Explain the general trend in first ionisation energy across period 2 in the periodic table.
- Across period 2, the nuclear charge increases from Li (3+) to Ne (10+) as protons are added to the nucleus. - The electros are removed from the same main energy level and electrons in the same main energy level do not shield each other well. - Therefore, the force of attraction, from the nucleus, on the outer electrons increases from left to right across the period and the outer electron is more difficult to reove for neon. - The neon atom is smaller than the lithium atom and, therefore, the outer electron is closer to the nucleus amd more strongly held.
EA
Related Chemistry IB answers
All answers ▸Explain why successive ionization energies of an element increase and how they account for the existence of three main energy levels in the sodium atom
What is the charge of iron in the following complex: [Fe(H2O)6]Cl2 ?
Is breaking bonds endothermic or exothermic?
Explain why successive ionization energies of an element increase