Printed on 10/26/2014

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Lesson 104:

ATOMS & MATTER A review of the properties of atoms and all forms of matter.

Fundamental Questions Attempting to give thorough and reasonable answers to the following questions will help you gauge your level of understanding this lesson. Students that can confidently answer these questions have mastered the concepts of this lesson.

1. How are atoms, elements, and matter all related to each other?

2. How is a molecule like a basketball team? 3. How is an atom like a church and a radio? 4. Make a list of things that are matter. 5. Make a list of things that are elements.

6. Make a list of things that are compounds. 7. What is the difference between matter and energy? 8. Why does matter change or does it? 9. How are you different from a rock? How are you the

same?

Lesson Objectives At the end of this lesson, students should have mastered the objectives listed below.

1. Students understand that atoms are the building blocks of all matter. 2. Students understand the relationship between matter and energy discovered by Einstein (E = mc2). 3. Students can use the periodic table to determine the number of protons, electrons, and neutrons that an atom of any

element has. 4. Students can easily identify the name of an element based on its chemical symbol and vice versa. 5. Students can draw and label the parts of an atom. 6. Students recognize that electrons are nearly weightless and move randomly at nearly the speed of light. 7. Students can calculate density and can describe how the density of a substance would change if the mass, volume,

or temperature of the substance were to change. 8. Students recognize that water is one of the few substances known to be a denser liquid than solid. 9. Students can name and describe the four states of matter. 10. Students understand that the temperature of an object usually dictates the state it is in. 11. Students understand that more heat means faster atomic vibrations, but that pressure can limit molecular movement. 12. Students are familiar with the six phase changes of matter. 13. Students understand density and how it is affected by phase changes. 14. Students can compare and contrast an atom and a molecule. 15. Students can describe the electrical charges of atomic particles and ions and how they interact with each other. 16. Students can explain how elements are different than compounds. 17. Students know that the density of pure liquid water is 1.0 g/mL and pure ice is 0.92 g/mL and can explain why ice is

less dense. 18. Honors students can determine the mass of each element in a 100 gram sample of water or another compound. 19. Students are familiar with the abundance of elements on Earth and throughout the universe.

Important Terms The following terms are some of the vocabulary that students should be familiar with in order to fully master this lesson.

1. E = mc2 2. matter 3. atoms 4. elements 5. the atomic model 6. nucleus 7. electrons 8. protons 9. neutrons 10. isotopes 11. carbon-14

12. periodic table 13. atomic number 14. atomic mass 15. mass number 16. chemical

properties 17. physical

properties 18. chemical

properties 19. solid

20. melting 21. sublimation 22. liquid 23. evaporation 24. freezing 25. gases 26. condensation 27. deposition 28. plasma 29. molecule 30. compound

31. covalent bond 32. ions 33. ionic bond 34. cations 35. anions 36. metallic bond 37. mixtures 38. solutions 39. energy level 40. crystal

Assessment Questions The following are examples of questions that students should be able to answer. These or similar questions are likely to appear on the exam.

1. What is an element? 2. What particles make up atoms?

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3. What are isotopes? 4. What are compounds and why do they form? 5. How do chemical bonds differ? 6. Compare and contrast solids, liquids, and gases. 7. The isotopes of carbon have from 2 to 16

neutrons. Use this information to make a table that shows the 15 isotopes of carbon and the atomic number and mass number of each.

8. What are the relative masses of the particles that make up an atom?

9. The elements magnesium and calcium have similar chemical properties. Explain why?

10. The atomic mass for the element carbon © is 12.011 amu. Explain how this number indicates that carbon is a mixture of isotopes. What is the mass number of the most common, naturally-occurring isotope of carbon?

11. Oxygen is often found in chemical combinations with other elements, such as magnesium. Using the concepts of valence electrons and energy levels, explain why oxygen might combine easily with magnesium.

12. The element copper (Cu) has 29 electrons. Draw a diagram of an atom of copper that shows the placement of its electrons in the correct energy levels and the number of protons it has.

