Instructor: Liu Dapeng
( Department of Chemistry, College of Science )
E-mail: liudp@upc.edu.cn
Teaching Plan
Chapter 1: Introduction Chapter 2: Measurement
Chapter 3: Stoichiometry Chapter 4: Reactions in Solution
Chapter 5: Gases
Chapter 6: Thermochemistry
Chapter 7: Atomic structure
Chapter 8: Periodic Table
Chapter 9: Chemical Bonds
Chapter 14: Chemical Equilibrium
Chapter 15: Acids and Bases
Chapter 17: Chemical Thermodynamics
1.7 Teaching Arrangement
1. Content
Ch1-Ch9, Ch14-15 , Ch17
Two main topics:
Basic laws and principles of chemical reactions
and their applications in different systems,
(macroscopical)
Atomic structure and structure of substance.
(microscopical)
2. Ways to learn and Requirements
Preparation
Attendance of the lecture and necessary notes
Review and homework
Experiments in lab
Question- answering
All-around review and examination
Learning skills:
(1) Listen to the teacher carefully and take notes when
necessary. (The teacher repeated: important? Can not
understand in class?)
(2) Read the textbook and find out problems. (Refer to related
books? Search online? Discuss with classmates? Discuss
with the teacher?)
(3) Finish the assignments by yourself.
(4) Summarize each chapter. (Understand the theory. Know
the general procedure of solving problems. Remember the
important parts. )
Make progress everyday!
3. Evaluation and score
The final score = Attendence×10% + Homework×10%
+ Experiment operation and report×10% +
Examination×70%
Your final score depends on your own performance!
1 Introduction
Contents
1-1 The Scope of Chemistry
1-2 Properties of Matter: Physical and Chemical properties
1-3 Classification of Matter:
Elements, Compounds and Mixtures
1-4 The Scientific Method
1-5 Atoms
1-6 Naming Inorganic Compounds
1-7 Teaching Arrangement
1-1
The Scope of Chemistry
• Chemistry is the science that is concerned with the
composition, structure, and properties of matter and the changes
that matter undergoes.
•
Matter is anything that occupies apace. Matter is made up of
almost infinitesimally small building blocks called atoms.
•
Atoms can combine together to form molecules.
Molecules of a few
familiar substances
are represented here.
The Classification of Chemistry:
• Chemistry is the science that is concerned with the
composition, structure, and properties of matter and changes
that matter undergoes. Generally chemistry mainly includes
four branches, they are:
Chemistry
Inorganic
Chemistry
Analytical
Chemistry
Organic
Chemistry
Physical
Chemistry
• Inorganic Chemistry (initial chemistry)
The study of the synthesis and behavior of inorganic and
organometallic compounds. It has applications in every aspect
of the chemical industry including:
Catalysis
Material Science
Solid State Chemistry
Semiconductor
Petroleum Industry
Analytical Chemistry (measurement chemistry)
The science of obtaining, processing, and communicating
information about the composition and structure of matter. It is
the art and science of determining what the matter is and how
much of it exists.
Environmental Chemistry
Pharmaceutical Analysis
Chemical Analysis
oil quality analyzer I
oil quality analyzer 2
It can detect the quality of the oil and get much information
about oil in three minutes. It is very light, portable and convenient
for analyzing the oil that is being used in all kinds of fields. It can
also be used to analyze the quality of water and other materials if
you have the appropriate software.
8-hq
Real-Space Identification of Intermolecular Bonding with
Atomic Force Microscopy
AFM measurements of 8-hq assembled clusters on Cu(111).
• Organic Chemistry (synthesis mechanism)
The branch of chemistry that deals with the structure,
properties, and reactions of compounds that contain carbon.
Pharmaceutical Chemistry
Biochemistry
Polymer
Synthesis Chemistry
• In 19C, Liebig analyzed a lot of organic compounds.
• In 1824, Wöhler synthesized urea successfully.
• In 1865, KeKule proposed the ring structure of benzene.
