Question 1

Which of the following statements is true about the ionization energy of Mg⁺? A) It will be equal to and opposite in sign to the electron affinity of Mg. B) It will be equal to and opposite in sign to the electron affinity of Mg⁺. C) It will be equal to the ionization energy of Li. D) It will be equal to and opposite in sign to the electron affinity of Mg²⁺. E) none of the above

Accepted Answer

The ionization energy of Mg⁺ is equal to and opposite in sign to the electron affinity of Mg²⁺. This is because the ionization energy is the energy required to remove an electron from an atom or ion, while the electron affinity is the energy released when an electron is added to an atom or ion. The ionization energy of Mg⁺ is the energy required to remove an electron from Mg⁺, which is equal to the energy released when an electron is added to Mg²⁺.

Question 2

Place the elements C, N, and O in order of increasing ionization energy.
A) N, O, C
B) C, N, O
C) O, N, C
D) C, O, N
E) none of these

Accepted Answer

The answer of Place the elements C, N, and O...

Question 3

The valence electron configuration of an element is ns²(n - 1)d¹⁰np². To which group does X belong? A) Group 3A B) Group 4A C) Group 6A D) Group 5A E) Group 7A

Accepted Answer

The element has a valence electron configuration of ns²np², which corresponds to Group 4A (or Group 14 in IUPAC numbering) in the periodic table.

Question 4

Place the elements Ge, S, and Ne in order of increasing atomic radius.
A) Ge, Ne, S
B) S, Ne, Ge
C) S, Ge, Ne
D) Ge, S, Ne
E) Ne, S, Ge

Accepted Answer

Atomic radius increases as you move down a group and decreases as you move across a period from left to right. Ne (Neon) is a noble gas, S (Sulfur) is in the same period but to the left of Ge (Germanium), making Ne the smallest and Ge the largest in atomic radius.

Question 5

Which element is most likely to form an ion with a charge of 2+?
A) Rb
B) Al
C) F
D) S
E) Ca

Accepted Answer

Ca (calcium) is most likely to form an ion with a charge of 2+ because it has two valence electrons that it can lose to achieve a stable octet electron configuration. The other options either have fewer valence electrons or would have to gain electrons to form an ion with a 2+ charge.

Question 6

Which statements about hydrogen are true? I. H has a lower ionization energy than He. II. H^- is smaller than H. III. H has a higher effective nuclear charge than He. IV. H is always a metal.V. H does not have a second ionization energy. A) II, IV, V B) I, III, V C) I, III, IV, V D) I, V E) II, IV

Accepted Answer

I: This statement is false as He has a lower ionization energy than H. II: This statement is true as H^- is a sulfur ion and has more electrons than hydrogen. III: This statement is true as the effective nuclear charge increases with atomic number, and H has a higher atomic number than He. IV: This statement is false as H can be either a metal or a nonmetal depending on the context. V: This statement is true as H only has one electron and therefore cannot have a second ionization energy.

Question 7

Sodium losing an electron is an ________ process, and fluorine losing an electron is an _______ process.
A) exothermic, endothermic
B) endothermic, exothermic
C) exothermic, exothermic
D) More information is needed.
E) endothermic, endothermic

Accepted Answer

The answer of Sodium losing an electron is an ________...

Question 8

Consider the following orderings.
I. Al < Si < P < Cl
II. Be < Mg < Ca < Sr
III. I < Br < Cl < F
IV. NaS1U1P1+S1S1P0 < MgS1U1P12+S1S1P0 < AlS1U1P13+S1S1P0 < SiS1U1P14+S1S1P0
-Which of the following statements is true of second ionization energies?
A) That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to take the second electron away.
B) That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital, so it is easier to take away.
C) That of Al is lower than that of Mg because Mg wants to lose the second electron, so the energy change is greater.
D) The second ionization energies are equal for Al and Mg.
E) That of Al is higher than that of Mg because the electrons are taken from the same energy level, but the Al atom has one more proton.

Accepted Answer

The second ionization energy of Al is higher than that of Mg because after losing one electron, Mg achieves a stable noble gas configuration (Ne), making it less willing to lose a second electron. Al, on the other hand, after losing one electron, still does not achieve a noble gas configuration and has a higher nuclear charge due to one more proton, making it harder to remove the second electron.

Question 9

Four electrons are confined to a one-dimensional box 5.64 × 10^-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Accepted Answer

The answer of Four electrons are confined to a one-dimensional...

