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Chapter 1

Chapter 1. What is quantitative observation? Pg 7 deals with numbers or amounts What is qualitative observation? Pg 7 deals with descriptions that cannot be expressed in numbers

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Chapter 1

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  1. Chapter 1 What is quantitative observation? Pg 7 deals with numbers or amounts What is qualitative observation? Pg 7 deals with descriptions that cannot be expressed in numbers What is inferring? What is inferring based upon? Pg 8 when you explain or interpret things that you observe. Based on reasoning and prior knowledge What does predicting mean? Pg 9 making a statement or claim about what will happen in the future based on past experience or evidence

  2. What is weight? What do you use to measure weight? Pg 16 the measure of the force of gravity acting on an object. A spring scale is used to measure weight What is mass? What do you use to measure mass? Pg 16 amount of matter in an object . Triple beam balances measure mass What is volume? List 2 ways of measuring volume? Pg 17 amount of space taken up by an object. LxWxH for rectangular solids, water displacement method for irregular solids What is density? What is the formula for density? Pg 18 measure of how much mass is contained in a given volume. Density = mass/volume (D=m/v)

  3. What do line graphs show? Pg 31 they show how the dependent variable changes in response to the independent variable What is a hypothesis? Pg 36 a possible answer to a scientific question What is an independent variable? Dependent variable? Pg 37 Independent- one factor that is purposely changed to test a hypothesis. Dependent- the factor that may change in response to the independent variable How many variables are changed in a controlled experiment? Pg 38 only 1 variable is changed at a time in a controlled experiment

  4. METRIC SYSTEM PREFIXES AND CONVERSIONS (K-H-D-U- d-c-m) A scientific explanation is? Pg 42 drawing a conclusion from an experiment

  5. Chapter 2 What is observing? Pg 53 using your senses to gather information What is objective reasoning based upon? What is subjective reasoning based upon? Pg 56 Obj- reasoning based on evidence. Subj- based on personal feelings or personal values Scientific method is characterized by what? What does it rely upon? Pg 59 characterized by an ordered approach to learning about the world. Relies on objective analysis of data obtained thru careful observation What is a model? Why do scientists use models? Pg 61 any representation of an object or process. To test their ideas about things they cannot observe directly

  6. What is feedback? Give 1 example. Pg 63 output that changes a system in some way. Ex. When you exercise your heart receives feedback that makes your heart pump faster A scientific theory is? Pg 69 well tested explanation for a wide range of observations and experimental results A scientific law describes what? Pg 70 what scientists expect to happen every time under a particular set of conditions

  7. Understanding scientific research and thinking can help societies do what? Pg 72 make good decisions and solve problems in everyday life What are social concerns? How does science help with social concerns? Pg 77 are ideas people have about how they should treat others and the world around them. By providing people with housing, protecting the environment, treating and preventing disease

  8. Mid Term Examination Study Guide Chapter 7 and 8

  9. Chapter 7 • What is matter? It is anything that has mass and takes up space. • What is a substance? It is one type of matter, that is composed of a specific make up or composition. Examples – water, salt • What is the basic particle from which all elements are made of? Atoms • What is a chemical bond? Is the force of attraction between 2 or more atoms. • What does a chemical formula show? Shows the elements and the ratio in a molecule/compound Examples – H2O, N3

  10. What is a solid? a stage of matter that has a definite shape and definite volume. 2 types of solids – a) Crystalline=particles are arranged in a regular, repeating pattern (salt). b) Amorphous=particles are not arranged in a regular pattern (rubber). What is a liquid? It is a state of matter that has NO definite shape but a definite volume.

  11. What is surface tension? Inward force or pull among the molecules in a liquid that brings the molecules at the top closer together. What is viscosity? Is a liquid’s resistance to flow e.g. honey. • What is gas? State of matter in that has NO definite shape or volume. • What is pressure? The pressure of a Gas is the force of its outward push divided by the area of the wall. Pressure=Force (N)/Area(m2)

  12. The freezing point of water is 0o Celsius; this is the same as its melting point. What is vaporization? It is a change in state from liquid to gas. A) Evaporation =when this occurs at the surface B) Boiling=when this occurs below and at the surface of a liquid What is condensation? It is the reverse of vaporization; it is a change from gas to solid. What is sublimation? It is the change from solid to gas (skipping liquid) as in Dry Ice.

