AP Chemistry                                                                 Unit 2

Chapter 2                                                                        Atoms, Molecules, and Ions               

Daily

 

Multiple Choice Questions

1. The mass of an apple, orange, grape and banana are 800, 750, 72 and 650 g, respectively. Determine the combined mass of 10 apples, 6 oranges, 20 grapes and 5 bananas.

A.  17190g

                     B. 8595 g

                     C. 2272 g

                     D. 95200g

 

2. The oxides of CO and CO2 must have the following carbon-to-oxygen mass ratio

 

               A.                  12:16, 12:32

                     B.           12:12, 12:16

                     C.           12:8, 12:4

                     D.           12:12, 12:24

 

3.       Every atom contains

 

                     A.           As many neutrons as electrons

                     B.           As many protons as neutrons

                     C.           As many nuclei as neutrons

                     D.           As many electrons as protons

 

4.       Which of the following elements has Z 68 and A 167?

                     A. Erbium

                     B. Californium

                     C. Calcium

                     D. Dysprosium

 

5.       Atom A has 30 protons, 32 neutrons and 30 electrons. Atom B has 30 protons, 28 neutrons, and 30 electrons. Atoms A and B are

A. Isotopes

B.  Isobars

C.  Isomers

D.  Isoneutrons

 

6.       How many total protons are found in two molecules of C20H300?

A. 102

B.  316

C.  302

D.  600

 

7.       What is the charge of an ion with 38 electrons, 38 neutrons and 35 protons?

A. 0

                                                B. +3

                                                                                     C.  -3

D.

 

8.        An ion has a charge of +3 and 55 electrons. Which of the following elements is that ion?

           A.Th                             B Ce                           C.Mn                          D.Co

 

9.        Atom A loses 1 electron and atom B gains 2 electrons. What formula results if these two ions combine to produce a neutral compound?

           A.AB                            B. A2B                                                            D.A2B3

 

10.     Which one of the following chemical symbols does not represent an element?

           A.SO                             B Gd                           CAm                           D.Au

 

11.     Which group of elements belongs to the Transition Metal family

           A.  Ru, C, Hg, Ir         B. Pd, Ir, Ac, Re       C. Bi, Sc, Pu, Rn      D. Ti, Sc, Au, Fr

 

12.     The (S04)-2 ion is called

           A.  Sulfite ion             B. Sulfate ion           C. Sulfur tetroxide ion D. Sulfur oxide

 

13.     The formula for iron(III) carbonate is

           A.  FeCO3                          B. Fe2(CO)3,              C. Fe2(CO3)3              D. Fe3(CO)3

 

14.     The ion SCN is named
           A.  Sulfocvano ion     B. Thiocyano ion     C. Cyano ion             D. Thiocyanate ion

 

15.     A compound in which the nitrite to metal ion ratio is 2:1 has the following formula

           A.  M(N02)2                       B. M(N02),                 C. M2N02                         D. MNO2

 

16.     The formula for hvdrosulfuric acid is

           A.  H2S                         B. H2S02,                   C. H2S04                           D. HSO3

 

17.     The name for (Br03-1) is

           A.  Bromite                 B. Perbromate         C. Bromate               D. Hypobromite

 

18.     The oxoacid HIO is named

           A.  Hypoiodous           B Iodic                       C. Iodous                   D. Periodic

 

19.                            What formula does ammonium perchlorate have?

A.NH3ClO3                             B. NH4ClO4                C. NH3ClO                D. NH3ClO2

 

 

Free Response Exercises

20.  In an exothermic (heat producing) reaction, chlorine reacts with 2.0200 g of hydrogen to form 72.92 g of hydrogen chloride gas. How many grams of chlorine reacted with hydrogen?

 

21.  Sulfur and oxygen can react to form both sulfur dioxide and sulfur trioxide. In sulfur dioxide, there are 32.06 g of sulfur and 32.00 g of oxygen. In sulfur trioxide, 32.06 g of sulfur are combined with 48.00 g of oxygen.

 

a.   What is the ratio of the weights of oxygen that combine with 32.06 g of sulfur?

b.   How do these data illustrate the law of multiple proportions?

 

22.  By experiment it has been found that 2.18 g of zinc metal combines with oxygen to yield 2.71 g of zinc oxide. How many grams of oxygen reacted with zinc metal?

 

23.  A sample of H2S04 contains 2.02 g of hydrogen, 32.07 g of sulfur, and 64 g of oxygen. How many grams of sulfur and grams of oxygen are present in a second sample of H2S04 containing 7.27 g of hydrogen’?

 

24.  How many protons and neutrons are in each of the following elements’?

a. Y89

b. 73Ge

c. 24Mg+2

         d. 238U

 

25.   How mans protons, neutrons, and electrons are in each of the following?

          a. 195Pt+1                                 d. 16O2-                                      g. 184W

           b.   93Nb                                    e. 122Sb+2                                           h. 133Cs+

           c.   40Ar-1                                  f. 56Fe+2                                i. 28Si-3

 

26.   Name the family to which each of the following elements belongs:

           a.   Fe                                       c.Ar                                         e.Rb

           b.   CI                                       d. Sr                                        f. Nd

 

27.   Are the following elements metals or nonmetals?

           a.   Mg                                      d. Br                                       g. Co

           b.   Si                                        e. O                                         h. Mo

           c.   Ge                                       f. Bi                                         i.  Xe

 

 

28. Given the position in the periodic table, what is the most likely oxidation state that each element will nave when forming an ion?

a. Cs

b. N

c. Br                                                        

d. K                                                                                                    

 

 

29. An element combines with 2 atoms of chlorine to form an ionic compound. The element has 20 neutrons in its most abundant form. Write the formula of the compound.

