Activity series of metals

In this case, the direction of the arrows show that Brafaq) and Cl (aq) stay as they are. The conclusion is that there is no reaction at room temperature. 

Using the standard reduction potentials In Table 7.1, determine whether the following reactions may occur  

The more negative the standard electrode potential, of a redox couple M (aq)/M(s), the more powerful a reducing agent is that metal. This means it is a more reactive metal because it loses electrons more easily. We can arrange the metals in order of reducing power, producing an activity series of metals (Table 7.2). The metals at the top of the series are more reactive than those below. 

A metal in solution can react with a metal ion that appears below it in the table. Hydrogen is included so that the reactivity of metals with aqueous acids may be worked out when a metal above hydrogen is added to an acidic solution, a reaction will occur and hydrogen gas is given off. 

Never mix strongly reducing metals, such as potassium, with acid solutions — the reactions are extremely violent. 

Ionic equations can also be balanced using the change-in-oxidation-number method shown in Example 17.6. To illustrate this method, let s use the equation from Example 17.10. 

Balance this equation using the change-in-oxidation-number method  

Assign oxidation numbers and balance the charges with Cr (reduction) 

Equalize the loss and gain of electrons, by multiplying the oxidation step by 3  

Balance electrically. Because the solution is basic, use OH to balance charges. The charge on the left side is -2 and on the right side is 0. Add 2 OH ions to the right side of the equation  

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Table 6.1 Activity Series of Metals in Aqueous Solution...

Zinc metal reacts spontaneously with an aqueous solution of copper sulfate when they re placed in direct contact. Zinc, being a more reactive metal than copper (it s higher on the activity series of metals presented in Chapter 8), displaces the copper ions in solution. The displaced copper deposits itself as pure copper metal on the surface of the dissolving zinc strip. At first, the reaction may appecir to be a simple single replacement reaction, but it s also a redox reaction. 

Using your an ox and red cat mnemonics, you know that the anode is the site of aluminum (Al) oxidation, while the cathode is the site of tin (Sn) reduction. This idea is also apparent from the activity series of metals (see Chapter 8), which shows that aluminum is far more reactive than tin. 

You actually need to evaluate the second portion of this question first. A simple glance at the activity series of metals in Chapter 8 tells you that cadmium is more active than tin, so it must be cadmium that is oxidized and makes up the anode, and tin must be reduced and make up the cathode. The half-reactions are therefore... 

Use the activity series of metals (Table 4.3) to predict the outcome of each of the following reactions. If no reaction occurs, write N.R. 

Not every element will take the place of another element in a compound, though. Whether the reaction will take place or not depends on the activity of the two elements. For metals, there is a list called the activity series of metals that lists the metals in... 

Activity series Of metals A table listing metals in order of decreasing activity. 

Describe how to use the activity series of metals and the activity series of halogens. 

Refer to Appendix A for a more complete activity series of metals and of halogens. 

Redox Sequence. Even the most well-known reactions of metals with diluted acid solutions to form salt solutions and hydrogen gas can also be interpreted as redox reactions or electron transfers (see E8.5) metal atoms are oxidized, H + (aq) ions of acid solutions are reduced to Ei atoms, these combine to form H2 molecules and the hydrogen gas is released in the form of small bubbles. Because copper and the noble metals are not soluble in diluted acids, the redox pair Ei + /H is placed in a location before the copper pair in the Activity Series of Metals. The name metal series (sequence) can be replaced by the general name redox series (sequence). A partial listing is shown as follows ... 

Activity series of metals and halogens can be used to predict if single-replacement reactions will occur. 

This is an example of direct electron transfer. Zinc gives up two electrons (becomes oxidized) to the Cu ion that accepts the electrons (reducing it to copper metal). In Chapter 8,1 show you that nothing happens if you place a piece of copper metal into a solution containing Zn because zinc gives up electrons more easily than copper. I also show you the activity series of metals that allows you to predict whether or not a displacement (redox) reaction will take place. 

Activity Series of Metals Electrol57tic and Voltaic Cells... 

Zinc is a more reactive metal than copper, so when corrosion occurs, the zinc preferentially reacts. Zinc is above hydrogen in the Activity Series of Metals copper is below hydrogen. 

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