Question 1

Which of the following objects, all moving at the same speed, will have the largest de Broglie wavelength?

Accepted Answer

A) a proton 
B) an electron 
C) a bowling ball 
D) a neon atom 
E) a neutron 
A) a proton 
B) an electron 
C) a bowling ball 
D) a neon atom 
E) a neutron

Question 2

Indicate which of the following photons can cause emission of photoelectrons from a surface of gallium (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 6.7   F1F1F1S1F1F1F10J).

Accepted Answer

A) 350 nm 
B) 400 nm 
C) 200 nm 
D) 650 nm 
E) 500 nm 
A) 350 nm 
B) 400 nm 
C) 200 nm 
D) 650 nm 
E) 500 nm

Question 3

Which of the following elements would you expect to have the lowest first ionization energy?

Accepted Answer

A) F 
B) Br 
C) Cl 
D) I 
E) Xe 
A) F 
B) Br 
C) Cl 
D) I 
E) Xe

Question 4

How many orbitals are possible for the n F1F1F1S1F1F1F10 2 shell?

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 5 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5

Question 5

`If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector?
(1 eV   F1F1F1S1F1F1F101.60   F1F1F1S1F1F1F10J)

Accepted Answer

3.2 @#IMG-DLM& F1F1F

Question 6

Which of the following atoms has no unpaired electrons?

Accepted Answer

A) B 
B) C 
C) O 
D) Mg 
E) Na 
A) B 
B) C 
C) O 
D) Mg 
E) Na

Question 7

What is the kinetic energy of the photoelectrons emitted from a sodium surface (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10   F1F1F1S1F1F1F10J) when it is irradiated by photons with a wavelength of 350 nm?

Accepted Answer

A) 2.9   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
B) 5.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
C) 0 J 
D) 2.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
E) 3.6   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
A) 2.9   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
B) 5.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
C) 0 J 
D) 2.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J 
E) 3.6   F1F1F1S1F1F1F1010F1F1F1S1F1F1F1019 J

Question 8

Which of the transitions in the hydrogen atom energy-level diagram shown here is not possible?

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 9

What is the minimum energy that a photon must have to ionize a hydrogen atom from the n F1F1F1S1F1F1F10 3 energy level?

Accepted Answer

2.4 @#IMG-DLM& F1F1F

Question 10

What is the energy (E, in J) of the photons emitted by an ArF1F1F1S1F1F1F10 laser with a wavelength of F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 488 nm?

Accepted Answer

A) 2.46   F1F1F1S1F1F1F10J 
B) 9.69   F1F1F1S1F1F1F10J 
C) 1.36   F1F1F1S1F1F1F10J 
D) 4.07   F1F1F1S1F1F1F10J 
E) 2.46   F1F1F1S1F1F1F10J 
A) 2.46   F1F1F1S1F1F1F10J 
B) 9.69   F1F1F1S1F1F1F10J 
C) 1.36   F1F1F1S1F1F1F10J 
D) 4.07   F1F1F1S1F1F1F10J 
E) 2.46   F1F1F1S1F1F1F10J

Question 11

A certain shell is known to have a total of 16 orbitals. Which shell is it?

Accepted Answer

A) n   F1F1F1S1F1F1F104 
B) n   F1F1F1S1F1F1F1016 
C) n   F1F1F1S1F1F1F108 
D) n   F1F1F1S1F1F1F102 
A) n   F1F1F1S1F1F1F104 
B) n   F1F1F1S1F1F1F1016 
C) n   F1F1F1S1F1F1F108 
D) n   F1F1F1S1F1F1F102

Question 12

Across a row in the periodic table, the ionization energy ________

Accepted Answer

A) increases because the n quantum number changes. 
B) increases because the   quantum number changes. 
C) decreases because the effective nuclear charge decreases. 
D) increases because the effective nuclear charge increases. 
E) changes little because the outer electrons are all in the same shell. 
A) increases because the n quantum number changes. 
B) increases because the   quantum number changes. 
C) decreases because the effective nuclear charge decreases. 
D) increases because the effective nuclear charge increases. 
E) changes little because the outer electrons are all in the same shell.

Question 13

In quantum mechanics, an atomic orbital ________

Accepted Answer

A) provides the position of an electron at any instant of time in the space around an atomic nucleus. 
B) locates all the electrons in an atom. 
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom. 
D) identifies the most probable position of an atomic nucleus. 
E) provides the probability of finding an electron at any point in the space around an atomic nucleus. 
A) provides the position of an electron at any instant of time in the space around an atomic nucleus. 
B) locates all the electrons in an atom. 
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom. 
D) identifies the most probable position of an atomic nucleus. 
E) provides the probability of finding an electron at any point in the space around an atomic nucleus.

Question 14

Which of the following is the ground-state electron configuration of the Mg2F1F1F1S1F1F1F10 ion?

Accepted Answer

A) 1s22s22p63s2 
B) [Ne]3s2 
C) [Ne]3s23p2 
D) [He]2s22p6 
E) [He]2s22p8 
A) 1s22s22p63s2 
B) [Ne]3s2 
C) [Ne]3s23p2 
D) [He]2s22p6 
E) [He]2s22p8

Question 15

Which arrangement is in the correct order of decreasing radii?

