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(A) (B) (C) (D) (E)
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Questions on this chapter are incorporated into the chapters concerning the specific experiments
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84 If 75% of a sample of pure 3 H decays in 246 yr, 1 what is the half-life of 3 H 1 (A) (B) (C) (D) (E) 246 yr 184 yr 123 yr 615 yr 307 yr
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1 D The others form anions 2 B Decreasing radii for increasing charges, or for going up a column (with equal charges), or moving towards the right in a period of the periodic table (Note: This explanation would not be sufficient for the free response portion of the test) 3 C The element that is furthest from F
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3+ 4 E Hexaammine = (NH3)6; cobalt(III) = Co ; and nitrate = NO3
15 A H2C2O4 is the limiting reagent 2 mol MnSO 4 ( 25 mol H 2C 2O 4 ) 5 mol H 2C 2O 4 16 A (0400 mol Ba)(l mol H2/l mol Ba) (224 L/mol)
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17 E This is an application of Charles s law 18 D The heavier gas is moving more slowly 19 E The basic difference between ideal and real gases 20 D (135 g Al)(1 mol Al/270 g Al) (3 mol H2/2 mol Al)(224 L/mol H2) 21 A The mole fraction of CO times the total pressure yields the partial pressure The mole fraction of CO is the moles of CO divided by the total moles 22 A n = PV/RT = (0993 atm)(0237 L)/ (00821 L atm/K mol)(373 K) 3 = 769 10 mol
3 molar mass = 0548 g/769 10 mol = 713g/mol
5 D This was determined by bombarding gold foil with alpha particles
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6 A All others, except D, are Lewis bases D is neither a Lewis acid nor a Lewis base 7 A 3 Mn(OH)2(s) + 2 H3AsO4(aq) Mn3(AsO4)2(s) + 6 H2O(l) 8 E PbSO4 forms 9 A [Cu(NH3)4] forms 10 C Fe(OH )3 forms 11 D Ca(OH)2, NaOH, and Na2CO3 are strong electrolytes and should be separated Cancel all + spectator ions (Na and OH ) 12 C The hydroxide took some of the iron with it, 2+ so Fe will be low The nitrate is double the potassium because there are two nitrates per iron(II) nitrate instead of one, as in potassium hydroxide
23 A The molar mass of the gas must be the square of the molar mass of helium
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24 E Definition 25 C Basic postulate of kinetic molecular theory 26 A One of the properties of free energy 27 B Definition 28 B [2 ClF(g)+O2 ( g ) Cl 2O(g)+OF2 (g )]
1 2 1
(1675 kJ) ( 435 kJ)
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13 C (01000 mol Cr2O72 /1000 mL) (4520 mL) 2+ 2 (6 mol Fe /1 mol Cr2O7 )(1/7500 mL) (1000 mL/L) 14 E Percent Mn in each oxide: (A)774; (B) 696; (C) 720; (D) 632; (E) 495
[ 2F2 ( g ) + O2 ( g ) 2OF2 ( g )]
[Cl 2O(g)+3 OF2 (g ) 2 ClF3 ( l ) + 2 O2 ( g )]
1 2 (3941 kJ) 1351 kJ
ClF(g) + F2(g) ClF3(l)
28 U STEP 2 Determine Your Test Readiness
29 C The one with the greatest increase in the moles of gas 30 D Nonspontaneous means G > 0 Becoming spontaneous at lower temperature means H < 0 and S < 0
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47 D Both graphite and diamond are covalentnetwork solids 48 A Calcium is a metal, and answer A applies to metallic bonding 49 C Calcium carbonate is ionic 50 B This is a polar molecule 51 D Definition 52 D This is a consequence of metallic bonding 53 C The carbonyl and OH groups are capable of participating in hydrogen bonds 54 C The more OH groups, the more hydrogen bonding, and the more soluble in water 55 B Definition
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31 C Atoms with completely filled shells or subshells are not paramagnetic These are: Be, Mg, He, Kr, and Zn 32 C Transition metal ions are s C could be Cr 33 E Noble gases, except helium, are ns np In this case, n = 4 34 D Halogens are ns np In this case, the halogen is F 35 A The 1p orbital does not exist 36 D Definition 37 E The electrons enter the 2p orbitals individually 38 A Definition 39 B The d orbitals are less effectively shielded than the s orbitals
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