13. Which two elements are most common on Earth? 14. Which two elements are most common in the

entire Universe? 15. Compare and contrast elements and compounds. 16. Why are negative ions usually larger than

positive ions? 17. Explain why molecules held together by covalent

bonds don't have electrical charges. 18. Compare and contrast mixtures and compounds. 19. What determines the shape of a crystal? 20. Draw a chart that shows the 3 main phases of

matter (ignoring plasma), the 6 phase changes ,

and the thermal energy required for each phase change.

21. How many electrons, protons, and neutrons does an atom of chlorine have?

22. What is the average atomic mass of uranium? 23. What is the chemical symbol for silicon? 24. Describe, in detail, how a Galilean thermometer

is able to accurately display what the temperature of the air is in our classroom. In other words, how does a Galilean thermometer work?

25. The chemical formula for water is H2O. A 100-millilter sample of water has a mass of approximately 100 grams. If you separate all of the hydrogen atoms from the oxygen atoms, what is the mass of the pile of hydrogen atoms? What is the mass of the pile of oxygen atoms? Show your work

26. You have discovered a substance in your kitchen that has a mass of 225.00 grams. Through experimentation, you have determined that the substance is a compound consisting of two elements, and the mass of a single molecule of the substance (molecular mass) is 58.44 amu. If you separate the two elements into two piles of atoms, you will find that one pile has a mass of 88.51 grams and the other pile has a mass of 136.49 grams. What are the two elements that the substance is made of? What is the substance? Write your answer on the back of this paper. Show all of your work on the back of this paper.

27. Explain what Einstein’s famous equation, E = mc2, means and why it is important to science?

28. Determine the density of a substance that has a mass of 42.8 grams and a volume of 2.0 milliliters.

29. Which element’s atom has 5 protons in its nucleus?

Related Web Sites The following are some web sites that are related to this lesson. You are encouraged to check out these sites to obtain additional information.

1. http://www.britannica.com/EBchecked/topic/41549/atom 2. http://www.nobelprize.org/educational/physics/matter/1.html 3. http://sciencespot.net/Pages/kdzchem.html 4. http://en.wikipedia.org/wiki/Atom 5. http://www.projectcrystal.org/m-cos-atomsandmatter.html 6. http://www.ndt-ed.org/EducationResources/HighSchool/Electricity/basicstructure.htm

Related Book Pages The following are the pages from your book that correspond to this lesson.

Comprehensive E.S. Book Intensive/Honors E.S. Book Meteorology/GIS Book pp. 34-43 pp. 52-75 N/A

Massachusetts Standards The following are the Massachusetts Framework Standards that correspond to this lesson.

Earth Science Learning Standard(s) 1.x

What’s Next?

V. What is Matter and what is it made of? A. Matter

1. Matter is anything that has mass and takes up space. 2. This paper, the sun, the air you breathe, the food you eat, and everyone you know are examples of matter. 3. All types of matter are essentially made of the same stuff: atoms.

B. Atoms 1. Atoms are the "building blocks" of matter. 2. The arrangement of atoms and the types of atoms that are connected together give matter its properties. 3. There are over a hundred different kinds of atoms. 4. An atom is the smallest particle of matter that has all the characteristics of an element and cannot be broken down into

smaller particles by ordinary chemical processes. C. Elements

1. Some forms of matter contain only one type of atom. These substances are called elements . 2. Because there are over 100 different types of atoms, there are also over 100 different types of elements (118 are known) 3. Examples of elements are gold, copper, oxygen, silicon, neon, hydrogen, and helium. Water, air, gasoline, and salt are

common examples of matter that are used everyday, but they are not elements because they are made of more than one kind of element.

D. The Atomic Model 1. Atoms are far too small to be seen with the naked eye. Even ordinary microscopes cannot allow us to see what an atom

looks like. Individual atoms have been seen using scanning electron microscopes, but the structure of an atom (what the atom is made of and how it is constructed) remains unseen. However, scientists have been able to construct a model of the atom by observing how an atom reacts to other atoms and to all forms of light.

