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 ▸Define the an acid/base according to the Bronsted-Lowry and Lewis theories. Support with equation to illustrate an acid-base reaction for each theory, identifying them clearly. Also state the bond type formed in an Lewis acid-base reaction.
What happens to the equilibrium constant of an endothermic reaction, that is in equilibrium, when the temperature increases? What would the effect of increasing pressure have on the reaction and on the value of Kc?
Why are noble gases so unreactive?
Describe how an increase in temperature affects the equilibrium of the main exothermic reaction of the Haber process?