Accepted Answer

A) As3F1F1F1S1F1F1F10   F1F1F1S1F1F1F10Br F1F1F1S1F1F1F10   F1F1F1S1F1F1F10KF1F1F1S1F1F1F10 
B) FF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 MgF1F1F1S1F1F1F10   F1F1F1S1F1F1F10Cs 
C) NaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10CsF1F1F1S1F1F1F10   F1F1F1S1F1F1F10IF1F1F1S1F1F1F10 
D) Be   F1F1F1S1F1F1F10BaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10O2F1F1F1S1F1F1F10 
E) LiF1F1F1S1F1F1F10   F1F1F1S1F1F1F10NaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10KF1F1F1S1F1F1F10 
A) As3F1F1F1S1F1F1F10   F1F1F1S1F1F1F10Br F1F1F1S1F1F1F10   F1F1F1S1F1F1F10KF1F1F1S1F1F1F10 
B) FF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 MgF1F1F1S1F1F1F10   F1F1F1S1F1F1F10Cs 
C) NaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10CsF1F1F1S1F1F1F10   F1F1F1S1F1F1F10IF1F1F1S1F1F1F10 
D) Be   F1F1F1S1F1F1F10BaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10O2F1F1F1S1F1F1F10 
E) LiF1F1F1S1F1F1F10   F1F1F1S1F1F1F10NaF1F1F1S1F1F1F10   F1F1F1S1F1F1F10KF1F1F1S1F1F1F10

Question 16

Which one of the following diagrams represents the electron configuration of a carbon atom?

Accepted Answer

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

Question 17

According to de Broglie, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will ________

Accepted Answer

A) decay until the electron falls into the nucleus. 
B) diverge, allowing the electron to escape. 
C) be stable. 
D) cause the electron to emit a photon. 
E) not be circular. 
A) decay until the electron falls into the nucleus. 
B) diverge, allowing the electron to escape. 
C) be stable. 
D) cause the electron to emit a photon. 
E) not be circular.

Question 18

Which of the following sources produces the lowest energy photons?

Accepted Answer

A) a dentist's X-ray source 
B) the UV lamp at a tanning bed 
C) radio waves from an MRI imager 
D) gamma rays from a supernova 
E) microwave radiation from a radiotelescope 
A) a dentist's X-ray source 
B) the UV lamp at a tanning bed 
C) radio waves from an MRI imager 
D) gamma rays from a supernova 
E) microwave radiation from a radiotelescope

Question 19

Arrange the following elements in order of increasing electron affinity: Li, O, Ne, Cl.

Accepted Answer

Ne @#IMG-DLM& F1F1F1S1F1F1F10L

Question 20

The study of light emitted by the hydrogen atom by Johann Balmer, Johannes Rydberg, Niels Bohr, and others revolutionized physics because it revealed that ________

Accepted Answer

A) energy is quantized. 
B) light intensity does not affect the number of atoms excited. 
C) the emitted light is produced by the electron making a transition between quantized energy levels. 
D) blackbody radiation is continuous. 
E) atomic spectra are continuous. 
A) energy is quantized. 
B) light intensity does not affect the number of atoms excited. 
C) the emitted light is produced by the electron making a transition between quantized energy levels. 
D) blackbody radiation is continuous. 
E) atomic spectra are continuous.

Exam 7: A Quantum Model of Atoms: Waves and Particles

Which of the following objects, all moving at the same speed, will have the largest de Broglie wavelength?

Indicate which of the following photons can cause emission of photoelectrons from a surface of gallium (  6.7 J).

Which of the following elements would you expect to have the lowest first ionization energy?

How many orbitals are possible for the n  2 shell?

`If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector? (1 eV 1.60 J)

Which of the following atoms has no unpaired electrons?

What is the kinetic energy of the photoelectrons emitted from a sodium surface (  J) when it is irradiated by photons with a wavelength of 350 nm?

Which of the transitions in the hydrogen atom energy-level diagram shown here is not possible?

What is the minimum energy that a photon must have to ionize a hydrogen atom from the n  3 energy level?

What is the energy (E, in J) of the photons emitted by an Ar laser with a wavelength of   488 nm?

A certain shell is known to have a total of 16 orbitals. Which shell is it?

Across a row in the periodic table, the ionization energy ________

In quantum mechanics, an atomic orbital ________

Which of the following is the ground-state electron configuration of the Mg2 ion?

Which arrangement is in the correct order of decreasing radii?

Which one of the following diagrams represents the electron configuration of a carbon atom?

According to de Broglie, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will ________

Which of the following sources produces the lowest energy photons?

Arrange the following elements in order of increasing electron affinity: Li, O, Ne, Cl.

The study of light emitted by the hydrogen atom by Johann Balmer, Johannes Rydberg, Niels Bohr, and others revolutionized physics because it revealed that ________

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

What is the energy (E, in J) of the photons emitted by an Ar^ laser with a wavelength of   488 nm?

Which of the following is the ground-state electron configuration of the Mg²^ ion?