Question 1

Which set of quantum numbers could be correct for the highest energy electron in tin, Sn?

Accepted Answer

A) n = 4, $ l $ = 1, ml = -1, ms = -½ 
B) n = 4, $ l $ = 0, ml = 0, ms = +½ 
C) n = 5, $ l $ = 1, ml = 0, ms = -½ 
D) n = 5, $ l $ = 2, ml = 0, ms = +½ 
E) n = 5, $ l $= 0, ml = 0, ms = -½ 
A) n = 4, $ l $ = 1, ml = -1, ms = -½ 
B) n = 4, $ l $ = 0, ml = 0, ms = +½ 
C) n = 5, $ l $ = 1, ml = 0, ms = -½ 
D) n = 5, $ l $ = 2, ml = 0, ms = +½ 
E) n = 5, $ l $= 0, ml = 0, ms = -½

Question 2

Arrange the following elements in order of increasing first ionization energy: 13Al, 56Ba, 49In, 15P, 18Ar.

Accepted Answer

The answer of Arrange the following elements in order of...

Question 3

Which of the following metals would be an appropriate choice for the construction of a photon detector for 550 nm light?

Accepted Answer

A) sodium ($\varPhi$ = 2.9 *10-19 J) 
B) rubidium ($\varPhi$ = 3.5 *10-19 J) 
C) barium ($\varPhi$ = 4.3 *10-19 J) 
D) gold ($\varPhi$ = 8.2 *10-19 J) 
E) platinum ($\varPhi$ = 9.1 *10-19 J) 
A) sodium ($\varPhi$ = 2.9 *10-19 J) 
B) rubidium ($\varPhi$ = 3.5 *10-19 J) 
C) barium ($\varPhi$ = 4.3 *10-19 J) 
D) gold ($\varPhi$ = 8.2 *10-19 J) 
E) platinum ($\varPhi$ = 9.1 *10-19 J)

Question 4

Which of the following is the correct condensed electron configuration for germanium Ge)?

Accepted Answer

A) [Ar]4s23d 104p2 
B) [Ar]4s23d 84p3 
C) [Ar]3d104p2 
D) [Ar]4s23d 54p6 
E) [Ar]4s13d104p2 
A) [Ar]4s23d 104p2 
B) [Ar]4s23d 84p3 
C) [Ar]3d104p2 
D) [Ar]4s23d 54p6 
E) [Ar]4s13d104p2

Question 5

Which statement below regarding ionization energy is FALSE?

Accepted Answer

A) Ionization energy is the energy required to remove a mole of electrons from a mole of gas-phase atoms or ions. 
B) The ionization energy increases as Zeff increases. 
C) Anomalies in ionization energy trends can occur due to electron pairing in orbitals. 
D) Atoms in the same column of the periodic table have equal ionization energies. 
E) Ionization energies are always positive because it takes energy to pull the negative electron away from the positive nucleus. 
A) Ionization energy is the energy required to remove a mole of electrons from a mole of gas-phase atoms or ions. 
B) The ionization energy increases as Zeff increases. 
C) Anomalies in ionization energy trends can occur due to electron pairing in orbitals. 
D) Atoms in the same column of the periodic table have equal ionization energies. 
E) Ionization energies are always positive because it takes energy to pull the negative electron away from the positive nucleus.

Question 6

Which of the following is the correct condensed electron configuration for tellurium?

Accepted Answer

A) [Ar]5s24d105p4 
B) [Kr]5s24d104p4 
C) [Kr]4d105p5 
D) [Ar]4s23d104p4 
E) [Kr]5s24d105p4 
A) [Ar]5s24d105p4 
B) [Kr]5s24d104p4 
C) [Kr]4d105p5 
D) [Ar]4s23d104p4 
E) [Kr]5s24d105p4

Question 7

Suppose a blue light emitting photons with λ = 470 nm is rated at 100 W (100 J of energy are emitted per second).How many photons are emitted in 5.0 seconds?

Accepted Answer

A) 7.0 *1019 photons 
B) 1.2 * 1021 photons 
C) 2.3 * 1020 photons 
D) 3.5 * 1038 photons 
E) 2.7* 109 photons 
A) 7.0 *1019 photons 
B) 1.2 * 1021 photons 
C) 2.3 * 1020 photons 
D) 3.5 * 1038 photons 
E) 2.7* 109 photons

Question 8

Which of the following types of electromagnetic radiation has the lowest frequency?

Accepted Answer

A) gamma rays 
B) x-rays 
C) radio waves 
D) infrared 
E) visible 
A) gamma rays 
B) x-rays 
C) radio waves 
D) infrared 
E) visible

Question 9

Calculate the wavelengths in nanometers corresponding to the three lowest energy transitions in the Balmer series of the hydrogen emission spectrum.What are the ninitial values associated with each?

Accepted Answer

656.2 nm,

Question 10

The first eight successive ionization energies IE1, IE2, …) for Al are 578; 1817; 2745; 11,577; 14,842; 18,379; 23,326; and 27,465 kJ/mol.What is the probable explanation for the large jump in energy observed between IE3 and IE4?

