TS Inter 1st Year Chemistry Notes Chapter 2 Classification of Elements and Periodicity in Properties

Here students can locate TS Inter 1st Year Chemistry Notes 2nd Lesson Classification of Elements and Periodicity in Properties to prepare for their exam.

TS Inter 1st Year Chemistry Notes 2nd Lesson Classification of Elements and Periodicity in Properties

→ According to Modern periodic law, the physical and chemical properties of ele-ments are periodic functions of their atomic numbers (or) electronic configurations.

→ In the Long form of the periodic table the elements are arranged in the increasing order of their atomic numbers.

→ There are seven horizontal rows (periods) and eighteen vertical columns (groups) in the long form of periodic table.

→ Based on the entering of differentiating electron, elements are classified into four blocks. They are s – block, p – block, d – block and f – block.

→ Based on the number of incompletely filled shells, elements are classified into four types. They are :

  • Inert gas elements
  • Representative elements
  • Transition elements
  • Inner transition elements.

→ Repetition of properties of elements (i.e., similar elements) after definite regular intervals is called periodicity. The cause of periodicity is due to similar outer electronic configuration.

TS Inter 1st Year Chemistry Notes Chapter 2 Classification of Elements and Periodicity in Properties

→ The distance between the nucleus and outermost electron of an atom is called atomic radius.

→ The regular decrease in the size of lanthanides from left to right, due to the ineffective shielding offered by inner f – orbital is called Lanthanide contraction.

→ The decrease in the attractive force of the nucleus on the valence electrons by the electrons of inner shells is called screen-ing effect or shielding effect.

→ The minimum amount of energy required to remove an electron present in the out-ermost orbit of a neutral isolated gaseous atom is called ionisation potential.

→ The amount of energy released when an electron is added to a neutral, isolated gaseous atom is called electron affinity.

→ The tendency of an atom to attract shared pair of electrons towards itself in a cova-lent molecule is called Electronegativity.

→ According to Mullikan scale, the E.N. value of an element is an average of its IP and E.N.

→ According to Pauling scale the difference in the E.N. values is given by
XA – XB = 0.208 √Δ.

→ The combining capacity of an atom with other atoms is called valency. It is the number of H atoms or the number of Cl atoms or double the number of ‘O’ atoms with which one atom of the element combines.

→ The tendency of losing electrons is called Electropositivity.

→ Metallic oxides are basic and non-metallic oxides are acidic.

→ The reluctance of ns2 electrons to get un-paired and take part in bonding is called inert pair effect’.

→ The first element of a group shows some similarities with the second element of the next higher group. This is called diagonal relationship’.

TS Inter 1st Year Chemistry Notes Chapter 3 Chemical Bonding and Molecular Structure

Here students can locate TS Inter 1st Year Chemistry Notes 3rd Lesson Chemical Bonding and Molecular Structure to prepare for their exam.

TS Inter 1st Year Chemistry Notes 3rd Lesson Chemical Bonding and Molecular Structure

→ The force of attraction between the constituent atoms of a molecule is called chemical bond.

→ The principle of attaining eight electrons in the outermost shell of an atom for attaining stability is called octet rule.

→ The electrostatic force of attraction bet-ween oppositely charged ions formed by the transfer of electrons is called Ionic Bond or Electrovalent Bond.

→ The amount of energy released, when one mole of ionic substance is formed from its constituent oppositely charged ions separated by infinite distance are brought nearer together, is called lattice energy.

→ Born – Haber cycle is used for the indirect determination of lattice energy. This method is based on Hess’s law.

→ The smallest part of ionic substance, which develops the entire crystal on repetition in three dimensional space is called unit cell.

TS Inter 1st Year Chemistry Notes Chapter 3 Chemical Bonding and Molecular Structure

→ Ionic substances are polar and are soluble in polar solvents like water and are insoluble in non-polar solvents like Benzene etc.

→ Covalent bond is formed due to mutual sharing of electrons. This is also called electron-pair bond.

→ Molecules which have less number of electrons on the central atom than octet are called electron deficient molecules.
Ex : BeCl2, BF3 etc.

→ The covalent bond formed by head on overlap of half-filled orbitals is called sigma bond.

→ Sigma bond is a stronger bond than a pi bond because the extent of overlapping is more in sigma bond than in a pi bond.

→ VSEPR theory explains the shapes and bond angles of molecules without reference to the theory of hybridisation.

→ Presence of lone pair distorts the structure and decreases the bond angle.

