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Review for Advanced 7th Grade Final Exam

Review for Advanced 7th Grade Final Exam. Dr. Makin Clarence Middle School. Scientific Method. Metric Conversions Ladder Method. T. Trimpe 2008 http://sciencespot.net/. 1. 2. 3. Meters Liters Grams. How do you use the “ladder” method? . 1 st – Determine your starting point.

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Review for Advanced 7th Grade Final Exam

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  1. Review for Advanced 7th Grade Final Exam Dr. Makin Clarence Middle School

  2. Scientific Method

  3. Metric Conversions Ladder Method T. Trimpe 2008 http://sciencespot.net/

  4. 1 2 3 MetersLitersGrams How do you use the “ladder” method? 1st – Determine your starting point. 2nd – Count the “jumps” to your ending point. 3rd – Move the decimal the same number of jumps in the same direction. Starting Point Ending Point __. __. __. 2 3 1 Ladder Method KILO1000Units HECTO100Units DEKA10Units DECI0.1Unit CENTI0.01Unit MILLI0.001Unit 4 km = _________ m How many jumps does it take? 4. = 4000 m

  5. 1 mile 1.6 kilometers 1 yard = 0.9444 meters 1 inch = 2.54 centimeters English vs. Metric Units Which is longer? A. 1 mile or 1 kilometer B. 1 yard or 1 meter C. 1 inch or 1 centimeter Left Image: http://webapps.lsa.umich.edu/physics/demolab/controls/imagedemosm.aspx?picid=1167Right Image: http://share.lancealan.com/N800%20ruler.jpg

  6. A. 1 meter or 105 centimeters B. 4 kilometers or 4400 meters C. 12 centimeters or 102 millimeters D. 1200 millimeters or 1 meter km Metric Units m cm mm The basic unit of length in the metric system in the meter and is represented by a lowercase m. Standard: The distance traveled by light in absolute vacuum in 1⁄299,792,458 of a second. Metric Units 1 Kilometer (km) = 1000 meters 1 Meter = 100 Centimeters (cm) 1 Meter = 1000 Millimeters (mm) Click the image to watch a short video about the meter. Which is larger?

  7. 1 centimeter = 10 millimeters What is the length of the line in centimeters? _______cm What is the length of the line in millimeters? _______mm What is the length of the line to the nearest centimeter? ________cm HINT: Round to the nearest centimeter – no decimals. Measuring Length How many millimeters are in 1 centimeter? Ruler: http://www.k12math.com/math-concepts/measurement/ruler-cm.jpg

  8. 1 pound = 453.6 grams 1 ounce of gold = 28,349.5 milligrams 100 kilogram = 220 pounds English vs. Metric Units Which is larger? 1. 1 Pound or 100 Grams 2. 1 Kilogram or 1 Pound 3. 1 Ounce or 1000 Milligrams

  9. Kilogram Prototype A. 1 kilogram or 1500 grams B. 1200 milligrams or 1 gram C. 12 milligrams or 12 kilograms D. 4 kilograms or 4500 grams kg Metric Units cg mg g Mass refers to the amount of matter in an object. The base unit of mass in the metric system in the kilogram and is represented by kg. Standard: 1 kilogram is equal to the mass of the International Prototype Kilogram (IPK), a platinum-iridium cylinder kept by the BIPM at Sèvres, France. Metric Units 1 Kilogram (km) = 1000 Grams (g) 1 Gram (g) = 1000 Milligrams (mg) Click the image to watch a short video about mass. Which is larger? Kilogram Prototype Image - http://en.wikipedia.org/wiki/Kilogram

  10. Once you have balanced the scale, you add up the amounts on each beam to find the total mass. What would be the mass of the object measured in the picture? _______ + ______ + _______ = ________ g Measuring Mass We will be using triple-beam balances to find the mass of various objects. The objects are placed on the scale and then you move the weights on the beams until you get the lines on the right-side of the scale to match up. Top Image: http://www.southwestscales.com/Ohaus_Triple_Beam_750-SO.jpgBottom Image: http://www.regentsprep.org/Regents/biology/units/laboratory/graphics/triplebeambalance.jpg

  11. 1st – Place the film canister on the scale. 2nd – Slide the large weight to the right until the arm drops below the line. Move the rider back one groove. Make sure it “locks” into place. 3rd – Repeat this process with the top weight. When the arm moves below the line, back it up one groove. 4th – Slide the small weight on the front beam until the lines match up. Measuring Mass – Triple-Beam Balance 5th – Add the amounts on each beam to find the total mass to the nearest tenth of a gram. Click here to try an online activity.

