Atomic Bonding, Balancing Chemical Equations, Endothermic and Exothermic Reactions Lesson PowerPoint

3. -Nice neat notes that are legible and use indents when appropriate. -Example of indent. -Skip a line between topics - -Make visuals clear and well drawn. Label please. Neutron Proton Electron

4. • RED SLIDE: These are notes that are very important and should be recorded in your science journal. • BLACK SLIDE: Pay attention, follow directions, complete projects as described and answer required questions neatly. Copyright © 2010 Ryan P. Murphy

8. • More Units Available at… Earth Science: The Soil Science and Glaciers Unit, The Geology Topics Unit, The Astronomy Topics Unit, The Weather and Climate Unit, and The River and Water Quality Unit, and The Water Molecule Unit. Physical Science: The Laws of Motion and Machines Unit, The Atoms and Periodic Table Unit, Matter, Energy, and the Environment Unit, and The Science Skills Unit. Life Science: The Infectious Diseases Unit, Cellular Biology Unit, The DNA and Genetics Unit, The Botany Unit, The Taxonomy and Classification Unit, Ecology: Feeding Levels Unit, Ecology: Interactions Unit, Ecology: Abiotic Factors, The Evolution and Natural Selection Unit and The Human Body Systems and Health Topics Unit. Copyright © 2010 Ryan P. Murphy

13. This is really difficult learning ahead and I’m going to try my best to learn it. I’m not going to give up.

15. This is really difficult learning ahead and I’m going to try my best to learn it. I’m not going to give up. This is really difficult and I’m going to quit as soon as I don’t know it. I’m going to check out completely or create issues for those choosing A.

44. “Ionic Please.” “Transferred.” “Not shared.”

55. Learn more: http://web.jjay.cuny.edu/~ acarpi/NSC/5-bonds.htm

69. Video: Ionic and Covalent Bonds http://www.youtube.com/watch?v=Kj3o0Xv hVqQ&feature=results_main&playnext=1& list=PL85B1E4851BDEE325

75. • Activity! Generating heat by breaking metallic bonds. – Bend spoon back and forth to generate very hot temperatures, WATCH OUT! – Do not try this in the lunchroom! Copyright © 2010 Ryan P. Murphy

76. • Video! Ionic and Covalent Bonding. • http://www.youtube.com/watch?v=QqjcCv zWwww

77. • Video Link! (Optional) Khan Academy, Atomic Bonding. – http://www.khanacademy.org/video/ionic-- covalent--and-metallic-bonds?playlist=Chemistry

82.  Ion: A charged atom.  When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy “Hoot” “Hoot” “Did anybody see me on that charged atom.”

83.  Ion: A charged atom.  When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy “Hoot” “Hoot” “Did anybody see me on that charged atom.”

84. “Ahh, I just lost an electron?”

85. “Ahh, I just lost an electron?” “Are you positive?”

86. “Ahh, I just lost an electron?” “Are you positive?” “I can’t take this anymore”

87. The closer and more tightly bound an electron is to the nucleus, the more difficult it will be to remove, and the higher its ionization energy will be.

88. Protons stink! I hate being in this shell. This is the worst. Nightmare

89. Protons stink! I hate being in this shell. This is the worst. Nightmare

90. Protons stink! I hate being in this shell. This is the worst. Nightmare This is so nice I’m so happy.

91. Protons stink! I hate being in this shell. This is the worst. Nightmare This is so nice I’m so happy.

93. The atom has a neutral charge when the number is the same.

94. The atom has a neutral charge when the number is the same. When you remove an electron

95. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive

96. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive Yay, we lost Grumpy. I feel so more positive.

97. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) Yay, we lost Grumpy. I feel so more positive.

98. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +)

99. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) When you add an electron the atom becomes more negative.

100. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) When you add an electron the atom becomes more negative. Anion -

101. The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) When you add an electron the atom becomes more negative. Anion - More negativity

103. • Which atom below is the anion, and which is the cation?

