Consider Figure 4.19 in the text. Why is it that the formulas for ionic compound are always empirical formulas?
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Bonds Electrostatic: the ability of an object to acquire an electron o Holds matter together o Trend on the Periodic Table: Increases going down the columns Increases going across the rows Phases: solid, liquid, and gas o Spacing between molecules Gas > Solid > Liquid Forces: o London (induced dipole) Every molecule have these forces Very weak Larger molecular weight = more electrons Larger the molecule = Stronger the force BP determined by molecular weight Ex. CH4, CH3CH, CH3CH2CH3 CH3CH2CH3 > CH3CH > CH4 o If they are similar Molecules
Textbook: Introductory Chemistry: A Foundation
Author: Steven S. Zumdahl, Donald J. DeCoste
This textbook survival guide was created for the textbook: Introductory Chemistry: A Foundation, edition: 7. Introductory Chemistry: A Foundation was written by and is associated to the ISBN: 9781439049402. Since the solution to 12 from 8 chapter was answered, more than 260 students have viewed the full step-by-step answer. The answer to “Consider Figure 4.19 in the text. Why is it that the formulas for ionic compound are always empirical formulas?” is broken down into a number of easy to follow steps, and 19 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 21 chapters, and 2203 solutions. The full step-by-step solution to problem: 12 from chapter: 8 was answered by , our top Chemistry solution expert on 03/14/18, 08:03PM.