  12. 1 fl oz = 29.573 ml 1 12-oz can of soda would equal approximately 355 ml. 1 quart = 0.946 liters 1 gallon = 3.79 liters It would take approximately 3 ¾ 1-liter bottles to equal a gallon. English vs. Metric Units Which is larger? A. 1 liter or 1 gallon B. 1 liter or 1 quart C. 1 milliliter or 1 fluid ounce

  13. kL Metric Units cL mL L Volume is the amount of space an object takes up. The base unit of volume in the metric system in the liter and is represented by L or l. Standard: 1 liter is equal to one cubic decimeter Metric Units 1 liter (L) = 1000 milliliters (mL) 1 milliliter (mL) = 1 cm3 (or cc) = 1 gram* Which is larger? Click the image to watch a short video about volume. A. 1 liter or 1500 milliliters B. 200 milliliters or 1.2 liters C. 12 cm3 or 1.2 milliliters* * When referring to waterLiter Image: http://www.dmturner.org/Teacher/Pictures/liter.gif

  14. What causes the meniscus? A concave meniscus occurs when the molecules of the liquid attract those of the container. The glass attracts the water on the sides. Measuring Volume We will be using graduated cylinders to find the volume of liquids and other objects. Read the measurement based on the bottom of the meniscus or curve. When using a real cylinder, make sure you are eye-level with the level of the water. What is the volume of water in the cylinder? _____mL Top Image: http://www.tea.state.tx.us/student.assessment/resources/online/2006/grade8/science/images/20graphicaa.gifBottom Image: http://morrisonlabs.com/meniscus.htm

  15. Measuring Liquid Volume What is the volume of water in each cylinder? Images created at http://www.standards.dfes.gov.uk/primaryframework/downloads/SWF/measuring_cylinder.swf A B C Pay attention to the scales for each cylinder.

  16. 9 cm 8 cm 10 cm We can measure the volume of irregular object using water displacement. Amount of H2O with object = ______About of H2O without object = ______Difference = Volume = ______ http://resources.edb.gov.hk/~s1sci/R_S1Science/sp/en/syllabus/unit14/new/testingmain1.htm Measuring Solid Volume We can measure the volume of regular object using the formula length x width x height. _____ X _____ X _____ = _____ Click here for an online activity about volume. Choose Lessons  Volume & Displacement

  17. DENSITY Density is defined as mass per unit volume. It is a measure of how tightly packed and how heavy the molecules are in an object. Density is the amount of matter within a certain volume.

  18. Proof that water and ice have different densities

  19. To find the density 1- Find the mass of the object 2- Find the volume of the object 3- Divide Density = Mass Volume

  20. Units for density g/cm3 or g/ml Formula: M = mass V= volume D = density M = D x V V = M / D D = M / V

  21. To find density: • Find the mass of the object • Find the volume of the object • Divide : Density = Mass - Volume Ex. If the mass of an object is 35 grams and it takes up 7 cm3 of space, calculate the density.

  22. To find density: • Find the mass of the object • Find the volume of the object • Divide : Density = Mass - Volume Ex. If the mass of an object is 35 grams and it takes up 7 cm3 of space, calculate the density. Set up your density problems like this: Given: Mass = 35 grams Volume = 7 cm3 Unknown: Density (g/ cm3) Formula: D = M / V Solution: D = 35g/7 cm3 D = 5 g/cm3

  23. Elements & Atoms

  24. An atom refresher • Matter is anything that takes up space and has mass. • All matter is made of atoms • Atoms are the building blocks of matter, sort of how bricks are the building blocks of houses.

