Science Review: Measurements, Graphs, and Atomic Theory

1. Final Review 2013

2. Chapts 1-2 • a)Hypothesis:tentative answer to a questionb) Control : used for comparisonc)Theory: explanation supported by many experimentsd)Law: relationship in nature supported by experimentse) Independent Variable: one changed by the experimenterf) Dependent variable: one changed because of the independent variable

3. Review 2a) Safety: -goggles -apron -closed toe shoes -hair tied back

4. Review • -follow directions -report accidents to teacher -place waste in designated containers -know the location of safety equipment -no horseplay

5. Review c) Flush with water for 5 minutesd) Rinse in safety shower (fully clothed)

6. Review 3. mass- electronic balance volume- graduated cylinder length – metric ruler time- stop watch temperature – thermometerAll measurements should have a NUMBER and UNIT!

7. SI Units for Measurements • Mass – grams • Volume – liters • Length – meter • Time – seconds • Temperature - ˚C

8. Accuracy & Precision Accurate- measurements are CLOSE to the accepted value Not accurate- measurements are NOT CLOSE to the accepted value PRECISE – series of measurements close to each other

9. Review c) Percent error: d) density: e) quantitative data: numerical data (numbers) f) qualitative data: information describing color, odor, shape etc

10. Accepted value is 1.59 g/ml 5a) Group A most accurate Group C precise None

11. % error for Group A 5d) (1.59 – 1.57) X 100 1.59 = 1.3%

12. Scientific Notation 6a) 4.5 x 10-5 = .000045 b) 8.7 x 106 = 8700000 7a) 238,000 = 2.38 x 105 b) 0.00072 = 7.2 x 10-4 2 sig figs 2 sig figs 3 sig figs 2 sig figs

13. Density 8) 9) 2100g Density = 30g/mL 70mL 75g 20mL Density = 3.75g/mL

14. Density • 20/5 = 4g/mL B is the same • Read the BOTTOM of the meniscusVolume is 43.0mL

15. Graphs 13a) Pie graph- percentages b) Bar graph- comparisonsc) line graph- shows how the dependent variable changes with a change in the independent variable

16. Graphing Rules • Title • Labeled axes • Equal intervals • Use up most of the page • Use a key if needed X-axis – independent variableY-axis – dependent variable

17. Chapter 3 14) Definitions are in the textbooka) Cutting plastic - physical b)Rotting meat- chemicalc) water evaporating- physical d) Dissolving salt- physical e) Bubbles formed when vinegar reacts- chemical f) Gold conducting electricity- physical g) Magnesium burning- chemical 15) bubbles- chemical change ex odor, heat, precipitate

18. Definitions/examples • Element example- Au, Zn, Br etcCompound examples- NaCl N2O5ZnBr2

19. Homo vs Hetero • Salt water- homo b)clay and oil- hetero c) sweet tea- homo d) kool-aid- homo e) vegetable soup- hetero f)chunky peanut butter- hetero g) muddy water- hetero

20. Separating Substances • Colors in black ink- chromatography b) salt water- evaporation c)sand and water- filtration d)iron filings and sulfur- magnetism f) two different liquids- distillation Chromatography Filtration Distillation

21. Types of Mixtures b is a suspension Tyndall effect

22. Atomic Theory Scientists • USE THE TEXTBOOK – page 103 to 104 • Use the textbook for definitions • See page 114 of the textbook • Atomic # is number of PROTONS a) lithium atomic # 3 b) 3 protons and electrons c) sulfur – 16 Protons d) Lithium – 4 neutrons • silver-107 47 protons and 60 neutrons • neutrons = mass – protons = 31 neutrons 57 Fe26

23. Types of Radiation 27a) Alpha beta gamma b) c) 0ϒ0 4 He2 0β-1

24. Nuclear Equations d) 226 222 Ra  Rn + 88 86ii) 14 14 C  N + 67 4 He2 0β-1

25. Fission vs Fusion 28) • Fusing small nuclei • LARGE amounts of energy produced • Occurs in the sun • Responsible for all elements heavier than H • Splitting a heavy nucleus • Energy produced **Cheap source of energy with less pollution than burning coal, however, expensive to build the plant, problems with getting rid of nuclear waste etc

26. Half- Life 29)

27. Half- Life 29b)

28. Half-Life application 30) Using C-14 to determine the age of a fossil

29. Isotopes 31) Mg-24 contributes the most to the average atomic mass of magnesium (closest to the number on the periodic table), so it is the most abundant in nature.

