Unit 4: TOXINS Stoichiometry, Solution Chemistry, and Acids and Bases Living By Chemistry Unit 4: TOXINS Stoichiometry, Solution Chemistry, and Acids and Bases

In this unit you will learn: how toxins are defined how chemists determine toxicity the mechanisms by which toxic substances act in our bodies and what this has to do with chemical reactions

Section I: Toxic Changes Lesson 1 Toxic Reactions Lesson 2 Making Predictions Lesson 3 Spare Change Lesson 4 Some Things Never Change Lesson 5 Atom Inventory Lesson 6 What’s Your Reaction?

Lesson 1: Toxic Reactions Chemical Equations

ChemCatalyst 1. What toxins have you encountered in your life? 2. How can toxins enter the body? 3. How can toxins harm you?

Key Question How do chemists keep track of changes in matter?

You will be able to: complete basic translations of chemical equations give a basic definition of a toxin

Prepare for the Demonstration (cont.) Hydrochloric acid is corrosive. Wear safety goggles. Have extra baking soda on hand for spills. HCl(aq) + NaHCO3(aq)  NaCl(aq) + H2O(l) + CO2(g)

Discussion Notes HCl(aq) + NaHCO3(aq)  NaCl(aq) + H2O(l) + CO2(g) The chemical equation represents a change in matter using symbols and formulas.

Discussion Notes (cont.) Toxins can enter the body in a limited number of ways. Toxins often react with water in the human body. Toxins may be molecular, ionic, or metallic substances.

Wrap Up How do chemists keep track of changes in matter? Chemical equations help chemists keep track of the substances involved in chemical changes. Chemical equations use chemical formulas to indicate the reactants and products of chemical changes. They also show what phase a compound is in. Toxins are substances that interact with living organisms and cause harm.

Check-in Consider this reaction between sodium cyanide and a solution of hydrochloric acid: NaCN(s)  HCl(aq)  NaCl(aq)  HCN(g) Write an interpretation of the chemical equation. Sodium cyanide is highly toxic. What is the most likely way it will enter the body?

Lesson 2: Making Predictions Observing Change

ChemCatalyst Consider this chemical equation: AgNO3(aq)  KCl(aq)  KNO3(aq)  AgCl(s) a) What do you expect to observe if you carry out this reaction in a laboratory? b) Write an interpretation of the chemical equation, describing what is taking place.

Key Question How can you predict what you will observe based on a chemical equation?

You will be able to: relate chemical equations to real-world observations make predictions based on chemical equations

Prepare for the Lab Work in groups of four. Wear safety goggles at all times. Do not touch the dry ice with your fingers. It causes burns. NaOH, Ca(OH)2, and NH4OH can irritate or burn skin. In case of a spill or contact with skin, rinse with large amounts of water.

Discussion Notes AgNO3(aq)  KCl(aq)  KNO3(aq)  AgCl(s)

Discussion Notes (cont.) Chemical equations contain certain information that you can use to predict what you might observe if a procedure is performed. Sometimes change is described by more than one chemical equation. Chemical equations allow you to track changes in matter on an atomic level. There is some information that a chemical equation can’t provide.

Wrap Up How can you predict what you will observe based on a chemical equation? Chemical equations allow chemists to predict and track changes in matter. They indicate how many products are formed, what those products are, and the phase of each product. Observations of chemical procedures provide information not covered by a chemical equation (and vice versa). Observations alone cannot tell you what substances are present.

Check-in Examine this chemical equation. Write an interpretation of the chemical equation, describing what is taking place. CaCl2(aq) + 2NaOH(aq)  Ca(OH)2(s)  2NaCl(aq)

Lesson 3: Spare Change Physical Versus Chemical Change

ChemCatalyst A chunk of blue, solid cobalt (II) chloride, CoCl2, is placed into some water. The water turns from colorless to pink in color. What type of change has taken place? How do you know? Was something new made? Explain.

Key Question How are changes in matter classified?

You will be able to: define physical and chemical change and explain the gray areas between them classify chemical equations as representing physical changes or chemical changes

Discussion Notes Physical changes are changes in the appearance or form of a substance. Chemical changes produce new substances with new properties. Physical change: A change in matter in which a substance changes form but not identity. Chemical change: A change in matter that results in the formation of a new substance or substances with new properties.

Discussion Notes (cont.) CoCl2(s)  CoCl2(aq) CoCl2(aq) + Ca(OH)2(aq)  Co(OH)2(s) + CaCl2(aq) It is not always possible to distinguish between physical and chemical change based on observations alone. It is possible to argue that dissolving a substance in water changes the properties of that substance.

Discussion Notes (cont.) Ionic compounds do not dissolve in the same way as molecular solids. The dissolving of ionic solids can be shown with a type of equation that stresses the formation of ions in solution. CaCl2(s)  CaCl2(aq) CaCl2(s)  Ca2(aq) + 2Cl−(aq)

Wrap Up How are changes in matter classified? Chemical changes involve the formation of new substances. Physical changes, such as phase changes, involve a change in form. Dissolving generally is considered a physical change, but it has something in common with chemical change as well. Chemical equations often provide more straightforward information about the type of change than do mere observations.

Check-in Does this chemical equation describe a physical change or a chemical change? Explain how you can tell. C17H17O3N(s) + 2C4H6O3(l)  C21H21O5N(s) + 2C2H4O2(l)

Lesson 4: Some Things Never Change Conservation of Mass

ChemCatalyst Consider this reaction: a. Describe what you will observe when sodium carbonate, Na2CO3(aq), and calcium chloride, CaCl2(aq), are mixed. b. Will the mass increase, decrease, or stay the same after mixing? Explain. Na2CO3(aq) + CaCl2(aq)  2NaCl(aq) + CaCO3(s)

Key Question How does mass change during a chemical or physical change?

