The first ionization potential of the elements B, C, and N (atomic numbers 5, 6, and 7) steadily increases, but that of O is less than that of N. The best interpretation of the lower
value for O is that:
1. the ionization potential of N is a maximum and the values decrease steadily for the elements O, F, and Ne.
2. there is more shielding of the nuclear charge in O than in B, C, or N.
3. the electron removed from O is farther from the nucleus and therefore less tightly bound than that in N.
4. the electron removed from O corresponds to a different value of the quantum number L than that of the electron removed from B, C,or N.
5. the half-filled set of p orbitals in N makes it more difficult to remove an electron from N than from O.
I think the answer is 1, but I'm not sure.
#1 CAN'T be right.
I.P. N = 1402
I.P. O = 1314
I.P. F = 1681
I.P. Ne = 2080
You can look these up yourself at www.webelements.com as I did. The table shows I.P. does NOT decrease steadily.
I would look at #5 for the correct answer.
To determine the best interpretation of the lower ionization potential of oxygen (O) compared to nitrogen (N) in this scenario, we need to consider some key factors.
The ionization potential refers to the energy required to remove an electron from an atom or ion. A higher ionization potential means it takes more energy to remove an electron, indicating a stronger hold on the electron by the nucleus.
In the given question, it states that the ionization potentials of elements B, C, and N increase steadily, which means it becomes more difficult to remove an electron from these elements as you move across the period from left to right. However, it also states that the ionization potential of O is less than that of N, which means it is easier to remove an electron from O compared to N.
Now, let’s go through the options one by one to determine the best interpretation:
1. This option suggests that the ionization potential of N is a maximum, and the values decrease steadily for the elements O, F, and Ne. However, this contradicts the given information stating that the ionization potential of N is higher than that of O.
2. This option suggests that there is more shielding of the nuclear charge in O than in B, C, or N. Shielding refers to when inner electron shells partially block the attraction between the outermost electrons and the nucleus. In this case, the greater shielding in O could result in a weaker attraction, making it easier to remove an electron. This is a plausible explanation.
3. This option suggests that the electron removed from O is farther from the nucleus and therefore less tightly bound than in N. This explanation is consistent with the idea that a looser binding between the outer electron and the nucleus could result in a lower ionization potential for O compared to N.
4. This option suggests that the electron removed from O corresponds to a different value of the quantum number L than that of the electron removed from B, C, or N. The quantum number L refers to the orbital angular momentum, which does not directly impact ionization potential. Therefore, this option is less likely to be the best interpretation.
5. This option suggests that the half-filled set of p orbitals in N makes it more difficult to remove an electron from N than from O. However, this option does not align with the given information stating that the ionization potential of O is lower than that of N.
Considering these points, options 2 and 3 seem to provide the most reasonable explanations. The best interpretation, in this case, is option 3: the electron removed from O is farther from the nucleus and therefore less tightly bound than the electron in N.
The correct answer is 3. The lower value for the first ionization potential of oxygen (O) compared to nitrogen (N) can be interpreted as the electron being less tightly bound in O. This means that the electron in O is farther from the nucleus and therefore easier to remove than the electron in N.
Option 1 is incorrect because the ionization potential values do not decrease steadily for O, F, and Ne.
Option 2 is incorrect because shielding of the nuclear charge does not explain the lower ionization potential of O compared to N.
Option 4 is incorrect because the quantum number L does not directly affect the ionization potential.
Option 5 is incorrect because the half-filled set of p orbitals in N does not directly affect the ionization potential.