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Subject:. Date:. Today’s Topic. Chemistry. Jan 24, 2014. Intro to Chemistry. Today’s Starter Question:. I n your own words, describe the term Chemistry. Answer:. The study of matter and it’s changes. Today’s Objectives:. One:.

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  1. Subject: Date: Today’s Topic Chemistry Jan 24, 2014 Intro to Chemistry Today’s Starter Question: In your own words, describe the term Chemistry Answer: The study of matter and it’s changes. Today’s Objectives: One: Gain an understanding of terms related to basic chemistry Two: Three: Receive an introduction to Chemistry Summary Notes: Next Page

  2. Subject: Date: Today’s Topic Chemistry Jan 27, 2014 Intro to Chemistry Today’s Starter Question: Define substance Answer: A substance, also known as a chemical, is matter has a definite composition. Today’s Objectives: Explain the formation and importance of ozone. One: Describe the development of chlorofluorocarbons. Two: Three: Matter: anything that has mass and takes up space. Chemistry is the study of everything around us All the stuff in the universe is made from building blocks formed in the stars. Summary Notes: Next Page

  3. Chemistry Notes Continued These building blocks and everything Made from them Are called matter. Chemistry is the study of matter and the changes it undergoes. Ultraviolet light damages living organisms. Earth's atmosphere contains a layer of ozone that absorbs ultraviolet light and protects living organisms. The Exosphere: 500 km Thermosphere: between 85 km and 500 km Mesosphere: between 50 and 85 km Stratosphere: between 10 and 50 km Troposphere: from the ground up to 10 km Ozone is a substance in the atmosphere made up of oxygen. A substance, also known as a chemical, is matter has a definite composition. Summary Notes: Next Page

  4. Chemistry Notes Continued Ozone is born when oxygen gas is exposed to ultraviolet radiation. And the mid-1980s, scientists detected in areas in the ozone layer over Antarctica. What do because I know zone hole? Chlorofluorocarbons, (CFCs) argues as coolant in refrigerators and propellant in aerosol cans. CFCs were considered safe because they are not toxic and don't react to other chemicals, CFCs were 1st detected in the atmosphere in the 1970s, and the concentration continued to increase through the 1990s. Was there a connection between ozone thinning and increasing CFCs in atmosphere? All of the stuff in the universe is made of a. Mixtures b. Matter c. O zone d. Mass Which of the following protects living organisms from harmful ultraviolet light? A. CFC B. Oxygen gas C. Exosphere D. Ozone Compare and contrast mass and weight Explain why chemists are interested in a submicroscopic description of matter. Summary Notes: Next Page

  5. Subject: Date: Today’s Topic Chemistry Jan 28, 2014 Intro to Chemistry Today’s Starter Question: Explain why chemists are interested in a submicroscopic description of matter. Answer: The structure, composition, and behavior of all matter can be described on this sub microscopic atomic level . Today’s Objectives: Identify the areas of emphasis the various branches of chemistry. One: Two: Technology: a practical application of scientific information. Three: Branches of chemistry involve the study of different kinds of matter. Matter has many different forms mass is a measurement that reflects the amount of matter. Weight is a measure of mass and the force of gravity on in object. Summary Notes: Next Page

  6. Chemistry Notes Continued Weight can change from place to place, but mass is constant. Much of matter and his behavior is macroscopic Meaning that it can be observed without a microscope. The structure, composition, and behavior of all matter can be described on this sub microscopic atomic level Chemistry explains events on the atomic level that causes macroscopic observations. A model is a verbal, visual, or mathematical explanation of experimental data A model is a verbal, visual, or mathematical explanation of experimental data Branches Area of emphasis Examples of emphasis Organic chemistry pharmaceuticals, plastics most carbon containing chemicals minerals, in general, mattered at does not contain carbon Inorganic chemistry the behavior and changes a matter and the related energy changes reaction rates reaction mechanisms Physical chemistry Analytical chemistry food nutrients components and composition of substance matter and processes of living organisms Metabolism fermentation Biochemistry Summary Notes: Next Page