You will be able to: provide evidence that supports the law of conservation of mass

Discussion Notes In the first and second procedures, the mass of the reactants is equal to the mass of the products. In the third procedure, the measured mass decreases slightly because a gas escapes. Matter can be neither created nor destroyed in physical and chemical changes. On the planet there is essentially an unchanging number of atoms.

Discussion Notes (cont.) Mass and weight have different meanings. Because a sample of gas does not appear to weigh much, it is tempting to conclude that gases do not have mass.

Wrap Up How does mass change during a chemical or physical change? Individual atoms are conserved in chemical reactions and physical changes: The number of atoms of each element remains the same from start to finish. Mass is conserved in chemical reactions: The total mass of the products equals the total mass of the reactants.

Wrap Up (cont.) The law of conservation of mass states that matter can be neither created nor destroyed in physical and chemical changes. Matter is conserved. Gases have mass.

Check-in Consider this reaction: Describe what you will observe when copper (II) carbonate, CuCO3(s), and sulfuric acid, H2SO4(aq), are mixed. Will the mass increase, decrease, or stay the same after mixing? Explain. CuCO3(s) + H2SO4(aq)  CO2(g) + CuSO4(aq) + H2O(l)

Lesson 5: Atom Inventory Balancing Chemical Equations

ChemCatalyst Does this equation obey the law of conservation of mass? Why or why not? CuCl2(aq) + Na2S(aq)  CuS(s) + NaCl(aq)

Key Question How do you balance atoms in a chemical equation?

You will be able to: balance a simple chemical equation explain the role of coefficients in chemical equations

Discussion Notes A balanced chemical equation is one that shows the true mathematical relationship between the reactants and the products in a chemical reaction.

Discussion Notes (cont.) CH4(g) + O2(g)  CO2(g) + H2O(g) Inventory of Atoms Reactants Products 1 C 4 H 2 H 2 O 3 O

Discussion Notes (cont.) CH4(g) + O2(g)  CO2(g) + 2H2O(g) Inventory of Atoms Reactants Products 1 C 4 H 2 O 4 O

Discussion Notes (cont.) CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Inventory of Atoms Reactants Products 1 C 4 H 4 O

Discussion Notes (cont.)

Discussion Notes (cont.) There are two types of numbers in a chemical equation: coefficients and subscripts. Coefficients: The coefficients in a chemical equation are the numbers in front of the chemical formulas of the reactants and products. They show the correct ratio in which the reactants combine to form the products. The coefficients in a chemical equation indicate how many “units” of an element or a compound you have.

Wrap Up How do you balance atoms in a chemical equation? In order for matter to be conserved, the number of atoms on both sides of a chemical equation must be equal. When a chemical equation is balanced, it indicates how many molecules or moles of each substance take part in a reaction and how many molecules or moles of the product(s) are produced.

Check-in Balance this equation: Ca(s) + O2(g)  CaO(s)

Lesson 6: What’s Your Reaction? Types of Reactions

ChemCatalyst Consider these reactions: CaCO3(aq)  CaO(aq) + CO2(g) CO2(g) + NaOH(aq)  NaHCO3(aq) How are these two reactions different? How would you describe, in words, what happens to the reactants in each case?

Key Question How do atoms rearrange to form new products?

You will be able to: identify patterns in chemical equations that reflect different types of reactions classify chemical equations as representing combination, decomposition, single exchange, or double exchange reactions

Discussion Notes CaCO3(aq)  CaO(aq) + CO2(g) Combination CO2(g) + NaOH(aq)  NaHCO3(aq) Decomposition CaCO3(aq)  CaO(aq) + CO2(g) Single exchange Cl2(g) + 2NaBr(s)  2NaCl(s) + Br2(l) Double exchange 2AgCl(s) + BaBr2(aq)  2AgBr(s) + BaCl2(aq)

Discussion Notes (cont.) Combination A + B  AB Decomposition AB  A + B Single exchange A + BC  AC + B Double exchange AB + CD  AD + CB

Discussion Notes (cont.) Chemical reactions can be divided into categories based on how the atoms in the reactants rearrange to form the products. Combination reaction: Several reactants combine to form a single product. Combination reactions are easy to spot because there is only one compound on the product side of the equation. The general reaction can be written as A  B  AB.

Discussion Notes (cont.) Decomposition reaction: A compound breaks down as a result of the chemical change. Decomposition reactions are easy to spot because there is only one reactant. The general reaction can be written as AB  A  B.

Discussion Notes (cont.) Single exchange reaction: A compound breaks apart, and one part combines with the other reactant—either an atom or a group of atoms such as OH-, CO32-, or NO3. Typically, one of the reactants is an element. The general reaction can be written as A  BC  AC  B, where A displaces B.

Discussion Notes (cont.) Double exchange reaction: Both reactants break apart. Their parts then recombine into two new products. Thus, the two reactants exchange parts. The general reaction can be written as AB + CD  AD + CB, where B and D exchange with each other (or A and C exchange with each other).

Discussion Notes (cont.) Toxins can react in any of these ways in the body, depending on the toxin and the circumstances.

Wrap Up How do atoms rearrange to form new products? Chemical reactions can be sorted into categories based on how the atoms in the reactants rearrange to form the products. Four general types of chemical reactions are combination reactions, decomposition reactions, single exchange reactions, and double exchange reactions.

Check-in Examine this chemical equation, which describes a double exchange between silver nitrate and sodium chloride. Predict the products. Make sure the equation is balanced. AgNO3(aq)  NaCl(aq)  Ag____(s) + Na_____(aq)