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CP Chemistry Mid-Term Exam Review Sheet - 2015 I. Vocabulary Chemistry matter units metric system length / meter mass / kilogram time / second volume density chemical property physical property malleability ductility conductivity reactivity phase state solid liquid gas melting / freezing evaporating / condensing mixture solution substance homogeneous heterogeneous element compound atom molecule formula unit diatomic elements nucleus isotope energy frequency wavelength light electromagnetic waves photons quantized subatomic charge neutron proton electron ion cation anion polyatomic symbol atomic number atomic mass mass number radiation radioactivity stable background radiation nuclide decay emission , , and bombardment half-life fission chain reaction nuclear fission reactor reaction vessel fuel rods control rods fusion nuclear fusion reactor radioisotopes tracers quantum numbers n, l, m, s energy level orbital shape orientation spin electron configuration triads octaves period metal non-metal metalloid group / family period alkali metals earth alkali metals transition metals rare earth metals halogens noble gases subscript formula element compound ionic covalent hydrocarbon isoelectronic atomic radius ionic radius electronegativity mole Avogadro’s number molar mass percent composition hydrate reaction equation law of conservation of mass and energy system surroundings reactant product yield aqueous synthesis combustion decomposition dissociation dissolve single displacement activity series double displacement solubility precipitate net ionic equation spectator ions mole ratio stoichiometry II. Lists Greek Prefixes for the Metric System Prefix Abbreviation Factor megakilodecicentimillimicronanopico- M K d c m n p 106 103 10-1 10-2 10-3 10-6 10-9 10-12 Polyatomic Ions - (see sheet) Greek Prefixes for covalent compounds Prefix Number monoditritetrapentahexaheptaoctanonadeca- One Two Three Four Five Six Seven Eight Nine Ten Prefix Number methethpropbutpenthexheptoctnondec- One Two Three Four Five Six Seven Eight Nine Ten Prefixes for hydrocarbons People Atomic Theory Democritus Dalton Thomson Rutherford Chadwick Bohr Atomic Models solid sphere model plum pudding model nuclear / planetary model revised planetary model Bohr atom modern atom Periodic Table Dobereiner Newlands Mendeleev Moseley Ramsay III. Problems A. Mathematics 1. Scientific Notation exponents: positive exponent - move decimal to the right eg. 3.78x104 = 37,800 negative exponent - move decimal to the left eg. 3.78x10-4 = 0.000378 operations: addition and subtraction - exponents must be the same; keep exponent eg. 1.2x105 + 3.4x105 = 4.6x105 multiplication - add exponents eg. (6.0x107)(8.0x109) = 48x1016 division - subtract exponents eg. 3.6x109 / 1.2x104 = 3.0x105 Sample Problems 1. Convert to or from scientific notation. a. 0.00003 = b. 65,000 = d. 0.0017x109 = Calculate. a. 6.5x102 + 2.0x103 = b. 7.8x105 - 5.5x104 = (4.0x10-2)(3.0x104) = d. 12x10-6 / 4x102 = c. c. 2. 480x10-2 = Units addition and subtraction - units must be the same eg. 1.2x105 dm + 3.4x106 cm = 1.2x106 cm + 3.4x106 cm = 4.6x106 cm multiplication and division - units do not have to be the same but they may cancel eg. (7.8x10-14 s-1)(9.0x108 J.s) = 70x10-6 J Sample Problems 4.8x10-3 L + 3.7x101 mL = (80 km/hour)(4 hours) = B. Symbols atomic number - number of protons (and number of electrons in a neutral atom) the atomic number is the “fingerprint” of an element atomic mass - mass of a mole of atoms of an element (weighted to include isotopes) mass number - number of protons and neutrons in the nucleus isotopes - atoms of the same element with different numbers of neutrons (and different mass numbers) mass number 40 atomic number 20 symbol: Ca atomic symbol: Ca-40 - the symbol for the element just the symbol for the element and the mass number use the periodic table to find the atomic number Sample Problem How many protons, neutrons and electrons are in Cu-64? Write the symbol for this isotope of copper. C. Nuclear Chemistry 1. Balancing nuclear equations a. balance mass number and atomic number separately b. assign element symbol eg. 