CH1000 Fundament als of Chemistry Module 1 – Chapter 3 Elements and Atoms • What is an element? • An element is a fundamental substance that cannot be broken down by chemical means into a simpler substance. • Elements are the building blocks of matter. • Elements can occur naturally or be synthesized in labs. • The smallest unit of an element that retains its properties and chemical behavior is called an atom. • Atoms are made up of subatomic particles, but they do not have the properties of the element Elements •Ten elements make up almost 99 % of the mass of the Earth’s crust, seawater and atmosphere. •Oxygen accounts for about 20 % of the atmosphere and is found in nearly all rocks, sand and soil. 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. Introduction to the Periodic Table •Elements with similar chemical properties are placed in columns called groups. •Four groups have special identifying names, like Noble Gases, in group 8A, which are all unreactive gases. Introduction to the Periodic Table •The eight tall columns are called representative elements, or main group elements. These are shown in red. •The elements in the center are called the transition metals, or sometimes the “inner transition metals.” These are shown in purple. Introduction to the Periodic Table •Elements can be further classified as metals, metalloids and nonmetals. •Notice the bold, black “staircase” on the table. Everything to the left of the staircase is a metal and everything to the right of the staircase is a non metal. • The exception is Hydrogen, which is why some periodic tables will show hydrogen disconnected from the main body of the table. •The elements in grey touching the “staircase” are called metalloids, or semiconductor metals. These metals are used in the semiconductor industry. Metals, Nonmetal s and Metalloids • Solid at room temperature (except mercury) • Shiny • Good conductors of heat and electricity • Malleable (can be shaped) • Ductile (can be drawn into wires) • Most metals have a high melting point and density Metals • Not shiny • Have fairly low melting points and densities • Are poor conductors of heat and electricity Non Metals • Metalloids have properties between metals and nonmetals. • These elements are positioned diagonally on the Periodic Table separating the metals and nonmetals. Metalloid s Diatomic Elements •Diatomic molecules contain exactly two atoms •Seven elements exist as diatomic molecules and are shown in the table to the left •Diatomic elements can be separated. Compounds •A compound is a substance containing two or more elements that are chemically combined in a definite proportion by mass •Compounds, unlike elements, can be decomposed chemically into simpler substances ...

1. CH1000
Fundament
als of
Chemistry
Module 1 – Chapter 3
Elements and Atoms
• What is an element?
• An element is a fundamental substance that cannot be broken
down by chemical
means into a simpler substance.
• Elements are the building blocks of matter.
• Elements can occur naturally or be synthesized in labs.
• The smallest unit of an element that retains its properties and
chemical
behavior is called an atom.
• Atoms are made up of subatomic particles, but they do not
have the properties of the
element
Elements
•Ten elements make up

2. almost 99 % of the mass of
the Earth’s crust, seawater
and atmosphere.
•Oxygen accounts for about
20 % of the atmosphere
and is found in nearly all
rocks, sand and soil.
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.
Introduction to
the Periodic Table
•Elements with similar
chemical properties are placed
in columns called groups.
•Four groups have special
identifying names, like Noble
Gases, in group 8A, which are
all unreactive gases.

3. Introduction to
the Periodic
Table
•The eight tall columns are called representative elements, or
main group
elements. These are shown in red.
•The elements in the center are called the transition metals, or
sometimes
the “inner transition metals.” These are shown in purple.
Introduction to the Periodic
Table
•Elements can be further classified
as metals, metalloids and
nonmetals.
•Notice the bold, black “staircase”
on the table. Everything to the left
of the staircase is a metal and
everything to the right of the
staircase is a non metal.
• The exception is Hydrogen,
which is why some periodic
tables will show hydrogen
disconnected from the main
body of the table.

4. •The elements in grey touching the
“staircase” are called metalloids, or
semiconductor metals. These metals
are used in the semiconductor
industry.
Metals,
Nonmetal
s and
Metalloids
• Solid at room temperature (except mercury)
• Shiny
• Good conductors of heat and electricity
• Malleable (can be shaped)
• Ductile (can be drawn into wires)
• Most metals have a high melting point and density
Metals
• Not shiny
• Have fairly low melting points and densities
• Are poor conductors of heat and electricity
Non
Metals
• Metalloids have properties between metals and
nonmetals.
• These elements are positioned diagonally on the Periodic
Table separating the metals and nonmetals.

