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Transcript
PAP FALL SEMESTER EXAM REVIEW 2012 KEY Explain the difference between each pair of terms. 1. Pure substances vs. mixtures a. Pure substance – substance that has a fixed (non-changing) composition with the same properties and characteristics in every sample (elements and compounds) b. Mixtures – substance that has a variable (changing) composition made up of two or more types of matter 2. elements vs. compounds a. element – pure substance made up of only one type of atom (anything on the periodic table) b. compounds – substance that is made from the chemical combination of two or more different types of atoms 3. physical properties vs. chemical properties a. physical – a characteristic that can be observed or measured without changing the identity of the substance b. chemical – the ability of a substance to undergo a change that transforms it into a different substance 4. extensive vs. intensive properties a. extensive – property that depends on the amount of matter present b. intensive – property that depends on the identity of the substance 5. 6. Classify changes of matter as physical or chemical. ____P____ A piece of metal is heated until it turns red. ____C____ Aluminum and oxygen react to produce aluminum oxide. ____C____ An iron nail rusts. ____P____ A piece of copper metal is hammered into a thin sheet. ____P____ An ice cube melts. ____C____ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. ____P____ Magnesium chloride is dissolved in water Define the following terms. atomic number – number of protons in an atom (also number of electrons in neutral atom) mass number – sum of protons and neutrons in the nucleus of an atom average atomic mass – average mass of all naturally occurring isotopes of an atom (on the periodic table) isotope – atoms of the same element with different mass numbers (same protons, different neutrons) ion – an atom with a charge (uneven amount of protons and electrons) valence electrons – electrons in the outer shell of the atom (used in chemical bonding) Octet Rule – atoms gain, lose and share electrons to get 8 valence electrons (full outer shell) electronegativity – the ability of an atoms to pull electrons towards itself in a bond ionization energy – energy required to remove a valence electron atomic radius – the size of an atom 7. Arrange each group of elements in order of increasing ionization energy. a. F, Br, I, Cl I BrClF b. Ga, Al, Tl, B TlGaAlB c. Al, Si, Cl, S AlSiSCl 8. For each group of elements, choose the element with the smallest atomic radius. a. Na, Li, K, Fr Li b. Tc, Rh, Zr, Y Rh c. Hf, Cs, Pb, Pt Pb 9. For each group of elements, choose the element with the greatest electronegativity. a. He, Rn, Xe, Ar b. As, N, P, Bi He c. Ba, Hf, Os, Hg N Hg 10. In general, ionization energies of the elements increase across each period and generally decrease down each group. 11. In general, electronegativities of the elements increase across each period and generally decrease down each group. 12. In general, the atomic radii of the element increases down a group and decreases across each period. 13. The atomic radii of group 3 elements are generally larger than the atomic radii of group 6 elements. 14. The atomic radii of period 2 elements are generally smaller than the atomic radii of period 6 elements. 15. The modern periodic table is arranged according to increasing atomic number. 16. Label the number of valence electrons for each group: 1 __1__ 2___2___ 13___3___ 14 __4___ 15 __5___ 16 ___6___ 17 ___7____ 18 ___8___ 17. Elements in the same family have similar characteristics/properties. 18. List group numbers or describe the location of each of the following groups of elements. 19. Contrast the properties of metals and nonmetals. Explain the location of each on the periodic table. • Metals - Properties: • Properties: – lustrous (shiny) – Dull appearance – good conductors of heat & electricity – Brittle when solids – malleable & ductile – Do not conduct heat or electricity well – solids at RT (except Hg) – May be solid, liquid or gas at RT 20. Identify the location in the atom, mass, charge, and volume for each of the subatomic particles a. proton – nucleus, 1 amu, +1, no volume b. neutron - nucleus, 1 amu, no charge, no volume c. electron – electron cloud, 0 amu, -1, all volume of the atom 21. Describe the experiments and their conclusions for: a. JJ Thompson - used the cathode ray tube to discover the 1st subatomic particle - the electron b. Ernest Rutherford - gold foil experiment - expected all of the radiation to pass through and was very surprised when some of the particles were deflected - led to the discovery of the NUCLEUS and the theory of the nuclear atom. Also discovered the proton. 