Chapter 16 - Solids, Liquids, and Gases

Size: px

Start display at page:

Download "Chapter 16 - Solids, Liquids, and Gases"

Leonard Hart
5 years ago
Views:

1 PHYSICAL SCIENCE Q2 Cumulative Review (for Physical Science B Final) Chapter 16 - Solids, Liquids, and Gases In the blank, write the term or phrase that best completes each statement or answers each question. 1. The particles that make up a sample of matter have energy. 2. A measure of the average kinetic energy of the particles in a sample of matter is its. 3. As the temperature of a material decreases, the average of its particles also decreases. 4. Matter that has a definite volume and a definite shape is a. 5. Matter in which particles are arranged in repeating geometric patterns is a. 6. A gaslike mixture with no definite volume or shape that is made up of positively and negatively charged particles is a. 7. Matter with no definite volume and no definite shape is a. 8. Matter that has a definite volume but no definite shape is a. 9. The most common state of matter in the universe is. 10. Matter in which the particles are free to move in all directions until they have spread evenly throughout their container is a. 11. Solid, liquid, gas and plasma are the of matter. 12. The state of water at 25 C is. 13. The physical state of ice is. 14. The state of water vapor is. 15. The idea stating that matter is made up of small particles that are in constant motion is. 16. The particles that make up a solid move than do the particles that make up a gas. 17. Most matter when heated and when cooled. This is called. 18. Water that contains such high levels of unwanted materials that it is unacceptable for use is. 19. Excess heat in rivers is caused by pollution. 20. Hot water that is produced by electric power plants and released into rivers and streams causes. 21. Pesticides, fertilizers, and industrial wastes can all. 22. As a sample of matter is heated, its particles.

2 23. Changing of a liquid to a gas gradually at temperatures below the boiling point is called. 24. Changing of a gas to a liquid is called. 25. The amount of energy needed to change a material from the solid state to the liquid state is the heat of. 26. The amount of energy needed to change a material from the liquid state to the gas state is the heat of. 27. Amount of force exerted per unit area is. 28. The SI unit for pressure is the. 29. What causes the pressure in a gas? 30. The pressure of a gas will as the volume of the container decreases provided temperature does not change. This statement is law. 31. The idea that the volume of a gas with increasing temperature provided the pressure does not change is law. 32. If a balloon is placed in a pile of snow for 10 minutes, its temperature decreases and its volume. This illustrates law. 33. Charles and Boyle s laws apply to these state/s of matter: 34. law explains why sitting on your bicycle increases the pressure in your tires. 35. The temperature at which all particle motion would stop is. 36. state/s are classified as fluids because the particles are able to flow. 37. As the velocity of a fluid increases, the pressure exerted by the fluid decreases. This statement is. 38. Bernoulli s principle explains why. 39. Fluids flow when forced to flow through narrow spaces. This is known as _. 40. The dots on the balloon represent particles of air. Use what you know about pressure, temperature, volume, and the kinetic theory of matter to write a hypothesis explaining what will happen to the volume of the balloon if pressure is kept constant and the temperature is lowered.

3 Complete each of the following diagrams by showing how the positions of the particles will change under the conditions described. Also, explain why the particles positions would change to that new position Balloon cooled, pressure constant Melts 45. What are three ways people use fresh water each day? 46. What can people do to reduce water pollution? 48. Compare and contrast condensation, boiling, and evaporation. Include the kinetic theory of matter in your response. 49. Explain how an airplane wing makes a plane move upward, using a concept from Chapter 8. You may choose to include a diagram as part of your explanation. Chapter 17 - Atomic Structure and the Periodic Table Determine whether the italicized term makes each statement true or false. If the statement is true, write the word true in the blank at the left. If the statement is false, write in the blank the term that makes the statement true. 1. The symbol for chlorine is C. 2. The central core of an atom is called the hub. 3. The mass of an electron is about equal to the mass of a proton. 4. The region around the nucleus occupied by the electrons is called the negative zone. 5. The number of protons in an atom is called the atomic mass. 6. The identity of an element is determined by the number of protons. 7. According to present atomic theory, the location of an electron in an atom is best represented by a electron cloud. 8. The maximum number of electrons in the second energy level of an atom is Quarks can be produced by bombarding protons with protons. 10. The sum of the number of protons and the number of neutrons in an atom is the mass number. 11. The weighted average of the mass numbers of all the isotopes that occur in nature for a particular element is the average atomic number.

