1. IndexThomsons model of the atomRutherfords atomic modelBohrs model of electronsAtomic number and mass numberIsotopes
2. Thomsons model of The aTomAtoms and molecules are the fundamental buildingblocks of matter. The presence of matter around usin different forms is a result of the difference inatoms constituting them. Till the 19thcentury, Dalton’satomic theory captured the minds of people. Histheory stated that atoms are indivisible, but soon itwas observed that atoms are not indivisible.
3. Many scientists have performed various experiments toverify the presence of charged particles in atoms. J.J.Thomson identified electrons (negatively charged particles),while E. Goldstein discovered protons (positively chargedparticles) present in atoms.As an atom is always neutral, the number of electrons isequal to the number of protons present in an atom. The nextchallenge for the scientists was to suggest a model for theatoms i.e. an arrangement of the subatomic particles in theatom.
4. Sir J. J Thomson, credited for the discovery of electrons,proposed the first model for atoms. His proposal statedthat the model of an atom is similar to the model of a plumpudding or watermelon. Thomson’s model can be explainedwith the help of a watermelon. He said that the positivecharge in the atom is spread all over like the red edible partof the watermelon. Also, the electrons are embedded in thepositively charged sphere like the seeds in the watermelon(as shown in the given figure).
5. Explanation of Thomson’s model.Hence, according to Thomson’s atomic model: An atom consists of a positively charged sphere with electrons embedded in it. The negative and positive charges present inside an atom are equal in magnitude. Therefore, an atom as a whole is electrically neutral.
6. Thomson’s model of the atom is also known as the plum pudding model.Positivelycharged sphere ElectronsThomson’s model of the atom became very popular as it proved that atoms are neutral entities. However, this model was not able to explain the results of experiments obtained by other scientists such as Earnest Rutherford, who was performing experiments on radioactivity.
7. RuTheRfoRds aTomIc modelErnest Rutherford, while performing experiments onradioactivity, bombarded fast moving alpha particles on athin gold foil (about 1000 atoms thick). He selected the goldfoil because of its high ductility; and doubly charged alphaparticles because of their large amount of energy. Heexpected to see small deflections of alpha particles by thesub-atomic particles present in gold atoms. The followingfigure shows the set-up of his experiment.
8. From the experiment, he made the following observations:1. Most of the fast moving α-particles passed straight through the gold foil.2. Some α-particles were deflected through the foil by small angles.3. Surprisingly, one out of every 12,000 particles rebounded i.e., they got deflected by an angle of 180º.
9. Deflection pattern of alpha rays as observed byRutherford
10. Rutherford derived the following conclusions from the gold foil experiment:1. Since most α-particles passed through the gold foil without any deflection, most of the space inside an atom is empty.2. Very few particles suffered a deflection from their path. This means that positive charge occupies very little space inside an atom.3. As a small fraction of particles got deflected completely by the angle of 180º, all positive charge and mass of gold atoms are present within a very small volume inside the atom.
11. Explanation of α -particle scattering experiment
12. Rutherford gave a new atomic model known as the Rutherford atomic model ornuclear model of the atom. The major features of the model are as follows.1 All protons are present inside the nucleus, which is situated at the centre ofthe atom.2. Electrons reside outside the nucleus and revolve around the nucleus in well-defined orbits.3. The size of the nucleus is very small in comparison to the size of an atom. Asper Rutherford’s calculations, the size of the nucleus is 105 times smaller thanan atom.4. As the mass of the electron is negligible in comparison to the mass of theproton, almost all the mass of the atom is concentrated in the nucleus.
13. Rutherford’s atomic model
14. Drawbacks of Rutherford’s nuclear modelThe Rutherford’s model explains the structure of atom in a very simple way.But, it suffers from the following drawbacks1. An electron revolving around the nucleus gets accelerated towards thenucleus. According to the electromagnetic theory, an accelerating chargedparticle must emit radiation, and lose energy. Because of this loss of energy,the electron would slow down, and will not be able to withstand the attractionof the nucleus. As a result, the electron should follow a spiral path, andultimately fall into nucleus. If it happens then the atom should collapse inabout 10-8 second. But, this does not happen: atoms are stable. This indicatesthat there is something wrong in the Rutherford’ mass nuclear model ofatom..
15. 2. The Rutherford’s model of atom does not say anything aboutthe arrangement of electrons in an atom.Therefore, Rutherfords model was not accepted.
16. Bohrs Model of electronsRutherford’s atomic model was able to explain all theobservations except the stability of atoms. In 1913, Niels Bohrgave some postulates to explain the structure of atoms andthe distribution of charged particles in it.Bohr’s postulates:1.Only certain special orbits known as discrete orbits ofelectrons are allowed inside the atom.2.While revolving in discrete orbits, the electrons do notradiate energy.
17. Bohr named these orbits as energy levels. These orbits orshells are represented by the letters K, L, M, N…, or thenumbers n = 1, 2, 3, 4…etc.
18. Merits of Bohr’s ModelBohr’s model explains the arrangement anddistribution of electrons in an extra nuclearspace. He successfully explained the stability ofatoms by his proposal of the presence ofenergy levels around the nucleus of the atomsin which the electrons revolve without radiatingenergy.
