The second energy level feels a + 13 charge and the outer energy level feels a + 5 charge. Using the concepts of shielding and attraction explain why sulfur is smaller in radius than silicon. Sulfur’s outer level of electrons feels a +6 charge pulling on it from the nucleus.
Q. How much energy does it take to remove an electron from magnesium?
Magnesium has the electron configuration of 1s22s22p63s2. The first two electrons are removed from the third level. The third electron is removed from the second level. Electrons in lower levels feel a greater attraction to the nucleus and are more difficult to remove….Ionization Energy.
Table of Contents
- Q. How much energy does it take to remove an electron from magnesium?
- Q. Would it be more difficult to remove an electron from fluorine or nitrogen?
- Q. Why is the ionization energy of phosphorus lower than nitrogen?
- Q. Does magnesium or phosphorus have a larger ionization energy?
- Q. Does phosphorus or sulfur have a higher ionization energy?
- Q. Why is it easier to remove an electron from sulfur than phosphorus?
- Q. Why is the first ionisation energy of phosphorus higher than sulfur?
- Q. Does sulfur have a higher ionization energy than oxygen?
| Element | P |
|---|---|
| I2 | 1890 |
| I3 | 2905 |
| I4 | 4950 |
| I5 | 6270 |
Q. Would it be more difficult to remove an electron from fluorine or nitrogen?
For similar reasons as question 1, it would take more energy to remove an outer electron from an atom of fluorine than from nitrogen. The outer electron from fluorine feels a stronger force of attraction from the nucleus.
Q. Why is the ionization energy of phosphorus lower than nitrogen?
Since the 3p electrons in sulfur (that sulfur would lose) are paired, sulfur has more electron repulsion in those orbitals than phosphorus does, so it takes less energy input to remove an electron from sulfur. …
Q. Does magnesium or phosphorus have a larger ionization energy?
First ionisation energy
| Element | Symbol | First ionisation energy /kJ mol–1 |
|---|---|---|
| magnesium | Mg | 738 |
| aluminium | Al | 578 |
| silicon | Si | 789 |
| phosphorus | P | 1012 |
Q. Does phosphorus or sulfur have a higher ionization energy?
Either all unpaired or all paired makes it stable, so if phosphorus is all unpaired it take more energy to remove an electron than it would from sulfur in which one electron can be removed making it more stable. Because it takes more energy for phosphorus, it has a higher ionization energy.
Q. Why is it easier to remove an electron from sulfur than phosphorus?
Since the 3p electrons in sulfur (that sulfur would lose) are paired, sulfur has more electron repulsion in those orbitals than phosphorus does, so it takes less energy input to remove an electron from sulfur.
Q. Why is the first ionisation energy of phosphorus higher than sulfur?
In sulfur, the 4 electrons in the 3p level, are all paired. While in phosphorus there are 2 paired electrons and 1 lone electron in the 3p level. Therefore, the first ionisation energy for sulfur will be slightly lower than that of phosphorus, due to the paired electrons in its 3p sub-level.
Q. Does sulfur have a higher ionization energy than oxygen?
The sulfur ion has an extra shell than an oxygen ion, so the atomic size of sulfur should be greater than oxygen. Therefore, the ionization energy of an oxygen ion should be more than a sulfur ion because the electrons in oxygen are closer to the nucleus when compared to sulfur.
