Study Buddy Chemistry Review Questions - Unit 1 PDF

STUDY BUDDY QUESTIONS UNIT 1 – Chemistry Answer these questions with a study buddy. Try to answer as many as you can verbally. If you need to work it out on paper, that’s fine also. 1.1 Properties of matter 1. Why are physical and...

STUDY BUDDY QUESTIONS UNIT 1 – Chemistry Answer these questions with a study buddy. Try to answer as many as you can verbally. If you need to work it out on paper, that’s fine also. 1.1 Properties of matter 1. Why are physical and chemical properties of substances useful to know in some cases? 2. What is the difference between a physical and a chemical property? 3. Name any three physical properties that we didn't discuss in the notes so far. _______________________________________________________________ 1.2/1.3 Physical & Chemical Properties 1. What is a physical change? 2. What is a chemical change? 3. What are two differences between a physical and a chemical change? 4. Give two examples of physical changes that we didn't discuss so far (your own ideas). 5. Give two examples of chemical changes that we didn't discuss so far. 6. What are the 5 clues that you can use to tell if something is undergoing a chemical change? 7. What is it called when a gas turns into a liquid? When a gas turns into a solid? ________________________________________________________________ 1.5 WHMIS and Lab Safety 1. What is the importance of an MSDS? 2. What is the importance of WHMIS? ________________________________________________________________ 1.6 Atoms and Rutherford-Bohr Diagrams 1. What information do Bohr-Rutherford diagrams contain? 2. Can the nucleus of one element be exactly the same as a nucleus of a different element? 3. How many electrons (in each energy level) would a nitrogen atom have? A potassium atom? 1.7 Periodic table patterns 1. What information on the periodic table lets you predict the number of electrons in an atom? 2. Compare metals and non-metals in terms of their number of electrons in the outermost orbit. 3. Refer to the periodic table to name and write the symbols for the following elements: a) the halogen of the second period b) the alkaline earth metal in the fifth period c) the noble gas with the smallest atomic number d) the alkali metal of the fourth period e) the metal of the third period with three outermost electrons f) the unreactive gas of the second period 4. Compare the number of outermost electrons: a) within a period b) within a group ________________________________________________________________ 1.7 Periodic Trends and Ions 1. Which elements are naturally found as "doubles" (bonded to itself) in normal conditions? 2. What is the difference between an anion and a cation? 3. List three atoms or ions that have the same number of electrons as each of the following: a) S2- b) Al3+ c) P3- 4. Justify why these ions do not exist under normal conditions: a) K2+ b) Al2+ 5. What, technically, is an ionic bond? 6. Why are full outer orbits in atoms considered ideal? 1.8 Ionic Compounds and Nomenclature (Naming) 1. What is an ionic compound? 2. What kind of elements combine to form ionic compounds? 3. Explain why two non-metallic elements are not likely to form ionic bonds. 4. When each of these compounds dissolves in water, what ions are released and in what ratio? a) NaF b) Li3N c) FeCl3 5. Compare the electrical conductivity of pure water, tap water, and seawater. You can look this up. Why is there a difference in conductivity? 6. Magnesium and chlorine react to form an ionic compound. How many electrons must the atoms of each element gain or lose to become a stable ion? 7. What is a transition metal and how is it different from a Group I or Group II metal? 8. What do you have to do differently when you are naming an ionic compound that contains a transition metal? 9. What is a polyatomic ion? How is it different from other ions? 10. What are the chemical names of the following: a) NaNO3 b) K2SO4 c) (NH4)2SO4 1.9 Naming Molecular Compounds 1. What is a molecular compound? 2. How does bonding in molecular compounds differ from ionic compounds? 3. What are the types of elements that form molecular compounds? 4. What is different about how to name molecular compounds compared to ionic compounds? 5. Name the following: a) CO b) PF5 c) PCl3 d) OCl2 6. What are the chemical formulas for the following: a. Carbon dioxide b. Phosphorus tetrachloride c. Nitrogen tribromide d. Dinitrogen tetroxide ________________________________________________________________ 2.1 Introduction to Chemical Reactions 1. What is the purpose of the arrow in a chemical equation? 2. What is the difference between a word equation and a chemical equation? 3. If energy is written in the products, does the reaction feel warm or cold? What if the energy is written as part as the reactants? 