Presentation on theme: "Unit 7 Chemical Reactions Chapter 7 pp. 175 - 200."— Presentation transcript:
Unit 7 Chemical Reactions Chapter 7 pp. 175 - 200
What is a chemical reaction? It is the process by which atoms of one or more substances are rearranged to form NEW different substances. Consider the following demonstration… What happens when an antacid tablet is added to water? Lets take a look…
How can you tell if a chemical reaction has occurred? Temperature change – Adding a strong acid to water causes a dramatic increase in temp. Color change – A rusty nail changes from silver to orange/brown Odor – The smell of rotten eggs when you burn sulfur in the lab Gas bubbles – When baking bread, the bread rises because of gas production Precipitate or formation of a solid – A solid appears after adding two liquids together
Chemical Equations In every chemical equation there are three parts. 1.Reactants 2.Yield symbol or 3.Products Reactant 1 + Reactant 2 Product 1 + Product 2 Sometimes there are symbols that go above the Yield symbol. Often times these symbols represent catalysts or energy added or released from a reaction.
Symbols in chemical equations Physical States (s) - solid (l) - liquid (g) - gas (aq) – aqueous or in solution Symbols above the Heat – heat energy Δ – energy (often heat) - electricity Sy – Elemental symbol acting as a catalyst
An important reminder… The following elements exist as diatomic molecules in their natural state. H 2 F 2 Cl 2 Br 2 I 2 O 2 N 2
Representing Chemical Reactions Word Equations Writing equations in the English language to explain the process of a chemical reaction. Example: iron (s) + chlorine (g) iron(III)chloride (s) Solid Iron and gaseous chlorine react to produce solid iron(III)chloride.
Writing Word Equations Lets look at another example. Sodium (s) + Water (l) Sodium Hydroxide (aq) + Hydrogen (g) Now you try to write it correctly in English. Answer: Solid sodium and liquid water reacted to form aqueous sodium hydroxide and hydrogen gas.
Writing Skeleton Equations Word equations are useful for describing chemical reactions, however, they are cumbersome and lack important information. Lets look at an example of the earlier iron reaction… iron (s) + chlorine (g) iron(III)chloride (s) Skeleton equations use symbols in place of the names of atoms and compounds Fe (s) + Cl 2(g) FeCl 3(s)
Writing Skeleton Equations Lets look at an example: Carbon (s) + Sulfur (s) Carbon disulfide (l) Now you try to write the skeleton equation Answer: C (s) + S (s) CS 2 (l)
Practice Write the following as Word Equations hydrogen (g) + bromine (g) hydrogen bromide (g) carbon monoxide (g) + oxygen (g) carbon dioxide (g) Write the following as Skeleton Equations Solid barium and oxygen gas react to produce solid barium oxide. Solid iron and aqueous hydrogen sulfate (sulfuric acid) react to produce aqueous iron(III)sulfate and gaseous hydrogen.
Answers Hydrogen gas reacted with gaseous bromine producing gaseous hydrogen bromide. Gaseous carbon monoxide reacted with oxygen gas to produce carbon dioxide gas. Ba (s) + O 2(g) BaO (s) Fe (s) + H 2 SO 4(aq) Fe 2 (SO 4 ) 3(aq) + H 2(g)
Chemical Reactions Both of these types of equations are useful, but still something is missing… When a reaction occurs it is important to remember the Law of Conservation of Mass. Mass (atoms) cannot be created nor destroyed. Therefore, the previous types of equations wont do for chemical analysis.
Balanced Chemical Equations Lets look at the iron equation one more time. Fe (s) + Cl 2(g) FeCl 3(s) Notice anything strange? Where did the extra chlorine atom come from in the iron(III)chloride? To accurately represent this equation it is important to show that the number of atoms in the reactants is equal to the atoms of product.
Balancing Chemical Equations Whenever the number of atoms of reactant(s) are equal to the number of atoms of product(s) we say that the equation is a Balanced Chemical Equation. How do we get the reactants and products to balance out? Coefficients – (different than subscripts!) Whole numbers placed in front of an atom or compound to indicate more than one of each.
Balancing Chemical Equations Lets look at the previously discussed iron equation when it is balanced… 2Fe (s) + 3Cl 2(g) 2FeCl 3(s) Notice that there are 2 atoms of iron and 6 atoms of chlorine. (or 3 molecules of chlorine gas) The same can be said for the atoms of iron and chlorine in the iron(III)chloride compound.
Steps for balancing equations. Step 1: Write the skeleton equation for the reaction. Step 2: Count the atoms of the elements in the reactants. Step 3: Count the atoms of the elements in the products. Step 4: Change the coefficients to make the number of atoms of each element equal on both sides of the equation. Step 5: Write the coefficients in their lowest possible ratio. Step 6: Check your work.
