Use the activity series of metals to write a balanced chemical equation for each single-replacement reaction? K is much more reactive than Ag, so that the reaction should proceed in the opposite direction.
There are many different types of chemical reactions. Chemists have classified the many different reactions into general categories. The chemical reactions we will explore are a representation of the types of reactions found in each group.
Synthesis Reaction Combination Reaction In a synthesis reaction, two or more substances combine to form a new compound. This type of reaction is represented by the following equation.
The following examples are representative of synthesis reactions. Aluminum and Bromine Formation of Aluminum Bromide: When Al is placed on the surface of liquid Br2 an exothermic reaction occurs. The ionic product, AlBr3, can be observed on the watch glass after the reaction.
Sodium and Chlorine Formation of Sodium Chloride: Molten sodium burns when it is put into a container of chlorine gas. In the reaction a sodium ion loses an electron to form a sodium cation and a chlorine atom simultaneously gains an electron to form a chloride anion. The product of the reaction is the ionic compound sodium chloride, which is the white solid observed.
Zinc and Oxygen Formation of Zinc Oxide: Oxidation is a loss of electrons and reduction is a gain of electrons. The oxidation of metallic Zn by O2 to form ZnO s is illustrated at the molecular level. The transfer of electrons from Zn to O2 is shown. Atoms can be observed to change as they are oxidized or reduced, respectively to their ionic forms.
When a small piece of Na is added to a solution containing an indicator, evidence of the reaction can be observed by the change in the color of the solution as NaOH is formed, by the melting of the Na and by the movement of the Na caused by formation of hydrogen gas.
K is more reactive than Na as demonstrated by its reaction with water.
This reaction produces enough heat to ignite the H2 produced.Now try writing some net ionic equations, using the rules above. Example. This is a double replacement reaction.
Both compounds are soluble, so everything ionizes. If anything is formed, This one is a single replacement, so you need to consider the activity series.
Since halogens are involved, you can determine their activity by using. Single replacement reactions we use an activity series to predict if they will occur.
For a reaction to proceed to completion all of the reactants must mix: they may need to be stirred, or heated to assist in the process of them reacting.
In a single-replacement reaction (displacement reaction) one element replaces a similar element in the compound. Single-replacement reactions can be represented by the following equations.
Students learn about safety procedures, the names of equipment, chemical reactions (in this example-a single replacement reaction), evidence of chemical reactions and their characteristics (ie, endothermic or exothermic, producing a gas, color change, or precipitate).
balanced chemical equation for each reaction, showing the product(s), and classify the reaction as to type: combustion, oxidation, synthesis, decomposition, single replacement, double replacement.
Zinc and Lead (II) nitrate react to form Zinc Nitrate and Lead.
Zn + Pb(NO 3) 2 Zn(NO 3) 2 + Pb Single Replacement 2. Aluminum Bromide and Chlorine gas react to form Aluminum Chloride and Bromine gas. 2AlBr 3 + 3 Cl 2 powder is created in an exothermic reaction.