[150][151], Bohr received numerous honours and accolades. The unpaired electrons in Al and Si are present in 3p orbital. [156][157] On 7 October 2012, in celebration of Niels Bohr's 127th birthday, a Google Doodle depicting the Bohr model of the hydrogen atom appeared on Google's home page. Q9. 2 m2 r2) = K Z e2 / r2, It is the expression for Bohrs radius, which is about 0.5 A, for first orbit of hydrogen atom, n = 1, Z = 1, then we have r = 0.529 A, Ques. Numerous scholars have argued that the philosophy of Immanuel Kant had a strong influence on Bohr. Bohr was also a philosopher and a promoter of scientific research.. Bohr developed the Bohr model of The result will be based on the idea that electromagnetic radiation is made of a series of particles called photons. Torque is also called rotational force or turning effect. Ans: Energy of one photon (E) = $32.27\times {{10}^{-20}}J$, Therefore, $32.27\times {{10}^{-20}}J$ of energy is present in 1 quantum number of quanta in 2J of energy = $\frac{2J}{32.27\times {{10}^{-20}}J}=6.19\times {{10}^{18}}$. [120][121] Chadwick arranged for Bohr to visit the United States as a Tube Alloys consultant, with Aage as his assistant. He was also involved with the founding of the Research Establishment Ris of the Danish Atomic Energy Commission, and served as its first chairman from February 1956. Taking the example of a gun, before firing, both the guns remain in position of rest. Bohr writes: It is decisive to recognize that, however far the phenomena transcend the scope of classical physical explanation, the account of all evidence must be expressed in classical terms. Previously the Rydberg formula was known only experimentally, but theoretically, it was not proved, the Bohr model introduced the theoretical concept successfully. Hence, the number of protons in the element i.e., x is 35. We can say that if a student follow our CBSE class 11 chemistry Notes, then they need not to take much panic for other books. 8. [94] Therefore, for Bohr, we need to use classical concepts to describe experiments that deal with the quantum world. Years later, his brother Harald similarly left the church before getting married. For the Balmer series, a transition from ${{n}_{i}}$ = 2 to ${{n}_{f}}$= 3 is allowed. Energy Levels are the discrete energy values absorbed by a quantum mechanical system or particle that is bound or spatially restricted. Hence proved that angular momentum is a vector quantity. An Electron Is in One of the 3D Orbitals. Sketch up a diagram of the Geiger-Marsden experiment. Calculate the Wavelength for the emission transition if it starts from the orbit having radius 1.3225 nm and ends at 211.6 pm. The given set of quantum numbers is not possible because the value of the principal quantum number (n) cannot be zero. . Heisenberg explained that he had visited Copenhagen to communicate to Bohr the views of several German scientists, that production of a nuclear weapon was possible with great efforts, and this raised enormous responsibilities on the world's scientists on both sides. [160], "Bohr" redirects here. (ii). Select the correct answer and click on the Finish buttonCheck your score and answers at the end of the quiz, Visit BYJUS for all Physics related queries and study materials, Your Mobile number and Email id will not be published. b) Calculate the threshold frequency of the radiation. If the radiation source has a duration of 2 ns and the number of photons emitted during the pulse source is $2.5\times {{10}^{15}}$ , calculate the energy of the source. Similar to Electron Diffraction, Neutron Diffraction Microscope is Also Used for the Determination of the Structure of Molecules. You may think of Qualitatives analysis towards the end, as it needs very less time. Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of a multi-electron atom. The process of how the electron is distributed in the orbitals is called the electronic configuration and that is the main topic of this chapter. This implies that the total momentum of the gun (when firing is not done) is zero. (Elements had been predicted and discovered since 1871 by chemical properties[57]) and Bohr was immediately challenged by the French chemist Georges Urbain, who claimed to have discovered a rare-earth element 72, which he called "celtium". 25. Following are some important applications of this law -. Also format of Class 11 chemistry Notes is too attractive which is very important to create interest of the students in reading. The Bohr Model of the hydrogen atom should be taken into account when calculating the rotational energy levelformula. These concepts are important for them to understand, as these will build a strong foundation of Chemistry. To complete his experiments, he had to make his own glassware, creating test tubes with the required elliptical cross-sections. Toppers CBSE also contains NCERT solutions, Notes, Sample papers, Quizzes and much more. (With a Bohr radius of 0.53, this is the case. "[145][146], Meanwhile, Scandinavian countries formed the Nordic Institute for Theoretical Physics in 1957, with Bohr as its chairman. Atomic Spectra and the Bohr The relationship between the angular velocity, A convex lens of glass is immersed in water compared to its power in air, its power in water will, decrease for red light increase for violet light, A circular disc is rotating about its own axis. The photoelectric effect is a phenomenon in physics. For l = 4, the minimum value of n is 5. Substituting the value of mv from expression (ii) in expression (i): $\frac{hr}{\lambda }=n\frac{h}{2\pi }$ ----------------- (iii). Also, the total momentum in this case also remains conserved. Thus, the transition is from the ${{5}^{th}}$ orbit to the ${{2}^{nd}}$ orbit. What type of questions is present in NCERT Solutions for Class 11 Chemistry Chapter 2 Structure of Atom? Among the given orbitals only 2s and 2p are possible. WebSecure good marks by referring to NEET Class 11 Structure of Atom revision notes prepared by Vedantu experts. Also, we will discuss the concepts of subshells, shells, de Broglie's relationship, dual nature of light and matter, Heisenberg uncertainty principle, shapes of s, the concept of orbitals, p and d orbitals, quantum numbers, etc. Ans: The general convention of representing an element along with its atomic mass (A) and atomic number (Z) is $_{Z}^{A}X$. Online quizzes are also accessible to registered users only. This chapter will also introduce the students to advanced theories like Rutherford's model, Thomson's model and Bohr's model, their uses and their limitations. Among p-orbitals, 4p orbitals are farthest from the nucleus of bromine atoms with (+35) charge. (a) Find the Total Number of Protons in 34mg of $N{{H}_{3}}$ at STP. \[\Rightarrow 1.6022\times {{10}^{-19}}C\] charge is carried by 1 electron. There are enough electrons in a circular orbit around the nucleus. With Vedantu such important matters can be understood simply. Ans: Chemistry is a scoring subject where if you understand the concept and the type of questions you can come across during the exam, you can easily answer. Substituting the values in the expression of $\lambda $: \[\lambda =\frac{6.626\times {{10}^{-34}}Js}{(9.10939\times {{10}^{-31}}kg)(2.05\times {{10}^{7}}m{{s}^{-1}})}=3.548\times {{10}^{-11}}m\], Hence, the wavelength of an electron moving with a velocity of $2.05\times {{10}^{7}}m{{s}^{-1}}$ is $3.548\times {{10}^{-11}}m$. Vedantu gives good information on such important topics. According to this model, In an atom, the electrons revolve around the nucleus in definite energy levels called orbits/shells. This may be observed in the electron energy level formula, which is as shown below. Following Results are Observed When Sodium Metal is Irradiated With Different Wavelengths. 