Decomposition. Composition
|
|
|
- Elisabeth Hoover
- 4 years ago
- Views:
Transcription
1 Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus (V) oxide powder is sprinkled over distilled water. 3. Solid potassium oxide is added to water. 4. Solid calcium oxide is heated in the presence of sulfur trioxide gas. 5. Calcium metal is heated strongly in nitrogen gas. 6. Drops of dinitrogen trioxide are added to distilled water. 7. Excess chlorine gas is passed over hot iron filings. 8. The gases boron trifluoride and ammonia are mixed. 9. Carbon dioxide gas is bubbled into magnesium oxide. 10. Samples of boron trichloride gas and ammonia gas are mixed. 11. Magnesium solid is heated in the presence of nitrogen gas. 12. Sulfur dioxide gas is bubbled into calcium oxide. 13. Solid sodium oxide is added to distilled H 2 O. 14. Sulfur dioxide gas is bubbled into distilled H 2 O. 15. Phosphorus trihydride gas is bubbled into liquid boron trichloride.
2 Double Replacement 1. Excess concentrated sulfuric acid is added to solid calcium phosphate. 2. Hydrogen sulfide gas is bubbled into a solution of mercury (II) chloride. 3. Solutions of manganese (II) sulfate and ammonium sulfide are mixed. 4. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate. 5. Solid lithium hydride is added to water. 6. Carbon dioxide is bubbled through water containing a suspension of calcium carbonate. 7. Solutions of ammonia and hydrofluoric acid are mixed. 8. Equal volumes of 0.1 M sulfuric acid and 0.1 M potassium hydroxide are mixed. 9. A solution of copper (II) sulfate is added to a solution of barium hydroxide. 10. Equal volumes of equimolar solutions of disodium hydrogen phosphate and hydrochloric acid are mixed. 11. Ammonia gas is bubbled into a solution of ethanoic (acetic) acid. 12. Solid ammonium carbonate is added to a saturated solution of barium hydroxide. 13. Concentrated hydrochloric acid is added to solid manganese (II) sulfide. 14. Magnesium nitrate is added to hot distilled H 2 O. 15. A solution of tri-potassium phosphate and zinc nitrate are mixed. 16. Dilute sulfuric acid is added to a solution of lithium carbonate. 17. Hydrogen sulfide gas is bubbled into a solution of nickel (II) nitrate. 18. Equal volumes of equimolar solutions of sodium hydroxide and sodium dihydrogen phosphate are mixed. 19. Solutions of zinc sulfate and sodium phosphate are mixed. 20. Solutions of silver nitrate and lithium bromide are mixed. 21. Excess hydrochloric acid solution is added to a solution of potassium sulfide. 22. Solutions of ammonium sulfate and barium hydroxide are mixed. 23. An acetic acid solution is mixed with a sodium bicarbonate solution. 24. Dilute sulfuric acid is added to solid calcium fluoride. 25. Dilute hydrochloric acid is added to dilute mercury (I) nitrate solution. 26. Solutions of cobalt (II) nitrate and sodium hydroxide are mixed. 27. Equal volumes of equimolar solutions of phosphoric acid and potassium hydroxide are mixed. 28. Excess potassium hydroxide solution is added to a solution of aluminum nitrate. 29. Solid potassium amide is added to distilled H 2 O. 30. A solution of nickel (II) chloride is added to a solution of sodium sulfide.
3 Redox 1. A stream of chlorine gas is passed through a solution of cold, dilute sodium hydroxide. 2. A solution of iron (II) nitrate is exposed to air for an extended period of time. 3. A concentrated solution of hydrochloric acid is added to solid potassium permanganate. 4. A solution of potassium dichromate is added to an acidified solution of iron (II) chloride. 5. A solution of potassium iodide is electrolyzed. 6. A concentrated solution of hydrochloric acid is added to powdered manganese dioxide and gently heated. 7. Solutions of potassium permanganate and sodium oxalate are mixed. 8. A strip of copper is immersed in dilute nitric acid. 9. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide. 10. A strip of silver is immersed in dilute nitric acid. 11. A solution of Iron (II) nitrate is added to a basic solution of hydrogen peroxide. 12. A solution of tin (II) chloride is added to an acidic solution of potassium permanganate. 13. Solid sodium dichromate is added to an acidified solution of sodium iodide. 14. Solutions of potassium iodide and potassium iodate are mixed in an acidic solution. 15. Hydrogen peroxide is added to an acidified solution of sodium bromide. 16. Solutions of tin (II) chloride and iron (III) chloride are mixed. 17. A solution of sodium bromide is added to an acidified solution of potassium bromate. 18. Hydrogen gas is passed over hot iron (II) oxide powder.
