molecular molecular ionic molecular ionic other molecular molecular e 20 e H N Cl 42 e N Cl Cl trigonal pyramid polar

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Homer York
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1 1. a. lassify each of the following as molecular, ionic or other. 2 l 2 2 K Nl 2 MgS 4 Xe P 3 l a. b. Show the Lewis structure of each substance you classified as molecular. or ionic compounds, write charges on the cation and anion. c. Give the total number of electrons in each compound. d. Draw and name the VSEPR shape for molecular compounds. e. Indicate whether the substance is or non. f. Name the dominant intermolecular force in each substance. g. Place the compounds in order of increasing predicted melting point. molecular molecular ionic molecular ionic other molecular molecular 1 4 e 2 14 e 2 l 14 e 32 e l l b., c., d., e. l 58 e l tetrahedral l l 1 4 e 2 12 e 16 e 22 e linear non e 1 N 5 e 1 1 e 2 l 14 e 20 e N l l 42 e N l l trigonal pyramid N l l e 54 e non 1 P 5 e 3 21 e 26 e P 42 e P trigonal pyramid P 1 1 e 1 6 e 1 l 7 e 14 e 26 e l l bent (109.5 o ) l f. dipoledipole g. London ion-ion -bond ion-ion London dipoledipole -bond 2 Xe P 3 2 l 4 l Nl 2 K MgS 4

2 2. a. lassify each of the following as molecular, ionic or other. 4 Se 4 NaB 4 2 N as Ar S 3 a. b. Show the Lewis structure of each substance you classified as molecular. or ionic compounds, write charges on the cation and anion. c. Give the total number of electrons in each compound. d. Draw and name the VSEPR shape for molecular compounds. e. Indicate whether the substance is or non. f. Name the dominant intermolecular force in each substance. g. Place the compounds in order of decreasing predicted boiling point. molecular molecular ionic molecular ionic other molecular molecular 1 4 e 4 28 e 32 e b., c., d., e. 42 e tetrahedral non f. London g. 1 Se 6 e 4 28 e 34 e Se 70 e Se see-saw Se dipoledipole e 1 N 5 e 3 3 e 1 6 e 14 e N 18 e N N trigonal pyramid bent N e 18 e non 1 S 6 e 3 18 e 24 e S 40 e S trigonal planar S non 1 1 e 1 6 e 1 l 7 e 14 e 18 e both bent (109.5 o ) ion-ion -bond ion-ion London London -bond as NaB 4 2 N Se 4 4 S 3 Ar

3. lassify the following solids as molecular, network (covalent), metallic, ionic or atomic. a. benzene, molecular b. diamond network c. krypton atomic d. d metallic e. copper(ii) chloride ionic f.

or the two dimensional arrays shown below, draw a set of lattice points, a single primative unit cell and a centered unit cell. 5. ow many whole atoms are in a primitive cubic unit cell? 1 6.

3 3. lassify the following solids as molecular, network (covalent), metallic, ionic or atomic. a. benzene, molecular b. diamond network c. krypton atomic d. d metallic e. copper(ii) chloride ionic f. ice molecular g. S 8 molecular h. Mg 3 (P 4 ) 2 ionic i. quartz (Si 2 ) network j. P 4 molecular 4. or the two dimensional arrays shown below, draw a set of lattice points, a single primative unit cell and a centered unit cell. 5. ow many whole atoms are in a primitive cubic unit cell? 1 6. ow many whole atoms are in a body-centered cubic unit cell? 2 7. ow many whole atoms are in a face-centered cubic unit cell? 4 8. Polonium crystallizes in a sc unit cell with a density of 9.20 g/cm 3. alculate the radius of a Po atom. 209 g Po 1 mole Po 1 atom Po 1 cm 1 mole Po x 10 atoms Po 1 unit cell 9.20 g Po x x x x 10 cm V a V x 10 cm x 10 cm 8 a x 10 r 1.68 x 10 8 cm = 1.68 Å 2 2

9. opper crystallizes in a fcc unit cell, and has an atomic radius of 128 pm. alculate the density of copper. 63.546 g u 1 mole u 4 atoms u 1 mole u 6.

7453 x 10 23 cm 3 mass of unit cell 22 4.2209 x 10 g/unit cell volume of unit cell 23 3 4.7453 x 10 cm /unit cell density = = = 3 8.89 g/cm 10.