104. • Sodium formed a cation because it lost 1 electron and became positive.

105. • Chlorine formed an anion because it gained -1 electron. More negative.

106. • Which atom below formed a cation, and which formed an anion?

121. Copyright © 2010 Ryan P. Murphy Who wants it? It is ionic because it's a bond between a metal(potassium) and a non-metal(chlorine). Potassium has one electron in its valence shell, and chlorine has seven electrons in its valence shell. Following the octet rule, the potassium gives an electron to the chlorine. Then the negatively charged chlorine ion and the positively charged potassium ion stick together because of their opposite charges. Ionic bonds give electrons, covalent bonds share electrons Do we want to know the difficult explanation beneath this box or skip it? Why?

122. Copyright © 2010 Ryan P. Murphy Who wants it? It is ionic because it's a bond between a metal(potassium) and a non-metal(chlorine). Potassium has one electron in its valence shell, and chlorine has seven electrons in its valence shell. Following the octet rule, the potassium gives an electron to the chlorine. Then the negatively charged chlorine ion and the positively charged potassium ion stick together because of their opposite charges. Ionic bonds give electrons, covalent bonds share electrons Do we want to know the difficult explanation beneath this box or skip it? Why?

123. Copyright © 2010 Ryan P. Murphy Who wants it? It is ionic because it's a bond between a metal(potassium) and a non-metal(chlorine). Potassium has one electron in its valence shell, and chlorine has seven electrons in its valence shell. Following the octet rule, the potassium gives an electron to the chlorine. Then the negatively charged chlorine ion and the positively charged potassium ion stick together because of their opposite charges. Ionic bonds give electrons, covalent bonds share electrons

127. • Answer: This Chlorine atom will want to gain one electron rather than lose seven. – It has a high electron affinity. Copyright © 2010 Ryan P. Murphy Learn more: Ionization. http://www.wisegeek.com/what- is-ionization.htm

138. • Precipitation Reactions: Occur when cations and anions of aqueous solutions combine to form an insoluble ionic solid, called a precipitate. Copyright © 2010 Ryan P. Murphy See Video (2 minutes) http://www.youtube.com/watch?v=8RmVwz2fNGc First - AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) Second- AgNO3(aq) + NaI(aq) → AgI(s) + NaNO3(aq)

139. • Video Link! Precipitation Reactions Crash Course. – Advanced and Optional – http://www.youtube.com/watch?v=IIu16dy3ThI&li st=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr

140. • Acids and Bases optional PowerPoint in folder. – Nice reading can be found here. – http://www.visionlearning.com/library/module_ viewer.php?mid=58

141. • Acid: a substance which when added to water produces hydrogen ions [H+]. – React with zinc, magnesium, or aluminum and form hydrogen (H2(g)) – React with compounds containing CO3 2- and form carbon dioxide and water – Turn litmus red – Taste sour (lemons contain citric acid, for example) – Tasting Acids in the lab would be unsafe.

142. • Acid: a substance which when added to water produces hydrogen ions [H+]. – React with zinc, magnesium, or aluminum and form hydrogen (H2(g)). – React with compounds containing CO3 2- and form carbon dioxide and water. – Turns litmus red. – Taste sour (lemons contain citric acid, for example). – Tasting Acids in the lab would be unsafe.

143. • Base: a substance which when added to water produces hydroxide ions [OH-]. – Feel soapy or slippery – Turn litmus blue – They react with most cations to precipitate hydroxides – Taste bitter like soap. – Do not taste in the lab.

144. • Base: a substance which when added to water produces hydroxide ions [OH-]. – Feel soapy or slippery. – Turns litmus blue. – They react with most cations to precipitate hydroxides. – Taste bitter like soap. – Do not taste in the lab.

145. • Which is an Acid and which is a Base? OH- OH- OH- OH- OH- Lots of OH-, High pH

149. • Which is an Acid and which is a Base?

