Atomic radius generally increases as we move down a group and from left to right across a period O up a group and from right to left across a period O up a group and from left to right across a period down a group; the period position has no effect down a group and from right to left across a period

Atomic radius generally increases as we move down a group and from left to right across a period O up a group and from right to left across a period O up a group and from left to right across a period down a group; the period position has no effect down a group and from right to left across a period

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 53A

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Similar questions

Consider the following statement "The ionization energy for the potassium atom is negative, because when K loses an electron to become K +, it achieves a noble gas electron configuration." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the incorrect information and explain.
6.80 Describe how valence electron configurations account for some of the similarities in chemical properties among elements in a group.
The energy needed to remove one electron from a gaseous potassium atom is only about two-thirds as much as that needed to remove one electron from a gaseous calcium atom, yet nearly three times as much energy as that needed to remove one electron from K+ as from Ca+ . What explanation can you give for this contrast? What do you expect to be the relation between the ionization energy of Ca+ and that of neutral K?
Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.
Account for the fact that the line that separates the metals from the nonmetals on the periodic table is diagonal downward to the right instead of horizontal or vertical.
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
For each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Sm or Sm3+ (b) Mg or Ca (c) I orXe (d) Ge or As (e) Sr+ or Rb
Identify the atom or ion corresponding to each of the following descriptions: (a) an atom with ground-state electron configuration [Kr]4d105s25p1 (b) an ion with charge 22 and ground-state electron configuration [Ne]3s23p6 (c) an ion with charge +4 and ground-state electron configuration [Ar]3d3
We expect the atomic radius to increase going down a group in the periodic table. Can you suggest why the atomic radius of hafnium breaks this rule? (See data below.)
Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.