Question 1

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

Accepted Answer

The answer of Which of the following elements would you...

Question 2

Which of the following shows the correct expression for the ionization energy indicated?

Accepted Answer

The answer of Which of the following shows the correct...

Question 3

Calculate the wavelengths in nm 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 nm corresponding to...

Question 4

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

Accepted Answer

The first ionization energy generally increases from left to right across a period of the periodic table. Fluorine is the furthest to the right and has the smallest atomic radius, which means that it has the strongest attraction for its electrons and requires the most energy to remove one from its outermost shell.

Question 5

Which arrangement is in the correct order of increasing radii?

Accepted Answer

The trend for increasing radii is from right to left and from top to bottom on the periodic table. Based on this trend, option C is the only arrangement that follows this trend. The radii increase from P to As to a larger complex ion with extra S and P orbitals. Options A, B, D, and E are not in the correct order of increasing radii according to the periodic trend.

Question 6

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 it easier to remove an electron compared to phosphorus.

Question 7

Radiation with a wavelength of __________ nm is produced by the n = 5 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...

Question 8

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

Accepted Answer

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

Question 9

Which row 2 element probably has the following successive ionization energies IE₁,1314 IE₂,3389 IE₃,5298 IE₄,7471 IE₅,10,992 IE₆,13,329 IE₇,71,345 IE₈,84,087

Accepted Answer

The successive ionization energies increase as electrons are removed from an element, and the jumps in energy between ionization steps can indicate the number of valence electrons an element has. Based on the given ionization energies, the element with 6 valence electrons (which would require removing electrons up to the 6th ionization energy listed) is oxygen (O).

Question 10

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

Accepted Answer

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

Question 11

Which of the following elements would you expect to have the most negative electron affinity?

Accepted Answer

Fluorine has the highest electron affinity because it has the smallest atomic radius and the highest effective nuclear charge. The small size allows it to hold on to an additional electron more tightly because there is less distance between the nucleus and the valence electrons.

Question 12

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 13

Electron affinity is the energy change that occurs ________________

Accepted Answer

Electron affinity is defined as the energy change that occurs when a gas-phase atom or ion in its ground state gains an electron. This definition corresponds to answer choice B.

Question 14

Which of the following statements regarding electron affinity is NOT true?

Accepted Answer

Z_eff (effective nuclear charge) does impact electron affinity values, as it influences the attraction between the nucleus and the added electron.

Question 15

The Swift Explorer launched in 2004 by NASA can detect electromagnetic bursts with frequencies up to about 3.6 $\times$ 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 launched in 2004 by...

Question 16

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 $\times$ 10^-¹⁹ J)

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

Which of the following statements regarding ionization energy is NOT true?

Accepted Answer

Atoms in the same column (group) of the periodic table do not have equal ionization energies. This is because ionization energy increases as you move from left to right across a period, due to an increase in effective nuclear charge. However, within a group, ionization energy decreases as you move down the group due to an increase in electron shielding.

Question 19

Which arrangement is in the correct order of decreasing radii?

Accepted Answer

The answer of Which arrangement is in the correct order...

Question 20

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 observed between IE₃ and IE₄ can be explained by the removal of an inner shell electron with a lower n value, which requires a significantly higher amount of energy to remove compared to the outer shell electrons. This is because the inner shell electrons are more tightly bound to the nucleus and experience a stronger effective nuclear charge.

Quiz 3: Atomic Structure-Explaining the Properties of Elements

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

Which of the following shows the correct expression for the ionization energy indicated?

Calculate the wavelengths in nm 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?

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

Which arrangement is in the correct order of increasing radii?

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 = 5 to n = 2 transition in the hydrogen atom; this transition occurs in the region of the electromagnetic spectrum.

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

Which row 2 element probably has the following successive ionization energies IE₁,1314 IE₂,3389 IE₃,5298 IE₄,7471 IE₅,10,992 IE₆,13,329 IE₇,71,345 IE₈,84,087

Which of the following elements would you expect to have the most negative electron affinity?

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

Electron affinity is the energy change that occurs ________________

Which of the following statements regarding electron affinity is NOT true?

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

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 $\times$ 10^-¹⁹ J)

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

Which of the following statements regarding ionization energy is NOT true?

Which arrangement is in the correct order of decreasing radii?

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?

Quiz 3: Atomic Structure-Explaining the Properties of Elements

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

Which of the following shows the correct expression for the ionization energy indicated?

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

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

Which arrangement is in the correct order of increasing radii?

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 = 5 to n = 2 transition in the hydrogen atom; this transition occurs in the __________ region of the electromagnetic spectrum.

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

Which row 2 element probably has the following successive ionization energies IE1,1314 IE2,3389 IE3,5298 IE4,7471 IE5,10,992 IE6,13,329 IE7,71,345 IE8,84,087

Which of the following elements would you expect to have the most negative electron affinity?

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

Electron affinity is the energy change that occurs ________________

Which of the following statements regarding electron affinity is NOT true?

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

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 ×\times× 10-19 J)

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

Which of the following statements regarding ionization energy is NOT true?

Which arrangement is in the correct order of decreasing radii?

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?

Calculate the wavelengths in nm 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 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 = 5 to n = 2 transition in the hydrogen atom; this transition occurs in the region of the electromagnetic spectrum.

Which row 2 element probably has the following successive ionization energies IE₁,1314 IE₂,3389 IE₃,5298 IE₄,7471 IE₅,10,992 IE₆,13,329 IE₇,71,345 IE₈,84,087

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

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 $\times$ 10^-¹⁹ J)

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?