4. When chemicals have (aq) written beside them, what does this mean? 2.3 Conservation of Mass 1. What is meant by the "Law of Conservation of Mass"? 2. What does it mean by "balancing a chemical equation"? 3. What is a "coefficient" in chemistry? 4. Which best represents the Law of Conservation of Mass: a skeleton equation, or a balanced chemical equation? Explain. 5. Are the following situations exceptions to the Law of Conservation of Mass? Justify your answer. a) The mass of a hamburger decreases as it is barbecued. b) A tree's mass is continually increasing as the tree grows. c) You are often lighter in the morning than you were when you went to bed. ___________________________________________________________ 2.4 Types of Reactions 1. What are the 4 major types of reactions? 2. Which two types seems to be the "opposite" of each other? 2.4a Combustion 1. What two chemical products are usually produced when combustion takes place? 2. a) What is the main difference between complete and incomplete combustion? b) What conditions must be met for incomplete combustion to happen? c) Why is incomplete combustion dangerous? 3. What is soot? 4. Write the general equation for complete combustion using "fuel" as a reactant. 2.4b Corrosion 1. What is the difference between combustion and corrosion? What are the similarities? 3. What causes some metals to rust/corrode? 2.7 Intro to Acids and Bases 1. Name any 5 things that are considered to be acidic. 2. Name any 3 things that are considered to be basic. 3. What does "corrosion" mean (in terms of acids/bases)? 4. List any two differences between acids and bases. __________________________________________________________ 2.8a Acids 1. In general, how can you recognize an acid by its chemical formula? (i.e. what elements in the chemical formula can indicate that the substance is an acid)? 2. What is the difference between binary acids and oxyacids? 3. Explain how acids: a) react with metals b) react with carbonates c) conduct electricity 4. What does the symbol "(aq)" mean? 5. What is the name of these acids? a) HNO3 b) H2SO4 c) HCl 6. Give at least three properties of acids. ___________________________________________________________ 2.8b Bases 1. In general, how can you recognize a base by its chemical formula (what polyatomic ion)? 2. What is an "indicator" in chemistry? 3. Compounds can be ionic or molecular. What kind of compound is an acid? A base? Explain. 4. Give at least three properties of bases. 5. What is the name of these bases? a) NaOH b) Ca(OH)2 ___________________________________________________________ 2.7 Intro to pH 1. Explain how the pH scale works (that is, what is pH 7, what does it mean if it's higher than 7, etc.?) 2. Explain how blue and red litmus paper behaves when exposed to acids and bases. 3. If one solution has a pH of 5, and another has a pH of 1, which one is the most acidic? 4. Why do you think that household products be stored in their original containers? 5. Name two foods that are acidic. Name two foods that are basic. _____________________________________________________ 2.9 The pH Scale (continued) 1. What does "neutralization" mean in chemistry? 2. What do we mean when we describe a solution as being "neutral"? 3. Describe the pH changes expected if an acid is used to neutralize a base with a pH of 12. 4. Write the chemical equations for each of these acid-base reactions (and balance): a) hydrochloric acid and calcium hydroxide b) sulfuric acid and potassium hydroxide 5. Which would be the best to neutralize a large acid spill in your school lab: a) sodium hydroxide or baking soda? Explain. 6. Fish muscle contains bases that give cooked fish their "fishy" odour. Suggest why a squirt of lemon juice often makes this odour disappear. 7. Over time, a crusty deposit of calcium carbonate forms on the heating element inside a kettle. Use your understanding of acids and bases to suggest a way to remove this deposit. ___________________________________________________________ 2.10 pH in the Environment 1. Why is the soil pH important to farmers in particular? 2. What is meant by the term "acid leaching"? 3. How can we make use of acids or bases to: a) remove heavy metals from soils? b) improve crop yields? c) prevent the growth of micro-organisms in swimming pools? 4. How do lakes become acidic? What can be done to help with the problem? What is meant by the term "acid precipitation"? 2. How is acid precipitation formed? What two groups of compounds are largely responsible for causing acid precipitation? 3. Name one typical source of SO2. Name one typical source of NO2/NO3 4. List three ways in which acidic precipitation can have an environmental impact. 5. Explain how acid precipitation can affect a country's economy. 6. Explain how acid precipitation can be prevented or reduced in our society. 7. Why is global co-operation essential in our battle against the effects of acid precipitation?