22. Sketch the evolution of the atomic model. Include the name of the model and the scientist associated with it. Thomson's Plum Pudding Rutherford Bohr Modern Electron Cloud 23. An element consists of three naturally occurring isotopes with the following mass numbers: 24, 25 and 26. The relative abundances of these three isotopes are 78.70, 10.13 and 11.17 percent respectively. Calculate the average atomic mass and identify the element. Show your work! (24.32 amu) (24 x .7870) + (25 x .1013) + (26 x .1117) 24. A naturally occurring element, X, exists as 92.21% 28X, which has an atomic mass of 27.97693 amu, 4.70% 29X, which has an atomic mass of 28.97659 amu, and 3.09% 30X, which has an atomic mass of 29.97376amu. Calculate the average atomic mass and identify the element. Show your work! (28.11 amu) (28 x .9221) + (29 x .0470) + (30 x .0309) 25. Complete the following chart. Isotope Name Carbon-13 Nitrogen - 17 Boron - 5 Francium -223 Nuclear Symbol Atomic Number Mass Number # of Protons # of Neutrons # of Electrons 6C 6 13 6 7 6 N 7 17 7 10 7 5B 5 11 5 6 5 87Fr 87 223 87 136 87 13 17 7 11 223 26. The electron configuration s2p6 represents a. A halogen b. A metalloid c. A noble gas Write the complete electron configuration, Noble gas configuration, orbital notation, dot diagram, and quantum numbers for the following elements. 27. Selenium (Se) – number of electrons _______34____________ complete e – configuration: 1s22s22p63s23p64s23d104p4 Noble gas notation: [Ar]4s23d104p4 Dot diagram: All orbitals full with arrows in opposite directions through 3d Orbital notation: 1s ___ 2s___2p___ ____ ____3s___3p___ ____ ___4s___3d___ ___ ___ ___ ___4p___ ___ ___ Quantum numbers 4,1,-1,- ½ 28. Chromium (Cr) – number of electrons ________24___________ complete e – configuration: 1s22s22p63s23p64s23d4 Noble gas notation: [Ar]4s23d4 All orbitals full with arrows in opposite directions through 4s Orbital notation: 1s ___ 2s___2p___ ____ ____3s___3p___ ____ ___4s___3d___ ___ ___ ___ ___ Quantum numbers: 3, 2, 1, + ½ 29. Magnesium (Mg) – number of electrons _______12____________ complete e – configuration: 1s22s22p63s2 Noble gas notation: [Ne]3s2 Dot diagram: All orbitals full with arrows in opposite directions through 2p Orbital notation: 1s ___ 2s___2p___ ____ ____3s___ Quantum numbers: 3, 0,0, - ½ 30. Complete the following table about nuclear particles: Particle Charge Composition Penetrating Power (can be stopped by…) α +2 2 protons, 2 neutrons (helium nuclei) Paper, cloth β -1 Electron Wood, concrete 0 Electromagnetic waves Lead, 6ft concrete Symbol Alpha 4 2He, Beta 0 -1e, Gamma γ Balancing Nuclear Equations 31. 23994Pu + 10n 24094Pu 32. 10745Rh 10746Pd + 0-1e 33. 126 C+ 24496Cm 254102No + 210n 34. 42He + 2713Al 3014Si + 11H 35. 23892U + 10n 23992U 36. 115B + 25198Cf 259 103Lr + 310n 37. Define the following terms chemical bond – any force that holds two or more atoms together cation – positively charged ion (metals, lost electrons) anion – negatively charged ion (nonmetals, gained electrons) ionic bond – electrostatic attraction between cations and anions after a transfer of electrons covalent bond – two nonmetals sharing electrons metallic bond – pure metals bonding through the sea of electrons electron sea model – stationary metal nuclei release their valence electrons which are free to float between them all 38. Write names for the following compounds Sodium sulfate Na2(SO4) Ammonium sulfide (NH4)2S Barium phosphide Ba3P2 39. Write formulas for the following compounds. Sr(NO3)2 strontium nitrate P4Cl10 tetraphosphorus decachloride N3O7 trinitrogen heptoxide Cu(C2H3O2)2 copper (II) acetate Lead (IV) hydroxide Pb(OH)4 Tin (II) hydroxide Sn(OH)2 Iron (II) carbonate Fe(CO3) Carbon dioxide CO2 Cd(NO3)2 Li2CO3 Zn3(PO2)2 cadmium nitrate lithium carbonate zinc hypophosphite 40. Differentiate between fission and fusion reactions. Fission splits a large nucleus into smaller nuclei. Fusion combines two small nuclei into one larger one. 41. Briefly describe what happens that allows you to see colors in the flame tests and the gas tubes. When energy is added to an atom, an electron jumps to a higher energy level (excited state). It does not stay in the excited state for long, so as it falls back to its original location (ground state), it releases energy in the form of electromagnetic radiation which based on energy, frequency and wavelength will show as a different color. 42. What is the energy of a quantum of light with a frequency of 4.31 X 1014 1/s or Hz? (2.86 x 10-19 J) E = hv = (6.63 x 10-34 Js)( 4.31 X 1014 Hz) 43. A certain violet light has a wavelength of 413 nm. What is the frequency of the light? (7.26 x 1014 Hz) c = vλ v = c/λ = (3.0 x 108 m/s) / (413 x 10-9 m) 44. What is the energy of light with a wavelength of 662 nm? (3.00 x 10-19 J) c = vλ v = c/λ = (3.0 x 108 m/s) / (662 x 10-9 m) = 4.53 x 1014 Hz E = hv = (6.63 x 10-34 Js)( 4.53 X 1014 Hz) 45. For each substance listed below draw the Lewis structure, determine the geometric shape, and polarity. H2S bent (104.5°) polar SiF4 tetrahedral (109.5°) nonpolar PH3 trigonal pyramidal (107°) N2 linear (180°) NO2- bent (104.5°) SO3 trigonal planar (120°) polar nonpolar polar nonpolar 46. For sodium sulfate, calculate the percent composition of each element. (32.4% Na, 45.1% O, 22.6% S) 47. How many moles are in 30g of NaCl? (0.5 moles) 48. How many molecules are in 3.00 moles of KCl? (1.81X1024 molecules) 49. What is the empirical formula for a compound which contains 67.1% zinc and the rest is oxygen? (ZnO2) 50. If the empirical formula of a compound is CH and the molecular mass is 78.12g/mol, what is the molecular formula? 51. How many grams are in 5 moles of H2O? (90 grams)