EQUATION REVIEW
Transcription
EQUATION REVIEW
Name: ______________________ EQUATION REVIEW Fill-in: In a chemical _________________________, the substance(s) entering the reaction are(is) called _____________________ and the substance(s) that are(is) formed are(is) called the ____________________. In a chemical reaction, atoms, molecules, or ions interact and ____________________ themselves to form the products. During this process, chemical __________ are broken and ______________ bonds are formed. The reactants and products may be in the solid, _____________, or _______________ state, or in ______________________ solution. A chemical _____________________________, is a shorthand expression for a chemical change or ______________________. A ____________________ equations states in words, in equation form, the substance involved in a chemical _________________________. For example, when mercury (II) oxide is heated, it ______________________ to form mercury and oxygen gas. The word equation: _______________________ and heat mercury and ______________________ is bulky and cumbersome to use and does not give ______________________ information. So a _____________________ equation is written first, showing correct formula and symbols and states of matter: _______________________ Hg(l) + ______________________. According to the law of conservation of ____________, the equation must be balanced so that there are equal number(s) of each kind of atom (_________________) on both sides of the arrow. This is done by placing numbers in front of each formula (for a compound) or symbol (for an element) that are called _______________________. _______HgO(s) _______Hg(l) + _________O2(g). This equation is called a _____________________________ equation and shows formulas, composition, and relative amounts of all substances involved. It does not show how much _________ is needed to cause decomposition or anything about the __________________ of reaction. Many symbols other than those for the elements are used in an equation. A ____________________ is used to separate reactants and/or products. An _______________ means “________________” and separates products from reactants. An arrow pointing in each direction, means the reaction is _____________. A triangle above the arrow means _______ was added, and if there is a symbol of an element or formula for a compound above the arrow, it means this substance is a __________. A solid can be shown with a _________or ________, gas with a _______ or ________, and liquid with a ________. (aq) means the substance is an ____________ solution. Reactions may be classified into types to assist in writing equations and to aid in ______________ products. There are six principal reactions types. The general form for the first is A + B AB, and this type is called ______________or ___________________ reactions. The general form of the second is AB A + B, and this type is called ____________ or _________________ reactions. In a ___________________ reaction there are two general forms, A + BC C + BA, or A + BC B + AC. The first example is showing A as a _________ replacing a ___________ ion. The second example is showing A as a ____________, replacing a _____________ ion. The fourth type shown by general form, AB + CD AD + CB is called a ________________________________ reaction and usually takes place in an ______________ solution. The fifth kind involves the ___________________ or _______________________ combustion of a carbon compound. The other reactant is ____________ gas and the products are water and ___________________________ in complete combustion OR water and __________________________ in incomplete. This kind just talked about also fits into a category called oxidation-reduction (red-ox) reaction and even some reactions in the first five categories. These reactions will be talked about later. For reactions that take place in water another kind of equation can be written. A _______ ionic equation only shows those ions involved in the chemical reaction and eliminates ____________ ions who do not participate in the reaction and are said to just watch the reaction. These reactions will have ______________ in aqueous solutions on the reactant side and compounds on the product side as either a _____________, __________ or ___________. PRACTICE PROBLEMS: 1. Oxygen gas and potassium chloride are formed by heating potassium chlorate. Write a…………. a. Word Equation b. Skeleton and then balanced equation 2. Water can be decomposed into its elements by using electricity when catalyzed by sulfuric acid. Write a…………. a. Word Equation b. Skeleton and then balanced equation 3. Lithium metal reacts with water making hydrogen gas and sodium hydroxide. Write a…………. a. Word Equation b. Skeleton and then balanced equation DESCRIPTIVE CHEMISTRY: Predict products, then balance. All products need to also have states of matter, ie.: (aq), (g), etc. You do not need to write net ionic equations in this section, but may do so for practice to the right of each equation. 