NAME:
PERIOD:
REVIEW
CHEMISTRY
MID-TERM
2013 -2014
Mr. Chuba
~
~
1. Express the following numbers in scientific notation to three significant figures:
d , 70 1-f 0 8
a. 0.000000027
iJr
b. 356
S to
9,
c. 0.096
~ (0
(,0 "1,0
a
-J
iJ.
Z' • 0 2> "/. I ()
d. 802.6
2. Convert the following numbers to regular form:
00
a. 1.52 x 1041sa
b. 7.78
c. 3.256
d. 6.03
o.
10-8
X
X
10-5
3JS ~
0000
(),
17 f
&0 -B 0000
106
X
0000000
3. Determine the number of significant figures in each of the following numbers:
AI
a. 4867 miles
cJ
b. 56 mL
c. 60104 tons
d. 2900.0 g
S
5
e. 0.0000003 ern
f. 4.6 x 1019 atoms
~
4. Express each answer in the correct number of significant figures:
a. 7.310
-7-
5.70
-3
b. 3.26 x 10-3 - 7.88
X
10-5
3. I
8
1. 10
d. 4.51 x 3.6666
e. 3.70 - 2.9133
OVER
5. A lead sphere has a mass of l.20 x 104g and its volume is l.05 x 103 ern'. Calculate the density oflead.
u
V
VV1
/,:)4)(/Oj
I,OS,
3&..13
'{..(0
6. Mercury is the only metal that is a liquid at room temperature.
grams of mercury will occupy a volume of95.8 crrr'?
Its density is 13.6 g/cm", How many
0/.: !!1
V
fYL
d. V
z:
;7
( /
3,
c
'%m
J) (
t?s.
s
CMt
3)
7. The price of gold on a certain day in 2004 was $315 per ounce. Determine the price of I.OOg of gold on
that day.
1 oz = 3l.03g
11 31$
1,0°.1
lot
8. The speed of sound in air at room temperature is 343 m/s, Determine the speed in mi/hr.
1 mi = 1.609 km
h1L
h,..
-
31.{3nr
--
Is
IkVl1
1 () 00
J
I.
Iv!
003
11-\ ~
~oq JCvtt
I tl1/n
~OIlfI''J
/ hr
--
7~ 7
h,...
9. The human stomach can expand to hold up to 4.20 quarts of food. A pistachio nut has a volume of
0.900 mL. Determine the number of pistachio nuts that the stomach can hold.
1 gallon = 3.79 L
1 gallon
1 L = 1000 mL
= 4 quarts
3.71 L
tt
flSTf1(!J!16
AiUr.5
.::
~~
I
I.{
gt
0J
J5
I{)OO "" L
IL-
I nIJ
+
o . CJOOWl
,
/11£
L
10. Determine whether these statements describe either a physical (P) or chemical (C) property:
a: C
b.C(Jl
c.
P
fertilizers help increase agricultural production.
L water boils below 100 e on top of a mountain.
0
p
d.
P
e.
f. ~
g.
oxygen gas supports combustion.
lead is denser than aluminum.
uranium is a radio~ctive element.
iron has a tendency to rust.
L rainwater
in industrialized regions tends to be acidic.
II. Determine whether each of the following is either a physical change (P) or a chemical change (C):
P
a.
when a glass of water is left out in the sun, the water gradually disappears.
b. ~
carbon dioxide in air is converted to more to more complex molecules by plants during
photosynthesis.
c. ~
the helium gas in a balloon tends to leak out after a few hours.
d. ~
rocks are ground into sand.
e. ~
frozen orange juice is liquefied by adding water to it.
C
f.
g.
digesting a pizza.
L a spoonful of table salt dissolves in a bowl of soup.
12. Which of these properties are intensive (I) and which are extensive (E)?
area
a.
b.
:r
color
c.
r
density
d.
~
length
e.
,;
volume
f.
j.
g.
h. ~
17
temperature
mass
ductility
OVER
13. Classify each of these substances as an element (E), compound (C), homogeneous mixture (hom), or
heterogeneous mixture (het):
a.