150. • Which is not true of a base? A.) Feel soapy or slippery. B.) Turns litmus red. C.) They react with most cations to precipitate hydroxides. D.) Taste bitter like soap. – Do not taste in the lab.

154. • Which is not true of a base? A.) Feel soapy or slippery. B.) Turns litmus blue. C.) They react with most cations to precipitate hydroxides. D.) Taste bitter like soap. – Do not taste in the lab.

156. • Which is not true of acids? A.) Acid: a substance which when added to water produces hydrogen ions [H+]. B.) React with zinc, magnesium, or aluminum and form hydrogen (H2(g)). C.) They react with most cations to precipitate hydroxides D.) Turn litmus red. E.) Taste sour (lemons contain citric acid, for example). • Tasting Acids in the lab would be unsafe.

160. • Which is not true of acids? A.) Acid: a substance which when added to water produces hydrogen ions [H+]. B.) React with zinc, magnesium, or aluminum and form hydrogen (H2(g)). C.) React with compounds containing CO3 2- and form carbon dioxide and water D.) Turn litmus red. E.) Taste sour (lemons contain citric acid, for example). • Tasting Acids in the lab would be unsafe.

171. • The most strongly electronegative element, Fluorine (F). • The least electronegative element is Francium (Fr). Copyright © 2010 Ryan P. Murphy “I want to give away electrons.” “I want to gain electrons”

173. • Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. – The higher the electronegativity of an atom, the greater its attraction for bonding electrons. Copyright © 2010 Ryan P. Murphy

174. • Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. – The higher the electronegativity of an atom, the greater its attraction for bonding electrons. Copyright © 2010 Ryan P. Murphy “Those elements attract electrons like wicked.”

175. • Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. – The higher the electronegativity of an atom, the greater its attraction for bonding electrons. Copyright © 2010 Ryan P. Murphy “Not the Noble Gases however.” “They’re wicked different.”

176. – Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. – Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. Copyright © 2010 Ryan P. Murphy and Ions)Ionization energy is the energy required to remove an electron. (Gases and Ions)

181. • A polar bond: Results in the unequal sharing of the electrons in the bond. – When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity Copyright © 2010 Ryan P. Murphy

182. • A polar bond: Results in the unequal sharing of the electrons in the bond. – When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity Copyright © 2010 Ryan P. Murphy The presence or absence of polar bonds within a molecule plays a very important part in determining chemical and physical properties of those molecules. Some of these properties are melting points, boiling points, viscosity and solubility in solvents.

189. • Hydrogen Bond: A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom.

190. • Hydrogen Bond: A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom.

191. • Hydrogen Bond: A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom. – Especially a nitrogen, oxygen, or flourine atom of another molecule.

192. • Hydrogen Bond: A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom. – Especially a nitrogen, oxygen, or flourine atom of another molecule.

202. • The three classes of bonds

203. • The three classes of bonds – Nonpolar Covalent

204. • The three classes of bonds – Nonpolar Covalent – Polar Covalent

205. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic

206. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element.

207. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar.

208. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference

209. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44

210. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 =

211. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24

214. Try Ethane C2H6?

215. Try Ethane C2H6?

216. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff.

217. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55

218. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 =

219. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35

220. • The three classes of bonds – Nonpolar Covalent – Polar Covalent – Ionic • The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. – Differences 1.7 or greater, the bond is usually ionic, – Differences Less than 1.7, the bond is usually covalent, » Unless the difference is less than 0.5 the bond has some degree of polarity – Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35

226. • Which one is polar covalent and which one nonpolar?

233. • Layering liquids with different densities. • Use a clear container and add the following in this order…. – Corn Syrup – Water (food Coloring) – Vegetable Oil

240. • I would recommend completing these questions right away.

242. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44

243. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Do we want to see the answers?

244. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Do we want to see the answers?

245. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers?

246. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

250. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

254. Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

257. • Video! Ionic and Covalent Bonding. • http://www.youtube.com/watch?v=QqjcCv zWwww

258. • Video Link! Ionic and Covalent Bonds – https://www.youtube.com/watch?v=7DjsD7Hcd9U

259. • (Optional Link): Khan Academy • Ionization Energy (12 min) Advanced • http://www.khanacademy.org/video/periodi c-table-trends--ionization- energy?playlist=Chemistry

260. • Video Link! Speaking Chemistry Crash Course. – Optional and Advanced. – http://www.youtube.com/watch?v=mlRhLicNo8Q&l ist=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr

261. • Remember: • Covalent – Sharing an Electron many of the SPONCH elements.

262. • Remember: • Covalent – Sharing an Electron many of the SPONCH elements. • Ionic – Opposite charges + / -

263. • Remember: • Covalent – Sharing an Electron many of the SPONCH elements. • Ionic – Opposite charges + / - • Metallic – Many electrons

283. • Bonus: Name the actor and movie character.

305. • Bonus: Name the actor and movie character.

306. • Bonus: Name the actor and movie character. Sean Connery

307. • Optional worksheets / quizzes associated with atomic bonding (Links) – http://moodle.northsideprep.org/pluginfile.php/ 8956/mod_resource/content/0/Electronegativit y-ws1-nh4.pdf – Atomic Bonding Electronegativity Differences – Atomic Bonding and Electronegativity Sheet

308. • Optional PowerPoint “Properties of Water” – Found in activities folder. – More about polar and nonpolar.

309. • Video Link! Carbon Crash Course and Nice Review of Unit. (Optional) – Preview for language and content. – http://www.youtube.com/watch?v=QnQe0xW_J Y4&list=EC3EED4C1D684D3ADF

311. • Check out this awesome chemical reaction

313. • Demonstrations of chemical change.

315. • Demonstration – Fill bottle with screw top with vinegar. – Fill balloon with baking soda using funnel. – Attach bottom of balloon to top of bottle making sure that no baking soda enters bottle. – Turn balloon upright so contents fall into bottle and observe. Copyright © 2010 Ryan P. Murphy

316. • The baking soda (NaHCO3) mixes with the vinegar (HC2H3O2) –HC2H3O2 + NaHCO3 ===> NaC2H3O2 + H2CO3 –The H2CO3 quickly breaks down • H2CO3 ===> H2O + CO2 • Carbon dioxide can be used to put out fire. Copyright © 2010 Ryan P. Murphy

322. • Activity Demonstration – Electrolysis. – What is happening in the beaker? Can you guess the chemical change? Copyright © 2010 Ryan P. Murphy Please set-up the following. Dissolve about a spoonful of salt into warm water.

323. • Activity Demonstration – Electrolysis. – What is happening in the beaker? Can you guess the chemical change? Copyright © 2010 Ryan P. Murphy Please set-up the following. Dissolve about a spoonful of salt into warm water. Connect one end on the positive side of the battery and the other to the tip of the pencil.

324. • Activity Demonstration – Electrolysis. – What is happening in the beaker? Can you guess the chemical change? Copyright © 2010 Ryan P. Murphy Please set-up the following. Dissolve about a spoonful of salt into warm water. Connect one end on the positive side of the battery and the other to the tip of the pencil. Do the same for the negative side connecting it to the second pencil top. Place the other two ends of the pencil into the salt water.

325. • Activity Demonstration – Electrolysis. – What is happening in the beaker? Can you guess the chemical change? Copyright © 2010 Ryan P. Murphy Please set-up the following. Dissolve about a spoonful of salt into warm water. Connect one end on the positive side of the battery and the other to the tip of the pencil. Do the same for the negative side connecting it to the second pencil top. Place the other two ends of the pencil into the salt water. Observe Bubbles that form at the bottom of the pencil in the water.