Accepted Answer

A) Zeff decreases as electrons are removed. 
B) Electrons in ns and np orbitals are equal in energy. 
C) IE4 reflects that inner-shell electrons with a lower n value are starting to be removed. 
D) Aluminum cannot lose four electrons, so IE4 is meaningless. 
E) Electrons with higher angular momentum are harder to remove. 
A) Zeff decreases as electrons are removed. 
B) Electrons in ns and np orbitals are equal in energy. 
C) IE4 reflects that inner-shell electrons with a lower n value are starting to be removed. 
D) Aluminum cannot lose four electrons, so IE4 is meaningless. 
E) Electrons with higher angular momentum are harder to remove.

Question 11

Which of the following states that each electron in an atom must have a unique set of four quantum numbers?

Accepted Answer

A) Hund's rule 
B) the Pauli exclusion principle 
C) the aufbau principle 
D) the Rydberg equation 
E) the Heisenberg uncertainty principle 
A) Hund's rule 
B) the Pauli exclusion principle 
C) the aufbau principle 
D) the Rydberg equation 
E) the Heisenberg uncertainty principle

Question 12

You think you have identified a new type of atom based on its atomic emission spectrum.Based on empirical data, it appears as though the energy levels of the atom are inversely proportional to N2, like hydrogen.When an electron falls from ninitial = 5 to nfinal = 2, a 1.4 *10-18 J photon is emitted.What is the value of the Rydberg constant for this atom?

Accepted Answer

A) 6.7 * 10-18 J 
B) 4.7* 10-18 J 
C) 4.2* 10-18 J 
D) 1.5 * 1017 J 
E) 2.1 * 1017 J 
A) 6.7 * 10-18 J 
B) 4.7* 10-18 J 
C) 4.2* 10-18 J 
D) 1.5 * 1017 J 
E) 2.1 * 1017 J

Question 13

Which of the following lasers emits photons with the highest frequency?

Accepted Answer

A) a Nd:YAG laser with $\lambda$ = 1064 nm 
B) an Ar+ laser with $\lambda$ = 514.5 nm 
C) a Kr+ laser with $\lambda$= 647 nm 
D) an ArF laser with $\lambda$ = 193 nm 
E) a HeNe laser with $\lambda$ = 633 nm 
A) a Nd:YAG laser with $\lambda$ = 1064 nm 
B) an Ar+ laser with $\lambda$ = 514.5 nm 
C) a Kr+ laser with $\lambda$= 647 nm 
D) an ArF laser with $\lambda$ = 193 nm 
E) a HeNe laser with $\lambda$ = 633 nm

Question 14

What is the change in energy of the hydrogen atom when it undergoes an electronic transition from ninitial = 5 to nfinal = 2?

Accepted Answer

A) 2.09 * 10-18 J 
B) 4.57 * 10-19 J 
C) 1.55 * 10-19 J 
D) 4.90 *10-20 J 
E) 1.55* 10-20 J 
A) 2.09 * 10-18 J 
B) 4.57 * 10-19 J 
C) 1.55 * 10-19 J 
D) 4.90 *10-20 J 
E) 1.55* 10-20 J

Question 15

Which of the following statements is NOT true regarding blackbody radiation, the ultraviolet catastrophe, and Planck's view of electromagnetic radiation?

Accepted Answer

A) A blackbody radiator does not absorb and emit one wavelength preferentially over another. 
B) The emission spectrum of a blackbody radiator depends on its temperature. 
C) A blackbody radiator cannot emit an infinite amount of radiation. 
D) Planck theorized that real objects can only absorb or emit discrete packets of electromagnetic radiation. 
E) The ultraviolet catastrophe disappears if the emission spectrum of a blackbody radiator is continuous. 
A) A blackbody radiator does not absorb and emit one wavelength preferentially over another. 
B) The emission spectrum of a blackbody radiator depends on its temperature. 
C) A blackbody radiator cannot emit an infinite amount of radiation. 
D) Planck theorized that real objects can only absorb or emit discrete packets of electromagnetic radiation. 
E) The ultraviolet catastrophe disappears if the emission spectrum of a blackbody radiator is continuous.

Question 16

Which element is likely to have the ground-state electron configuration [Kr]5s14d10?

Accepted Answer

A) Au 
B) Cu 
C) In 
D) Ag 
E) Cd 
A) Au 
B) Cu 
C) In 
D) Ag 
E) Cd

Question 17

Which combination of quantum numbers would be allowed for one subshell containing five orbitals?

Accepted Answer

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

Question 18

What is the approximate uncertainty in the position of a proton 1.673 * 10-27 kg) in a particle accelerator if its velocity is known to about $\pm$2.5 m/s (total uncertainty is 5.0 m/s)?

