NAME:
PERIOD:
REVIEW
CHEMISTRY MID-TERM
2013 - 2014
Mr. Chuba
~
~
I. Express the following numbers in scientific notation to three significant figures:
s. 70 1- (08
a. 0.000000027
b. 356
S(p
XlO
9. ~o
'I.
~.
c. 0.096
61
-.1
10
;;.
g. 0:3 -y I 0
d. 802.6
2. Convert the following numbers to regular form:
Isaoo
a. l.52 x 104
b. 7.78
c. 3.256
d. 6.03
X
X
00 00000
O.
10-8
X
c.
10-5
~O
106
17 f
ooo03JS~
-s OOOQ
3. Determine the number of significant figures in each of the following numbers:
~
a. 4867 miles
d
b. 56 mL
S
c. 60104 tons
d. 2900.0 g
5
e. 0.0000003 cm
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
d. 4.51 x 3.6666
X 10-5
3. I 8 'f. 10
J~, S
e. 3.70 - 2.9133
OVER
5. A lead sphere has a mass of 1.20 x 104g and its volume is 1.05 x 103 cm3. Calculate the density oflead.
1./
1,;J4X/OJ
6. Mercury is the only metal that is a liquid at room temperature.
grams of mercury will occupy a volume of95.8 crrr'?
dV
Its density is 13.6 g/cm'.
How many
=
7. The price of gold on a certain day in 2004 was $315 per ounce. Determine the price of 1.00g of gold on
that day.
loz=31.03g
::
/' 11 31S
_',_0_0_..5_11-_)_0_1,. __
I
I
::
3/. 0 3j
IOl
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
3l/3vr(
/I'll'
h,..
=
--
-/s
I e 00
~OS
11%~
fk:»t
111I
!lI1./n
~o q jc.V)'l
I.
,
to 011(""
/ hr
--
7" 7 TrJnl
9. The human stomach can expand to hold up to 4.20 quarts offood. 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 L = 1000 mL
1 gallon = 4 quarts
AI • .io ;.
v
.:
=
3.71L
6t
lJol
I.{
I
.::
t
IJ ".f
t/JjC)/;
~ct"
/000"",
I nu
L
() • Clo(jk'>"
Il.-
7
3
r"/.
'f.J 'A 10
L
--
I'ISTII~/O
AiVT.j
-t-
]
L
10. Determine whether these statements describe either a physical (P) or chemical (C) property:
C
a:
oxygen gas supports combustion.
P
fertilizers help increase agricultural production.
c.
p
water boils below
d.
p
lead is denser than aluminum.
b.CUl
P
e.
f. ~
g.
ioo-c
on top of a mountain.
uranium is a radioactive element.
iron has a tendency to rust.
L rainwater
in industrialized regions tends to be acidic.
11. 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.
f
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.
f. ~
digesting a pizza.
g.
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)?
a.
E
area
b.
:r
color
c.
.r
density
d.
~
length
e.
,;
f.
..l-
g.
[
h. ~
volume
temperature
mass
ductility
OVER
._--
_._-----------_._._-
..._.-
_. -'----
.-.-
13. Classify each ofthese substances as an element (E), compound (C), homogeneous mixture (horn), or
heterogeneous mixture (het):
a.
C
water
b.
E
gold
c.
he.J
d. ~
orange soda
C
e.
raisin bran cereal
rubbing alcohol (C3H70H)
f. _C_sugar
g. ~
cellulose
h.
E
i.
he, t
j. ~
uranium
sand on the beach
brass
13. List the major contributions of each of the following scientists:
a. Dalton
-
b. Thomson
-
bll S
47VMfC
Tl4c
c;.
"DEVELOPED
-n-l~Otl.t
e-
CO'\}t'fLED
of
c. Milliken
ATOYl1.
d. Rutherford
-
GOL.i)
eMPT'f
e. Chadwick
FOIL
IS.
hfOSn
)
ExPEJi!.\ W\tt-JT)
SPA.C£
- t-JEU"'fv<'O,.J
14. Define the following:
a. atomic number
b. mass number
-
-
,.w W\B~
fte.oTO "-' S
oF"
+
c. average atomic mass - WE"IGI-ITh-n
()F- AN
Pt2.oTt)"-..U
NeU rtl..O,JS
411fTlAGt:
mASS
of=: ALl...
11-/(;
ISoToPe,s
'=.L/;"...1
t:N T
15. Why does a knowledge of atomic number enable us to deduce the number of electrons present in an
atom?
:/I Pteo TON.s
s:
Y
16. Why do all atorris of an element have the same atomic number, although they may have different mass
numbers? DII=FI3Z.I?NT
ISOTOPE,:)
of
AN FLEIYIl!l\lT
I-!F/V/£
blt="Fi::"""R..f:7JT
NtJYY\tSEtl..
tJElJT(l.oI'JS
of
IN
mE
tJVC.LEVS
#
17. What do we call atoms of the same element with different mass numbers?
.I..$0 TOP ES
18. Explain the meaning of each term in the symbol ~X.
4
z;
l
.s:
Y\'\
A
So S
A TO
YV\ ,
IJ
C.