Physical Chemistry (based theory)
•to develop a fundamental understanding at the molecular and
atomic level of how materials behave and how chemical
reactions occur. With the knowledge that is relevant in nearly
every area of chemistry, it has diverse topics:
Material Science
Fundamental Chemistry
Quantum computers
Petroleum Industry
Gilbert Newton Lewis was an
American physical chemist known for
(1) the discovery of the covalent bond
(2) purification of heavy water
(3) reformulation of chemical
thermodynamics in a mathematically
rigorous manner accessible to ordinary
chemists
(4) his theory of Lewis acids and bases
(5) his photochemical experiments
(6) coined the term “photon" for the smallest
G. N. Lewis
(1875-1946)
unit of radiant energy.
G. N. Lewis have responded: Physical chemistry is
everything that is interesting!
Scope of Chemistry
food, clothing, housing and transportation -- the four
basic needs of everybody.
agriculture, industry, national defense and science and
technology.
new materials, energy, health and environment.
Chemists
work in all
these areas.
Chemists must design strategies to extract or
synthesize all kinds of things from relatively simple
stating material;
Society requires improved methods of pollution
control;
substitutes for scarce materials;
nonhazardous means of disposing of toxic
wasters;
and more efficient ways to extract energy from
fuels.
Definition
definition
Chemistry
definition
Atom:
Matter
The smallest representative particle
of an element.
definition Anything that occupies space and
has mass; the physical material of
the universe.
definition
Molecule
The scientific discipline that treats
the composition, properties, and
transformations of matter.
A chemical combination of two or
more atoms.
Why Study Chemistry
• Chemistry is the study of the properties of materials
and the changes that materials undergo.
• Chemistry is central to our understanding of other
sciences.
• Chemistry is also encountered in everyday life.
Graphene
The SEM images graphene
The Raman images graphene
Graphene has been studied and applied widely all over the
world for its unique properties such as the thinnest and hardest
nanomaterial, almost completely transparent, very high thermal
conductivity and electron mobility higher than that of carbon
nano-tube or silicon crystal, the world's minimum resistivity.
Graphene
The ideal crystalline structure of graphene is a hexagonal grid
Challenges to 21 Century
• Global warming and environmental protection
• Development of new energy sources
• Development of nano-technology
• Development of life science
Chemistry is the central science today!
Nanotech in sustainable energy application
solar panels
nanocatalysts in
petroleum treating
1-2
Properties of Matter
Properties of matter can be
divided into physical properties
and chemical properties.
Hardness, color,
melting point
and density
physical properties
Properties of
matter
chemical properties
sodium and
potassium react
with water
Properties of matter also can be divided into
intensive properties and extensive properties.
such as density,
color, and
boiling point
Properties of
matter
intensive
properties
extensive
properties
such as mass
and volume:
depend on
sample size
Physical and Chemical properties
Properties that do not involve substances changing into other
substances are called physical properties, which are those
that we can determine without changing the identity of the
substance we are studying.
For instance
The physical properties of
sodium metal is: it is a soft,
lustrous,
silver-colored
metal with a relatively low
melting point and low
density.
Figure 1.1 shows a chunk
of metallic sodium.
Properties that involve substances changing into other
substances are called chemical properties, which describe the
way a substance can change or react to form other substances.
For example
One chemical property of
sodium and potassium is that
they can react with water:
2Na(s) + 2H2O(l)
2NaOH(aq) + H2(g)
These properties, then, must be determined using a process
that changes the identity of the substance of interest. To
determine, we would have to combine an alkali metal with water
and observe what happens.
Physical and Chemical changes
changes of
matter
Physical
changes
Chemical
changes
All changes of
state are
physical
changes
Changes of
matter’s
chemical identity
•A change that doesn’t involve changing any substance into any
other substance is called a physical change. In a chemical
change, one or more substances are changed into other
substances.
The changes undergone by sodium and potassium when they
react with water are chemical changes. Matter can also undergo
physical changes. One example is the melting of a solid.
Figure 1.2 Three States of the matter
Questions
1. A freshly cut surface of sodium quickly becomes
dull with a film of white sodium oxide when it is
exposed to air. Is this a physical change or a
chemical change?
Physical or Chemical
choice
Questions
2. Another property of sodium is that it conducts
electricity, as do all metals. Is electrical conductivity
an intensive or extensive property of sodium metal?
Intensive or Extensive
choice
1.3
Classification of matter by composition
Pure Substances and Mixtures
• Elements consist of a unique type of atom.
• Molecules can consist of more than one type of
element.
– Molecules that have only one type of atom (an
element).
