Chemistry for Class Ix-X

CHEMISTRY 1. States of Matter: Solid, liquid and gaseous states(general characteristics), Change of states, effect of change of temperature and pressure on states of matter, evaporation, mixture, solution, its type and its concentration(percent strength by volume and by mass), separation of components from a mixture using various physical methods, physical and chemical changes, compounds 1. NCERT class IX text book (chapter 1 and 2) 2. Foundation Science(Chemistry) :Class IX A. K. Singh ( Bharati Bhawan) (Chapter 1 and 2) 3. A New Approach to ICSE Chemistry(Part-I) Goyal Brothers Prakashan (Chapter 1 and 3) 2. Atoms and Molecules/ Mole concept Dalton’s atomic theory, atoms, molecules, ions, atomic mass, molecular mass, atomic scale units(CU), symbol, valency of ions, formula of ions and compounds, Writing ionic equations, solubilty rules, balancing simple equations by hit and trial method, Mole concept, percentage composition of elements in compounds, empirical and molecular formula determination Reference: 1. NCERT class IX text book(chapter 3) 2. Foundation Science(Chemistry) :Class IX A. K. Singh ( Bharati Bhawan)(Chapter 3) 3. A New Approach to ICSE Chemistry(Part-I) Goyal Brothers Prakashan (Chapter 4) 4. UTSE study materials given below 3. Atomic Structure : Fundamental particles of atom(electron, proton, neutron), Discovery of Nucleus by Gold foil experiment, Rutherford’s model of atom and its demerits, Bohr’s model of atom atomic number, mass number, isotopes, isobars, Distribution of electrons in shells, Valency Reference : 1. NCERT class IX text book(Chapter 4) 2. . Foundation Science(Chemistry) :Class IX A. K. Singh ( Bharati Bhawan) (Chapter 4) 3. A New Approach to ICSE Chemistry(Part-I) Goyal Brothers Prakashan (Chapter 7) 4. UTSE study materials given below 4. Periodic Classification Periodic classification of elements: Salient Features of modern periodic(Long form), Periodic law, acquainting with alkali metals, alkaline earth metals, boron, carbon, nitrogen, oxygen, halogen, noble gas family members, Variation of periodic properties such as atomic size, ionisation energy, electron affinity, electronegativity, metallic and nonmetallic character, valency among normal elements. Reference : 1. A New Approach to ICSE Chemistry(Part-I) Goyal Brothers Prakashan (Chapter 8) 2. UTSE study materials given below 5. Chemical Bonding: Ionic bond and properties of ionic compounds, covalent bond(nonpolar and polar types), Lewis structures of simple covalent molecules, properties of covalent compounds, Preliminary ideas of metallic bond and inermolecular forces. Reference :

Reference: 1. UTSE Study materials given below 6. Oxidation-Reduction: Oxidation-reduction in terms of loss and gain of electrons, OXIDATION NUMBER(ON) or OXIDATION STATE(OS). Reference: 1. UTSE Study materials given below 7. Chemical Reactions: Types: (a) Redox and (b) Non-redox(Metathesis) types Types of metathesis reactions: Double displacement, Neutralisation and precipitation reactions, reactions of carbonates, sulphites, sulphides and nitrites with dilute HCl/H2SO4, reaction of nometallic oxides with water, reactions of metallic oxides with water, heating of ammonium salts with a base, thermal decompostion of carbonates and bicarbonates, hydrolysis of nitrides, phosphides, carbides, sulphides; amphoterism of certain metallic and nonmetallic oxides and hydroxides. Types of some simple redox reactions: Displacement reactions(metal activity series and halogen activity series), synthesis, analysis or decomposition, combustion and some simple redox reactions. Reference: 1. UTSE Study materials given below PHYSICS: Motion : Motion in one dimension: uniform and non-uniform motion, distance, displacement, velocity, acceleration, distance-time and velocity-time graphs for uniform and uniformly accelerated motion, derivation of equations of motions by graphical method, acceleration due to gravity, free fall motion. 2. Forces : Contact and non-contact forces, friction-factors affecting friction, sliding and rolling friction, advantages and disadvantages of friction, control of friction. 3. Newtons Laws of Motion : 1st, 2nd and 3rd laws- inertia of a body, inertial mass, momentum, force and acceleration, conservation of momentum, action and reaction forces, mass and weight. Law of gravitation, 4. Heat : Concepts of heat and temperature, Temperature scales(Celcius, Fahrenheit and Kelvin), mercury theormometer, clinical thermometer, Specific heat capacities, change of states and Latent heats of fusion and vaporization, calculation of heat lost or gained by method of mixtures, Thermal expansion of solids, liquids and gases(simple idea), coefficient of linear and volume expansion, humidity and relative humidity. 5. Wave motion and Sound : General concepts of wave motion, Simple harmonic oscillation(simple idea) wiith graphical representation, types of waves and their examples, amplitude, frequency, wavelength, velocity of a wave and their inter-relationship, Nature of sound and its propagagion, range of hearing in humans, effects of medium on sound waves, Reflection of sound: echo, SONAR, pitch, loudness and quality. Reference books: 1. NCERT class IX text book 2. A New Approach to ICSE Physics(Part I) for Class IX : Goyal Brother Prakashan 3. Foundation Science: PHYSICS by Prof. H.C. Verma(IIT, Kanpur) for class IX (Bharati Bhawan) (The students are strongly requested to get a good concept of each topic for UTSE first from the physics book written by Prof. H.C. Verma(Bharati Bhawan). This is the No.1 book in physics for concept building for high school students). IMPORTANT NOTE: 1. Previous Years Questions(last three years) and their detailed solution in each topic will be uploaded by December 30, 2010. Model Question for UTSE-2011 will also be uploaded by the same time. The examinees are required to thoroughly prepare the topics from the refrence books and study materials given below. 2. Readers are requested to inform us immediately(theuraniumodisha@gmail.com OR theuranium@dataone.in) when they find any mistake in the study materials for verification and rectification.

