Question 1

Which of the following statements regarding the energy of a particle is NOT correct?

Accepted Answer

A) The ground state of a particle is the lowest and most stable energy state. 
B) The energy of a particle is zero when it is in its ground state. 
C) An excited state is any energy state above the ground state. 
D) When the particle undergoes a transition from a higher energy state to a lower one, energy is emitted. 
E) The energy state of a particle increases when it absorbs a photon. 
A) The ground state of a particle is the lowest and most stable energy state. 
B) The energy of a particle is zero when it is in its ground state. 
C) An excited state is any energy state above the ground state. 
D) When the particle undergoes a transition from a higher energy state to a lower one, energy is emitted. 
E) The energy state of a particle increases when it absorbs a photon.

Question 2

Work function values are often given in electron volts (1 eV = 1.602 * 10-19 J).You create an oxide material that has a work function of 6.10 eV.How many electrons would be emitted from the material per second when it is irradiated by the 172 nm light of a 55.0 W xenon excimer lamp, and what is their kinetic energy? Assume all of the incident photons cause electron emission.

Accepted Answer

A) none; 172 nm is not energetic enough 
B) 8.70 * 1017 electrons; 8.70 * 10-19 J 
C) 4.78 *1019 electrons; 1.73 -10-19 J 
D) 5.5 *1017 electrons; 5.40 *10-17 J 
E) 1.86*1016 electrons; 5.37 *10-17 J 
A) none; 172 nm is not energetic enough 
B) 8.70 * 1017 electrons; 8.70 * 10-19 J 
C) 4.78 *1019 electrons; 1.73 -10-19 J 
D) 5.5 *1017 electrons; 5.40 *10-17 J 
E) 1.86*1016 electrons; 5.37 *10-17 J

Question 3

How many electrons can be in the n = 4 shell of an atom? Include all orbitals that have (n = 4.)

Accepted Answer

The answer of How many electrons can be in the...

Question 4

The energy change for an electronic transition in a one-electron atom or ion H, He+, Li2+, etc.) from n initial to n final  Is given by $ \left(-2.178 \times 10^{-18} \mathrm{~J}\right) Z^{2}\left(\frac{1}{n_{\text {final }} 2}-\frac{1}{n_{\text {initial }} 2}\right) $ where Z is the atomic number.How much energy is required to ionize a ground-state Li2+ion (nfinal =$\infty$)?

Accepted Answer

A) 2.18 *10-18 J 
B) 4.36 * 10-18 J 
C) 1.96 * 10-17 J 
D) 1.09 *10-18 J 
E) 5.45 * 10-19 J 
A) 2.18 *10-18 J 
B) 4.36 * 10-18 J 
C) 1.96 * 10-17 J 
D) 1.09 *10-18 J 
E) 5.45 * 10-19 J

Question 5

Which arrangement is correct for increasing atomic radius?

Accepted Answer

A) C $\lt$ N $\lt$ F 
B) Rb $\lt$ K $\lt$ Li 
C) Sc $\lt$ Ge $\lt$ Br 
D) Se $\lt$ Cu $\lt$ Ca 
E) H $\lt$ He 
A) C $\lt$ N $\lt$ F 
B) Rb $\lt$ K $\lt$ Li 
C) Sc $\lt$ Ge $\lt$ Br 
D) Se $\lt$ Cu $\lt$ Ca 
E) H $\lt$ He

Question 6

The work function of sodium is $\varPhi$ = 2.90 *10-19 J.What is the maximum wavelength that can cause the ejection of photoelectrons from a sodium surface?

Accepted Answer

A) 151 nm 
B) 222 nm 
C) 45.1 nm 
D) 451 nm 
E) 685 nm 
A) 151 nm 
B) 222 nm 
C) 45.1 nm 
D) 451 nm 
E) 685 nm

Question 7

The mathematical description of an electron as a wave was developed by _______.

Accepted Answer

A) Bohr. 
B) Heisenberg. 
C) Einstein. 
D) de Broglie. 
E) Schrödinger. 
A) Bohr. 
B) Heisenberg. 
C) Einstein. 
D) de Broglie. 
E) Schrödinger.

Question 8

What is the approximate total uncertainty in the velocity of an electron (9.11 *10-31 kg) confined within a gold atom whose diameter is about 270 pm? The uncertainty in the position of the electron is $\pm$5.0% of the atom's diameter.