Steps for balancing equations example. Hydrogen gas reacted with chlorine gas to produce hydrogen chloride. Step 1: H 2(g) + Cl 2(g) HCl (g) Step 2: H 2 + Cl 2 (2 atoms of H) (2 atoms of Cl) Step 3: HCl ( 1 atom H + 1 atom Cl) Step 4: H 2(g) + Cl 2(g) 2HCl (g) (2 atoms H) (2 atoms Cl) (2 atoms H +2 atoms Cl)
Steps for balancing equations example. Step 5: The ratio 1 hydrogen molecule to 1 chlorine molecule to 2 hydrogen chloride molecules (1:1:2) is the lowest possible ratio because the coefficients cannot be reduced and still remain whole numbers. Step 6: Make sure the chemical formulas are written correctly. Then, check that the number of atoms of each element is equal on both sides of the equation. Thats it!
OK, maybe thats not all… Sometimes equations are more complex than others, especially when polyatomic ions are involved. Here are a couple of extra tips. 1. Begin balancing with the most complex formula. 2. Balance polyatomic ions as a single unit.
Practice Time Write the balanced chemical equations for the following: Aqueous sodium hydroxide and aqueous calcium bromide react to produce solid calcium hydroxide and aqueous sodium bromide. Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas.
Why differentiate? When you go to the library, you see many different types of books that are organized in a way to help you find them… –Fiction, Nonfiction, Mysteries, Biographies, History, Fantasy, etc. Like books, there are also many different kinds of chemical reactions and scientists need a way to organize them.
Types of Chemical Reactions Synthesis Combustion Decomposition Single-replacement Double-replacement
Synthesis Reactions A chemical reaction in which two or more substances react to produce a single product. A + B AB Example 1 - 2 elements 2Fe (s) + 3Cl 2(g) 2FeCl 3(s) Example 2 - 2 compounds CaO (s) + H 2 O (l) Ca(OH) 2(s) Example 3 - 1 element + 1 compound 2SO 2(g) + O 2(g) 2SO 3(g)
Combustion Reactions Oxygen combines with a substance and releases energy in the form of heat and light. Example 1 2H 2(g) + O 2(g) 2H 2 O (g) Example 2 C (s) + O 2(g) CO 2(g) Notice that both of these reactions are also Synthesis reactions as well...
Combustion contd. Not all combustion reactions are also synthesis types. Sometimes oxygen will react with compounds called hydrocarbons that contain carbon and hydrogen. In these reactions, such as the one below, carbon dioxide and water are produced. CH 4(g) + 2O 2(g) CO 2(g) + 2H 2 O (g) This is the same type of reaction that powers a car. In that instance octane (C 8 H 18 ), another hydrocarbon, is a reactant, but the products are the same.
Decomposition Reactions A reaction in which a single compound breaks down into two or more elements or new compounds. AB A + B Example NH 4 NO 3(s) N 2 O (g) + 2H 2 O (g) These types of reactions often require an energy source, such as heat, light, or electricity, to occur.
Decomposition contd. One of the best examples of decomposition is in automobile airbags. Airbags are inflated when an electrical signal starts a reaction with sodium azide (NaN 3 ) pellets within the bag. These pellets produce nitrogen gas which quickly inflates the bag. 2NaN 3(s) 2Na (s) + 3N 2(g)
Single Replacement Reactions Atoms of one element replace atoms of another element in a compound. When studying this type of reaction we must look closely at the element that we believe will replace another element Some metals are more reactive than others. If a metal is more reactive than the element it is replacing, it will take its place. IF a metal is less reactive than the element it is replacing, ultimately, it will not replace it.
Single Replacement Contd. How do we know if one element will replace another? Activity Series of Metals – A table indicating the general level of reactivity of different elements
Single Replacement Example 1 Mg + Zn(NO 3 ) 2 Mg(NO 3 ) 2 + Zn Example 2 Mg + 2AgNO 3 Mg(NO 3 ) 2 + 2Ag Example 3 Mg + LiNO 3 No Reaction
Double Replacement An exchange of positive ions between two compounds in a chemical reaction Generally, these types of reactions occur in solution Often times, in these types of reactions, one of the products will come out of solution as either, a gas, a pure liquid, or a solid.
Double Replacement Contd. Example 1 – One product is soluble, the other is a precipitate. Na 2 S (aq) + Cd(NO 3 ) 2(aq) CdS (s) + 2 NaNO 3(aq) Example 2 – One product is a gas that bubbles out of the mixture 2NaCN (aq) + H 2 SO 4(aq) 2HCN (g) + Na 2 SO 4(aq) Example 3 – One product is a molecular compound, such as water, which separates from the compounds in solution. Ca(OH) 2(aq) + 2HCl (aq) CaCl 2(aq) + 2H 2 O (l)