  7. Chemistry Notes Continued pollution, biochemical cycles Environmental chemistry matter and the environment Industrial chemistry chemical processes in industry paints coatings Polymer chemistry polymers and plastics textile coating and plastic Theoretical chemistry chemical interactions any areas of emphasis heat of reaction Thermo chemistry It’s involved in chemical processes Summary Notes: Next Page

  8. Subject: Date: Today’s Topic Chemistry Jan 29, 2014 Intro to Chemistry Today’s Starter Question: In your own words, describe the difference between a theory and a scientific law Answer: A theory is an explanation that has been repeatedly supported by many experiments. A scientific law is a relationship in nature that is supported by many experiments and no exceptions to these relationships are found. . Today’s Objectives: Gain an understanding of scientific inquiry and learn the systematic approach which is an organize method of solving a problem. One: Two: Three: Scientists use scientific methods to systematically pose and test solutions to questions and assess the results of the tests. The scientific method is a systematic approach used in scientific study, whether it is chemistry, physics, biology, or another science. It is an organized process used by scientists to do research, and provides methods for scientist to verify the work of others. Summary Notes: Next Page

  9. Chemistry Notes Continued The steps in a scientific method are repeated until a hypothesis is supported or discarded An observation is the act of gathering information. Qualitative data is obtained through observations that describe color, smell, shape or other physical characteristics that is related to the 5 senses A hypothesis is a tentative explanation for what has been observed. Quantitative data is obtained from numerical observations that describe how much, how little, how big or how fast. In experiment is a set of controlled observations that test the hypothesis. A variable is a quantity or condition that can have more than one value An independent variable is the variable you plan to change. The dependent variable is the variable of the changes in value in response to the change in the independent variable. A control is a standard for comparison in an experiment A conclusion is a judgment based on the information obtained from the experiment. Summary Notes: Next Page

  10. Chemistry Notes Continued A hypothesis is never proven, only supported or discarded. A model can be used to make predictions. Molina and Rowland's motto show how CFCs could destroy the ozone. Ultraviolet radiation combines with oxygen. A theory is an explanation that has been repeatedly supported by many experiments. A theory takes a broad principle of nature that has been supported over time by repeated testing. Theory are successful if they can be used to make predictions that are true. A scientific law is a relationship in nature that is supported by many experiments and no exceptions to these relationships are found. Compare and contrast pure research, applied research, and technology Apply knowledge of laboratory safety synthetic: something that is human made and does not necessarily occur in nature. Summary Notes: Next Page

  11. Chemistry Notes Continued Some scientific investigations result into development of technology that can improve our lives and the world around us. Pure research is research to gain knowledge for the sake of knowledge itself. Applied research is research undertaken to solve a specific problem. Chance discovery occurred when scientists obtain results that are far different from what they expected You are responsible for your safety and the safety of others around you Applied research showed that CFCs and a few other chemicals react with the ozone many nations agreed in 1987 to the Montréal protocol, to phase out CFC use. From 1986 to 2000 CFCs in antarctica parts for Treo dropped from over 500 to less than 200. Scientists have learned the ozone thinning occurs over antarctica every spring. Chemists solve many real problems we face today such as: Ozone depletion Finding cures for disease Reducing the weight of cars Models are tools that scientists, including chemists use Summary Notes: Next Page

  12. Chemistry Notes Continued Macroscopic observations of matter replant the action of Atoms on a submicroscopic scale. There are several branches of chemistry including organic industry in organic chemistry physical chemistry analytical chemistry and biochemistry Scientific methods are systematic approaches to solving problems. Qualitative data describes an observation; Quantitative data use numbers. Independent variables are changed in an experiment Dependent variables change in response to the independent variable. A theory is a hypothesis that is supported by many experiments. Scientific methods can be use in pure research or in applied research. Some scientific discoveries are accidental, and some are the result of diligent research in response to a need. Laboratory safety is the responsibility of everyone in the laboratory. Many of the conveniences we enjoy today are technological applications of chemistry. Summary Notes: Next Page

