Question 1

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

Accepted Answer

First ionization energy generally decreases as you move down a group in the periodic table. Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), and Bismuth (Bi) are all in the same group, with Bismuth being the lowest. Therefore, Bismuth would have the lowest first ionization energy among the options given.

Question 2

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 10¹⁹ Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

Accepted Answer

The answer of The Swift explorer that NASA launched in...

Question 3

Astronomers have detected hydrogen atoms in interstellar space in the n = 732 energy level.Suppose an atom in this excited state emits a photon and undergoes a transition from n = 732 to n = 632.How much energy does the atom lose as a result of this transition? What is the frequency of this radiation? In which spectral region does this radiation lie?

Accepted Answer

The answer of Astronomers have detected hydrogen atoms in interstellar...

Question 4

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

The large jump in energy between the third and fourth ionization energies indicates that after removing the first three electrons (which are in the outermost shell), the fourth electron to be removed comes from a closer, more tightly bound inner shell, reflecting a significant increase in ionization energy.

Question 5

Electron affinity is the energy change that occurs _______.

Accepted Answer

The answer of Electron affinity is the energy change that...

Question 6

Which row 2 element probably has the following successive ionization energies:

Accepted Answer

The answer of Which row 2 element probably has the...

Question 7

De Broglie proposed that $\lambda$ = h/mv.Define the symbols in this equation and describe the significance of de Broglie's proposal.

Accepted Answer

The answer of De Broglie proposed that $\lambda$ = h/mv.Define...

Question 8

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10^-19 J.)

Accepted Answer

The answer of Cesium has a work function of 2.1...

Question 9

Which statement below regarding electron affinity is FALSE?

Accepted Answer

Electron affinity values are influenced by the effective nuclear charge (Z_eff), as it affects the attraction between the incoming electron and the nucleus. A higher Z_eff typically leads to a more negative electron affinity, indicating a stronger attraction to the electron.

Question 10

A mercury vapor lamp can be used as an 185 nm light source.What is the energy of one photon in joules? Of one mole of photons in kilojoules?

Accepted Answer

The answer of A mercury vapor lamp can be used...

Question 11

What is the minimum energy that a photon must have to ionize a ground= state hydrogen atom to the
n = 4 energy level?

Accepted Answer

The answer of What is the minimum energy that a...

Question 12

Which element below is expected to have the most negative electron affinity?

Accepted Answer

Fluorine (F) is expected to have the most negative electron affinity because it is the most electronegative element, meaning it has a strong tendency to attract electrons to itself.

Question 13

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?

Accepted Answer

The answer of Calculate the wavelengths in nanometers corresponding to...

Question 14

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

The answer of What is the uncertainty in the position...

Question 15

Place these types of radiation in order of increasing energy per photon.
I.yellow light from a street lamp
II.x-rays from a dental x-ray
III.microwaves from your cell phone
IV.radio waves from your favorite FM station

Accepted Answer

The answer of Place these types of radiation in order...

Question 16

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE₁ for S lower than that of P when the usual trend is for IE to increase across a row?

Accepted Answer

Removing an electron from sulfur results in a half-filled 3p subshell, which is more stable due to reduced electron-electron repulsions, making its ionization energy slightly lower than that of phosphorus.

Question 17

Calculate the de Broglie wavelength of an electron (9.11* 10^-31 kg) moving at 99% of the speed of light.This is closest in size to which of the following (approximate dimensions are given): a proton (2 fm); a helium atom (60 pm); a bacterium (10 µm); a mosquito (1 mm); a baseball bat 1 m); a football field (100 m)?

Accepted Answer

The answer of Calculate the de Broglie wavelength of an...

Question 18

Astronomers have detected hydrogen atoms in interstellar space in the n = 732 energy level.Suppose an atom in this excited state emits a photon and undergoes a transition from n = 732 to n = 2.How much energy does the atom lose as a result of this transition? What is the wavelength of the emitted radiation? Is this transition part of the Lyman, Balmer, or Paschen series?

Accepted Answer

The answer of Astronomers have detected hydrogen atoms in interstellar...

Question 19

If light at 193 nm from an argon-fluoride laser is incident on a gold-metal surface, electrons with a kinetic energy of 1.80 *10^-19 J are produced.What is the work function of gold in kilojoules per mole? What is the minimum wavelength of light in nanometers required to produce photoelectrons from gold (zero kinetic energy)?

Accepted Answer

The answer of If light at 193 nm from an...

Question 20

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

The answer of Radiation with a wavelength of _______ nm...

Quiz 3: Atomic Structure Explaining the Properties of Elements

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

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 10¹⁹ Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

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?

Electron affinity is the energy change that occurs _______.

Which row 2 element probably has the following successive ionization energies:

De Broglie proposed that $\lambda$ = h/mv.Define the symbols in this equation and describe the significance of de Broglie's proposal.

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10^-19 J.)

Which statement below regarding electron affinity is FALSE?

A mercury vapor lamp can be used as an 185 nm light source.What is the energy of one photon in joules? Of one mole of photons in kilojoules?

What is the minimum energy that a photon must have to ionize a ground= state hydrogen atom to the n = 4 energy level?

Which element below is expected to have the most negative electron affinity?

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?

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.)

Place these types of radiation in order of increasing energy per photon. I.yellow light from a street lamp II.x-rays from a dental x-ray III.microwaves from your cell phone IV.radio waves from your favorite FM station

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE₁ for S lower than that of P when the usual trend is for IE to increase across a row?

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.

Quiz 3: Atomic Structure Explaining the Properties of Elements

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

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 1019 Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

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?

Electron affinity is the energy change that occurs _______.

Which row 2 element probably has the following successive ionization energies:

De Broglie proposed that λ\lambdaλ = h/mv.Define the symbols in this equation and describe the significance of de Broglie's proposal.

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10-19 J.)

Which statement below regarding electron affinity is FALSE?

A mercury vapor lamp can be used as an 185 nm light source.What is the energy of one photon in joules? Of one mole of photons in kilojoules?

What is the minimum energy that a photon must have to ionize a ground= state hydrogen atom to the n = 4 energy level?

Which element below is expected to have the most negative electron affinity?

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?

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.)

Place these types of radiation in order of increasing energy per photon. I.yellow light from a street lamp II.x-rays from a dental x-ray III.microwaves from your cell phone IV.radio waves from your favorite FM station

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE1 for S lower than that of P when the usual trend is for IE to increase across a row?

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.

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 10¹⁹ Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

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?

De Broglie proposed that $\lambda$ = h/mv.Define the symbols in this equation and describe the significance of de Broglie's proposal.

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10^-19 J.)

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?

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.)

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE₁ for S lower than that of P when the usual trend is for IE to increase across a row?

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.