5. Metalloid
s
Diatomic Elements
•Diatomic molecules
contain exactly two atoms
•Seven elements exist as
diatomic molecules and are
shown in the table to the
left
•Diatomic elements can be
separated.
Compounds
•A compound is a substance
containing two or more
elements that are chemically
combined in a definite
proportion by mass
•Compounds, unlike elements,
can be decomposed chemically
into simpler substances
•Elements in compounds are
always combined in whole
number ratios.

6. Molecular and Ionic
Compounds
•Compounds fall into two general
types, molecular and ionic.
•Molecular compounds are held
together by covalent bonds
•Ionic compounds are held
together by attractive forces
between the positive and negative
charges.
Molecules and Ions
• What is a molecule?
• Molecules are the smallest unchanged individual unit of a
compound formed by two or
more atoms.
• A molecule cannot be further divided without destroying its
identity.
• What is an ion?
• Ions are charged atoms or groups of atoms. Ions can be
positively or negatively
charged.
• A positively charged ion is called a cation.

7. • A negatively charged ion is called an anion.
Writing
Formulas
of
Compound
s
The formula of a compound contains the symbols of all the
elements in the compound
When a formula contains only one atom of an element, the
number 1 is not needed as a subscript
When a formula contains more than one atom of an element,
the number is indicated by a subscript written after the symbol
Writing
Formulas
of
Compound
s
When the formula contains more than one of a group
of atoms that occur as a unit, parentheses are placed
around the group and the number of units is
represented by a subscript outside the parentheses.
Formulas show the number and kind of atoms in a
compound, but not the connectivity of the elements.

8. Composition of
Compounds
•A particular compound
always contains the same
elements in the same
proportions by mass no matter
what the origin.
•The Law of Definite
Composition states that a
compound always contains
two or more elements
chemically combined in a
definite proportion by mass.
Composition of
Compounds
•The Law of Multiple
Proportions states that atoms
of two or more elements may
combine in different ratios to
produce more than one
compound.
Reading
Review
What is the name of the periodic table group 8A?

9. What is the molecular formula for the diatomic
molecule, nitrogen?
What is the difference between a cation and anion?
What is the atomic number and symbol for the
potassium?
What are the elements in the center section of the
periodic table called?
Slide 1Elements and AtomsElementsSymbols of the
ElementsIntroduction to the Periodic TableIntroduction to the
Periodic TableIntroduction to the Periodic TableMetals,
Nonmetals and MetalloidsDiatomic
ElementsCompoundsMolecular and Ionic CompoundsMolecules
and IonsWriting Formulas of CompoundsWriting Formulas of
CompoundsComposition of CompoundsComposition of
CompoundsReading Review
CH1000
Fundament
als of
Chemistry
Module 1 – Chapter 4
Properties of
Substances
• Each substance has a set of properties that are characteristic
and give it a unique
identity.

10. • Properties are classified as either physical or chemical
• Physical properties are inherent characteristics that can be
determined without
altering the composition.
• Chemical properties describe the ability of a substance to
either undergo a
reaction with another substance or to decompose.
• No two substances have identical physical and chemical
properties.
Physical Changes
•Physical changes are changes in physical properties (such as
size
and density) or changes in states of matter without a change in
composition.
•No new substances are formed during a physical change!
•Sawing wood is a physical change – the wood changes shape,
but
the resulting pieces are still wood!
•Burning wood is a chemical change resulting in the release of
energy in the form of heat and light
Chemical
Changes

11. •In a chemical change, new
substances are formed that
have different properties and
composition from the original
material.
•For example, when copper
metal (Cu) is heated in air, the
shiny metal turns black as
copper(II) oxide is formed on
the surface.
Chemical Equations
•A chemical equation is
used to represent a
chemical change
•Reactants are on the left
hand side of the
equation. They are the
starting substances of a
reaction.
•Products are on the right
hand side of the
equation. They are the
substances produced in
the chemical reaction.
Reactants Products