 

 

30.Predict the formula and state the name of the compound likely to be formed from the following substances:

          a.   calcium and phosphite ion     b. potassium and pernitrate ion

 

31. Name each of the following compounds:

          a.    PbI2                                                  e. CsC1                                   i. K2Cr2O7
          b.   NH4Cl                                  f. 0s04                                                  j. Na2SO4
          c.    Fe203                                               g. Cr(OH)3                                      k. KH2PO4
          d.   LiH                                      h. NaC2H3O2

 

 

 

 

32. Write formulas for each of the following compounds:

 

a.      sodium cyanide

b.       tin (II) fluoride

c.       sodium hydrogen sulfate

     d.    lead (II) nitrate

     e.    iron (III) oxide

     f.     calcium phosphate

     g.    sodium bromate

 

 

 

33. Write formulas for each of the following compounds:

 

a.  potassium carbonate

b.  magnesium hydroxide

c.   dinitrogen tetroxide

d.  hypoiodous acid

e.  iron (III) chloride

f.   tin (IV) oxide

g.  rubidium nitrate

h.  potassium chlorite

i.  carbon tetrachloride

j.   sodium iodate

k.  potassium permanganate

1.  sulfurous acid

m. potassium hydrogen phosphate

n. ammonium acetate

o.  ammonium d.ichromate

p.  hydrobromic acid

 

3 4. Give the names of the following acids:

a. H2SO5

b. HIO2

c. HBr

d. HNO2

 

35. Give formulas for the following acids:

 

a.  pernitric acid b. hydrofluoric acid

c. sulfurous acid d. hydrocyanic acid

e. hyposulfurous acid f. acetic acid

 

36. Give the Coordination # for the following positive cations

a. Ag+1

b.Cu+2

c. Cr+3

 

37. Give the name for the following ligand compound

a [Co(NH3)5Cl]Cl2

b K3Fe(CN)6

c. [Fe(H2O)2(NO2)2]2FeCl4

 

 

38 Give the formula for the following ligand compound

a. Triamminebromoplatinium(IV) chloride

b. potassium hexafluorocobaltrate(III)

c. tetraamminechromium(III) hexacyanoferrate(III)

 

39. Give the formula for the following organic compounds

a. 2 cloro pentane

b. 2,2,3 trimethyl 4 octene

c. 2 methyl hexanol

d. 3,3 diethyl 2 pentanone

e.  propanoic acid

f. methyl ethanoate

g. ethoxypropanol

 

40. Give the name for the following carbon compounds on the following sheet

 

 

 

 

 

 

 

 

 

 

 

 

 

41. Complete the first half only of the reactions below

(a)    Sodium metal is added to water.     

(b)    Dilute sulfuric acid is added to a solution of lithium hydrogen carbonate.

(c)    Ethanol and formic acid (methanoic acid) are mixed and warmed.

(d)    Excess concentrated potassium hydroxide solution is added to a precipitate of zinc hydroxide.

(e)    The gasses boron trifluoride and ammonia are mixed.

(f)     A solution of tin (II) chloride is added to a solution of iron (III) sulfate.

(g)    Phosphorous (V) oxytrichloride is added to water.

(h)     An acidified solution of sodium permanganate is added to a solution of sodium sulfite.

(i)      Excess potassium hydroxide solution is added to a solution of aluminum nitrate.    

(j)      A solution of sodium bromide is added to an acidified solution of potassium bromate.    

(k)    Sulfur dioxide gas is bubbled into distilled water.   

(l)      Phosphine (phosphorous trihydride) gas is bubbled into liquid boron trichloride.

(m)  Hydrogen gas is passed over hot iron (II) oxide powder.   

(n)    Solid potassium amide is added to distilled water.

(o)    A strip of magnesium metal is heated strongly in pure nitrogen gas.

(p)     A solution of nickel chloride is added to a solution of sodium sulfide.

(q)    Solid calcium is added to warm water.   

(r)     Powdered magnesium oxide is added to a container of carbon dioxide gas.   

(s)     Gaseous hydrogen sulfide is bubbled through a solution of nickel (II) nitrate.  

(t)      Excess concentrated sodium hydroxide solution is added to solid aluminum hydroxide.

(u)    Solid silver is added to a dilute nitric acid (6M) solution.  

(v)    Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate.

(w)  Hydrogen peroxide solution is added to a solution of iron (II) sulfate.   

(x)      Propanol is burned completely in air.

(y)    Solid calcium carbonate is strongly heated.  

(z)     A piece of nickel metal is immersed in a solution of copper (II) sulfate.  

(aa) Equal volumes of equimolar solution of disodium hydrogen phosphate and hydrochloric acid are mixed. 

(bb) Chlorine gas is bubbled into a solution of sodium bromide. 

(cc) Ammonia gas is bubbled into a solution of ethanoic (acetic) acid. 

(dd) Solid ammonium carbonate is added to a saturated solution of barium hydroxide.  

(ee) Drops of liquid dinitrogen trioxide are added to distilled water.  

(ff)     Solutions of potassium permanganate and sodium oxalate are mixed.