Chemistry
For Engineers
Lecture Worksheet
Prepared by:
Engr. Andrew Cesar M. Rimando
Chemical Engineer
Faculty College of Education and Sciences
Lorma Colleges
Chemistry for Engineers Worksheet
Page 1
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Significant Figures and Unit Conversion
1. Compute the density of a 5.0 ml computer chip weighing 30 pounds. Express answer in
kg/m3 and in g/ml.
2. Compute the volume capacity of a cylinder with an inside diameter of 2.0 cm and an inside
length of 1.2 inches. Express answer in cubic centimetre and cubic inch.
3. Going abroad to work as a computer engineer, you are asked to accomplish a form asking for
your height in meters. How do you convert your height of 5’ 5” to meters? Express answer in
three significant figures.
Chemistry for Engineers Worksheet
Page 2
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Significant Figures and Unit Conversion
4. The generally accepted normal body temperature is 37OC. If you are in United Kingdom
working in a computer automation company and your body temperature using thermometer
there indicates that your temperature is 101 OF, do you have fever or not?
5. Generally people with blood sugar or blood glucose of 4 to 6 mmol/L are considered not
diabetic. Those who have much higher are considered diabetic like if your blood glucose level is
10mmol/L specially if you are a computer engineer working without any exercise. If you have
an average blood glucose level of 200 mg/dL, are you diabetic? (1mmol/L=18mg/dL)
6. Assuming that blood flows in an aorta near the heart at 1200 mm/s, what is this speed in km
per hour and in miles per hour?
Chemistry for Engineers Worksheet
Page 3
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Electronic Configuration of Atoms
A. As engineers, you should know the basic composition of matter. Write the electronic
configuration of the following common atoms (assuming that they are neutral or uncharged)
based on their atomic number in the periodic table and indicate their number of valence
electrons.
1. Carbon
2. Hydrogen
3. Oxygen
4. Nitrogen
5. Phosphorous
6. Potassium
7. Sulfur
8. Silicon
9. Chlorine
10. Fluorine
Chemistry for Engineers Worksheet
Page 4
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Intramolecular Chemical Bonds and Electronegativity
A. Draw the Lewis dot structure of the following compounds, indicate if metallic, ionic or
covalent bond, determine the difference of electronegativities between bonded atoms and
predict their shapes.
1. CO2
2. NaCl
3. CH4
4. Steel
5. HCl
Chemistry for Engineers Worksheet
Page 5
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Formula of Inorganic Salts
A. Give the formula of the following salts and research one importance of each to our body.
1. potassium phosphate
2. sodium sulphate
3. potassium chloride
4. calcium fluoride
5. magnesium phosphate
6. potassium sulphate
7. ferric phosphate
8. calcium sulphate
9. sodium phosphate
10. calcium phosphate
Chemistry for Engineers Worksheet
Page 6
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Naming of Acids and Bases
Give the name of the following acids and bases and research on one use each.
1. HSO3F
2. H2SO4
3. Ca(OH)2
4. HCl
5. HNO3
6. NaOH
7. Mg(OH)2
8. H3PO4
9. H2CO3
10. Sr(OH)2
Chemistry for Engineers Worksheet
Page 7
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Hydrocarbons
Write the structural, condense, line and give the molecular formula of the following
hydrocarbons and research on one use each:
1. propane
2. butane
3. 1-butyne
4. propene
5. octane
Chemistry for Engineers Worksheet
Page 8
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Sigma and Pi Covalent Bonds
Indicate if the statement described or is referring to a sigma bond or pi bond with a carbon
atom by writing the word sigma or pi.
