d. Differentiate between the following experiments as basic (pure) science or technology (label the following examples) (pg 7)

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Physical Science Fall 08 Semester Review Name 10. There will be a reading section on the test.. 11. General Science Knowledge [Chapter 1] a. What two things are studied in physical science?

1 Physical Science Fall 08 Semester Review Name 10. There will be a reading section on the test General Science Knowledge [Chapter 1] a. What two things are studied in physical science? (hint: physics and chemistry are not the answer) _matter_ and energy_ b. Define the steps of the scientific method and related vocabulary (be able to recognize applications) i. Experiment(pg 13) an organized procedure for testing a hypothesis ii. Hypothesis(pg 13) possible answer that is testable iii. Variable(pg 13) a factor that changes in an experiment iv. Control(not in book) a standard for comparison (normal conditions) v. Constant(pg 14) a variable that does not change vi. Dependent variable(pg 21)variable investigated/measured in the experiment vii. Independent variable(pg 21) variable changed by the experimenter c. What is the difference between a science law and a science theory? i. Science theory _- theories explain the natural world ii. Science law _-describe the natural world, often in the form of a math equation_ d. Differentiate between the following experiments as basic (pure) science or technology (label the following examples) (pg 7) i. The determination of the age of the universe pure science ii. The determination of the best material for car safety _ technology iii. Study growth of plant life in a pond pure science iv. Study of the length of a Mars year _ pure science v. Develop models to predict weather patterns on Earth _technology e. When should you use each type of graph? i. Bar graph(pg 21) comparing numbers of different things ii. Circle or Pie graph(pg 21) dividing up a whole, percentage iii. Line graph(pg 21) x-y data, trends/changes in time f. Know how to measure and convert measurement units(pg 16, reading not covered) i. How many meters in 26 centimeters? 0.26 m ii. What is the reading on the graduated cylinder? 38 ml_ 12. Classification of Matter[mainly chapter 2] Vocabulary: Mixture Two or more substances that do not chemically combine Substance_elements and compounds, matter that has definite properties Page 7 of 7

2 physical property_features that are descriptive (mass, length, color, ) chemical property_potential to undergo a chemical change (flammable, reactivity ) physical change_change in matter that does not change the chemical properties chemical change_occurs when a substance changes form making new substances element_substance that cannot be separated or broken down by chemical means compound_substance made of two or more types of atoms chemically connected sublimation(pg 75)_change in state of matter from a solid to a gas (does not melt) 13. Atomic structure [chapter 4] a. What is a chemical symbol? an abbreviation version of the name of a chemical element name (found in the periodic table) b. Complete the following table Particle Relative Mass (amu) Charge Location in atom electron ~0-1 electron cloud Neutron 1 0 Inside nucleus proton 1 +1 Inside nucleus c. What is the difference between the atomic number and the atomic mass of an atom? Atomic number is the number of protons only while the mass includes the mass of the neutron d. What units are used to express atomic mass? amu (atomic mass unit) e. An atom of some unknown element has 5 neutrons, 4 protons and 4 electrons. (skill) i. What is this atom s atomic number? 4 ii. What is it s atomic mass? 9 (5 + 4) iii. What is the overall charge on this atom? 0 (= #p - #e) iv. Identify the element. Berylleum (4 protons = atomic number 4) v. Draw the Bohr model showing energy levels vi. How would this atom form ions? Would they be positive or negative?it would lose 3 electrons to become +3 ion f. Atoms with the same number of protons but different numbers of neutrons are called isotopes_. 14. Periodic Table [chapter 4] Page 8 of 8

3 a. On the Periodic table, columns of elements represent _groups_ or families, and all have the same number of valence (outer) electrons_. b. Rows of elements are called _periods and represent the outer _energy level/orbitals occupied by these element s valence electrons. c. Elements to the left of on the periodic chart are _metals_ and those to the FAR right are _nonmetals_. d. What is the name of the notation for neon at the right? Dot diagram i. What do the dots represent? Outer (valence)electrons ii. Draw a similar diagram for Chlorine. 15. Chemical reactivity [chapters 4 and 5] a. For most atoms, how many electrons are required in the outer energy level for it to be stable? 8 b. Name 3 ways an atom can stabilize (fill) its outer energy level. Gain electrons, lose electrons, share electrons c. What information is given by a chemical formula? Types of atoms and their ratios d. Explain the function of each in a chemical formula i. subscripts written below, shows the ratio of types of atoms ii. superscripts written above, shows the charge on ions iii. chemical symbol shows the types of atoms in the molecule or ion iv. coefficients show the ratios of substances needed for a reaction e. Complete the following table Periodic Group # of valence e - f. Explain how an ionic bond forms.ions form when atoms gain or lose electrons g. Write the chemical formulas for the following ionic compounds. Remember to balance charges using proper subscripts. KCl CaBr 2 Fe 2 O 3 potassium chloride calcium bromide Iron III Oxide Page 9 of 9