  13. Chapter 8 • What is weight? It is the measure of the force of gravity on matter. • What is mass? It’s the amount of matter in an object. The amount of matter doesn’t change, but weight changes – it depends upon gravitational pull. • 2 ways to calculate volume: For Volume in a square-shaped Object is V=LxWxH (M3) Volume of an irregular-shaped item use water displacement. (mL)

  14. What is density? Is the measure of the mass of a material in a give volume. Density=Mass (grams)/Volume (m3 or mL) • What determines if an object can float or sink? If an object has a density greater than water, it will sink. Water Density = 1,000.00 kg/m³ • What is physical property? A characteristic of a substance that can be observed without changing it into another substance. Examples=luster, malleability, ductile

  15. What is a chemical property? Characteristic of a substance that describes its ability to change into different substances. Examples= flammability, reactivity • What is a physical change? When the appearance or form of a substance has changed, but no new substance is created/produced. Examples = breaking, bending, crushing, dissolving

  16. What is a chemical change/reaction? Is a change in matter that produces one or more new substances. Outcome = 1 or more new Examples = Photosynthesis, hydrogen peroxide poured on the skin, breaking down of food in one’s stomach

  17. MID TERM STUDY GUIDE CHAPTER 9

  18. 1. How did Mendeleev organize the first periodic table? Pg 315 • By increasing atomic mass 2. Define and list location of the following. Nucleus, proton, neutron, electron. Pg 318 • Nucleus – Neutral, nucleus • Proton – Positive, nucleus • Neutron- neutral, nucleus • Electron – Negative, Electron Cloud 3. What is the atomic number? Same as the number of? Pg 318 • Number of Protons, same as number of electrons.

  19. 4. A neutral atom has the same number of what 2 particles? Pg 318 • Protons and Electrons 5. An element’s properties can be predicted from its what? Pg 322 • Group ( Number of Valence Electrons) 6. What is a period? In which direction do they go? Pg 322 • Series of elements going across left to right. 7. Elements in the same period follow the same what? Pg 322 • Repeating pattern of properties

  20. 8. What is a group? Which direction do they go? Pg 323 • Column of elements with similar properties going up and down 9. The majority of the elements on the periodic table are what? Pg 325 • Metals 10. List and define the 4 physical properties of metals. Pg 326 • Malleable Ductile • Luster Conductive (thermal and electrical)

  21. 11. In which group would you find the alkali metals? What’s special about group 1? Pg 328 • Group 1. Most reactive metals in table. 12. Most non-metals exist in which state of matter? Pg 333 • Gases 13. Which group contains elements important to the chemistry of life? Pg 335 • Group 14 – Carbon Family

  22. 14. Which elements make up the halogen family? Pg 337 • Fluorine (F) , Chlorine (Cl) ,Bromine(Br and Iodine(I) 15. Which group contains the noble gasses? Why are the called noble? Pg 338 • Group 18. Do not bond “mix w/others” easily. 16. What is a metalloid? Pg 339 • Element that has some properties of metals and nonmetals. 17. What did Rutherford’s model of the atom suggest about the nucleus? Pg 344 • That it is mostly open space with positive center.

  23. Chapter 10

  24. What is a valence electron? Pg 359 • Electron with highest energy level, outermost level (shell), does bonding • What does the number of valence electrons determine? Pg 359 • How reactive element is (chemical property) • What is an ion? Pg 365 • Atom or group of atoms that has a charge from gaining or losing electrons.

  25. 4. When a neutral atom loses a valence electron it becomes what? Pg 365 • An Ion with a positive charge. 5. When a neutral atom gains a valence electron it becomes what? Pg 365 • An ion with a negative charge. 6. What is an ionic bond? Pg 366 • A bond between two or more oppositely charged ions.