_____________1. The first bond made with any other atom.
_____________2. The second or third bond made with any other atom.
_____________3. This is the only bond present between carbon atoms of alkanes.
_____________4. This bond is present in alkenes and alkynes but not in alkanes.
_____________5. This is the bond between carbon and hydrogen in hydrocarbons.
_____________6. The weaker bond.
_____________7. The stronger bond.
_____________8. This bond is made from leftover p orbitals or carbon.
_____________9. This bond is made from hybridized orbitals of 2s and 2p orbitals of carbon.
_____________10. This is present in double and triple bonds but not in single bond of carbon.
_____________11. This is the only bond present in single bonds of carbon.
_____________12. This bond is present ONLY when a carbon atom has sp2 or sp hybrid orbitals.
_____________13. This bond is the only bond when a carbon atom has only sp 3 hybrid orbitals.
_____________14. This bond is not present in methane.
_____________15. This bond is represented by the 18th letter of Greek alphabet.
Chemistry for Engineers Worksheet
Page 9
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Organic Functional Groups (alcohol and aldehyde)
Write the structural, condense, line and give the molecular formula of the following organic
compounds and research on one use each:
1. 2-propanol (isopropyl alcohol)
2. glycerol (glycerine, triol)
3. butanal (butyraldehyde)
4. propanal
5. ethylene glycol
Chemistry for Engineers Worksheet
Page 10
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Intermolecular Forces
Indicate whether the statement is describing the following intermolecular forces, hydrogen
bonding, dipole-dipole, ion-dipole, ion-induced dipole, London dispersion forces.
Note: The van der Waals’ forces like hydrogen bonds and London dispersion forces is a general
term for intermolecular interactions that do not involve covalent bonds or ions.
_____________1. The force of attraction between the lone pair of an electronegative atom and
a hydrogen atom that is bonded to nitrogen, oxygen or fluorine.
_____________2. This bond maybe described as a strong electrostatic dipole-dipole interaction
involving hydrogen.
_____________3. This bonding is the reason why water has a high boiling point.
_____________4. This bond is also the one that connects the two strands of DNA, between
adenine and thymine and between guanine and cytosine.
_____________5. This is between the positive end of one polar molecule and the negative end
of another polar molecule.
_____________6. The partially positive end of a polar molecule is attracted to the partially
negative end of another.
_____________7. An example of this is the attractive forces between HCl molecules.
_____________8. This force is an attractive force that results from the electrostatic attraction
between an ion and a neutral molecule that has a dipole (polar molecule).
_____________9. An example of this is the force generated between polar water molecule and
a sodium ion.
_____________10. This force consists of an ion and a non-polar molecule interacting.
_____________11. An example of this is a phosphide ion interacting with oxygen molecule in
water.
_____________12. This is considered the weakest intermolecular force.
_____________13. These forces are found between noble gases and between non-polar
molecules.
_____________14. This results when the electrons in two adjacent atoms of different
molecules occupy positions that make the atoms form temporary dipoles.
_____________15. This force is sometimes called induced dipole-induced dipole attraction.
Chemistry for Engineers Worksheet
Page 11
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Organic Functional Groups (ketones and carboxylic acid)
Write the structural, condense, line and give the molecular formula of the following organic
compounds and research on one use each:
1. 2-butanone (ethyl methyl ketone)
2. diacetyl (butanedione)
3. butanoic acid (butyric acid)
4. hexanoic acid (caproic acid)
5. lauric acid (dodecanoic acid)
Chemistry for Engineers Worksheet
Page 12
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Organic Functional Groups (ethers and esters)
Write the structural, line and give the molecular formula of the following organic compounds
and research on one use each:
1. diethyl ether
2. dimethyl ether
3. ethyl hexanoate
4. butyl propanoate
5. ethyl heptanoate
Chemistry for Engineers Worksheet
Page 13
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Organic Functional Groups (amine and amide)
Write the structural and line formula then give the molecular formula of the following organic
compounds and research on one use each:
1. ethylamine
2. diethylamine
3. dimethylamine
4. propanamide
5. ethanamide
Chemistry for Engineers Worksheet
Page 14
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Writing Structures of Organic Functional Groups (alkyl halide)
Write the structural formula and give the molecular formula of the following organic
compounds and research on one use each:
1. dichloromethane
2. carbon tetrachloride
3. CFC-11 or R-11 or Freon-11
4. chloroform
5. R134A or 1,1,1,2-tetrafluoroethane
Chemistry for Engineers Worksheet
Page 15
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Give the name of the following organic compounds:
1.
