structure of atom 3

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Atom 1a) Charged particles in matter :- b) Discovery of sub atomic particles :- Dalton’s Atomic Theory (experiment based!) Subatomic Particles Thomson’s Atomic Model b) Rutherford’s model of an atom :- c) Bohr’s model of an atom :- 4) Valency :- Atomic Number Mass Number Contents

Atoms :

Atoms

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“ Atoms are said to be the very tiny particles of any matter that cannot be divided any more after a certain stage “ for example : Take a chair and keep on doing its pieces , a stage will come when there will small particle left that particle can be said to be an atom. Atom

1a) Charged particles in matter :-:

1a) Charged particles in matter :- Atoms have three types of sub atomic particles. They are electrons, protons and neutrons. Electrons are negatively charged (e - ), protons are positively charged (p + ) and neutrons have no charge (n). The mass of an electron is 1/2000 the mass of a hydrogen atom. The mass of a proton is equal to the mass of a hydrogen atom and is taken as 1 unit. The mass of a neutron is equal to the mass of a hydrogen atom and is and is taken as 1 unit.

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b ) Discovery of sub atomic particles :- In 1900, J.J.Thomson discovered the presence of the negatively charged particles called electrons in the atom. In 1886, E.Goldstein discovered new radiations in gas discharge and called them canal rays. These rays were positively charged. This later led to the discovery of the positively charged particles called protons in the atom.

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In 1932 Chadwick discovered the presence of particles having no charge in the atom called neutrons. Neutrons

Thomson’s Atomic Model:

Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “ plum pudding ” model. J. J. Thomson

Dalton’s Atomic Theory (experiment based!):

Dalton’s Atomic Theory (experiment based!) Atoms of different elements combine in simple whole-number ratios to form chemical compounds In chemical reactions, atoms are combined, separated, or rearranged – but never changed into atoms of another element. All elements are composed of tiny indivisible particles called atoms Atoms of the same element are identical. Atoms of any one element are different from those of any other element. John Dalton (1766 – 1844)

Subatomic Particles:

Subatomic Particles Particle Charge Mass (g) Location Electron (e - ) -1 9.11 x 10 -28 Electron cloud Proton (p + ) +1 1.67 x 10 -24 Nucleus Neutron (n o ) 0 1.67 x 10 -24 Nucleus

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b) Rutherford’s model of an atom :- Rutherford’s alpha scattering experiment :- Rutherford allowed a beam of fast moving alpha particles ( α – particles) having positive charge to fall on a thin gold foil. He observed that :- i) Most of the α – particles passed straight through the gold foil. ii) Some of the α – particles were slightly deflected by small angles. iii) Very few α – particles appeared to rebound.

Defects of Rutherford’s model of the atom :-:

Defects of Rutherford’s model of the atom :- Any particle in a circular orbit would undergo acceleration and during acceleration the charged particle would radiate energy. So the revolving electrons would lose energy and fall into the nucleus and the atom would be unstable. We know that atoms are stable. Negatively charged electron Positively charged nucleus Very small positively charged nucleus Negatively charged electrons in orbits around the nucleus - - - + Rutherford’s model of an atom

c) Bohr’s model of an atom :- :

c) Bohr’s model of an atom :- i) An atom has a positively charged nucleus at its centre and most of the mass of the atom is in the nucleus. ii) The electrons revolve around the nucleus in special orbits called discrete orbits. iii) These orbits are called shells or energy levels and are represented by the letters K, L, M, N etc. or numbered as 1, 2, 3, 4, etc. iv) While revolving in the discrete orbits the electrons do not radiate energy.

3) Distribution of electrons in different shells :-:

3) Distribution of electrons in different shells :- The distribution of electrons in the different shells was suggested by Bhor and Bury. The following are the rules for filling electrons in the different shells. i) The maximum number of electrons in a shell is given by the formula 2n 2 where n is the number of the shell 1, 2, 3 etc. First shell or K shell can have = 2n 2 = 2 x 1 2 = 2x1x1 = 2 electrons Second shell or L shell can have = 2n 2 = 2 x 2 2 = 2x2x2 = 8 electrons Third shell or M shell can have = 2n 2 = 2 x 3 2 = 2x3x3 = 18 electrons Fourth shell or N shell can have = 2n 2 = 2 x 4 2 = 2x4x4 = 32 electrons and so on.

