answer

Question 3

The following combinations of quantum numbers are not allowed.Correct each set by changing only one quantum number,and write in an appropriate corrected value.

Accepted Answer

a.n = 3
b.

Question 4

In the quantum mechanical treatment of the hydrogen atom,the energy depends on the principal quantum number n but not on the values of l or ml.

Accepted Answer

A) True 
 B)False

Question 5

a.Calculate the wavelength in nm of a photon whose energy is 6.00 $\times$ 10-19 J.
b.Would the photon in (a)have enough energy to ionize a hydrogen atom in its ground state (i.e. ,to separate the proton and electron completely)? Use the Bohr equation to explain your answer.

Accepted Answer

a.331 nm
b.No.2.18 @#LAT-DLM&

Question 6

Explain the context and meanings of the terms "orbit" and "orbital",making a clear distinction between them.

Accepted Answer

Orbit is a term from the Bohr theory,and

Question 7

a.Use the Bohr equation to calculate the energy needed to ionize a hydrogen atom from its ground state.
b.What is the minimum wavelength of a photon needed for it to have the energy needed in (a)?

Accepted Answer

a.2.18 @#LAT-DLM& 10

Question 8

Use the Bohr equation to calculate the energy of
a.the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom.
b.the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

Accepted Answer

a.1.64 @#LAT-DLM& 10^-18</

Question 9

Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom?

Accepted Answer

A) Planck 
B) Bohr 
C) Rydberg 
D) Rutherford 
E) Thomson 
A) Planck 
B) Bohr 
C) Rydberg 
D) Rutherford 
E) Thomson

Question 10

a.Use Bohr's equation to calculate how much energy (in J)is needed to promote an electron from the H-atom ground state to the n = 4 level.
b.If a photon provides the energy in (a),what is its wavelength in nm?

Accepted Answer

a.2.04 @#LAT-DLM& 10

Question 11

Line spectra are characteristic of atoms in the gas phase.

Accepted Answer

A) True 
 B)False

Question 12

For the following orbitals,state the values of n,l and ml which apply,and draw a sketch showing the shape and orientation of the orbital.
a.3s
b.2px

Accepted Answer

a.3s n = 3,l = 0,m_l =

Question 13

Line spectra from all regions of the electromagnetic spectrum,including the Paschen series of infrared lines for hydrogen,are used by astronomers to identify elements present in the atmospheres of stars.Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3.(R = 1.096776 $\times$ 107 m-1)

Accepted Answer

A) 205.1 nm 
B) 384.6 nm 
C) 683.8 nm 
D) 1282 nm 
E) > 1500 nm 
A) 205.1 nm 
B) 384.6 nm 
C) 683.8 nm 
D) 1282 nm 
E) > 1500 nm

Question 14

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

Accepted Answer

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

Question 15

A photon has an energy of 5.53 $\times$ 10-17 J.What is its frequency in s-1?

Accepted Answer

A) 3.66 $\times$ 10-50 s-1 
B) 1.20 $\times$ 10-17 s-1 
C) 3.59 $\times$ 10-9 s-1 
D) 2.78 $\times$ 108 s-1 
E) 8.35 $\times$ 1016 s-1 
A) 3.66 $\times$ 10-50 s-1 
B) 1.20 $\times$ 10-17 s-1 
C) 3.59 $\times$ 10-9 s-1 
D) 2.78 $\times$ 108 s-1 
E) 8.35 $\times$ 1016 s-1

Question 16

Who was the first scientist to propose that an object could emit only certain amounts of energy?

Accepted Answer

A) Planck 
B) Einstein 
C) Bohr 
D) Rydberg 
E) de Broglie 
A) Planck 
B) Einstein 
C) Bohr 
D) Rydberg 
E) de Broglie

Question 17

The energy of an electron in the hydrogen atom is determined by

Accepted Answer

A) the principal quantum number (n)only. 
B) the angular momentum quantum number (l )only. 
C) the principal and angular momentum quantum numbers (n & l ). 
D) the principal and magnetic quantum numbers (n & ml). 
E) the principal,angular momentum and magnetic quantum numbers. 
A) the principal quantum number (n)only. 
B) the angular momentum quantum number (l )only. 
C) the principal and angular momentum quantum numbers (n & l ). 
D) the principal and magnetic quantum numbers (n & ml). 
E) the principal,angular momentum and magnetic quantum numbers.