V
<:-7t
(tV~
""'
a -n
U f\t'\ ·..;d:' i~
=
v
r-;
SYM60L
/::.~'I"V\aJ"
19. Write the isotopic symbol for each of the following:
a. platinum-195
pi t
lqS
7g
b. copper-63
c. tungsten-186
20. Write the name for each ofthe following isotopes:
a.
33S
16
b. 20lHg
M82CU..e. 'I - ;)0
I
80
c.
23Na
SODIIJM -
II
~3
d. 64Ni
28
21. Complete the following table:
SYMBOL
PROTONS
NEUTRONS
ELECTRONS
MASS NUMBER
SI.P
~ S
1'1"
3/
dS
7
155
/07
;;) (,
115
173
/15
;J2~
25
262Bh
107
10
288UUp
115
204Hg
80
$1
2/.,
,::'e
&>-0
0)(,
?O
124
s
I
,
OVER
26
56
;)
;;0 V
57
22. What are allotropes?
A L-LOT12.0P£S
AN LsoTVI't=
How are allotropes different from isotopes?
FFl2e8\lT
PIiYSlcAL
fJICI!4A1GEII19JTS
A~t: nl
of
AIJ
VAtel E.)
/:;LE~ENT
fjY
THE
NUWlt5~
0-':::
/-iN
of
cLE"rYlf:A.lT.
NE(jmON.S
.IA..!
THt: NUC.LI::.IJ~,
23. Determine the average atomic mass of titanium given the following information:
relative
relative
relative
relative
relative
mass = 45.95 amu
mass = 46.95 amu
mass = 48.00 amu
mass = 48.95 amu
mass = 49.94 amu
Titanium-46
Titanium-47
Titanium-48
Titanium-49
Titanium-50
(48.00)(73.7)
I
abundance = 8.000%
abundance = 7.500%
abundance = 73.70%
abundance = 5.500%
abundance = 5.300%
+ (1/!.q$)(S.S)+(~9.
Qlf)
o0
24. Name the concept, theory, model, etc. that each of the following scientists is known for in the
development of the modem atomic model:
a. Max Planck
b. Bohr
QuA.·..IT)I.\
OF
PLArJETAr2 'I
6JE'i<G"
/::::NI::."YlG Y
fYlOO6L -
€ -
THE
EX IS T
AT
C.E!2TfJIAi
LEvElS
PM..TICLE
c. de Broglie
WA"~
d. Heisenberg
UN C8HA
e. Schrodinger
WAvE
IN 1"(
bU A L I i
Y
p~ I Ai C I P L E
EQ VAnON
25. Write the abbreviation for and describe each of the following quantum numbers:
n
a. principal quantum number
J
b. azimuthal quantum number
c. magnetic quantum number
d. spin quantum number
rY1
YY) ~
S
at<1 /:;7Jm 17 0 Ai
SPIN
OF
mE
.J:JJ
sPACE
l:'"l.fC~o,,-1
ALLOWeD
(5.3)
26. Define each of the following:
a. Pauli Exclusion principle
A r'YlA')( 11'1 UrY) of TWO
(3vT
IF
ol\..ll'i
THE
b. Aufbau Principle
EAC-I-l ELtCnto,J
c. Hund's Rule
at=C~oN.s
LEVeL
I-IAVE
EU~CnlO".J.s
OCCuPIES
THE
ft
OCCVP'I
M/)8
ELE<:.i£o,...).j
OPPOSITE
SPIN$"
'="7Vf!26-Y
LOw6'ST
ot<l3rrJC/L
W In\ "TI4t:- SAmE"
SPIN
f'VIvsr
occupy
I="Y-/CH
1..) SIf.J6L Y (j~"j(E"
f-/DO' nOA/AL
cLECmO/l.lS
E<4>VAL
(0 a.e,TA
SPINS
CArJ
occuPy
Tl-/E
SAmE
/-}7VrvtIC
s/AfGLE
W
In-i
f-/vf-/ILAtSLF
l=7V1:1€.6 Y
o,oPOS I IE'
ORJ3ITALS
d. Heisenberg's Uncertainty principle
.:tT I.$ FVNDA""E"NTf-\Ll'( .rn'l.aoS51I.3Lt=
TO I<AlO LV fl'(Ee/~f:L
y /Jom
VaO(.IT'f
AND f'05mOI'J
oF' A
(lAR:nCi..E AT THE S(.Jm€' TIME.
27. Complete the following table:
Value of!
Letter
Range of nu
0
S
1
f
2
of
-~\-I,OI'IJ.