→ The average inter – nuclear distance bet-ween bonded atoms is called bond length.

→ The amount of energy required to break a mole of covalent bonds is called bond energy.

→ The process of inter-mixing of atomic or-bitals of nearly same energy of an atom and forming the same number of identical new orbitals is called hybridisation.

→ A pure covalent bond is formed by equal sharing of bonded electrons, between two identical atoms.

→ A polar covalent bond is formed by unequal sharing of bonded electrons.

→ The product of charge and inter-nuclear distance is called Dipolemoment. It is a vector quantity and is measured in debye units.

→ Bond formed due to mutual sharing of electron pair, but shared pair belonging to only one of the atoms involved in the bond is called coordinate covalent bond (or) dative bond.

→ The weak electrostatic bond between a covalently bonded H atom and a highly E.N. atom is called hydrogen bond.

→ The force of attraction that holds the metal atoms firmly together in a metallic crystal is called metallic bond.

→ The number of electrons an atom contri-butes towards covalent bond formation in a molecule is known as its covalency.

→ The number of electrons lost or gained by an atom, during the formation of ‘ionic compound’, is its ‘electrovalency’.

→ Molecular orbital theory (M.O.T) was proposed by Hund and Mulliken. The m.o’s are formed by the method called linear combination of atomic orbitals’ (LCAO method).

TS Inter 1st Year Chemistry Notes Chapter 3 Chemical Bonding and Molecular Structure

→ Order of energy levels of m.o’s
(a) In Li2, Be2, B2, C2 and N2 molecules :
σ1s < σ*1s < σ*2s < σ*2s < π2Py
= π2Pz < σ2Px < π2Py = π2Pz < σ*2Py

(b) In O2, F2 and Ne2 molecules :
σ < σ*1s < σ2s < σ*2s < σ2Px < π2Py
= π2Pz < π*2Py = π2Pz < σ*2Px

TS Inter 1st Year Chemistry Notes Chapter 4 States of Matter: Gases and Liquids

Here students can locate TS Inter 1st Year Chemistry Notes 4th Lesson States of Matter: Gases and Liquids to prepare for their exam.

TS Inter 1st Year Chemistry Notes 4th Lesson States of Matter: Gases and Liquids

→ Parameters of gases are pressure, volume, temperature and number of moles.

→ Boyle’s law: It states that “at constant temperature, the volume of a given mass of a gas is inversely proportional to its pressure”.

→ Charles’ law : It states that “at constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature”.

→ Avogadro’s law: It states that “at constant temperature and pressure, equal volumes of all gases contain equal number of molecules or moles”.

→ A gas which obeys Boyle’s law, Charles’ law and Avogadro’s law is called ideal gas.

→ Ideal gas equation is PV = nRT.

→ R is universal gas constant which denotes work done by a gas.

→ The equation of state is represented as
\(\frac{\mathrm{P}_1 \mathrm{~V}_1}{\mathrm{~T}_1}=\frac{\mathrm{P}_2 \mathrm{~V}_2}{\mathrm{~T}_2}\)

→ A real gas behaves as an ideal gas at high temperature and low pressure.

→ Diffusion is a phenomenon of intermixing of gases irrespective of gravitational force of attraction.

→ Effusion is diffusion through a small hole from a high pressure to low pressure area.

TS Inter 1st Year Chemistry Notes Chapter 4 States of Matter: Gases and Liquids

→ Graham’s law of diffusion : It states that “at constant pressure and temperature the rate of diffusion of gas is inversely proportional to the square root of its density”.

→ Dalton’s law of partial pressure: It states that “the total pressure of a gaseous mixture which do not react chemically with each other is equal to the sum of the partial pressures of the component gases”.

→ Partial pressure = Total pressure × Mole fraction.

→ The pressure exerted by water vapour over liquid water surface when both of them are in equilibrium is called water vapour pres¬sure or aqueous tension.

→ Kinetic gas equation is given by PV = \(\frac{1}{3}\)mnc2.

→ Kinetic energy of a gas is equal to \(\frac{3}{2}\) nRT.

→ The velocity possessed by maximum number of molecules is called the most probable velocity.

→ The ratio of sum of the velocities to the total number of molecules is called average velocity.

→ Square root of average for the squares of the velocities is called RMS velocity.

→ RMS velocity represents all gas molecules and is used in deriving kinetic gas equation.

→ The ratio of the three types of velocities is given as Cp : C̅ : C = 1 : 1.128 :1.224.