2.
3.
4.
5.
Chemistry for Engineers Worksheet
Page 16
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
6.
7.
8.
9.
10.
Chemistry for Engineers Worksheet
Page 17
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
11.
12.
13.
14.
15.
Chemistry for Engineers Worksheet
Page 18
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Molar Mass
Calculate the molar mass of the following compounds.
1. Aspirin
2. Amphetamine
3. isopropyl alcohol
4. ethanoic acid
5. guanine
Chemistry for Engineers Worksheet
Page 19
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Moles and Molar Mass
Calculate the moles of the following:
1) 50 grams of butane
2) 100 grams of hydrochloric acid
3) 150 grams of water
4) 200 grams of carbon dioxide
5) 250 grams of ethanol
Chemistry for Engineers Worksheet
Page 20
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Mass and Molar Mass
Calculate the mass of the following:
1. 50 moles of glucose
2. 5 moles of sucrose C12H22O11
3. 20 moles of sodium chloride
4. 5 moles of nitric acid
5. 6 moles of carbonic acid
Chemistry for Engineers Worksheet
Page 21
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Chemical Reaction and Balancing
Write the chemical reaction equation of the following then balance them.
1. Pentane is burned with oxygen gas to produce carbon dioxide and water.
2. During photosynthesis carbon dioxide reacts with water to produce glucose and oxygen gas.
3. Iron reacts with silver chloride in an aqueous solution to form silver metal and ferric
chloride.
4. Ethyl alcohol is oxidized in our stomach to produce ethanal.
5. Barium sulphate is precipitated when barium chloride reacts with sodium sulphate.
Chemistry for Engineers Worksheet
Page 22
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
6. Calcium carbonate is decomposed in high heat to calcium oxide and carbon dioxide.
7. Magnesium metal reacts with oxygen gas to form magnesium oxide.
8. Propanoic acid reacts with ethanol to produce ethyl propanoate and water
9. Hydrogen peroxide is decomposed to water and oxygen gas.
10. Nitric acid reacts with copper to produce copper(II) nitrate, nitrogen dioxide and water.
Chemistry for Engineers Worksheet
Page 23
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Molarity, Molality and Normality
1. What is the molarity of a 2 L solution containing 5 moles of solute?
2. What is the molality of a solution containing 20 moles of solute dissolved in 5 kg of solvent?
3. What is the normality of a 5 Liter solution that contains 5 moles of calcium hydroxide?
4. How many moles solute are there in 2 Liters of 5M solutions?
5. What is the volume of a 5M solution containing 2 moles of solute?
Chemistry for Engineers Worksheet
Page 24
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
6. What is the final concentration of a 5M solution with a volume of 2 L if 3 L of water is added?
7. If 100 grams of sucrose is added to water to form a 500 ml solution, what is its molarity?
8. What is the mass of carbon dioxide that is dissolved in 200 ml of 2M solution?
9. How much water should you add to a 10M solution with a volume of 500 ml to reduce its
concentration to 8M?
10. If you mix 500 ml of 2M solution to 300 ml 5M solution, what will be the final
concentration?
Chemistry for Engineers Worksheet
Page 25
Score: ___________
Surname: _________________________________ Date Submitted: _____________________
First Name: ________________________________ Course, Year and Section: ______________
Electrochemistry
1. Lithium battery is now being used in most computer power storage application because it
lasts longer and has lesser maintenance cost. Write the half cell reactions, potentials and the
complete reaction of a lithium ion battery.
2. Write the chemical reactions and electric potentials of an alkaline battery.
3. Write the half cell reactions, potentials and the complete reaction of car lead battery.
Inorganic and Organic Chemistry Worksheet
Appendix
Page 26
SI BASE UNITS
1. Meter (m) is the length of the path traveled by light in vacuum during a time interval of
1/299,792,458 of a second.
2. Kilogram (kg) is the unit of mass; it is equal to the mass of the international prototype of the kilogram
–a platinum iridium cylinder kept in France.
