CH1000 Fundament als of Chemistry Module 2 – Chapter 6 Common and Systematic Names • 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: 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 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 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. • 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 ...

1. CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 6
Common and Systematic Names
• 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

2. 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:
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

3. 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
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.

4. •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
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

5. 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.
• 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

6. 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
di 2 hepta 7
tri 3 octa 8
tetra 4 nona 9
penta 5 deca 10

7. 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
learned.
•Rules for naming compounds
containing polyatomic ions
• Name the cation

8. • Name the anion
Name Formula Charge Name Formula Charge
Acetate C2H3O2
- -1 Cyanide CN- -1
Ammonium NH4
+ +1 Dichromate Cr2O7
2- -2
Hydrogen
Carbonate
HCO3
- -1 Hydroxide OH- -1
Hydrogen
Sulfate
HSO4
- -1 Nitrate NO3
- -1
Bromate BrO3
- -1 Nitrite NO2
- -1
Carbonate CO3
2- -2 Permanganate MnO4
- -1

9. Chlorate ClO3
- -1 Phosphate PO4
3- -3
Chromate CrO4
2- -2 Sulfate SO4
2- -2
Sulfite SO3
2- -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)
•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

10. 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

11. - Sodium hydrogen
carbonate
NaHS Na+; HS-
Sodium hydrogen
sulfide
MgNH4PO4
Mg2+; NH4
+;
PO4
3-
Magnesium
ammonium
phosphate
NaKSO4 Na
+; K+; SO4
2- 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

12. • 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
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

13. synthesise learning to effectively communicate understanding of
the chosen professional issue including local, national and/or
international perspectives
reflect critically on a professional issue justifying your position
presenting a rationale
critically evaluate relevant literature to demonstrate conceptual
understanding of the professional issue
communicate the processes and the conclusions of study i n a
clear manner, making effective use of academic conventions
and meeting the needs of both academic and professional
audiences.
Choose two key readings relevant to your chosen professional
issue and write a critical analysis of them, synthesising
important points and findings.
What is the central argument of the piece?
What reasons does the author give to support the argument? Are
they logical? Are there any assumptions made?
Is the conclusion the author makes sound in terms of these
reasons? If not, what are the flaws?
Are the recommendations for practice reasonable in terms of the
strength of the argument?
Are there any possible flaws in the research, including in the
interpretation of data?
What other studies or further research would you need to
validate your view of this study?
Do other people reach similar conclusions to you (note: do a
citation search on the paper to find out whether other authors
have cited the paper and what they said about it)?

14. In evaluating external voices and positions, the writer:
challenges a theory or research findings
argues persuasively for an alternative
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.

15. • 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

16. 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

17. • 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.

18. b) Balance each element sequentially, using whole
numbers. It is often best to balance metals first.
mercury(II) oxide mercury + oxygen
Δ
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.

19. 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: 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

20. 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
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

21. 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
Decomposition
Reactions
A single reactant breaks down (decomposes) into
two or more products
AB A + B

22. 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
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

23. 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
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

24. 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
•Products are at a higher
potential energy than
reactants.
•Activation energy: Amount
of energy needed to initiate a
chemical reaction.
Reaction Coordinate
Diagram

25. 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?
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

26. 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
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 7
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

27. 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
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

28. 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
% 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

29. 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
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

30. 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?
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

31. Composition from Experimental DataEmpirical and Molecular
FormulaCalculating Empirical FormulasCalcula ting 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!
• 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

32. •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.
Problem Solving for Stoichiometry Problems
Problem Solving for Stoichiometry Problems
Problem Solving for
Stoichiometry
Problems

33. •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
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

34. 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?
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