– Molecules that have more than one type of atom
(a compound).
• If more than one atom, element, or compound are
found together, then the substance is a mixture.
Compounds
• Most elements interact to form compounds.
• Example, H2O
• The proportions of elements in compounds are the
same irrespective of how the compound was formed.
• Law of Constant Composition (or Law of Definite
Proportions):
–The composition of a pure compound is always the
same.
• Pure
Substances
and Mixtures
• Pure Substances and Mixtures
• If matter is not uniform throughout, then it is a
heterogeneous mixture.
• If matter is uniform throughout, it is homogeneous.
• If homogeneous matter can be separated by physical
means, then the matter is a mixture.
• If homogeneous matter cannot be separated by
physical means, then the matter is a pure substance.
• If a pure substance can be decomposed into
something else, then the substance is a compound.
Definition
definition
matter that has distinct properties and a
composition that does not vary from
sample to sample.
definition
substances that cannot be
decomposed into simpler substances.
On the molecular level, each element is
composed of only one kind of atom.
Substance
Elements
Compounds
Mixtures
definition substances composed of two or
more elements; they contain two or
more kinds of atoms .
definition combinations of two or more
substances in which each substance
retains its chemical identity.
Have varying compositions and can
be separated by physical changes.
Definition
definition
Phase
Homogeneous
definition Have only one phase. Mixtures that are
uniform throughout are homogeneous.
Homogeneous mixtures are also called
solutions
definition
Heterogeneous
A sample of matter that is uniform
in composition and physical state
and is separated from other phases
by definite boundaries.
Do not have the same properties
throughout the sample.
Questions
Each of the following can be classified as
a heterogeneous mixture, pure substance,
compound, or element. How would you
classify each?
1.
2.
3.
4.
Iced tea
Isopropyl alcohol
Helium
Sugar
Answers:
1. Iced tea: heterogeneous mixture
2. Isopropyl alcohol: pure substance
3. Helium: pure substance and element
4. Sugar: pure substance and compound
Matter can be classified according to its composition.
All matter
No
Can it be separated
by physical method?
Substance
Yes
Can it be
decomposed by
chemical process?
Compound
Yes
Mixture
No
No
Yes
Is it uniform
throughout?
Element
Heterogeneous
Homogenous
Methods of Separating Mixtures
A mixture can be separated into its components by
appropriate physical means. For example: we can
by filtration
A heterogeneous
mixture
Separate
a homogeneous
mixture
the components
of ink
by distillation
using chromatography
• Chromatography can be used to separate mixtures
that have different abilities to adhere to solid
surfaces.
• The greater the affinity the component has for the
surface (paper) the slower it moves.
• The greater affinity the component has for the liquid,
the faster it moves.
• Chromatography can be used to separate the
different colors of inks in a pen.
States of Matter
• Matter can be a gas, a liquid, or a solid.
• These are the three states of matter.
• Gases take the shape and volume of their container.
• Gases can be compressed to form liquids.
• Liquids take the shape of their container, but they do
have their own volume.
• Solids are rigid and have a definite shape and
volume.
Filtratioin
A mixture of solid and liquid
can be separated by
filtration through a funnel
and filter paper, which is
physical means.
Figure 1.3 Filtration separates a liquid from a solid.
Distillation
Saltwater is a
homogeneous mixture
and a solution.
Saltwater can be
heated until the water
changes into steam
and then cooled until it
becomes water again.
This is the process of
distillation.
Figure 1.4 The solution is boiled and steam is driven off.
Distillation
Salt remains and the
water is vaporized and
cooled again. The
principles of the
method is utilizing the
different boiling
points of the different
components of the
mixture.
Figure 1.5 Salt remains after all water is boiled off.
Distillation is the physical change.
Figure 1.6 No chemical change occurs when salt
water is distilled.
Union of Filtration and Distillation
Figure 1.7 Separation of a sand-saltwater mixture.
Decomposing water
For
Example
Each, can be decomposed into other substances
by a chemical process. For example, the water
can be decomposed into oxygen and hydrogen ,
namely electrolysis.
2H2O(g)
89 percent
O2(g) + 2H2(g)
11 percent
The substances produced by the electrolysis of water cannot be
further separated by any physical or chemical means. Water is
11 percent hydrogen and 89 percent oxygen by mass. This is an
example of the law of constant composition.