2. The Nucleus a. Like a comet, an atom has a nucleus that is located at its center. b. The nucleus of the atom is usually composed of two kinds of particles: protons and neutrons. c. Protons are tiny particles that have a positive (+) electrical charge. d. Neutrons are particles that have no electrical charge, so they are considered neutral.

3. Electrons a. Electrons are negatively (-) charged particles that move around the nucleus of an atom at tremendous speeds

(nearly the speed of light). b. For elements, the number of electrons an atom has is exactly the same as the number of protons the atom has. c. The mass of an electron is 9.09 x 10-28 grams. d. Contrary to traditional teachings, electrons do not move around the nucleus in clearly defined orbits like planets

revolving around the sun. Instead, the movement of electrons is undeterminable. Part of the reason that the movements of electrons cannot be predicted is because electrons do not move in direct lines such as a bullet or a planet. Electron motion is similar to the motion of light - electrons move like a wave.

4. Isotopes a. If the number of protons in an atom is changed then a new and different element forms. However, changing the

number of neutrons in an atom will not change the element, although the mass of the atom will change. b. Atoms of the same element that have different numbers of neutrons in their nuclei are called isotopes . c. Isotopes, such as carbon-14, are often used to determine the ages of really old rocks, bones, artifacts, etc.

VI. The Periodic Table A. The periodic table is a tabular arrangement of all the known elements. It is organized based on increasing atomic number

and similarities in chemical properties. B. Atomic Number

1. The atomic number of an atom is equal to the number of protons in the nucleus of the atom. 2. Because elements are electrically neutral, the atomic number also equals the number of electrons an element has. 3. All atoms of the same element have the same atomic number. For example, the atomic number for carbon is 6 so all

carbon atoms will always have six protons. C. Atomic Mass

1. The atomic mass (or mass number ) of an atom is equal to the number of protons and neutrons an atom has. The more particles an atom has, the more atomic mass it has. Electrons are not counted when determining the mass number of an atom because the mass of electrons is much, much smaller than protons and neutrons.

2. If you look at the periodic table, you will see that carbon ordinarily has a mass number of about 12.011. This number can be rounded to the nearest whole number, so the mass number for an ordinary carbon atom is 12. The mass number tells us that there are 12 particles in the nucleus of a carbon atom. But how many protons and how many neutrons are there? To determine how many protons there are, all we have to do is look at what the atomic number is. The atomic number for carbon is always 6, so there are always 6 protons in a carbon atom. To figure out how many neutrons there are in a carbon atom having a mass number of 12, all we have to do is subtract the atomic number from the mass number. Therefore, there are also 6 neutrons in an ordinary carbon atom.

VII. Properties of Matter A. The way two different elements combine to make something new is result of chemical properties of the elements.

Elements/compounds are often identified by their chemical properties. B. Properties of element/compound that can be observed without changing substance into new substance are physical properties . C. Density

1. Density is physical property of matter that can be used to describe or identify a substance. 2. Density - the mass of a substance per unit of volume. In other words, density is the measure of how much stuff (matter) is

inside a specific amount of space. 3. Mathematical definition for density is D = m/V, where D is density of substance, m is its mass, and V is its volume. 4. In general, the density of substance is less when in gaseous state, and most dense when in solid form. Water (H2O) is an

exception. 5. When an object that is not very dense is placed into substance that’s more dense than the object, object will float. When

object that is very dense is placed into substance that is less dense than object, object will sink. VIII. States and State Changes of Matter

A. Solids 1. have definite shape and volume. 2. In solid state, individual atoms of a substance vibrate, but they cannot switch positions relative to each other. 3. Atoms in a solid have the strongest attraction to one another. 4. To change from solid to liquid (melting ) energy must be added to substance. To change from solid to gas (sublimation ) even

more energy must be added to substance. B. Liquids

1. In liquid state, individual atoms of a substance vibrate more than in solid state, and can switch positions with each other which allows the liquid to flow.

2. Liquids do not have a definite shape (they take the shape of their container), but do have definite volume. 3. To change from liquid to gas (evaporation ) energy must be added to substance. To change from liquid to solid (freezing )

energy must be taken away from the substance. 4. Gases

1. In gaseous state, individual atoms of substance vibrate freely and have little attraction for one another. 2. Gases do not have a definite shape or volume – they fill their container completely.