57. \[\lambda =\frac{(6.626\times {{10}^{-34}})(3\times {{10}^{8}})}{5.45\times {{10}^{-19}}}=3.647\times {{10}^{-7}}m\], 20. The general convention of representing an element along with its atomic mass (A) and atomic number (Z) is $_{Z}^{A}X$. [13], In 1910, Bohr met Margrethe Nrlund, the sister of the mathematician Niels Erik Nrlund. Since for Bohr, the -function is not a literal pictorial representation of reality, there can be no real collapse of the wavefunction. Bohr was also a philosopher and a promoter of scientific research. 4. When the balloon stays at rest, the momentum of that balloon is zero. They went through samples from Copenhagen's Museum of Mineralogy looking for a zirconium-like element and soon found it. Assuming the threshold wavelength to be ${{\lambda }_{0}}nm$ , the kinetic energy of the radiation is given as: the question is not done due to the incorrect values of velocity given in the question. [94] The model proposes that the maximum number of electrons that can be accommodated in any particular orbit is 2n2 where n is the number of orbits. The weightage of this topic is also high. We can also find the nature of the wave of an electron, which explains the energy states of the electron along with the quantized electron orbits. [32], Planetary models of atoms were not new, but Bohr's treatment was. Chapter 1: Some Basic Concepts of Chemistry Class 11 Notes, Chapter 2: Structure of Atom Class 11 Notes, Chapter 3: Classification of Elements and Periodicity in Properties Class 11 Notes, Chapter 4: Chemical Bonding and Molecular Structure Class 11 Notes, Chapter 5: States of Matter & Solid State Class 11 Notes, Chapter 8: Redox Reactions Class 11 Notes, Chapter 10: The s Block Elements Class 11 Notes, Chapter 11: The p Block Elements Class 11 Notes, Chapter 12: Organic Chemistry Some Basic Principles and Techniques Class 11 Notes, Chapter 14: Environmental Chemistry Class 11 Notes, Chapter 1: Some Basic Concepts of Chemistry, Chapter 3 Classification of Elements and Periodicity. 55. Historical Studies in the Physical Sciences, vol. For a given value of n, l can have values from zero to (n 1). Hence, for the transition to be observed at 1285 nm, n = 5. Also, explain the type of momentum seen in the case of electrons and atoms. Bohr was dissatisfied with Heisenberg's argument, since it required only that a measurement disturb properties that already existed, rather than the more radical idea that the electron's properties could not be discussed at all apart from the context they were measured in. It is the product of mass and velocity of a particle traveling in a definite medium. (b) How would the radius and ground state energy of a muonic atom be modified if the electron in the atom was replaced by a particle (muon) with the same charge but a mass around 200 times that of the electron? CBSE Class 11 Chemistry handwritten Notes are alsovery helpful for the competition classes also. The longest wavelength doublet absorption transition is observed at 589 and 589.6 nm. Question 2: The electron in Bohrs Hydrogen atom, revolves around the nucleus with a speed of 2.18 106 m/s in orbit of radius 5.3 10-11 m. Find the magnetic field which is produced by electrons on protons in the nucleus. Substituting the values in the expression of$\Delta p$, $\Delta p=\frac{1}{0.002nm}\frac{6.626\times {{10}^{-34}}Js}{4\times 3.14}$, $\Rightarrow \Delta p=2.637\times {{10}^{-23}}kgm{{s}^{-1}}$, Actual momentum = $\frac{h}{4\pi m\times 0.05nm}$= $\frac{6.626\times {{10}^{-34}}Js}{4\times 3.14\times 5.0\times {{10}^{-11}}m}=1.055\times {{10}^{-24}}kgm{{s}^{-1}}$. Hence, taking ${{n}_{f}}$ = 3, we get: \[\overset{-}{\mathop{\upsilon }}\,=\left( \frac{1}{{{(2)}^{2}}}-\frac{1}{{{(3)}^{2}}} \right)(1.097\times {{10}^{7}}{{m}^{-1}})\], \[\overset{-}{\mathop{\upsilon }}\,=\left( \frac{1}{4}-\frac{1}{9} \right)(1.097\times {{10}^{7}}{{m}^{-1}})\], \[\overset{-}{\mathop{\upsilon }}\,=1.5236\times {{10}^{6}}{{m}^{-1}}\], 18. Ans: Let the number of electrons in the ion carrying a negative charge be x. You can also refer to Vedantu; NCERT Solutions for Class 11 Chemistry Chapter 2 to find out the answers related to the discovery of atoms. Robert Oppenheimer credited Bohr with acting "as a scientific father figure to the younger men", most notably Richard Feynman. Einstein and Bohr had good-natured arguments over such issues throughout their lives. CBSE Class 11 Chemistry handwritten Notes are Best ever notes prepared by our awesome team members. Ans: Energy (E) of a photon having wavelength ($\lambda $) is given by the expression, $\lambda $ = wavelength of yellow light = $0.50{{A}^{o}}$ = $0.5\times {{10}^{-10}}m$, \[E=\frac{(6.626\times {{10}^{-34}})(3\times {{10}^{8}})}{0.5\times {{10}^{-10}}}J\], 7. Q.3. [94], Faye notes that Bohr's interpretation makes no reference to a "collapse of the wave function during measurements" (and indeed, he never mentioned this idea). NCERT Solutions Class 11 Biology Chapter 2 Biological Classification - FREE Pdf Here! He later submitted an improved version of the paper to the Royal Society in London for publication in the Philosophical Transactions of the Royal Society. This force acts as the rotational equivalent of linear force in a system having angular rotation. The ionization energy for the H atom in the ground state is $2.18\times {{10}^{-18}}Jato{{m}^{-1}}$ . Ans: Among the given orbitals only 2s and 2p are possible. 33 As the orbital radius increases so does the energy 1<2<3<4<5.. 40. Also format of Class 11 chemistry Notes is too attractive which is very important to create interest of the students in reading. The emitted electrons are called photoelectrons. David Favrholdt argued that Kierkegaard had minimal influence over Bohr's work, taking Bohr's statement about disagreeing with Kierkegaard at face value,[91] while Jan Faye argued that one can disagree with the content of a theory while accepting its general premises and structure. Quantum mechanics emerged in the mid-1920s. Assign the symbol to this ion. b) The given set of quantum numbers is possible. The following formula is used to compute the ionisation energy: The ionisation energy of a particular particle will increase by 200 times, and the mass of that particle will increase by 200 times. WebPlanetary Model of the Atom. 47. Harald had received his doctorate the previous year. Hence, the electrons in the 4p orbital will experience the lowest effective nuclear charge. Informal statistics from the server log indicate about 15 hits per user on average, so 50 million hits translates to over 3 million users per year. The students have to practice Class 12 Physics Term 2 Important Questions given on this page to get good marks in the exam. (iii). Q4: How to prepare for Chemistry with Vedantu? Students will feel that the solutions are in a simple language and can understand the difficult topics easily. K.E of electron m v2 = K Z e2 / 2r (i), P.E of electron in the orbit, E = KE + PE, Putting the value of r = n2 h2 / 4 . You can also download the Structure of Atom Class 11 questions and answers PDF, and go through them. As a result, the primary quantum number in this excited state has a value of 2. b) Electron ground state energy = -13.6 eV, Total energy of the atom in this excited state is, A boy of mass 50kg is standing at one end of a, boat of length 9m and mass 400kg. Vedantu provides the best study material for tough topics. When the impact parameter increases, the particle is nearly undeviated. Bohr brought the news to the United States where he opened the Fifth Washington Conference on Theoretical Physics with Fermi on 26 January 1939. Deduce the Electronic Configuration of the Given