Question 10

Which two elements are most likely to have the same oxidation state in an ionic compound?
A) Al, Cl
B) S, Ca
C) Li, Be
D) Cl, F
E) none of these

Accepted Answer

The two elements that are most likely to have the same oxidation state in an ionic compound are those that are close to each other in the periodic table. Both chlorine (Cl) and fluorine (F) are halogens and are located in the same group, so they have the same valence electron configuration and therefore have the same oxidation state in ionic compounds. The other answer choices do not fit this criterion.

Question 11

Researchers recently formed a new synthetic element with atomic number 108. Which of the following elements would have chemical properties most similar to this new element?
A) Mo
B) Ac
C) Ti
D) Kr
E) Fe

Accepted Answer

The answer of Researchers recently formed a new synthetic element...

Question 12

Write the electron configuration of Ni²⁺.

Accepted Answer

The answer of Write the electron configuration of Ni²⁺....

Question 13

Consider the following orderings.
I. Al < Si < P < Cl
II. Be < Mg < Ca < Sr
III. I < Br < Cl < F
IV. NaS1U1P1+S1S1P0 < MgS1U1P12+S1S1P0 < AlS1U1P13+S1S1P0 < SiS1U1P14+S1S1P0
-Which of the following exhibits the correct orders (increasing) for atomic radius and ionization energy, respectively?
A) F, S, O, and O, S, F
B) F, O, S, and S, O, F
C) S, O, F, and F, O, S
D) S, F, O, and S, F, O
E) none of these

Accepted Answer

The answer of Consider the following orderings.
I. Al < Si...

Question 14

Consider the following orderings.
I. Al < Si < P < Cl
II. Be < Mg < Ca < Sr
III. I < Br < Cl < F
IV. NaS1U1P1+S1S1P0 < MgS1U1P12+S1S1P0 < AlS1U1P13+S1S1P0 < SiS1U1P14+S1S1P0
-Which of these give(s) a correct trend in ionization energy?
A) I, IV only
B) I, II only
C) I, III, IV
D) III only
E) none of them

Accepted Answer

The answer of Consider the following orderings.
I. Al < Si...

Question 15

Consider the following orderings.
I. Al < Si < P < Cl
II. Be < Mg < Ca < Sr
III. I < Br < Cl < F
IV. NaS1U1P1+S1S1P0 < MgS1U1P12+S1S1P0 < AlS1U1P13+S1S1P0 < SiS1U1P14+S1S1P0
-Which of these give(s) a correct trend in size?
A) II only
B) IV only
C) II, IV
D) III
E) I

Accepted Answer

The answer of Consider the following orderings.
I. Al < Si...

Question 16

Which of the following sets has elements with the most nearly identical atomic radii?
A) Mg, K, Rb, Ba
B) Be, B, C, N
C) Ne, Kr, Ar, He
D) Si, P, Se, Br
E) Ni, Fe, Co, Mn

Accepted Answer

Elements Ni, Fe, Co, and Mn are all transition metals in the same period on the periodic table, which means they have similar atomic radii due to their similar electron configurations and the filling of d orbitals.

Question 17

How many unpaired electrons does cobalt have in its ground state?
A) 7
B) 27
C) 5
D) 3
E) 1

Accepted Answer

Cobalt has 27 electrons, with the electron configuration [Ar] 3d7 4s2. The 3d sublevel has 5 orbitals, each with a maximum capacity of 2 electrons. In the ground state, the 7 electrons in the 3d sublevel will each occupy their own orbital, leaving 3 unpaired electrons. Therefore, the answer is D) 3.

Question 18

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is
A) consistent with the general trend relating changes in ionization energy across a period from left to right, because it is harder to take an electron from an oxygen atom than from a nitrogen atom.
B) incorrect.
C) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that the oxygen atom has two doubly occupied 2p orbitals and nitrogen has only one.
D) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that oxygen has one doubly occupied 2p orbital and nitrogen does not.
E) consistent with the general trend relating changes in ionization energy across a period from left to right, because it is easier to take an electron from an oxygen atom than from a nitrogen atom.

Accepted Answer

Oxygen has one doubly occupied 2p orbital, which leads to electron-electron repulsion, making it easier to remove an electron compared to nitrogen, which has half-filled stable 2p orbitals.

Question 19

Consider the following sets of quantum numbers. Which set(s) represent(s) impossible combinations?

Accepted Answer

The answer of Consider the following sets of quantum numbers....

Question 20

The energy equation for a particle in a cubic box of dimensions Lx = L_y = Lz is E_{nx, ny, nz} = Assume that 8 electrons occupy the allowed energy levels and that 2 electrons can occupy each allowed energy level.

Accepted Answer

The answer of The energy equation for a particle in...

Quiz 12: Quantum Mechanics and Atomic Theory

Which of the following statements is true about the ionization energy of Mg⁺?