4 12. Two isotopes of carbon are carbon-12 and carbon-14. These isotopes differ from one another by two electrons. 13. The atomic masses of the elements are not whole value numbers because of the existence of quarks. 14. The chart showing the classifications of elements according to their properties and increasing atomic numbers is called the periodic table. 15. Elements arranged in vertical columns in the periodic table are called periods. 16. Nonmetals are poor conductors of heat and electricity. In the blank at the left, write the term or phrase that correctly answers each question or best completes each statement. 17. A chemical symbol represents the of an element. 18. A particle that moves around the nucleus is a(n). 19. Each energy level of an atom has a maximum number of it can hold. 20. Particles of matter that make up protons and neutrons are. 21. The is used to accelerate protons in the study of subatomic particles. 22. A certain atom has 12 protons, 12 electrons, and 13 neutrons. Its mass number is. 23. Atoms of the same element with different numbers of neutrons are called. 24. Horizontal rows of the periodic table are called. 25. Elements in groups 3 through 12 are called. 26. Complete the following table. The atomic number of carbon is 6. Name Mass Number Atomic Number Number of Protons Carbon - 12 Carbon - 13 Carbon - 14 Number of Neutrons Answer the following questions in the space provided. 28. Explain why the periodic table is such a useful tool. 29. Scientists often use mental pictures to explain their ideas. What do we call these mental pictures? Why are they useful?

5 30. Compare and contrast the masses of protons, neutrons, and electrons. 31. Why is family 18 called the noble gases? 32. Suppose that you have just discovered a new element and have named it neptunite. While studying your new element you find that it has two isotopes. These are neptunite-220 and neptunite-250. What is the average atomic mass of your new element? (Assume that these two isotopes are present in equal amounts in nature.) 33. Be sure you know the names & symbols for the 42 elements listed below. List the symbols for the following elements. Be sure to use the correct cases for your letters. aluminum platinum bromine strontium neon fluorine carbon uranium beryllium zinc xenon radon iodine barium cobalt tin helium oxygen sodium silicon potassium cesium nitrogen lithium gold iron calcium hydrogen chlorine chromium copper mercury magnesium lead boron nickel argon plutonium sulfur krypton silver phosphorus 34. Complete the following table: Name fluorine sodium gold arsenic zirconium krypton Atomic Number Mass Number Period Group Metal/Nonmetal /Metalloid 35. Draw models for the following atoms. Include the symbol for the specific isotope you choose. phosphorus beryllium oxygen hydrogen boron potassium

6 Chapter 20 - Chemical Bonds Determine whether the italicized term makes each statement true or false. If the statement is true, write the word true in the blank. If the statement is false, write in the blank the term that makes the statement true. 1. The properties of a compound are the same as the properties of the elements making up the compound. 2. Particles formed from the covalent bonding of atoms are called ions. 3. Molecules are neutral. 4. When an atom gains or loses electrons, the charged particle that results is called a molecule. 5. Because a water molecule has a slight positive charge at one end and a slight negative charge at the other end, it is a nonpolar molecule. 6. Hazardous materials are poisonous if they are corrosive. 7. Gasoline is a hazardous compound because it is flammable. 8. Battery acid and bleach are examples of corrosive compounds. 9. The formula SO 4 2- stands for ammonium. In the blank, write the term or phrase that completes the statement or answers the question. 10. In a chemical formula, the ratio of atoms in the compound is shown by numbers called. 11. The elements that make up a compound and the ratios of the atoms of those elements can be shown in a. 12. What is the total number of atoms in the compound Sr(MnO 4 ) 2? 13. How many hydrogen atoms are present in one molecule of ammonium bicarbonate, NH 4 HCO 3? 14. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable? 15. Why do the noble gases NOT form compounds readily? 16. Laughing gas is a compound containing a ration of two atoms of nitrogen to one atom of oxygen. What is the correct formula for laughing gas? 17. A chemical bond that occurs when atoms share electrons is a(n) bond. 18. What kind of chemical bond is formed when electrons are transferred from atom to atom? 19. A group of atoms that acts together as one charged atom is a. 20. The name given to the combining ability of an atom is. 21. The sum of the oxidation numbers in a neutral compound is. 22. The oxidation number of an atom is shown with a. 23. When O becomes O 2-, were electrons gained or lost? 24. When Na becomes Na 1+, were electrons gained or lost? 25. What is the name of a binary compound made up of fluorine and sodium?

