Chemistry: First Semester Exam Prep #4 (Chooso
1. Which unit is NOT used tbr volume?
a) L
b) trlL
Which piece of equipment would be best to
mcasure 56.7 mL of water?
c) test tube
d) electroaic balance
3.
Which of these are the smallest?
~ I milliliter
d) I kiloliter
4. The prefix kilo means:
a) 100times laracr
~ 1000 times !~er~
c) I 000 000 times larger
d) IOtimes smaller
5. The metric prefix milli means:
a) 100 times larger
b) 1900 times!~gcC,
Q-~c) 1000 tim=es smaller ,~,3
d) 100~ifnes smaller
6. The number 2 X 10~ expressed ira standard
notation is:
~3~-.2~0 0
c) 2
d) 0.O2
7. The number 3 X I 0 3 expressed in standard
notation is
a) 300
b) O.3OO
10. When adding and subtracting lneasurements one should
limit and round answers to:
a) the least number of siguificant figures in any of the
c) t~e tenfl~ place
d) three significant figares
I I. When multiplying and dividing measurements, one
shoald limit and round answers to:
a) the leas! number of significant figures in auy of the
Q
b) ~fl~r’~mber ofdecunal places m any ol he
c) the tenths place
d) three siguificant figures
12. When measuring tile vohunc of a liquid iu a graduated
cyliuder, tl~c mcasaremeat should be read from the:
a) top of the meniscus
~b~.49p of the cylindej2
d) table top
13. If the mass of a dry beaker is 19.02 grams and increases
to 22.40 grams when a sample is added, what is the
mass of the sanaple?
a) 22.40 g
d) 1.10g
14. The mass ofa sanlple is 4.1 lgrams. The volume is
2.00cm3, What is its density7
a) 8.22g/cm3
c) 0.49g/cm3
d) not enough information
15. A student estimated a mass to be 250g, but upon
carefully measuring it, lbund il to be 240g, What is the
percent error of the estimated mass?
d) 3.000
8. How many of!be zeros in the measurement
0.000040300 are significant?
C b) 4.2 °~.)
c) -4.0%
d) -4.2%
a) 8
16. The number of electrons in a sulfur atom is:
a. 32.06
b. 32
9. The number of significant figures in the
measurement 0,070g is:
4
-~t7"~48
Chemistry: First Semester Exam Prep #4 (Choose the BEST answer.)
17. The stun of the protons and neutrons in a
lithium atom is:
a. 12
b. 13
18. The electron was discovered by
a. J3ohr
d. Becqnerel
26. Rntherlbrd’s alpha scattering experiment showed that
tile char,,e on tile nucleus of an atom must be:
I~ neutraq
c. negative
d. none of the above
27. The nug,.Le.u.s_o&tLle atom has
c.
d,
Maxwell
Dalton
19. Tile nnmbcr of neutrous in n lluorine atom is:
c. 9
d. 18.998
20. The net charge oi! any atom is:
a. positive
~d~ o~n the element
21. The sum of the protons and neutrous in an atom
equals the:
a. atomic number
b. number of electrons
~_ atom ic mas~:)
d. Inass ntlnlber
b.
c.
d.
a Iow-~fensilv
a negative charge
no charge
28. All-?on-alw_a}~s con~3so
~ unequal number of protons and electrons~)
~l~er----o-f’-protons and e~--’~e~tron=’=7 -c. unequal nunlber of protons and neutrons
d. equal number of protons and neutrons
29. Tile whole number that is closest to tile atomic mass of
an atom is the
a. atomic ilunl bet
~7 ~Vdg~air6~g~m in b e r
d. namber of neutrons
30. Which subatonaic particle did Thompson include ill his
"plunlb pudding model"?
a. protons
b. neutrons
22. Which of these statements is false?
d. -i~i~e-~Tth e nbovc
charged.
d. The neutron is [bund in the nnclens of an
atonl.
23. Au atom with atomic number 48 and tnass
uut?~h~;, ! 20 contains: .......................................................
b. 72 protons, 48 electrons, and 48 neutrous
c. 120 protons, 48 electrons, and 72 neatrons
d. 72 protons, 72 electrons, and 48 neutrons
24. An element which has a mass nunlber of 23 and
has 13 neutrons is the element:
a. Lithium
b. Potassium
c.
31. Which of the [bllowing types o[" reactions resnlts ill a
~i!!gl,~ pmdt!g[~
c.
a.
single replacement
double replacement
32. In the reactiou 2KCIO3 "-) 2KCI + 302 oxygen is a _ ..
a. r~a~a.a[ ....
¯
c. coefficient
d. subscript
33. Supersaturated solutious are characterized by
a. being super hot
b._.,?pving great gt~bJlily ..................................................................
<17 h~}iii~ g ia)ger ainmmt of solute thnn can be
..... ~e0. ..................................................
d. being able to exis{ a~ snper-low temperatures
25. The experiment that revealed the charge of the
electron involved the use of
a. gold foil
b. ~.Rulherlbr~.