Accepted Answer

A) ($\pm$1.4 *103 m/s) 
B) ($\pm$2.1 * 105 m/s) 
C) ($\pm$3.7 * 105 m/s) 
D) ($\pm$2.1 * 106 m/s) 
E) ($\pm$4.3 * 106 m/s) 
A) ($\pm$1.4 *103 m/s) 
B) ($\pm$2.1 * 105 m/s) 
C) ($\pm$3.7 * 105 m/s) 
D) ($\pm$2.1 * 106 m/s) 
E) ($\pm$4.3 * 106 m/s)

Question 9

What is the speed of an average argon atom that has a de Broglie wavelength of 5.2 pm? 
(1 amu = 1.66054 *10-27 kg.)

Accepted Answer

A) 0.52 m/s 
B) 5.2 * 103 m/s 
C) 1.9 * 103 m/s 
D) 1.9 m/s 
E) 25 m/s 
A) 0.52 m/s 
B) 5.2 * 103 m/s 
C) 1.9 * 103 m/s 
D) 1.9 m/s 
E) 25 m/s

Question 10

Radiation with a wavelength of _______ nm is produced by the n = 4 to n = 2 transition in the hydrogen atom; this transition occurs in the _______ region of the electromagnetic spectrum.

Accepted Answer

486, visib

Question 11

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 
E) all are possible 
A) a 
B) b 
C) c 
D) d 
E) all are possible

Question 12

What is the difference in energy between the two electronic levels in hydrogen that are responsible for the emission line observed at 1282 nm, and to which series does this line belong?

Accepted Answer

A) 1.55 * 10-19 J, Balmer 
B) 1.05 * 10-19 J, Paschen 
C) 1.55 * 10-19 J, Paschen 
D) 1.82 *10-19 J, Balmer 
E) 1.82 *10-19 J, Lyman 
A) 1.55 * 10-19 J, Balmer 
B) 1.05 * 10-19 J, Paschen 
C) 1.55 * 10-19 J, Paschen 
D) 1.82 *10-19 J, Balmer 
E) 1.82 *10-19 J, Lyman

Question 13

What is the de Broglie wavelength of a fast neutron (1.6749 * 10-27 kg) traveling at 14,000 km/s?

Accepted Answer

A) 53 fm 
B) 5.3 pm 
C) 28 pm 
D) 28 fm 
E) 25 m/s 
A) 53 fm 
B) 5.3 pm 
C) 28 pm 
D) 28 fm 
E) 25 m/s

Question 14

Which subshell has only five orbitals?

Accepted Answer

A) $ l $= 2 
B) $ l $= 1 
C) $ l $ = 5 
D) $ l $ = 3 
E) $ l $= 4 
A) $ l $= 2 
B) $ l $= 1 
C) $ l $ = 5 
D) $ l $ = 3 
E) $ l $= 4

Question 15

Suppose a laser emits light in the visible region of the spectrum at 4.62 * 1014 s-1.What color is the light?

Accepted Answer

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

Question 16

What is the uncertainty in the position of a helium atom traveling at 1360 m/s, approximately its speed at room temperature? The atom's velocity is known to about $\pm$1%.
(1 amu = 1.66054 * 10-27 kg.)

Accepted Answer

∆v = 2.92 *10<sup>-1

Question 17

Which of the following statements regarding degenerate orbitals is correct?

Accepted Answer

A) Orbitals sharing the same principal and angular momentum quantum numbers are degenerate. 
B) Orbitals sharing the same magnetic quantum number are degenerate. 
C) Electrons with the same value of n are equal in energy in all atoms. 
D) Orbitals sharing the same $ l $ value are degenerate. 
E) As the effective nuclear charge increases, all orbitals in a shell become equal in energy. 
A) Orbitals sharing the same principal and angular momentum quantum numbers are degenerate. 
B) Orbitals sharing the same magnetic quantum number are degenerate. 
C) Electrons with the same value of n are equal in energy in all atoms. 
D) Orbitals sharing the same $ l $ value are degenerate. 
E) As the effective nuclear charge increases, all orbitals in a shell become equal in energy.

Question 18

Which of the following atoms or ions has a single unpaired electron?

Accepted Answer

A) S2+ 
B) Sr 
C) Fe3+ 
D) Ba2+ 
E) Br 
A) S2+ 
B) Sr 
C) Fe3+ 
D) Ba2+ 
E) Br

Question 19

How much energy would be required to excite one mole of hydrogen atoms from their ground state to n2 = 10?

