____________
_________
Chemistry LN14L: CO
LNT’
Name:
Review
Period:
Packet
Date:______________________
Classification of Matter & Chemical! Physical Changes
1.
are substances that are made up of two or more elements which are
chemically combined
2. &ti)d-vV
is made from two or more substances that are physically combined
3.
are substances that are made up of only one type of atom
4.
is anything that has both mass and volume
5•
is a solid, produced by a reaction that separates a solution.
6. A_____________________________ consists of a solute in a solvent
7. List 2 lab safety precautions.
E/Cn-i.e)+
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8.
Identify the following pieces of equipment:
Rckcy?e EJc
thrtq
I
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C
LA
10. Which piece of equipment is used as a cover for the evaporating dish?
CrueL ;;
1Vt’fr-
aJ,C S
11. Where is the hottest part of the Bunsen burner flame?
rp
oc4
i2er
eoi
12. How do you take a meniscus reading?
-
Eve
iev/
1
-
otbr
_____________________________
13. Define what a heterogeneous mixture
each.
=
and a homogeneous mixture are and provide an example of
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r hope
DO
pcs>
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72
g /&kY
14. Suppose that during a reaction a chemistry student touches the I?eaker and observes that it feels COLD. The
student should conclude that the chemical reaction is
Er1OH4YY 1 Q
a) Why?
Eeg
,
bycI
15, Suppose that during a reaction a chemistry student touches the beaker and observes that it feels HOT. The
student should conclude that the chemical reaction is
I
a) Why?
Q,,
iS
16. Classify the following,s an element, compound, homogeneous mixture or heterogeneous mixture.
a) Table salt
(J2i7 /L3
1
b) Aluminuip
he/-?-F
c) Dirt___________________
d) Sugar water_____________________________
17. Define the terms chemical and physical change
e
i
Sme sziu
18. Classify the following as,Shemical change or physical change.
a) Iron rusting
b) Ice melting
c) Evaporation
/
d) HC1 reacting with g to create H
2 gas________________
PM
19. Another name for a homogeneous mixture is a(n)
20. What are four indicators of a chemical reaction?
ei pfrdt)
...
/e4i?
-puS
2
Jy
____________mL
____________g
_________________________
Measurement & Density
1. What is the difference between a qualitative measurement and a quantitative measurement?
p,i/tS
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2. ‘mL
“
/jj
yDt
Levi •11’)
ç ç
is a unit that measures
3. “cm” is a unit that measures
4. g” is a unit that measures
5. “mm Hg” is a unit that measures
6. “K” is a unit that measures
7. What is the difference between accuracy and precision?
C-
Clos-e
ap VlV
evr
/ jtLh t*ke
8. Try these conversions:
a. 5000mg
b. 1L=
9. Write the following numbers in scientific notation.
7. ‘/ )( 7t
a. 74,600 km
‘1 ‘/3
b. 0.0443 km
‘‘
X/’
10. Write the following numbers in ordinary notation.
a. 7
8.5xlO
k
m
5O) OO
b. 4
9.67x10
k
m
00
Oo97
11. Define density.
mAcc
.
0
T
71
—
12. Find the density of an unknown solid given that a 5.62g sample occupies 2.35 cm
3
2
3c3
__________
Atomic Structure, Quantum Numbers, and Electron Notation
1. proton
a. the total number of protons and neutrons
in the nucleus of an atom
b. the weighted average mass of the atoms
in a naturally occurring sample of an element
c. 1/12 the mass of a carbon-12 atom
2. atom
3. mass number
4. atomic mass unit
4
c3
1.
d. the number of protons in the nucleus of an
element
e. atoms with the same number of protons
5. electron
but different number of neutrons
f. negatively charged subatomic particle
g. the smallest particle of an element that
retains the properties of that element
h. a counting unit; 6.022 x 1023
i. positively charged subatomic particle
j. subatomic particle with no charge
6. mole
7. average atomic mass
8. atomic number
9. neutron
10. isotopes
Suppose an atom has 27 protons and 32 neutrons. What is the mass number?
2. Suppose an atom has 29 protons and 35 neutrons. How many electrons does it have?
Z
3. Suppose an isotope has a mass number of 27 and an atomic number of 13.
71 27
a. Write the hyphen notation for this isotope.
b. Write the nuclear symbol for this isotope.
2
4. What is electromagnetic radiation? Provide examples.
dt116I2
/hA- 4k/Y
1 Vrtyç
cLtcws
-
5. What is the BEST way to describe the nature of an electron?
t2 oLV AVZ
6. Fill in the chart below. What do the four quantum numbers indicate?
Spin Quantum Number
I
0v7
t(-Y?
r’E
4
7. One orbital can hold a MAXIMUM of
Z
electrons.