4 9. opper crystallizes in a fcc unit cell, and has an atomic radius of 128 pm. alculate the density of copper g u 1 mole u 4 atoms u 1 mole u x 10 atoms u 1 unit cell 22 x x = x 10 g/unit cell 23 8 a 2 4r 4(1.28 x 10 cm) 8 r = ; a = = = x 10 cm V = a 3 = ( x 10 8 cm) 3 = x cm 3 mass of unit cell x 10 g/unit cell volume of unit cell x 10 cm /unit cell density = = = g/cm 10. The radius of iron is 124 pm, and it crystallizes in a bcc unit cell, what is the volume of the unit cell. a 3 4r 4(124 pm) r = ; a = = = pm V = a 3 = ( pm) 3 = 2.35 x 10 7 pm or the heating curve below:

5 Temperature (o) a. (name of the energy) fusion b. (name of the energy) vaporization c. Temperature ( o ) d. eat (J) e. (name of phase change) melting f. (name of phase change) boiling 12. alculate the energy released when g of 2 3 goes from 0.0 o to 75.0 o. normal mp 2 3 (s) normal bp 2 3 (l) vaporization 2 3 (l) s 2 3 (l) s 2 3 (g) o 26.6 o kj/mole J/g o J/g o eat (J) q = mst = g x J/g o x ( o ) = J 2. = J/mole x g x 1 mole/ g = J 3. q = mst = g x J/g o x ( 75.0 ( 26.6 o )) = J q total = ( J) + ( J) + ( J) = J = kj

6 13. Given the phase diagram of xenon, Xe, answer the following: a. Estimate the normal boiling point of xenon. 107 o b. Estimate the normal melting point of xenon. 112 o c. Estimate the vapor pressure of Xe(l) at 110 o. 0.8 atm d. Is Xe(l) or Xe(s) more dense? Explain. Xe(s), the mp line slopes to the right. 14. alculate the difference in solubility of nitrogen (mole fraction in air = 0.78) in blood at sea level (P = 1.0 atm) versus 10 m underwater (P = 2.0 atm). Assume that blood is identical to water and k N2 = 7.0 x 10 4 mole/l atm. N2 = kp N2 = 7.0 x 10 4 mole/l atm x (1.0 atm x 0.78) = 5.5 x 10 4 M N 2 N2 = kp N2 = 7.0 x 10 4 mole/l atm x (2.0 atm x 0.78) = 1.1 x 10 3 M N alculate the concentration of oxygen gas in water at sea level and 1.00 atm. The partial pressure of oxygen gas is 0.21 atm and enry s constant for oxygen (in water at RT) is 1.3 x 10 3 M atm 1. 2 = kp 2 = 1.3 x 10 3 mole/l atm x (1.00 atm x 0.21) = 2.7 x 10 4 M Is solid iodine (I 2 ), more soluble in benzene (see #3), or chloroform, 3 l? benzene; I 2 is non and so is benzene

7 17. lassify the following as molecular or ionic. What is the value of i for each when dissolved in water? a. copper(ii) chloride ul 2, ionic, i = 3 b. 3 molecular, i = 1 c. Mg 3 (P 4 ) 2 ionic, i = 5 d. sucrose, molecular, i = 1 e. benzene, 6 6 molecular, i = A solution is prepared by dissolving 5.00 g of glucose, , in g of water. alculate: a. the vapor pressure of water at 90 o. The vapor pressure of pure water at 90 o is torr. 1 mole g x g 2 = mole mole g x g x g g 2 P sol n = water P o water = (0.995)(525.8 torr) = torr b. the boiling point of the solution. 1 mole g x g = m kg 2 T b = i K b m = (1)(0.52 o /m)( m) = 0.14 o higher T b = o o = o 19. a. alculate the freezing point of a solution of 2.00 moles of Nal in ml of water (density of water = 1.00 g/ml) mole Nal kg 2 = 20.0 m Nal T f = i K b m = (2)(1.86 o /m)(20.0 m) = 74.4 o lower T f = 0.0 o 74.4 o = 74.4 o

8 b. alculate the freezing point of a solution of 2.00 moles of al 2 in ml of water mole al kg 2 = 20.0 m al 2 T f = i K b m = (3)(1.86 o /m)(20.0 m) = 112 o lower T f = 0.0 o 112 o = 112 o

General Chemistry II Worksheet #2 Intermolecular interactions, properties of liquids and solids Dr. Brosius

General Chemistry II Worksheet #2 Intermolecular interactions, properties of liquids and solids Dr. Brosius General hemistry II ame: Worksheet #2 Intermolecular interactions, properties of liquids and solids Dr. Brosius 1 Rank these hydrocarbons, pentadecane, pentane, octadecane 1532, 512, 1838 in terms of increasing: