5.2 and 5.3 SALTS & ORGANIC COMPOUNDS

1. 5.2 and 5.3 SALTS & ORGANIC COMPOUNDS

2. Uses of SALT • Salt is a preservative, a flavor enhancer, and can also be used as a cleaning agent, a medical disinfectant and many others. • SOME OTHER USES: • 1. Adding salt to water doesn’t make it boil faster, but it does make water boil at a higher temperature. This can come in handy when you need to reduce cooking time by using hotter water. • If you put salt on your salad, it will add flavour and will keep the lettuce crisp. • If you cook with onions, you can get rid of the smell on your hands, pots, cutting boards with a mixture of salt and vinegar. • You can put out a grease fire with a handful of salt.

3. Uses of SALT • SOME OTHER USES: • If you are battling poison ivy, or have a lot of aches and pains, soak in a salt bath. • If you have a throat infection, gargle with salt water to kill the bacteria. • If you have an ant problem, put salt on and around the ant hills to destroy the worker ants and queen. You can also put salt around the doors or windows where ants get into your house. • Salt is a good weed killer as well. If you spread salt in the cracks and crevices between the rocks and brick it will prevent weeds from growing there. Make sure that you water the salt so it washes down to the roots.

6. 5.2 and 5.3 SALTS & ORGANIC COMPOUNDS Recognize a salt when presented with its formula, name, or properties. Define organic compounds and inorganic compounds Distinguish between organic and inorganic compounds based on their chemical structures. Recognize a compound as organic or inorganic from its name, from its chemical formula, or from a diagram or model.

7. 5.2 and 5.3 VOCABULARY • Salts • Neutralization • Compounds • Organic Compound • Inorganic Compound • Hydrocarbon • Alcohol

8. 5.2 SALTS • Table salt, NaCl, is found in sea water, salt lakes or rock deposits. • Salt was once more valuable than gold. • Iodine is now added to salt to minimize goiter (a disease of the thyroid). See pages 234 - 235 (c) McGraw Hill Ryerson 2007

9. IODINE & THYROID GLANDS The thyroid gland needs a very large amount of iodine to make the hormone thyroxin. Thyroxin controls our metabolic rate.

10. GOITER

11. 5.2 SALTS Salts are found in many things: • In batteries, explosives and fertilizers • In multivitamins • In many living cells See pages 234 - 235

12. 5.2 Acid-BASE NEUTRALIZATION • SALTS are made when an acid and a base react to produce a salt and water. • This is called a NEUTRALIZATION REACTION. • HCl(aq) + NaOH(aq)  NaCl(s) + H2O(l) acid base salt water See pages 236 - 237 (c) McGraw Hill Ryerson 2007

13. 5.2 SALTS • NaCl is only one kind of salt. • A salt is made up of a positive ion from a base and a negative ion from an acid. EXAMPLES: • a. HCl + NaOH --> NaCl + HOH • b. H2SO4+ 2 NH4OH --> (NH4)2SO4 + 2 HOH • c. 2 NaOH + H2CO3 --> Na2CO3 + 2 HOH See pages 234 - 235

14. 5.2 SALTS • Which one is the Acid? Base? Salt? Mg(OH)2 + 2HF MgF2 (salt) + 2HOH See pages 234 - 235 (c) McGraw Hill Ryerson 2007

15. 5.2 Acid-BASE NEUTRALIZATION • IMPORTANCE OF NEUTRALIZATION? • When you get heartburn or ulcers, it is because your stomach is making too much hydrochloric acid and it is starting to burn or eat away at your stomach or esophagus lining. • What do we do to solve this? Take antacids which contain a base (for example: aluminum hydroxide (Al[OH]3) or magnesium hydroxide (Mg[OH]2). These antacids neutralize the acid to make salt and water. • Ie: 3HCl + Al (OH)3 AlCl3 + 3H(OH) Why not just take sodium hydroxide? This is the substance we use to unclog drains and clean ovens. You would end up with a worse problem than before.