4 Complexation 1. Excess sodium cyanide solution is added to a solution of silver nitrate. 2. An excess of nitric acid solution is added to a solution of tetraamminecopper (II) sulfate. 3. Solid aluminum oxide is added to a solution of sodium hydroxide. 4. Concentrated ammonia solution is added to a solution of zinc iodide. 5. Excess concentrated ammonia solution is added to a suspension of silver chloride. 6. Excess concentrated potassium hydroxide solution is added to a precipitate of zinc hydroxide. 7. Excess concentrated sodium hydroxide solution is added to a precipitate of aluminum hydroxide. 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. 9. A concentrated solution of ammonia is added to a suspension of zinc hydroxide. 10. Excess hydrochloric acid is added to a solution of diammine silver (I) nitrate. Combustion 1. Ethanol is burned in oxygen gas. 2. Solid copper (II) sulfide is strongly heated in oxygen gas. 3. Propanol is burned in oxygen gas. 4. Carbon disulfide vapor is burned is excess oxygen. 5. Ethene gas is burned in air.
5 Single Reaction 1. A bar of zinc metal is immersed in a solution of copper (II) sulfate. 2. A piece of sodium metal is added to distilled water. 3. A piece of aluminum is added to a solution of silver nitrate. 4. A piece of nickel is immersed in a solution of copper (II) sulfate. 5. Chlorine gas is bubbled into a solution of sodium bromide. 6. A solution of tin (II) chloride is added to a solution of iron (III) sulfate. 7. Solid calcium is added to distilled water. 8. A piece of lead is immersed in a solution of silver nitrate. 9. Hydrogen gas is passed over hot iron (III) oxide. 10. A strip of zinc is added to a solution of 6.0 molar hydrobromic acid.
6 Solutions: Redox 1. C1 2 + OH - Cl - + ClO - + H 2 O (89)(95) 2. Fe 2+ + O 2 + H 2 O Fe 2 O 3 + Fe(OH) 3 (95) 3. H + + Cl - + KMnO 4 K + + Mn 2+ + Cl 2 + H 2 O (94) 4. Cr 2 O Fe 2+ + H + Cr 3+ + Fe 3+ + H 2 O (94) 5. I - + H 2 O I 2 + H 2 + OH - (92) 6. H + + Cl - + MnO 2 Mn 2+ + Cl 2 + H 2 O (91) 7. MnO C 2 O 2-4 MnO 2 + CO 2 (96) 8. Cu + H + + N0-3 Cu 2+ + NO 2 + H 2 O (93) 9. MnO H Mn 2+ + O 2 + H 2 O (93) 10. Ag + + H + + N0-3 Ag 0 + NO 2 + H 2 0O (87) 11. H 2 O 2 + Fe 2+ Fe 3+ + H 2 O (Fe(OH) 3 ) (87) 12. Sn 2+ + H + + MnO - 4 Sn 4+ + Mn 2+ + H 2 O (89) 13. Na 2 Cr 2 O 7 + I - + H + Cr 3+ + I 2 + H 2 O + Na + (81) 14. H + + I - + IO - 3 I 2 + H 2 O (82) 15. H 2 O 2 + Br - + H + Br 2 + H 2 O (82) 16. Sn 2+ + Fe 3+ Sn 4+ + Fe 2+ (98) 17. H + + Br - + BrO - 3 Br 2 + H 2 O (97) 18. H 2 + FeO H 2 O + Fe (97)
