CH1000 Fundament als of Chemistry Module 2 – Chapter 8 Chemical Equations • Chemists use chemical equations to: • Summarize a chemical reaction by displaying the substances reacting and forming. • Indicate specific amounts of materials consumed or produced during the reaction. • Reactants: substances consumed during the reaction. • Products: substances formed during the reaction. • Atom balance must be maintained in all chemical reactions. • All atoms from reactants must appear as part of products. a A + b B c C + d D The coefficient 1 is not written in a balanced equation. Chemical Equations 1. Reactants and products are separated by an arrow. 2. Reactants are on the left side of the arrow, products are on the right. 3. Whole number coefficients are placed in front of substances to balance the atoms in the equation. 4. The numbers indicate the units of the substance reacted or formed during the reaction. 5. Information about the reaction (temperature, time) may be placed above or below the reaction arrow. 6. The physical state is written in brackets after the formula of the substance. (g) for gas, (l) for liquid, (s) for solid, (aq) for aqueous a A + b B c C + d D Reactant s Products Symbol Summary Symbol Significance Produces (points towards products) (s) Solid (written after substance) (l) Liquid (written after substance) (g) Gas (written after substance) (aq) Substance dissolved in an aqueous solution Heat is added (above or below reaction arrow) Δ Law of Conservation of Mass • The total mass of substances in a chemical reaction must remain constant. water hydrogen + oxygen 100.0 g 11.2 g 88.8 g 100.0 g total of productsreactants In any chemical reaction: Mass of reactants = Mass of products Writing and Balancing Chemical Equations A balanced chemical equations contain the same number of each kind of atom on both sides of the equation. 1. Write a word equation for the reaction. 2. Write the correct formula for each substance (unbalanced): 3. Balance the equation a) Count the number of each atom on the reactants and products side and determine what requires balancing. b) Balance each element sequentially, using whole numbers. It is often best to balance metals first. mercury(II) oxide mercury + oxygenΔ HgO Hg + O2 Δ Hg: 1 O: 1 Hg: 1 O: 2 HgO Hg + O2 Δ Oxygen atoms need balancing on the reactants side. 2 HgO Hg + O2 Δ Hg: 2 O: 2 Hg: 1 O: 2 Now Hg atoms need balancing on the products side. Writing and Balancing Chemical Equations 4. Check after adding coefficients that all atoms still balance. Adjust as needed (a 2 is needed in front of Hg). 5. Do a final check to make sure all atoms now balance on both sides of the equation. 2 HgO 2 Hg + O2 Δ Hg: 2 O: 2 Hg: ...

1. CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 8
Chemical Equations
• Chemists use chemical equations to:
• Summarize a chemical reaction by displaying the substances
reacting and
forming.
• Indicate specific amounts of materials consumed or produced
during the
reaction.
• Reactants: substances consumed during the reaction.
• Products: substances formed during the reaction.
• Atom balance must be maintained in all chemical reactions.
• All atoms from reactants must appear as part of products.
a A + b B c C + d D
The
coefficient
1 is not
written in
a balanced

2. equation.
Chemical Equations
1. Reactants and products are separated by an arrow.
2. Reactants are on the left side of the arrow, products are on
the right.
3. Whole number coefficients are placed in front of substances
to
balance the atoms in the equation.
4. The numbers indicate the units of the substance reacted or
formed
during the reaction.
5. Information about the reaction (temperature, time) may be
placed
above or below the reaction arrow.
6. The physical state is written in brackets after the formula of
the
substance. (g) for gas, (l) for liquid, (s) for solid, (aq) for
aqueous
a A + b B c C + d D
Reactant
s
Products
Symbol