→ Gas constant per molecule is called
Boltzmann constant (K = \(\frac{\mathrm{R}}{\mathrm{N}}\)).

→ The method of separation of a mixture of two gases making use of the difference in their relative rates of diffusion or effusion is called atmolysis.

TS Inter 1st Year Chemistry Notes Chapter 5 Stoichiometry

Here students can locate TS Inter 1st Year Chemistry Notes 5th Lesson Stoichiometry to prepare for their exam.

TS Inter 1st Year Chemistry Notes 5th Lesson Stoichiometry

→ The standard reference for relative atomic masses is Carbon – 12.

→ \(\frac{1}{12}\)th of the mass of C -12 is called atomic 12 mass unit (amu).

→ The value of amu is 1.66 × 10-24 gm. This is known as Avogram.

→ The weight of a substance in grams, numerically equal to its molecular weight is called gram molecular weight or gram mole.

→ Number of atoms present in one gram molecular weight of element is called Avogadro’s number. Its value is 6.023 × 1023.

→ The volume occupied by one gram molecular weight of a gas at STP is called gram molar volume (GMV). Its value is 22.4 lits or 22,400 cc.

→ Mole is the SI unit for the amount of a substance.

→ Mole is that mass of a substance which contains Avogadro number of structural units.

→ The apparent charge that an atom appears to have in its combined state is called its oxidation number. It may be + ve (or) – ve (or) fractional or zero.

→ The element that never exhibits + ve oxidation number is Fluorine.

TS Inter 1st Year Chemistry Notes Chapter 5 Stoichiometry

→ The process of removal of electron is called Oxidation.

→ The process of addition of electron is called Reduction.

→ The substance which gains electrons is called Oxidant.

→ The substance which loses electrons is called Reductant.

→ A chemical reaction which involves both oxidation and reduction is called redox re-action.

→ Redox reactions can be balanced by
(a) Ion electron method
(b) Oxidation number method.

→ The actual masses of substances conveyed by a balanced equation is known as Stoichiometry.

→ One hundred times to the weight ratio of an element and the compound containing the element is called percentage composition of the element.

→ The formula that gives the simplest ratio of atoms of the constituent elements present in a compound is called empirical formula.

→ The formula that gives the exact number of atoms of the constituent elements present in a compound is called Molecular formula.

→ Molecular formula = Empirical formula × n
where, n = \(\frac{\text { Molecular formula weight }}{\text { Empirical formula weight }}\)

→ Increase in oxidation number is oxidation and decrease in oxidation number is reduction.

TS Inter 1st Year Chemistry Notes Chapter 6 Thermodynamics

Here students can locate TS Inter 1st Year Chemistry Notes 6th Lesson Thermodynamics to prepare for their exam.

TS Inter 1st Year Chemistry Notes 6th Lesson Thermodynamics

→ In the study of thermodynamics, we divide the entire universe into two segments. One small segment of it is the one on which we conduct out studies. This is called system. The rest of the universe is considered ar-bitrarily as surroundings.

→ Systems are classified as open, closed and isolated systems.

→ Properties of the system are classified as intensive (non-depending on amount of matter), extensive (depending on amount of matter) and thermodynamic properties.

→ Thermodynamic properties are internal energy (E), enthalpy (H), Gibbs energy (G), entropy (S), work (W) etc.

→ Zeroth law deals with thermal equilibrium between the bodies. First law is concerned with conservation of energy, second law deals with spontaneity of a process and the third law deals with heat changes at absolute zero.

→ Application of first law of thermodynamics to chemical changes is known as thermo chemistry.

TS Inter 1st Year Chemistry Notes Chapter 6 Thermodynamics

→ We define the heat changes quantitatively for different processes. These are forma-tion, dissociation, combustion, netrtralizatipn, sublimation, ionization and dilution processes.

→ Heat changes can be experimentally deter-mined using calorimeters.

→ ΔG = ΔH – T ΔS. ΔG is negative for spontaneous and is positive for non-spontaneous and zero for equilibrium reactions.

→ Entropy (S), a thermodynamic property is introduced to express the molecular disorder of a chemical system.

TS Inter 1st Year Chemistry Notes Chapter 7 Chemical Equilibrium and Acids-Bases

Here students can locate TS Inter 1st Year Chemistry Notes 7th Lesson Chemical Equilibrium and Acids-Bases to prepare for their exam.

TS Inter 1st Year Chemistry Notes 7th Lesson Chemical Equilibrium and Acids-Bases

→ The mixture of reactants and products in the equilibrium state is called an equilibrium mixture.