7 Single Replacement 1. Zn + Cu 2+ Zn 2+ + Cu (95) 2. Na + H 2 O Na + + OH - + H 2 (94)(85) 3. Al + Ag + Al +3 + Ag (92) 4. Ni + Cu 2+ Ni +2 + Cu (96) 5. C1 2 + Br - Cl - +Br 2 (96) 6. Sn 2+ + Fe 3+ Sn 4+ + Fe 2+ (85) 7. Ca + H 2 O Ca(OH) 2 + H 2 (87) 8. Pb + Ag + Pb 2+ + Ag (81) 9. H 2 + Fe 2 O 3 Fe + H 2 O (FeO) (82) 10. Zn + H + Zn 2+ + H 2 (98)
8 Double Replacement Precipitation Reactions, Solubility Rules, Acid-Base Reactions 1. H 2 SO 4 + Ca 3 (PO 4 ) 2 H 3 PO 4 + CaSO 4 (95) 2. H 2 S + Hg +2 HgS + H + (95) 3. Mn 2+ + S 2- MnS (94) 4. Mg 2+ + OH - Mg(OH) 2 (92) 5. LiH + H 2 O Li + OH - + H 2 (92) 6. CaCO 3 + H20 + C0 2 Ca HCO 3 (92) (H 2 CO 3 ) 7. NH 3 + HF NH F - (92) 8. H + + OH - H 2 O (91) 9. Cu 2+ + SO Ba 2+ +OH - Ca(OH) 2 + BaSO 4 (91) 10. HPO H + H 2 PO NH 3 + HC 2 H 3 O 2 C 2 H 3 O NH 4 + (96) (96) 12. (NH 4 ) 2 CO 3 + Ba 2+ + OH - NH 3 + BaCO 3 + H 2 O (96) 13.H + + MnS H 2 S + Mn 2+ (93) 14. Mg 3 N 2 + H 2 O Mg(OH) 2 + NH 3 (93) 15. Zn 2+ + PO 3-4 Zn 3 (PO 4 ) 2 (93) 16. H + + HCO - 3 H 2 O + CO 2 (85) 17. H 2 S + Ni 2+ NiS + H + (87) 18. OH H 2 PO 4 PO H 2 O (87) 19. Zn 2+ + PO 3-4 Zn 3 (PO 4 ) 2 (89) 20. Ag + + Br - AgBr (89) 21. H + + SO 2-3 H 2 O + SO 3 (H 2 SO 3 ) (89) 22. NH SO Ba 2+ + OH - BaSO 4 + NH 3 + H 2 O (81) 23. HC 2 H 3 O 2 + HCO C 2 H 3 O 2 + H 2 O + CO 2 (81) 24. H + + SO CaF 2 HF + CaSO 4 (82) 25. Hg 2+ + Cl - Hg 2 Cl 2 (82) 26. Co 2+ + OH - Co(OH) 2 (98)
9 27. H 3 PO 4 + OH - H 2 PO H 2 O (98) 28. A OH - Al(OH) 3 (97) 29. KNH 2 + H 2 O NH 3 + K + + OH - (97) 30. Ni 2+ + S 2- NiS or (Ni 2+ + H 2 S) (97)
10 Decomposition/Composition Decomposition 1. (NH 4 ) 2 CO 3 NH 3 + H 2 O + CO 2 (82)(94) 2. CaCO 3 CaO + CO 2 (96) 3. CaSO 3 CaO + SO 2 (98) Composition 1. BaO + H 2 O Ba OH - (95) 2. P 4 O 10 + H 2 O H 3 PO 4 (94) 3. K 2 O + H 2 O K + + OH - (92) 4. CaO + SO 3 CaSO 4 (91) 5. Ca + N 2 Ca 3 N 2 (91) 6. N 2 O 3 + H 2 O HNO 2 (96) 7. Fe + Cl 2 FeCl 3 (93) 8. BF 3 + NH 3 BF 3 NH 3 (85) 9. MgO + CO 2 MgCO 3 (87) 10. BC1 3 + NH 3 BC1 3 NH 3 (89) 11. Mg + N 2 Mg 3 N 2 (81) 12. SO 2 + CaO CaSO 3 (81) 13. Na 2 O + H 2 O Na + + OH - (98) 14. SO 2 + H 2 O H 2 SO 3 (97) 15. PH 3 + BCl 3 H 3 PBCl 3 (97) 16. Mg + N 2 Mg 3 N 2 (97)
11 Complex Ion Formations 1. CN - + Ag + - Ag(CN) 2 2. H + + Cu(NH 3 ) 2+ 4 Cu NH 4 3. Al 2 O 3 + OH - - Al(OH) Zn + NH Zn(NH 3 ) 4 (94) (92) (91) (91) 5. AgCl + NH 3 Ag(NH 3 ) Cl - (93) 6. Zn 2+ + OH - Zn(OH) OH - + Al(OH) 3 Al(OH) 4 - (85) (87) 8. Fe 3+ + SCN - Fe(SCN) 2+ (81)(89) 9. Zn(OH) 2 + NH 3 Zn(NH 3 ) OH - (82) 10. H + + Cl - + [ Ag(NH 3 ) 2 ] + AgCl + NH 4 + (98) Combustion 1. C 2 H 5 OH + O 2 CO 2 + H 2 O (81)(95) 2. CuS+ O 2 Cu + SO 2 (CuO, Cu 2 O) (91) 3. SO 2 + OH - HSO 3 - (93) 4. C 3 H 7 OH + O 2 CO 2 + H 2 O (87) 5. CS 2 + O 2 CO 2 + SO 2 (SO 3 ) (89) 6. C 2 H 4 + O 2 CO 2 + H 2 O (98)