12. Energy
• Energy is the capacity of matter to do work.
• Types of energy include mechanical, chemical, electrical and
nuclear.
• Potential energy (PE) is stored energy, the energy an obj ect
possesses due to its
position.
• Water backed up behind a dam
• Kinetic energy (KE) is energy that matter possesses due to its
motion.
• When the water backed up behind a dam is released, the PE
converts to KE in motion which
can be used to produce electricity.
• Law of Conservation of Energy: Energy cannot be created or
destroyed, only
transformed from one form to another.
• In chemistry, energy is most frequently released as heat.
Heat:
Quantitative
Measurement
•The SI unit for energy is
the joule (J).
•The specific heat of a
substance is the amount

13. of heat (gained or lost)
required to change the
temperature of 1 g of the
material by 1 °C.
•The specific heat of
water is much higher than
most substances.
Specific Heat Capacity
•When an object is heated
or cooled, the amount of
energy transferred depends
on three things:
• The amount of material
• The magnitude of the
temperature change
• The identity of the
material gaining or losing
energy
Reading Review
WHAT IS THE DIFFERENCE
BETWEEN PHYSICAL AND
CHEMICAL PROPERTIES?
WHAT IS THE DIFFERENCE
BETWEEN PHYSICAL AND

14. CHEMICAL CHANGES?
WHAT IS THE DIFFERENCE
BETWEEN POTENTIAL AND
KINETIC ENERGY?
WHAT IS THE LAW OF
CONSERVATION OF
ENERGY?
WHAT IS THE DIFFERENCE
BETWEEN SPECIFIC HEAT
AND HEAT?
Slide 1Properties of SubstancesPhysical ChangesChemical
ChangesChemical EquationsEnergyHeat: Quantitative
MeasurementSpecific Heat CapacityReading Review
CH1000
Fundament
als of
Chemistry
Module 1 – Chapter 5
Dalton’s Model of the Atom (Early
1800s)
• Elements are composed of small, indivisible particles called
atoms.

15. • Atoms of the same element are identical in mass and size.
• Atoms of different elements differ in their mass and size.
• Compounds are formed by combining two or more atoms of
different
elements.
• Atoms combine to form compounds in simple whole number
ratios.
• Atoms of two elements may combine in different ratios,
leading to
formation of different compounds.
Revisions to Dalton’s Theory
• Elements can be decomposed under certain conditions
• Not all atoms of the same element have identical mass.
• These are called isotopes.
• Atoms are not indivisible.
• Atoms are composed of subatomic particles.
The Atom
•Consists of subatomic particles
• Electron
• Proton
• Neutrons
•Protons and Neutrons exist in the
middle of the atom inside the
nucleus

16. • Protons have a positive charge
• Neutrons have no charge – they are
neutral
•Electrons exist on different orbitals
surrounding the nucleus
• Electrons have a negative charge
Electrons, Protons and Neutrons
• Atoms are composed of three smaller,
subatomic particles: electrons, protons
and neutrons.
• Protons and neutrons are located in
the nucleus.
• Electrons are dispersed throughout the
remainder of the atom (mainly open
space).
• Neutral atoms contain the same
number of protons and neutrons to
maintain charge balance.
The Effect of
Subatomic Particles
•Atoms can become ions by gaining or
losing electrons from this sphere
•Electrons are lost from atoms to form
cations.

17. •Electrons are gained from atoms to give
anions
Atoms, Ions, Mass
Number, Atomic
Number
•The number of protons and electrons are equal in an
atom
•In an ion, the number of protons does not equal the
number of electrons, providing a charge
•If the number of protons is greater than the number of
electrons, the ion is positively charged and called a
cation
•If the number of electrons is greater than the number
of protons, the ion is negatively charged and called an
anion
•The mass number is the number of protons and
neutrons in the nucleus. This also determines the atomic
weight
•The atomic number is the number of protons in the
nucleus.
Atomic Number and
Isotopes
•The atomic number is the
number of protons in the

18. nucleus of an atom
•The atomic number determines
the identity of the atom
•Atomic numbers for every
element are above the element’s
symbol in the periodic table
•Though all atoms of the same
element have the same number
of protons, atoms of the same
element may have different
numbers of neutrons
Isotopes of the
Elements
•An isotope is an atom of an
element which has the same
atomic number, but a different
number of neutrons from the
element
•The mass number is the total
number of protons and
neutrons for an element
Atomic Mass
• Because the mass of a single atom is so small, it is
inconvenient to use this as a mass unit.
• Instead, relative atomic mass units (amu) are used.
• Using carbon-12, C, as a standard, 1 atomic mass unit is equal
to 1/12th the mass of a carbon-
12 atom.