3. Summary
Symbol Significance
Produces (points towards products)
(s) Solid (written after substance)
(l) Liquid (written after substance)
(g) Gas (written after substance)
(aq) Substance dissolved in an aqueous
solution
Heat is added (above or below reaction
arrow)
Δ
Law of Conservation of Mass
• The total mass of substances in a chemical reaction must
remain
constant.
water hydrogen + oxygen
100.0 g 11.2 g 88.8 g
100.0 g total of productsreactants
In any chemical reaction:
Mass of reactants = Mass of products
Writing and
Balancing

4. Chemical
Equations
A balanced chemical equations contain the same
number of each kind of atom on both sides of the
equation.
1. Write a word equation for the reaction.
2. Write the correct formula for each substance
(unbalanced):
3. Balance the equation
a) Count the number of each atom on the reactants and
products side and determine what requires
balancing.
b) Balance each element sequentially, using whole
numbers. It is often best to balance metals first.
mercury(II) oxide mercury + oxygenΔ
HgO Hg + O2
Δ
Hg: 1
O: 1
Hg: 1
O: 2
HgO Hg + O2
Δ
Oxygen atoms

5. need balancing
on the reactants
side.
2 HgO Hg + O2
Δ
Hg: 2
O: 2
Hg: 1
O: 2
Now Hg atoms
need balancing
on the products
side.
Writing and
Balancing
Chemical
Equations
4. Check after adding coefficients that all atoms still
balance. Adjust as needed (a 2 is needed in front of
Hg).
5. Do a final check to make sure all atoms now balance
on both sides of the equation.
2 HgO 2 Hg + O2
Δ
Hg: 2

6. O: 2
Hg: 2
O: 2
Note: always use the smallest whole
numbers!
4 HgO 4 Hg + 2 O2
Δ
Balanced but incorrect form!
Information in
a Chemical
Equation
© 2014 John Wiley & Sons, Inc. All rights reserved.
Information from a Chemical
Equation
• From the chemical equation below, how many moles of
oxygen are
needed to burn 2 molecules of propane (C3H8)?
• a) 5 molecules of oxygen
• b) 6 molecules of oxygen
• c) 10 molecules of oxygen
• d) 15 molecules of oxygen
C3H8 + 5 O2 3 CO2 + 4 H2O

7. For every 1 molecule of propane,
5 molecules of O2 are needed to fully
react.
Two molecules of propane would then
require
2 x 5 = 10 molecules of oxygen.
Types of
Chemical
Equations
1. Combination reactions
2. Decomposition reactions
3. Single displacement reactions
4. Double displacement reactions
5. Oxidation-reduction (redox) reactions
(Chapter 17)
Reactions are classified into subtypes to aide in
predicting
the products of chemical reactions.
Reactions are classified into five major categories:
Combination Reactions Two reactants combine to give a single
product.
A + B AB

8. Decomposition
Reactions
A single reactant breaks down (decomposes) into
two or more products
AB A + B
Single Displacement
Reactions
One element (A) reacts with a compound (BC) to replace
one element in the compound, giving a new element (B)
and a different compound (AC).
General Types of Single Displacement Reactions
Double Displacement
Reactions
Two compounds exchange partners with one
another to yield two new compounds.
AB + CD AD + CB
General Types of Double Displacement Reactions

9. Double Displacement
Reactions
Two compounds exchange partners with one
another to yield two new compounds.
AB + CD AD + CB
General Types of Double Displacement Reactions Writing
Reaction Equations Practice
1. Write the reaction equation between aqueous
solution of hydroiodic acid and sodium
hydroxide.
2. First convert names to chemical formulas and
determine the type of reaction.
HI (acid)/NaOH(base)
Neutralization Reaction
acid + base salt + water
HI (aq) + NaOH (aq) NaI (aq) + H2O (l)
Salt formula must charge balance (Na+ and I–)
Heat in
Chemical
Reactions
Terminology
Energy transfer and changes accompany any chemical reaction
Heat of reaction: quantity of heat actually produced during a