(ELECTRONIC CONFIGURATION IN ATOMS)
Each shell is divided into a fixed number of subshells. Shells are designated by shell no.(principal quantum number(n) 1, 2, 3...... while the subshells are designated by subshell numbers(azimuthal quantum numbers(l) 0,1,2,3.......... The following table gives the shells and subshells with their quantum numbers. The number of subshells(i.e the number of l values) is equal to shell number(Principal quantum number) n. Shell Number(n):(Prncipal Quantum No.) Subshell No.(l) (Azimuthal Quantum No.) n =1 K- Shell l=0 s-subshell n=2 L- Shell l=1 p-subshell n=3 M-shell l=2 d-subshell n=4 N-Shell l=3 f-subshell K- Shell(n=1) 1- subshell – s-subshell (l=0) ( K shell has one subshell i.e s-subshell) L- Shell (n=2) 2-sublshells – s-sushell( l=0) & p-subshell(l=1) ( L shell has two subshells i.e s- and p-subshells) M- Shell(n=3) 3-subshells - s-subshell (l=0), p-subshell(l=1) & d-subshell(l=2) (M shell has three subshells i.e s, p and d-subshells) N- Shell(n=4) 4-subshells - s-subshell (l=0), p-subshell(l=1) d-subshell(l=2) f-subshell(l=3) (N shell has four subshells i.e s,p,d and f subshells) ORBITALS: Each Subshell is made of some orbitals (no. of oribitals = 2l +1) Electrons live in orbitals i.e the rooms in which electrons stay. s-subshell 1 orbital - s- orbital (s-subshell is the s-orbital itself while K shell is the s-orbital itself) p-subshell 3 orbitals - px, py and pz orbitals d- subshell - 5 orbitals - 5 d orbitals (names not given) f – subshell - 7 orbitals - 7 f orbitals (names not given) PAULI’S EXCLUSION PRINCIPLE: One orbital can at the most accommodate two electrons with opposite spin i.e if one spins clockwise then the other has to spin anticlockwise. The box diagram below shows an electron pair present in any orbital.

Each s-orbital has two electrons, each p-subshell has 3 X 2 = 6 electrons, each d-subshell has 5X2 = 10 electrons while each f-subshell has 7X2 = 14 electrons. MAXIMUM NUMBER OF ELECTRONS IN EACH SHELL 1(K) SHELL: 2, 2(L) SHELL: 2 + 6 =8, 3(M) SHELL: 2 + 6 + 10 = 18 4(N) SHELL: 2+ 6 + 10 + 14 = 32 Maximum number of electrons in shell = 2n2 (where n = shell number or principal quantum number) DEGENERATE ORBITALS: Orbitals having same energy are called degenerate orbitals. 3- p orbitals are degenerate, 5-d orbitals are degenerate, 7-f orbitals are degenerate HUND’s RULE: All the degenerate orbitals are filled with one electron each with parallel spin and then pairing of electrons occurs Example : Suppose we have to fill three electrons in p-subshell which contains three orbitals. We have to fill each orbital with one electron with same spin(either all clockwise or all anticlockwise). If there are 4 electrons, then the 4th electron will be paired with the first one and so on.

(i) p3 :

(ii)

(iii) (correct)

(wrong)

(wrong)

Similary you triy for filling six electrons in the d-subshell containing 5 orbitals. First each of the five orbitals will be singly occupied and then the sixth electron will pair the 1st electron. AUFBAU PRINCIPLE(I): (aufbau – building up) (n+l) Rule: The subshell having greater (n+l) value has a greater energy. If (n+l) value of two subshells are same, then the one having higher n value has greater energy. Example: Between 4s and 3d subshells which one has higher and which has lower energy. (n+l) for 4s subshell = 4 + 0 = 4, (n+l) for 3d subshell = 3 + 2 = 5; So 4s < 3d Using the (n+l) rule for all the subshells belonging to different shells from 1st to 7th shell, tthe increasing order of energy of subshells is given below. Let us remind you that the orbitals belonging to a particular subshell have same energy i.e they are degenerate orbitals. ORDER OF ENERGY AMONG SUBSHELLS 1s