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S-133

S-133. Write the formula for Palladium (IV) Oxide Calcium Fluoride Cadmium (II) Nitride Write the name for Al 2 S 3 Rb 3 P CrO 3. SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter.

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S-133

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  1. S-133 • Write the formula for • Palladium (IV) Oxide • Calcium Fluoride • Cadmium (II) Nitride Write the name for • Al2S3 • Rb3P • CrO3

  2. SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter. Demonstrate the Law of Conservation of Matter in a chemical reaction. Apply the Law of Conservation of Matter by balancing the following types of chemical equations; Synthesis Decomposition Single Replacement Double Replacement Unit 7 Chemical Reaction

  3. What is the law of conservation of mass? Why must chemical equations be balanced? Why do chemists use the mole? How can you calculate the mass of a reactant or product in a chemical reaction? 7.1 Describing Reactions

  4. 7.1 Describing Reactions What is the law of conservation of mass? • Chemical Equations • Reactants – the substances that are present before a reaction • Products – the substances present after a reaction is complete • Always given in the form Reactants  Products • Example:Carbon + Oxygen  Carbon Dioxide • Or C + O2 CO2

  5. 7.1 Describing Reactions What is the law of conservation of mass? • Writing Equations - Practice • Copper and Oxygen make Copper (II) Oxide • Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride • Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water. • Hydrogen and Chlorine combine to make Hydrogen Chloride

  6. 7.1 Describing Reactions What is the law of conservation of mass? • Conservation of Mass • Mass is not created or destroyed in a chemical reaction • For practical purposes • Same types of atoms before and after a reaction • Same number of each type of atom before and after • Equations must show this • They are called balanced equations

  7. S-134 • Write the formula for • Dinitrogen Trioxide • Copper (II) oxide • Dinitrogen Pentaoxide Write the name for • CCl4 • CrBr3 • Mo2O5

  8. S-135 • Write the equation for a reaction of hydrogen sulfide with aluminum oxide to make aluminum sulfide and water.

  9. 7.1 Describing Reactions Why must chemical equations be balanced? • Balancing Equations • If an equation does not have the same elements on both sides, it is a false equation • Can not actually occur • Coefficient – a number placed in front of a substance in a chemical equation • Used to balance equations

  10. 7.1 Describing Reactions Why must chemical equations be balanced? • Balancing Equations - Steps • First write out the equation • Hydrogen and Oxygen make water becomes • H2 + O2 H2O • List the elements on each side H-2  H-2 O-2 O-1 • Add substances until both sides are equal

  11. 7.1 Describing Reactions Why must chemical equations be balanced? • Balancing Equations - Practice • Copper and Oxygen make Copper (II) Oxide • Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride • Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water.

  12. S-137 • Balance the following equations H2SO4 + Al(OH)3 Al2(SO4)3 + H2O

  13. 7.1 Describing Reactions Why do chemists use the mole? 18 Ar 39.95 Argon • Counting With Moles • A unit of measurement • Equals 6.02 x 1023 of anything • Used only to count atoms, molecules, formula unit • One mole of an element is equal to its atomic mass converted to grams (put a g beside the number)

  14. 7.1 Describing Reactions How can you calculate the mass of a reactant or product in a reaction? • Molar Mass • For an element equal to its atomic mass • For a compound • For each element – multiply the mass x the number of that element in the compound • Add the total

  15. 7.1 Describing Reactions How can you calculate the mass of a reactant or product in a reaction? • Molar Mass-Example • C2H4 • Carbon 12.01g x 2 = 24.02g • Hydrogen 1.01g x 4 = 4.04g • Total 28.06

  16. 7.1 Describing Reactions How can you calculate the mass of a reactant or product in a reaction? • Molar Mass-Example • Pb(OH)4

  17. S-137 • What is the molar mass of Al2(SO4)3

  18. What are the general types of chemical reactions? 7.2 Types of Reactions

  19. Types of Reactions What are the general types of reactions? • Classifying Reactions • Describe how reactants interact to form products • Help to predict the products of reactions

  20. Types of Reactions What are the general types of reactions? • Synthesis • Two or more substances react to form a single substance • Pattern A + B  AB • Always has one product • Examples • 2Na + Cl2 2NaCl • 2H2 + O2 2H2O

  21. Types of Reactions What are the general types of reactions? • Decomposition • One substance breaks apart into two or more products • Pattern AB  A + B • Always has one reactant • Examples • CaCO3 CaO + CO2 • 2H2O 2H2 + O2

  22. Types of Reactions What are the general types of reactions? • Single Replacement (Displacement) • A compound switches parts with an element • Pattern A + BC  B + AC • Always has one element and one compound on each side • Examples • Cu + 2AgNO3 2Ag + Cu(NO3)2 • 2K + 2H2O  H2 + KOH

  23. Types of Reactions What are the general types of reactions? • Double Replacement (Displacement) • Two compounds switch parts • Often results in the formation of a precipitate • Pattern AB + CD  AD + CB • Always has two compounds on each side • Examples • Pb(NO3)2 + 2KI  PbI2 + 2KNO3 • CaCO3 + 2HCl  CaCl2 + H2CO3

  24. Types of Reactions What are the general types of reactions? • Combustion • Reacts rapidly with oxygen • Everything combines with oxygen • Pattern AB + O2 AO + BO • Always has oxygen as a reactant • Examples • CH4 + O2 CO2 + 2H2O • 2Ca + O2  2CaO

  25. S-138 • Balance the following reactions and tell what type(s) they are. • Pb(NO3)2 + HCl  PbCl2 + HNO3 • Ca + HCl  CaCl2 + H2

  26. S-139 • Write out the reaction, then balance it and tell what type it is. • Mercury reacts with oxygen to form Mercury (II) Oxide

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