8. What it the correct electron configuration notation and orbital notation for Na and Al
Diagonal Rule:
j$i
Z
I
J
2
ç
0
Periodic Table
are elements that show the properties of both metals and nonmetals.
.
2. How are elements arranged on the Periodic Table?
3. What is electronegativity?
abi
4c
4. What is the most electronegative element?
5. Write whether an increase or decrease of a trend occurs as you go across the Periodic Table from icfi
to right in a period, and when you go from top to bottom in a group.
Trend
1st Ionization Energy
4-
Atomic radius
Electronegativity
Across a Period
Down a Group
_____j).
_____
_____
_____
What name is given to the following?
6.
a.
Group #1 Elements:
b.
Group #2 Elements:
c.
Groups #3-12 Elements:
d.
Group #18 Elements:
e.
Group #17 Elements:
Mi—Efr2
iç
.
7. Use the elements from part of period three, listed below, to answer the following questions. Write the
symbol of the element described in the blank provided. (lpt.each)
j
11
18
Na
Mg
Al
Si
P
S
Cl
Ar
22.99
24.30
26.98
28.09
30.97
32.07
35.45
39.95
/l]6k. i). an element in the same group as potassium (refer to
a). an element with 15 electrons
wall chart to find potassium-K)
IU& b). the most reactive metal
(
17
16
15
14
13
12
an element that forms an ion with a charge of—2
c). the most reactive nonmetal
(4
‘i
d). an element with 12 protons
k). an element with a atomic number of 14
e). an element with the atomic number of 17
f). the MOST stable element
h). an element in the halogen group
Bonding
1. A bond where there is a sharing of electrons:
d) ionic
b) electronegativity
a) mutual
2. A bond where there is transferring of electrons so an attraction between positive and negative ions is
established:
b) electronegativity
a) mutual
c) covalent
3. What is the difference between no,polar covalent and polar covalent bond type?
hS
C
avalL
4. How many valance eleetfons are und in the following groups?
a. Group 1
b. Group 2
c. Group 13
d. Group 14
e. Group 15
f. Group 16
g. Group 17
h. Group 18
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)
6
5. Circle the lone pair electrons in the following dot formula of water.
6. With respect to bonds formed between the following pairs of atoms:
• Determine the electronegativity difference. SHOW WORK!
• Determine the probable bond type (ionic, polar covalent, or nonpolar covalent).
• Assign partial charges to atoms that are part of a polar covalent bond.
Pairs of
Atoms
Electronegativity
Difference
Probable
Bond Type
Partial Charge (if
polar-covalent)
HandH
SandO
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KandBr
7. A molecule is a
/lC
/.Vht I
group of atoms held to together by
L bonds.
(‘nLjZ 111-7 7
8. What is the difference between a cation and an anion?
i
?,
6,’e
/&
e
,1
9. List the naturally occurring diatomic elements?
2 AJ Ci
k’
10. What is the molecular geometry of BF
3
Tn
onai
11. What is the molecular geometry of CH
4
7phd
12. What is the molecular geometry of CO
2
a.
o=c=o
a,
a,
7
_______________________
________________________
________________
_____________
_______________
___________________
Writini Formulas & Chemical Equations
Name the following:
Write formulas for the following:
2hg i-e
Ci’cmrn,irn OXi-t
)
PO
3
Pb
2
)
4
Zinc chloride
3
0
2
Cr
Aluminum hydroxide_________
1. What are the four types of chemical reactions? Write a simple equation to represent each type of reaction.
s/ S
A+
-
8
je p
—)
2. The empirical formula is the
implest whole number ratio
c) actual mole ratio
b) actual composition
3. A compound that contains water is called a(n)______________
hydrate
b) hydroxide
d) none of these
c) anhydrate
4. A calculation that determines the mass/mass or mass/mole relationship is
a) quantitative
d) molar mass
3stoichiometry
b) qualitative
5. The substance that comes through the funnel during the filtering process is the
a) filter residue
b) the filter paper
cjlt!:at,
6. Heating until you get a matching weight is referred to as
d) the decant
a) being careful b) following directions c) heating to accuracy 3Nieating to precision
7. A hydrate that has been heated until dr is a
a) decomposed anhydrous
c) hydrated
d) oxidized
8. An insoluble product that forms from the reaction of two liquids is called
a) solute
precipitate
c)flakes
d) residue
9. To balance an equation, one uses______________
a) subscripts
b) roman numerals
coefficients d) stoichiometry
10. The law of conservation of mass states that the mass of the reactants must be
products
a) greater than
b) less than
gLtQ
the mass of the
d) cannot be determined
11. Tarring (re-zeroing) the scale is taking into consideration the
a) mass of a substance
m
emt&tainer
+3Ca(OH) 3
(S0 2
2
A1
3
)
I 2.When the equation 4
-2Al(OH)
Ca(OH), is______________
3
b)2
c)l
+
c) mass of the reactants
4 is correctly balanced, the coefficient for
3CaSO
d)4
(S0 and CaSO
2
A1
3
)
?