  13. Chemistry Test 1. ______ is anything that has_______ and takes up space. B. Mass; manner A. Matter; mass C. Matter; weight D. Weight; mass 2. Chemistry tries to explain_______ observations based on_________ observations. A. Macroscopic; submicroscopic B. Macroscopic; nuclear D. Microscopic; macroscopic C. Atomic; submicroscopic 3. Scientific methods are______ approaches to solving problems. A. Dependent B. Independent D. Systematic C. Hypothetical 4. What are accidental discoveries, like penicillin, called? A. Applied discoveries B. Chance discoveries D. Newton's law C. Pure discoveries 5. Quantitative data describes observations that are _____. A. Numerical B. Conditions D. Hypothesis C. Independent Summary Notes: Next Page

  14. Chemistry Test 6. Which of the following is not an example of qualitative data? A. 1.35 kg B. Red flower C. Green car D. Orange flower 7. What kind of research is done for the sake of knowledge? A. Pure B. Exploratory C. Applied D. Model 8. Which of the following has a definite composition? B. Variable A. Building block D. Mixture C. Substance 9. What varies with change in gravitational force? A. Matter B. Weight D. Composition C. Mass 10. Which of the following would be an example of quantitative data? A. Blue socks B. Square peg D. Loud noise C. 6 kg Summary Notes: Next Page

  15. Chemistry Test 11. Which of the following describes a systematic approach to solving problems? A. Pure research B. Hypothetical method C. Theoretical method D. Scientific method 12. Laboratory safety is the responsibility of everyone in the laboratory. A. Everyone in the Lab B. The science teacher only D. The students in the lab only C. The Principal 13 A control is a __________ for comparison in an experiment A. Independent variable B. Dependent variable D. Response C. Standard 14. Mass can change from place to place, but weight is constant. A. False B. True 15. Dependent variables change in response to the independent variable. A. False B. True Summary Notes: Next Page

  16. Chemistry Test 16. What is the discovery of nylon an example of? A. Pure research B. Applied research C. Variables D. Chance discovery 17. ________ is/are anything that has mass and takes up space. A. Solids B. Building block D. Matter C. Forces 18. Which type of variables are controlled by the scientists? A. Independent B. Dependent D. Response C. Pure 19. Weight is a measure of________ and________. A. Force; gravity B. Mass; gravity D. Gravity; motion C. Matter; mass 20. Producing heat resistant plastics is an example of what kind of research? A. Independent B. Dependent defendant C. Pure D. Applied Summary Notes: Next Page

  17. Chemistry Test 1. ______ is anything that has_______ and takes up space. B. Mass; manner A. Matter; mass C. Matter; weight D. Weight; mass 2. Chemistry tries to explain_______ observations based on_________ observations. A. Macroscopic; submicroscopic B. Macroscopic; nuclear D. Microscopic; macroscopic C. Atomic; submicroscopic 3. Scientific methods are______ approaches to solving problems. A. Dependent B. Independent D. Systematic C. Hypothetical 4. What are accidental discoveries, like penicillin, called? A. Applied discoveries B. Chance discoveries D. Newton's law C. Pure discoveries 5. Quantitative data describes observations that are _____. A. Numerical B. Conditions D. Hypothesis C. Independent Summary Notes: Next Page

  18. Chemistry Test 6. Which of the following is not an example of qualitative data? A. 1.35 kg B. Red flower C. Green car D. Orange flower 7. What kind of research is done for the sake of knowledge? A. Pure B. Exploratory C. Applied D. Model 8. Which of the following has a definite composition? B. Variable A. Building block D. Mixture C. Substance 9. What varies with change in gravitational force? A. Matter B. Weight D. Composition C. Mass 10. Which of the following would be an example of quantitative data? A. Blue socks B. Square peg D. Loud noise C. 6 kg Summary Notes: Next Page

