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Chemical Reactions

Chemical Reactions. Chapter 6. Today we will…. Explain Chemical and Physical properties and changes using Cornell Notes and white boards. 1. Observing chemical change. 2. Properties of matter 3. Physical property 4. does not change into a different substance 4. Examples.

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Chemical Reactions

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  1. Chemical Reactions Chapter 6

  2. Today we will… ExplainChemical and Physical properties and changes using Cornell Notes and white boards.

  3. 1. Observing chemical change 2. Properties of matter 3. Physical property 4. does not change into a different substance 4. Examples

  4. 3. Chemical property 4. A new substance has the ability to form 4. Examples 5. 5. 5. 5.

  5. 2. Changes in matter 3. Physical change 4. no new substance is formed

  6. 3. Chemical change 4. Chemical reaction 4. Atoms are rearranged to form new substances with new properties 4. Reactants 5. Substances that undergo change in a reaction 4. Products 5. New substances formed by the reaction

  7. 2. Bonding and chemical change 3. Chemical changes occur when bonds break and form new bonds 3. New substances are created

  8. + Googleimages.com

  9. 2. Changes in properties 3. Chemical reactions involve changes in properties AND changes in energy that you can observe

  10. 3. Precipitate 4. Solid that forms from a solution during a chemical reaction 5. EX: Sugar crystals 3. Gas formed from solid or liquid reactants 4. Ex: ammonia + bleach = bad gas! 3. Changes in texture or softness

  11. 2. Changes in energy 3. Endothermic reaction 4. Breaking and making of bonds that absorb the energy in the form of heat 3. Exothermic reaction 4. breaking and making of bonds that results in the release of energy in the form of heat

  12. Today we will… Explainchemical equations and conservation of matter while formulatingbalanced equations using Cornell Notes and white boards.

  13. 1. Describing chemical equations 2. Chemical equations – what are they? 3. Short, easy way to show a chemical reaction, using symbols instead of words 3. Reactant + reactant product + product

  14. 2. Conservation of matter 3. During a chemical reaction, matter is neither created nor destroyed. 3. The mass of the reactants must equal the mass of the products 3. The number of atoms stays the same no matter how they are arranged.

  15. 2. Open and closed systems 3. Open system – matter can enter from or escape the surroundings 4. ex: Fire place southernchimneysweep.com

  16. 3. Closed system – Matter not allowed to leave or enter. 4. Pumpkin decaying in a bag. sleeplessinamman.com

  17. 2. Balancing equations 3. A chemical equation must show the SAME number of each type of atom on both sides of the equations

  18. 3. Steps to balancing equations Step 1: write the equation Step 2: Count the atoms Step 3: Use Coefficients to balance atoms Step 4: Look back and count 3. Coefficient – what are they? 4. Number placed in front of a chemical formula

  19. LEFT PAGE

  20. Homework: Complete practice problems for balancing equations: 1) ____ Na3PO4 + ____ KOH  ____ NaOH + ____ K3PO4 2) ____ MgF2 + ____ Li2CO3 ____ MgCO3 + ____ LiF 3) ____ P4 + ____ O2 ____ P2O3 4) ____ RbNO3 + ____ BeF2 ____ Be(NO3)2 + ____ RbF 5) ____ AgNO3 + ____ Cu  ____ Cu(NO3)2 + ____ Ag

  21. Homework: 6) ____ CF4 + ____ Br2  ____ CBr4 + ____ F2 7) ____ HCN + ____ CuSO4  ____ H2SO4 + ____ Cu(CN)2 8) ____ GaF3 + ____ Cs  ____ CsF + ____ Ga 9) ____ BaS + ____ PtF2  ____ BaF2 + ____ PtS 10) ____ N2 + ____ H2  ____ NH3

  22. Today we will… Classify chemical reactions using Cornell Notes, our brains, and various strategies.

  23. 1. Describing Chemical reactions

  24. 2. Classifying chemical reactions 3. Synthesis 4. Put things together 4. Two or more elements or compounds combine to make a more complex substance 4. Ex: 2H + O = Water

  25. 3. Decomposition 4. Compounds break down into simpler products 4. Ex: Hydrogen peroxide breaks down into water and oxygen 2H202 2H20 + O2

  26. 3. Replacement 4. When one element replaces another in a compound 4. When two elements in different compounds trade place 2Cu2O + C 4Cu + CO2

  27. Chemistry is • A characteristic of a substance that can be observed without changing the substance into another substance • The study of matter and how matter changes • Anything that has mass and takes up space • A rapid reaction between oxygen and a substance called fuel.

  28. Anything that has mass and takes up space is considered • Matter • Energy • Chemistry • Endothermic

  29. What happens when chemical bonds break and new bonds form? • A physical change • A chemical reaction • Matter is destroyed • Surface area increases

  30. The only sure evidence for a chemical reaction is • The formation of a gas • A color change • The production of one or more new substances • Changes in properties

  31. A chemical reaction that absorbs energy in the form of heat is described as • Endothermic • Exothermic • Combustion • Unbalanced

  32. CaCO3 represents a chemical • Symbol • Formula • Subscript • Reaction

  33. A shorter, easier way to show chemical reactions, using symbols instead of words, is called a • Chemical equation • Chemical formula • Symbol • Subscript

  34. The substances listed on the left side of a chemical equation are the • Products • Coefficients • Precipitates • Reactants

  35. In a(n) ____ change, elements and/or compounds rearrange to form new substances.

  36. A material used to decrease the rate of a reaction is called a _____.

  37. The process of solid ice changing into liquid water is a(n) ____ change.

  38. A precipitate is a(n) ____ that forms from solution during a chemical reaction.

  39. The ____ is the amount of one material present in a given volume of another material.

  40. In a chemical equation, the substances written on the right side of the arrow are called?

  41. A chemical reaction that releases energy in the form of heat is a(n) _______ reaction.

  42. Every chemical reaction involves a change in • Energy • Concentration • State • Mass

  43. The number placed below an element’s symbol in a chemical formula is called a • Subscript • Coefficient • Reactant • Product

  44. The minimum amount of energy that has to be added to start a reaction is the • Chemical energy • Activation energy • Endothermic energy • Exothermic energy

  45. What is the purpose of a coefficient?

  46. Chemistry is? • The study of matter and how matter changes • Anything that has mass and takes up space • A rapid reaction between oxygen and a substance • The study of physics

  47. Chemicals that act as biological catalysts by speeding up reactions in living things are • Enzymes • Fuels • Inhibitors • Reactants

  48. List three examples of a chemical change

  49. Define Synthesis and decomposition.

  50. Discuss with your group the following questions. • Why is learning exothermic and endothermic reactions important to your life? • Based on what you know, how would you explain chemical reactions?

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