Place the elements C, N, and O in order of increasing ionization energy.

The valence electron configuration of an element is ns²(n - 1) d¹⁰np². To which group does X belong?

Place the elements Ge, S, and Ne in order of increasing atomic radius.

Which element is most likely to form an ion with a charge of 2+?

Which statements about hydrogen are true? I. H has a lower ionization energy than He. II. H^- is smaller than H. III. H has a higher effective nuclear charge than He. IV. H is always a metal.V. H does not have a second ionization energy.

Sodium losing an electron is an __ process, and fluorine losing an electron is an _ process.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of the following statements is true of second ionization energies?

Four electrons are confined to a one-dimensional box 5.64 × 10^-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Which two elements are most likely to have the same oxidation state in an ionic compound?

Researchers recently formed a new synthetic element with atomic number 108. Which of the following elements would have chemical properties most similar to this new element?

Write the electron configuration of Ni²⁺.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of the following exhibits the correct orders (increasing) for atomic radius and ionization energy, respectively?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of these give(s) a correct trend in ionization energy?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of these give(s) a correct trend in size?

Which of the following sets has elements with the most nearly identical atomic radii?

How many unpaired electrons does cobalt have in its ground state?

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is

Consider the following sets of quantum numbers. Which set(s) represent(s) impossible combinations?

The energy equation for a particle in a cubic box of dimensions Lx = L_y = Lz is E_{nx, ny, nz} = Assume that 8 electrons occupy the allowed energy levels and that 2 electrons can occupy each allowed energy level.

Quiz 12: Quantum Mechanics and Atomic Theory

Which of the following statements is true about the ionization energy of Mg+?

Place the elements C, N, and O in order of increasing ionization energy.

The valence electron configuration of an element is ns2(n - 1) d10np2. To which group does X belong?

Place the elements Ge, S, and Ne in order of increasing atomic radius.

Which element is most likely to form an ion with a charge of 2+?

Which statements about hydrogen are true? I. H has a lower ionization energy than He. II. H- is smaller than H. III. H has a higher effective nuclear charge than He. IV. H is always a metal.V. H does not have a second ionization energy.

Sodium losing an electron is an ________ process, and fluorine losing an electron is an _______ process.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na+ < Mg2+ < Al3+ < Si4+ -Which of the following statements is true of second ionization energies?

Four electrons are confined to a one-dimensional box 5.64 × 10-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Which two elements are most likely to have the same oxidation state in an ionic compound?

Researchers recently formed a new synthetic element with atomic number 108. Which of the following elements would have chemical properties most similar to this new element?

Write the electron configuration of Ni2+.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na+ < Mg2+ < Al3+ < Si4+ -Which of the following exhibits the correct orders (increasing) for atomic radius and ionization energy, respectively?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na+ < Mg2+ < Al3+ < Si4+ -Which of these give(s) a correct trend in ionization energy?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na+ < Mg2+ < Al3+ < Si4+ -Which of these give(s) a correct trend in size?

Which of the following sets has elements with the most nearly identical atomic radii?

How many unpaired electrons does cobalt have in its ground state?

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is

Consider the following sets of quantum numbers. Which set(s) represent(s) impossible combinations?

The energy equation for a particle in a cubic box of dimensions Lx = Ly = Lz is Enx, ny, nz = Assume that 8 electrons occupy the allowed energy levels and that 2 electrons can occupy each allowed energy level.

Which of the following statements is true about the ionization energy of Mg⁺?

The valence electron configuration of an element is ns²(n - 1) d¹⁰np². To which group does X belong?

Which statements about hydrogen are true? I. H has a lower ionization energy than He. II. H^- is smaller than H. III. H has a higher effective nuclear charge than He. IV. H is always a metal.V. H does not have a second ionization energy.

Sodium losing an electron is an __ process, and fluorine losing an electron is an _ process.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of the following statements is true of second ionization energies?

Four electrons are confined to a one-dimensional box 5.64 × 10^-10 m long. If two electrons can occupy each allowed energy level, calculate the wavelength of electromagnetic radiation necessary to promote the highest-energy electron into the first excited state.

Write the electron configuration of Ni²⁺.

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of the following exhibits the correct orders (increasing) for atomic radius and ionization energy, respectively?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of these give(s) a correct trend in ionization energy?

Consider the following orderings. I. Al < Si < P < Cl II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ -Which of these give(s) a correct trend in size?

The energy equation for a particle in a cubic box of dimensions Lx = L_y = Lz is E_{nx, ny, nz} = Assume that 8 electrons occupy the allowed energy levels and that 2 electrons can occupy each allowed energy level.