  19. Chemistry Test 11. Which of the following describes a systematic approach to solving problems? A. Pure research B. Hypothetical method C. Theoretical method D. Scientific method 12. Laboratory safety is the responsibility of everyone in the laboratory. A. Everyone in the Lab B. The science teacher only D. The students in the lab only C. The Principal 13 A control is a __________ for comparison in an experiment A. Independent variable B. Dependent variable D. Response C. Standard 14. Mass can change from place to place, but weight is constant. A. False B. True 15. Dependent variables change in response to the independent variable. A. False B. True Summary Notes: Next Page

  20. Chemistry Test 16. What is the discovery of nylon an example of? A. Pure research B. Applied research C. Variables D. Chance discovery 17. ________ is/are anything that has mass and takes up space. A. Solids B. Building block D. Matter C. Forces 18. Which type of variables are controlled by the scientists? A. Independent B. Dependent D. Response C. Pure 19. Weight is a measure of________ and________. A. Force; gravity B. Mass; gravity D. Gravity; motion C. Matter; mass 20. Producing heat resistant plastics is an example of what kind of research? A. Independent B. Dependent defendant C. Pure D. Applied Summary Notes: Next Page

  21. Chemistry Jan 30, 2014 Subject: Date: Today’s Topic SI Units Today’s Starter Question: Why do you think we use the SI for the standards worldwide? Answer: To keep all research consistent all around the world. Today’s Objectives: Learn SI base units. One: Learn prefixes used with SI units Two: Learn how to recognize and determine significant digits Three: SI Based Units. Base quantity Base Unit Symbol Length meter m Mass kilogram kg Time second s Temperature kelvin K Amount of Substance mole mol Electric current ampere A Luminous candela cd Summary Notes: Next Page

  22. Chemistry Jan 31, 2014 Subject: Date: Today’s Topic SI Units Today’s Starter Question: Write the symbols for the following base quantities: Length, Mass, Time, Temperature, Amount of Substance,Electric Current Luminous Intensity. Answer: m, kg, s, K, mol, A, cd Today’s Objectives: “Continued:” Learn prefixes used with SI units One: Learn how to recognize and determine significant digits Two: Three: Prefixes Used with SI Units Prefix Symbol Multiplier Scientific Notation Example femto f 0.000000000000001 10 -15 femtosecond (fs) pico p 0.000000000001 10 -12 picometer (pm) nano n 0.000000001 10 -9 nanometer (nm) micro µ 0.000001 10 -6 microgram (µg) -3 milli m 0.001 10 milliamps (mA) -2 centi c 0.01 10 centimeter (cm) deci d 0.1 10 -1 deciliter (dL) 3 kilo k 1000 10 kilometer (km) mega M 1,000,000 10 6 megagram (Mg) 9 giga G 1,000,000,000 10 gigameter (Gm) tera T 1,000,000,000,000 10 12 terahertz (THz)

  23. Student input: Atom e- Protons Nucleus p+ n Neutrons e- Electrons

  24. Student input: Covalent Bond Molecule of Water p+ e- e- e- Protons e- p+ e- e- 8p+ Nucleus 8n e- Neutrons e- e- e- The 1st energy level can hold 2 electrons H O 2 The second energy level can hold 8 electrons Electrons

