Midterm Part 2

32. Valence electrons and atomic numbers. Atomic numbers increase as you move across the periodic table Number of valence electrons also increase Transition elements are exception

33. What are the subatomic particles for an isotope. Ex. Carbon-12 & Carbon-14 6 protons for each Carbon-12 – Neutrons = 6 Carbon-14 – Neutrons = 8

34. Oxidation Number Electrons lost or gained See periodic table Metals (positive) & nonmetals (negative)

35. Fission and Fusion Fission: when 2 nuclei separate(chain reaction) Fusion: when 2 nuclei come together – Ex. Sun Both take small masses and convert into great amounts of energy

36. Uses of nuclear applications Medical – Radioactive tracers – Radiation for cancer treatment Nuclear power plants Nuclear weapons

37. Molecule and Atom Molecule: covalently bonded group of elements – Smallest part of a compound Atom : smallest piece of matter

38. Types of Chemical Bonds Ionic: metal + nonmetal Covalent: nonmetal + nonmetal – Single, double, or triple bonds – Polyatomic ions

39. Chemical bonding and stability To complete outer energy level * remember * 8 valence electrons Exception: Hydrogen and Helium Argon Atom

40. How does covalent bonding cause stability? Ex. Group 14: 4 valence electrons – Would take too much energy to lose or gain 4 electrons – More chemically stable to just share

42. Ionic & Covalent Bonding Ionic Bonds (crystalline) – Metal + Nonmetal – Ex. NaF, MgO, Al 2 O 3 Covalent Bonds (molecular) – Nonmetal + nonmetal – *Prefixes* – Ex. P 3 N 5, PCl 3

43. Writing chemical formulas for Binary Ionic Compounds Write name of positive ion first, then add –ide to end of negative ion Ex. KCl – Potassium Chloride Ex. BaF 2 – Barium Fluoride

44. Balanced chemical equation Balance using only coefficients Same number of atoms of each element on each side 2Mg(s) + O 2 (g)  2Mgo(s)

45. Law of Conservation of Mass Reactants = products Matter is neither created nor destroyed.

46. Endothermic and Exothermic Reactions Endothermic: energy is used, temperature decreases – Ex. Cold pack Exothermic: energy released, temp. increases – Fire

47. Evidence of Chemical Reaction Evolution of gas Precipitate formation Changes in : – Temperature – Color – Smell

48. Synthesis Equation A + B  C CaO(s) + H 2 O  Ca(OH) 2 (aq)

49. Decomposition Equation C  A + B NH 4 NO 3  N 2 O + 2H 2 O

50. Single and Double Displacement Reaction Single Displacement A + BC  AC + B Fe + CuSO 4  FeSO 4 + Cu Double Displacement AB + CD  AD + CB Ba(NO 3 ) 2 + K 2 SO 4  BaSO 4 + 2KNO 3

51. Reaction Rates Affected by: – Temperature – Surface area – Add a catalyst (does not change amount of product)

Buoyancy (Archimede’s Principle) Bernoulli’s Principle Pascal’s Principle Heterogeneous Mixture Homogeneous Mixture Kinetic Theory Charles’s law Boyle’s Law

Exam Group Names Symbols (S, l, g, & aq)