10. chemical reaction.
Units: kilojoules (kJ) or kilocalories (kcal)
Exothermic reactions: release heat. H2 (g) + Cl2 (g)
2 HCl (g) + 185 kJ
Heat can be treated as a product
Endothermic reactions: absorb heat. N2 (g) + O2 (g)
+ 181 kJ 2
NO (g)
Heat can be treated as a product
C (s) + O2 (g) CO2 (g) + 393 kJ
1 mol of C reacts with 1 mol of O2 to provide 1
mol of CO2 and 393 kJ
of heat
are released.
Heat in Chemical Reactions
Equations Practice
Heat as an Energy
Transfer
Vehicle in Nature
Graphical
Representations of
Endothermic
Reactions

11. •Products are at a higher
potential energy than
reactants.
•Activation energy: Amount
of energy needed to initiate a
chemical reaction.
Reaction Coordinate
Diagram
Graphical
Representations of
Exothermic
Reactions
•Products are at a lower
potential energy than
reactants.
•Activation energy: Amount
of energy needed to initiate a
chemical reaction.
Reaction Coordinate
Diagram
Reading
Review
How do you know if a reaction is a
combustion reaction?

12. What is an endothermic reaction?
What is an exothermic reaction?
What are the four types of chemical
equations?.
How do you know if an equation is
balanced?
Slide 1Chemical EquationsChemical EquationsSymbol
SummaryLaw of Conservation of MassWriting and Balancing
Chemical EquationsWriting and Balancing Chemical
EquationsInformation in a Chemical EquationInformation from
a Chemical EquationTypes of Chemical EquationsCombination
ReactionsDecomposition ReactionsSingle Displacement
ReactionsDouble Displacement ReactionsDouble Displacement
ReactionsHeat in Chemical Reactions TerminologyHeat as an
Energy Transfer Vehicle in NatureGraphical Representations of
Endothermic ReactionsGraphical Representations of Exothermic
ReactionsReading Review
Strategic Marketing Plan
MKT/574 v1
Page 3 of 3
Part B: Marketing Data Analysis
(Due in Wk 4)
Internal Data
Evaluate internal sources of information available to you inside
the organization and what information you will receive from
each source. Identify 3-6 sources of internal data. Insert or
remove rows as needed.
Source
What it Measures

13. Data
Potential Usage
Example: Sales data
Monthly sales by specific product
Average sales that month in US dollars for each of 10 pr oducts.
Data can be segmented by business and consumer markets.
Can be used for trend analysis, projections, and to measure
effectiveness of promotions.
Secondary Data
Evaluate secondary data sources and the specific information

14. you need from each source. Insert or remove rows as needed.
Source
What it Measures
Data
Potential Usage
Example: retail store analytics
Dollar value of sales by quarter by major product categories
Total sales of major players
Market Share Analysis
Seasonal patterns

15. Primary Data
Evaluate primary data needs to create and evaluate the
marketing plan. Insert or remove rows as needed.
Source
What it Measures
Data
Potential Usage
Example: Focus group
Product usage, motives, identify group level satisfaction,
decision process, etc.
Qualitative
Identify different reactions of market segments to product.
Identify marketing opportunities, product/service flaws and
opportunities

16. Customer Relationship Management
Establish customer touchpoints and develop appropriate CRM
events for customer acquisition, retention, and profitability.
Insert or remove rows as needed.
CRM Touchpoint
Purpose & CRM Objective
Data
Potential Data Usage
Example: Customer profile information on website
Starts the account for visitors: name, geography, email address
(Customer acquisition)
Presale: geographic location; customer id, source of reference
Email address
Post sales: address, product purchased, quantity, price.
Track new and returning customer counts, total period
purchases by customer ID, geographic sales data. Can be used
for loyalty rewards, retention, and targeted marketing.

17. Copyright 2020 by University of Phoenix. All rights reserved.
Rubic for assignment
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 6
Common and Systematic Names

18. • Chemical nomenclature is the systematic naming of chemical
compounds
• Common names are historical names of compounds which are
not based
on systematic rules
• Common names are often used because systematic names are
too long
and technical for everyday use
• Chemists prefer systematic names that precisely identify the
chemical
composition of compounds.
• Example CaO
• Common name: lime
• Systematic name: calcium oxide
Naming
Flowchart
We will focus on nomenclature of inorganic compounds
Elements and Ions
• The formula for most elements is the symbol of the element
off of
the periodic table.
• Diatomic molecules are an exception:
• Two other elements also exist in polyatomic arrangements:

19. Naming Anions
•Remember from Chapter 5
that any neutral atom that
gains an electron is called
an anion
•When naming anions,
change the element ending
to -ide
Symbols
of the
Elements
•Each element has an
abbreviation called a symbol.
•The first letter of a symbol
must always be capitalized.
•If a second letter is needed, it
should be lowercase.
Predicting Ion
Charge from
Periodic Table
•Metals form cations
•The positive charge is equal
to the group number

20. Predicting Ion
Charge from
Periodic Table
•Nonmetals form anions
•The negative charge is equal
to 8 – the group number
Writing Formulas from Names of Ionic Compounds
•Ionic compounds contain both a cation and
an anion.
•Ionic compounds must have a net charge of
0
•The sum of charges of the cations and
anions in an ionic compound equal 0
•Rules for writing formulas for ionic
compounds:
• Write the metal ion followed by the
nonmetal ion formula
• Combine the smallest whole numbers
of each ion to provide an overall
charge equal to zero
• Write the compound formula for the
metal and nonmetal, using subscripts

21. determined from Step 2 for each ion
Naming Ionic
Binary
Compounds
•Binary compounds containing
a metal which forms only one
cation
•By convention, the cation is
written/named first followed
by the anion
•Rules for naming binary ionic
compounds:
• Name the cation
• Write the anion root and
add the –ide suffix
Naming
Compounds
Containing
Metals with
Multiple
Charges
•Rules for Naming Compounds Involving Metals that Could
Form
Multiple Charges
• Write the cation name.

22. • Write the cation charge in Roman numerals in parentheses.
• Write the root of the anion and use the –ide suffix.
•Exception: for metals that only form two cations, a Latin root
with
either an –ous or –ic suffix can also be used.
Formula Name Classical Name Formula Name Classical Name
Cu+ Copper(I) cuprous Sn2+ Tin(II) stannous
Cu2+ Copper(II) cupric Sn4+ Tin(IV) stannic
Fe2+ Iron(II) ferrous Pb2+ Lead(II) plumbous
Fe3+ Iron(III) ferric Pb4+ Lead(IV) plumbic
Naming Molecular
Compounds
•Molecular compounds contain two nonmetals
•Rules for naming molecular compounds:
• Write the name for the first element, including the appropriate
prefix
(mono is rarely used).
• Write the name for the second element, including the
appropriate prefix
and -ide ending (mono is used for the 2nd element).
Prefix Number Prefix Number
mono 1 hexa 6

23. di 2 hepta 7
tri 3 octa 8
tetra 4 nona 9
penta 5 deca 10
Naming Binary
Acids
Rules for naming Binary Acids:
Write the prefix hydro followed by the root
of the second element and add an –ic suffix Add the word acid
Hydrogen is always written first in an acid formula.
This is the indicator that it is an acid
Certain binary compounds containing hydrogen behave as acids
in water and have special names.
HCl(g) is hydrogen chloride HCl(aq) is hydrochloric acid
Naming
Polyatomic Ions
•A polyatomic ion is anion that
contains two or more
elements
•The names, formulas and
charges of common
polyatomic ions should be