Electrolysis, the
decomposition of water
by an electric current, is
a chemical process.
Figure 1.8 Electrolysis of H2O
1-4
The Scientific Method
Observation: natural or experimental
Tentative explanation: hypothesis
Revise if experiments show
hypothesis is inadequate
Experiments designed to test hypothesis
Theory(or model) that amplifies hypothesis
and gives predictions
Modify theory if experiments
show model is inadequate
Experiments to test predictions of theory
Theory established unless later experiments or
observations show inadequacies of model
The Scientific method
observation
experimentation
hypotheses
theories
The Scientific method is
the combination of.
However, it is wrong to suppose that merely following a set of
procedures, rather like using a cookbook, will guarantee
scientific success.
Definition
definition
Natural law
definition
hypothesis
Theory
concise statements, often in
mathematical form, of the facts of
nature.
A hypothesis is a tentative
explanation of a natural law.
definition A model or way of looking at nature
that can be used to explain natural
laws and make further predictions
about natural phenomena.
1-5
Atoms
• Matter is made up of very small particles called atoms.
• The modern atomic theory was suggested by an English
schoolteacher, John Dalton, in 1803-07:
1. All matter is composed of atoms. Atoms is the smallest
particles of an element that takes part in chemical reactions.
2. All atoms of a given element are alike. Atoms of different
elements are different.
3. Compounds are combinations of atoms of more than one
element; in a given compound, the relative number of each
type of atom is always the same.
4. Atoms cannot be created or destroyed.
• Nucleus: is at the center of the atom and is
small, dense, and positively charged.
Proton: Small particles with a unit of positive charge
in the nucleus of a atom.
Neutron: Particles with no charge and are present in
the nuclei of all atoms expect one isotope of
hydrogen.
• Electron: is an extremely small particles with a unit
of negative charge.
1-6
Naming of Inorganic Compounds
Binary Compounds of Metals and Nonmetals
Binary Compounds are those formed between two element.If one
of the elements is a metal and the other a nonmetal,the binary
compounds is usually made up of ions; that is, it is a binary ionic
compound.To name a binary compound of a metal and a
nonmetal
 Write the unmodified name of the metal
 Then write the name of the nonmetal,modified to end in ide
Name unchanged
NaCl
=
“ide” ending
Sodium chloride
Ionic compounds, though made up of positive and
negative ions, must be electrically neutral. The net, or total,
charge of the ions in a formula unit must be zero.
Name
Lithium ion
Sodium ion
Potassium ion
Rubidium ion
Cesium ion
Magnesium
Calcium ion
Barium
Aluminum ion
Zinc ion
Positive ions (cations)
Symbol
Name
Li+
Chromium (II) ion
Chromium(III) ion
Na+
K+
Iron(III) ion
Rb+
Iron(II) ion
Cs+
Copper(I) ion
Mg2+
Copper(II) ion
Ca2+
Mercury(I) ion
Mercury(II) ion
Ba2+
Al3+
Tin(II) ion
Zn2+
Lead(II) ion
Symbol
Cr2+
Cr3+
Fe3+
Fe2+
Cu+
Cu2+
Hg22+
Hg2+
Sn2+
Pb2+
Negative ions (anions)
Name
symbol
Name
symbol
Hydride ion
H-
Iodide ion
I-
Fluoride ion
F-
Oxide ion
O2-
Chloride ion
Cl-
Sulfide ion
S2-
Writing formulas when names of compounds are given
Write formulas for the compounds barium oxide,calcium
fluoride,and iron(III) sulfide.
Solution
In each case, identify the cations and charges, based on
periodic table group numbers or on oxidation states
appearing as Roman numberals in names : Ba+,Ca2+,and
Fe3+.Then identify the anions and their charges:O2-,F-,and
S2- .Combine the cations and anions in the relative
numbers required to produce electrically neutral formula
units.
barium oxide: one Ba2+and one O2- = BaO
calcium fluoride: one Ca2+ and two F- =CaF2
iron(III) sulfide: two Fe3+ and three S2- = Fe2S3
Naming compound when their formulas are given.
Write acceptable name for the compounds Na2S, AlF3, Cu2O.