326. • Activity Demonstration – Electrolysis. – What is happening in the beaker? Can you guess the chemical change? Copyright © 2010 Ryan P. Murphy Please set-up the following. Dissolve about a spoonful of salt into warm water. Connect one end on the positive side of the battery and the other to the tip of the pencil. Do the same for the negative side connecting it to the second pencil top. Place the other two ends of the pencil into the salt water. Observe Bubbles that form at the bottom of the pencil in the water. This is hydrogen gas.

327. • Electrolysis of water is the decomposition of water (H2O) into oxygen (O2) and hydrogen (H).

328. • Water and hydrogen could be the answer to finding a clean renewable source of energy.

343. • Balancing Chemical Equations.

344. • Balancing Chemical Equations. – This is what happens in a chemical reaction

345. • Balancing Chemical Equations. – This is what happens in a chemical reaction

346. • Balancing Chemical Equations. – This is what happens in a chemical reaction – It describes what you started with…and ended with.

351. • Balancing Chemical Equations. – This is what happens in a chemical reaction – It describes what you started with…and ended with. – It also describes the phases of each (s) (l) (g)

352. • Balancing Chemical Equations. – This is what happens in a chemical reaction – It describes what you started with…and ended with. – It also describes the phases of each (s) (l) (g) – It also describes the amount of each.

356. • Balancing a chemical equation refers to establishing the mathematical relationship between the quantity of reactants and products.

357. • Balancing a chemical equation refers to establishing the mathematical relationship between the quantity of reactants and products. – Reactant: Starting

360. • Balancing a chemical equation refers to establishing the mathematical relationship between the quantity of reactants and products. – Reactant: Starting – Products: Ending

372. Big Bang All Matter

373. Big Bang All Matter Particles join together

374. Big Bang All Matter Particles join together Gravity attracts particles, forms stars, planets Galaxies

375. Big Bang All Matter Particles join together Gravity attracts particles, forms stars, planets Galaxies Sun releases particles, photons through nuclear processes

376. Big Bang All Matter Particles join together Gravity attracts particles, forms stars, planets Galaxies Sun releases particles, photons through nuclear processes Plants harness Photons to make sugars with available molecules on Earth from formation

377. Big Bang All Matter Particles join together Gravity attracts particles, forms stars, planets Galaxies Sun releases particles, photons through nuclear processes Plants harness Photons to make sugars with available molecules on Earth from formation

378. Big Bang All Matter Particles join together Gravity attracts particles, forms stars, planets Galaxies Sun releases particles, photons through nuclear processes Plants harness Photons to make sugars with available molecules on Earth from formation Matter from the formation of the planets, sometime after the big bang.

382. • Remember the Law Conservation of Mass: Matter cannot be created or destroyed. That means we need to have the same amount of chemicals on each side of the . • For this reason, put a square around the chemical formulas. • Example

384. • Remember the Law Conservation of Mass: Matter cannot be created or destroyed. That means we need to have the same amount of chemicals on each side of the . • For this reason, put a square around the chemical formulas.

386. • Begin balancing chemical equations by putting numbers (coefficients) in front of them.

387. • Begin balancing chemical equations by putting numbers (coefficients) in front of them. – Example H2O on one side could become 2 H2O

388. • Begin balancing chemical equations by putting numbers (coefficients) in front of them. – Example H2O on one side could become 2 H2O – Remember that each side needs to have same number of Hydrogen and Oxygen

389. • Begin balancing chemical equations by putting numbers (coefficients) in front of them. – Example H2O on one side could become 2 H2O – Remember that each side needs to have same number of Hydrogen and Oxygen • Note – Don’t change the subscript • Example H2O becomes H3O

390. • Begin balancing chemical equations by putting numbers (coefficients) in front of them. – Example H2O on one side could become 2 H2O – Remember that each side needs to have same number of Hydrogen and Oxygen • Note – Don’t change the subscript • Example H2O becomes H3O

391. • Balancing Equations Available Sheet. – Complete each equation as we cover it in class.

