Academic Chemistry
UNIT 9 (Chapter 9)
STOICHIOMETRY
Name:
Class Period:
Test Date:
1
2/9/15
Calendar
Monday
18
Tuesday
19
Wednesday
20
Thursday
21
Friday
JANUARY 22
Mole Review
Investigation: All
that remains
HW: pg. 3
29
25
26
27
28
Mol to mol
conversions
Mass to Mass and
other conversions
QUIZ
HW: pg. 7
FEBRUARY 1
HW: pg. 10
2
Extra
Stoichiometry
Practice
HW: pg. 12
3
4
HW: Finish Lab
5
Limiting Reagent
Percent Yield
Stoichiometry Lab
Stoichiometry Lab
HW: pg. 15
8
Limiting Reagent
Practice
Day/Percent Yield
9
HW: pg. 21
10
HW: Test Review
11
HW: Test Review
12
Test Review Due
UNIT 9 TEST
Begin Gases Unit
S’MORE’S LAB
P.15-16
HW: Study
Scan to take you to the KHS Academic Chemistry Website!
2
MOLE REVIEW
For conversions between mass, volume (of a gas), and number of particles, we use the
___________________________to guide our use of _____________________
_________________________.
Chemical Conversion Factors to Know:
1 mole = molar mass (g)
1 mole = 6.02 x 1023 particles (atoms, ions,
molecules, formula units)
1 mole = 22.4 L of a gas at STP
STP = standard temperature and pressure
(T = 273K, P = 1 atm)
With dimensional analysis, you multiply the given by one or more conversion factors in the form of a
fraction.
Example:
Practice Problems
1. What is the mass of 4.00 moles of oxygen gas?
2. What is the volume of 3.4 x 1025 molecules of CH4 at STP?
Homework Problems:
3. What is the mass of the helium inside a balloon with a volume of 2.3 liters?
4. How many moles of water are in a 45 gram sample?
3
Investigation: All That Remains
Predict the outcome and then test your prediction: How much solid mass will remain after decomposing 2.00g
of sodium hydrogen carbonate by heating? (Hint: 2NaHCO3(s) -> Na2CO3(s) + CO2(g) + H2O(g))
Prediction (include your reasoning):
Design: Plan your investigation with your team. Write your procedure, including any diagrams, in the space
below. Be prepared to discuss your plan with the class.
Safety: Discuss safety precautions that must be used and list them below.
Investigate: After class discussion, write in the space below any changes to your original procedure.
Data and Calculations:
Analysis and Conclusions:
1. How did your final mass compare with your prediction?
2. What did you observe as you heated the sodium hydrogen carbonate?
3. Does your final mass measurement include either the water or carbon dioxide products? Explain.
4. Does your result match your prediction? Why or why not?
4
MOL TO MOL CONVERSIONS
RECALL: Balancing Chemical Equations
Directions: Using coefficients, balance the following equation -
____ C6H6 + ____O2 → ____CO2 + ____H2O
Cooking Analogy:

Grill Master K.T. Tiger has the art of grilled cheese sandwich making down to a science. The Grill
Master's recipe requires 2 pieces of cheese between 2 slices of bread, grilled to perfection. What is the
coefficient ratio of the ingredients to the product?
2
+
2
→
____ : ____ : ____

Grill Master Tiger knows that a 20 pack of sliced bread and a 20 pack of sliced cheese will always make
the same number of grilled cheese sandwiches with no leftovers. How many?
____________________________________________________________________________________

What happens to the Grill Master's grilled cheese sandwiches if he changes the quantities of
ingredients? Will he have enough ingredients? Will there be leftovers?
____________________________________________________________________________________
o
Practice grilled cheese sandwich making here:
http://phet.colorado.edu/en/simulation/reactants-products-and-leftovers
What Cooking Really Is...
STOICHIOMETRY:


_____________________________________________________________________________________
N2 (g) + 3H2 (g) → 2NH3 (g)
o How many molecules of each reactant are required to produce 2 molecules of product? Ratio?
o
______________________________________________________________________________
How many moles of each reactant are required to produce 2 moles of product? Ratio?
______________________________________________________________________________
Instead of cups, teaspoons, or tablespoons, we have…
1. ______________________________________________:

___ molecule of nitrogen gas reacts with ___ molecules of hydrogen gas to produce ___ molecules
of ammonia gas.

It's always in the same coefficient ratio; just like 2 slices of bread plus 2 slices of cheese produce 1
grilled cheese sandwich!
5
2. ______________________________________________:

___ mol of nitrogen gas reacts with ___ mol of hydrogen gas to produce ___ mol of ammonia gas.
3. ______________________________________________:

Law of conservation of mass says mass of reactants must ________________ mass of products.