Solution
Na2S : sodium sulfide
AlF3 : aluminum fluoride
Cu2O : copper(I) oxide
Binary Compounds of Two Nonmetals
If the two elements in a binary compound are both
nonmetals instead of a metal and a nonmetal, the compound
is a molecular compound. The method of naming these
compounds is similar to that just discussed. For example
HCl = hydrogen chloride
Generally, we indicate relative numbers of atoms through
prefixes: mono =1,di =2,tri =3, tetra =4,penta =5,hexa =6,
and so on.
SO = sulfur dioxide
2
SO3 = sulfur trioxide
B2Br4 = diboron tetrabromide
When the prefix ends in a or o and the element name begins with
a or o,the final vowel of the prefix is dropped for ease of
pronunciation.For example,carbon monoxide, not carbon
monooxide,and dinitrogen tetroxide,not dinitrogen
tetraoxide.However, PI3 is phosphorus triiodide, not phosphorus
triodide.
In both the formula and the
name, we write the element
with the positive oxidation
Binary Acids
In naming acids we use the prefix hydro followed by the
name of the other nonmetal modified with an ic ending. The
most important binary acids are listed below
HF (aq) = hydrofluoric acid
HCl (aq) = hydrochloric acid
HBr (aq) = hydrobromic acid
HI (aq) = hydroiodic
H2S (aq) = hydrosulfuric acid
The symbol (aq)
signifies a
substance in
aqueous(water)
solution
Polyatomic Ions
In polyatomic ions, two or more atoms are joined together
by covalent bonds. These ions are commonly encountered,
especially among the nonmetals. Some Common Polyatomic Ions
Name
Formula
Typical
Cation: Ammonium ion
NH4+
NH4Cl
Anions: Cyanide ion
CN-
NaCN
Hydroxide ion
OH-
NaOH
Hypochlorite ion
ClO-
NaClO
Perchlorate ion
ClO4-
NaClO4
Nitrite ion
NO2-
NaNO2
Nitrate ion
NO3-
NaNO3
Phosphate ion
PO43-
Na3PO4
Hydrogen phosphate ion
HPO42-
Na2HPO4
Sulfate ion
SO42-
Na2SO4
Hydrogen sulfate ion
HSO
-
NaHSO4
Oxyacids
The majority of acids are ternary compounds. They
contain three different elements-hydrogen, and two other
nonmetals. If one of the nonmetals is oxygen, the acid is
called an oxoacid. The table for naming oxoacids is similar to
that outlined for oxoanions, except that the ending ous is
used instead of ite and ic instead of ate.
Nomenclature of Some Oxoacids and Their Salts
Oxidation Formula of acid
state
Name of acid
Formula
of salt
Name of salt
Cl: +1
HClO
Hypochlorous acid NaClO
Cl: +5
HClO3
Chloric acid
NaClO3 Sodium chlotate
Cl: +7
HClO4
Perchloric acid
NaClO4 Sodium perchlorate
N: +3
HNO2
Nitrous acid
NaNO2
Sodium nitrite
N: +5
HNO3
Nitric acid
NaNO3
Sodium nitrate
S: +6
H2SO4
Sulfuric acid
NaSO4
Sodium sulfate
S: +4
H2SO3
Sulfurous acid
NaSO3
Sodium sulfite
Sodium
hypochlorite
Applying Various Rules in Naming Compounds.
Name the compounds (a)ClO2; (b)Ca(H2PO4)2
Solution
(a) Both Cl and O are nonmetals.ClO2 is a binary
molecular compound called chlorine dioxide.
ClO2 is not chlorite ion,it
carries no net charge
(b) The polyatomic anion H2PO4- is dihydrogen
phosphate ion.Two of these ions are present for every
Ca2+ ion in the compound calcium dihydrogen
phosphate.
Applying Various Rules in Writing Formulas
Write the formula of the compound (a) tetranitrogen
tetrasulfide; (b) ammonium chromate; (c) calcium
hypochlorite.
Solution
(a)Molecules of this compound consist of four n atoms and four
S atoms. The formula is N4S4.
(b) Two ammonium ions (NH4+ )must be present for every
chromate ion(CrO42-). Place parentheses around NH4+
,followed by the subscript 2.The formula is (NH4)2CrO4.
(c) Here there are one Ca2+ and two ClO- ions in a formula
unit.This leads to the formula Ca(ClO)2.