  25. An atom refresher • An atom has three parts: • Proton = positive • Neutron = no charge • Electron = negative • The proton & neutron are found in the center of the atom, a place called the nucleus. • The electrons orbit the nucleus. Picture from http://education.jlab.org/qa/atom_model_03.gif

  26. What are elements? • Elements are the alphabet to the language of molecules. • To make molecules, you must have elements. • Elements are made of atoms. While the atoms may have different weights and organization, they are all built in the same way. Information & picture from Chem4kids at http://www.chem4kids.com/files/atom_structure.html

  27. Graphic from http://education.jlab.org/atomtour/fact2.html

  28. More about Elements.. • Elements are the building blocks of all matter. • The periodic table is a list of all of the elements that can build matter. It’s a little like the alphabet of chemistry. • The periodic table tells us several things…

  29. Periodic Table Atomic Number: Number of protons and it is also the number of electrons in an atom of an element. 8 O Element’s Symbol:An abbreviation for the element. Oxygen Elements Name Atomic Mass/Weight: Number of protons + neutrons. Almost always a decimal 15.99

  30. Atom Models • There are two models of the atoms we will be using in class. • Bohr Model • Lewis Dot Structure

  31. Bohr Model • The Bohr Model shows all of the particles in the atom. • In the center is circles. Each circle represents a single neutron or proton. Protons should have a plus or P written on them. Neutrons should be blank or have an N. • In a circle around the nucleus are the electrons. Electrons should have a minus sign or an e. - + + -

  32. Electrons have special rules…. • You can’t just shove all of the electrons into the first orbit of an electron. • Electrons live in something called shells or energy levels. • Only so many can be in any certain shell.

  33. Nucleus 1st shell 2nd shell 3rd shell Adapted from http://www.sciencespot.net/Media/atomsfam.pdf

  34. Electrons have special rules…. • You can’t just shove all of the electrons into the first orbit of an electron. • Electrons live in something called shells or energy levels. • Only so many can be in any certain shell. • The electrons in the outer most shell of any element are called valance electrons.

  35. So let’s try it…. • How to draw a Lithium atom • First, look at the Periodic Table • Second, determine the number of protons (Look @ the atomic number) • Then determine the number of neutrons (Atomic mass – atomic number) • Then determine the number of electrons (Look @ the atomic number) 3 Li Lithium 7

  36. So let’s try it…. Protons = 3 3 Li Lithium 7 - + + + - - Electrons = 3 2 in the 1st shell, 1 in the 2nd shell Neutrons = 4 (7-3=4)

  37. - - - - - - - - + + + + + + + + Lewis Dot Structure • The Lewis Dot Structure is a bit different from the Bohr model. • It only shows the element symbol and it’s outer most electron shell. • • O • • • •

  38. Periodic Table of Elements

  39. chlorine nitrogen silver gold mercury oxygen hydrogen helium sodium niobium neodymium carbon

  40. Elements • Science has come along way since Aristotle’s theory of Air, Water, Fire, and Earth. • Scientists have identified 90 naturally occurring elements, and created about 28 others.

  41. Elements • The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe.

  42. The most abundant element in the earth’s crust is oxygen.

  43. Periodic Table • The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table. • For example, you can predict with reasonably good accuracy the physical and chemical properties of the element. You can also predict what other elements a particular element will react with chemically. • Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 118 known elements.

  44. Valence Electrons • The number of valence electrons an atom has may also appear in a square. • Valence electrons are the electrons in the outer energy level of an atom. • These are the electrons that are transferred or shared when atoms bond together.

  45. Properties of Metals • Metals are good conductors of heat and electricity. • Metals are shiny. • Metals are ductile (can be stretched into thin wires). • Metals are malleable (can be pounded into thin sheets). • A chemical property of metal is its reaction with water which results in corrosion.

  46. Properties of Non-Metals • Non-metals are poor conductors of heat and electricity. • Non-metals are not ductile or malleable. • Solid non-metals are brittle and break easily. • They are dull. • Many non-metals are gases. Sulfur

  47. Properties of Metalloids • Metalloids (metal-like) have properties of both metals and non-metals. • They are solids that can be shiny or dull. • They conduct heat and electricity better than non-metals but not as well as metals. • They are ductile and malleable. Silicon

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