3. Second (s) is the duration of 9,192,631,770 periods of the radiation corresponding to the transition
between the two hyperfine levels of the ground state of the cesium 133 atom.
4. Ampere (A) is that constant electric current which, if maintained in two straight parallel conductors of
infinite length, of negligible circular cross-section, and placed 1 meter apart in vacuum, would
produce between these conductors a force equal to 2 x 10-7 Newton per meter of length.
5. Kelvin (K), unit of thermodynamic temperature, is the fraction 1/273.16 of the thermodynamic
temperature of the triple point of water.
6. Mole (mol) is the amount of substance of a system which contains as many elementary entities as
there are atoms in 0.012 kilogram of carbon 12; its symbol is "mol." When the mole is used, the
elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles,
or specified groups of such particles.
7. Candela (cd) is the luminous intensity, in a given direction, of a source that emits monochromatic
radiation of frequency 540 x 1012 hertz and that has a radiant intensity in that direction of 1/683
watt per steradian.
Prefixes in the SI System
Prefix
Symbol
Multiple
anton
yotta
zetta
exa
peta
tera
giga
mega
kilo
hecto
deca
deci
centi
milli
micro
nano
pico
femto
atto
zepto
yocto
A
Y
Z
E
P
T
G
M
k
h
da
d
c
m
µ
n
p
f
a
z
y
(10100)100
(1010)100
10100
1024
1021
1018
1015
1012
109
106
103
102
101
10-1
10-2
10-3
10-6
10-9
10-12
10-15
10-18
10-21
10-24
English and SI Converstion Factors
Common
Name
antonplex
googolplex
googol
heptillion
hexillion
quintillion
quadrillion
trillion
billion
million
thousand
hundred
ten
tenth
hundreth
thousandth
millionth
billionth
trillionth
quadrillionth
quintillionth
hexillionth
heptillionth
Inorganic and Organic Chemistry Worksheet
Appendix
Length:
1 in = 2.54 cm
1 mi = 1.6093 km
1 m = 3.2808 ft
Volume:
1 gal = 3.7854 L
1 fluid ounce (fl oz) = 29.574 ml
1 teaspoon = 5 ml (approximate)
1 tablespoon = 15 ml (approximate)
1 cup = 250 ml (approximate)
1 gallon = 4 quarts
1 quart = 2 pints
1 pint = 2 cups
1 cup = 48 teaspoon
1 cup = 16 tablespoon
1 tablespoon = 3 teaspoon
Mass:
1 kg = 2.2046 lb
1 oz = 28.35 g
1 MT = 1000 kg
Temperature:
o
F = 1.8oC + 32
o
C = (oF – 32)/1.8
K = 273.15 + oC
o
R = 460 + oF
Scientific Notation – used to simplify the handling of cumbersome values - expressed in the form
N = a x 10n
Derived Units: volume, density
Page 27
Inorganic and Organic Chemistry Worksheet
Appendix
Page 28
SIGNIFICANT FIGURES
Definition: The digits that indicate the precision with which a measurement is used
All digits of a measured quantity are significant, including the last digit, which is uncertain
Guidelines applied to determine the number of significant figures in a measured quantity
1. All non-zero digits are significant
2. Zeroes between non-zero digits are significant
3. Zeroes to the right of the decimal point but to the left of the first non-zero digit are not
significant
4. Zeroes to the right of a non-zero digit and to the right of a decimal point are significant
5. When a number ends in zero but contains no decimal point, the zeroes may or may not be
significant. Exponential notation is used to avoid potential ambiguity of whether the zeroes are
significant or not.
6. Always carry one or two additional significant figures through a multi-step calculation and round
off to the desired number of significant figures the final answer only.
