Instructor: Liu Dapeng ( Department of Chemistry, College of Science )

E-mail: liudp@upc.edu.cnTeaching 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

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)

1. Content

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.

Chemistry

Inorganic Chemistry

AnalyticalChemistry

Physical Chemistry

Organic

Chemistry

• Chemistry is the science that is concerned with the composi

tion, structure, and properties of matter and changes that matte

r undergoes. Generally chemistry mainly includes four branches,

they are:

The Classification of Chemistry:

• Inorganic Chemistry (initial chemistry)

The study of the synthesis and behavior of inorganic and organometallic compounds. It has appli

cations 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 inform

ation about the composition and structure of matter.  It is the art

and science of determining what the matter is and  how much of i

t exists.

Environmental Chemistry

Pharmaceutical Analysis

Chemical Analysis

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.

oil quality analyzer 2 oil quality analyzer I

Real-Space Identification of Intermolecular Bonding with

Atomic Force Microscopy

AFM measurements of 8-hq assembled clusters on Cu(111).

8-hq

• Organic Chemistry (synthesis mechanism)

The branch of chemistry that deals with the structure, propertie

s, 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 at

omic 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

G. N. Lewis (1875-1946)

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

unit of radiant energy.

G. N. Lewis have responded: Physical chemistry is everything that is interesting!

Scope of Chemistry

new materials, energy, health and environment.

food, clothing, housing and transportation -- the four basic needs of everybody.

agriculture, industry, national defense and science and technology.

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.

Chemists work in all

these areas.

Chemists must design strategies to extract or synthesize all kinds of things from relatively simple stating material;

Definition

Chemistrydefinition The scientific discipline that treats

the composition, properties, and transformations of matter.

Matterdefinition Anything that occupies space and

has mass; the physical material of the universe.

Atom:definition

The smallest representative particle of an element.

Moleculedefinition

A chemical combination of two or more atoms.

• 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.

Why Study Chemistry

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.

The ideal crystalline structure of graphene is a hexagonal grid

Graphene

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

physical properties

chemical properties

Hardness, color, melting point and density

sodium and potassium react

with water

Properties of matter can be divided into physical properties and chemical properties.

Properties of matter

intensive properties

extensive properties

such as mass and volume: depend on sample size

Properties of matter also can be divided into

intensive properties and extensive properties.

such as density, color, and

boiling point

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.

The physical properties of sodium metal is: it is a soft, lustrous, silver-colored metal with a relatively low melting point and low density.

For instance

Figure 1.1 shows a chunk of metallic sodium.

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.

2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)

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 exampleOne chemical property of sodium and potassium is that they can react with water:

•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.

Physical and Chemical changes

changes of matter

Physicalchanges

Chemical changes

All changes of state are physical changes

Changes of matter’s

chemical identity

Figure 1.2 Three States of the matter

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

Questions

choice

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

Questions

choice

1.3 Classification of matter by composition

• 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.

Pure Substances and Mixtures

Compounds

• Most elements interact to form compounds.

• Example, H2O

• The proportions of elements in compounds are the s

ame irrespective of how the compound was formed.

• Law of Constant Composition (or Law of Definite P

roportions):

–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

Substancedefinition

combinations of two or more substances in which each substance retains its chemical identity. Have varying compositions and can be separated by physical changes.

Compoundsdefinition substances composed of two or

more elements; they contain two or more kinds of atoms .

Elementsdefinition substances that cannot be

decomposed into simpler substances. On the molecular level, each element is composed of only one kind of atom.

Mixturesdefinition

matter that has distinct properties and a composition that does not vary from sample to sample.

Definition

Homogeneous

definition Have only one phase. Mixtures that are uniform throughout are homogeneous. Homogeneous mixtures are also called solutions

Phasedefinition A sample of matter that is uniform

in composition and physical state and is separated from other phases by definite boundaries.

Heterogeneousdefinition

Do not have the same properties throughout the sample.

1. Iced tea2. Isopropyl alcohol3. Helium4. Sugar

Questions

Each of the following can be classified as a heterogeneous mixture, pure substance, compound, or element. How would you classify each?

1. Iced tea: heterogeneous mixture

2. Isopropyl alcohol: pure substance

3. Helium: pure substance and element

4. Sugar: pure substance and compound

Answers:

Matter can be classified according to its composition.

All matter

Can it be separated by physical method?

No Yes

Substance Mixture

Can it be decomposed by

chemical process?

Is it uniform throughout?

Compound Element HomogenousHeterogeneous

NoYes No Yes

Separate

A heterogeneous mixture

the components of ink

by filtration

using chromatography

a homogeneous mixture

by distillation

Methods of Separating Mixtures

A mixture can be separated into its components by appropriate physical means. For example: we can

• 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.

Figure 1.3 Filtration separates a liquid from a

solid.

A mixture of solid and liquid

can be separated by

filtration through a funnel

and filter paper, which is

physical means.

Filtratioin

Figure 1.4 The solution is boiled and steam is driven off.

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.

Distillation

Figure 1.5 Salt remains after all water is boiled off.

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.

Distillation

Figure 1.6 No chemical change occurs when salt water is distilled.

Distillation is the physical change.

Figure 1.7 Separation of a sand-saltwater mixture.

