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 ▸Under which conditions does CH4 have the same number of molecules as 100cm^3 of O2 at 27 degrees celsius and 1.0x10^5 Pa?
Describe how an increase in temperature affects the equilibrium of the main exothermic reaction of the Haber process?
Calculate: (a) The amount, in mol, of white phosphorus used, (b) the limiting reagent, (c) the excess amount, in mol, of the other reagent.
Which intermolecular forces do I need to know about and how do they differ in strength?