Question 18

What are the possible values for the following quantum numbers in an atom?
a.n
b.l
c.ml

Accepted Answer

a.n = 1,2,3,...
b.l

Question 19

What is the speed of an electron in m/s if its wavelength is 0.155 nm?

Accepted Answer

4.69 @#LAT-DLM& 10<s

Question 20

The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz.Find the wavelength of these waves.

Accepted Answer

A) 4.30 $\times$ 10-2 m 
B) 0.144 m 
C) 6.94 m 
D) 232 m 
E) > 103 m 
A) 4.30 $\times$ 10-2 m 
B) 0.144 m 
C) 6.94 m 
D) 232 m 
E) > 103 m

Exam 7: Quantum Theory and Atomic Structure

Contact lenses can focus light due to the ___________ of the waves.

Use the Rydberg equation to calculate the wavelength,in nm,of the least energetic (longest wavelength)line in the visible series (n1 = 2)of the spectrum of atomic hydrogen.

The following combinations of quantum numbers are not allowed.Correct each set by changing only one quantum number,and write in an appropriate corrected value.

In the quantum mechanical treatment of the hydrogen atom,the energy depends on the principal quantum number n but not on the values of l or ml.

a.Calculate the wavelength in nm of a photon whose energy is 6.00 ×\times× 10-19 J. b.Would the photon in (a)have enough energy to ionize a hydrogen atom in its ground state (i.e. ,to separate the proton and electron completely)? Use the Bohr equation to explain your answer.

Explain the context and meanings of the terms "orbit" and "orbital",making a clear distinction between them.

a.Use the Bohr equation to calculate the energy needed to ionize a hydrogen atom from its ground state. b.What is the minimum wavelength of a photon needed for it to have the energy needed in (a)?

Use the Bohr equation to calculate the energy of a.the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom. b.the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom?

a.Use Bohr's equation to calculate how much energy (in J)is needed to promote an electron from the H-atom ground state to the n = 4 level. b.If a photon provides the energy in (a),what is its wavelength in nm?

Line spectra are characteristic of atoms in the gas phase.

For the following orbitals,state the values of n,l and ml which apply,and draw a sketch showing the shape and orientation of the orbital. a.3s b.2px

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

A photon has an energy of 5.53 ×\times× 10-17 J.What is its frequency in s-1?

Who was the first scientist to propose that an object could emit only certain amounts of energy?

The energy of an electron in the hydrogen atom is determined by

What are the possible values for the following quantum numbers in an atom? a.n b.l c.ml

What is the speed of an electron in m/s if its wavelength is 0.155 nm?

The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz.Find the wavelength of these waves.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Use the Rydberg equation to calculate the wavelength,in nm,of the least energetic (longest wavelength)line in the visible series (n₁ = 2)of the spectrum of atomic hydrogen.

In the quantum mechanical treatment of the hydrogen atom,the energy depends on the principal quantum number n but not on the values of l or m_l.

a.Calculate the wavelength in nm of a photon whose energy is 6.00 $\times$ 10^-19 J. b.Would the photon in (a)have enough energy to ionize a hydrogen atom in its ground state (i.e. ,to separate the proton and electron completely)? Use the Bohr equation to explain your answer.

For the following orbitals,state the values of n,l and m_l which apply,and draw a sketch showing the shape and orientation of the orbital. a.3s b.2p_x

A photon has an energy of 5.53 $\times$ 10^-17 J.What is its frequency in s^-1?

What are the possible values for the following quantum numbers in an atom? a.n b.l c.m_l