Which of the following has the largest second ionization energy?
Question 29 options:
a) S
b) Mg
c) Si
d) Na
e) P
The correct answer is c) Si
To determine which element has the largest second ionization energy among the provided options (S, Mg, Si, Na, and P), you need to understand the concept of ionization energy.
Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase. The second ionization energy refers to the energy required to remove a second electron from the same atom or ion.
Generally, ionization energy increases across a period from left to right in the periodic table because the atomic radius decreases, and the electrons are held more tightly by the nucleus. This results in a higher ionization energy.
Let's compare the options:
a) S (sulfur) - Sulfur is located to the right of magnesium and sodium in the periodic table, so it is expected to have a higher ionization energy than them.
b) Mg (magnesium) - Magnesium is located in the alkaline earth metals group, which has a lower ionization energy compared to the elements in the group after the noble gases.
c) Si (silicon) - Silicon is located to the right of magnesium and sodium, so it is expected to have a higher ionization energy.
d) Na (sodium) - Sodium is located in the alkali metals group, which generally has lower ionization energy compared to other elements.
e) P (phosphorus) - Phosphorus is located between sulfur and silicon, so it is expected to have a higher ionization energy than magnesium and sodium, but potentially lower than sulfur or silicon.
Based on these comparisons, the element with the largest second ionization energy among the options is most likely:
c) Si (silicon).
Keep in mind that the actual values of ionization energy can vary, and it is best to consult a reliable source or reference table for precise values.
To determine which element has the largest second ionization energy, we need to understand what ionization energy is. Ionization energy is the energy required to remove an electron from an atom or ion. The second ionization energy refers to the energy required to remove a second electron from a singly charged ion.
To find the element with the largest second ionization energy among the given options, we need to look at the electron configurations and the trends in the periodic table.
Looking at the options:
a) Sulfur (S) has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁴
b) Magnesium (Mg) has the electron configuration: 1s² 2s² 2p⁶ 3s²
c) Silicon (Si) has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p²
d) Sodium (Na) has the electron configuration: 1s² 2s² 2p⁶ 3s¹
e) Phosphorus (P) has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p³
Examining the options, we can see that both magnesium (Mg) and silicon (Si) have completed their first energy level (n=1) and second energy level (n=2) electron configurations. Since they have already reached a stable configuration, it would require a relatively large amount of energy to remove another electron from them.
Comparing the remaining elements:
a) Sulfur (S) has more electrons in its configuration compared to both sodium (Na) and phosphorus (P). This means that the electron-electron repulsion is more significant, making it easier to remove an electron.
d) Sodium (Na) has only one electron in its outermost energy level (3s¹). Removing the outermost electron would require less energy compared to removing the second electron from magnesium or silicon.
e) Phosphorus (P) has one more electron in its outermost energy level (3p³) compared to sodium (Na). Since it has more electrons, the electron-electron repulsion is relatively higher, making it slightly more difficult to remove an electron compared to sodium.
Based on the electron configurations and the trends in the periodic table, the element with the largest second ionization energy among the given options would be b) Mg (Magnesium).