Organic Chemistry Presentation Grp 1_2003

I. Matters 1. 2. 3. 4. 5.

Definition of Matters States of Matter Changing processes of Matter Properties of Matter Substance vs. Mixture

II. Atoms 1. Structure • • •

Electron Nucleus De Broglie and Bohr models

1. Atomic and mass number 2. Application

II. Molecules 1. Definition and general overview 2. Formulas • •

Classification Nomenclature

IV.Ions 1. 2. 3. 4. 5.

Definition Classification Ionic vs. molecule compound Nomenclature Applications

1.Definition of Matters • The common definition of matter is anything that has both mass and volume (occupies space). Example : Car, pen, ball…etc…

2.States of Matter •There are 4 states of Matters : o Solid o Liquid o Gas o Plasma

Conservation between 4 states of Matter

Remember !!! Solid => Liquid => Gas => Plasma Higher temperature Plasma is a type of matters appear almost everywhere in the universe. – Very high temperature and low pressure. – The electrons are separate from nucleus

Plasma

3.Changing processes of Matter 3.1 Physical changes A change that each substance involved in the change remains at it origin and no new elements or compounds are formed. Ex : Water freezing at -0oC 3.2 Chemical changes A change that one or more elements or compounds (substances) are formed. Ex : HCl + NaOH => NaCl + H20

4.Properties of Matter 4.1 Physical properties • Boiling point • Freezing point • Solubility • Viscosity • Density • …..etc…

4.Properties of Matter 4.2 Chemical properties • Oxidation • Flammability • Chemical stability • Toxicity • …etc…

5.Mixture vs. Substance • Substance : A chemical substance is a material with a specific chemical composition. Elements and compounds are substances. • Mixture : A mixture is when two or more different substances are mixed together but not combined chemically. Mixture contains of Homogeneous and Heterogeneous mixture

Classification of substances • Element : A substance that cannot be broken down into simpler substances by any kind of reactions. Ex : Carbon, Gold , Iodine… • Compound : A substance composed of two or more elements chemically combined in fixed ratios by mass. Ex : Water , Carbon dioxide , Methane…

Classification of mixture •

Homogeneous : A mixture having only one phase with the same properties Ex : Milk, blood, shampoo..

•

Heterogeneous : A mixture with more than one phase with different properties Ex : Pizza, water and oil, cereal and milk…

Summary

1.Definition and - history In 1897, J. J. Thomson showed by his famous experiment that there were small charged particles; today we call these particles electrons

Cathode - ray tube Joseph John Thomson 1856-1940

1.Definition and Ernest Rutherford discovered that atom has positively charged history nucleus through the gold foil experiment (1911).

Ernest Rutherford 18711937

An atom includes: nucleus and electrons

1.Definition and history Bohr’s model (1913)

• Electrons travel in discrete orbit around the nucleus like the Solar System. • Electrons gain or lose energy when they change to another orbits.

Niels Bohr (18851962)

2. Structure Electron - A stable negatively charged subatomic particle with a mass 1,836 times less than that of the proton, found in all atoms and acting as the primary carrier of electricity in solids.

2. Structure Has negative charge (-1) • Weigh 9.1 x 10-28 g • Movement: orbits the nucleus arranges in shells creates electron cloud

Orbital • Describes the volume of space around a nucleus that an electron is most likely to occupy. • There are four different kinds of orbitals.

- The orbitals in an atom are organized into different layers, or electron shells, of successively larger size and energy.

• Different shells contain different numbers and kind of orbitals • Each orbital within a shell can be occupied by two electrons. + The 1st shell: only a single s orbital - 1s - holds only 2 electrons. + The 2nd shell: one 2s orbital + three 2p orbitals - holds a total of 8 electrons. + The 3rd shell: a 3s orbital, three 3p orbitals, and five 3d orbitals - total capacity of 18 electrons.

Nucleus 1/ Proton -Has positive charge (+1) -Weigh 1.67 x 10-24 g 2/ Neutron -Has no electric charge - Weigh 1.67 x 10-24 g -The number of neutrons determines the isotope of an element.