4 h. Write the chemical names for the following ionic compounds. Lithium fluoride sodium sulfide lead chloride LiF Na 2 S PbCl 2 i. Write the formula for the compound formed from the polyatomic ions hydroxide and ammonium, then give the proper chemical name. Ammonium = NH4 + Hydroxide = OH - NH 4 OH = ammonium hydroxide j. Explain how a covalent bond is formed. Electrons are shared by atoms k. What is a polar compound? A covalently bonded molecule that has unequal sharing of electrons so there is a + and - part 16. Properties and names of groups in the periodic table [chapter 5] a. Describe the properties of metals.- shiny, conduct electrons, solid on the left b. Specifically, what do malleable and ductile mean?malleable able to be flattened, ductile able to be drawn into wires c. _alkali metals, (group 1), are the most reactive, as well as _alkaline-earth_ metals (group 2), and therefore only appear as compounds in nature. d. What special designation is given to the metals in groups 3 12? Transition metals/elements e. Noble Gases (Group 18) are inert, do not form compounds. Explain. They have filled outer shells f. The name for this group (group 17) literally means salt former because these elements readily form ionic compounds with metals called salts. halogens g. Why semiconductors given that name? they conduct electrons or heat only under certain conditions h. Why is hydrogen placed in group 1 but classified as a non-metal? It has one valence electron i. Describe three allotropes of carbon. Graphite soft, pencil lead; diamond hard, jewelry; fullerines spherical, like a soccer ball 17. Organic and Biological Compounds [chapter 5] a. Hydrocarbons contain only what 2 elements? H and C only Page 10 of 10

5 b. Name the following compounds: Methane Propene Butyne Benzene c. Which of the above are saturated? Explain.Methane all single bonds d. Which of the above are aromatic? Explain.Benzene ring structure e. Match the term on the right with the group it best fit on the left. 5. Proteins 6. Nucleic Acids 7. Carbohydrates 8. Lipids 18. Chemical Reactions [chapter 6] a. DNA & RNA 2 b. starch 3 c. glucose & fructose 3 d. olive oil 4 e. cholesterol 4 f. amino acids 1 a. How many atoms of each element are in the following compounds Na 2 SO 4 Na 2 S 1_ O 4_ Ba(OH) 2 Ba _1_ O 2_ H 2_ (NH 4 ) 3 PO 4 N _3 H 12 P 1 O 4 b. In a chemical equation the substances on the left of the are called _reactants_ and those on the right are called products. c. Differentiate between catalysts and inhibitors i. Catalysts speed up reaction rates ii. Inhibitors slow down reaction rates d. In a combustion reaction, oxygen reacts with another substance to produce _CO 2 and water. e. Balance each equation and indicate what type it is: synthesis, decomposition, single-displacement, double displacement, combustion Reaction Type i. AlBr 3 + K KBr + Al _single displacement ii. CH 4 + O 2 CO 2 + H 2 O _combustion iii. Bi + F 2 BiF 3 synthesis iv. Al 2 O 3 Al + O 2 decomposition v. FeO + PdF 2 FeF 2 + PdO double displacement Page 11 of 11

6 f. When there is a net release of energy during a chemical reaction ( usually in the form of heat) it is exothermic but if energy is absorbed and then temperature decreases it is _endothermic. g. _activation energy is the minimum amount of energy needed to start a reaction. h. What is a mole? (The physical unit not the cute little animal that burrows n the ground or the hairy thing growing on your neighbor s arm.) (ancillary reference)a mole is a unit related to number of atoms (1 mole = 6.02 x atoms) and is related to the molar mass i. Calculate the mass in grams of the following i. 1 mole of argon 40grams (40 x 1) ii. 2 moles of carbon 24 grams (12 x 2) iii. 1 mole of sodium chloride [NaCl] ~ 58.5grams ( ) iv. 1 mole of calcium carbonate [CaCO 3 ] 100grams ( (3 x 16)) Page 12 of 12

Lab safety and equipment: Sig Figs and Metric Conversions. Matter. Chemistry Review

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