الرئيسية
أحدث الصور
عبدالله معارك الأحد فبراير 19, 2012 10:12 am محافظة القاهرة
إدارة حدائق القبة التعليمية
Ahmed maher experimental language school
Objective :
At the end of this lesson studenties should be able to
Identify the atomic structure
Obtain the skill to producing cathode ray and its properties
Lesson :Atomic structure
Aid : using work sheet
Plane : we must know the Atomic structure
1-Greek philosopher
2-Aristotle attempt
3- Boyle attempt
-Element
4- Dalton attempt
Cathode rays
1- Gases normally do not conduct electricity but it could conduct electricity in discharge tubes with pressure ranges between 0.01 – 0.001 mm Hg and potential difference of about 10,000volts
2- A stream of invisible rays was emitted from the cathode causing a fluorescent glow on the tube wall
5- Discovery of cathode rays
A stream of electrons produced at the negative electrode (cathode) of a vacuum glass tube containing a gas at low pressure.
*Properties of cathode rays
1- They are considered as subatomic particles
2- They are having thermal effect
3- They are having negative charge
4- They are deflected by magnetic and electric fields
5- They are move in straight line
6- They are do not differ in their nature and behavior by the difference of cathode substance or type of gas so it proved by that it entrees in the structure of all matter
6- Thomson's atom
7- Ernest Rutherford atoms
He deduced the following postulates about the structure of the atom
1- The atom: it is small in size and has complicated structure that is similar to the solar system
2- The nucleus: is much smaller than the atom with a positive charge and lie in the center of atom, there is vast space between the nucleus and the orbits of electrons
3- A negative charged electrons rotate around the nucleus
a- The mass of the atom is concentrated in its nucleus because the mass of electrons negligible if it is compared to the mass of nucleus
b- The atom is electrically neutral because the number of (+ve) charges inside the nucleus (protons) equals the number of (-ve) charges out side the nucleus electrons
c- The electrons travel around the nucleus in special orbits at a tremendous speed despite of the mutual attraction between them the attraction force is overcome by another force that equals in quantity and opposes in direction namely the centrifugal force
Excited atom It the atom which has gained an amount of energy sufficient to transfer electron from their original energy level to higher ones
The quantum Is the amount of energy absorbed or emitted when the electron jumps from one energy level to another
Or it is limited amount of energy that can't be divided or multiplied
The orbit
It is an imaginary circular line where the electron moves in a certain direction
Inadequacy of Bohr's atomic model
Modern atomic theory
The dual nature of electron
That is to say the electron has dual nature
The difference between matter wave and electromagnetic wave
Evaluation
What is the:
Properties of cathode rays
· The orbit
· The quantum
· The dual nature of electron
محافظة القاهرة
إدارة حدائق القبة التعليمية
Ahmed maher experimental language school
Objective :
At the end of this lesson studenties should be able to
Identify the Quantum numbers
Obtain the skill to producing Quantum numbers
Lesson : Quantum numbers
Aid : using work sheet
Plane : we must know the Quantum numbers
*It is used to define the number of the principle [main] energy levels which are equal to seven in the heaviest known atom in its ground state
- There are seven principle energy levels in the heaviest atom that can be found around the nucleus in its ground and are designated by the symbols K, L, M, N, O, P and Q
- It takes any positive whole number values 1, 2, 3, 4…Excluding zero
- It is used to determine the maximum number of electrons required filling a certain energy level or which saturated a certain energy level, from the rule [2n2 ] where n is the shell number
- Bohr has used this number in explaining the spectrum of hydrogen atom
- There is big difference in energy between the principle energy levels of the atom
The subsidiary [orbital or azimuthal] quantum number [l]
*It define the number of energy sublevels in each energy level
1- There are four energy sublevels are designated by symbols s,> p,> d,> f.
2- There is a small difference in energy between the sublevels in the same energy level
3- The number of sublevels equals the number of the principal energy level it takes any positive whole numbers values [n]
The magnetic quantum number [m]
The quantum number that defines the number of orbital in each sublevel containing it
* It defines the number of orbital in each sublevel containing it and it defines the shape of sublevel in space or their direction [orientation] in space
Sommerfield
The scientist which introduced the energy sublevels and define its number by using a spectroscope with high resolving power - Each orbital is saturated with two electrons
*Sublevel [S]
Has one orbital of spherical symmetrical shape around the nucleus
*Sublevel [P]
Consists of three orbital [PX, PY, PZ.] are perpendicular to each other
The electron cloud of each orbital takes the form of two pears meeting head to head [dumb- bell shaped] at a node at which the electron density = zero
The spin quantum number [ms]
It used to describe the spin motion of an electron around its axis or nucleus in either a clockwise or anticlockwise direction
ms = 1/2 or -1/2
Principle of distributing electrons
1- Aufbau [building up] principle
"Electrons occupy the sublevels in the order of increasing their energy the lowest energy sublevels are filled first"
2- Hund's rule
No pairing of electron takes place until each orbital contains one electron
Evaluation
Write the electronic configuration of the following
1- N7 3- Al13 5- Zn30
2- O8 4- Cl17
Write the electronic configuration of the following elements according to Hund's rule
1- N7 3- Al13 5- Ar18
2- O8 4- Cl17
Give reasons
1- The electron does not fall in the nucleus inspite of the attraction
force between them.