Isotope Atoms of one element have : The same number of protons Different from the number of neutrons  It means the same atomic number Z, but different mass numbers A

Atomic and mass number 3.1 Atomic Number The atomic number (Z) is the number of protons in the nucleus of an atom of an element.

3.2 Atomic Mass Number The mass number (A) is the total number of nucleons (sum of the numbers of protons and neutrons) in one atom of an element.

4.Application 4.1 Radioactivity decay:

The process of losing energy of an unstable atomic releases ionizing particles and radiation. Plant: The scientists use radioactive rays to influence the nucleic acid and to make mutation. This is a way to create a new strain but we can’t control the mutation yet. Therefore, the scientists must test the new strain and propagate the good strain.

Green peas

Oat

Wheat

Some examples of using radioactive rays on plant Plant Mutated Location Mutation Green peas Oat Wheat

Rice …

species and time Weibull Switzerland Increases productivity 5Stralart , 1953 10% Alamo-X America, Increases resistance 1961 NP 836 India, 1961 Increase productivity, resistance and heatresistant DT10 Vietnam, Increases productivity, 1990 short growth time

4.Application

4.2 Kill the harmful insect:

a. Set free the male insects were made sterile by radioactive rays. These male insects will copulate with female insects to produce those sterile eggs Reduce the population of insect or cause extinct b. Set free the male and female insects have detrimental gene due to radioactive rays. They will copulate with normal insect to produce defective generation. Reduce the population of insect or cause extinct

4.Application 4.3 X-rays

• X-rays have been use in medical imaging. • X-rays is largely used for the management of cancer.

Radiotherapy equipment

X-ray image

4.Application 4.4 Chemotherapy

• The treatment that using agents which poison cells to demolish the goal tumor. • Most of the drugs are transported by the bloodstream; most do not cross the blood–brain barrier.  Cannot reach the central nervous system.

4.Application 4.5 Marking in Bioresearches - Using the isotope to mark researching molecules in living bodies. * Example: In plants research, sciencetists use O18 to replace O16 for finding out the source of Oxygen eliminated after photosynthesis.

1.Definition and general overview • Definition - What is the molecule?  Molecule is the smallest particle of a compound that has all the chemical properties of that compound  Molecules are made up of two or more atoms joined by one or more covalent chemical bonds

1.Definition and general overview • Size  Almost molecules are too small to be seen by naked eye  The smallest molecule is the diatomic hydrogen (H2)

1.Definition and general overview • Examples Carbon Dioxide (CO2) 1 black carbon atom 2 red oxygen atoms

1.Definition and general overview • Examples Sulfuric acid (H2SO4) 1 yellow sulfur atom 4 red oxygen atoms 2 white hydrogen atoms

2.Formulas • Classification  Empirical formulas

A formula that gives the simplest whole-number ratio of atoms in a compound.  Molecular formulas

The molecular formula specifies the actual number of atoms of each element in a molecule.

3.Nomenclature - Add prefixes to indicate numbers of atoms. Omit “mono-” prefix on the FIRST element. -Change the ending of the second element to “-ide”.

3.Nomenclature PREFIX monoditritetrapentahexaheptaoctanonadeca-

Number 1 2 3 4 5 6 7 8 9 10

3.Nomenclature • Examples – H2O :

Dihydrogen monoxide

– SO2 :

Sulfur dioxide

– N2O5:

Dinitrogen pentoxide

– PCl5:

Phosphorus pentacloride

NF3 NO NO2 B2O3 N2O N2O4 PCl3 SF6 PCl5 CO2

NF3 NO NO2 B2O3 N2O N2O4 PCl3 SF6 PCl5 CO2

Nitrogen trifluoride

NF3

Nitrogen trifluoride

NO

Nitrogen monoxide

NO2 B2O3 N2O N2O4 PCl3 SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO

Nitrogen monoxide Nitrogen dioxide

NO2 B2O3 N2O N2O4 PCl3 SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O N2O4 PCl3 SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4 PCl3 SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4