Mass of nitrogen gas = _________ and mass of hydrogen gas = ________

Their sum equals the mass of the products = ____________
4. ______________________________________________:

1 mol of gas = __________________ at Standard Temperature and Pressure (STP)
o
_________ L of nitrogen gas reacts with __________ L of hydrogen gas to produce ________ L
of ammonia.
Mol to Mol Conversion Calculations:


N2 (g) + 3H2 (g) → 2NH3 (g)
What is the mole coefficient ratio of the above equation?
____ : ____ : ____

Because we know the ratio, we can calculate to find the number of moles of another substance.
Example: How many mol of NH3 are produced when 0.60 mol of nitrogen gas reacts with hydrogen gas?
Practice Problems
Directions: Using the balanced chemical equation, calculate the following mol conversions -
MnO2 + 4HCl → MnCl4 + 2H2O
1. How many mol of H2O are produced when 3.20 mol of MnO2 reacts with hydrochloric acid?
2. How many mol of HCl are consumed (used) when 1.65 mol of Manganese (IV) chloride are produced?
3. How many mol of water are produced when 4.35 moles of MnCl4 are also produced?
6
Homework: Interpreting Coefficients as Moles
Directions: Given the equation, calculate each of the following; balance the equation if necessary -
____CH4 (g) + ____O2 (g) → ____CO2 (g) + ____H2O (g)
1. How many mol of carbon dioxide (CO2) are formed when 40 mol of oxygen (O2) is consumed?
2. How many mol of methane (CH4) are needed to form 200 mol of water?
3. How many mol of oxygen (O2) combine with 0.05 mol of methane (CH4)?
____NO (g) + ____O2 (g) → ____NO2 (g)
4. How many mol of oxygen (O2) combine with 500. mol of NO?
5. How many mol of NO2 are formed from 0.25 mol of NO?
6.
a. If you have 80. mol of NO, how many mol of oxygen (O2) would you use?
b. If you had started with 200. mol of oxygen (O2), how many would you have left?
7
MASS TO MASS AND OTHER UNIT CONVERSIONS
RECALL: The Mole Highway...it's been expanded and construction is complete!
Like before, the Mole Highway can be used as a map toward setting up an appropriate conversion
HOW IT'S USED:
1. Find the starting point; use the value, substance, and unit you are given
2. Find the ending point; use the value, substance, and unit are you being required to solve
3. You must stay on the highway!!!
4. Each road taken represents 1 step in your conversion!
5. Once the destination is reached, solve mathematically by multiplying across the top, multiplying
across the bottom, and dividing the top value by the bottom value.
NOTE:
1. Before any math can be done, a BALANCED CHEMICAL EQUATION is required.
2. If the starting value isn't in the unit "mol," your first step is to convert it there.
3. Going from mol of substance A to mol of substance B requires a Mol to Mol conversion; USE YOUR
COEFFICIENTS FROM THE BALANCED CHEMICAL EQUATION!
Mass to Mass Conversion Calculations
 N2(g) + 3H2 (g) -> 2NH3 (g)
 Like yesterday, in order to go from the mass of one substance, to the mass of a new substance, a mol to
mol conversion will be necessary.
Example: Calculate the number of grams of NH3 produced by the reaction of 5.40 g of H2 with excess N2 (g).
8
Practice Problems - ALL UNITS