7 26. What is the name of the compound with the formula KI? 27. What is the correct formula for calcium chlorate? 28. What is the charge of carbonate in Cs 2 CO 3? 29. What is the ratio of aluminum atoms to fluorine atoms in a binary compound made from these two elements? 30. What is the correct name for Na 3 PO 4? 31. What is the correct formula for barium oxide? 32. What is the name of the compound with the formula Cu 2 S? 33. What is the name of the compound with the formula SrI 2? 34. Complete a concept map of the types of chemical bonding using the the following terms or phrases: covalent bonding, ions, positive ions, polar, nonpolar, negative ions, ionic bonding, molecules chemical bonding Answer the following questions in the space provided. 35. Explain how the formula for a binary compound is written. 36. Explain the rules that you must follow to name a binary compound from its formula. 37. When writing a formula, why do the oxidation numbers have to add up to zero? 38. What is the difference between an ion and an atom? 39. Compare and contrast the physical and chemical properties of H 2 O and H 2 O 2. (LAB!!!)

8 40. If H 2 O and H 2 O 2 are both made up of hydrogen and oxygen, why do they not have the same properties? 41. What is the difference between an ionic bond and a covalent bond? 42. A sodium atom has 11 protons and 11 electrons. A chlorine atom has 17 protons and 17 electrons. Using a Lewis dot structure (dot diagram), explain how an atom of sodium and an atom of chlorine combine by ionic bonding. Using the information given, your common ion chart and periodic table, write chemical formulas for the following. 43. S 2- H potassium oxide 44. Zn 2+ OH rubidium sulfide 45. Na 1+ I sodium sulfate 46. Ni 2+ NO NH 4 1+ CO calcium hydroxide 52. potassium fluoride Using the information given, your common ion chart and periodic table, name the following compounds. Don t forget to use Roman numerals when necessary. 53. LiCl 56. (NH 4 ) 2 Cr 2 O K 2 S 57. NaOH 55. Ca(NO 3 ) FeS

9 Chapter 21 - Chemical Reactions Determine if the italicized word makes each statement true or false. If the statement is true, write true in the blank. If the statement is false, write the word or phrase that makes it true in the blank. 1. Substances that slow down chemical reactions are called inhibitors. 2. Each substance to the left of the arrow in a chemical equation is a reactant. 3. The breakdown of one substance into two or more substances is a decomposition reaction. 4. Subscripts are numbers that are placed before symbols or formulas in a chemical equation. 5. A substance that speeds up a chemical reaction without becoming involved in the reaction is a preservative. In the blank at the left, write the term or phrase that best completes each statement or answers each question. 6. Each substance to the right of the arrow in a chemical equation is a. 7. Each substance on the left side of the arrow in a chemical equation is a. 8. In the equation, BaCl 2 + K 2 CrO 4 BaCrO 4 + KCl potassium chloride is a. 9. In the equation, P 4 + Cl 2 PCl 3, chlorine is a. 10. According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare to the mass of the reactants? 11. When heated, mercury (II) oxide produces oxygen plus mercury. What would be the combined mass of oxygen and mercury if 20 g of mercury (II) oxide were heated? 12. According to the law of conservation of mass, if two atoms of hydrogen are used as a reactant, how many atoms of hydrogen must be part of the product? 13. Numbers that precede symbols and formulas in a chemical equation are. 14. A substance that does not dissolve in solution and settles to the bottom is a. 15. Ozone in the atmosphere protects living things from. 16. Ozone in the atmosphere is broken down by. 17. A(n) chemical equation has the same number of atoms of each element on both sides of the equation. 18. When one element displaces another element in a compound, the reaction is a reaction. 19. What type of reaction is shown in the following chemical equation: NH 3 + HCl NH 4 Cl? 20. What type of chemical reaction is shown in the equation 2H 2 O 2H 2 + O 2?