Union of Filtration and Distillation

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.

Decomposing water

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) O2(g) + 2H2(g)

For Exampl

e

11 percent

89 percent

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

However, it is wrong to suppose that merely following a set of procedures, rather like using a cookbook, will guarantee scientific success.

The Scientific method

observation experimentation

hypothesestheories

The Scientific method is the combination of.

Definition

Natural lawdefinition concise statements, often in

mathematical form, of the facts of nature.

Theorydefinition A model or way of looking at nature

that can be used to explain natural laws and make further predictions about natural phenomena.

hypothesisdefinition

A hypothesis is a tentative explanation of a natural law.

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 co

mpounds is usually made up of ions; that is, it is a binary ionic co

mpound.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 = Sodium chloride

“ide” ending

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 Symbol Name Symbol

Lithium ion Li+ Chromium (II) ion Cr2+

Sodium ion Na+ Chromium(III) ion Cr3+

Potassium ion K+ Iron(III) ion Fe3+

Rubidium ion Rb+ Iron(II) ion Fe2+

Cesium ion Cs+ Copper(I) ion Cu+

Magnesium Mg2+ Copper(II) ion Cu2+

Calcium ion Ca2+ Mercury(I) ion Hg22+

Barium Ba2+ Mercury(II) ion Hg2+

Aluminum ion Al3+ Tin(II) ion Sn2+

Zinc ion Zn2+ Lead(II) ion Pb2+

Positive ions (cations)

Name symbol Name symbol

Hydride ion H- Iodide ion I-

Fluoride ion F- Oxide ion O2-

Chloride ion Cl- Sulfide ion S2-

Negative ions (anions)

Writing formulas when names of compounds are given

Write formulas for the compounds barium oxide,calcium fluoride,and iron(III) sulfide.SolutionSolution

In each case, identify the cations and charges, based on

periodic table group numbers or on oxidation states appea

ring as Roman numberals in names : Ba+,Ca2+,and Fe3+.The

n identify the anions and their charges:O2-,F-,and S2- .Comb

ine the cations and anions in the relative numbers require

d to produce electrically neutral formula units.

 barium oxide: one Babarium oxide: one Ba2+2+and one Oand one O2- 2- = BaO= BaO

calcium fluoride: one Cacalcium fluoride: one Ca2+2+ and two F and two F-- =CaF =CaF22

iron(III) sulfide: two Feiron(III) sulfide: two Fe3+3+ and three S and three S2- 2- = Fe= Fe22SS33

Naming compound when their formulas are given.

Write acceptable name for the compounds Na2S, AlF3, Cu2O.

SolutionSolution

Na2S : sodium sulfide

AlF3 : aluminum fluoride

Cu2O : copper(I) oxide

Binary Compounds of Two NonmetalsBinary 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. SO2 = sulfur dioxide

SO3 = sulfur trioxide

B2Br4 = diboron tetrabromideWhen the prefix ends in When the prefix ends in aa or or oo and the element name begins with and the element name begins with

aa or or oo,the final vowel of the prefix is dropped for ease of pronuncia,the final vowel of the prefix is dropped for ease of pronuncia

tion.For example,carbon tion.For example,carbon monmonoxide, not carbon oxide, not carbon monomonooxide,and dioxide,and di

nitrogennitrogen tetrtetroxide,not dinitrogen oxide,not dinitrogen tetratetraoxide.However, PI3 is phospoxide.However, PI3 is phosp

horushorus tri triiodide, not phosphorusiodide, not phosphorus tritriodide.odide.

In both the formula and the name, we write the element with the positive oxidation state first.

Binary Acids

In naming acids we use the prefix hydro followed by the na

me of the other nonmetal modified with an ic ending. The m

ost important binary acids are listed below

HF (aq) = hydrofluoric acid

HCl (aq) = hydrochloric acid

HBr (aq) = hydrobromic acid

HI (aq) = hydroiodic

H2S (aq) = hydrosulfuric acidThe symbol (aq) signifies a substance in aqueous(water) so

lution

Polyatomic Ions

In polyatomic ions, two or more atoms are joined together by covalent bonds. These ions are commonly encountered, especially among the nonmetals.

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 HSO4- NaHSO4

Some Common Polyatomic Ions

Oxyacids

The majority of acids are ternary compounds. They contai

n three different elements-hydrogen, and two other nonmetal

s. If one of the nonmetals is oxygen, the acid is called an oxo

acid. The table for naming oxoacids is similar to that outlined

for oxoanions, except that the ending ous is used instead of i

te and ic instead of ate.

Oxidation state

Formula of acid Name of acid Formula of salt

Name of salt

Cl: +1 HClO Hypochlorous acid NaClO Sodium hypochlorite

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

Nomenclature of Some Oxoacids and Their Salts

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.

(b) The polyatomic anion HH22POPO44- - is dihydrogen phos is dihydrogen phos

phate ion.Two of these ions are present for every Caphate ion.Two of these ions are present for every Ca2+ 2+ ion in the compound calcium dihydrogen phospha ion in the compound calcium dihydrogen phosphate.te.

ClO2 is not chlorite ion,it carries no net charge

Applying Various Rules in Writing Formulas

Write the formula of the compound (a) tetranitrogen tetrasulf

ide; (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 chr

omate 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.