Question 1

Choose the element with the highest ionization energy.
A)Na
B)Mg
C)Al
D)P
E)S

Accepted Answer

Phosphorus (P) has the highest ionization energy among the given options because it is furthest to the right and top on the periodic table, where ionization energy generally increases.

Question 2

Of the following elements,which is most likely to form a negative ion with charge 1-?
A)Ba
B)Ca
C)Si
D)P
E)Cl

Accepted Answer

Chlorine (Cl) is the most likely to form a negative ion with a charge of 1-, as it has only 1 valence electron and needs to gain one more electron to achieve a stable octet configuration. The other elements have a tendency to lose electrons to achieve a stable octet, forming positive ions.

Question 3

Order the elements S,Cl,and F in terms of increasing atomic radii.
A)S,Cl,F
B)Cl,F,S
C)F,S,Cl
D)F,Cl,S
E)S,F,Cl

Accepted Answer

Atomic radius increases down a group and decreases across a period on the periodic table. Since S, Cl, and F are in the same group with F at the top, followed by Cl, and then S, the order from smallest to largest atomic radius is F < Cl < S.

Question 4

Order the elements S,Cl,and F in terms of increasing ionization energy.
A)S,Cl,F
B)Cl,F,S
C)F,S,Cl
D)F,Cl,S
E)S,F,Cl

Accepted Answer

Ionization energy generally increases across a period from left to right due to the increasing nuclear charge. Since S, Cl, and F are in the same period with S being the furthest left and F being the furthest right, the order of increasing ionization energy is S < Cl < F.

Question 5

Which of the following electron configurations is different from that expected?
A)Ca
B)Sc
C)Ti
D)V
E)Cr

Accepted Answer

The expected electron configuration for Cr is [Ar] 3d5 4s1, but in reality, it is [Ar] 3d5 4s2. This is due to the stability gained from a half-filled d subshell.

Question 6

Consider the ionization energy (IE)of the magnesium atom.Which of the following is not true? A)The IE of Mg is lower than that of sodium. B)The IE of Mg is lower than that of neon. C)The IE of Mg is lower than that of beryllium. D)The IE of Mg is higher than that of calcium. E)The IE of Mg is lower than that of Mg⁺.

Accepted Answer

The answer of Consider the ionization energy (IE)of the magnesium...

Question 7

Which of the following is the highest energy orbital for a silicon atom?
A)1s
B)2s
C)3s
D)3p
E)3d

Accepted Answer

The answer of Which of the following is the highest...

Question 8

Copper exhibits the expected electron configuration.

Accepted Answer

Copper exhibits a special electron configuration due to the stability gained by having a half-filled d subshell. Its actual electron configuration is [Ar] 3d10 4s1.

Question 9

Which of the following have 10 electrons in the d orbitals?
A)Mn
B)Fe
C)Cu
D)Zn
E)two of the above

Accepted Answer

Cu and Zn have 10 electrons in their d orbitals. Cu has an electron configuration of [Ar] 3d^10 4s^1, and Zn has an electron configuration of [Ar] 3d^10 4s^2, both filling the d orbitals with 10 electrons.

Question 10

Which of the following concerning second ionization energies is true?
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 higher than that of Mg because the electrons are taken from the same energy level,but the Al atom has one more proton.
C)That of Al is lower than that of Mg because Mg wants to lose the second electron,thus the energy change is greater.
D)That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital,thus it is easier to take.
E)The second ionization energies are equal for Al and Mg.

Accepted Answer

The second ionization energy measures the energy required to remove a second electron from a positively charged ion. In the case of Mg and Al, both elements have two electrons in their outermost energy level (3s), so the first electron removal takes similar energy. However, Al has one more proton in its nucleus than Mg, meaning the positive charge is stronger and the electrons are held more tightly. Therefore, it takes more energy to remove the second electron from Al, making its second ionization energy greater than that of Mg.

Question 11

Which of the following processes represents the ionization energy of bromine? A)Br(s) Br⁺(g)+ e^- B)Br(l) Br⁺(g)+ e^- C)Br(g) Br⁺(g)+ e^- D)Br(s) Br⁺(s)+ e^- E)Br₂(g) Br₂⁺(g)+ e^-

Accepted Answer

The ionization energy of bromine refers to the energy required to remove an electron from a bromine atom in the gaseous state. Therefore, the correct process should have gaseous bromine as a reactant. Choice C represents the correct process as it has gaseous bromine (Br(g)) as a reactant, and it shows the process of removing an electron from a bromine atom (e^-). The other choices have either solid or liquid bromine as a reactant, or they show a different type of reaction.

Question 12

When electron configurations differ from expected,it is because orbitals want to be half-filled.

Accepted Answer

This is known as Hund's rule which states that orbitals prefer to be half-filled or fully filled due to greater stability. This can lead to deviations in expected electron configurations.

