The incorrect statement among the given options is:

d. The first ionisation potential of Al (Al =13) is less than the first ionisation potential of Mg (Mg =12)

Explanation:

Ionization energy is the energy required to remove an electron from an atom or ion. It generally increases across a period (from left to right) on the periodic table and decreases down a group (top to bottom).

a. The third ionization potential of Mg is greater than the third ionization potential of Al. This is correct because Mg (Magnesium) loses two electrons easily as it achieves the stable noble gas configuration. But the third electron is from a new shell closer to the nucleus, so it requires more energy to remove.

b. The second ionization potential of Mg is greater than the second ionization potential of Na (Na =11). This is correct because after losing one electron, Na (Sodium) achieves the stable noble gas configuration. But Mg (Magnesium) still has one electron in the same shell, so it requires more energy to remove the second electron.

c. The first ionization potential of Na is less than the first ionization potential of Mg. This is correct because Na (Sodium) is to the left of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases.

d. The first ionization potential of Al (Al =13) is less than the first ionization potential of Mg (Mg =12). This is incorrect because Al (Aluminium) is to the right of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases. Therefore, the first ionization potential of Al should be greater than the first ionization potential of Mg.

Question

The incorrect statement among the given options is:

d. The first ionisation potential of Al (Al =13) is less than the first ionisation potential of Mg (Mg =12)

Explanation:

Ionization energy is the energy required to remove an electron from an atom or ion. It generally increases across a period (from left to right) on the periodic table and decreases down a group (top to bottom).

a. The third ionization potential of Mg is greater than the third ionization potential of Al. This is correct because Mg (Magnesium) loses two electrons easily as it achieves the stable noble gas configuration. But the third electron is from a new shell closer to the nucleus, so it requires more energy to remove.

b. The second ionization potential of Mg is greater than the second ionization potential of Na (Na =11). This is correct because after losing one electron, Na (Sodium) achieves the stable noble gas configuration. But Mg (Magnesium) still has one electron in the same shell, so it requires more energy to remove the second electron.

c. The first ionization potential of Na is less than the first ionization potential of Mg. This is correct because Na (Sodium) is to the left of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases.

d. The first ionization potential of Al (Al =13) is less than the first ionization potential of Mg (Mg =12). This is incorrect because Al (Aluminium) is to the right of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases. Therefore, the first ionization potential of Al should be greater than the first ionization potential of Mg.

Knowee AI · Accepted Answer

The incorrect statement among the given options is:

d. The first ionisation potential of Al (Al =13) is less than the first ionisation potential of Mg (Mg =12)

Explanation:

Ionization energy is the energy required to remove an electron from an atom or ion. It generally increases across a period (from left to right) on the periodic table and decreases down a group (top to bottom).

a. The third ionization potential of Mg is greater than the third ionization potential of Al. This is correct because Mg (Magnesium) loses two electrons easily as it achieves the stable noble gas configuration. But the third electron is from a new shell closer to the nucleus, so it requires more energy to remove.

b. The second ionization potential of Mg is greater than the second ionization potential of Na (Na =11). This is correct because after losing one electron, Na (Sodium) achieves the stable noble gas configuration. But Mg (Magnesium) still has one electron in the same shell, so it requires more energy to remove the second electron.

c. The first ionization potential of Na is less than the first ionization potential of Mg. This is correct because Na (Sodium) is to the left of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases.

d. The first ionization potential of Al (Al =13) is less than the first ionization potential of Mg (Mg =12). This is incorrect because Al (Aluminium) is to the right of Mg (Magnesium) in the same period of the periodic table. As we move from left to right in a period, the ionization energy generally increases. Therefore, the first ionization potential of Al should be greater than the first ionization potential of Mg.

Question

Solution

Similar Questions

Upgrade your grade with Knowee