C,
water
b.
E'
gold
c.
heJ-
d. ~
e.
raisin bran cereal
orange soda
~e~ rubbing
alcohol (C3H70H)
f. ~e~sugar
g. ~
h.
i.
cellulose
E
he, r
uranium
sand on the beach
j. ~brass
13. List the major contributions of each of the following scientists:
a. Dalton
-
b. Thomson
71-1G'Otl'/
e-
b:>lsto'\JIS1LED
_
47lJhf (C,
11-1 c:
I;;;.
ofVELof'ED
of
e-
c. Milliken
d. Rutherford
-
GOl-U
em
e. Chadwick
-
EXPEf2.IME?-JT)
FOIL
SPAC£'
(=IT"
II:V1l'<.O,J
f..•
14. Define the following:
a. atomic number
b. mass number
-
-
of
NU 1'Y\8Ell.
~TOtJS
+
I'i/:UT/l.oAlS
c. average atomic mass ~ W e-I G I-lThcj)
{JF-
ArJ
Pl2oro",CS
.<1"€1l1-1G E"
eusr«
oP ALL
tEN T
15. Why does a knowledge of atomic number enable us to deduce the number of electrons present in an
atom?
:# P/ZO TOAI.s
s:
16. Why do all atoms of an element have the same atomic number, although they may have different mass
numbers? DI f=FI3Z.e...\T
r50ToPc=.::>
of AAl ELEfV1cN T
/../f/VG
blr:!=""l::7ll:AJT
tJuYY\tSett
of
AiEVTTlONS
EN
71-IE
A1 U C.U::VS,
17. What do we call atoms of the same element with different mass numbers?
.I. so TO P
Es
18. Explain the meaning of each term in the symbol ~X.
4
Yl'\
l
f\ 5.S
ATOM Ie.
.s:
E1t
#J U ()"\~
NUfV\5(:.1{
19. Write the isotopic symbol for each of the following:
)QS
72
a. platinum-195
pi
t
b. copper-63
c. tungsten-186
20. Write the name for each of the following isotopes:
a. 33S
16
b. 20lHg
80
- ~ol
M82C.U~'"
c. 23Na
SODiUM
II
-
.;j3
d. 64Ni
28
21. Complete the following table:
SYMBOL
PROTONS
NEUTRONS
S~
,ysM",
262Bh
107
288UUp
115
204Hg
80
57
2(,
,:'e
MASS NUMBER
3/
~5
56
7
155
/07
;;; f..t ;;)
115
173
/15
,;;~fr
25
10
ELECTRONS
?O
,;q,
?O
124
3 I
,
OVER
26
,J;)°V
57
22. What are allotropes? How are allotropes different from isotopes?
A L.LOn-:OPI~..s fllt.E vlf:'"i-;'E/ZSAi-r
Pi../y.flC/;)I..
I1KI!A,.JGEnte-fTJ
AN
.ISOTVPF
n-l ~
of
AAi c"I..E!fo1E!--sT VP,!(!6..5
f;Y
TI-fc-
OF
NiJ,r;vSFfZ
/-IAI
of
cLf::Il1&7vT.
NEurriZoNS
.rl\..l
(..! lJC LI::'U S. ,
23. Determine the average atomic mass of titanium given the following information:
Titanium ..46
Titanium ..47
Titaniurn-48
Titanium-49
Titanium-50
relative
relative
relative
relative
relative
mass = 45.95 amu
mass = 46.95 amu
mass = 48.00 amu
mass = 48.95 amu
mass = 49.94 amu
of
( I.( 8. a 0)
("73, 7)
abundance = 8.000%
abundance = 7.500%
abundance = 73.70%
abundance = 5.500%
abundance = 5.300%
+
(I.(
t. q:;) (5, ~ )
-i-
('19. o tf) (S.:3)
100
/00
24. Name the concept, theory, model, etc. that each of the following scientists is known for in the
development of the modern atomic model:
b. Bohr
PLA,,1 E m£. 'f {'['OD 61.