4
13. Using the equation in #12, what is the mole ratio between 4
a)2:3
b) 1:2
c)2:3 l:3
d)mass of the products
_______
14. A substance that increases the rate of a reaction without itself being changed is a(n)
a) precipitate
catalyst
c) inhibitor
d) none of the above
15. What is a reversible reaction? How is a reversible reaction represented’?._..
ZF2
16. Label the products, reactants and yields arrow.
yic
4
CH
+
202
2
CO
+
0
2
2H
17. Fill in the correct symbol that would used when writing a chemical equation based on the meaning provided.
Meaning
Symbol
—?
“yields” indicates result of a reaction
Indicates a reversible reaction
ç’
j,
A reactant or product in the solid state
J
A reactant or product in the liquid state
a
Alternative to (s); used only for a precipitate (solid) falling out of solution
A reactant or product in aqueous solution (dissolved in water)
A reactant or product in the gaseous state
1’
A.,
21
Alternative to (g); used only for a gaseous product
Reactants are heated
Pressure at which the reaction is carried out, in this case 2
Temperature at which reaction is carried out, in this case 0°C
114
—
A catalyst is used to speed up the reaction rate, in this case Mn02 would be used
to speed up the reaction rate.
9
Kinetic Theory, Solids, Liquids, Gases, Phase Chan2es
1.
Name the 3 parts of the kinetic molecular theory.
41
15
K
PtI 7#4iOc’
‘t
M( Colli.ni&
th’
I-i
117
e9nS,it 41’M2
’
6ç7
flerjy 1
ttkf
2. How does temperature affect the kinetic energy of a substance?
-
‘TV
‘
?-Ch1?,
3. List the values for STP.
/
Pt-c
cui-r
o
7omm&,
/4ii, /‘‘
4, If the volume of a gas is decreased, then gas pressure will
P’
ei€
5. If the volume of a gas is increased, then gas temperature will______________
6. How does eva oration differ from sublimation?
7. Complete the chart by identifying the correct phase of matter.
Phase
c’/
/
Shape
Volume
AvQ. Kinetic
Enerqy
befinite
befinite
Slow
befinite
Medium
Particle SpacinQ
Particle Motion
Very close
together
Moderately
spaced
Vibrating in a
fixed position
Vibrating around
moving points
Continuous,
ran dom motion
d
tiq i,,
‘d
p
Not
befinite
Not
befinite
Not
befinite
Not
befinite
Not
befinite
Fast
Very far apart
Very fast
Very far apart
IM Forces
Most significant
Less significant
Little to none
Little to none
Violent
8. What is the difference between a crystalline solid and an amorphous solid?
v 1a- I/k13 p&i*.frii
n4 )Iltirj 7O It) ic
Iliô tLUc4 i/’fAq
rwç
Alo Ct*r
9. Which of he 4 phases of matter is consired to have the most significant intermolecular forces?
5L li
a) The least significant intermolecular forces?
—
C
10. A liquid will boil when its equilibrium vapor pressure EQUALS
11. When a system at equilibrium is disturbed by apic tion fa stress, it attains a new quilibm position that
minimizes the stress. This is known as
t/
5
10
12. Use the phase diagram below to answer the following questions:
a.
c.
C
b. The area on the graph that represents the liquid phase is: E
The area on the graph that represents the gas phase is:
I
The area on the graph that represents the solid phase is:_______
1,5
p
d. When does the triple point occur?
B
A
(atm) LO
‘
o.5
e. What happens ;o a substance as you move from point A to point
B?________________
C
30 O 70 0 110 130
TC)
Mixtures: Solutions, Suspensions & Colloids
I. Define the following terms: solution, colloid. suspension
mcoooç m x’u,
ojL II
rna//s* 1a*c
t1€t7L5
f//7 O9toc
2.
’7
Suppose 15 g of sugar is dissolved in 1000 g of water. The sugar is the/(1/( and the water is the) /Veti
3. Explain what the phrase “like dissolves like” means and give an example
5i
x!
