Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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- Write the ground state electron configuration for (a) Mg, Mg2+(b) N, N3- (c) Ti, Ti4+ (d) Sn2+ Sn4+arrow_forwardWhich of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is ls2 2s1 ) is exothermic-that is, removing this electorn gives off energy. d. The He atom is larger than the H+ ion. e. The Al atorn is smaller than the Li atom.arrow_forward1.arrow_forward
- Explain, in terms of Coulombic energy and Exchange energy, why the ground-state electron configuration of Cr is [Ar]4s13d5 instead of [Ar]4s23d4.arrow_forward6. What is the name of the element in the ground state with the shorthand electron configuration of (Kr]Ss24d105p4? Is this element paramagnetic or diamagnetic? Illustrate with a box diagram.arrow_forwardWrite the full electron configuration of the Period 3 elementwith the following successive IEs (in kJ/mol):IE₁=738 ,IE₂=1450 ,IE₃=7732 ,IE₄=10,539 ,IE₅=13,628arrow_forward
- Consider a magnesium (Mg) atom that could have an electronic configuration of either [Ne]3s2 or [Ne]3s13p1. Discuss the following: a) Give one argument for why the [Ne]3s2 configuration might be more stable. b) Give one argument for why the [Ne]3s13p1 configuration might be more stable. c) Which configuration does Mg actually adopt and why?arrow_forward6arrow_forwardUse the periodic table to identify the elements with the following electron configurations. [Xe]6s2 Spell out the full name of the element.arrow_forward
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