![Fe 3+ + SCN - Fe(SCN) 2+ (81)(89) 9. Zn(OH) 2 + NH 3 Zn(NH 3 ) 4 2+ + OH - (82) 10. H + + Cl - + [ Ag(NH 3 ) 2 ] + AgCl + NH 4 + (98) Combustion 1.](/docs-images/46/21601954/images/page_11.jpg "C 2 H 5 OH + O 2 CO 2 + H 2 O (81)(95) 2. CuS+ O 2 Cu + SO 2 (CuO, Cu 2 O) (91) 3. SO 2 + OH - HSO 3 - (93) 4. C 3 H 7 OH + O 2 CO 2 + H 2 O (87) 5.")
AP Chemistry Reaction Questions
AP Chemistry Reaction Questions Directions: Give the formulas to show the reactants and the products for the following chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise
WRITING AP EQUATIONS
WRITING AP EQUATIONS AP equation sets are found in the free-response section of the AP test. This is a 15 point question and you can practice for it all year! You are given three equations and you must
NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide
NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate
Balancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
Naming Compounds Handout Key
Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion
Nomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula
Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the
HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
Nomenclature of Ionic Compounds
Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
Moles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
Nomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride
Nomenclature Packet Worksheet I: Binary Ionic Compounds (representative metals) metals from groups 1A, 2A, and 3A (1, 2, and 13) have constant charges as ions and do NOT get Roman Numerals in their names
Naming Ionic Compounds
Naming Ionic Compounds I. Naming Ions A. Cations (+ions) 1. Element name followed by "ion" (when in Group IA, IIA, Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag +, Ni 2+ ). Na + sodium ion, K + potassium ion, Al 3+ aluminum
CHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
Name: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.
Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying
Stoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
Chemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
Writing and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
Chapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
Unit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
Solution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
Experiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
CHEMICAL NAMES AND FORMULAS
9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the
Aqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
Chemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
WRITING CHEMICAL FORMULA
WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.
Periodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE
T-6 Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE FORMULAS: A chemical formula shows the elemental composition of a substance: the chemical symbols show what elements are present and the numerical
IB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
Molar Mass Worksheet Answer Key
Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol
Name period Unit 3 worksheet
Name period Unit 3 worksheet Read chapter 8, 2.52.7 1. Explain the difference between metallic, ionic, and covalent bonding Metallic cations share a sea of electrons Ionic atoms give and take electrons
Chapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
Chapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
Naming Ionic Compounds Answer Key
Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl
Unit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:
Problem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
W1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
neutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
Electrochemistry - ANSWERS
Electrochemistry - ANSWERS 1. Using a table of standard electrode potentials, predict if the following reactions will occur spontaneously as written. a) Al 3+ + Ni Ni 2+ + Al Al 3+ + 3e - Al E = -1.68
1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
Polyatomic Ions Worksheet. 2. Name or write the formula for the following Type I polyatomic ionic compounds
Polyatomic Ions Worksheet Polyatomic Practice 1. Name or write the formula for the following polyatomic ions sulfate - CO nitrite MnO perphosphate - SO hypoiodite BrO chlorite - CO phosphite - PO percarbonate
APPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources
Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Introduction This document is intended to help you review the basics of writing
Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
Chapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
MOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule
General Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas
Date In Class Homework 10/22 Thur Counting By Mass Lab 10/23 Fri (mole day!!!) THE MOLE! in room 137 10/26 Mon (LSM) More on the Mole Watch empirical and molecular formula video. 10/27 Tue % Composition
SEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS. Oxidation-Reduction
SEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS OxidationReduction Oxidation is loss of electrons. (Oxygen is EN enough to grab e away from most elements, so the term originally meant
Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction
Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,
Exercise 3.5 - Naming Binary Covalent Compounds:
Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used
4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?
HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm
Chemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
Lab #13: Qualitative Analysis of Cations and Anions
Lab #13: Qualitative Analysis of Cations and Anions Objectives: 1. To understand the rationale and the procedure behind the separation for various cations and anions. 2. To perform qualitative analysis
CHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
Experiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
Santa Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12
Chapter 4 Compounds and Their Bonds
Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons. is associated with the stability of the noble gases. He is stable with 2 valence electrons (duet).
Chapter 12: Oxidation and Reduction.
207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following
Chemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
Chapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
Formulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
80. Testing salts for anions and cations
Classic chemistry experiments 203 80. Testing salts for anions and cations Topic Qualitative analysis. Timing Description 12 hours. Students attempt to identify the anions and cations present in a salt
Chemical Proportions in Compounds
Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of
b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
Chapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
Solubility of Salts - Ksp. Ksp Solubility
Solubility of Salts - Ksp We now focus on another aqueous equilibrium system, slightly soluble salts. These salts have a Solubility Product Constant, K sp. (We saw this in 1B with the sodium tetraborate
CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
Sample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side
Polyatomic ions can form ionic compounds just as monatomic ions.
1 POLYATOMIC IONS We have seen that atoms can lose or gain electrons to become ions. Groups of atoms can also become ions. These groups of atoms are called polyatomic ions. Examples: O hydroxide ion NO
2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
Name period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.
CHAPTER 9 1. The coefficients of the balanced chemical equation for a reaction give the relative numbers of molecules of reactants and products that are involved in the reaction.. The coefficients of the
CHEMICAL NOMENCLATURE
CHEMICAL NOMENCLATURE Chemical nomenclature The process of giving unambiguous chemical formulas or chemical names to elements and compounds Introduction Chemistry is the study of matter (elements and compounds)
Oxidation States of Nitrogen
Oxidation States of Nitrogen HNO 3 NH 3 HNO 2 NO N 2 O N 2 HN 3 N 2 H 5 + +3 +2 +1 0-1/3-2 Oxidation +5-3 Reduction Oxidation States of Chlorine HClO 4 HClO 3 ClO 2 HClO 2 HClO Cl 2 HCl +5 +4 +3 +1 0 Oxidation
Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
Chapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
Chapter 3 Chemical Compounds
Chapter 3 Chemical Compounds 3.1 (a) formula unit; (b) strong electrolyte; (c) molecular compound; (d) acid; (e) nonelectrolyte; (f) oxoanion 3.2 (a) molecular formula; (b) weak electrolyte; (c) ionic
Module Four Balancing Chemical Reactions. Chem 170. Stoichiometric Calculations. Module Four. Balancing Chemical Reactions
Chem 170 Stoichiometric Calculations Module Four Balancing Chemical Reactions DePauw University Department of Chemistry and Biochemistry Page 1 Introduction to Module Four When making a cheeseburger you
ATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 Chapter 1 Chemistry: The Study of Change 1. Element, compound, homogeneous mixture (solution), or heterogeneous mixture: a) orange juice b)