4. Explain the difference between an unsaturated, saturated and a supersaturated solution. Define these terms!
Ths
i
h
h/d
L.p /
/ç
7
2
Uh5#
5. What 3 things can increase the rate at which a solute will dissolve?
7. How could you identify a colloid?
74//
fr
7
1
t
Ai’fi/
1aM jF
/-
7l
___
Acids/Bases/Salts
1. Describe acids and bases according to the theory of Arrhenius.
re1ea i/ n O
?4-
//
,‘2tieLc(
-
I
67
y117 O
Explain how blue and red litmus paper determine if a substance is an acid, base or salt.
2.
ed /c ned,
B/vt
B/
nS A
ecj
Explain the process of neutralization using a chemical equation.
3.
3
4
z
4.
a/
Define pH and draw the pH scale showing the locations of acids, bases, and neutral substances.
0
o
5.
f
19
2 is produced?
2 or H
What happens during a splint test? How do you know 02, CO
/‘ c/7
a
ç
cp
/
9
2
/>i d5 aiJ
2
y
?&p,’ -q
tlfld
Nuclear Chemistry
1. Name and describe each of the 3 types of radiation.
I
z
Oh
kped
4
F
,-
/
e
2. What is a half-life?
Oi 9•.
Th
3. Write the nuclear symbol and the hyphen notation for an isotope of phosphorus with a mass number of 32.
1/
32?
12
4. What is the difference between fission and fusion?
M
1
Hh
DiY
5. Balance the following nuclear reactions.
2/0—s
—
b + He
2
P
±
-*
He
I
I
I
I
I
I
I
II Thinqs to study:
o ALL Notes
o Labs
o Ieview Guides (Content & Math)
N
o Mrs. Hostetter’s website (review PowerPoints)
o www.epasd.org/hostetter
II
I
The ACCUMULATIVE Final Is Worth 100 points:
o 100 multiple choice questions
STUbY&GQOb LUCK!!
=
=
=
=
=
=
=
=
=
=
=
=
=
=
=
=
=
11
13
__
4ThRevIew
Chemistry LND4L:
Period:_____
Name:
Calculate the molar mass of iron (II) phosphate. 358g
1.
3
D
LIb
Find the percent composition of sodium carbonate. ‘oNa=43’o,%Cll%,4Q44
2.
Q
3
C
2
112
I
/0
(,z)
iJ
3
3.
atoo
Convert 6.25 g of sodium cloride to moles.
/
T
25
mi
/ AItC/
(6eA37
4.
Convert 0.500 mol of potassium iodide to grams. 83g
,
I
5.
//k
What is the empirical and molecular formula of a compound with the following percent composition:
P = 26.7%, N = 12.1 %, Cl = 61.2%. The molar mass of the compound is 695 g/mol.
c!MF=f6N6cJ12
?LZ1411D
0
i
1
O
Jmo/
I
3
5
1L
;O
t
rvc
:
fr-ô1/’
,)-
5
ii1’
3
l
Is
11
f
3
6. How many grams of sodium phosphate are needed to completely react with 25.0 g of barium chloride.
i32O5g
3tn1
&2
2 at 20°C and 98.5 kPa.5.79L
7. Calculate the volume of I 5g of SO
G, z)
L/95O7
(v
‘
8.
(° Z39,o
ylio1k
(z9
Calculate the pressufTñmm Hg of 0.639 mol of neon at 22°C & occupying 18.5L.
557mmHg
?Vtni€r
(c’C62
(/
I
9. Write the electron configuration notation, orbital notation, and the Lewis electron dot symbol for arsenic.
\/a4Me.
$
e
4s:
Is
10. Suppose a g is collected in 145 mL flask whef-tfle temperature of the gas is 23°C and the pressure of the
gas is 785 mm Hg. Calculate the volume of the gas at STP. .1.38432.m.L
PI
i
_
1
t
1
‘II -/‘/c
-7
—
T/
23°C *173
.-2-9 ?
\j
7v
5
Wrfrv3f
Z73k>)
mL
II. Suppose 25.0 mL of a gas is at 24°C. Calculate the temperature at which the gas will occupy 30.0
assuming constant pressure. 356.4K
I
VI
29 7/c
73
T
“i’
L
) (z)
‘2;
percent error if the string is
12, Suppose the length of a piece of string is measured to be 33.45 cm. Calculate the
actually 34.50 cm long. 3.04%
=
/
1’keo—
stoichiornetry calculations it
13. Suppose 4.25 g of sodium chloride is collected after a chemical reaction. Through
t yield.,.5q
is determined that the theoretical yield of sodium chloride is 5.00 g. Calculate the percen
fltecrchcct/
7/CO
months. How much of the
14. Suppose an unknown radioactive substance with a mass of 120 g has a half-life of 6
substance will remain after 2 years? 75g
h1-r
—
D:
j( I-r
ivc5
9j
13