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 fromProcedure 1.ReactionObservation (Color)Light orangeLight pinkBr, water + NaClBr, water + NalCl2 water + NaBrOrange to brownDark pinkDark pinkDark pinkCl, water + Nal2 water + NaBr12 water+ NaCI TThe yellow is the halogens.

A question based on redox reaction, 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: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 11STP

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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

1. Record your observations (or copy and paste your table) for the halogens and halides from
Procedure 1.
Reaction
Observation (Color)
Light orange
Light pink
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+ NaCI T
The yellow is the halogens.

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