→ Reactions which proceed in one direction only are called irreversible reactions.

→ Reactions which proceed from reactants to products and also from products to reactants, simultaneously are called reversible reactions.

→ The state of a reversible reaction at which the rate of forward reaction is equal to the rate of backward reaction is called Equilibrium.

→ Chemical equilibrium is dynamic.

→ Increased concentration of reactants shifts the equilibrium position to products side and increased concentration of products shifts the equilibrium position to reactants side.

→ High temperature favours Exothermic reaction and low temperature favours Endothermic reaction.

→ A catalyst has no influence on the position of equilibrium. The catalyst is used to establish the equilibrium quickly.

TS Inter 1st Year Chemistry Notes Chapter 7 Chemical Equilibrium and Acids-Bases

→ For a general reaction aA + bB ⇌ cC + dD
Kc = \(\frac{[\mathrm{C}]^{\mathrm{c}}[\mathrm{D}]^{\mathrm{d}}}{[\mathrm{A}]^{\mathrm{a}}[\mathrm{B}]^{\mathrm{b}}}\); Kp = \(\frac{P_C^c P_D^d}{P_A^a P_B^b}\)
Kp = Kc(RT)Δn; Δn = (c + d) – (a + b)

→ For, H2 + I2 ⇌ 2HI; Kp = Kc
For, N2 + 3H2 ⇌ 2NH3; Kp < Kc (∵ Δn = -2)
For, PCl5 ⇌ PCl3 + Cl2; Kp > Kc (∵ Δn = 1)

→ Le Chatelier principle states that When a system at equilibrium was subjected to stress, the system shifts in such a way so as to undo the effect of the change.

→ According to Le Chatelier principle, High pressure and low temperature are favourable in Haber’s process and in Con-tact process.

→ Substances are classified into acids, bases and salts depending on their chemical behaviour and properties.

→ According to Bronsted theory proton donor is an acid and proton acceptor is a base.

→ An acid and a base which differ by a single proton are called conjugate acid-base pairs.

→ Leveling by water of all strong acids to the strength of H3O+ and all strong bases to the strength of OH ions is called leveling effect of water.

→ According to Lewis electron pair acceptor is an acid and electron pair donor is a base.

→ The product of hydrogen ion (H+) and hydroxyl ion (OH) in pure water or in any aqueous solution is called ionic product of water.

→ The negative value of the logarithm of the hydrogen ion concentration is called pH.
A solution which resists the change in its pH value on dilution or on addition of small amounts of acid or base is called buffer solution.

→ The number of moles of acid or base requi-red to be added to the one litre of a buffer solution to register a change of one unit in the pH is called buffer capacity (Φ).

→ The substance which exhibits one colour in acidic medium and another colour in alkaline medium is known as acid-base indicator.

TS Inter 1st Year Chemistry Notes Chapter 7 Chemical Equilibrium and Acids-Bases

→ The interaction of anion or cation or both of a salt with water to form basic or acidic or neutral solution is known as salt hydrolysis.

→ The aqueous solutions of salts of weak acid and strong base are basic. The aqueous solutions of salts of weak base and strong acid are acidic.

→ The product of the concentrations of the cation and the anion in a saturated solution of a salt at room temperature is called solubility product (Ksp)
Ksp = [Mn+][An-]

→ Relation between solubility product (Ksp) and solubility (s) is, S = \(\left[\frac{K_{S p}}{x^x y^y}\right]^{y_{x+y}}\)

→ The solubility of an electrolyte in water decreases on addition of an electrolyte which has one ion common with the electrolyte, is called common ion effect.

→ Common ion effect principle is used in the systematic qualitative analysis of cations.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Students must practice these Maths 2A Important Questions TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type to help strengthen their preparations for exams.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 1.
Form the polynomial equation of the lowest degree whose roots are 1, – 1, 3. [May ’06]
Solution:
Let α = 1; β = – 1, γ = 3
The equation having roots α, β, γ is
(x – α) (x – β) (x – γ) = 0
⇒ (x – 1) (x + 1) ( x – 3) = 0
⇒ (x2 – 1) (x – 3) = 0
⇒ x3 – 3x2 – x + 3 = 0.

