Rank the halogens by oxidizing strengthand the halide ions by reducing strengthfrom strongest to weakest, write balancednet ionic equations for the combinationand which equations are the reductionpotentials for the reactions? 1. Record your observations (or copy and paste your table) for the halogens and halides fromProcedure 1.Observation (Color)Light orangeLight pinkReactionBr, water + NaClBr, water + NalCl2 water + NaBrOrange to brownDark pinkDark pinkDark pinkCl, water + Nal2 water + NaBr12 water + NaCITThe yellow is the halogens.

A question based on reduction potential, which is to be accomplished.

Rank the halogens by oxidizing strength and the halide ions by reducing strength from strongest to weakest, write balanced net ionic equations for the combination and which equations are the reduction potentials for the reactions?

Rank the halogens by oxidizing strength and the halide ions by reducing strength from strongest to weakest, write balanced net ionic equations for the combination and which equations are the reduction potentials for the reactions?

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Rank the halogens by oxidizing strength
and the halide ions by reducing strength
from strongest to weakest, write balanced
net ionic equations for the combination
and which equations are the reduction
potentials for the reactions?

1. Record your observations (or copy and paste your table) for the halogens and halides from
Procedure 1.
Observation (Color)
Light orange
Light pink
Reaction
Br, water + NaCl
Br, water + Nal
Cl2 water + NaBr
Orange to brown
Dark pink
Dark pink
Dark pink
Cl, water + Nal
2 water + NaBr
12 water + NaCIT
The yellow is the halogens.

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