238 U 4He + 234Th 2. Half-life amount of sample remaining after n half-lives = (1/2)n eg. How many grams of a 1.5-mol sample of Mo-91 remain after one hour and 2 minutes if the half-life of Mo-91 is 15.5 minutes? Amount of sample remaining = (1/2)4 (1.5 moles) (91 grams/mol) = 8.5 grams Mo-91 Sample Problems 1. Balance the following and label the parent, daughter, and particle emitted or absorbed. a. 0 227 _____ e + Ac -1 b. 27 1 n Al + 13 c. 27 4 Al + 13 _____ 0 He 2 1 _____ + n 0 2. How many moles of a 125-gram sample of Cl-39 remain after 166.5 minutes if the half-life of Cl-39 is 55.5 minutes? D. Electrons 1. Quantum Numbers n = Principal Quantum Number - energy level l = orbital (shape) l=0 s 1 p 2d 3f m = orientation for p orbitals, x, y, and z for d orbitals, x2-y2, xz, yz, xy, and z2 for f orbitals, x(y2-z2), y(x2-z2), z(x2-y2), etc. s = spin Eg. For an electron in the n = 4 energy level, l= 0 or s 1 or p 2 or d m= 0 -1, 0, +1 -2, -1, 0, +1, +2 s = +1/2 and -1/2 for each m 2. Symbolism n=1 l = 0 (n-1) m = -l…0…+l s = +1/2 or -1/2 3 or f -3, -2, -1, 0, +1, +2, +3 nlm eg. For an electron with the quantum numbers n = 2, l =1, m = +1, s = +1/2, the symbol would be 2px or 2py or 2pz. For an electron with the quantum numbers n =2, l=1, m = -1, s = +1/2 the symbol would be 2px or 2py or 2pz but different from the previous symbol. Sample Problems What are all of the possible sets of quantum numbers for electrons in the n = 3 energy level? Write the symbol for an electron with the quantum numbers n = 3, l = 2, m = -2, s = +1/2. Write the symbol for an electron with the quantum numbers n = 3, l = 2, m = -1, s = +1/2. Write the symbol for an electron with the quantum numbers n = 3, l = 2, m = -1, s = -1/2. E. Periodic Trends atomic radius - increases down and to the left ionic radius - depends on whether the ion is positive or negative same number of protons, the positive ion is smaller same number of electrons, the positive ion is smaller electronegativity - increases up and to the right (noble gases = 0) Sample Problems Write the following in increasing order atomic radius : Al, Cl, P ionic radius : Br-, Kr, Se-2 F. electronegativity: F, N, O Chemical Formulas 1. Be, Ca, Mg Br-, Cl-, FK, Na, Rb Writing formulae a. Ionic Compounds monatomic ions: Group 1 : +1 Group 2 : +2 Group 3 : +3 Group 15 : -3 Group 16 : -2 Group 17 : -1 transition metals : use ion sheet or use Roman numerals polyatomic ions : use ion sheet Opposites attract : the positive or more metallic ion goes first when writing the formula The farther to the left on the periodic table, the more metallic. When writing a compound’s formula, write the ions’ symbols with the charge. If the charges add up to zero, then just put the symbols together to form the formula. If the charges do not add up to zero, switch the charges and reduce. Example: Make a compound from acetate and calcium. Calcium goes first because calcium is positive. +2 + -1 = 1 since 1 does not equal 0, switch the charges… Ca(C2H3O2) 2 !!! (use parentheses for polyatomic ions) b. Transition metals The Roman numeral indicates the charge on the metal. Example: cerium (IV) sulfate Ce+4 SO4-2 so 2 sulfate ions are needed to cancel the charge on cerium Ce(SO4)2 c. Covalent compounds Use prefixes to determine the number of atoms of each element. Example: silicon tetrafluoride No prefix means one atom of silicon and tetra- means 4 atoms of fluorine. SiF4 d. Hydrocarbons Use the prefix to find the number of carbon atoms. Use the suffix to calculate the number of hydrogen atoms. -ane : 2n+2 -ene : 2n -yne : 2n-2 Example: propyne prop- means 3 carbon atoms, -yne means double the carbons and add 2. C3H4 2. Naming Compounds a. Ionic: Metal + Non-metal / polyatomic The name of the metal comes first. Do not change the name. The name of the non-metal goes last. If the non-metal is monatomic, change the ending to “-ide”. If the non-metal is polyatomic, just use its name. Eg. CaCl2 - calcium chloride the metal is calcium so it keeps its name the non-metal, chlorine, is monatomic, so it changes its ending to “-ide” b. Transition metals These are the ones that are on the polyatomic ion sheet and have weird names. The