Explanation Strontium (Sr) is an alkaline earth metal which belongs to group (2) while the antimony is a metalloid which belongs to group 15. Since, both the elements belong to same period 5, so the general periodic trend of reducing character will be applied on them. In a period, generally the reducing character decreases from left to right due to the increase in nuclear charge. This increasing nuclear charge decreases the tendency to lose electrons. Hence, the strontium situated in extreme left of the period will be more reducing in nature as compared to the antimony. So, strontium will be better reducing agent than antimony. As per the feasibility of reaction: 2 S b 3 + ( a q )

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Author: John E. McMurry, Robert C. Fay, Jill Kirsten Robinson

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Chapter 4, Problem 4.113SP

Interpretation Introduction

To determine:

The better reducing agent between strontium and antimony and the feasibility of given reaction:

2Sb3+(aq)+3Sr(s)→2Sb(s)+3Sr+2(aq)

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Chapter 4, Problem 4.112SP

Chapter 4, Problem 4.114SP

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The better reducing agent between strontium and antimony and the feasibility of given reaction: 2 S b 3 + ( a q ) + 3 S r ( s ) → 2 S b ( s ) + 3 S r + 2 ( a q )

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To determine: The better reducing agent between strontium and antimony and the feasibility of given reaction:2Sb3+(aq)+3Sr(s)→2Sb(s)+3Sr+2(aq)

Want to see the full answer?

Chapter 4 Solutions

To determine:

The better reducing agent between strontium and antimony and the feasibility of given reaction:

2Sb3+(aq)+3Sr(s)→2Sb(s)+3Sr+2(aq)