***Write a balanced formula, and then set up your conversion calculations.***
1. How many grams of O2 (g) are produced when a sample of 29.2 g of water decomposes?
2. Using the same equation, how many liters of hydrogen gas are produced when 1.33 x 1017 molecules of
water decompose?
2SO2 (g) + O2 (g) → 2SO3 (g)
3. How many liters of O2 are needed to produce 19.8 L of SO3?
4. How many molecules of oxygen are consumed in the formation of 187.4 L of SO3?
5. How many molecules of Sulfur dioxide are consumed in the formation of 4.41 x 1027 molecules of sulfur
trioxide?
9
Homework: Mixed Mole Conversions
1. Find the molar mass of the following:
a. 1 mol of CH4 = ____________g of CH4
b. 1 mol of Ag2SO4 = _______________g of Ag2SO4
c. 1 mol of P2O5 = _____________g of P2O5
d. ___________g of NaBr = 1 mol of NaBr
e. ___________g of Al(NO3)3 = 1 mol of Al(NO3)3
f.
___________g of Ba3(PO4)2 = 1 mol of Ba3(PO4)2
CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O (g)
2. How many moles of O2 are needed to produce 5.2 moles of CO2?
3. How many liters of CH4 are needed to produce 0.38 grams of H2O at STP?
4. How many molecules of CO2 are produced from 12.9 grams of O2?
10
Mass, Volume, and Particle Stoichiometry Extra Practice
Balance:
___Ba3(PO4)2 + ___HI (g)  ___BaI2 + ___H3PO4
1. How many grams of BaI2 are produced from 4.37 x 1027 molecules of HI?
2. How many formula units of BaI2 are produced from 96.2g of HI?
3. How many grams of H3PO4 are produced from 2.0 moles of Ba3(PO4)2?
4. How many liters of HI are needed to produce 72.54g of BaI2 at STP?
5. Practice drawing the expanded Mole Highway from memory. Remember, the only addition is that Mol
can now be converted to Mol.
11
Homework: Mass, Volume, and Particle Stoichiometry
1. If you have 1.91 x 1025 molecules of ethane (C2H6), how many molecules of oxygen are needed to react
completely? (molecules= particles!)
C2H6 + O2  CO2 + H2O
2. Aluminum and sulfur react to produce aluminum sulfide. How many grams of sulfur are needed to
produce 18.62 grams of aluminum sulfide?
3. Ammonia and water combine to produce ammonium hydroxide. At STP, how many liters of water are
needed to produce 6.54 liters of ammonium hydroxide?
4. How many atoms of phosphorus are needed to produce 16.0 x 1024 molecules of phosphine (PH3)?
(atoms & molecules = particles!)
P + H2  PH3
5. How many grams of oxygen are needed to produce 6.55 x 1024 formula units of potassium oxide?
K + O2  K2O?
6. How many liters of hydrogen gas will be produced if 38.5 g of hydrochloric acid reacts with zinc?
Zn + HCl  ZnCl2 + H2
12
Limiting Reagents (Reactants)
Back to cooking…
1. What is Grill Master Tigers' recipe for grilled cheese sandwiches?_______________________________________
2. What happens if the Grill Master receives only half of his order of cheese for the day?____________________
3. So, in this case, what is limiting the number of grilled cheese sandwiches he can make? ___________________
4. What if the Grill Master received 3 times the amount of cheese he needed?_____________________________
5. What would be limiting him in this case? ________________________________________________
Limiting Reagent (aka Limiting Reactant)
 The same thing applies to chemical reactions…