Conversion Factor – fraction whose numerator and denominator are the same quantity expressed in
different units
Dimensional Analysis
- approach in problem-solving in which the units or dimensions of the quantities are
examined to see what conversions are required
-
uses conversion factor to change one unit to another
Inorganic and Organic Chemistry Worksheet
Appendix
Electronic Configuration, Orbitals and Quantum Numbers
Naming of Ionic Compounds or Salts
Page 29
Inorganic and Organic Chemistry Worksheet
Appendix
Page 30
Ionic Compounds are composed of cation and anion joined together by an ionic bond due to
the attraction of positive to negative charges. The cation (positively charged ion, normally
metal) name retains the same name as the element. The anion (negatively charged ion,
normally non-metal) name is similar to the name of the element but the ending is replaced by
“-ide” like chloride, oxide, fluoride, carbide, sulphide, etc. For polyatomic ions (composed of
two or more atoms covalently bonded/molecular ion), they retain the same names like
ammonium hydroxide, potassium chromate, etc. Following are some common polyatomic ions.
If a metallic element has cations of different charges (or different oxidation states), the Stock
System can be used by including the Roman Numeral (representing its charge) in parentheses
after its name like copper(II) chloride. An older method uses the Latin name and suffix “ic” for
higher charge and “ous” for lower charge like the following.
Inorganic and Organic Chemistry Worksheet
Appendix
Page 31
Naming Inorganic Acids and Bases
The cation of an inorganic acid is the hydrogen ion. In binary acids (with one anion), the prefix is
“hydro” plus the name of the ion whose ending becomes a suffix “ic” plus the word acid.
For acids with polyatomic anions, the suffix “ate” is replaced with “ic” and those with suffix
“ite” with “ous”. Those with one extra oxygen have the prefix “per” and suffix “ic”. Those with
one fewer oxygen have the prefix “hypo” and the suffix “ous”.
The anion for inorganic bases is the hydroxide, a polyatomic ion. The naming is the same as the
rules in naming ionic compounds. For example Mg(OH)2 is named magnesium hydroxide
Inorganic and Organic Chemistry Worksheet
Appendix
Page 32
Naming of Molecular Inorganic Compounds
Molecular compounds are composed of two or more atoms of elements that are covalently
bonded by sharing valence electrons. Normally it is between atoms of non-metals.
When naming molecular compounds, prefixes are used to indicate the number of a given
element present in the compound. ” mono-” indicates one, “di-” is two, “tri-” is three, “tetra-”
is four, “penta-” is five, and “hexa-” is six, “hepta-” is seven, “octo-” is eight, “nona-” is nine,
and “deca” is ten. For example, N2O is called dinitrogen monoxide.
If the first element has only one atom, the prefix “mono” does not have to be included or may
be dropped. For example NO2 is called nitrogen dioxide and NOT mononitrogen dioxide.
If the second element is one atom of oxygen or any atom beginning with a vowel, instead of
naming it monooxide, it is named monoxide. One of the “o” is dropped.
Normally, the less electronegative atom is written first before the more electronegative ion.
Following are other examples.
Naming Inorganic Hydrates
Hydrates are compounds that contain loosely bonded water. An example is CuSO4 · 5H2O
which is a blue colored compound. Anhydride is a hydrate that has lost water through many
means like heating. Anhydrous is a substance that does not contain or not linked to any water.
Hydrates are named by naming first the compound where the water is attached then followed
by numerical Latin prefix that indicates the number of water molecules attached and the suffix
“hydrate”. For example CuSO4 · 5H2O is named of copper(II) sulphate pentahydrate.
Inorganic and Organic Chemistry Worksheet
Appendix
Page 33
Naming Organic Compounds
Organic compounds are generally named based on the number of carbons in its longest chain
and on its branches. The IUPAC (International Union of Pure and Applied Chemistry) is the
internationally acceptable system of organic nomenclature. However, many chemists still use
common names which are shorter sometimes. The prefixes based on the number of carbons
are as follows:
1
2
3
4
5
6
7
meth
eth
prop
but
pent
hex
hept
8
9
10
11
12
13
14
oct
non
dec
undec
dodec
tridec
tetradec
15
16
17
18
19
20
30
pentadec
hexadec
hepta
octadec
nondec
eicos
triacont
Naming is also based on the following functional groups.
