Homework 6 Atomic (Covalent) Radius 1- How and why do atomic radii change as we
ID: 304261 • Letter: H
Question
Homework 6 Atomic (Covalent) Radius 1- How and why do atomic radii change as we move from left to right across a period in the periodic table? From bottom to top within a group? 2- Which member of each of the following pairs would be predicted to have the larger atomic (covalent) radius? a) Si or S b) Si or Sn c) Si or Ga d) Si or Al f) Si or F ) Si or C h) Sr or Sb i) K or Mg e) Si or Mg P or Ge 3- Arrange each of the following series in order of decreasing atomic radi(largest first: a) Na, Be, Mg b) Se, S, As c) Ar, H, Ba, Te, Au, Ag d) K, Ca, Rb, Ti, Br, Cl lonization Energy 1- a) Why is the second ionization energy of an element always larger than the first ionization b) The first ionization energy of Na is low, but the second ionization energy of Na is very high, energy? even higher than the third ionization of Al. Explain this observation.Explanation / Answer
1) From left to right atomic radius decreases in a period. This is because of increase in nuclear attraction and electrons add to the same electronic shell, which makes contraction of atom
From bottom to top in a group atomic radius decreases because of decrease in principle quantum number i.e shell number
2) with the explanation given in question 1 answers to 2nd are
a) silica b)Sn c)Ga d)Al .e) mg f)si g) si h) sb I)K j)Ge
3) a) Na>Mg>Be
b) As>se>S
C)Ba> Au> Ag> Te> Ar>H
As per chegg rules only 1 or 2 questions should be answeere once please repost the other questions .thanks
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