393. • A way to start off the process is to create an inventory of your chemicals.

394. • A way to start off the process is to create an inventory of your chemicals. BOXES!!!

428. • Now look at the inventory and begin the process of balancing the equation.

430. One Sodium

431. One Sodium Two Sodium

432. One Sodium Two Sodium Let’s add a 2 here and see if it balances. 2

433. Did it balance? Are we done? 2

434. Did it balance? Are we done? We should do a new inventory chart. 2

435. 2

436. 2

437. 2

438. 2 2

439. 2 2

440. 2 2

441. 2 2 2

442. 2 2 2

443. 2 2 2

444. 2 2 2 6

445. 2 2 2 6

446. 2 2 2 6

447. 2 2 2 6 5

448. 2 2 2 6 5

449. One Sodium Two Sodium Let’s try again and add a 2 to the other side. 2 2

450. Does it balance this time?

463. This is a balanced equation.

464. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O

465. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O

468. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… BOXES! __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O

470. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1

471. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1

472. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1 4 2

473. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1 4 2

474. • It should work most of the time although it can be very tricky. Always keep an inventory chart or it will get all messed up. Try to balance… __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1 4 2 2 3

475. __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1 4 2 2 3

476. __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O 1 1 4 2 2 3 What should we put to equal 4?

477. • See if this is right? __CH4 + __O2 --> __CO2 + __H2O__CH4 + __O2 --> __CO2 + __H2O C H O

478. • Answer: Incorrect – The inventory does not match. __CH4 + __O2 --> __CO2 + __H2O1 CH4 + 2 O2 --> 2 CO2 + 2 H2O C H O 1 2 4 4 4 5

479. • Answer: See if this is right? __CH4 + __O2 --> __CO2 + __H2O1 CH4 + 2 O2 --> 1 CO2 + 2 H2O C H O

480. • Answer: See if this is right? __CH4 + __O2 --> __CO2 + __H2O1 CH4 + 2 O2 --> 1 CO2 + 2 H2O C H O

481. • Answer: See if this is right? • Answer: Yes, A balanced equation __CH4 + __O2 --> __CO2 + __H2O1 CH4 + 2 O2 --> 1 CO2 + 2 H2O C H O 1 1 4 4 4 4

482. • What’s this famous equation? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2

483. • What’s this famous equation? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2

484. • What’s this famous equation? • Can you balance it? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2 ___CO2 + ___H2O = __C6H12O6 + __O2 Element Before After

485. • What’s this famous equation? • Can you balance it? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2 ___CO2 + ___H2O = __C6H12O6 + __O2 Element Before After 1 6 2 122 3 8

486. • What’s this famous equation? • Does this balance? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2 ___CO2 + ___H2O = __C6H12O6 + __O2 Element Before After

487. • What’s this famous equation? • Does this balance? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2 ___CO2 + ___H2O = __C6H12O6 + __O2 Element Before After 6 6 12 12 18 18

488. • What’s this famous equation? • Does this balance? ___CO2 + ___H2O + light energy = __C6H12O6 + __O2 ___CO2 + ___H2O = __C6H12O6 + __O2 Element Before After 6 6 12 12 18 18

489. • Which of the following equations is the correct equation for photosynthesis? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • C) 6CO2 + 6CO2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 6H2 + light energy = C6H12O6 + 6H2O • E) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • F) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • G) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • H) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • I) 6CO2 + H2O + light energy = C6H12O6 + 6O2 • J) C6H12O6 = 6CO2 + 6H2O + light energy + 6O2 Copyright © 2010 Ryan P. Murphy

490. • Which of the following equations is the correct equation for photosynthesis? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • C) 6CO2 + 6CO2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 6H2 + light energy = C6H12O6 + 6H2O • E) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • F) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • G) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • H) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • I) 6CO2 + H2O + light energy = C6H12O6 + 6O2 • J) C6H12O6 = 6CO2 + 6H2O + light energy + 6O2 Copyright © 2010 Ryan P. Murphy

