Question 1

In the Bohr model of the atom

Accepted Answer

A) gravitational forces play a significant role. 
B) electrons do not radiate energy when they are in a stable orbit. 
C) the electrons spiral into the nucleus. 
D) the energy of an electron in a stable orbit is an integral multiple of h/(2$\pi$). 
E) None of these is correct. 
A) gravitational forces play a significant role. 
B) electrons do not radiate energy when they are in a stable orbit. 
C) the electrons spiral into the nucleus. 
D) the energy of an electron in a stable orbit is an integral multiple of h/(2$\pi$). 
E) None of these is correct.

Question 2

An electron in a hydrogen atom jumps from the n = 5 to n = 3 level.Is a photon absorbed or emitted in this process? What is the wavelength of the photon? State whether the photon is in the visible,ultraviolet,or infrared range of the electro-magnetic spectrum.

Accepted Answer

A) absorbed,1280 nm,infrared 
B) emitted,605 nm,visible 
C) emitted,1280 nm,infrared 
D) absorbed,605 nm,visible 
E) emitted,605 nm,infrared 
A) absorbed,1280 nm,infrared 
B) emitted,605 nm,visible 
C) emitted,1280 nm,infrared 
D) absorbed,605 nm,visible 
E) emitted,605 nm,infrared

Question 3

Use the following figure for the next problem.  
-Which of the following transitions from (a)to (e)is(are)not allowed?

Accepted Answer

A) (a)and (b) 
B) (d)and (e) 
C) (c)and (e) 
D) (c) 
E) (d) 
A) (a)and (b) 
B) (d)and (e) 
C) (c)and (e) 
D) (c) 
E) (d)

Question 4

The equation derived by Bohr for the wavelengths of $\lambda$ of the lines in hydrogen- like spectra is   The first member of the Balmer series of hydrogen has $\lambda$ = 660 nm.Doubly ionized   is hydrogen-like.The wavelength of the first member of the Balmer series for doubly ionized   is

Accepted Answer

A) 73 nm 
B) 5.9 $\times$ 103 nm 
C) 150 nm 
D) 60 nm 
E) 1.8 $\times$ 10-3 nm 
A) 73 nm 
B) 5.9 $\times$ 103 nm 
C) 150 nm 
D) 60 nm 
E) 1.8 $\times$ 10-3 nm

Question 5

The number of oxygen's eight electrons that are found in the p state is

Accepted Answer

A) zero 
B) 2 
C) 4 
D) 6 
E) 8 
A) zero 
B) 2 
C) 4 
D) 6 
E) 8

Question 6

What is the difference in wavelength between the longest wavelength in the Lyman series and that of the longest wavelength in the Paschen series?

Accepted Answer

A) 1754 nm 
B) 1876 nm 
C) 535 nm 
D) 1220 nm 
E) None of these is correct. 
A) 1754 nm 
B) 1876 nm 
C) 535 nm 
D) 1220 nm 
E) None of these is correct.

Question 7

A photon of wavelength 80 nm is absorbed by the electron in the ground-state level of the hydrogen atom.Is this enough energy to ionize the atom? If so calculate the kinetic energy of the free electron.

Accepted Answer

A) No,ionization does not occur. 
B) Yes,1.9 eV 
C) Yes,12 eV 
D) Yes,29 eV 
E) Yes,19 eV 
A) No,ionization does not occur. 
B) Yes,1.9 eV 
C) Yes,12 eV 
D) Yes,29 eV 
E) Yes,19 eV

Question 8

Z for the element whose electronic configuration is   must be

Accepted Answer

A) 11 
B) 14 
C) 17 
D) 21 
E) 25 
A) 11 
B) 14 
C) 17 
D) 21 
E) 25

Question 9

The energy of the nth level in a one-electron atom is En = -13.6(Z2/n2)eV.Consider a beryllium ion with all but one of its electrons removed (a beryllium atom normally has four electrons).What is the energy of the electron when it is in the third-lowest energy state?

Accepted Answer

A) -24 eV 
B) -7.6 eV 
C) -1.5 eV 
D) 24 eV 
E) 7.6 eV 
A) -24 eV 
B) -7.6 eV 
C) -1.5 eV 
D) 24 eV 
E) 7.6 eV

Question 10

The orbital angular momentum L is related to the orbital quantum number   by

Accepted Answer

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

Question 11

The constant in the Rydberg-Ritz formula is RH = 10.96776 µm-1.The wavelength predicted by this formula for n1 = 3 and n2 = 2 is

Accepted Answer

A) 656 nm 
B) 486 nm 
C) 434 nm 
D) 410 nm 
E) None of these is correct. 
A) 656 nm 
B) 486 nm 
C) 434 nm 
D) 410 nm 
E) None of these is correct.