1. COMBINATION (various kinds) a. Metal + Oxygen Mg(s) + O2(g) Al(s) O2(g) + b. Nonmetal + Oxygen makes water) S(s) + O2(g) H2(g) + O2(g) Metal Oxide (Hint: use periodic table to predict product products formula) Nonmetal Oxide (Hint: first reaction makes sulfur dioxide, the second c. Metal + Nonmetal Na(s) + Cl2(g) Al(s) Br2(g) + Salt (Hint: use periodic table to predict products formula) d. Metal Oxide + Water e. Na2O(s) + H2O(l) CaO(s) + H2O(l) Metallic hydroxides (aka-a base or the hydroxide ion) Nonmetal Oxide + Water SO3(g) + H2O(l) CO2(g) + H2O(l) Oxy-acid 2. DECOMPOSITION (various kinds) a. Metal Oxide Metal + Oxygen MgO(s) Al2O3(s) b. Metallic Carbonate Metal Oxide + Carbon Dioxide CaCO3(s) Al2(CO3)3(s) c. Misc. KClO3 ? + Oxygen gas KCl (s) NaNO3 (s) + NaNO2 (s) (s) H2O2(aq) 3. SINGLE REPLACEMENT (various kinds) a. Metal* + Acid Hydrogen Gas + Salt Zn(s) + HCl Ca(s) + H2SO4 (aq) (aq) *(K, Ca, Na, Mg, Al, Zn, Fe, Ni, Sn, Pb, all react with acids) b. Metal** + Water Cs(s) + H 2O (l) Ca(s) + H 2O (l) Hydrogen Gas + Metal Hydroxide **(K, Ca, Na, (Li, Al, Zn, Fe) only with steam) c. Metal*** + Salt(aq) Fe(s) + CuSO4 Cu(s) + AgNO3 Metal + Salt(aq) (Hint: both metal ions are +2 in charge) (aq) (aq) ***(H, Ca, Na, Mg, Al, Zn, Fe, Ni, Sn, Pb, Cu, Ag, Hg, Au) d. Halogen + Halide Salt(aq) F2(g) + NaBr Cl2(g) + NaI Activity Decreases Halogen + Halide Salt(aq) (aq) (aq) 4. DOUBLE - REPLACEMENT (various kinds) a. Acid + Base Water + Salt H2SO4(aq) + HCl(aq) + Mg(OH)2 NaOH(aq) b. Sol’n + Sol’n CaCl2(aq) + Sol’n + Precipitate (aka –an insoluble salt) AgNO3(aq) K2SO4(aq) + c. (aq) BaCl2 (aq) Formation of a Gas (Hint: first reaction makes a gas with a rotten egg smell and second and third equation will produce three products) HCl(aq) + ZnS(s) HCl(aq) + CaCO3 HCl(aq) + NaHCO3 (s) (s) Write a balanced equation for each statement. When appropriate you must also write a net ionic equation. 1. Calcium metal slowly rust overtime when exposed to air. 2. Solid phosphorus (P4) is heat in a test tube with oxygen gas makes solid diphosphorus pentaoxide. 3. Butane (C4H10) in a cigarette lighter undergoes complete combustion. 4. Nitric acid is neutralized with calcium hydroxide. 5. Aqueous solutions of mercurous nitrate and lithium chloride are mixed in a test tube. 6. A solution of silver nitrate is added to a nail made from iron in a test tube. The solution goes from being colorless to a light yellow-green color. 7. Strontium chlorate is heated in a test tube. A wood splint that is glowing red relights when placed in the mouth of the test tube. 8. Sodium metal is placed into a beaker of distilled water. Classify the following reactions by placing on the blank the following symbols. If no reaction takes place – NR, otherwise use: DR – double replacement; SR – single replacement; C- combination (synthesis); D- decomposition (analysis). Then predict products and balance. All products need to also have states of matter, ie.: (aq), (g), etc. ________ 1. SO2(g) + H2O(l) ________ 2. H2SO4(aq ) + ________ 3. KI(aq ) + ________ 4. ZnCO3(s ) + ________ 5. H2 (g ) + ________ 6. (NH4)2S (aq ) + ________ 7. MgCO3(s ) ________ 8. BaCl2(aq ) + ________ 9. K(s ) + ________ 10. Ag2O(s ) ________ 11. Cu(l ) + ________ 12. K2O(s ) + H2O(l) ________ 13. KCl (aq ) + NaNO3(aq) ________ 14. Mg(ClO3)2(s) ________ 15. Cl2(g ) + NaF(aq) ________ 16. Fe(s ) + O2(g) ________ 17. Mg(s) + NaOH(aq) Br2(s) HCl(aq) Cl2(g) HI(aq) Na2SO4(aq) H2O(l) HCl(l) Zn(NO3)2(aq) ________ 18. ZnCl2(aq ) + ________ 19. F2(s ) + ________ 20. CaO(s ) + NaOH(aq) NaI(aq) H2O(l) AP Chemistry Free Response #4 Directions In the box follow these directions (5 points extra credit for each) Write the formulas to show the reactants and products for ALL of the laboratory situations described below. In all cases a reaction occurs. Assume that solutions are aqueous unless otherwise indicated. Represent substances in solution as ions if the substances are extensively ionized. Omit formulas for any ions or molecules that are unchanged by the reaction. You need to balance the equations. 1. A solution of potassium hydroxide is added to a solution of copper (II) sulfate. a. 2. Identify the spectator ions Liquid chlorine is shaken with a sodium iodide solution. a. Which substance is undergoing reduction? 3. Aluminum metal is added to a solution of hydrochloric acid. a. What subatomic particle is being exchanged between the reactants and how many