N2 (g) + 3H2 (g) → 2NH3 (g)
___ mol of N2(g) reacts with ___ mol of H2 (g) mol to form __ mol of NH3 (g).
What happens if you only have 0.5 mol of nitrogen gas?
_____________________________________________________________________________________

How much hydrogen gas would you use?
_____________________________________________________________________________________

How much ammonia would you make?
_____________________________________________________________________________________
 Limiting Reagent/Reactant:______________________________________________________________
_____________________________________________________________________________________
 Excess Reagent/Reactant:__________________________________________________________
_____________________________________________________________________________________

Example: Sodium chloride can be prepared by the reaction of sodium metal with chlorine gas.
Suppose that 6.70 mol of Na reacts with 3.20 mol of Cl2. What is the limiting reagent?
Follow these five steps….
 Step 1: ______________________________________________________________________________
 Step 2: ______________________________________________________________________________
 To do this, convert the given info for each reactant (mol, in this problem) to mol of product.
 If the original substances are given in grams, you’d have an extra step – converting mass to moles –
but the rest of the process would be the same.
 NOTE: If the original substances are given in grams, what do you need to do before this step?
o Convert to mol.
13
 Step 3: ______________________________________________________________________________
 You will have _____ answers for moles of product. Why? _________________________________
________________________________________________________________________________
 So which one do I use? _____________________________________________________________
 The __________________ of the two answers is the ______________________________ because
you only have enough reactants to make that amount. You will run out of the reactants before the
larger amount is made.
 From this, you can figure out your limiting reagent and excess reagent.
 Step 4: ______________________________________________________________________________
 Once you know your maximum product, look all the way to the ________ of that calculation. The
reactant that produced that smaller amount of product is your _____________________.
 It “limited” you to making the ______________________________________________.
 The other reactant – that started the other calculation – is the _________________________.
 Step 5: ______________________________________________________________
 Convert mol of your limiting reagent to mol of product (or whatever the original question asks for).
Practice Problem
2Cu (s) + S (s) → Cu2S (s)
1. What is the limiting reagent when 80.0 g Cu reacts with 25.0 g of S?
2. What is the maximum number of grams of Copper (I) sulfide produced?
14
Homework: Limiting Reagent/Reactant
Directions: Reference Notes #3 to complete the following Limiting Reagent word problems. Find a balanced
chemical equation if necessary and follow the four steps.
1. What mass of water can be produced from 2.0 mol of H2 and 4.0 mol of O2?
2. What mass of water can be produced from 16 g of H2 and 8 g of O2?
3. What mass of water can be produced from 0.49 g of H2 and 1.3 g of O2?
4. What mass of water can be produced from 3.5 mol of H2 and 4.5 mol of O2?
____Cu + ____AgNO3 --> ____Cu(NO3)2 + ____Ag
5. How many mol of Ag can be produced from 6.3 mol of Cu and 4.2 moles of AgNO3?
6. What mass of Cu(NO3)2 can be produced from 5.5 g Cu and 1.95 g AgNO3?
7. How many mol of Ag can be produced from 1.5 g Cu and 7.2 g of AgNO3?
15
Percent Yield
Cooking, yet again… 
 Grill Master Tiger's recipe yields 10 grilled cheese sandwiches when 20 slices of bread and 20 slices of
cheese are used

So, the recipe tells you the theoretical yield: ________________________________________________
_____________________________________________________________________________________

What you actually make is the actual yield: _________________________________________________
_____________________________________________________________________________________

Percent yield:
_____________________________________________________________________________________
_____________________________________________________________________________________
 Formula: ____________________________
x
100
Food for Thought: Could the percent yield normally be larger than 100%? Smaller? What might cause the %
yield to vary?
Example: Using the following equation, what is the theoretical yield of CaO if 24.8g CaCO3 is heated? What is
the percent yield if 13.1g of CaO is produced?
 Follow the steps below…
o Step 1: Convert grams of the given substance to grams of the questioned substance.
 Which means…