10 21. A term that means putting together is. 22. The breaking down of a compound into simpler substances is. 23. A chemical reaction in which energy is released is. 24. If thermal energy must be added to a chemical reaction for the reaction to take place, the reaction is. 25. In the lab, when water was added to ammonium chloride, the beginning temperature was 23 C and the final temperature was 15 C. The reaction was. 26. A substance that speeds up a chemical reaction without undergoing a permanent change itself is. 27. Substances that slow down chemical reactions are called. 28. Citric acid is added to some foods to slow spoilage, it is called a(an). 29. Complete the concept map below by using the terms endothermic and exothermic and give examples of each. gives off energy energy changes in chemical reactions requires energy reactions example reactions example 30. Give an example of each of the following types of reactions: single displacement double displacement decomposition synthesis

11 31. In the spaces below, write the term that correctly describes the part of the equation identified by each letter. a b c d e f Sr(cr) + 2H 2 O(l) --> Sr(OH) 2 (aq) + H 2 (g) g h a. e. b. f. c. g. d. h. Short Essay: Answer the following questions. 32. Explain why enzymes and preservatives are important to you. 33. Some reactions turn the solution cloudy; why is this? 34. Why is it necessary to balance a chemical equation? Using your common ion chart, write a balanced chemical equations for the following reactions. 35. Sodium plus chlorine yields sodium chloride. 36. Silver nitrate plus potassium bromide yields silver bromide plus potassium nitrate.

12 Balance each equation and identify each of the below reactions as: Syn= Synthesis Dec= Decomposition SD= Single Displacement DD= Double Displacement 37. Pb(NO 3 ) 2 PbO + NO 2 + O NH 3 + HCl NH 4 Cl 39. Li + F 2 LiF 40. CuCl 2 + H 2 S CuS + HCl 41. Al 2 O 3 Al + O Ba(OH) 2 + HNO 2 Ba(NO 2 ) 2 + H 2 O 43. Cl 2 + NaBr NaCl + Br Na 2 O + CO 2 Na 2 CO H 2 O + Fe Fe 2 O 3 + H KClO 3 KCl + O 2

13 Chapter 23 - Acids, Bases, and Salts Determine whether the italicized term makes each statement true or false. If the statement is true, write the word true in the blank. If the statement is false, write in the blank the term that makes the statement true. 1. Normal rain is slightly basic. 2. Acid rain deposits important mineral nutrients as it moves through the soil. 3. Acid rain causes the rapid weathering of buildings and statues made of limestone. 4. The process of making soap is called synthesis. In the blank, write the term or phrase that completes the statement or answers the question. 5. A substance that produces H 1+ ions in solution is a(n). 6. A substance that produces OH 1 ions in solution is a(n). 7. A solution with a bitter taste and a slippery feel is most likely a(n). 8. HCl is the formula for. 9. Hydrochloric acid is sometimes used to remove impurities from metals in a process called. 10. H 3 O 1+ units are called. 11. In a titration, the point where the indicator changes color is the. 12. In a titration, the solution for which the concentration is known is called the. 13. The terms dilute and concentrated refer to the of a solution. 14. The strength of a base that only partly dissociates in solution would be described as. 15. When the acidity of a substance is determined by the hydronium ion concentration, the of the substance is being calculated. 16. Organic substances that change color in the presence of an acid or a base are called. 17. Name the best indicator of the number of hydronium ions in a solution. 18. Coffee has a ph of about 5. That makes coffee a(n). 19. What is the ph of a solution that is neither acidic nor basic? 20. One cause of acid rain is the. 21. A process that uses a solution of known concentration to find the concentration of another solution is called. 22. A reaction between an acid and a base that produces a salt and water is a reaction.