19. Discovery of the NeutronsIn 1932, J. Chadwick discovered another subatomic particleand named it neutron. It has no charge and has a massnearly equal to that of a proton. Neutrons are present in thenuclei of all atoms, except hydrogen. It is generallyrepresented by ‘N’.The mass of the neutron has been found to be 1.6749 ×10−27 kg, which is slightly more than that of the proton.Hence, the mass of the atom is equal to the sum of themasses of protons and neutrons present in the nucleus.
20. Distribution of the electrons in the nucleusThe number of electrons that a particular orbit canaccommodate is fixed. Therefore, the number ofelectrons present in different orbits is different.Bohr and Bury together suggested certain rules toshow how electrons are distributed in differentorbits. These rules have to be followed for writing thenumber of electrons in different energy levels.
21. First rule: The maximum number of electrons present in a shell is given bythe formula 2n², where ‘n’ is the orbit number or energy level index (1, 2,3…). Hence, the maximum number of electrons that different shells canaccommodate is as follows: 1. First orbit or K-shell can accommodate maximally 2 x 1² = 2 electrons. 2. Second orbit or L-shell can accommodate maximally 2 x 2² = 8 electrons. 3. Third orbit or M-shell can accommodate maximally 2 x 3² = 18 electrons. 4. Fourth orbit or N-shell can accommodate maximally 2 x 4² = 32 electrons.
22. Second rule: The maximum number of electrons that canbe accommodated in the outermost orbit is eight.Third rule: Electrons cannot be filled in the outer shell untilthe inner shells are completely filled. This means that shellsare filled in a step-wise manner, starting from the innershell.
23. ValencyFrom the Bohr-Bury scheme, we know that the outermostshell of an atom can hold a maximum of eight electrons. Theelements, whose atoms have a completely filled outermostshell, have very little chemical activity. Such elements aresaid to have zero combining capacity or valency. For e.g.,neon atom has eight electrons in its outermost shell. Itcannot hold more than eight electrons. Hence, its valency iszero. We all know that neon is inert in nature.
24. The combining capacity of atoms of the elements is their tendencyto react with other atoms of the same or different molecules toattain a filled outermost shell. The outermost shell, which haseight electrons, is said to possess an octet and every atom tendsto achieve an octet in its outermost shell. This is done by gaining,losing, or sharing its electrons. The number of electrons gained,lost, or shared by an atom to complete its octet is called thecombining capacity or valency of that atom.Both hydrogen and sodium contain one electron each in theiroutermost shells. Thus, both can lose one electron. Hence, theirvalency is one.
25. It is not always true that the number of electrons present inthe outermost shell of an atom represents its valency. Forexample, in fluorine, there are seven electrons in theoutermost shell, but the valency of fluorine is one. This isbecause it is energetically suitable for fluorine atom toaccept one electron, rather than donate seven electrons.Hence, its valency is obtained by subtracting sevenelectrons from the octet.
26. Atomic Number and Mass Number
27. The number of protons present inhydrogen, carbon, and sodium are 1, 6, and11 respectively. Hence, the atomic numberof hydrogen, carbon, and sodium is 1, 6, and11 respectively.
28. MASS NUMBERThe mass of an atom is equal to the number of protons andneutrons present in that atom, because the mass ofelectrons is very less and is considered negligible whencompared to the mass of protons and neutrons. Protonsand neutrons are present inside the nucleus of an atom.Hence, protons and neutrons are also called nucleons.Thus, the mass of an atom resides in its nucleus.
29. The mass number is defined as the sum of the total number ofprotons and neutrons present inside the nucleus of anatom. The mass number is usually denoted by ‘A’. The unit used torepresent the mass number is unified atomic mass unit i.e. ‘u’. Thegeneral representation or symbolic notation to represent an atomwith its atomic number and mass number is shown below.Here, ‘E’ is the symbol of the element, ‘Z’ is the atomic number, and‘A’ is the mass number.
30. Relation between the Atomic Mass and Mass Number of anAtom:Mass number (A) of an atom = Number of protons + Number ofneutronsTherefore, Mass number (A) = Atomic number (Z) + Number ofneutronsTherefore, Number of neutrons = A - ZHence, the number of neutrons can be calculated if the atomicnumber and mass number of an element are known.
31. An atom of sodium contains 11 protons and 12 neutrons. Now, mass number (A) = number of protons + number of neutronsTherefore, mass number of sodium atom = 11 + 12= 23Hence, the mass number of sodium is 23 u.
32. IsotopesUnlike the mass number, the atomic number is unique for anelement. In nature, a number of atoms of some elementshave been identified having the same atomic number, butdifferent mass numbers. Such atoms are knownas isotopes.Isotopes are defined as atoms having the same atomicnumber, but different mass numbers. These atomscontain an equal number of protons and electrons, but adifferent number of neutrons.
33. ApplicationsIn nature, an element is found as a mixture of its isotopes.The chemical properties of all isotopes of an element arethe same, but physical properties are different. Therefore,the isotopes of some elements have specific properties thatmake them very useful.For example, an isotope of uranium exhibits nuclear fissionproperties. It is used in nuclear reactions as a fuel. Anisotope of cobalt is used to treat cancer, and an isotope ofiodine is used to treat goitre.
34. IsobarsIsobars are atoms of different elements having the same mass number. These elements have an equal number of nucleons, but different number of protons, neutrons, and electrons.
35. Thank You Make Presentation much more funMade by – Anushka NinamaClass – IXth