Question 12

Use the following figure for the next problem.  
-What is the longest wavelength needed for an electron to make the transition labeled (f)?

Accepted Answer

A) 151 nm 
B) 365 nm 
C) 422 nm 
D) 821 nm 
E) 1459 nm 
A) 151 nm 
B) 365 nm 
C) 422 nm 
D) 821 nm 
E) 1459 nm

Question 13

The wavelength of the photon emitted when a hydrogen atom undergoes a transition from the n = 10 state to the n = 1 state is approximately

Accepted Answer

A) 0.920 $\times$ 10-6 nm 
B) 1.085 $\times$ 10-4 nm 
C) 92.0 nm 
D) 0.0900 nm 
E) 46.5 nm 
A) 0.920 $\times$ 10-6 nm 
B) 1.085 $\times$ 10-4 nm 
C) 92.0 nm 
D) 0.0900 nm 
E) 46.5 nm

Exam 36: Atoms

In the Bohr model of the atom

An electron in a hydrogen atom jumps from the n = 5 to n = 3 level.Is a photon absorbed or emitted in this process? What is the wavelength of the photon? State whether the photon is in the visible,ultraviolet,or infrared range of the electro-magnetic spectrum.

Use the following figure for the next problem. -Which of the following transitions from (a)to (e)is(are)not allowed?

The equation derived by Bohr for the wavelengths of λ\lambdaλ of the lines in hydrogen- like spectra is The first member of the Balmer series of hydrogen has λ\lambdaλ = 660 nm.Doubly ionized is hydrogen-like.The wavelength of the first member of the Balmer series for doubly ionized is

The number of oxygen's eight electrons that are found in the p state is

What is the difference in wavelength between the longest wavelength in the Lyman series and that of the longest wavelength in the Paschen series?

A photon of wavelength 80 nm is absorbed by the electron in the ground-state level of the hydrogen atom.Is this enough energy to ionize the atom? If so calculate the kinetic energy of the free electron.

Z for the element whose electronic configuration is must be

The energy of the nth level in a one-electron atom is En = -13.6(Z2/n2)eV.Consider a beryllium ion with all but one of its electrons removed (a beryllium atom normally has four electrons).What is the energy of the electron when it is in the third-lowest energy state?

The orbital angular momentum L is related to the orbital quantum number by

The constant in the Rydberg-Ritz formula is RH = 10.96776 µm-1.The wavelength predicted by this formula for n1 = 3 and n2 = 2 is

Use the following figure for the next problem. -What is the longest wavelength needed for an electron to make the transition labeled (f)?

The wavelength of the photon emitted when a hydrogen atom undergoes a transition from the n = 10 state to the n = 1 state is approximately

Systems of Measurement

Motion in One Dimension

Motion in Two and Three Dimensions

Newtons Laws

Applications of Newtons Laws

Work and Energy

Conservation of Energy

Systems of Particles and Conservation of Linear Momentum

Rotation

Conservation of Angular Momentum

Gravity

Static Equilibrium and Elasticity

Fluids

Oscillations

Wave Motion

Superposition and Standing Waves

Temperature and the Kinetic Theory of Gases

Heat and the First Law of Thermodynamics

The Second Law of Thermodynamics

Thermal Properties and Processes

The Electric Field I: Discrete Charge Distributions

The Electric Field Ii: Continuous Charge Distributions

Electric Potential

Capacitance

Electric Current and Direct-Current Circuits

The Magnetic Field

Sources of the Magnetic Field

Magnetic Induction

Alternating-Current Circuits

Maxwells Equations and Electromagnetic Waves

Properties of Light

Optical Images

Interference and Diffraction

Wave Particle Duality and Quantum Physics

Applications of the Schrodinger Equation

Molecules

Solids and the Theory of Conduction

Relativity

Nuclear Physics

Elementary Particles and the Beginning of the Universe

Filters

The energy of the nth level in a one-electron atom is E_n = -13.6(Z²/n²)eV.Consider a beryllium ion with all but one of its electrons removed (a beryllium atom normally has four electrons).What is the energy of the electron when it is in the third-lowest energy state?

The constant in the Rydberg-Ritz formula is R_H = 10.96776 µm^-1.The wavelength predicted by this formula for n₁ = 3 and n₂ = 2 is