24. learned.
•Rules for naming compounds
containing polyatomic ions
• Name the cation
• Name the anion
Name Formula Charge Name Formula Charge
Acetate C2H3O2- -1 Cyanide CN- -1
Ammonium NH4+ +1 Dichromate Cr2O72- -2
Hydrogen
Carbonate HCO3
- -1 Hydroxide OH- -1
Hydrogen
Sulfate HSO4
- -1 Nitrate NO3- -1
Bromate BrO3- -1 Nitrite NO2- -1
Carbonate CO32- -2 Permanganate MnO4- -1
Chlorate ClO3- -1 Phosphate PO43- -3
Chromate CrO42- -2 Sulfate SO42- -2
Sulfite SO32- -2
Naming
Oxyanions
•Oxyanions are polyatomic ions that contain
oxygen
•Often end in suffix –ate or –ite
•-ate compounds contain more O atoms
than ite compound(s)

25. •For elements that form multiple ions with
oxygen, prefixes are also needed:
• Per: add one oxygen to the –ate root
• Hypo – subtract one oxygen from the –
ite root
Anion
Formula Anion Name
Anion
Formula Anion Name
ClO- hypochlorite HClO hypochlorous acid
ClO2- chlorite HClO2 chlorous acid
ClO3- chlorate HClO3 chloric acid
ClO4- perchlorate HClO4 perchloric acid
More Complicated
Polyatomics
•Inorganic ions can be formed from more
than 3 elements
•The same method is used as before:
• Identify the ions and name in order
• Cations before anions
Compound Ions Name
NaHCO3 Na+; HCO3-
Sodium hydrogen

26. carbonate
NaHS Na+; HS- Sodium hydrogen sulfide
MgNH4PO4
Mg2+; NH4+;
PO43-
Magnesium
ammonium
phosphate
NaKSO4 Na+; K+; SO42-
Sodium potassium
sulfate
Naming Acids
• Acids generally begin with hydrogen
• To recognize oxyacids, make sure:
• H is the first element in the formula
• The compound contains a polyatomic ion with oxygen
• The following modifications are made to the name of the
acid:
• -ate ions are changed to –ic acids
• -ite ions are changed to –ous acids
• -ic acids contain one more oxygen than –ous acids
Naming Acids

27. Flowchart
Reading
Review
What type of ions do metals form?
What type of ions do nonmetals
form?
What is the chemical formula for
potassium sulfide?
Name the compound CrCl3.
Acids often begin with what element?
Slide 1Common and Systematic NamesNaming
FlowchartElements and IonsNaming AnionsSymbols of the
ElementsPredicting Ion Charge from Periodic TablePredicting
Ion Charge from Periodic TableWriting Formulas from Names
of Ionic CompoundsNaming Ionic Binary CompoundsNaming
Compounds Containing Metals with Multiple ChargesNaming
Molecular CompoundsNaming Binary AcidsNaming Polyatomic
IonsNaming OxyanionsMore Complicated PolyatomicsNaming
AcidsNaming Acids FlowchartReading Review
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 7

28. The Mole (or mol)
• In chemistry, a mole (mol) is a standard scientific unit for
measuring large
quantities of very small entities such as atoms, molecules, or
other
specified particles.
• The number represented by 1 mole above is also called
Avogadro’s number.
• 1 mol of any element contains the same number of atoms, but
can vary
greatly in the overall mass. (Atoms of different elements have
different
masses)
Molar Mass
•Molar Mass is the atomic mass
of an element or compound in
grams which contains Avogadro’s
number of particles
• Molar masses are expressed
to 4 significant figures in the
text
•Convert atomic mass units on
the periodic table to grams and
sum the masses of the total
atoms present

29. Mole Map
** Not found in the textbook,
save for easy access
Molar Mass of Compounds
•Much like an element, molar
mass can be defined for a
compound
•Molar Mass is the mass of one
mole of the formula unit of a
compound
• The molar mass of a
compound is equal to the
sum of the molar masses of
all the atoms in the
molecule
Percent
Composition of
Compounds
Percent composition is the mass percent of each
element in a compound.
• Percent = parts per 100 parts
• Molar mass is the total mass (100%) of the compound