Do gases have a definite density then? 3. To change from gas to liquid (condensation ) energy must be taken away from the substance. To change from gas to solid

(deposition ) even more energy must be taken away from the substance. 5. Plasma

1. Most matter is in plasma state. 2. composed of ions and electrons 3. Most common example of substance made of plasma: stars 4. Plasma substance on Earth: lightning bolts

IX. Combinations of Atoms A. Molecules and Compounds

1. Molecules a. Atoms of the same element and of different elements can combine together to form a molecule. b. A molecule is the smallest particle of matter that is made up of two or more atoms that have combined.

2. Compounds a. A compound is a type of matter that is made up of two or more kinds of elements. b. Compounds have properties that are different from the properties of each of the elements in it. c. Compounds are always made from molecules.

3. Examples of some of the most abundant compounds on Earth: water and quartz a. Water is composed of the elements hydrogen (H) and oxygen (O) which are normally gases on the Earth, but they form a

liquid when they combine chemically. A molecule of water consists of two hydrogen atoms bonded to one oxygen atom. b. Quartz is one of the most common minerals (“rocks”) found on Earth. It is composed of silicon (Si) and oxygen (O) atoms,

the two most abundant elements on earth. A molecule of quartz consists of two oxygen atoms bonded to one silicon atom. B. Covalent Bonds and Ions

1. Atoms can combine in a few different ways. One of the ways involves elements forming a molecule by sharing one or more electrons. When this type of combination occurs, the atoms are said to have formed a covalent bond .

2. Other molecules are formed by atoms that have become positively or negatively charged and are then attracted to atoms that have the opposite electrical charge. Electrically charged atoms are called ions . a. Normally, atoms of elements are neutral, meaning that they have no electrical charge. This is because the negative

charges of the electrons are normally balanced by the positive charges of the protons. However, sometimes atoms lose or gain electrons, giving the atom an electric charge.

b. When an atom gains one or more electron, the electrical charge of the atom is negative. Atoms with negative electrical charges are called anions .

c. When an atom loses one or more electrons, the electrical charge of the atom is positive. Atoms with positive electrical charges are called cations .

C. Mixtures and Solutions 1. Mixtures are combinations of different substances in which each of the components in the mixture keeps their own physical and

chemical properties despite being mixed. An example of a mixture would be the books, pens, notebooks, etc. in your book bag. Each of the items in your bag can be easily removed from the mixture and the properties of the item due not change.

2. Solutions are a type of mixture that involves the dissolving of one substance into another. a. Seawater is an excellent example of a solution. Seawater is ordinary water with several different types of salts dissolved

into it. The salts that dissolve into the water seem to disappear because a water molecule separates each atom of the salt from each other. This gives the solution the same appearance of ordinary water, but the salt atoms are still present so the water is not pure.

b. Solutions are the same throughout. In other words, the substance that is dissolved in the solution is evenly distributed throughout the mixture.

AmorphousAnionAtomsCationCompoundsCrystalElectronsElementsEnergyGasIonsIsotopesLiquidMatterMixturesMoleculesNeutronsNucleusPlasmaProtonsSolidSolutionsStates of MatterTypes of Matter

Energy

Matter

Neutrons

Protons

1. An atom is like a feather because: 2. An atom is like a church because: 3. An atom is like the solar system because: 4. An atom is like an earthquake because: 5. An atom is like ice cream because: 6. An atom is like Lord of the Rings, the Matrix, The

Grudge, and Pirates of the Caribbean because: 7. An atom is like a radio because: 8. An atom is like the letters E, E, G, H, I, N, R, T, V, and Y

because: 9. An atom is like a dollar in Bill Gates’ savings account

because: 10. An atom is like George Bush’s brain because:

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OPTICAL ILLUSION PROJECT 40 Points