~Ei<6
'I
-
AT
TH E
LEVEew
bur::"Lli'(
e. Schrodinger
t:OV/2,TtorJ
WAvE
25. Write the abbreviation for and describe each of the following quantum numbers:
Vl
a. principal quantum number
11
J{
b. azimuthal quantum number
c. magnetic quantum number
d. spin quantum number
l'Y/ 9.
rY1S
SPiN
OF
mE
26. Define each of the following:
a. Pauli Exclusion principle
A
fYlA'll'IMtJlVl
t.3\JT
010
of
L'l IF
TWO
THE
b. Aufbau Principle
EAt-I-I f'LIECmo,,",
I-IAVE
EL\~Crr<()"-lS
occuPIES
THE
It
OCCUr''!
MA~I
ELEC712oN...)
OPPOSiTe
LOW€S T
SltJGLI::.-
/-lTVI11IC
SPltJ3,.
1::.-7Vf!<.6"'1
OR/!)fn::JL
AvAILAtSLE"
c. Hund's Rule
8£ClR.o1'olS LVIn! '"fiofG SAMe
SPIN
mus r occupy i=1'IC-H EqJVt-H. t=Jvi::-r<6 Y
LEVEL (O((f.)\"T'A\..)
SIioJ6lY
BEFOIf.£
ADO/DONAL
l::'LEe.rreo",IS
w/n-j
o,oPOStTF
SP/I.JS
CAN OCCUP'( THE' SAMe
Ot<!3ITr.:ns
d. Heisenberg's Uncertainty principle
.:tT IS FVNDAME"I\JTALL"f
.It'YV'oSS tell:
TO I<AlO tV
VELOc..IT'f
AtJD
A
oF'
Po:)lTloJ0
f'Af(TIC.Lt::
AT
mEe./~f::-"L
mE"
SAmE
Y
(joTH 'THE
TIME.
27. Complete the following table:
Value of I
Letter
0
S
I
f
2
of
3
t
Range of m,
Number of
orientations
Maximum # of electrons
I
d
0
-~\-/)()I'la
-3-d-IOI;}3
I
I
)
f£J
3
~ I) OJ I
I
I
I
S
10
1
1'-/
28. Write the complete electron configuration for each of the following:
a. As
Is 2
~S Z-
d.f (, .& z 3f (.,~Is
2.
3d
10 t..J
f3
29. Draw the orbital diagram for each of the following:
a.O
1~1 1
--dft
1~ 1~
l
b. V
111
Is 2c. Al
11.J s 2-
1 I, 11,
11--
--Jf to
1/,
11/
Isz,.
Jsz.
11 1 _
1~ 1~1~ 1Y ---1l:. --3flo
<Is'
3$'
1~ 1l-- 1~
-~
af'"
1~
~-~
3$'
3f
OVER
I
3d
3
30. Determine the frequency of electromagnetic radiation with a wavelength of 3 .33 x 10-8 m.
2
.3.00)( 10
c
A
.::
=
8
3,33 ~ 10-
9,0/
x/o
,s
S
-/
31. Determine the minimum frequency oflight needed to eject an electron from an atom of platinum if the
energy required is 9.08 x 10-19 J.
_
-.)
=:
1=
~.o8'1. /0
_
h
t. . (,,:3
-'9
IS
_
=
")('0-3'-1
1,37X/O
32. The argon-fluoride laser used in some refractive eye surgeries emits a wavelength of
1.933 x 1O-7m. Determine the energy of this laser.