30. % Composition is independent of sample size
% Composition can be determined by:
• 1. Knowing the compound’s formula
• 2. Using experimental data
Percent Composition from the Compound’s Formula
Percent Composition from Experimental Data
Empirical
and
Molecular
Formula
Empirical Formula
Smallest whole number ratio of
atoms in a compound
Molecular Formula
Actual formula of a compound.
Represents the total number of
atoms in one formula unit of the
compound
Calculating
Empirical

31. Formulas
•Special Case:
• If fractions are
encountered,
multiply by a
common factor to
provide whole
numbers for each
subscript.
Calculating the Molecular Formula from the Empirical Formula
•If molar mass is known,
the molecular formula can
be calculated from the
empirical formula
•Molecular formula is a
multiple of the empirical
formula.
Reading
Review
What is Avagadro’s
number?
How would you
convert from grams
to atoms of an
element?

32. What is a mole?
What is the
difference between
empirical and
molecular formulas?
What is the special
case when
calculating empirical
formulas?
Slide 1The Mole (or mol)Molar MassMole MapMolar Mass of
CompoundsPercent Composition of CompoundsPercent
Composition from the Compound’s FormulaPercent
Composition from Experimental DataEmpirical and Molecular
FormulaCalculating Empirical FormulasCalculating the
Molecular Formula from the Empirical FormulaReading Review
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 9
Introduction to Stoichiometry
• Equations must always be balanced before calculation of any
mass,
moles, or volume of a reactant or product!

33. • Stoichiometry is the area of chemistry that deals with
quantitative
relationships between products and reactants in chemical
equations.
• Solving stoichiometry problems always requires the use of:
• A balanced chemical equation (coefficients must be known!)
• Conversion factors in units of moles (mole ratios)
Mole Ratios
•Mole ratio is the conversion
factor between any two
species in a chemical reaction
•The mole ratio will come from
the coefficients of a balanced
chemical equation
Mole Ratios in Practice
•The mole ratio can be used as a
conversion factor to convert
between moles of one substance
and another.
•The desired quantity goes in the
numerator and the known
quantity goes into the
denominator of the mole ratio
•Same method as the solution
map from chapter 2.

34. Problem Solving for Stoichiometry Problems
Problem Solving for Stoichiometry Problems
Problem Solving for
Stoichiometry
Problems
•Remember that Step 1 is to
always ensure you have a
balanced equation!!!
•You must be in moles to
convert from one substance to
another!
Limiting
Reactants
•In chemical reactions, the
reaction will occur until one of the
reactants runs out
•Think of a burning fire. You need
oxygen, heat and fuel to keep a
fire going. If the fuel (wood) all
burns, the fire goes out. The wood
would be the limiting reactant

35. because had it not all burned, the
fire would continue to exist.
•In a chemical reaction, the
maximum amount of product
formed depends on the amount of
reactant not in excess, the limiting
reactant
Reaction Yield
• The amount of products formed calculated by stoichiometry
are the
maximum yields possible (100%)
• Yields are often lower in practice due to side reactions, loss of
product while isolating/transferring the material, etc.
• The theoretical yield is the maximum possible yield for a
reaction,
calculated based on the balanced chemical equation.
• The actual yield is the yield obtained from the reaction
• The percent yield is the ratio of the actual and theoretical
yield
Reading
Review
What is stoichiometry?
What unit must you be in to convert from one
substance to another?

36. What is the limiting reactant?
What is the difference between theoretical
and actual yields?
How do you calculate the percent yield?
Slide 1Introduction to StoichiometryMole RatiosMole Ratios in
PracticeProblem Solving for Stoichiometry ProblemsProblem
Solving for Stoichiometry ProblemsProblem Solving for
Stoichiometry ProblemsLimiting ReactantsReaction
YieldReading Review