  26. What is an ionic compound? What is its overall charge? Pg 366 • Substance formed by ionic bonds. Neutral • What is a covalent bond? Pg 369 • Bond formed when 2 atoms share electrons between them and form a new substance.

  27. Study GuideChapter 11 1. What is the difference between a pure substance and a mixture? Pg 391 Pure substance is a single kind of matter that has a specific makeup Mixture is two or more substances together in the same place but their atoms are not chemically bonded

  28. 2. Contrast heterogeneous and homogeneous mixtures and give two examples of each. Pg 393 • Heterogeneous – mixture in which you can see the different parts and can easily separate them (trail mix/oil and vinegar salad dressing) • Homogeneous - mixture evenly mixed you can’t differentiate the parts by looking at the mixture (salt water/metal alloy like brass)

  29. 3. Name and describe 4 ways mixtures can be separated. Pg 395 Filtration – separation by pouring through a filter Magnetic Attraction – iron objects can be separated from a mixture using a magnet Distillation – liquids can be separated from each other by heating the mixture to the boiling point of one of the substances, changing it to a gas, then condensing to the separated liquid Evaporation – leave in open air allowing liquid to evaporate, leaving solid components behind

  30. 4. Define the terms solution, solvent, and solute. Pg 397 Solution – mixture containing a solvent and at least one solute and has the same properties throughout Solvent – part of a solution usually present in the largest amount; it dissolves the other substances Solute – the substance that is dissolved by the solvent

  31. 5. How are colloids and suspensions different from solutions? Pg 399 Solutions have the same properties throughout with molecules or ions that are too small to see, while both colloids and suspensions have particles that are not dissolved. Colloid - particles do not settle out and are too small to see without a microscope, but are large enough to scatter a beam of light Suspension – particles can be seen and can be easily separated by filtration or settling

  32. 6. Explain the differences between a dilute solution, a concentrated solution, and a saturated solution. Pg 403 Dilute Solution – mixture that has only a little solute dissolved in a certain amount of solvent Concentrated Solution – mixture that has a lot of solute dissolved in the solvent Saturated Solution – so much solute has been added no more will dissolve

  33. 7. Name and describe three factors that affect solubility. Pg 405 Pressure – solubility of a gas solute in a liquid solvent increases as the pressure of the gas over the solution increases Solvents – solute and solvent must be compatible; ionic and polar compounds usually dissolve in polar solvents and nonpolar compounds dissolve in nonpolar solvents Temperature – with most solid solutes solubility increases with temperature increase; gases become less soluble with temperature increase

  34. Study GuideChapter 12 1. Explain the law of conservation of mass. Pg 418 Matter is not created or destroyed in any chemical or physical change. 2. Contrast exothermic and endothermic reactions in terms of heat. Pg 419 Exothermic Reaction – energy in the form of heat is released during a chemical reaction Endothermic Reaction – energy in the form of heat is absorbed from the surrounding area during a chemical reaction

  35. 3. What are three ways to detect chemical change? Describe each. Pg 421 Formation of a precipitate – mix two liquids and solid forms Gas is produced – solid or liquid reactants may release bubbles Color is changed – reaction that results in a color change may signal a new substance 4. What is the structure of a chemical equation, in terms of reactants and products? Draw it. Pg 423 Reactant + Reactant → Product + Product

  36. 5. What does a coefficient placed in front of a chemical formula in an equation tell you? Pg 427 The coefficient tells the amount of a reactant or a product that takes part in a reaction. 6. Do all chemical reactions need activation energy? Why or why not? Pg 431 All chemical reactions need just enough activation energy for the bonds of the reactants to begin to break. Once the reaction begins, enough energy is usually present to continue the reaction of the remaining reactants.

  37. 7. What are the roles of catalysts, enzymes, and inhibitors in a chemical reaction? Pg 435 Catalysts – increases the reaction rate by lowering the activation energy needed. Enzymes – biological catalysts that help reactions to occur at body temperature. Inhibitor – material used to decrease the rate of a chemical reaction.

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