f
g
he
z:
.:
A
t. Q33y,
33. State the periodic law.
THE PI-NS/CAL
Al\lb
A-,(E
A
x/0 )
(ro.~3'f,IO'34)(3.00
C.HE'MltI-lL
FUrJc.no,J
f'8'l/ODIC
/, o~CJ XID
10-7
P~OP~7<TI&5 OF
of
1}IEI~
71-I1E
ATOmiC
-18
..T
ELehll<::NiS
A!uml3t7<,
34. Identity each of the following as a metal, nonmetal or metalloid
a. phosphorus
N (Y)
c. arsenic mEn1
e. krypton
N
LLbl
D
fV)
b. niobium
[\'\
d. holmium
M
f. strontium
M
35. Name each of the following groups by their family name.
a. Group 17
HALOGENS
b. Group 1
c. Group 18
NO(!)Lt:
d. Group 2
GA~€S
ALj«ALI
n1ETALS
ALI<.ALI N E
i::I1RTH
h-'lETAW
36. Classify each of the following elements as a (an) alkali metal, alkaline earth metal, halogen, or noble
gas.
a. rubidium
A U<A L I
b. bromine
tJ ALOG8J
c. radium
ALKALltJ E
CAI2.THS
d. iodine
HAL06E"1J
e. radon
i\lOP.>LE GAS
f. lithium
ALKAL I
37. State the trend for atomic radius.
T -'> f!J
38. State the trend for ionization energy.
39. State the trend for electronegativity.
bECI('EY-)SE
T
(j)
-7
nVCt€Ffl.$t:
L -> R
40. Arrange these elements in order of decreasing atomic radius: sulfur, tellurim, and oxygen.
-Ie >3
>0
41. Arrange these elements in order of increasing ionization energy: TI, Ga, In, B.
T J <:
r
f"\
<
Go. <. (3
42. Arrange these elements in order of decreasing electronegativity:
F>O>,..j>-
0, F, C, N.
Co
43. Name the following ionic compounds:
a.
f. Pb(N02)4
Mgh
MA(;t-.JESIOn-'\
I:otil'\:)E"
LEAD
(1'4) NITt2\TF
g. (NH4)3P04
b.
.l~o~ CU..')
PHoS'PHIDl?
AMtv\ 0,,", I V YV\
PHo:SfJHII77::
h. AI(HC03)3
c.
I1LUmlfoJUfVl
CA~t!;oJJAW
i. Ni(CN)3
d.
e.
OVER
~~~---~---------------
44. Write the formula for each of the following ionic compounds:
a.
/\l (
b.
f. iron (II) permanganate
nickel (III) acetate
Fe
(C;). 1{30,; ) 3
barium telluride
g. manganese (III) carbonate
I5:tTe
c.
d.
f'I) Y)a
(COS)3
tin (IV) cyanide
h. gallium sulfide
SV\ (ctJ) V
Gaa 3,3
cobalt (III) sulfite
I.
radium iodide
Ra. I a.
Co;;. (S03)3
e.
(MilOt{ ) J.
copper(l) bicarbonate
j. europium (II) phosphate
CtA. HC.OJ
t"U PO~
MID-TERM TOPIC SUMMARY
Unit 1
rules for significant figures
rounding rules
SI units
Unit conversions (railroad tracks)
Kilo-hecto-deca-base unit-deci-centi-milli
Unit 2
matter
mixtures (homogeneous & heterogeneous)
compounds
elements
allotropes
physical changes
chemical changes
physical properties
chemical properties
allotropes
Unit3
protons, electrons, neutrons
mass number
isotopes
isotopic symbol
average atomic mass calculations
Democritus
Dalton
- Rutherford
- Milliken
- Thompson
Unit 4
c=/cy
amplitude
frequency
speed of light
Planck's constant
E=hy
ground state
excited state
quantum numbers: n, I, mr, Ills
electron configurations: complete and abbreviated
Aufbau Principle
Pauli Exclusion Principle
Hund's Rule
orbital diagrams
Planck
Bohr
de Broglie
Heisenberg
Schrodinger
UnitS
Mendeleev
Moseley
metals, nonmetals, noble gases, metalloids
family names
trends in atomic radius, ionization energy, electronegativity
definitions of atomic radius, ionization energy, electronegativity
naming ionic compounds containing monatomic ions
writing formulas for ionic compounds containing monatomic ions
naming ionic compounds containing polyatomic ions
writing formulas for ionic compounds containing polyatomic ions
OVER