Dinitrogen tetroxide

PCl3 SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4

Dinitrogen tetroxide

PCl3

Phosphorus trichloride

SF6 PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4

Dinitrogen tetroxide

PCl3

Phosphorus trichloride

SF6

Sulfur hexafluoride

PCl5 CO2

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4

Dinitrogen tetroxide

PCl3

Phosphorus trichloride

SF6

Sulfur hexafluoride

PCl5

Phosphorus pentachloride

CO2

Carbon dioxide

NF3

Nitrogen trifluoride

NO NO2

Nitrogen monoxide Nitrogen dioxide

B2O3

Diboron trioxide

N2O

Dinitrogen monoxide

N2O4

Dinitrogen tetroxide

PCl3

Phosphorus trichloride

SF6

Sulfur hexafluoride

PCl5

Phosphorus pentachloride

CO2

Carbon dioxide

1.Definition Anion : •The atom which has negative charge. • From nonmetals we can form anions from reduction.

1.Definition Cation

• Atom or group of atoms carries a positive charge. • After oxidation a metal becomes cation The reaction between hydrogen and fluorine is an example of an oxidation-reduction reaction: H2 + F2 → 2 HF The overall reaction may be written as two halfreactions: H2 → 2 H+ + 2 e− (the oxidation reaction) F2 + 2 e− → 2 F− (the reduction reaction)

1.Definition Ionic compounds Definition: Ionic compounds are built from positive ions (cations ) and negative ions (anions ). Structure: large numbers of ions can attract to form clusters and crystals

2.Classification

2.1 Monatomic ions A monatomic ion is simply an ion consisting of one element. Ex: Na+ or Au+3 , or Zn+2 , or Al+3

2.Classification

2.2 Polyatomic ions

A polyatomic ion is consisting of more than one element. Ex: SO4-2 , or NO3-, or NH4+

3.Properties 3.1 Physical properties • Ionic compounds have high melting and boiling points. • Electrical conductivity when they’re melted • Ionic compounds are generally soluble in water and other polar solvents having high dielectric constants. However ionic compounds are insoluble in non-polar solvents.

3.Properties 3.2 Chemical properties • Neutralization reactions HCl + NaOH  NaCl + H20 H2SO4 + Ba(OH)2  BaSO4 + 2 H20 • Double displacement reactions NaCl + AgNO3  NaNO3 + AgCl

.Ionic vs. molecular compoun •When atoms join together, they form either molecules or ionic compounds. When atoms join together by covalent bonds, they form “molecules”.  When atoms join together by ionic bonds, they form “ionic compounds Nonmetal + nonmetal → covalent bond → molecular compound

Metal + nonmetal → ionic bond → ionic compound

Table compare molecular and ionic compounds

5.Nomenclature Most ionic compounds’s name have TWO parts.The first part is the name of the cation, and the second part is the name of the anion.

First: name the cation • If the cation just has only one possible charge , the name of cation will just be the name of element • If the cation is a transition metal (more than one charge), you need to specify whether charge of cation. Ex : Fe+3 ion just has the name "iron (III)".

5.Nomenclature Second : Name the anion The name of the anion is the same as the name of the element and "-ide" is added to the end Ex: oxygen becomes "oxide", sulfur becomes "sulfide", phosphorus is "phosphide

If the anion has more than one atom (polyatomic ion), look up the polyatomic ion in table Ex: OH- is "hydroxide", SO42- is sulfate

6.Applicati Methods on for producing useful water Water contains high concentration of Ca2+ Mg2+ Ag2+ is unusable for human beings. Treatment with anion (SO42- , PO33- …) can reduce the concentration of those cation. => makes water usable

References •

• • • • • • •

"The Columbia Encyclopedia, Sixth Edition. 2008. Retrieved September 19, 2009 from Encyclopedia.com: http://www.encyclopedia.com/doc/1E1molecule.html http://www.tutorvista.com/content/chemistry/chemistry-iii/chemicalbonding/ionic-compounds.php http://misterguch.brinkster.net/ionic.html http://antoine.frostburg.edu/chem/senese/101/compounds/ionicvscovalent.shtml Chemistry concepts and problems, 2nd edition, Clifford C. Houk – Richard Post Chemistry principles and reactions, sixth edition, Masterton – Hurley Cancer chemotherapy, Rachel Airley Chemistry, fifth edition, Zumdahl

THANKS FOR YOUR KIND ATTENTION

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