o
24.8 g of CaCO3 = _____g of CaO.
Step 2: Use the formula to find percent yield.
16
Homework Percent Yield Applications
Directions: Reference Notes #4 to complete the following percent yield word problems. All work must be shown.
1. A baker has a recipe for cookies that says he can bake a yield of 250 cookies. However, when he does
bake them, he finds that he can only make 125. What is the percent yield?
(Assume that all cookies are the exact same size as directed by the recipe)
2. A chemist runs an experiment and produces 100 g of sulfuric acid. The All-Knowing Chemistry Book
states he should have made 123 g of sulfuric acid. What is the percent yield?
3. A farmer out checking his fields looks in on his Hawaiian flower tree. He notices only 15 blooming
flowers. This is 73% of what it should be. What is the Hawaiian flower tree’s theoretical yield?
4. A man shelling pecans notices that each pecan is only producing 39% of the meat expected. In the
Pecan Man’s Handbook, he reads that each pecan should have a mass of 200 g. What is the actual yield
of each pecan?
5. Genny collected 1.05g of sodium carbonate by decomposing 2.00 g of sodium hydrogen carbonate.
According to the chemical equation
She should have been able to collect more. Use stoichiometry and the percent yield equation to find the
percent yield of Genny’s experiment.
17
Academic Chemistry Unit 9 Test Review (Due on Feb 8th)
STOICHIOMETRY TEST on Tuesday, February 9th
1. Define the following:
a. Stoichiometry
b. Limiting reagents
c. Excess reagents
d. Percent Yield
e. Actual Yield
f.
Theoretical Yield
2. Find the molar mass of the following:
a. __________g of CS2
c. _________g of P2O5
b. __________g of Ag3PO4
Directions: Balance the following equations and perform the appropriate conversions and calculations.
____HCl  ____H2 + ____Cl2
3. How many grams of HCl are needed to produce 5.2 moles of Cl2?
4. How many moles of H2 are produced from 6.3 L of HCl at STP?
18
5. How many moles of Cl2 are produced from 12.9 grams of HCl? (see equation on previous page)
____BaSO4 + ____HI (g)  ____BaI2 + ____H2SO4
6. How many moles of BaI2 are produced from 7.6 moles of HI?
7. How many grams of BaI2 are produced from 9.2L of HI at STP?
8. How many grams of H2SO4 are produced from 2.0 moles of BaSO4?
9. How many molecules of HI are needed to produce 72.54g of BaI2?
10. What is the volume of H2SO4 produced from .035 grams of HI at STP?
19
11. Balance the following equation and answer the questions that follow:
 ____Fe3O4
____Fe + ____H2O
a.
+ ____H2
What is the molar mass in grams of iron IV oxide?
b. What is the limiting reagent if 36.0g of water reacts with 167.0g of Fe?
c. Using the information in part b, If only 105 grams of Fe3O4 were produced, what is the percent
yield of the reaction?
20
STAAR CHEMISTRY
REFERENCE MATERIALS
c = fX
Speed of light = (frequency)(wavelength)
Ephoton =hf
Energy = (Planck's constant)(frequency)
Energy =
(Planck's constant)(speed of light)
Ephoton
(wavelength)
sum of the partial pressures )
Total pressure of a gas =
PT=PI+P2+P3+ ...
of the component gases
(Pressure)(volume) = (moles)(ideal gas constant)(temperature)
(Initial pressure)(initial volume)
(final pressure)(final volume)
(Initial moles)(initial temperature)
(final moles)(final temperature)
(Initial pressure)(initial volume) = (final pressure)(final volume)
(Initial volume)
(final volume)
(Initial temperature)
(final temperature)
PV = nRT
nlh
n2T2
p,v, = 5vÿ
v, 5
(Initial volume) = (final volume)
(Initial moles)
hc
Vi _ V2
(final moles)
ni
moles of solute
Molarity =
n2
mol
M-
liter of solution
L
,on)(hydrox,de,on) H+lroH
1
w
Ionization constant of water = ÿ concentration concentration
1 ]ÿ solution
= ( solutionÿf)
2 ]1volume
solution
( solution
Volume
of ]/molarity
of l/molarity 2f)
pH =-logarithm (hydrogen ion concentration)
specificl( change in )
Heat gained or lost = (mass) heat J[temperature
Enthalpyof / enthalpy ) ( enthalpy )
reaction = [of products - of reactants
ViMI=V2M2
pH = -Iog[H+]
C) = mc AT
p
