The ionisation energy of an element is the energy required to remove an electron from a gaseous atom or ion. The ionisation energy generally increases across a period (from left to right) on the periodic table and decreases down a group (from top to bottom). This is because as you move across a period, the number of protons in the nucleus increases, which means the positively charged nucleus attracts the negatively charged electrons more strongly, thus more energy is needed to remove an electron. On the other hand, as you move down a group, the outer electrons are further from the nucleus and are therefore held less tightly to the atom.

Given the elements Phosphorus, Nitrogen, Antimony, and Arsenic:

1. Phosphorus (P) is in Period 3, Group 15.
2. Nitrogen (N) is in Period 2, Group 15.
3. Antimony (Sb) is in Period 5, Group 15.
4. Arsenic (As) is in Period 4, Group 15.

Based on the periodic trends, Nitrogen, being furthest to the right and highest up, would have the highest ionisation energy among these elements.

Question

The ionisation energy of an element is the energy required to remove an electron from a gaseous atom or ion. The ionisation energy generally increases across a period (from left to right) on the periodic table and decreases down a group (from top to bottom). This is because as you move across a period, the number of protons in the nucleus increases, which means the positively charged nucleus attracts the negatively charged electrons more strongly, thus more energy is needed to remove an electron. On the other hand, as you move down a group, the outer electrons are further from the nucleus and are therefore held less tightly to the atom.

Given the elements Phosphorus, Nitrogen, Antimony, and Arsenic:

1. Phosphorus (P) is in Period 3, Group 15.
2. Nitrogen (N) is in Period 2, Group 15.
3. Antimony (Sb) is in Period 5, Group 15.
4. Arsenic (As) is in Period 4, Group 15.

Based on the periodic trends, Nitrogen, being furthest to the right and highest up, would have the highest ionisation energy among these elements.

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 ionisation energy generally increases across a period (from left to right) on the periodic table and decreases down a group (from top to bottom). This is because as you move across a period, the number of protons in the nucleus increases, which means the positively charged nucleus attracts the negatively charged electrons more strongly, thus more energy is needed to remove an electron. On the other hand, as you move down a group, the outer electrons are further from the nucleus and are therefore held less tightly to the atom.

Given the elements Phosphorus, Nitrogen, Antimony, and Arsenic:

1. Phosphorus (P) is in Period 3, Group 15.
2. Nitrogen (N) is in Period 2, Group 15.
3. Antimony (Sb) is in Period 5, Group 15.
4. Arsenic (As) is in Period 4, Group 15.

Based on the periodic trends, Nitrogen, being furthest to the right and highest up, would have the highest ionisation energy among these elements.

Using the periodic table which of the following elements has the highest ionisation energy? Phosphorus1Nitrogen2Antimony3Arsenic

Question

Using the periodic table which of the following elements has the highest ionisation energy?

Solution

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