491. • Find the Photosynthesis equation. • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • F) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • G) 6CO2 + 6H2 + light energy = C6H12O6 + 6O2 • H) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) CO2 + 6H2O2 + light energy = CH12O6 + 6O2 • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • O) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • P) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • Q) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • R) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • S) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • T) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 • U) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • V) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • W) CO2 + 6H2O2 + light energy = CH12O6 + 6O2 • X) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • Y) 6CO2 + 6H2 + light energy = C6H12O6 + 6O2 • Z) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 Copyright © 2010 Ryan P. Murphy

492. • Find the Photosynthesis equation. • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • F) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • G) 6CO2 + 6H2 + light energy = C6H12O6 + 6O2 • H) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) CO2 + 6H2O2 + light energy = CH12O6 + 6O2 • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N) 6CO2 + 6H2O + sugar = C6H12O6 + 6O2 • O) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • P) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • Q) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • R) 6CO2 + 6H2O + light energy = C6H2O6 + 6O2 • S) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • T) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 • U) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • V) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • W) CO2 + 6H2O2 + light energy = CH12O6 + 6O2 • X) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • Y) 6CO2 + 6H2 + light energy = C6H12O6 + 6O2 • Z) 6CO2 + 6H2O + light energy = C6H12O6 + 6O6 Copyright © 2010 Ryan P. Murphy

493. • What’s this famous equation? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O.

494. • What’s this famous equation? • Can you balance it? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O.

495. • What’s this famous equation? • Can you balance it? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O.

496. • What’s this famous equation? • Can you balance it? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. ___+C6H12O6 + __O2 = Released energy + __CO2 + __H2O Element Before After

497. • What’s this famous equation? • Can you balance it? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. ___+C6H12O6 + __O2 = Released energy + __CO2 + __H2O Element Before After 6 1 12 2 8 3

498. • What’s this famous equation? • Will this balance? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. ___+C6H12O6 + __O2 = Released energy + __CO2 + __H2O Element Before After

499. • What’s this famous equation? • Will this balance? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. ___+C6H12O6 + __O2 = Released energy + __CO2 + __H2O Element Before After 6 6 12 12 18 18

500. • What’s this famous equation? • Will this balance? ___C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. ___+C6H12O6 + __O2 = Released energy + __CO2 + __H2O Element Before After 6 6 12 12 18 18

501. • Which of the following equations is the correct one for the respiration equation? • A) C6H12O6 + 6H2O = Released energy + 6CO2 + 6H2O. • B) C6H12O6 + O2 = Released energy + C6H12O6 + 6CO2 + 6H2O. • C) C6H12O6 + 6O2 = Released energy + 6O2 + 6H2O. • D) C12H6O6 + 6O2 = Released energy + 6CO2 + 6H2O. • E) C6H12O6 + 6CO2 = Released energy + 6O2 + 6H2O. • F) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • G) C6H12O6 + 6O2 = Released energy + 6CO2 + 62O. • H) C6H12O6 + 6O2 = Light Energy + 6CO2 + 6H2O. • I) C6H12O6 + 6O2 = Released energy + 6O2 + 6H2O. • J) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • K) C6H12O6 + 16O2 = Released energy + 6O2 + 6H2O. • L) Released energy + 6CO2 + 6H2O C6H12O6 + 6O2 =  Copyright © 2010 Ryan P. Murphy

