Metals single-replacement reactions

A metal will not always replace another metal in a compound dissolved in water. This is because metals differ in their reactivities. A metal s reactivity is its ability to react with another substance. In Figure 10-10 you see an activity series of some metals. This series orders metals by their reactivity with other metals. Single-replacement reactions like the one between copper and aqueous silver nitrate determine a metal s position on the list. The most active... 

In this activity, you will use a few metals, their compounds, and dilute hydrochloric acid to show single-replacement reactions and construct an activity series. 

The standard redox potential of the reaction CeS+ + 3e Ce is -2.2336 V. The metal undergoes single replacement reactions, displacing less electropositive metals from their salts in solution or melt ... 

Iron also exhibits single replacement reactions, precipitating less electropositive metals out of their salt solutions. Thus, sohd iron can reduce many metals, such as copper, silver, gold, mercury, tin and nickel ... 

Mercury dimethyl undergoes single replacement reactions with several metals such as alkali and alkaline earth metals, zinc, aluminum, tin, lead and bismuth forming their corresponding dialkyls. 

Violent reactions can occur with many metal hahdes. For example, with zinc halides or iron halides, single replacement reactions take place. Such potassium-metal halide mixtures can react violently when subjected to mechanical shock. 

Simple Carbohydrate monosaccharides such as glucose, fructose, and galactose that cannot be broken down by water Single Replacement Reaction type of chemical reaction in which one element replaces another in a compound Smelting to melt an ore in order to refine a metal from the ore... 

Single replacement reactions in which metals replace other metals cire especially common. Not all single replacement reactions occur as written, though. You sometimes need to refer to a chart called the activity series to determine whether such a reaction will take place. 

Table 8-2 presents the activity series. To determine whether a single replacement reaction will occur, compare the two metals in the reaction ... 

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. 

These reactions are part of a larger category of reactions known as redox reactions (redox is short for oxidation-reduction). Sometimes these are called displacement reactions. These are chemical reactions in which atoms of one element replace the atoms of a second element in a compound. A general equation for a single-replacement reaction involving a metal (A), replacing a metallic cation in solution (B) is ... 

The reaction between lithium and water is one type of single-replacement reaction in which a metal replaces a hydrogen in a water molecule. Another type of single-replacement reaction occurs when one metal replaces another metal in a compound dissolved in water. For example. Figure 10-9 shows a single-replacement reaction occurring when a spiral of pure copper wire is placed in aqueous silver nitrate. The shiny crystals that are accumulating on the copper wire are the silver atoms that the copper atoms replaced. 

In single-replacement reactions, a metal may replace hydrogen in water, a metal may replace another metal in a compound dissolved in water, and a non-metal may replace another nonmetal in a compound. 

A single replacement reaction occurs when an element reacts with a compound in such a way that the element replaces an ion of a similar element from the compound. In order for the replacement to occur, the elemental reactant must be more reactive than the elemental product. The general format for a single displacement reaction, when the elemental reactant is a metal, is ... 

Interpreting Data Write the balanced equation for the single-replacement reaction between magnesium and copper(ll) chloride that occurred in step 2. Which metallic element, Cu or Mg, has the greater tendency (or oxidation potential) to lose electrons ... 

An oxidation-reduction reaction is one in which electrons are transferred from one reactant to another. They are often called redox reactions for short. Oxidation is the loss of one or more electrons by a species. The species losing electrons is oxidized. Reduction is the gain of one or more electrons by a species, and that species is reduced. Oxidation and reduction always occur simultaneously. The single-displacement reaction of copper metal with silver nitrate solution is both a single replacement reaction and an oxidation-reduction reaction. 

Single-replacement reaction carbon replaces iron in Fe203 forming C02 and freeing iron metal. 

Single-replacement reaction zinc replaces Pb in Pb(N03)2, forming Zn(N03)2 and lead metal. 

The first category of single-replacement reactions is one metal replacing another in a compound. Aluminum must replace nickel in NiCl2 to produce nickel metal, Nifo), and aluminum chloride (Al3+ + Cl" = AlCl3). Place the formula for aluminum chloride and the symbol for nickel metal in the blanks, and balance. The completed equation is ... 

Figure 9.13 An activity series, similar to the series shown here for various metals and halogens, is a useful tool for determining whether a chemical reaction will occur and for determining the result of a single-replacement reaction. 

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

Figure 8.15 Reaction of sodium with water. A single-replacement reaction occurs when sodium, an element, reacts with water, a compound. The metal sodium appears to replace hydrogen in water, 2 Na + 2 HOH (A + BX) 2 NaOH + Hj (AX + B). The... 

Acids react with some metals to form hydrogen gas in what is termed a single replacement reaction. In a single replacement reaction, one element is released from a formula and the remaining element combines with the reacting element. 

Acids react with certain metals to produce hydrogen gas (H2) and a salt. Active metals include potassium, sodium, calcium, magnesium, aluminum, zinc, iron, and tin. In these single replacement reactions, the metal ion replaces the hydrogen in the acid. 

In the activity series, the metals that lose electrons most easily are placed at the top, and the metals that do not lose electrons easily are at the bottom. Thus the metals that are more easily oxidized are above the metals whose ions are more easily reduced (see Table 15.3). Active metals include K, Na, Ca, Mg, Al, Zn, Fe, and Sn. In single replacement reactions, the metal ion replaces the H in the acid. Metals listed below H2( ) will not react with H from acids. 

Use the above activity series to predict the single-replacement reaction that will occur between aluminum metal and lead(II) nitrate (Pb(N03)2) in a water solution and write its balanced chemical equation. 

Aluminum is above lead in the activity series and therefore is more active. It will replace lead in its compounds in water solution. A single-replacement reaction will take place to form the nitrate of aluminum, a group 3A metal. The skeleton equation is shown below. 

In your previous chemistry course, you compared the reactivities of metals. You may recall that, when a piece of zinc is placed in an aqueous solution of copper(II) sulfate, the zinc displaces the copper in a single displacement reaction. This reaction is shown in Figure 10.1. As the zinc dissolves, the zinc strip gets smaller. A dark red-brown layer of solid copper forms on the zinc strip, and some copper is deposited on the bottom of the beaker. The blue colour of the solution fades, as blue copper(ll) ions are replaced by colourless zinc ions. 

Magnesium exhibits single displacement reactions, thus replacing lower metals in electrochemical series from their salt solutions or melt. For example, magnesium will replace iron from molten iron(II) chloride forming magnesium chloride ... 

It has already been stated that chromium complexes of tridentate metallizable azo compounds occupy their position as the single most important class of metal complex dyestuffs because of their high stability. It should be noted, however, that in this context the term stability is not used in the thermodynamic sense but relates to the kinetic inertness of the complexes.25 Octahedral chromium(III) complexes have a tP electronic configuration and the ligand field stabilization energy associated with this is high.26 Ligand replacement reactions involve either a dissociative... 

In a single displacement reaction, one element in a compound is displaced (or replaced) by another element. Two general reactions represent two different types of single displacement reactions. One type involves a metal replacing a metal cation in a compound, as follows ... 

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