14 23. To relieve an upset stomach due to excess acid, you should eat an antacid which is a(n). 24. A compound formed in solution from the negative ion of an acid and the positive ion of a base is a. 25. Name a characteristic that is not shared by soaps and detergents. 26. What is the function of the polar end of the soap molecule? 27. What is the function of the nonpolar end of the soap molecule? 28. A substance formed when an organic acid combines with an alcohol is. 29. Give an example of two substances that will react to form an ester. 31. How does the charge of the ions produced by an acid in solution differ from the charge of the ions produced by a base in solution? 32. List three characteristics that acids and bases have in common. 33. List three characteristics that acids and bases have that are different. 34. Write the name and chemical formula for 2 common acids. What about the formula makes it an acid? 35. Write the name and chemical formula for 2 common bases. What about the formula makes it a base? 37. What factor determines the strength of an acid or a base? 38. How is a weak acid different from a strong acid? 39. How is the concentration of an acid or base in solution different from the strength of the acid or base? 40. How is a salt formed?

15 41. What are some problems that are possibly caused by acid rain? What can be done to solve the problem of acid rain? 42. Show the balanced neutralization reaction between NaOH and H 3 PO 4 and label the following parts of the equation: acid, water, salt, and base. 43. Give the name of the salt formed in the above neutralization reaction. 44. If all of the reactants in the reaction in #42 completely reacted, what would you expect the results of the following tests to be: a. blue litmus paper? b. red litmus paper? c. ph paper (what ph#)? Chapter 15 - Classification of Matter Determine whether the italicized term makes each statement true or false. If the statement is true, write the word true in the blank. If the statement is false, write in the blank the term or terms that make the statement true. 1. All air pollutants are a result of human activity. 2. Homogeneous mixtures can be separated by physical changes. 3. The law of conservation of mass states that the mass of all substances before a chemical change equals the mass of all the substances after the change. 4. When a firecracker explodes, mass is lost. 4b. Hydrogen and oxygen form water in a chemical reaction. Compare the mass of hydrogen and oxygen before the reaction with the mass of water resulting from the reaction. What law does this abide by?

16 Draw diagrams below to represent models for the following items. Use small circles to represent atoms and when needed, use darkened circles to represent one element and undarkened circles to represent another element. 5. a pure element 8. mixture of two compounds 6. a pure compound 9. mixture of an element and a compound 7. mixture of two elements In the blank at the left, write the term or phrase that correctly answers each question or best completes each statement. 10. is a substance. 11. When two or more substances are combined so that each substance maintains its own properties, the result is a(n). 12. Substances are either elements or. 13. is one type of homogeneous mixture. 14. A(n) is not homogeneous. 15. is used to remove particles from water. 16. One type of air pollution is the colloid that is known to the public as. 17. Most larger particles are removed from water by. 18. The color of ink is a. 19. When gasoline is burned in an engine,. 20. When sugar and sand are mixed together, the properties of the final substances are those of the beginning substances. 21. A new substance is formed during a. List 4 examples of each of the following: 22. Element: 23. Compound:

17 24. Homogeneous Mixture: 25. Heterogeneous Mixture: 26. Physical Properties: 27. Chemical Properties: 28. Physical Changes: 29. Chemical Changes: 30. In the concept map below, fill in the following terms where they belong: heterogeneous mixtures, suspension, homogeneous mixtures, vinegar, colloid, mixtures, solution, muddy water, milk Answer the following questions with complete sentences. 31. What is the difference between a bottle of salt and a bottle of sodium & chlorine? 32. David was baking cookies for a school bake sale. He accidentally mixed chocolate pieces and shredded coconut together. He needed the chocolate pieces for one recipe and the coconut for another. Can you think of a method David could use to separate these things? Would this method be using physical or chemical properties?

Physical Science Study Guide

Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table