3
t
-3-~-IOld3
I
\ )
0
-I) 0, I
I I
Maximum # of electrons
Number of
orientations
I
I
;;
3
~
S
10
1
1'1
28. Write the complete electron configuration for each of the following:
a. As
I~/ ~s2. d,a Go 3.s Z 3(' ~~Is'
3d
If)
'-If3
29. Draw the orbital diagram for each of the following:
a.O
b. V
c. AI
1~1 .1
-df~1
1~ 1~
1v
Is 2-
1t-.
Jsz.
11r 1/' 1 ~
--Jf
fc
11r
1//
Is z:
,;}sz.
.1l
3£ 2-
1~ 1j,. 1b
dflD
--
1~ 1~1~
--3fiD
1~
3s 2-
jj,-
us z.
~-~
OVER
3f'
.11-~-3d
3
THE
30. Determine the frequency of electromagnetic radiation with a wavelength of 3.33 x 10-8 m.
c
,3,00 -X 10
-).
e
z:
,s
=
8
3,33 ~ 10-
r;,OI X/O
S
-I
31. Determine the minimum frequency of light needed to eject an electron from an atom of platinum if the
energy required is 9.08 x 10-19 J.
~
-J::-
Q,08)<.
=
h
-'9
,s
10
=
t. ,(,,:3 )( 10-3'1
/,37><10
S
-/
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
h(
z:
x/0 )
U(),~3~IO'34)(3.00
A
I. 0;)
:::
::
/,((33)</0-7
33. State the periodic law.
/HE
PI-I'ISICA LAND
"..(c: A
f'81'
C'.HEYl'\ Itl-l L
Fu tJ c. TJ(),J
0 Die
P~OPt~TI £,5 OF
OF
THE
ATOmiC
THE/~
9
-18
X 10
ae
)v)
.r
(;l\JiS
A/uml3c~.
34. Identify each of the following as a metal, nonmetal or metalloid
a. phosphorus
N (Y)
c. arsenic mEn1
e. krypton
LLbl
D
rJ fY)
b. niobium
M,
d. holmium
M
f. strontium
M
35. Name each of the following groups by their family name.
b. Groupl
a. Group 17 1-1ALO G ENS
c. Group 18
ALKALINE
d. Group 2
GA:>€,s
/'Jo(!>LE
AL!<::I-)LI
METALS
c-f-l,.ell-l h"IETf.\W
36. Classify each of the following elements as a (an) alkali metal, alkaline earth metal, halogen, or noble
gas.
a. rubidium
b. bromine
c. radium
A \...I<A
L
I
d. iodine
e. radon
HALOGE"IJ
ALVALIN
HALOGe-A.l
EEAll.n-IS
-----.-
f. lithium
--_.'
ALKAL
I
-- ._-------
_.- -_._---------
.._-_._.
__ ._---_
_-
-
37. State the trend for atomic radius.
T
-'> (j
38. State the trend for ionization energy.
39. State the trend for electronegativity.
b£0CEY-lSt=
T
(j)
-7
.rNe.R.€'fl~t:
L -">
R
40. Arrange these elements in order of decreasing atomic radius: sulfur, tellurim, and oxygen.
41. Arrange these elements in order of increasing ionization energy: TI, Ga, In, B.
T1 c
.L f'\
<
Gc..
<-
(3
42. Arrange these elements in order of decreasing electronegativity:
0, F, C, N.
(-'>O>,.j>-(!;
43. Name the following ionic compounds:
a.
f. Pb(NOZ)4
Mgh
MAGt-JESIljn'\
.roD \'\;)E"
L8\iJ
(I'J) NITI2\lt
g. (NH4)JP04
b.
AMW\ONI
v 1'\1)
Pl-/oSPH4~
h. Al(HC03)3
tlLU
It! I /\/U YV1
d.
i. Ni(CN))
e.
j. Zn(HC03)2
1- J'" C
e-I CAL.'()OA.i Arlf'
81 CtJRSo;J 1-1 re:
OVER
---.~-----
.------
..
--~----------
44. Write the formula for each of the following ionic compounds:
a.
f. iron (II) permanganate
nickel (III) acetate
Fe
Nt (CJ- 1-130.;)3
b.
barium telluride
g. manganese (III) carbonate
~Te
c.
d.
fY/ Y) CJ (COS)3
tin (Iv) cyanide
h. gallium sulfide
SV\ (etJ) t(
Gad. 3,3
cobalt (Ill) sulfite
I.
radium iodide
ReA.. I a.
Co;;. (503)3
e.
(fYJr'104 );).
j. europium (II) phosphate
copper(I) bicarbonate
etA- HCO.3
E U3(fO tf) d,
MID-TERM
TOPIC SUMMARY
Unit 1
rules for significant figures
rounding rules
sr 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
Unit 3
protons, electrons, neutrons
mass number
isotopes
isotopic symbol
average atomic mass calculations
Democritus
Dalton
- Rutherford
- MiJliken
- Thompson
Unit 4
c='Ay
amplitude
frequency
speed of light
Planck's constant
E=hy
ground state
excited state
quantum numbers: n, I, rnr, m,
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