502. • Answer! Which of the following equations is the correct one for the respiration equation? • A) C6H12O6 + 6H2O = Released energy + 6CO2 + 6H2O. • B) C6H12O6 + O2 = Released energy + C6H12O6 + 6CO2 + 6H2O. • C) C6H12O6 + 6O2 = Released energy + 6O2 + 6H2O. • D) C12H6O6 + 6O2 = Released energy + 6CO2 + 6H2O. • E) C6H12O6 + 6CO2 = Released energy + 6O2 + 6H2O. • F) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • G) C6H12O6 + 6O2 = Released energy + 6CO2 + 62O. • H) C6H12O6 + 6O2 = Light Energy + 6CO2 + 6H2O. • I) C6H12O6 + 6O2 = Released energy + 6O2 + 6H2O. • J) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • K) C6H12O6 + 16O2 = Released energy + 6O2 + 6H2O. • L) Released energy + 6CO2 + 6H2O C6H12O6 + 6O2 =  Copyright © 2010 Ryan P. Murphy

504. • Which one is the equation for photosynthesis, and which one is the equation for respiration? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) C6H12O6 + O2 = Released energy + 6CO2 + 6H2O. • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) C6H12O6 + 6O2 = Released energy + 6O2 + H2O. • F) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • G) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • H) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N.) C6H12O6 + 6O2 = light energy + 6CO2 + 6H2O. Copyright © 2010 Ryan P. Murphy

516. • Which one is the equation for photosynthesis, and which one is the equation for respiration? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) C6H12O6 + O2 = Released energy + 6CO2 + 6H2O. • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) C6H12O6 + 6O2 = Released energy + 6O2 + H2O. • F) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • G) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • H) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N.) C6H12O6 + 6O2 = light energy + 6CO2 + 6H2O. Copyright © 2010 Ryan P. Murphy Law Conservation of Matter:

517. • Which one is the equation for photosynthesis, and which one is the equation for respiration? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) C6H12O6 + O2 = Released energy + 6CO2 + 6H2O. • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) C6H12O6 + 6O2 = Released energy + 6O2 + H2O. • F) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • G) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • H) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N.) C6H12O6 + 6O2 = light energy + 6CO2 + 6H2O. Copyright © 2010 Ryan P. Murphy Law Conservation of Matter: In any physical or chemical reaction, matter cannot be created or destroyed.

518. • Which one is the equation for photosynthesis, and which one is the equation for respiration? • A) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • B) C6H12O6 + O2 = Released energy + 6CO2 + 6H2O. • C) 6CO2 + 6O2 + light energy = C6H12O6 + 6H2O • D) 6CO2 + 12H2O + light energy = C6H12O6 + 6H2O • E) C6H12O6 + 6O2 = Released energy + 6O2 + H2O. • F) 6CO2 + 6H2O + light energy = C6H12O6 + 6O2 • G) 6CO2 + 6H2O + light energy = C6H12O6 + 6CO2 • H) C6H12O6 + 6CO2 = Released energy + 6CO2 + 6H2O. • I) 6CO2 + 6H6O + light energy = C6H12O6 + 6O2 • J) 6CO2 + 6H2O + light energy = CH12O6 + 6CO2 • K) C6H12O6 + 6O2 = Released energy + 6CO2 + 6H2O. • L) 6CO2 + 6H2O + no energy = C6H12O6 + 6O2 • M) 6O2 + 6H2O + light energy = C12H6O6 + 6O2 • N.) C6H12O6 + 6O2 = light energy + 6CO2 + 6H2O. Copyright © 2010 Ryan P. Murphy Law Conservation of Matter: In any physical or chemical reaction, matter cannot be created or destroyed. Just changes form.

521. Mitochondria

522. Mitochondria

523. Mitochondria Chloroplast

532. • Try Again __CH4 + __O2 --> __CO2 + __H2O___ NaCl + __ BeF2 --> __ NaF +__ BeCl2 Na Cl Be F

533. • Try Again BOXES!!! __CH4 + __O2 --> __CO2 + __H2O___ NaCl + __ BeF2 --> __ NaF +__ BeCl2 Na Cl Be F

534. • Try Again BOXES!!! __CH4 + __O2 --> __CO2 + __H2O___ NaCl + __ BeF2 --> __ NaF +__ BeCl2 Na Cl Be F

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