Element. Ans: Power of laser = Energy with which it emits photons, \[E=\frac{(5.6\times {{10}^{24}})(6.626\times {{10}^{-34}}Js)(3\times {{10}^{8}}m{{s}^{-1}})}{(337.1\times {{10}^{-9}}m)}=3.33\times {{10}^{6}}J\], Hence, the power of laser is $3.33\times {{10}^{6}}J$. Total number of electrons in an atom for a value of n = $2{{n}^{2}}$, Total number of electrons = $2{{(4)}^{2}}=32$, The given element has a fully filled orbital as $1{{s}^{2}}2{{s}^{2}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{10}}$, $\therefore $ Number of electrons (having n = 4 and ${{m}_{s}}=-\frac{1}{2}$ ) = 16. [137] In 1957 he received the first ever Atoms for Peace Award. These electrons are shielded by electrons present in the 2p and 3p orbitals along with the s-orbitals. Hence, they will not cause enough deflection of $\alpha $-particles (positively charged). [49], Bohr did not enjoy teaching medical students. This section explains the definitions of the photoelectric effect and the experiments through which it was discovered. Students can order printed copy of our CBSE Class 11 Chemistry Notes. [107], In September 1943, word reached Bohr and his brother Harald that the Nazis considered their family to be Jewish, since their mother was Jewish, and that they were therefore in danger of being arrested. This portion takes on a new structure of atom referred to as the Quantum Mechanical Model. The result will be based on the idea that electromagnetic radiation is made of a series of particles called photons. [102], In 1957, Heisenberg wrote to Robert Jungk, who was then working on the book Brighter than a Thousand Suns: A Personal History of the Atomic Scientists. Study of the photoelectric effect will lead to an understanding of the quantum nature of light and electrons and influence the formation of the concept of wave-particle duality. 5. Roosevelt suggested that Bohr return to the United Kingdom to try to win British approval. [82] In the meantime, Bohr and Wheeler developed a theoretical treatment which they published in a September 1939 paper on "The Mechanism of Nuclear Fission". To avoid a brain drain to the United States, twelve European countries banded together to create CERN, a research organisation along the lines of the national laboratories in the United States, designed to undertake Big Science projects beyond the resources of any one of them alone. Number of electrons in $M{{g}^{+2}}$ = 10, Number of electrons in $C{{a}^{+2}}$ = 18. Now known as the Niels Bohr Institute, it opened on 3 March 1921, with Bohr as its director. Ans: Number of electrons present in 1 molecule of methane (\[C{{H}_{4}}\])= \[\{1(6)+4(1)\}=10\], Number of electrons present in 1 mole i.e., \[6.023\times {{10}^{23}}\] molecules of methane = \[6.023\times {{10}^{23}}\times 10=6.023\times {{10}^{24}}\], (ii). What are the important topics of Structure of Atoms? Wavelength associated with first transition, ${{\lambda }_{1}}=589nm=589\times {{10}^{-9}}m$, Wavelength associated with second transition, ${{\lambda }_{2}}=589.6nm=589.6\times {{10}^{-9}}m$, Frequency of first wavelength is, ${{v}_{1}}=\frac{c}{{{\lambda }_{1}}}=\frac{3\times {{10}^{8}}m{{s}^{-1}}}{589\times {{10}^{-9}}m}=5.093\times {{10}^{14}}{{s}^{-1}}$, And, frequency of second wavelength is, ${{v}_{2}}=\frac{c}{{{\lambda }_{2}}}=\frac{3\times {{10}^{8}}m{{s}^{-1}}}{589.6\times {{10}^{-9}}m}=5.088\times {{10}^{14}}{{s}^{-1}}$. By using the Bohr formula energy levels, we get, hv = E = (1 / n2 low 1 / n2 high) x 13.6eV, The equation for the energy levelformula of hydrogen atoms is, where Eo is 13.6 eV and n is any natural number from 1, 2and so on, Ques. 30. I even think it is one of the most delightful things I have ever read." \[R{{(1)}^{2}}\left( \frac{1}{{{n}_{1}}^{2}}-\frac{1}{{{n}_{2}}^{2}} \right)=\frac{3R}{4}\], \[\left( \frac{1}{{{n}_{1}}^{2}}-\frac{1}{{{n}_{2}}^{2}} \right)=\frac{3}{4}\] -------- (1), By