  25. Chemistry Feb 4, 2014 Biochemistry Subject: Date: Today’s Topic Today’s Starter Question: Explain the characteristics of the neutron, proton and electron . Neutrons and protons are located at the center of the atom which is called the nucleus. Protons are positively charged particles (P+). Electrons are negatively charged particles (E-) located on the outside of the nucleus. Electrons constantly move around the nucleus in energy levels. Answer: Today’s Objectives: Diagram the particles that make up an atom. Compare covalent and ionic bonds. One: An element is a pure substance that cannot be broken down into other substances By physical or chemical means. Elements are made of only one type of atom. Two: The periodic table of elements is organized into horizontal rows, called periods, and vertical columns called groups. Three: Atoms of the same element that have a different number of neutrons are called isotopes. Isotopes that give off radiation are called radioactive isotopes. A compound is a pure substance formed when two or more different elements combine. Compounds are always formed from a specific combination of elements in a fixed ratio. Compounds are physically and chemically different than the elements that comprise them. Compounds cannot be broken down into simpler compounds or elements by physical means, however, they can be broken down by chemical means. Summary Notes: Next Page

  26. Student input: Covalent Bond Molecule of Water e- p+ e- e- e- Protons e- e- p+ 8p+ Nucleus e- 8n e- Neutrons e- e- H O 2 Electrons

  27. Student input: Chapter 6 Ionic Bond: e- 7 e- 8 e- 8 e- 8 e- 8 e- 8 e- 2 e- 11 p+ 2 e- 17 p+ 11 p+ 17 p+ 11 n 2 e- 2 e- 11 n 17 n 17 n + + Sodium atom + Chlorine atom Sodium ion + Chlorine ion + NaCl Na Cl

  28. Chemical properties, such as reactivity, depend on an element’s electron configuration: When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. The chemical properties of an element depend on the number of valence electrons. These atoms all have two valence electron These atoms all have four valence electron These atoms all have six valence electron These atoms all have one valence electron Example These atoms all have three valence electron These atoms all have five valence electron These atoms all have Seven valence electron Electron Dot Diagrams for Some Group A Elements Group 7A 8A 2A 3A 4A 5A 6A 1A These atoms all have eight valence electron He H F C N O Be B Ne Li Al Na Mg Si Cl Ar P S Ga K Mg Ge As Kr Se Br two electron in outer most shell three electron in outer most shell four electron in outer most shell eight electron in outer most shell one electron in outer most shell five electron in outer most shell six electron in outer most shell seven electron in outer most shell

  29. Chemistry Subject: Date: Today’s Topic Scientific Notation Feb 6, 2014 Today’s Starter Question: Write the following numbers using scientific notation: 0.000000001, 0.000000000000001, 15,000,000, 19,000, 0.0000001, 1,000,000,000,000 Answer: -9 -15 7 4 -7 12 10 10 1.5 X 10 1.9 X 10 1.0 X 10 10 Today’s Objectives: One: Obtain a clear understanding of determining significant digits. Two: Three: Obtain a clear understanding of scientific notation Summary Notes: Next Page

  30. Scientific Notation 243,500,000,000 0.000000001 - 9 11 2.435 X 10 1.0 X 10 0.0000000231 0.00030007 - 4 - 8 3.0007 X 10 2.31 X 10

  31. Scientific Notation Precision is less precise than 30.0 m 30.01 and 30.01 is less precise than 30.001 5 X 10.3 = 51.5 The answer has to be 52 Because 5 is the least precise number in the equation

  32. Subject: Date: Today’s Topic Scientific Notation Today’s Starter Question: Identify the significant digits in the following numbers: 0.089, 5.3098, 78.10001, 4.21, 3.1 Answer: 2, 5, 7, 3, 2 Today’s Objectives: One: Distinguish between accuracy and precision. Two: Determine the precision of measured quantities. Three: Measurements quantify our observation. A measurement is a comparison between an unknown quantity and a standard. The degree of exactness of a measurement is called its precision. The precision of a measurement is one half the smallest division of the instrument. Summary Notes: Next Page

  33. Subject: Date: Sept. 28, 2011 Today’s Topic Scientific Notation Principles of Science Today’s Starter Question: Identify the significant digits in the following numbers: 0.089, 5.3098, 78.10001, 4.21, 3.1 Answer: 2, 5, 7, 3, 2 Today’s Objectives: “Continued” One: Distinguish between accuracy and precision. Two: Determine the precision of measured quantities. Three: A measure of 67.100 g is precise to the nearest thousandth of a gram. Accuracy describes how well the results of a measurement agree with the “real” value; that is the accepted value as measured by competent experimenters A common method for checking the accuracy of an instrument is called the two point calibration. Does the instrument read 0 when it should and secondly give a correct reading when it is measuring an accepted standard Summary Notes: Next Page