16. 5.2 SALTS • Salts are also produced when metals react with acids. • Metal plus an acid makes salt! • http://www.youtube.com/watch?v=MfsFRBh2tys Zn + HCl ZnCl (salt) + H2 (c) McGraw Hill Ryerson 2007

17. 5.2 ACIDS & METALS • Acids and Metals • The most reactive metals, are on the bottom of families 1 and 2 (alkali metals and alkali earth metals). • These will react vigorously with acids to produce HYDROGEN GAS (H2). • Other metals are less reactive. • Example: • 2HCl(aq) + Mg(s)  MgCl2(s) + H2(g) TRY FOR YOURSELF: http://www.teachersdomain.org/resource/lsps07.sci.phys.matter.metalshcl/

18. 5.2 SALTS • Salts are also made when carbonates (CO32-) react with acids. • The products of this type of reaction are SALT, water and carbon dioxide. • Egg shells and Bones contain calcium carbonate CaCO3 2H2C2H3O2 (vinegar) + CaCO3 Ca (C2H3O2)2 (salt) + H2O + CO2 If you put an egg in vinegar, and leave it for 3 days, the vinegar will dissolve the calcium carbonate and you’ll be left with a bouncing egg! Try it! (c) McGraw Hill Ryerson 2007

19. 5.2 SALTS • If you put a chicken bone in vinegar the same reaction will occur, and after 3 days you’ll be left with a rubber chicken bone that you can tie in a knot. Try it! 2H2C2H3O2 (vinegar) + CaCO3 Ca (C2H3O2)2 (salt) + H2O + CO2 (c) McGraw Hill Ryerson 2007

20. 5.2 METAL & NON-METAL OXIDES • A metal + oxygen => metal oxide • Metal oxides are used in making fireworks • Metal oxides react with water to form bases. • Na2O(s) + H2O(l)  2NaOH(aq) Memory trick: heavy metal bands have BASE players! YOU TUBE: http://www.youtube.com/watch?v=l9z5-mJ8NZk&feature=related

21. Memory trick: pollution makes ACID RAIN! 5.2 METAL & NON-METAL OXIDES • A non-metal + oxygen => non-metal oxide • Examples of non-metal oxides: • carbon monoxide, carbon dioxide, sulphur dioxide... • Non-metal oxides react with water to form acids • SO2(g) + H2O(l)  H2SO3(aq) • Non-metal oxides are formed when we burn fossil fuels (gas, coal…) • When these oxides join with water in the atmosphere, the resulting acids create acid rain. ACID RAIN VIDEO: http://www.bcscience.com/bc10/pgs/videos_010_acid_rain.html

23. 5.2 METAL & NON-METAL OXIDES

24. 5.3 ORGANIC COMPOUNDS • Organic compounds contain carbon and usually hydrogen. • “Organic” sounds like the compounds come from living things, and some do, but some do not. • Inorganic compounds are compounds that do not have carbon. See pages 244 - 246 (c) McGraw Hill Ryerson 2007

25. 5.3 ORGANIC COMPOUNDS Carbon has four electrons in its valence shell, which allows for more chemical bonding possibilities than any other element.

26. 5.3 ORGANIC COMPOUNDS Long chains of carbons form petroleum and plastics.

27. 5.3 ORGANIC COMPOUNDS Long chains of carbons form petroleum and plastics.

28. Why is CARBON so important? Carbon is so important to life _________________________ because all known life forms are associated with and depend on reactions involving carbon.

29. carbon is also the "BACKBONE OF LIFE"

30. 5.3 ORGANIC COMPOUNDS • Organic molecules always have C before H in their formulas. • This is different from acids, which almost always start with H.

31. 5.3 ORGANIC COMPOUNDS: HYDROCARBONS • A hydrocarbon is an organic compound that contains only carbon and hydrogen. • Hydrocarbons are based on a carbon chain, with hydrogen atoms added on the sides. • The simplest hydrocarbon is methane (CH4), followed by ethane (C2H6), propane (C3H8), butane (C4H10), and pentane (C5H12). • All hydrocarbons are flammable, and most are liquids are room temperature. See pages 246 - 247

32. 5.3 ORGANIC COMPOUNDS: ALCOHOLS • Alcohols are organic compounds with C, H, and O. • The simplest alcohols are methanol (CH4O), ethanol (C2H6O), and isopropyl alcohol (C3H8O). • Alcohols are very good solvents (they dissolve other substances). • Alcohols are generally very flammable. See pages 246 - 247 (c) McGraw Hill Ryerson 2007