The ionisation energy of an element is the energy required to remove an electron from a gaseous atom or ion. The first ionisation energy is the energy to remove the first electron, the second ionisation energy is the energy to remove the second electron, and so on.

In the periodic table, elements in the same group have the same number of electrons in their outer shell, and thus similar ionisation energies.

Looking at the given ionisation energies, there is a large jump between the second and third ionisation energies. This suggests that the element loses two electrons relatively easily, but the third electron is much harder to remove.

Therefore, the element likely has two electrons in its outer shell.

Looking at the options, the element that fits this description is Beryllium (Be), which is in Group 2 of the periodic table.

So, the answer is B. Be.

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The ionisation energy of an element is the energy required to remove an electron from a gaseous atom or ion. The first ionisation energy is the energy to remove the first electron, the second ionisation energy is the energy to remove the second electron, and so on.

In the periodic table, elements in the same group have the same number of electrons in their outer shell, and thus similar ionisation energies.

Looking at the given ionisation energies, there is a large jump between the second and third ionisation energies. This suggests that the element loses two electrons relatively easily, but the third electron is much harder to remove.

Therefore, the element likely has two electrons in its outer shell.

Looking at the options, the element that fits this description is Beryllium (Be), which is in Group 2 of the periodic table.

So, the answer is B. Be.

Knowee AI · Accepted Answer

The ionisation energy of an element is the energy required to remove an electron from a gaseous atom or ion. The first ionisation energy is the energy to remove the first electron, the second ionisation energy is the energy to remove the second electron, and so on.

In the periodic table, elements in the same group have the same number of electrons in their outer shell, and thus similar ionisation energies.

Looking at the given ionisation energies, there is a large jump between the second and third ionisation energies. This suggests that the element loses two electrons relatively easily, but the third electron is much harder to remove.

Therefore, the element likely has two electrons in its outer shell.

Looking at the options, the element that fits this description is Beryllium (Be), which is in Group 2 of the periodic table.

So, the answer is B. Be.

The first four ionisation energies (kJ mol-1) for a particular element are 550, 1064, 4210 and 5500respectively. This element should be placed in the same Group asA. LiB. BeC. BD. C

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