40
50
60
70
80
90
100
tetracont
pentacont
hexacont
heptacont
octacont
nonacont
hect
Inorganic and Organic Chemistry Worksheet
Appendix
Many organic compounds have also branches as follows:
Below are examples of aromatic organic compounds.
Page 34
Inorganic and Organic Chemistry Worksheet
Appendix
Page 35
Activity Series of Metals
Lithium
Potassium
Strontium
Barium
Calcium
Sodium
Li
K
Sr
Ba
Ca
Na
Magnesium
Aluminum
Manganese
Zinc
Chromium
Mg
Al
Mn
Zn
Cr
reacts with steam
and acids and forms
hydroxides and
hydrogen gas
Iron
Cadmium
Cobalt
Nickel
Tin
Lead
Fe
Cd
Co
Ni
Sn
Pb
reacts with acids
only and forms
hydroxides and
hydrogen gas
reacts with liquid
water, steam and
acids and forms
hydroxides and
hydrogen gas
Hydrogen gas
H2
Antimony
Arsenic
Bismuth
Copper
Sb
As
Bi
Cu
forms oxides
with air
Mercury
Silver
Palladium
Platinum
Gold
Hg
Ag
Pd
Pt
Au
found free in
nature, when
heated its
oxides
decompose
Solubility Rules
Soluble Compounds
Salts of of Group IA, ammonium,
chlorate, perchlorate, acetate and
nitrate
Salts of Cl-, Br- and ICompounds containing F-
Exceptions
Ag+, Hg2 + and Pb2+
Mg 2+, Ca 2+, Sr 2+, Ba 2+, Pb 2+
Salts of sulfate, SO4 2-
Sulfates of Sr 2+, Ba 2+, Pb 2+,
slightly soluble are Ca 2+ and Ag 1+
Insoluble Compounds
All salts of :
carbonate, phosphate, oxalate,
chromate, sulfide
hydroxide
Exceptions
Salts of NH4 +, and alkali metal ions
Ba 2+, Ca2+(slightly soluble)
Inorganic and Organic Chemistry Worksheet
Appendix
Page 36
Easily Oxidized – Anode-More Reactive
Negative Electrode – electrons are lost
Easily Reduced – Cathode – Less Reactive
Positive Electrode – electrons are gained
Standard Reduction Potentials
Acidic Solution
F2(g) + 2e- → 2 F-(aq)
O3(g) + 2H+(aq) + 2e- → O2(g) + H2O(l)
S2O82-(aq) + 2e- → 2SO42-(aq)
H2O2(aq) + 2H+(aq) +2e- → 2H2O(l)
MnO4-(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)
PbO2(s) + 4H+(aq) + 2e- → Pb2+(aq) + 4H2O(l)
Cl2(g) + 2e- → 2Cl-(aq)
Cr2O72-(aq) + 14H+(aq) + 6e- → 2Cr3+(aq) + 7H2O(l)
MnO2(s) + 4H+(aq) +2e- -> Mn2+(aq) + 2H2O(l)
O2(g) + 4H+(aq) + 4e- → 2H2O(l)
2IO3-(aq) + 12H+(aq) + 10e- → I2(s) + 6H2O(l)
Br2(l) + 2e- → 2Br-(aq)
NO3-(aq) + 4H+(aq) + 3e- → NO(g) + 2 H2O(l)
Ag+(aq) + e- → Ag(s)
Fe3+(aq) + e- → Fe2+(aq)
O2(g) + 2H+(ag) + 2e- → H2O2(aq)
I2(s) + 2e- → 2I-(aq)
Cu2+(aq) + 2e- → Cu(s)