  34. Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: In your own words, explain the difference between multiplying and dividing using scientific notation Answer: The main difference is the fact that you will add the exponents when multiplying and you will subtract the exponent of the divisor from the exponent of the dividend when you divide Today’s Objectives: One: Obtain an understanding of how to multiply and divide using scientific notation. Multiply the values of M and add the exponents n. Multiply the units. Two: 3 11 3 + 11 = (4 X 5) X 10 kg.m Example: (4 X 10 kg) (5 X 10 m) Three: 14 = 20 X 10 kg.m 15 = 2.0 X 10 kg.m Divide the value of M and subtract the exponent of the divisor from the exponent of the dividend. 6 3 8 X 10 m 2 X 10 m 8 2 Example: 6 – (-3) 3 - 2 = X 10 m -3 2 9 = 4 X 10 m Summary Notes: Next Page

  35. Scientific Notation Practice Multiplying and Dividing using Scientific Notation 4 9 4 + 9 (6 X 10 kg) (6 X 10 m) (6 X 6) X Kg.m = 10 13 = 36 Kg.m X 10 14 X 10 Kg.m = 3.6

  36. Scientific Notation Practice Multiplying and Dividing using Scientific Notation 8 4 9 X 10 m 9 - 4 4 2 8 - = 10 m X 4 2 m 3 3 X 10 2 4 X m = 3 10

  37. Multiplying and Divding Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: 4 5 Work the following problem: (5 X 10 kg) (3 X 10 m) 4 + 5 Answer: = (5 X 3) X 10 kg.m 9 = 15 X 10 kg.m 10 = 1.5 X 10 kg.m Today’s Objectives: One: Gain an understanding of how to add and subtract using the scientific notation: You can not add or subtract unlike terms. Two: Three: Practice the problems on the following pages to secure a complete understanding of how to add and subtract using scientific notation. Summary Notes: Next Page

  38. Scientific Notation First Period Practice Adding and Subtracting using Scientific Notation 9 8 9 9.0 X 10 kg + 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal one digit to the left. This causes the exponent to rise by 1 9 kg 0.9 X 10 Now, rewrite the equation like this This is the correct answer. 9 Make sure you line the decimals up 7.0 10 kg X 7.9 X kg 10 Now, simply add the bases and leave the exponents as is 9

  39. Scientific Notation All Periods: Practice Adding and Subtracting using Scientific Notation 8 8 6 9.0 X 10 kg - 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal two digits to the left. This causes the exponent to rise by 2 8 kg 9.0 X 10 Now, rewrite the equation like this This is the correct answer. 8 Make sure you line the decimals up - 0.07 10 kg X Now, simply subtract the bases and leave the exponents as is 8.93 X kg 10 8

  40. Multiplying and Divding Scientific Notation Subject: Date: Today’s Topic Today’s Starter Question: 5 4 Work the following problem: 5.0 X 10 kg + 3.0 X 10 kg 5 Answer: kg = 5.0 X 10 + 5 0.3 X kg 10 This is the correct answer 5 kg 5.3 X 10 Today’s Objectives: One: Learn how to convert related SI units: Standard: A standard is an exact quantity that people agree to use to compare measurements. Two: Three: Measurement: The dimensions, capacity, or amount of something. The international system of units, which is used to keep research consistent around the world. SI: Volume: The amount of space occupied by an object is called its volume. Mass: A measurement of quantity of matter in an object. Density; Is the mass per unit volume of a material. Summary Notes: Next Page