Due Date _____________

For this project, you will research optical illusions and create a digital poster of an illusion. Your poster will present the illusion along with an explanation for why the illusion is able to trick the human mind into thinking that it is real. Your project poster must meet the following requirements:

1. You will construct the poster digitally using computer software such as Photoshop, GIMP, CorelDraw, PowerPoint, LibreOffice Draw, etc. 2. The final product must be either a PDF or JPEG graphics file that can be opened on any computer. 3. The name of your file should be First Name Last Name Illusion Project. For example, if your name is John Smiffy, then the file name

should be John Smiffy Illusion Project. 4. By the specified due date, you will either email your project to jroberts@stonehamschools.org or save the project to the Student Drop

drive. 5. The dimensions of your poster should be exactly 13” x 19”. The orientation of your poster can be either landscape or portrait. 6. Your poster should be only 1-page long. That means you will need to fit all information onto one 13” x 19” page. 7. The poster must be easily readable from 3 feet away. 8. Your name should be subtly displayed in a corner of your poster. 9. Your poster should have an obvious title. 10. The poster should display the illusion. 11. The illusion is unique or at least uncommon. Try to pick something that other students won’t use. 12. The illusion should work. 13. The illusion should not be a video or animation. It must be an illusion that works when the poster is printed out onto paper. 14. The poster should include clear and concise directions on how to see the illusion. 15. The poster should include a basic scientific explanation for why the illusion works. In other words, how is the illusion able to trick our

eyes and brains? 16. You may add any other information you choose, but any additional information added to your poster should be relevant to your illusion.

DO NOT ADD ADDITIONAL ILLUSIONS UNLESS THEY ARE DIRECTLY RELATED TO YOUR MAIN ILLUSION! 17. Your poster should look like a professional made it. Creating a professional-looking poster will take time, vision, technique, and talent.

Study several professional posters to see what they did to improve the poster’s appearance and try to copy their techniques. Your grade will be based on how well your illusion works, how professional your poster appears, the accuracy of your directions and explanation, and how unique your illusion is. The following is the rubric that will be used to grade your project:

PROJECT REQUIREMENT MET? NO YES 1. The poster is turned in on time. -20%/day -0% 2. The poster is constructed digitally. -60% -0% 3. The final digital file is either a PDF or JPEG file. -20% -0% 4. The file name has your name in it and is written as instructed. -5% -0% 5. The file is either emailed to Mr. Roberts or saved to the Student Drop. -25% -0% 6. The dimensions of your poster are exactly 13” x 19”. -15% -0% 7. The poster is a single page. -35% -0% 8. The poster is easily readable on a 20” computer screen from 3 feet away. -10% -0% 9. Your name is subtly displayed in a corner of the poster. -5% -0% 10. The poster has an appropriate title. -5% -0% 11. The title is obvious and easy to find. -5% -0% 12. The poster displays your illusion. -100% -0% 13. The illusion is unique or at least uncommon. -5% -0% 14. The illusion works for most people viewing your poster. -20% -0% 15. The poster does not contain any video or animation. -30% -0% 16. The poster displays clear and concise directions on how to see the illusion. -15% -0% 17. The poster displays a basic scientific explanation for why the illusion works. -25% -0% 18. The directions and/or scientific explanation are not plagiarized. -50% -0% 19. The scientific explanation is easy to understand. -5% -0% 20. Any additional information on your poster is relevant and directly related to your illusion. -5% -0% 21. The poster has a neat line or border around the entire poster. -4% -0% 22. Font, line, polygon, background, and image colors work well together so that the poster is easy to read and interesting to

look at without creating a “sensory overload”. -4% -0% 23. The illusion image and all other images are high-resolution images, free from pixilation. -4% -0% 24. The poster is free from “dead spots” where there is too much empty space. -4% -0% 25. The poster is not overloaded with information and/or graphics. -4% -0% 26. The fonts on the poster are consistent, infrequently changing style and/or size. -4% -0% 27. The poster is eye-catching, but not in a way that creates sensory overload. -4% -0% 28. The arrangement of the poster is intuitive and easy to follow. -4% -0% 29. The poster looks like a professional graphic artist could have made it. -4% -0%