SO42-(aq) + 4H+(aq) + 2e- → 2H2O(l) + SO2(g)
Sn4+(aq) + 2e- → Sn2+(aq)
S(s) + 2H+(aq) + 2e- → H2S(g)
2H+(aq) + 2e- → H2(g)
Pb2+(aq) + 2e- → Pb
Sn2+(aq) + 2e- → Sn(s)
Fe2+(aq) + 2e- → Fe(s)
Zn2+ + 2e- → Zn(s)
Al3+(aq) + 3e- → Al(s)
Mg2+(aq) + 2e- → Mg(s)
Na+(aq) + e- → Na(s)
Ca2+(aq) + 2e- → Ca(s)
K+(aq) + + e- → K(s)
Li+(aq) + e- → Li(s)
Basic Solution
O3(aq) + H2O(l) + 2e- → O2(g) + 2OH-(aq)
OCl-(aq) + H2O(l) + 2e- → Cl-(aq) + 2OH-(aq)
O2(g) + 2H2O(l) +4e- → 4OH-(aq)
2H2O(l) + + 2e- → H2(aq) + 2OH-(aq)
2.866
2.075
2.01
1.763
1.51
1.455
1.358
1.33
1.23
1.229
1.2
1.065
0.956
0.8
0.771
0.695
0.535
0.34
0.17
0.154
0.14
0
-0.125
-0.137
-0.44
-0.763
-1.676
-2.356
-2.713
-2.84
-2.924
-3.04
1.246
0.89
0.401
-0.0828
Inorganic and Organic Chemistry Worksheet
Appendix
Solute
HF
HCl
HClO4
HClO4 · H2O
HBr
HI
HIO3
HNO3
HCOOH
CH3COOH
NH3
NH4Cl
NH4ClO4
NH4Br
NH4I
NH4IO3
NH4NO2
NH4NO3
NH4C2H3O2
NH4CN
NH4CNS
CH3NH3Cl
(CH3)3NHCl
N(CH3)4Cl
N(CH3)4Br
N(CH3)4I
AgClO4
AgNO2
AgNO3
LiOH
LiOH · H2O
LiF
LiCl
LiCl · H2O
LiClO4
LiClO4 · 3H2O
LiBr
LiBr · H2O
g
g
l
c
g
g
c
l
l
l
g
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
∆sol H°
kJ/mol
-61.50
-74.84
-88.76
-32.95
-85.14
-81.67
8.79
-33.28
-0.86
-1.51
-30.50
14.78
33.47
16.78
13.72
31.80
19.25
25.69
-2.38
17.57
22.59
5.77
1.46
4.08
24.27
42.07
7.36
36.94
22.59
-23.56
-6.69
4.73
-37.03
-19.08
-26.55
32.61
-48.83
-23.26
Enthalpy of Solutions of Electrolytes
∆sol H°
Solute
kJ/mol
LiBr · 2H2O
c
-9.41
LiBrO3
c
1.42
LiI
c
-63.30
LiI · H2O
c
-29.66
LiI · 2H2O
c
-14.77
LiI · 3H2O
c
0.59
LiNO2
c
-11.00
LiNO2 · H2O
c
7.03
LiNO3
c
-2.51
NaOH
c
-44.51
NaOH · H2O
c
-21.41
NaF
c
0.91
NaCl
c
3.88
NaClO2
c
0.33
NaClO2 · 3H2O
c
28.58
NaClO3
c
21.72
NaClO4
c
13.88
NaClO4 · H2O
c
22.51
NaBr
c
-0.60
NaBr · 2H2O
c
18.64
NaBrO3
c
26.90
NaI
c
-7.53
NaI · 2H2O
c
16.13
NaIO3
c
20.29
NaNO2
c
13.89
NaNO3
c
20.50
NaC2H3O2
c
-17.32
NaC2H3O2 · 3H2O
c
19.66
NaCN
c
1.21
NaCN · 0.5H2O
c
3.31
NaCN · 2H2O
c
18.58
NaCNO
c
19.20
NaCNS
c
6.83
KOH
c
-57.61
KOH · H2O
c
-14.64
KOH · 1.5H2O
c
-10.46
KF
c
-17.73
KF · 2H2O
c
6.97
KCl
c
17.22
Page 37
Solute
KClO3
KClO4
KBr
KBrO3
KI
KIO3
KNO2
KNO3
KC2H3O2
KCN
KCNO
KCNS
KMnO4
RbOH
RbOH · H2O
RbOH · 2H2O
RbF
RbF · H2O
RbF · 1.5H2O
RbCl
RbClO3
RbClO4
RbBr
RbBrO3
RbI
RbNO3
CsOH
CsOH · H2O
CsF
CsF · H2O
CsF · 1.5H2O
CsCl
CsClO4
CsBr
CsBrO3
CsI
CsNO3