Accepted Answer

A) ($\pm$6.4 *10-9 m) 
B) ($\pm$3.2 *10-9 m) 
C) ($\pm$1.3 *10-9 m) 
D) ($\pm$3.2 *10-8 m) 
E) ($\pm$6.4 *1-10 m) 
A) ($\pm$6.4 *10-9 m) 
B) ($\pm$3.2 *10-9 m) 
C) ($\pm$1.3 *10-9 m) 
D) ($\pm$3.2 *10-8 m) 
E) ($\pm$6.4 *1-10 m)

Question 19

What is the frequency ($\nu$ in hertz) of the photons emitted by a HeNe laser with a wavelength ($\lambda$) of 632.8 nm?

Accepted Answer

A) 4.738 * 105 Hz 
B) 1.897 * 102 Hz 
C) 1.897 * 1011 Hz 
D) 4.738 *1014 Hz 
E) 1.897 *1014 Hz 
A) 4.738 * 105 Hz 
B) 1.897 * 102 Hz 
C) 1.897 * 1011 Hz 
D) 4.738 *1014 Hz 
E) 1.897 *1014 Hz

Question 20

Which statement about electromagnetic radiation is NOT correct?

Accepted Answer

A) Electromagnetic radiation consists of perpendicular oscillating electric and magnetic fields. 
B) Electromagnetic radiation is emitted by all stars. 
C) All electromagnetic radiation is visible to the eye. 
D) Electromagnetic radiation spans a very wide range of wavelengths, from gamma rays to radio waves. 
E) The frequency and wavelength of electromagnetic radiation are inversely proportional to each other. 
A) Electromagnetic radiation consists of perpendicular oscillating electric and magnetic fields. 
B) Electromagnetic radiation is emitted by all stars. 
C) All electromagnetic radiation is visible to the eye. 
D) Electromagnetic radiation spans a very wide range of wavelengths, from gamma rays to radio waves. 
E) The frequency and wavelength of electromagnetic radiation are inversely proportional to each other.

Exam 3: Atomic Structure Explaining the Properties of Elements

Which set of quantum numbers could be correct for the highest energy electron in tin, Sn?

Arrange the following elements in order of increasing first ionization energy: 13Al, 56Ba, 49In, 15P, 18Ar.

Which of the following metals would be an appropriate choice for the construction of a photon detector for 550 nm light?

Which of the following is the correct condensed electron configuration for germanium Ge)?

Which statement below regarding ionization energy is FALSE?

Which of the following is the correct condensed electron configuration for tellurium?

Suppose a blue light emitting photons with λ = 470 nm is rated at 100 W (100 J of energy are emitted per second).How many photons are emitted in 5.0 seconds?

Which of the following types of electromagnetic radiation has the lowest frequency?

Calculate the wavelengths in nanometers corresponding to the three lowest energy transitions in the Balmer series of the hydrogen emission spectrum.What are the ninitial values associated with each?

The first eight successive ionization energies IE1, IE2, …) for Al are 578; 1817; 2745; 11,577; 14,842; 18,379; 23,326; and 27,465 kJ/mol.What is the probable explanation for the large jump in energy observed between IE3 and IE4?

Which of the following states that each electron in an atom must have a unique set of four quantum numbers?

Which of the following lasers emits photons with the highest frequency?

What is the change in energy of the hydrogen atom when it undergoes an electronic transition from ninitial = 5 to nfinal = 2?

Which of the following statements is NOT true regarding blackbody radiation, the ultraviolet catastrophe, and Planck's view of electromagnetic radiation?

Which element is likely to have the ground-state electron configuration [Kr]5s14d10?

Which combination of quantum numbers would be allowed for one subshell containing five orbitals?

What is the approximate uncertainty in the position of a proton 1.673 * 10-27 kg) in a particle accelerator if its velocity is known to about ±\pm± 2.5 m/s (total uncertainty is 5.0 m/s)?

What is the frequency ( ν\nuν in hertz) of the photons emitted by a HeNe laser with a wavelength ( λ\lambdaλ ) of 632.8 nm?

Which statement about electromagnetic radiation is NOT correct?

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

Arrange the following elements in order of increasing first ionization energy: ₁₃Al, ₅₆Ba, ₄₉In, ₁₅P, ₁₈Ar.

Calculate the wavelengths in nanometers corresponding to the three lowest energy transitions in the Balmer series of the hydrogen emission spectrum.What are the n_initial values associated with each?

The first eight successive ionization energies IE₁, IE₂, …) for Al are 578; 1817; 2745; 11,577; 14,842; 18,379; 23,326; and 27,465 kJ/mol.What is the probable explanation for the large jump in energy observed between IE₃ and IE₄?

What is the change in energy of the hydrogen atom when it undergoes an electronic transition from n_initial= 5 to n_final= 2?

Which element is likely to have the ground-state electron configuration [Kr]5s¹4d¹⁰?

What is the approximate uncertainty in the position of a proton 1.673 * 10^-27 kg) in a particle accelerator if its velocity is known to about $\pm$ 2.5 m/s (total uncertainty is 5.0 m/s)?

What is the frequency ( $\nu$ in hertz) of the photons emitted by a HeNe laser with a wavelength ( $\lambda$ ) of 632.8 nm?