Accepted Answer

A) 1.3 * 103 J/mol 
B) 1.3 *106 J/mol 
C) 2.2 * 103 J/mol 
D) 2.2 *106 J/mol 
E) 9.2 * 102 J/mol 
A) 1.3 * 103 J/mol 
B) 1.3 *106 J/mol 
C) 2.2 * 103 J/mol 
D) 2.2 *106 J/mol 
E) 9.2 * 102 J/mol

Question 20

How many times longer is the wavelength of electromagnetic radiation used in a microwave oven at 2.45 GHz than the copper K-$\alpha$ 1 x-ray radiation used in x-ray diffraction studies with an energy of 1.29 *10-15 J?

Accepted Answer

A) 6.29 * 107 times longer 
B) 7.54 * 107 times longer 
C) 7.92 * 108 times longer 
D) 7.95 * 1017 times longer 
E) 1.90* 1024 times longer 
A) 6.29 * 107 times longer 
B) 7.54 * 107 times longer 
C) 7.92 * 108 times longer 
D) 7.95 * 1017 times longer 
E) 1.90* 1024 times longer

Exam 3: Atomic Structure Explaining the Properties of Elements

Which of the following statements regarding the energy of a particle is NOT correct?

How many electrons can be in the n = 4 shell of an atom? Include all orbitals that have (n = 4.)

Which arrangement is correct for increasing atomic radius?

The work function of sodium is Φ\varPhiΦ = 2.90 *10-19 J.What is the maximum wavelength that can cause the ejection of photoelectrons from a sodium surface?

The mathematical description of an electron as a wave was developed by _______.

What is the approximate total uncertainty in the velocity of an electron (9.11 *10-31 kg) confined within a gold atom whose diameter is about 270 pm? The uncertainty in the position of the electron is ±\pm± 5.0% of the atom's diameter.

What is the speed of an average argon atom that has a de Broglie wavelength of 5.2 pm? (1 amu = 1.66054 *10-27 kg.)

Radiation with a wavelength of _______ nm is produced by the n = 4 to n = 2 transition in the hydrogen atom; this transition occurs in the _______ region of the electromagnetic spectrum.

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

What is the difference in energy between the two electronic levels in hydrogen that are responsible for the emission line observed at 1282 nm, and to which series does this line belong?

What is the de Broglie wavelength of a fast neutron (1.6749 * 10-27 kg) traveling at 14,000 km/s?

Which subshell has only five orbitals?

Suppose a laser emits light in the visible region of the spectrum at 4.62 * 1014 s-1.What color is the light?

What is the uncertainty in the position of a helium atom traveling at 1360 m/s, approximately its speed at room temperature? The atom's velocity is known to about ±\pm± 1%. (1 amu = 1.66054 * 10-27 kg.)

Which of the following statements regarding degenerate orbitals is correct?

Which of the following atoms or ions has a single unpaired electron?

How much energy would be required to excite one mole of hydrogen atoms from their ground state to n2 = 10?

How many times longer is the wavelength of electromagnetic radiation used in a microwave oven at 2.45 GHz than the copper K- α\alphaα 1 x-ray radiation used in x-ray diffraction studies with an energy of 1.29 *10-15 J?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

The work function of sodium is $\varPhi$ = 2.90 *10^-19 J.What is the maximum wavelength that can cause the ejection of photoelectrons from a sodium surface?

What is the approximate total uncertainty in the velocity of an electron (9.11 *10^-31 kg) confined within a gold atom whose diameter is about 270 pm? The uncertainty in the position of the electron is $\pm$ 5.0% of the atom's diameter.

What is the speed of an average argon atom that has a de Broglie wavelength of 5.2 pm? (1 amu = 1.66054 *10^-27 kg.)

Radiation with a wavelength of _ nm is produced by the n = 4 to n = 2 transition in the hydrogen atom; this transition occurs in the _ region of the electromagnetic spectrum.

What is the de Broglie wavelength of a fast neutron (1.6749 * 10^-27 kg) traveling at 14,000 km/s?

Suppose a laser emits light in the visible region of the spectrum at 4.62 * 10¹⁴ s^-1.What color is the light?

What is the uncertainty in the position of a helium atom traveling at 1360 m/s, approximately its speed at room temperature? The atom's velocity is known to about $\pm$ 1%. (1 amu = 1.66054 * 10^-27 kg.)

How much energy would be required to excite one mole of hydrogen atoms from their ground state to n₂ = 10?

How many times longer is the wavelength of electromagnetic radiation used in a microwave oven at 2.45 GHz than the copper K- $\alpha$ 1 x-ray radiation used in x-ray diffraction studies with an energy of 1.29 *10^-15 J?