zÿH= AHÿ(products)
o
- zÿHf(reactants)
STAAR CHEMISTRY
REFERENCE MATERIALS
mass
Density =
volume
m
D -- -V
.
[ accepted value - experimental value ÿ
wercenÿ error = /
ÿ ÿ
(100)
\
accepted value
/
(. actuo[ ield )
Percent yield = \ theoretical yield (100)
Avogadro's number = 6.02 x 1023 particles per mole
h = Planck's constant = 6.63 x 10-34 J • s
c = speed of light = 3.00 x 108 m
s
z4[ ÿmol 2
Kw= ionization constantofwater = 1.00x10-ÿT)
alpha particle (ÿz) 4
= He
beta particle 0
(13) =neutron
_1e
01n
=
standard temperature and pressure (STP) = 0°C and 1 arm
0°C = 273 K
volume of ideal gas at STP = 22.4
L
mol
lcm3 = lmL = lcc
1 atm = 760 mm Hg = 101.3 kPa
R = ideal gas constant = 0.0821
- 8.31
= 62.4
mol. K
mol. K
mol. K
1 calorie (cal) = 4.18 joules (J)
1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal)
..... £ ': ,. "
1. Non-zero digits and zeros between non-zero digits are always significant.
2. Leading zeros are not significant.
3. Zeros to the right of all non-zero digits are only significant if a decimal point is shown.
4. For values written in scientific notation, the digits in the coefficient are significant.
5. In a common logarithm, there are as many digits after the decimal point as there are
significant figures in the original number.
7
6
5
4
3
2
1
3
104
103
88
(262)
(226)
Radium
(223)
Francium
(267)
Rf
7
7B
Actinide Series
Lanthanide Series
60
231.036
Protactinium
232.038
Thorium
(227)
Actinium
91
Pa
Ac
Th
89
90
140.908
Cerium
144.242
(145)
61
Pm
Hassium
(270)
108
Hs
190.23
Osmium
Os
76
Ruthenium
101.07
44
Ru
Iron
55.845
Fe
26
8
Silicon
28.086
Si
Uranium
238.029
U
92
Neptunium
(237)
93
Np
Praseodymium Neodymium Promethium
140.116
138.905
Nd
59
Lanthanum
La
Pr
58
Bohrium
(271)
Seaborgium
(272)
107
Bh
(268)
Sg
106
Rhenium
186.207
Re
75
Dubnium
105
183.84
Tungsten
180.948
Tantalum
74
W
Db
(98)
43
Tc
Manganese
54.938
Mn
25
Molybdenum Technetium
95.96
42
Mo
Chromium
51.996
Cr
24
6
6B
Ta
73
Niobium
92.906
41
Nb
Vanadium
50.942
V
23
5
5B
Atomic mass
Symbol
Ce
57
Lawrencium Rutherfordium
Lr
Ra
87
Fr
178.49
Hafnium
Lutetium
Barium
Cesium
174.967
137.328
132.905
Hf
Ba
Lu
72
71
Cs
56
55
Zirconium
91.224
40
Zr
Yttrium
88.906
87.62
Strontium
85.468
Rubidium
Y
39
Sr
38
Rb
37
47.867
Titanium
44.956
Scandium
40.078
Calcium
39.098
Potassium
22
Ti
21
4
4B
Sc
19
3
3B
Ca
20
Sodium
K
24.305
Magnesium
22.990
Mg
12
11
Na
9.012
Beryllium
6.941
Lithium
Li
Be
4
Hydrogen
1.008
2
2A
H
Name
10
11
1B
12
2B
13
3A
14
4A
15
5A
16
6A
17
7A
(281)
Ds
110
Platinum
195.085
Pt
78
Palladium
106.42
46
Pd
Nickel
58.693
Ni
28
(280)
111
Rg
Gold
196.967
Au
79
Silver
107.868
47
Ag
Copper
63.546
Cu
29
Plutonium
(244)
94
Pu
Samarium
150.36
62
Sm
(247)
Curium
(243)
96
Cm
Americium
95
Am
157.25
Gadolinium
151.964
64
Gd
Europium
63
Eu
Meitnerium Darmstadtium Roentgenium
(276)
Mt
109
Iridium
192.217
Ir
77
Rhodium
102.906
45
Rh
Cobalt
58.933
Co
27
9
8B
Thallium
204.383
Tl
81
Indium
114.818
49
In
Gallium
69.723
Ga
31
Lead
207.2
Pb
82
Tin
118.711
50
Sn
Germanium
72.64
Ge
32
Silicon
28.086
Si
14
Carbon
12.011
C
6
Bismuth
208.980
Bi
83
Antimony
121.760
51
Sb
Arsenic
74.922
As
33
30.974
Phosphorus
P
15
Nitrogen
14.007
N
7
Berkelium
(247)
97
Bk
Terbium
158.925
65
Tb
Californium
(251)
98
Cf
Dysprosium
162.500
66
Dy
Einsteinium
(252)
99
Es
Holmium
164.930
67
Ho
Fermium
(257)
100
Fm
Erbium
167.259
68
Er
Mass numbers in parentheses are those of
the most stable or most common isotope.
Mercury
200.59
Hg
80
Cadmium
112.412
48
Cd
Zinc
65.38
Zn
30
Aluminum
26.982
Al
13
Boron
10.812
B
5
Mendelevium
(258)
101
Md
Thulium
168.934
69
Tm
Polonium
(209)
Po
84
Tellurium
127.60
52
Te
Selenium
78.96
Se
34
Sulfur
32.066
S
16
Oxygen
15.999
O
8
Radon
(222)
86
Rn
Xenon
131.294
54
Xe
Krypton
83.798
36
Kr
Argon
39.948
18
Ar
Neon
20.180
10
Ne
Helium
Updated Spring 2011
Nobelium
(259)
102
No
Ytterbium
173.055
70
Yb
Astatine
(210)
At
85
Iodine
126.904
I
53
Bromine
79.904
Br
35
Chlorine
35.453
Cl
17
Fluorine
18.998
F
9
4.003
He
2
14
1
Atomic number
18
8A
1
1A
PERIODIC TABLE OF THE ELEMENTS
STAAR CHEMISTRY
REFERENCE MATERIALS