2- Atom is electrically neutral.
إدارة حدائق القبة التعليمية
Ahmed maher experimental language school
At the end of this lesson studenties should be able to
Identify the atomic structure
Obtain the skill to producing cathode ray and its properties
Lesson :Atomic structure
Aid : using work sheet
Plane : we must know the Atomic structure
Summary
1-Greek philosopher
2-Aristotle attempt
3- Boyle attempt
-Element
4- Dalton attempt
Cathode rays
1- Gases normally do not conduct electricity but it could conduct electricity in discharge tubes with pressure ranges between 0.01 – 0.001 mm Hg and potential difference of about 10,000volts
2- A stream of invisible rays was emitted from the cathode causing a fluorescent glow on the tube wall
5- Discovery of cathode rays
A stream of electrons produced at the negative electrode (cathode) of a vacuum glass tube containing a gas at low pressure.
*Properties of cathode rays
1- They are considered as subatomic particles
2- They are having thermal effect
3- They are having negative charge
4- They are deflected by magnetic and electric fields
5- They are move in straight line
6- They are do not differ in their nature and behavior by the difference of cathode substance or type of gas so it proved by that it entrees in the structure of all matter
6- Thomson's atom
7- Ernest Rutherford atoms
He deduced the following postulates about the structure of the atom
1- The atom: it is small in size and has complicated structure that is similar to the solar system
2- The nucleus: is much smaller than the atom with a positive charge and lie in the center of atom, there is vast space between the nucleus and the orbits of electrons
3- A negative charged electrons rotate around the nucleus
a- The mass of the atom is concentrated in its nucleus because the mass of electrons negligible if it is compared to the mass of nucleus
b- The atom is electrically neutral because the number of (+ve) charges inside the nucleus (protons) equals the number of (-ve) charges out side the nucleus electrons
c- The electrons travel around the nucleus in special orbits at a tremendous speed despite of the mutual attraction between them the attraction force is overcome by another force that equals in quantity and opposes in direction namely the centrifugal force
Excited atom It the atom which has gained an amount of energy sufficient to transfer electron from their original energy level to higher ones
The quantum Is the amount of energy absorbed or emitted when the electron jumps from one energy level to another
Or it is limited amount of energy that can't be divided or multiplied
The orbit
It is an imaginary circular line where the electron moves in a certain direction
Inadequacy of Bohr's atomic model
Modern atomic theory
The dual nature of electron
That is to say the electron has dual nature
The difference between matter wave and electromagnetic wave
Evaluation
What is the:
Properties of cathode rays
· The orbit
· The quantum
· The dual nature of electron
class | period | date |
إدارة حدائق القبة التعليمية
Ahmed maher experimental language school
At the end of this lesson studenties should be able to
Identify the Quantum numbers
Obtain the skill to producing Quantum numbers
Lesson : Quantum numbers
Aid : using work sheet
Plane : we must know the Quantum numbers
Summary
The principle quantum number[n]*It is used to define the number of the principle [main] energy levels which are equal to seven in the heaviest known atom in its ground state
- There are seven principle energy levels in the heaviest atom that can be found around the nucleus in its ground and are designated by the symbols K, L, M, N, O, P and Q
- It takes any positive whole number values 1, 2, 3, 4…Excluding zero
- It is used to determine the maximum number of electrons required filling a certain energy level or which saturated a certain energy level, from the rule [2n2 ] where n is the shell number
- Bohr has used this number in explaining the spectrum of hydrogen atom
- There is big difference in energy between the principle energy levels of the atom
The subsidiary [orbital or azimuthal] quantum number [l]
*It define the number of energy sublevels in each energy level
1- There are four energy sublevels are designated by symbols s,> p,> d,> f.
2- There is a small difference in energy between the sublevels in the same energy level
3- The number of sublevels equals the number of the principal energy level it takes any positive whole numbers values [n]
The magnetic quantum number [m]
The quantum number that defines the number of orbital in each sublevel containing it
* It defines the number of orbital in each sublevel containing it and it defines the shape of sublevel in space or their direction [orientation] in space
Sommerfield
The scientist which introduced the energy sublevels and define its number by using a spectroscope with high resolving power - Each orbital is saturated with two electrons
*Sublevel [S]
Has one orbital of spherical symmetrical shape around the nucleus
*Sublevel [P]
Consists of three orbital [PX, PY, PZ.] are perpendicular to each other
The electron cloud of each orbital takes the form of two pears meeting head to head [dumb- bell shaped] at a node at which the electron density = zero
The spin quantum number [ms]
It used to describe the spin motion of an electron around its axis or nucleus in either a clockwise or anticlockwise direction
ms = 1/2 or -1/2
Principle of distributing electrons
1- Aufbau [building up] principle
"Electrons occupy the sublevels in the order of increasing their energy the lowest energy sublevels are filled first"
2- Hund's rule
No pairing of electron takes place until each orbital contains one electron
Evaluation
Write the electronic configuration of the following
1- N7 3- Al13 5- Zn30
2- O8 4- Cl17
Write the electronic configuration of the following elements according to Hund's rule
1- N7 3- Al13 5- Ar18
2- O8 4- Cl17
Give reasons
1- The electron does not fall in the nucleus inspite of the attraction
force between them.
2- Atom is electrically neutral.