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
c
∆sol H°
kJ/mol
41.38
51.04
19.87
41.13
20.33
27.74
13.35
34.89
-15.33
11.72
20.25
24.23
43.56
-62.34
-17.99
0.88
-26.11
-0.42
1.34
17.28
47.74
56.74
21.88
48.95
25.10
36.48
-71.55
-20.50
-36.86
-10.46
-5.44
17.78
55.44
25.98
50.46
33.35
40.00
Inorganic and Organic Chemistry Worksheet
Appendix
Name
Aluminum
Antimony
Argon
Arsenic
Astatine
Barium
Beryllium
Bismuth
Boron
Bromine
Cadmium
Calcium
Carbon
Cerium
Cesium
Chlorine
Chromium
Cobalt
Copper
Dysprosium
Erbium
Europium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hafnium
Helium
Holmium
Hydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lead
Lithium
Lutetium
Magnesium
Manganese
Mercury
Symbol
Al
Sb
Ar
As
At
Ba
Be
Bi
B
Br
Cd
Ca
C
Ce
Cs
Cl
Cr
Co
Cu
Dy
Er
Eu
F
Fr
Gd
Ga
Ge
Au
Hf
He
Ho
H
In
I
Ir
Fe
Kr
La
Pb
Li
Lu
Mg
Mn
Hg
Atomic
Mass
26.9815
121.76
39.948
74.9216
210
137.327
9.0122
208.9804
10.811
79.904
112.411
40.078
12.0107
140.116
132.9055
35.453
51.9961
58.9332
63.546
162.5
167.259
151.964
18.9984
223
157.25
69.723
72.64
196.9665
178.49
4.0026
164.9303
1.0079
114.818
126.9045
192.217
55.845
83.8
138.9055
207.2
6.941
174.967
24.305
54.938
200.59
Atomic
number
13
51
18
33
85
56
4
83
5
35
48
20
6
58
55
17
24
27
29
66
68
63
9
87
64
31
32
79
72
2
67
1
49
53
77
26
36
57
82
3
71
12
25
80
Name
Molybdenum
Neodymium
Neon
Nickel
Niobium
Nitrogen
Osmium
Oxygen
Palladium
Phosphorus
Platinum
Polonium
Potassium
Praseodymium
Promethium
Radium
Radon
Rhenium
Rhodium
Rubidium
Ruthenium
Samarium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulfur
Tantalum
Technetium
Tellurium
Terbium
Thallium
Thulium
Tin
Titanium
Tungsten
Vanadium
Xenon
Ytterbium
Yttrium
Zinc
Zirconium
Page 38
Symbol
Mo
Nd
Ne
Ni
Nb
N
Os
O
Pd
P
Pt
Po
K
Pr
Pm
Ra
Rn
Re
Rh
Rb
Ru
Sm
Sc
Se
Si
Ag
Na
Sr
S
Ta
Tc
Te
Tb
Tl
Tm
Sn
Ti
W
V
Xe
Yb
Y
Zn
Zr
Atomic
Mass
95.94
144.24
20.1797
58.6934
92.9064
14.0067
190.23
15.9994
106.42
30.9738
195.078
209
39.0983
140.9077
145
226
222
186.207
102.9055
85.4678
101.07
150.36
44.9559
78.96
28.0855
107.8682
22.9897
87.62
32.065
180.9479
98
127.6
158.9253
204.3833
168.9342
118.71
47.867
183.84
50.9415
131.293
173.04
88.9059
65.39
91.224
Atomic
number
42
60
10
28
41
7
76
8
46
15
78
84
19
59
61
88
86
75
45
37
44
62
21
34
14
47
11
38
16
73
43
52
65
81
69
50
22
74
23
54
70
39
30
40