~:~- the-~’ath~-=Tde ray
Chemistry: First Semester Exam Prep #4 (Choose tile BEST answe,’.)
34. In tile reactiou: N2(g) + 3Hz(g)’-) 2NH3(g) + heart
a. tile reaction is both endothermic and exothennic
b. tile reaction is endolhermic
~,.cU tile reaction J~ ~othermic
d7 t le reaction is ilel her endo heHlllC or
exothermic
a, 36.0 g
(~o. K] ,o.
~
,
35. How many oxygen atoms arein A12(SO433?
a. 3 atmnsofO
b. 4 atomsofO
c. 7 atomsofO
45. The sum of the atomic masses of all tile atems in a
c o n2j~9~ n ..d~.~_~3311 e d the .
36. The atomic mass of an element:
a. depends on the number of isotopes of that
element.
b. depends on the mass of each isotope of that
c.
d.
molar volume
percentage composition
element.
c.
depends on the relative abundance of isotopes
~_flaat element.
39. The weigh{ed average mass of all the atoms
........... {~gg~5~K<}~9(an element is the:
46. Tile number of atoms in one mole of an element is
equal to____.
a.
a nleasure
b.
c.
a gram
a formttla unit
(’’ft.- "a(6mic mas~ >
6. atomic umber
c. electron nttmber
d. netltrou nnmber
40.
Tile percentages of isotopes fotmd in a sample
of an element is given below.
22% Carbon-14 with a mass of 14 ainu
78% Carbon-12 with a mass of 12 area
The correct method for finding the average atomic mass
of the sample would be:
47. It is possible o convert moles Io particles by:
c.
d.
malfiplying by the molar mass
dividing by fl~e molar mass
48. How many molecales of sulfur dioxide are present in
1,~60~?aoles of~.ulfur dioxide?
c. 7.62x 10~
d. 3.76 x 10~
~ g-6~
"
a. (22) (14) - (78) (12)
b. (0.22) (14),: (0,783 (t~)-,
{(Z~2):{iai + [0 78) ( 121 )
49. Find the number of moles in 3.30 g of(NHa)2SOa
a. 132.1
b. 40.0
41. llow do the isotopes hydrogen-2 and hydrogen-3
difl’er?
a. Hydrogen-3 has one more electron than
hydrogea:2 ........
Hydrogen-3 has two neutrons. >,,
d. Hydrogen-2 has no protons.
42. Ilow many molccalcs are ill 4.50 moles O1"II20?
a. ~35o .............
c. 6.02x 1023
d. 3.00
~
50. Which contains more atoms?
a. 1.00 mole I1,0, q
c. .OOmdlCO ~
d. 1.00 toni K {
51. An elemenl v,,ith seven valence electrons v,,onld likely, be:
a. all alkaline earth metal
b. an alkalimetal
c. -a..:.~J~ gas
~ :~
Chemistry: First Semester Exam Prep #4 (Choose the BEST ans,ver.)
52. The most stable atoms are those of the
a. metals
b. metalloids
(~. nob
d, nonmetals
60. The likeliest charge an atom with 2 valence electrons
would develop is
B. 6+
d. 6-
Tile ~on w~4dka cha~,~g~f+l and the same
electron confutation as argon is
61. The likeliest charge an alom with 6 valence electrons
will develop is
a. 2+
~(- ~V.,,, (~: ~y~
d. magnesiunl
54. The tendency to lose electrons
as we move acrnss a period
on tile periodic table
a. increases
b. remains tile same
62. )~!,.J4~7¢Jest charge of an ion or tile element Bromine is
h. ~1
d. -2
d, no Irend exists
55. Generally, members of a
the same number of valence electrons.
a. period
b. series
C, row
63. Metals tend to .
a. gain electrons and become positively charged
cations
b. lose electrons mid become negatively charged
Q{]*’- lose ~lectrons and become positively charged
.___ cations
d. gain electrons and become negatively charged
56. An element which is considered to be a
metalloid is:
h-Y"CaU( [u in
c. Oxygen
d. Sodium
57. The eleme!?~t Iodine is a
a. period 5 alkali metal
b. perio~A_halo~
/’~*c. pghod 5 ~[9~ge!~
"~dT" pe~’*}iod--~ trans---ii:lon metal
58. Sodium and Potassium have similar properties
because they have tile same .
a. at~p)ic radius ..............................
c. ~omzat~on energy
d. electronegativity
59. The maximum nnmber of valence electrons in
an atom is .
a. 2
b. 4
64. The basis of the ionic bond is tile ,
a .. s raring-of an electron pair ............
