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Chemical Reactions & Acids, bases, and solutions

Chemical Reactions & Acids, bases, and solutions. Chapter 6 and 7. Today we will . Explain balancing equations using Cornell Notes and Vocab Maps. 1. Describing chemical equations. 2. Chemical equations – what are they?

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Chemical Reactions & Acids, bases, and solutions

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  1. Chemical Reactions & Acids, bases, and solutions Chapter 6 and 7

  2. Today we will Explain balancing equations using Cornell Notes and Vocab Maps.

  3. 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

  4. 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.

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

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

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

  8. 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

  9. Today we will… Classify chemical reactions using Cornell Notes, our brains, and concept maps.

  10. 1. Describing Chemical reactions

  11. 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

  12. http://www.soundonsound.com/sos/jul10/articles/polivoks.htm

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

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

  15. Questions How could you determine ….? What would happen if….? How would you categorize….?

  16. Homework Concept maps: Synthesis Decomposition Replacement

  17. Today we will…. Analyze solutions, concentrations and solubility using Cornell Notes and task cards.

  18. 1. Solutions – what are they? 2. A uniform mixture that contains a solvent and at least one solute 2. Solvent – what is it? 3. A Part of the solution present in the largest amount 2. Solute – dissolved by the solvent and cannot be seen in the solution

  19. 2. Example Water + Sugar = Sugar water Water = Solvent Sugar = Solute Sugar water = solution

  20. 2. Colloids – what are they? 3. Mixture that contains small, undissolved particles that do not settle out. 3. The particles are too small to be seen, but large enough to scatter a light beam 3. Examples: 4. Fats and proteins in milk 4. Fog 4. Jell-O 4. Shaving cream

  21. 2. Suspension – what is it? 3. A mixture in which particles can be seen and easily separated by settling or filtration. 3. Heterogeneous mixture 3. Examples : 4. Snow globe

  22. 2. Concentrated Solution 3. A lot of solute dissolved in a certain amount of liquid 3. Examples 4. Frozen fruit juices 4. 3 cups of sugar in lemonade

  23. 2. Measuring concentration 3. The amount of solute is compared to the amount of solution and measured by % 4. Solute/solution * 100 = % concentration

  24. Practice problem A solution contains 12 grams of solute dissolved in 36 grams of solution. What is the concentration of the solution?

  25. Practice problems Page 267 Numbers 4 and 5

  26. 2. Dilute solution – what is it? 3. Has a little solute dissolved in a certain amount of solvent. 3. Example 4. 1 Cup of sugar dissolved in 8 cups of lemonade 4. Frozen fruit juice with 8 cups of water added.

  27. 2. Solubility – what is it? 3. Measure of how much solute can dissolve in a solvent at a given temperature 3. Unsaturated solution 4. You can add more to the solution 3. Saturated solution 4. You cannot add more to the solution 3. Supersaturated solution 4. Has more solute than the solution can hold and usually it settles out.

  28. 3. Temperature 4. As temperature increases, solubility increases 5. the solution can hold more solute 4. To dissolve more sugar, heat the water 4. Gases tend to become more soluble in cold temperatures 5. Hot soda tastes “flat”

  29. Practice time  Page 266 numbers 1-4 on the graph.

  30. Today we will… Describe acids and bases using Cornell notes and litmus paper.

  31. 1. Acids and Bases 2. Acids – what are they? 3. A substance that tastes sour, and reacts with metals and carbonates 3. 0-6 on the pH scale 3. Can be corrosive 3. Turns blue litmus paper red 3. Produce a hydrogen ion H+ in water

  32. 3. Examples of Acids 4. 4. 4. 4. Oranges 4. Tomatoes 4. Spinach

  33. 2. Uses of Acids 3. Vitamin C 3. Various vitamins and minerals 3. Used to clean bricks and metals 3. Found in fertilizer 3. Batteries

  34. 2. Bases – what are they? 3. A substance that tastes bitter and feels slippery 3. 8-14 on the pH scale 3. Produces hydroxide ions OH- in water 3. Turns litmus red litmus paper blue

  35. 3. Examples 4. Ammonia 4. Glass cleaner 4. Baking Soda 4. Calcium Oxide and calcium hydroxide make mortar and cement

  36. 2. Uses of bases 3. Cleaning agent 3. Creates mortar and cement 3. Used in baking that make baked goods fluffy.

  37. Homework Memory map: Acid, Base

  38. Warm-up On the left side of your notes complete the following: Create a Venn Diagram to compare and contrast ACIDS vs Bases. You have 5 minutes!

  39. Today we will… Describe acids and bases in Solutions using Cornell Notes and a foldable.

  40. 1. Acids and Bases in solutions 2. Acids in solutions 3. H+ are present 3. HCl -> H+ + Cl- in water 3. In water the H breaks the bonds with the compound and forms H+

  41. 2. Bases in solutions 3. OH- (hydroxide ion) when bases dissolve in water 3. Not all bases contain OH- 4. ammonia NH3 3. Produces OH- ions in water

  42. 2. Strength of acids and bases 3. pH scale ranges from 0-14 4. Describes the concentration of ions 3. 0-6.99 acidic 4. lemon 3. 7 neutral 4. water 3. 7.1 – 14 basic4. Drain cleaner 3. 0 = Strong acid while 6 is a weak acid 3. 8 = weak base while 14 is a strong base

  43. 2. Acid-base reactions 3. Neutralization 4. reaction between an acid and a base causing it to become neutral

  44. Antacid Pre-Lab Question: Which antacid works the best? Hypothesis: Materials Procedure

  45. Antacid Table

  46. 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.

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

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

  49. 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

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