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ii) The maximum number of electrons that can be filled in the outermost shell is 8. iii) Electrons cannot be filled in a shell unless the filled. inner shells are

Composition of the atoms of the first eighteen elements :-:

Composition of the atoms of the first eighteen elements :- Name of element Symbol Atomic Number Number of Protons Number of Neutrons Number of Electrons Distribution Of Electrons K L M N Valency Hydrogen H 1 1 - 1 1 - - - 1 Helium He 2 2 2 2 2 - - - 0 Lithium Li 3 3 4 3 2 1 - - 1 Beryllium Be 4 4 5 4 2 2 - - 2 Boron B 5 5 6 5 2 3 - - 3 Carbon C 6 6 6 6 2 4 - - 4 Nitrogen N 7 7 7 7 2 5 - - 3 Oxygen O 8 8 8 8 2 6 - - 2 Fluorine F 9 9 10 9 2 7 - - 1 Neon Ne 10 10 10 10 2 8 - - 0 Sodium Na 11 11 12 11 2 8 1 - 1 Magnesium Mg 12 12 12 12 2 8 2 - 2 Aluminium Al 13 13 14 13 2 8 3 - 3 Silicon Si 14 14 14 14 2 8 4 - 4 Phosphorus P 15 15 16 15 2 8 5 - 3,5 Sulphur S 16 16 16 16 2 8 6 - 2 Chlorine Cl 17 17 18 17 2 8 7 - 1 Argon Ar 18 18 22 18 2 8 8 - 0

Atomic structure of the first eighteen elements :-:

Atomic structure of the first eighteen elements :- H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar

4) Valency :-:

4) Valency :- Valency is the combining capacity of an atom of an element. The electrons present in the outermost shell of an atom are called valence electrons. If an atom’s outermost shell is completely filled, they are inert or least reactive and their combining capacity or valency is zero. Of the inert elements Helium atom has 2 electrons in the outermost shell and the atoms of other elements have 8 electrons in their outermost shell. Atoms having 8 electrons in their outermost shell is having octet configuration and are stable. If an atom’s outermost shell is not completely filled it is not stable. It will try to attain stability by losing, gaining or sharing electrons with other atoms to attain octet configuration.

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The number of electrons lost, gained or shared by an atom to attain octet configuration is the combining capacity or valency of the element Eg :- Hydrogen, Lithium, Sodium atoms can easily lose 1 electron and become stable. So their valency is 1. Magnesium can easily lose 2 electrons. So its valency is 2. Aluminiun can easily lose 3 electrons. So its valency is 3. Carbon shares 4 electrons. So its valency is 4. Fluorine can easily gain 1 electron and become stable. So its valency is 1. Oxygen can easily gain 2 electrons. So its valency is 2. Nitrogen can easily gain 3 electrons. So its valency is 3.

Atomic Number:

Atomic Number Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. Element # of protons Atomic # (Z) Carbon 6 6 Phosphorus 15 15 Gold 79 79

Mass Number:

Mass Number Mass number is the number of protons and neutrons in the nucleus of an isotope: Mass # = p + + n 0 Nuclide p + n 0 e - Mass # Oxygen - 10 - 33 42 - 31 15 8 8 18 18 Arsenic 75 33 75 Phosphorus 15 31 16

Isotopes:

Isotopes Frederick Soddy (1877-1956) proposed the idea of isotopes in 1912 Isotopes are atoms of the same element having different masses , due to varying numbers of neutrons. Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials.

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Isotopes are atoms of the same element having different masses , due to varying numbers of neutrons. Isotope Protons Electrons Neutrons Nucleus Hydrogen–1 (protium) 1 1 0 Hydrogen-2 (deuterium) 1 1 1 Hydrogen-3 (tritium) 1 1 2

6) Isobars :-:

6) Isobars :- Isobars are atoms of different elements having different atomic numbers but same mass numbers. These pairs of elements have the same number of nucleons. Eg :- Calcium (Ca) – atomic number - 20 and Argon (Ar) – atomic number 18 have different atomic numbers but have the same mass numbers – 40. Iron (Fe) and Nickel (Ni) have different atomic numbers but have the same atomic mass numbers – 58. 20 18 40 40 58 58 27 26 Fe Ca Ar Ni

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