hit and trial method, the equality given by equation (1) is true only when ${{n}_{1}}=1$ and ${{n}_{2}}=2$. [117][118][119] Bohr's son Aage followed his father to Britain on another flight a week later, and became his personal assistant. Ans: Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of a multi-electron atom. 56. If the Wavelength Used Here is 800 PM, Calculate the Characteristic Velocity Associated With the Neutron. [124] In May 1944 the Danish resistance newspaper De frie Danske reported that they had learned that 'the famous son of Denmark Professor Niels Bohr' in October the previous year had fled his country via Sweden to London and from there travelled to Moscow from where he could be assumed to support the war effort. If the velocity of the electron in Bohrs first orbit is $2.19\times {{10}^{6}}m{{s}^{-1}}$ calculate the de Broglie wavelength associated with it. In a paper presented at the Volta Conference at Como in September 1927, Bohr emphasized that Heisenberg's uncertainty relations could be derived from classical considerations about the resolving power of optical instruments. Indicate the number of unpaired electrons, The electronic configuration of P is: $1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{3}}$. Find the velocity of electrons in the second orbit. Energy (E) of a photon is given by the expression. (iii).Which Atoms are Indicated by the Following Configurations? The transition for ${{n}_{2}}=2$to ${{n}_{1}}=1$ in hydrogen spectrum would have the same wavelength as Balmer transition n = 4 to n = 2 of $H{{e}^{+}}$spectrum. Bohr's friend, Supreme Court Justice Felix Frankfurter, informed President Roosevelt about Bohr's opinions, and a meeting between them took place on 26 August 1944. The next month, Bohr travelled to Leiden to attend celebrations of the 50th anniversary of Hendrick Lorentz receiving his doctorate. We have covered all topics of class 11 syllabus. What are the possible values of l and ${{m}_{l}}$ ? The angular momentum of an electron can be found as per the relation given by Bohr. [72] He conceived the philosophical principle of complementarity: that items could have apparently mutually exclusive properties, such as being a wave or a stream of particles, depending on the experimental framework. [27] Bohr received an invitation from Rutherford to conduct post-doctoral work at Victoria University of Manchester,[28] where Bohr met George de Hevesy and Charles Galton Darwin (whom Bohr referred to as "the grandson of the real Darwin"). [93] Regarding his ontological interpretation of the quantum world, Bohr has been seen as an anti-realist, an instrumentalist, a phenomenological realist or some other kind of realist. A thin foil of lighter atoms will not give the same results as given with the foil of heavier atoms. 15. The electronic configuration of the element is $[Ar]4{{s}^{2}}3{{d}^{1}}$=$1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{1}}$ . Concept and Topics Covered in Our Chemistry Notes, Matter, Physical Classification of Matter (Comparison), Chemical Classification of Matter, Pure Substance, Mixture, Elements, Classification of Elements, Compounds, Characteristics of a Chemical Compound, Classification of Compounds, Mixtures, Mixtures Are of Two Types, Properties of Matter and Their Measurement, Physical Properties, Chemical Properties, Measurement of a Physical Quantity, Mass, Weight, Volume, Density, Temperature, Dimensions Formulae of Some Physical Quantities, Some Important Conversions, Prefix Used In Si System, Conversion Related to Mass, Conversion Related to Length, Conversion Related to Pressure, Conversion Related to Volume, Some Useful Conversions, Rules For Determining The Number of Significant Figures, Exponential Numbers, Number of Significant Figures In Exponential Numbers, Rounding off a Number, Laws of Chemical Combination, Law of Conservation of Mass, Law of Multiple Proportions, Law of Reciprocal Proportions (Equivalent Proportions), Gay-Lussacs Law of Gaseous Volumes, Daltons Atomic Theory, Postulates of The Daltons Atomic Theory, Daltons Atomic Theory and Laws of Chemical Combination, Daltons Theory and The Law of Conservation of Mass, Daltons Theory and The Law of Constant Composition,Avogadros Law, Atoms, Molecules, Atomic and Molecular Masses, Atom, Molecule, Relative Atomic Mass , Atomic Mass (a), Relative Molecular Mass, Molecular Mass, Formula Mass, Molar Mass, Gram-Atomic Mass, Gram-Molecular Mass, Calculation of Molecular Mass From Atomic Masses, The Mole Concept, Mole Concept For Ionic Substances, Molar Mass of Ionic Substances, Molar Volume, Calculation of Moles In Certain Volume of a Gas, Calculation of Moles In Certain Mass of a Substance , Chemical Formulae (Empirical and Molecular Formulae) , Molecular Formula, Empirical Formula, Relationship Between The Empirical and Molecular Formulae, Steps For Writing The Empirical Formula, Steps For Writing The Molecular Formula, Chemical Equation,Essentials of a Chemical Equation, Balancing of Chemical Equations, By Hit and Trial Method, By Partial Equation Method, Stoichiometry and Stoichiometric Calculations, Limiting Reagent, Introduction, Subatomic Particles, Discovery of Electron (Cathode Rays): Discharge Tube Exp., Working of Experiment, Properties of Cathode Rays Cathode, Determination of Charge on an Electron, Characteristics of an Electron, Mass of an Electron, Charge on an Electron, Electron Is an Essential Constituent of Matter, Anode Rays (Or Canal Rays Protons), Origin of The Anode (Or Positive) Rays, Properties of Anode Rays, Discovery of The Proton, Characteristics of a Proton, Mass, Charge, Discovery of Neutron, Characteristics of Neutrons, Discovery of Radioactivity, Rutherford Observations, Thomson Model of The Atom, Rutherfords Scattering Experiment, Postulates of Rutherfords Model , Important Terms Related to Atom, Mass Number (a), Atomic Number (Z), Isotopes, Characteristics of Isotopes Isobars, Isotones, Nature of Light and Electromagnetic Radiations, Newtons Corpuscles Theory, Electromagnetic Theory, General Characteristics of Electromagnetic Radiation, Wavelength (), Frequency (), Wavenumber ( ), Composition of White Light, Particle Nature of Electromagnetic Radiation, Black-Body Radiation, Plancks Quantum Theory, Photoelectric Effect, Energy of Electromagnetic Radiation, Atomic Spectra, Atomic Emission Spectra, Atomic Absorption Spectra, Usefulness of The Atomic Spectra, Atomic Spectrum of Hydrogen, Various Series In Hydrogen Spectrum, Bohrs Atomic Model, Limitations of Bohrs Theory, Dual Nature of Particles, The De Broglie Equation, Heisenberg Uncertainty Principle, Uncertainty Principle and Electron, Schrodinger Wave Equation, Quantum Mechanical Model of Atom, Quantum Numbers, Principle Quantum Number, Secondary Quantum Numbers Or Azimuthal Quantum Number, Magnetic Quantum Number, Spin Quantum Number, Shapes of Orbitals, S Orbitals, P Orbitals, D Orbitals, Rules For Filling Electrons In The Orbitals of an Atom , Aufbau Principle, Paulis Exclusion Principle, Hunds Rule of Maximum Multiplicity, Some Examples of Electronic Configuration, Extra-Stability of Half-Filled & Completely-Filled Orbitals, Stability of Symmetry, Exchange Energy, Introduction, Dobereiners Triads , Limitation of Dobereiners Triads, Newlands Law of Octave , Periodic Table Given By The Newlands, Limitations of Newlands Law of Octaves, Lothar Meyers Atomic Volume Curve, Mendeleevs Periodic Table, Mendeleev Periodic Table, Merits of Mendeleevs Classification of Elements, Limitations of Mendeleevs Classification of Elements, Modern Periodic Law (Long Form Periodic), General Characteristics of The Long Form Periodic Table, Merits of Modern Periodic Classification, Defects In Long Form Periodic Table, Naming of Elements Having Atomic Numbers Above 103, Grouping of Elements Into Blocks, The S -Block Elements, Characteristics of S-Block Elements, The P-Block Elements, Characteristics of The P-Block Elements, The D-Block Elements, Characteristics of The D-Block Elements, The D-Block Series, The F-Block Elements, Characteristics of The F-Block Elements, Periodic Trends In Atomic Properties of Elements, Atomic Radius, Covalent Radius, The Van Der Waals Radius, Metallic Radius, Periodic Variation of Atomic Radii, Variation of Atomic Radii In a Group, Ionic Radius, Why Are Cations Smaller Than Their Parent Atoms?, Why Are Anions Bigger Than Their Parent Atoms, Factors Affecting The Ionisation Enthalpy, Periodic Variation of Ionisation Enthalpy, Variation of Ionisation Enthalpy In a Group, Variation of Ionisation Enthalpy In a Period, Exceptions to The General Trends of Ionisation Enthalpies, Electron Gain Enthalpy (Electron Affinity), Successive Electron Gain Enthalpies, Factors Affecting Electron Gain Enthalpy, Variation of Electron Gain Enthalpy In a Group, Variation of Electron Gain Enthalpy In a Period, Electronegativity, Factors Affecting Electronegativity, Variation of Electronegativity In a Group, Variation of Electronegativity In a Period, Valence , Variation of Valence In The Periodic Table, In a Period, Variation of Melting and Boiling Points In a Group, Electropositive Or Metallic Character, Variation of Electropositive Character In a Period, Variation of Electropositive Character In a Group, Electronegative Or Non-Metallic Character, Variation of Electronegative Character In a Group, Variation of Electronegative Character In a Period, Reactivity of Metals(In a Period, In a Group), Introduction, Cause of Chemical Combination, Lewis Symbols, Significance of Lewis Symbols, Octet Rule & Modes of Chemical Combination, Ionic Bond, Factors Influencing The Formation of an Ionic Bond, Born-Haber Cycle, Bond Parameters, Covalent Bond, Covalency, Single Bond, Double Bonds, Triple Bonds, Condition For Covalent Bond, Co- Ordinate Bond, Comparison of Ionic and Covalent Compounds, Exceptions to Octet Rule, Formal Charge, Geometry & Shape of Molecules and Vsepr Theory , The Main Postulate of Vsepr Theory, Shape of Molecules Containing Lone Pairs(L) and Bond Pair(B), Molecules Containing Three Electron Pairs , Molecules Containing Four Electron Pair, Molecules With Five Electron Pairs, Table For Different Shapes and Structure, Partial Ionic Character of Covalent Bond, Important of Dipole Moment, Calculation of % Ionic Character, Criteria For Zero Dipole Moments, Some Comparisons of Molecules For Dipole Moments, Orbital Overlap Concept of Covalent Bond, Sigma Bond, Pi Bond, Concept of Hybridisation, Characteristics of Hybrid Orbitals , Types of Hybridisation, The Sp3 Hybridisation (Or Tetrahedral Hybridisation), The Sp2 Hybridisation Or Trigonal Hybridisation, The Sp Hybridisation (Or Linear Hybridisation), The Sp3d Hybridisation (Trigonal Bipyramidal Hybridisation), The Sp3d2 Hybridisation: Octahedral Hybridisation, The D2sp3 Hybridisation: Octahedral Hybridisation, The Dsp2 Hybridisation: Square Planar Hybridisation, Molecular Orbital Theory (Mot), Difference Between Bonding and Anti-Bonding M.O., Types of Molecular Orbitals, Energy Level Diagram For Molecular Orbitals, Electronic Configuration and Molecular Behaviour (Stability of Molecule, Bond Order, Magnetic Behaviour), Molecules Behaviour Using Mo, Hydrogen Molecule (H2), Hydrogen Molecule Cation (H2+), Hydrogen Molecule Anion (H2-), Helium Molecule (He2), Nitrogen Molecule (N2), Oxygen Molecule (O2), Fluorine Molecule (F2), Hydrogen Bond, Conditions For Hydrogen Bonding, Influence of Hydrogen Bonding on The Properties, Types of Hydrogen Bonds, Intermolecular Hydrogen Bond, Intermolecular Hydrogen Bond. 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