  41. Scientific Notation Problem # 3 9 7 9 9.0 X 10 kg + 5.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal two digits to the left. This causes the exponent to rise by 2 9 kg 0.09 X 10 Now, rewrite the equation like this This is the correct answer. 9 Make sure you line the decimals up +5.00 10 kg X 5.09 X kg 10 Now, simply add the bases and leave the exponents as is 9

  42. Scientific Notation Problem # 4 7 7 4 4.0 X 10 kg - 7.0 X 10 kg Currently, these two terms are not alike in regard to scientific notation. The exponents are not the same In order to make the exponents the same Move the decimal three digits to the left. This causes the exponent to rise by 3 7 kg 4.000 X 10 Now, rewrite the equation like this This is the correct answer. 7 Make sure you line the decimals up - 0.007 10 kg X Now, simply subtract the bases and leave the exponents as is 3.993 X kg 10 7

  43. Chemistry Test 1 Matter is composed of small particles called ________. B. Particles A. Atoms C. Molecules D. ions 2. Atoms are made up of smaller particles called _______. A. pure compounds B. Ions D. neutrons, protons and electrons C. pure substances 3. A sub atomic particle that carries a negative charge. A. proton B. electron D. molecule C. neutron 4. A sub atomic particle that is located outside the nucleus . A. electron B. charge D. neutron C. proton 5. Elements on the periodic table that have the same number of electron in the outer shell are in the same _______ A. period B. level D. class C. group

  44. Chemistry Test 6. An isotope is an atom that has a different number of _____________. A. proton vs. electrons B. Ions vs particles C. neutrons vs. protons D. molecules vs atoms 7. A carbon atom that has 8 neutrons is called a(n) __________ . A. pure molecule B. isotope C. ion D. model 8. The atomic number tells you the number of ___________ that’s in an atom. B. variables A. Protons or electrons D. ions C. charges 9. A(n) _____ is a pure substance formed when two or more different elements combine. A. charged particle B. isotope D. compound C. neutral particle 10. Compounds can be broken down chemically. A. true B. false Summary Notes: Next Page

  45. Change the following numbers into Scientific Notation 11. 0.000000001 12. 0.000003001 14. 19, 000, 100 13. 243,500, 000, 000 15. 0.0000563

  46. Write the number of significant digits 16. 0.000000001 17. 0.000003001 19. 19, 000, 100 18. 243,500, 000, 000 20. 0.0000563

  47. Solve the following problems: 8 9 21. 5.0 X 10 kg + 3.0 X 10 kg 8 4 9 X 10 m 22. 4 2 m 3 X 10 7 9 23. 9.0 X 10 kg + 5.0 X 10 kg 7 5 24. 4.0 X 10 kg - 7.0 X 10 kg

  48. Converting SI Units A conversion factor is a ratio that is equal to one and is used to change One unit to another. For Example, There are 1,000 mL in 1 L, so 1,000 mL = 1 L. If both sides of this equation are divided by 1 L, the equation becomes: 1,000 mL = 1 1L To convert units, you multiply by the appropriate conversion factor. For Example, To convert 1.255 L to mL, multiply 1.255 L by a conversion factor. Use the conversion factor with new units (mL) in the numerator (on top), and the old units (L) in the denominator (on bottom). 1,000 mL = 1.255 L X 1,255 mL 1L Do all conversions using this concept.

  49. Converting SI Units Convert 1,567 centimeters to millimeters. 100 mm 1,567 cm 156,700 mm = = 1 cm Convert 520 kilometers to meters. Convert 55.012 kilograms to grams. Convert 1,000,000 micrometers to centimeters.

  50. Converting SI Units How long in centimeters is a 3,075 mm rope? Identify known values and the unknown value. Identify the known values. The rope is 3,075 mm 1m = 100 cm = 1,000 mm Identify the unknown value. How long in centimeters (cm). Solve the problem. This is the equation you need to use: 100cm ? Cm =3,075 mm X 1000 mm Cancel units and multiply: 100cm 3,075 mm X = 307.5 cm 1000 mm

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