30. Weighted Average Atomic Mass 32) Element X is BORON TOTAL: 10.812

31. Chapter 5 33) Get definitions from the textbook 34) s, p, d, fb) Various shapes- spherical, dumbbell etc

32. Sublevels c)

33. Electronic Configurations 35) Li- 1s22s1 [He] 2s1 b) Ne- 1s22s22p6 [He] 2p6 c) Al- 1s22s22p63s23p1[Ne] 3s23p1 d) Ca- 1s22s22p63s23p64s2[Ar] 4s2 36) Si b) F c) Na

34. Valence Electrons 37) Beryllium (group 2A) - 2 valence e- b) Nitrogen (group 5A) - 5 valence e- c) Argon- (group 8A) 8 valence e- d) Sulfur- (group 6A) 6 valence e- e) Boron- (group 3A) 3 valence e-

35. Flame Tests 38) Elements give of distinct colors when heated in a flame. The color of the flame is matched to the known element.

36. Electron Configuration 39a) 4p1 – Gallium b) 5s2 – Strontium c) 6p6 – Radon d) 7s1 – Francium 40) Same column- similar ending config

37. Concepts a) Valence e- is the SAME as the group number • Cesium – 1 Nitrogen – 5 Oxygen – 6c) d) Period tells you the # of energy levels (rings) e) s-block (groups 1 & 2) p-block (groups 3A-8A) d-block (transition metals) f-block (lanthanides & actinides) Cs O N

38. Periodic Trends c) Ionization Energy decreases down the group increases across Lowest IE – Francium Highest IE - Helium

39. Periodic Trends d) Electronegativity decreases down the groupincreases acrossLowest E– Francium Highest E - Fluorine

40. Periodic Trends e) Metals become SMALLER when they turn into ionsNon-metals become LARGER

41. Periodic Trends f) Francium is most active metal.Fluorine most active non-metal.

42. AKS 11b Trends on Element Properties

43. AKS11b Metal/Nonmetal/Metalloid • Metals left, nonmetals right , metalloids border the stairstep line. Stairstep line separates metals and nonmetals

44. AKS11b Metal/Nonmetal/Metalloid c) Metals - shiny, malleable, ductile, conduct electricity, react with acid Nonmetals - mostly gases, dull brittle, do not react with acids, nonconductorsMetalloids - have properties of BOTH metals & nonmetals d) Metals mostly s and d block Nonmetals and metalloids mostly p block

45. Chapter 8 - Ionic Bonding • a)b) CaCl2

46. Chapter 8 - Ionic Bonding 2a) Binary compounds – 2nd element gets “ide” b) Roman numerals used for transition metals that have more than one charge ex Fe2+ and Fe3+ 2a) KBr - Potassium Bromide b) CaCl2 - Calcium chloride c) SnO2 - Tin (IV) oxide d) Cu(NO3)2 – Copper (II) nitrate e) Sr(OH)2 – Strontium hydroxide

47. Ionic Bonding question #4

48. Ionic Bonding 5a) Na2SO4 - Sodium sulfate b) SnO2 - Tin (IV) oxide c) FePO4 - Iron (III) phosphate d) Ca(NO2)2 - Calcium Nitrite e) MgCO3 - Magnesium Carbonate f) Al(OH)3 - Aluminum hydroxide g) (NH4)3N - Ammonium nitride h) AgC2H3O2 - Silver acetate i) Fe3P2 - Iron (II) phosphide

49. Chapt 9 - Covalent Bonding 6)

50. Covalent Bonding 7) Binary covalent compounds end in “ide” 9) a) PH3 - phoshporustrihydride b) CCl4 - Carbon tetrachloride d) NO - Nitrogen monoxide f) As2O5 - Arsenic pentoxide