19. • Since most elements are a mixture of isotopes, the atomic
mass for an element
is the weighted average of all naturally occurring isotopes of
the element.
• To calculate the atomic mass:
• Take the sum of the atomic mass of each isotope multiplied by
its % abundance.
1 amu = 1.6606 x 10-24
g
Reading
Review
What are the three subatomic particles?
What is the relative charge for the three
subatomic particles?
What is the atomic number of an element?
What is an isotope?
What is atomic mass?
Slide 1Dalton’s Model of the Atom (Early 1800s)Revisions to
Dalton’s TheoryThe AtomElectrons, Protons and NeutronsThe
Effect of Subatomic ParticlesAtoms, Ions, Mass Number,
Atomic NumberAtomic Number and IsotopesIsotopes of the
ElementsAtomic MassReading Review

20. CH1000
Fundament
als of
Chemistry
Module 1 – Chapter 2
Scientific
Notation
Scientific notation is used to represent very
large or small numbers in math and science.
Writing a number as the product of a
number between 1 and 10 multiplied by 10
raised to some power is called scientific
notation
For help on using scientific notation on a
calculator, visit:
https://www.youtube.com/watch?
v=qE2BvtGiEMs
Measurement
and Uncertainty
•A measurement is always expressed by a
numerical value together with a unit of
measurement
•The certainty of a measurement is dependent
upon the calibration of the instrument

21. •It is customary when recording a
measurement to include all of the digits that
are known plus one digit that is estimated.
•The estimated digit introduces a level of
uncertainty into the measurement. It is
because of this uncertainty that every number
that expresses a measurement can only have
a limited number of digits
•These digits, used to express a measured
quantity are known as significant figures.
Significant
Figures
3 Rules
Nonzero digits
• All nonzero digits are significant
Exact Numbers
• Exact numbers occur in simple counting operations
• Direct conversions (12 inches in 1 foot) are also
considered exact numbers
• Exact numbers have no uncertainty
Zeros
• Only significant when:
• Between nonzero digits
• At the end of a number that includes a decimal point

22. • Not significant when:
• Before the first nonzero digit
• At the end of a number without a decimal point
Significan
t Figures
in
Calculatio
ns
For addition and subtraction use the
following rules:
Count the number of significant figures in the
decimal portion ONLY of each number in the
problem
Add or subtract in the normal fashion
Your final answer may have no more significant
figures to the right of the decimal than the LEAST
number of significant figures in any number in the
problem
For multiplication and division use the
following rule:
The LEAST number of significant figures in any
number of the problem determines the number of
significant figures in the answer. (You are now
looking at the entire number, not just the decimal
portion)
This means you have to be able to recognize
significant figures in order to use this rule
Example:
5.26 has 3 significant figures
6.1 has 2 significant figures
So, 5.26*6.1 = 32

23. To check your answers: https://www.sigfigscalculator.com/
The Metric
System
Also known as the
International or SI system, it
is a decimal system of units
for measurements of mass,
length, time and other
physical quantities
Common prefixes and
Numerical values for SI
units
SI Standard Units of
Measurement
Unit
Conversion
s
LENGTH (MM TO
M):
MASS (MG TO G):
VOLUME (L TO ML):

24. Temperatu
re
DEGREES CELSIUS = °C
KELVIN (ABSOLUTE) = K
DEGREES FAHRENHEIT = °F
K=°C + 273.15
°F = (1.8 * °C) +32
°C = (°F – 32)/1.8
HEAT IS THE FLOW OF ENERGY DUE TO
TEMPERATURE DIFFERENCE. HEAT ALWAYS
MOVES FROM HIGHER TEMPERATURE TO
LOWER TEMPERATURE
Density
• Ratio of mass to volume
Density
• Ratio of density of a
substance to the density
of water at 4°C
Specific Gravity
Reading Review
• How many significant figures are in 0.00025?

