Practice Chem-is-try

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  Bonding Practice

1.  Draw the dot diagrams for each of the following and use the dot diagram to answer questions 1-15. 

a.  CBr4

b.  SO3

c.  H2O

d.  HCN_

e..C2H2

f.  CO2

 

1-5 match the shape of each molecule.

A.  linear

B.  tetrahedral

C.  pyramidal

D.  bent

E.  trigonal planar

 

1.  Molecule a  _____________                                 

                                                                                   

2.  Molecule b  ____________          

                                                                                                           

3.  Molecule c  _____________

                                   

4.  Molecule d  ____________

 

5.  Molecule f  _____________

 

6-10  match the type of intermolecular force to each molecule

A.  hydrogen bond

B.  London forces

C.  dipole/dipole

 

6.  Molecule a  _____________                                 

                                                                                   

7.  Molecule b  ____________                                  

                                                                                   

8.  Molecule c  _____________                                 

 

9.  Molecule e  ____________

 

10.  Molecule f  _____________

 

11-15 determine the molecular polarity of each molecule

A. polar

B.  nonpolar   

 

11.  Molecule a  _____________                                                                                                                   

12.  Molecule b  ____________                                                                                                                    

13.  Molecule c  _____________                               

 

14.  Molecule d  ____________

 

15.  Molecule f  _____________

 

_____ 16. MgF2 is a compound which demonstrate

A.   A covalent bond which involves the transfer of electrons thus creating ions which are attracted to each other.

B.  An ionic bond which involves the transfer of electrons thus creating ions which are attracted to each other

C.  An attractive and repulsive forces between electrons of one atom and the protons of another atom.

D.  An attractive and repulsive forces between electrons and protons within the same atom.

 

_____ 17. In both ionic and covalent bonds:

A.  Only the outer shell electrons of the atoms are involved in the bonding process

B.  All the electrons of the atoms are involved in the bonding process.

 

_____ 18. A bond between carbon and oxygen is a (an)

A.  Polar covalent bond in which the electrons are shared unequally and are more attracted to the oxygen atom.

B.  Polar covalent bond in which the electrons are shared unequally and are more attracted to the carbon atom.

C.  An ionic bond which involves the transfer of electrons thus creating ions which are attracted to each other

D.  A metallic Bond

 

_____19.  Which of the following care polar molecules?

 A..  CO2

B.  CO

C.  H2O

D.  CF4

 

For 20 –25 match each substance to the type of bonds each substance contains.

A.  ionic bond

B.  polar covalent

C.  nonpolar covalent

D.  metallic

 

______20.  MgCl2                                        

                                                           

______21.  Fe

                                                                                               

______22.  PH3

 

______23.  N2

 

______24.  CaO

 

______25.  NH3

 

 

SOLUTION
1. The dissolution process is exothermic if the amount of energy released in bringing about a interactions exceeds the sum of the amounts of energy absorbed in overcoming b and c interactions.
                    a                       b                         c
a) solute-solute/ solvent-solvent/ solvent-solute
b) solvent-solvent /solute-solute /solvent-solute
c) solvent-solute /solute-solute /crystal lattice
d) solute-solute/ crystal lattice /solvent-solvent
e) solvent-solute/ solute-solute /solvent-solvent
2. Consider the three statements below. Which numbered response contains all the statements that are true and no false statements?
I. Hydration is a special case of solvation in which the solvent is water
II. The oxygen end of water molecules is attracted toward Ca‚ ions.
III. The hydrogen end of water molecules is attracted toward Cl, ions.
a) I
b) II
c) III
d) I and II
e) I, II, and III
3. Which of the following terms is not generally used in describing the dissolution of solids and gases in liquids?
a) miscibility
b) saturation
c) molality
d) molarity
e) % solute by mass
4. Which numbered response lists all of the following statements that are true, and no false statements?
I. Many solids that dissolve in endothermic processes have solubilities that increase as temperature increases.
II. The solubility in water of a gas that does not react with water increases as the partial pressure of that gas above the surface of the solution increases.
III. Most gases that are reasonably soluble in water are polar or else they react with water or ionize in water.
a) I
b) II
c) I and II
d) II and III
e) I, II, and III
5. To calculate the molality of a solution, which of the following must be measured?
I. mass of solute       II. mass of solvent         III. total volume of solution
a) I and II
b) I and III
c) II and III
d) only I
e) I, II and III
6. Calculate the molality of a solution that contains 25 g of H2SO4 dissolved in 80. g of H20.
a) 16 m
b) 2.2 m
c) 3.2 m
d) 6.3 m
e) 7.0 m
7. Calculate the molarity of a solution that contains 9.0 g of (COOH)2 in 1500. mL of solution.
a) 0.067 M
b) 0.10 M
c) 0.13 M
d) 0.20 M
e) 0.26 M
8. Which of these aqueous solutions would be expected to have the highest boiling point?
a) 0.100 m CaCl2
b) 0.200 m NaOH
c) 0.050 m K2SO4
d) 0.050 m Al2(SO3)3
e) 0.200 m CH3OH
9. If 4.27 grams of sucrose, C12H22011,are dissolved in 15.2 grams of water, what will be the boiling point of the resulting solution? Kb for water = 0.512oC/m.
a) 101.64oC
b) 100.42oC
c) 99.626oC
d) 100.73oC
e) 101.42oC
10. Calculate the freezing point of a solution that contains 8.0 g of sucrose, C12H22011, in 100.0g of H20. Kf for H20. = 1.86oC/m.
a) -0.044oC
b) -0.22oC
c) -0.39oC
d) -0.44oC
e) 0.04oC
11. The freezing point of a solution made by dissolving 0.200 g of a molecular compound in 100. g of H20. is -0.0120oC. Calculate the molecular weight of the compound. The compound does not ionize in water. Kf for H2O = 1.86oC/m.
a) 155 amu
b) 215 amu
c) 310 amu
d) 395 amu
e) 450 amu
12. When 20.0 grams of an unknown compound are dissolved in 500. grams of benzene, C6H6, the freezing point of the resulting solution is 3.77oC. The freezing point of pure benzene is 5.48øC, and the Kf for benzene is 5.12oC/m. What is the molecular weight of the unknown compound?
a) 120 g/mol
b) 80.0 g/mol
c) 100 g/mol
d) 140 g/mol
e) 160 g/mol

13.  Which of the following does NOT behave as an electrolyte when it is dissolved in water?

a. CH3OH       

b. K2CO3        

c. NH4Br

d. HI

e. Sodium acetate, CH3COONa

14.  Which of the following is predicted to be soluble in water?

a.  Fe(OH)3

b.  AgCl

c.  CaCl2

d.  BaSO4

15.    In which set of compounds below are all the compounds insoluble in water?

a.  NaCl,   AgCl,   ZnCl2

b.  Na2CO3,   CaCO3,   (NH4)2CO3

c.  (NH4)2S,   FeS,   Na2SO4

d.  ZnS,   NiS,   CoCO3

16.  If you want to make a water-soluble salt using the zinc(II) cation, Zn2+, what anion would you choose?

a.  NO3-

b.  CO32-

c.  C2O42-

d.  PO43-

 

 

 

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