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Review of Chemistry 20

What you really need to remember !. Review of Chemistry 20. Review Topics. Metric System Lab safety (WHMIS, household symbols) Nomenclature (inorganic, organic) Quantum Theory. Metric System. SI BASE UNITS. Quantity Base Unit Symbol length metre m mass gram g

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Review of Chemistry 20

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  1. What you really need to remember ! Review of Chemistry 20

  2. Review Topics • Metric System • Lab safety (WHMIS, household symbols) • Nomenclature (inorganic, organic) • Quantum Theory

  3. Metric System

  4. SI BASE UNITS QuantityBase UnitSymbol length metre m mass gram g volume litre L temperature kelvin K time second s amount of matter mole mol electric current ampere A luminous intensity candela cd

  5. SI DERIVED UNITS QuantityName of Unit Symbol in SI Base Units density kilogram per kg · m-3 kg · m-3 cubic metre (kg/m3) force Newton N kg · m · s-2 (kg · m / s2) pressure Pascal Pa N · m-2 (kg·s-2·m-1 , N / m2) heat energy Joule J N · m (kg·m2·s-2 )

  6. SI Prefixes Prefix Symbol Multiplication Factor Exponential Notation exa E1 000 000 000 000 000 000 1018 peta P 1 000 000 000 000 000 1015 teraT 1 000 000 000 000 1012 gigaG 1 000 000 000 109 mega M 1 000 000 106 kilo k 1 000 103 hectoh 100 102 decada 10101 THE BASE UNIT 1 100

  7. SI Prefixes Prefix Symbol Multiplication Factor Exponential Notation THE BASE UNIT1 100 deci d 0.110-1 centi c 0.0110-2 milli m 0.00110-3 microμ 0.000 001 10-6 nano n 0.000 000 001 10-9 pico p 0.000 000 000 001 10-12 femto f0.000 000 000 000 001 10-15 atto a0.000 000 000 000 000 001 10-18

  8. The Metric System • These tables must be memorized. • The quiz will be on ......

  9. Hazardous Materials in the Home • The eight-sided outline (octagonal) signifies that the contents of the container is dangerous. • The triangular outline signifies that the container is dangerous, usually because the contents are under high pressure.

  10. Hazardous Materials in the Home Poison • poisons can enter the body in one of three ways: a) ingestion (eating) b) inhalation (breathing) c) absorption through the skin d) injection

  11. Corrosive • are chemicals which can act on clothing, skin, eyes or internally by drinking or eating • can cause symptoms ranging from mild rash to serious skin damage • can damage clothing • can cause blindness • can cause death if ingested

  12. Flammable • are substances which can burn easily or cause other materials to burn

  13. Radiation • radioactive materials emit high energy atomic particles or high energy radiation (x-rays, gamma rays), or both • found in smoke detectors and involve no danger if kept at a safe distance

  14. Explosive • can cause injury or death as a result a blast or because of the materials expelled by the blast (metal shards) • usually are pressurized aerosol containers which may explode when heated

  15. WHMIS Workplace Hazardous Materials Information System

  16. Class A - Compressed Gas • danger lies in the pressure, not in the contents.

  17. Class B -Combustible and Flammable Material • may burn at relatively low temperatures, burn spontaneously or as a result of heat, sparks or friction • hydrocarbons and several chemicals like phosphorus, sodium and calcium carbide would be included in the list.

  18. Class C - Oxidizing Material • may cause a fire, react violently or explode when it comes into contact with combustible materials such as wood. • an oxidizer supplies the oxygen for a chemical reaction.

  19. Class D, Division 1 – Poisonous and Infectious Material; Immediate and Serious Toxic Effects • these substances have acute toxicity - refers to a substance which has immediate effects, usually within 24 hours

  20. Class D, Division 2 – Poisonous and Infectious Material; Other Toxic Effects • these substances have chronic toxicity - refers to the effects of a substance through repeated exposure at low levels over a long period (weeks, months or years). • effects include; organ damage, illness or death • the effects can also include cancer, allergies or chronic diseases (bronchitis, emphysema, cirrhosis of the liver, etc.) • long term alcohol or cigarette use would fall under this category

  21. Class D, Division 3 – Poisonous and Infectious Material; Biohazardous Infectious Material • refers to an infectious agent (bacteria, virus or some other organism) which may spread disease if improperly handled, also called a biohazard • this symbol is common in hospital emergency rooms on containers where used needles and dressings are deposited

  22. Class E - Corrosive Material • causes severe eye and skin irritation upon contact • causes severe tissue damage with prolonged exposure • may be harmful if inhaled • the effects are the same as under the household hazards

  23. Class F - Dangerously Reactive Material • is very unstable • may react with water to release a toxic or flammable gas • may explode as a result of shock, friction or increase in temperature • undergoes vigorous polymerization • all of these reactions happen very quickly; you have to be extremely careful around these substances

  24. Lab Procedures and Rules • No eating or drinking in the lab. • Treat all chemicals as if they were hazardous: • Never perform unauthorized experiments. • Report all accidents immediately. • If you get a chemical solution in your eye go to the eyewash station immediately and wash the eye for at least 5 minutes. • If you get chemicals on your clothes, wash the clothes thoroughly. • Do not wear loose clothing during a lab. Tie long hair back. • Do not sit on the lab bench; you do not know how clean it is. • Clean all equipment thoroughly and put it back where it belongs. • Follow directions concerning the safe disposal of chemicals and solutions. • Clean your lab station thoroughly after a lab.

  25. In Case of An Accident: • Inhaled Poison - Remove the patient to fresh air and apply artificial respiration if necessary. Keep the victim warm with blankets. • Contact of Poison with Skin or Eyes - Flood affected area with water, for at least 5 minutes. Remove contaminated clothing. DO NOT attempt to use chemical antidote. • Swallowed Poison - If the person is conscious and able to swallow, immediately dilute the poison by giving the victim 2 to 4 cups of milk or water. • Swallowed Corrosives - DO NOT INDUCE VOMITING. Give milk and water. If vomiting occurs naturally, hold head below hips to avoid choking.

  26. Laboratory Equipment • Be able to identify the items on the sheet given. • Note: the flask is an erlenmeyer flask

  27. Nomenclature

  28. Types of Chemical Substances • Inorganic • elements • molecular • ionic • Organic • aliphatic • cyclic • substituted • Common substances • inorganic or organic

  29. Naming • must be simple as possible • must be unique

  30. Elements • one kind of atom • most are monoatomic (one atom) • Cu, Fe, Al, He • 8 elements are diatomic (2 atoms) • H2 N2 O2 F2 Cl2 Br2 I2 (At2) • 2 are polyatomic • S8 • P4

  31. Common Substances • known by names other than their systematic names • be familiar with • formulas • systematic name • common name • know whether systematic or common name takes precedence

  32. Common Substances FormulaChemical NameCommon Name H2O hydrogen oxide water NaClsodium chloride table salt HCl hydrogen chloride hydrochloric acid HNO3 hydrogen nitrate nitric acid H2SO4 hydrogen sulfatesulfuric acid H3PO4 hydrogen phosphate phosphoric acid CH3COOH acetic acid vinegar CaSO4calcium sulfate gypsum (dry wall) NH3 nitrogen trihydrideammonia

  33. Common Substances FormulaChemical NameCommon Name H2O2hydrogen peroxide hydrogen peroxide C2H5OH ethanol drinking alcohol CH3OH methanol wood alcohol CH4methane natural gas O3ozoneozone C12H22O11sucrose table sugar KClpotassium chloride potash NaOHsodium hydroxide lye, caustic soda CaOcalcium oxide lime

  34. Molecular Compounds • made up of 2 non-metals bound together with covalent bonds:

  35. Molecular Compounds • can’t predict formula so naming is done on a numbering system. • prefixes in front of the element name tell you how many of that element are present in the compound: mono 1 hexa 6 di 2 hepta 7 tri 3 octa 8 tetra 4 nona 9 penta 5 deca 10

  36. Molecular Compounds • N2O5 dinitrogenpentaoxide(note ending) • CO2 carbon dioxide (no mono on first atom) • CO carbon monoxide • Cl2O7 dichlorineheptaoxide

  37. -ides C carbide Cl chloride N nitride As arsenide O oxide Seselenide F fluoride Br bromide Si silicide Te telluride P phosphide I iodide S sulfide

  38. Molecular Compounds • tetraphosphorus decaoxide P4O10 • tetrasulfur tetranitride S4N4 • bromine monofluoride BrF • diarsenic triselenide As2Se3

  39. Ionic Compounds • made up of cations and anions which come together as a result of ionic attraction:

  40. Ionic Compounds • there is no molecule, rather a crystal lattice. • chemical formula is ratio of cations to anions in crystal; formula unit • ionic substances are recognized because they contain a metal + non-metal

  41. Writing Formula Units • the formula unit of any ionic compound is the ratio of cations to anions in the crystal lattice. • the net charge of a formula unit is zero. • it is written as the lowest ratio of cations to anions.

  42. Examples • K1+ F1-gives KF • Mg2+ Cl1- gives MgCl2 • Al3+ S2- gives Al2S3 • Ca2+ S2- gives CaS • Sr2+ OH1- gives Sr(OH)2 • NH41+ SO42- gives (NH4)2SO4

  43. Do first half of nomenclature assignment

  44. Using Ion Charge to Predict Formulas a) K1+, Br1- f) Zn2+ , O2- KBrZnO b) Ca2+, Cl1- g) Mg2+, NO31- CaCl2Mg(NO3)2 c) Li1+, H1- h) Fe2+, O2- LiHFeO d) Fe3+, OH1-i) Fe3+, O2- Fe(OH)3Fe2O3 e) Ca2+, OH1- j) Sn4+, F1- Ca(OH)2SnF4

  45. k) Hg2+, O2- p) Mn7+ , O2- HgO Mn2O7 l) K1+, PO43- q) Na1+, SeO32- K3PO4 Na2SeO3 m) Si4+, O2- r) Na1+, SeO42- SiO2 Na2SeO4 n) NH41+, SO42- s) Al3+, SO42- (NH4)2SO4 Al2(SO4)3 o) Na1+, PO43- t) H1+, S2- Na3PO4 H2S

  46. Using Formulas to Predict Ion Charge a) ZnSO4 f) KSCN Zn2+ SO42- K1+ SCN1- b) Mn(NO3)3 g) Na2SO3 Mn3+ NO31- Na1+SO32- c) SnO h) Al2(Cr2O7)3 Sn2+ O2- Al3+ Cr2O72- d) LiHCO3i) MgC2O4 Li1+ HCO31- Mg2+ C2O42- e) Hg2Cl2 j) SrH2 Hg22+ Cl1- Sr2+ H1-

  47. Simple Ionic Compounds • cations from groups 1 & 2, Al, Zn, Ag, Cd, NH41+ (all have only one possible charge) • anions can be anything on the chart (including polyatomic ions) • only one formula unit possible, so name is a repetition of the ion names: • NaCl Na1+ Cl1- sodium chloride

  48. Simple Ionic Compounds • NH4NO3 NH41+ NO31- ammonium nitrate • Al2(CO3)3 Al3+ CO32- aluminum carbonate • Ag3P Ag1+ P3- silver phosphide

  49. Simple Ionic Compounds • cadmium chlorite Cd2+ ClO21- Cd(ClO2)2 • strontium nitride Sr2+ N3- Sr3N2

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