25. • Express 0.00025 in scientific notation.
• Draw a solution map from yd to m.
• What are the three most common temperature
scales?
• What is the difference between density and
specific gravity?
Slide 1Scientific NotationMeasurement and
UncertaintySignificant Figures 3 RulesSignificant Figures in
CalculationsThe Metric SystemUnit
ConversionsTemperatureDensityReading Review
CH1000
Fundament
als of
Chemistry
Module 1 – Chapter 1
An Introduction into Chemistry
• What is Chemistry?
• “Chemistry is the science of the composition, structure,
properties, and reactions of
matter, especially of atomic and molecular systems.”
• Simply put, chemistry is the study of matter and matter is any
object that has mass and
occupies space.
• The study of chemistry is vast and broad. From interactions
between atoms which form

26. the building blocks of the universe to large energetic changes
such as thermal transfer
which makes life possible. Your life is touched by chemistry
every day.
• Chemists try to understand the how and why chemical changes
occur.
• Chemists and other scientists use the scientific method as a
means to gain
understanding and solve problems.
The
Scientific
Method
Observations Laws
Hypothesis
Experiment
Theory
(model)
(analysis)
(explanation)
(analysis)
1. Make an observation / Form a question
2. Collect facts or data that is relevant to your

27. observation/question. (Generally done through
experimentation)
3. Formulate a hypothesis that accounts for the data on
hand and can be tested by further experimentation.
4. Plan and do additional experiments to test the
hypothesis.
5. Modify the hypothesis as necessary so that it is
compatible with all pertinent data.
Hypothesis
, Theory,
Laws
A hypothesis is a tentative explanation of certain facts that
provides a basis of further explanation.
• During experimentation, the hypothesis should be the expected
outcome of the process based on all previous information.
Once a hypothesis has become well tested and established,
it is called a theory, or a model.
• Scientific theory is well tested and generally established
information. It is
an explanation of the general principles of certain phenomena
with
considerable evidence or facts to support it.
• Scientific theory can be changed or disproven as new
information
becomes available and/or new discoveries are made.

28. Scientific laws are simple statements of natural phenomena
to which no exceptions are known under the given
conditions.
• An example of a scientific law is Newton’s law of gravity.
Gravity is a
natural phenomena which exists in the universe with no known
exceptions.
Physical States of Matter
– Solid, Liquid, Gas
•Solid
• Definite shape and volume
• Rigid particle structure
• Shape can be independent of
container
• Very slight compressibility
•Liquid
• Definite volume but indefinite
shape
• Firm but not rigid particle
structure (surface tension)
• Takes shape of container
• Slight compressibility
•Gas
• Indefinite volume and no

29. fixed shape
• Particles independent of each
other and far apart
• Highly compressible
Classifying Matter
•The term matter refers to all materials.
•A substance is a type of matter with a definite, fixed
composition.
•A pure substance is either an element or compound.
• Some common elements are copper, gold and iron
• Some common compounds are salt, sugar and water
•Homogeneous matter is uniform in appearance and has the
same
properties throughout
•Heterogeneous matter consists of two or more physically
distinct
phases
•A phase is the homogeneous part of a system separated from
other
parts by a physical boundary
•A system is simply the body of matter under consideration
Mixtures
• A mixture is a material
containing two or more

30. substances and can be
either heterogeneous or
homogeneous.
Pure Substance Mixture
Always has a definite
composition by mass.
Always contains two or more
substances that can be present
in varying amounts
The elements in a compound
lost their identities and may be
separated only by chemical
means.
The components of a mixture
do not lose their identities and
may be separated by physical
means
Matter
Pure Substance
(homogeneous
composition)
Mixtures of two
or more
substances
Elements Compounds

31. Solution
s
(homogeneous
composition – one
phase)
Heterogeneous
mixtures (two or
more phases)
Reading
Review
Provide an example of a homogeneous mixture.
Provide an example of a heterogeneous mixture.

32. List the physical states of matter.
True or False: A solution is another term for
homogeneous mixture
Fill in the blank: Oxygen is a ____ _________ which
exists in a mixture commonly known as air.
Slide 1An Introduction into ChemistryThe Scientific
MethodHypothesis, Theory, LawsPhysical States of Matter –
Solid, Liquid, GasClassifying MatterMixturesReading Review