Which of the following has the largest second ionization energy?
a) S
b) Mg
c) Si
d) Na
e) P
is the correct answer a)?
No, the correct answer is c) Si.
Ionization energy refers to the amount of energy required to remove an electron from an atom or ion. The second ionization energy is the energy required to remove a second electron from a singly charged ion.
Among the provided options, Si (silicon) has the largest second ionization energy.
Here is the order of the second ionization energies for the given elements:
a) S (sulfur)
b) Mg (magnesium)
c) Si (silicon)
d) Na (sodium)
e) P (phosphorus)
To determine the element with the largest second ionization energy among the given options, we need to understand what ionization energy is and how it changes across the periodic table.
Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous state. It is typically measured in units of kilojoules per mole (kJ/mol). The second ionization energy specifically refers to the energy required to remove a second electron from a singly charged ion.
As we move across a period in the periodic table from left to right, the ionization energy generally increases. This trend occurs because as we move from left to right, the atomic number (or the number of protons) increases. The increase in the positive charge in the nucleus makes it harder to remove electrons, resulting in higher ionization energy.
Looking at the options presented:
a) S (sulfur)
b) Mg (magnesium)
c) Si (silicon)
d) Na (sodium)
e) P (phosphorus)
Sulfur (S) is found in the third period of the periodic table, while the rest of the elements (Mg, Si, Na, P) are in the second period. Since we are comparing the second ionization energy, we need to focus on the elements within the second period.
Among the options in the second period, magnesium (Mg) has the highest atomic number (12), followed by silicon (Si, atomic number 14), sodium (Na, atomic number 11), and phosphorus (P, atomic number 15).
Therefore, the correct answer is b) Mg (magnesium) because it has the largest second ionization energy among the given options.
To determine the element with the largest second ionization energy among S, Mg, Si, Na, and P, we have to compare the trends across the periodic table.
Ionization energy refers to the energy required to remove an electron from an atom, creating a positive ion. Second ionization energy specifically refers to removing the second electron from a positively charged ion.
Looking at the periodic table, the general trend is that ionization energy increases as you move from left to right across a period and decreases as you move down a group.
Among the given elements, the one with the largest second ionization energy is the one that is closest to having a full valence shell, which would require the most energy to remove a second electron.
Let's analyze each option:
a) S (Sulfur) - Sulfur has an electron configuration of 1s² 2s² 2p⁶ 3s² 3p⁴. When one electron is removed from the sulfur ion (S⁺), the electron configuration becomes 1s² 2s² 2p⁶ 3s² 3p³. Removing a second electron requires energy, but it is easier since the electron is being removed from the 3p sublevel. Therefore, sulfur has a lower second ionization energy compared to other elements.
b) Mg (Magnesium) - Magnesium has an electron configuration of 1s² 2s² 2p⁶ 3s². When one electron is removed from the magnesium ion (Mg⁺), the electron configuration becomes 1s² 2s² 2p⁶ 3s¹. Removing a second electron requires more energy, as it would involve removing an electron from the 2p sublevel. However, compared to the other options, magnesium has a relatively lower second ionization energy.
c) Si (Silicon) - Silicon has an electron configuration of 1s² 2s² 2p⁶ 3s² 3p². When one electron is removed from the silicon ion (Si⁺), the electron configuration becomes 1s² 2s² 2p⁶ 3s² 3p¹. Removing a second electron requires more energy, as it would involve removing an electron from the 3p sublevel. Silicon has a higher second ionization energy compared to sulfur and magnesium.
d) Na (Sodium) - Sodium has an electron configuration of 1s² 2s² 2p⁶ 3s¹. When one electron is removed from the sodium ion (Na⁺), the electron configuration becomes 1s² 2s² 2p⁶. Removing a second electron requires a significant amount of energy, as it would involve removing an electron from the completely filled 2p sublevel. Sodium has a relatively higher second ionization energy compared to sulfur, magnesium, and silicon.
e) P (Phosphorus) - Phosphorus has an electron configuration of 1s² 2s² 2p⁶ 3s² 3p³. When one electron is removed from the phosphorus ion (P⁺), the electron configuration becomes 1s² 2s² 2p⁶ 3s² 3p². Removing a second electron requires even more energy, as it would involve removing an electron from the half-filled 3p sublevel. Phosphorus has the highest second ionization energy compared to the other options.
Therefore, the correct answer is e) P (Phosphorus).