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Why does the first ionisation energy inc...

Why does the first ionisation energy increase as we go from left to right along a given period of periodic table?

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It is due to decrease in atomic size and due to increase in effective nuclear charge.
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CENGAGE CHEMISTRY-APPENDIX - INORGANIC VOLUME 1-Exercise very short
  1. Why do alkali metals have lowest ionisation energy?

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  2. Why are lanthanides and actinides place at the bottom of the periodic ...

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  3. How do the basicity and solubility in water vary from Be(OH)(2) to Ba(...

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  4. Why are cations smaller than neutral atom?

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  5. Why are anions bigger than neutral atom?

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  6. Which is the smallest among Na^(o+),Mg^(2+),Al^(3+), and why?

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  7. Which has the largest ionic radius Ca^(2+),Mg^(2+),Ba^(2+)?

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  8. Define (a) metallic radius and (b) van der Waals radius.

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  9. Electronegativity

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  10. How does electronegativity move (a) down the group and (b) across the ...

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  11. Write general electronic configuration of p-block elements.

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  12. What is the nature of oxides formed by most of p-block elements?

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  13. Indentify the atom or ion which has larger radius in each of the follo...

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  14. Among the elements , Li, K, Ca, Cl and Kr, the element K has the lowes...

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  15. Which of the following pairs of elements would you expect to have lowe...

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  16. Why does the first ionisation energy increase as we go from left to ri...

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  17. Which out of the N or O has higher electron gain enthalpy?

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  18. Which of the following pair would have larger size? a.K or K^(o+) , ...

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  19. Atomic number (Z) of elements is 108. Write its electronic configurati...

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  20. Out of Na and Mg which has higher second ionisation energy?

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