...... b. electrical attraction between oppositely charged
\ ..............
ions. .................................................
d.
absorption of water into their solid structures
65. Elements tend to gain or lose electrons in order to
acquire lhe electron configuration o[’a
a. halogen
b. trallsicig~etal
}.\ _
69. When sodium combines with chlorine to lbrm sodinm
oh!pride, tile sodiuhl attains tile electron
coil figu!’ati9n of
a. heliui~:
b. neon ..... ....
c. aygon
d. ~lthium
70. The type of chemical bonding in which electron pairs
are shared is
a. ionic~oo.
/’~O(’~ ~’~ (~e:~
c.
d.
metallic
none of the above
Chemistry: First Semester Exam Prep #4 (Choose the BEST answer.)
d. balanced
7 I. Which oftbe following correctly matches the
names and formulas of the compounds?
a. AICI3. aluminum trichloride and N204 ,
nitrogen oxide
b. AIC]3, aluminum tricbloride and N104
dinitrogen letroxide
c. AICI~, aluminum chloride and N204 nitrogen
d,
74. Choose the con’ect set of coefficients needed to
balance the following equation:
PCI5 --) PCI3 + CI2
a. 2,2,1
b. 1,2,1
c....I., I =2,~v:: ...........
...... d. balanced ,/
AICI altnllilltnll chloride and N,Oa diniho~Ren/,~o}:~
75. Choose Ihe correct set of coefficients needed to
balance Ihe Ibl~owinu equalkm:
PbCh ~ Li~Q< @,iCI ~ PbNOa
7_3. Choose Ihc correct set uf coefl]cicnls needed tn
~balance the followilm equation:
~ + O~ --->~I I~O
a. 2,1,1
b.
c. 2,2,],I
d. balanced
Short Answer:
76. A copper penny has a mass of 3. I g and a volume of 0.35cm3. What is tbe density of copper?
77. A liquid has a density of 4,8 g/I. What is the mass ofa 2 liter sm~e?
78. What is the volume of a substance that has a mass of 80 g and a dens)~ of l0 g/cm ?
~q
79. Calculate the following quantities:
a. 1,100 cm
I~
b. I m
~OoO
c. 10 m
iOoG
d. 2.5 km
e. 4.05 kg
m
mm
cm
m.
g
80, Indicate the number ofsigaificant lqgurcs in
each of the following:
a. 12600 .~’~
b. 0.09 ~
c. 2001 ,~
d. 0.00500100 ~.~
83. Which of the lbllowing are empirical formulas and
which are molecular fbrmulas?
81. The a~cepted value or true value for the density
of le~{Pb) is 11.35~’~’)ml. Y~pti~- exp
lab
, value or obxserved value f~uhd during a
ig 9.65
84. Find the empirical lbrmula of each compound flom its
% composition.
,~,~e e~ror o~>~easur~nt.
@hat is tl~ent ~t~t%f your
(-)
82. Name the two temperature scales used in science?
Give the freezing pt., and boiling pt. of water for
each of them.
a. CH+N i=.~
b. NaO ~
c. C6H30~ ~=4
d. H202 [~
e. Na2SO3 ~:
f. C6HIOO4 ~
a. 72.4 % Fe and 27,6% 0
85. If given the empirical formula aud molar mass for a
compound, calculate the cold, pound’s molecular
formula?
~) Qi ~ z)~,C ~
a. CH20, mass = 90 g/tool
}-~ 2 L]K:~;~
b.
C3H502 Illass = 146 g/tool
Chemistry: First Semester Exam Prep #4 (Choose the BEST ans\ver.)
86. Find lhe missing density, mass, or volume of
the following:
a. The mass of a subslance is 45.6 g and the volnme
is 15 cm :
Density ~2,~- , (~,~
b, The volume of a substance is 2.9 ml its density is
6 g/ml: f>k
Mass
95. Calculate the % composition of each element by mass of:
Propane C3H~ ~ t~ Z "~2 / i~ ~] ~.
96. Which of the foisting are is cs?
a. NI2X
~713X ~U~aX
d. 2411X
97. Describe the major parts of Dalton’s Ato n c T ~eo "y
c. The density of a substance is 7.8 g/cm3 and the
massis 125g:
Voknne= i~,
¯ .,’
87. lfyoa have 6.7 1, of O~ at STP, Ipw many
moles do you have - ~: L)O~v~
98. Balance the followiag chemical equations:
88. What is the nmlar mass of Sn~(PO4)2?
89. How many moles are in 137.5 g of Mn?
90. What is the mass of 2 moles
91. What are the correct lbrmu Fs or namesfor the
folloxving compounds?
a. potassium sa!lhte
b. calcium phosphate
L
c, dis@fur heptoxide
d. trinitrogen pentahydride ~Q~ S ~3~ 5
100. Describe difference be~.ween homogenous,
heterogeneous mixtures, and pure substance:
92. List the diatomic molecules:
a..~3~ b. O c. "i~( d.
f. ~ g.
93. List the names & formulas oSithe 5 comnlon
94. What isthe o:~"~o~) charge of each
sabstance (ion) given’.
S "~+" "Z K @\
N
6