same rules go for the non-metal ( “-ide” or stay the same) The metal can either be the weird name that goes with the charge or The metal can keep its element name and simply take Roman numerals indicating its charge. Eg. FeCrO4 CrO4 is chromate. Fe can be ferrous (if its +2) or ferric (if its +3). CrO 4 has a charge of -2. No subscripts, so Fe must be +2 ferrous chromate or iron (II) chromate c. Covalent: Non-metal + Non-metal The more metallic element (closest to the metal/non-metal line) goes first. The first non-metal keeps its name. The non-metal changes its ending to “-ide”. Add a Greek prefix to both to indicate how many atoms of each element are used. (drop mono- if there is only one atom of the first non-metal) Eg. NO2 - nitrogen and oxygen. Nitrogen is more metallic so it goes first. Oxygen becomes oxide. One nitrogen and two oxygens. mononitrogen dioxide - drop the mono that comes first nitrogen dioxide d. Hydrocarbons The prefix comes from the number of carbon atoms. The suffix comes from number of hydrogens compared to the carbon atoms. Eg. C5H12 pent- is the prefix used for 5 carbons. -ane is the suffix when the number of hydrogens is double the number of carbons plus 2 pentane Sample Problems Name the following compounds. a. KI b. SO3 c. PbSO4 d. HBr e. C6H10 f. BaS Write the formulae for the following compounds. a. ammonium sulfide b. dinitrogen monoxide c. tin (II) nitrate d. butyne e. chromium cyanide f. ferrous carbonate G. Moles 1. avogdro’s Number - NA - the number of particles in one mole of a substance 1 mole = 6.02x1023 atoms, molecules, or formula units 2. molar mass - atomic mass on the periodic table gives you the mass (in grams) per 1 mole! Eg. Na2CO3 3. 2 Na = 46 g C = 12 g 3O = 48 g 106 g Na2CO3 1 mole Na2CO3 percent composition - add up the total molar mass of the compound. Then take the mass of each element divided by the total mass times 100. Sample Problems 1. How many moles are in 1.3x1024 atoms of Mg? 2. What is the mass of 3.8 moles Ba(NO3)2? 3. What is the percent composition of NaHCO3? H. Reactions and Equations 1. law of conservation of matter Equations must be balanced! 2. 5 types of reactions: A + B AB more than one reactant one product Eg. 2K + Cl2 2KCl a. synthesis 2A + O2 2AO synthesis with oxygen as one of the reactants Eg. 2Na + O2 2NaO b. combustion c. decomposition AB A + B one reactant breaks into more than one product Eg. H2CO3 CO2 + H2O d. single displacement A + BC AC + B an element plus a compound yields an element and a compound Careful! Check your activity series. The reactant that is an element must be stronger than the ion it’s replacing! eg. Cu + 2AgNO3 Cu(NO3)2 + 2Ag 2Ag + Cu(NO3)2 No Reaction! e. double displacement AB + CD AD + CB two compounds react to form two compounds Remember that a compound is made of a positive and a negative! Look for a precipitate on the products side. eg. H2SO4 + BaCl2 BaSO4 (pr) + 2HCl dissociation AB A+ + Bone reactant dissolves in water into its ions eg. NaCl Na+ + Clnet ionic equation eg. Calcium acetate reacts with potassium sulfate. 1. Write the overall equation. Ca(C2H3O2)2 + K2SO4 ----> 2KC2H3O2 + CaSO4 2. Write soluble compounds in ionic form. Ca+2 + 2C2H3O2- + 2K+ + SO4-2 ----> 2K+ + 2C2H3O2- + CaSO4 3. Cancel species that appear on both sides. Ca+2 + 2C2H3O2- + 2K+ + SO4-2 ----> 2K+ + 2C2H3O2- + CaSO4 4. Write the resulting equation. Ca+2 + SO4-2 ----> CaSO4 Sample Problems Balance and classify the following reactions: a. AgNO3 + KCl KNO3 + b. Al + O2 Al2O3 c. Sn + Cl2 SnCl4 d. Mg(OH)2 e. Fe + f. H3PO4 Mg+2 + Cu(C2H3O2)2 P2O5 + AgCl OH-1 Fe(C2H3O2)2 + H2O Write the net ionic equation for the following equation. Iron (III) bromide reacts with ammonium sulfide. Cu I. Stoichiometry Write the balanced equation. Start with what you are given. Always go through moles and the mole ratio! Don’t stop until you find what you were looking for. Sample Problems Copper (II) sulfate reacts with sodium sulfide to produce copper (II) sulfide and sodium sulfate. a. How many moles of sodium sulfate are formed from 0.3 moles of sodium sulfide? b. How many grams of copper (II) sulfate are needed to react with 20.3 grams of sodium sulfide?