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rom the activity list included in this problem, which element will react with Cu?  Which element/ion is the most resistant to reduction? Sn(s) ---> Sn2+ (aq)+ 2e¯ Pb(s0  --->Pb2+ (aq) +2e- H2(g) ---> 2H+ (aq)+2e- Cu(s) --->Cu2+ (aq)+2e- From the activity list included in this problem, which element/ion is the most difficult to oxidize? Li(s) --->Li+ (aq)+ e-

rom the activity list included in this problem, which element will react with Cu?  Which element/ion is the most resistant to reduction? Sn(s) ---> Sn2+ (aq)+ 2e¯ Pb(s0  --->Pb2+ (aq) +2e- H2(g) ---> 2H+ (aq)+2e- Cu(s) --->Cu2+ (aq)+2e- From the activity list included in this problem, which element/ion is the most difficult to oxidize? Li(s) --->Li+ (aq)+ e-

Chemistry
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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From the activity list included in this problem, which element will react with Cu?  Which element/ion is the most resistant to reduction?

Sn(s) ---> Sn2+ (aq)+ 2e¯

Pb(s0  --->Pb2+ (aq) +2e-

H2(g) ---> 2H+ (aq)+2e-

Cu(s) --->Cu2+ (aq)+2e-

From the activity list included in this problem, which element/ion is the most difficult to oxidize?

Li(s) --->Li+ (aq)+ e-

K(s) --->K+ (aq)+e-

Ca(s) --->Ca2+ (aq)+2e-

Na(s) --->Na+ (aq)+e-

 

 

 

 

 

 

**Activity Series:** 1. \( \text{Li}(s) \rightarrow \text{Li}^+(aq) + e^- \) 2. \( \text{K}(s) \rightarrow \text{K}^+(aq) + e^- \) 3. \( \text{Ca}(s) \rightarrow \text{Ca}^{2+}(aq) + 2e^- \) 4. \( \text{Na}(s) \rightarrow \text{Na}^+(aq) + e^- \) **Explanation:** This series lists the activity of metals based on their ability to lose electrons (oxidation) and form positive ions in aqueous solutions. The equations represent the oxidation half-reactions for lithium, potassium, calcium, and sodium. Each metal solid (\(s\)) is converted into its ionized form (\(aq\)) with the release of electrons. Calcium uniquely releases two electrons in its oxidation process, forming a \(Ca^{2+}\) ion.
Transcribed Image Text:**Activity Series:** 1. \( \text{Li}(s) \rightarrow \text{Li}^+(aq) + e^- \) 2. \( \text{K}(s) \rightarrow \text{K}^+(aq) + e^- \) 3. \( \text{Ca}(s) \rightarrow \text{Ca}^{2+}(aq) + 2e^- \) 4. \( \text{Na}(s) \rightarrow \text{Na}^+(aq) + e^- \) **Explanation:** This series lists the activity of metals based on their ability to lose electrons (oxidation) and form positive ions in aqueous solutions. The equations represent the oxidation half-reactions for lithium, potassium, calcium, and sodium. Each metal solid (\(s\)) is converted into its ionized form (\(aq\)) with the release of electrons. Calcium uniquely releases two electrons in its oxidation process, forming a \(Ca^{2+}\) ion.
**Activity Series** The following series of chemical equations represent the oxidation processes for different elements and the formation of their ions in aqueous solutions: 1. **Tin (Sn)** \[ \text{Sn(s)} \rightarrow \text{Sn}^{2+}\text{(aq)} + 2\text{e}^{-} \] 2. **Lead (Pb)** \[ \text{Pb(s)} \rightarrow \text{Pb}^{2+}\text{(aq)} + 2\text{e}^{-} \] 3. **Hydrogen (H\(_2\))** \[ \text{H}_{2}\text{(g)} \rightarrow 2\text{H}^{+}\text{(aq)} + 2\text{e}^{-} \] 4. **Copper (Cu)** \[ \text{Cu(s)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\text{e}^{-} \] In the activity series, metals and hydrogen are listed based on their ability to displace other elements in compounds, with more reactive elements listed above less reactive ones. The higher up in the series, the stronger the reducing agent.
Transcribed Image Text:**Activity Series** The following series of chemical equations represent the oxidation processes for different elements and the formation of their ions in aqueous solutions: 1. **Tin (Sn)** \[ \text{Sn(s)} \rightarrow \text{Sn}^{2+}\text{(aq)} + 2\text{e}^{-} \] 2. **Lead (Pb)** \[ \text{Pb(s)} \rightarrow \text{Pb}^{2+}\text{(aq)} + 2\text{e}^{-} \] 3. **Hydrogen (H\(_2\))** \[ \text{H}_{2}\text{(g)} \rightarrow 2\text{H}^{+}\text{(aq)} + 2\text{e}^{-} \] 4. **Copper (Cu)** \[ \text{Cu(s)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\text{e}^{-} \] In the activity series, metals and hydrogen are listed based on their ability to displace other elements in compounds, with more reactive elements listed above less reactive ones. The higher up in the series, the stronger the reducing agent.
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