Question 13

The first ionization energy of Mg is 735 kJ/mol.The second ionization energy is
A)735 kJ/mol
B)less than 735 kJ/mol
C)greater than 735 kJ/mol
D)More information is needed to answer this question.
E)None of these.

Accepted Answer

The second ionization energy of an element is always greater than its first ionization energy. So, the second ionization energy of Mg will be greater than 735 kJ/mol. Therefore, the correct answer is (C) greater than 735 kJ/mol.

Question 14

Of the following elements,which has the lowest first ionization energy?
A)Ba
B)Ca
C)Si
D)P
E)Cl

Accepted Answer

The first ionization energy generally decreases down a group in the periodic table due to the increasing distance between the valence electrons and the nucleus. Ba is located at the bottom of Group 2 (alkaline earth metals), therefore, it has the lowest first ionization energy among the given options.

Question 15

List the following atoms in order of increasing ionization energy: Li,Na,C,O,F.
A)Li < Na < C < O < F
B)Na < Li < C < O < F
C)F < O < C < Li < Na
D)Na < Li < F < O < C
E)Na < Li < C < F < O

Accepted Answer

Ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table. Thus, Na (being lower in the same group) has a lower ionization energy than Li, and as we move from C to O to F across the period, the ionization energy increases.

Question 16

Which of the following exhibits the correct orders for both atomic radius and ionization energy,respectively? (smallest to largest)
A)S,O,F,and F,O,S
B)F,S,O,and O,S,F
C)S,F,O,and S,F,O
D)F,O,S,and S,O,F
E)none of these

Accepted Answer

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

Question 17

For which of the following elements does the electron configuration for the lowest energy state show a partially filled d orbital?
A)Ti
B)Rb
C)Cu
D)Ga
E)Kr

Accepted Answer

The answer of For which of the following elements does...

Question 18

Consider a planet where the temperature is so high that the ground state of an electron in the hydrogen atom is n = 4.What is the ratio of ionization energy for hydrogen on this planet compared to that on Earth?
A)1 : 4
B)4 : 1
C)1 : 16
D)16 : 1
E)1 : 1

Accepted Answer

The ionization energy of hydrogen is given by:
E = -13.6/n^2 electron volts (eV)
On the planet, the ground state is n=4, so the ionization energy would be:
E = -13.6/4^2 = -0.85 eV
On Earth, the ground state is n=1, so the ionization energy would be:
E = -13.6/1^2 = -13.6 eV
The ratio of ionization energy between the planet and Earth would be:
-0.85/-13.6 = 1/16
Therefore, the ratio of ionization energy for hydrogen on this planet compared to that on Earth is 1:16.

Question 19

The number of unpaired electrons in the outer subshell of a Cl atom is
A)0
B)1
C)2
D)3
E)none of these

Accepted Answer

Chlorine atom has seven electrons in its outermost subshell. In order to achieve stability, it needs one more electron to complete the octet. Therefore, there is one unpaired electron in the outermost subshell of a chlorine atom.

Question 20

Which of the following atoms would have the largest second ionization energy?
A)Mg
B)Cl
C)S
D)Ca
E)Na

Accepted Answer

The second ionization energy is highest for Na because removing a second electron from Na requires breaking into a stable noble gas configuration (Ne), which requires significantly more energy.

Quiz 7: Atomic Structure and Periodicity

Choose the element with the highest ionization energy.

Of the following elements,which is most likely to form a negative ion with charge 1-?

Order the elements S,Cl,and F in terms of increasing atomic radii.

Order the elements S,Cl,and F in terms of increasing ionization energy.

Which of the following electron configurations is different from that expected?

Consider the ionization energy (IE) of the magnesium atom.Which of the following is not true?

Which of the following is the highest energy orbital for a silicon atom?

Copper exhibits the expected electron configuration.

Which of the following have 10 electrons in the d orbitals?

Which of the following concerning second ionization energies is true?

Which of the following processes represents the ionization energy of bromine?

When electron configurations differ from expected,it is because orbitals want to be half-filled.

The first ionization energy of Mg is 735 kJ/mol.The second ionization energy is

Of the following elements,which has the lowest first ionization energy?

List the following atoms in order of increasing ionization energy: Li,Na,C,O,F.

Which of the following exhibits the correct orders for both atomic radius and ionization energy,respectively? (smallest to largest)

For which of the following elements does the electron configuration for the lowest energy state show a partially filled d orbital?

Consider a planet where the temperature is so high that the ground state of an electron in the hydrogen atom is n = 4.What is the ratio of ionization energy for hydrogen on this planet compared to that on Earth?

The number of unpaired electrons in the outer subshell of a Cl atom is

Which of the following atoms would have the largest second ionization energy?