Question 2.
Form the polynomial equation of the lowest degree whose roots are 2 ± √3, 1 ± 2i. [May ’02, ’01]
Solution:
Let
α = 2 + √3, β = 2 – √3, γ = 1 + 2i, δ = 1 – 2i
The equation having α, β, γ, δ is
(x – α) (x – β) (x – γ) (x – δ) = 0
⇒ (x – 2 – √3) (x – 2 + √3) ((x – 1) – 2i) ((x – 1) + 2i) = 0
⇒ ((x – 2) – √3) ((x – 2) + √3) ((x – 1) – 2i) ((x – 1) + 2i) = 0
⇒ (x2 + 4 – 4x – 3) (x2 + 1 – 2x + 4) = 0
⇒ (x2 – 4x + 1) (x2 – 2x + 5) = 0
⇒ x4 + 5x2 – 2x3 – 4x3 + 8x2 – 20x + x2 – 2x + 5 = 0
⇒ x4 – 6x3 + 14x2 – 22x + 5 = 0

Question 3.
If 1, 1, α are the roots of x3 – 6x2 + 9x – 4 = 0. then find α. [AP – Mar. ’18; TS – May 2016; May ’11]
Solution:
Given equation is x3 – 6x2 + 9x – 4 = 0
Comparing this equation with ax3 + bx2 + cx + d = 0
we get, a = 1; b = – 6; c = 9; d = – 4
Since 1, 1, α are the roots of x3 – 6x2 + 9x – 4 = 0
then sum of the roots = s1 = \(\frac{-b}{a}\)
⇒ 1 + 1 + α = \(\frac{-(-6)}{1}\) = 6
⇒ 2 + α = 6
⇒ α = 4.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 4.
If – 1, 2 and α are the roots of 2x3 + x2 – 7x – 6 = 0, then find α.
[AP-Mar. 18; Mar. ’14, ’13, ’10, ’06, May’ 12, ’10]
Solution:
Given equation is 2x3 + x2 – 7x – 6 = 0
Comparing this with ax3 + bx2 + cx + d = 0 we get,
a = 2; b = 1; c = – 7; d = – 6
Since – 1, 2, α are the roots of 2x3 + x2 – 7x – 6 = 0
The sum of the roots = s1 = \(\frac{-b}{a}\)
– 1 + 2 + α = – \(\frac{1}{2}\)
1 + α = – \(\frac{1}{2}\)
⇒ α = – 1 – \(\frac{1}{2}\)
α = – \(\frac{3}{2}\)

Question 5.
If 1, – 2 and 3 are the roots of x3 – 2x2 + ax + 6 = 0, then find ‘a’. [TS – May 2015; March ‘04]
Solution:
Given equation is x3 – 2x2 + ax + 6 = 0
Since 1, – 2, 3 are the roots of x3 – 2x2 + ax + 6
Now 1 is a root of given equation then
13 – 2(1)2 + a(1) + 6 = 0
⇒ 1 – 2 + a + 6 = 0
a + 5 = 0
a = – 5

Question 6.
If the product of the roots of 4x3 + 16x2 – 9x – a = 0, is 9, then find ‘a’. [AP – Mar. 19, 17; TS – Mar. 16; May 13, 12, 08]
Solution:
Given equation is 4x3 + 16x2 – 9x – a = 0
Comparing this equation with ax3 + bx2 + cx + d = 0
we get, a = 4, b = 16, c = – 9, d = – a
Given that, the product of the roots = 9
s3 = 9
⇒ \(\frac{-\mathrm{d}}{\mathrm{a}}\) = 9
⇒ \(\frac{-(-a)}{4}\) = 9
⇒ a = 36.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 7.
If α, β and 1 are the roots of x3 – 2x2 – 5x + 6 = 0, then find α and β. [AP – May, Mar. 2016; May 09, March 08]
Solution:
Given equation is x3 – 2x2 – 5x + 6 = 0
Comparing this equation with ax3 + bx2 + cx + d = 0
we get a = 1, b = – 2, c = – 5, d = 6
Since α, β and 1 are the roots of x3 – 2x2 – 5x + 6 = 0
then s1 = α + β + 1
= \(\frac{-b}{a}=\frac{-(-2)}{1}\) = 2
⇒ α + β = 1 …………(i)
s3 = αβ . 1 = \(\frac{-d}{a}\)
⇒ αβ = \(\frac{-6}{1}\) =
⇒ αβ = – 6
(α – β)2 = (α + β)2 – 4αβ
= 1 – 4 ( -6)
= 1 + 24 = 25
⇒ α – β = 5 ……………(2)
Solve (1) and (2);

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type 1

Question 8.
If α, β and γ are the roots of x3 + 2x2 + 3x – 4 = 0, then find α2β2. [May ’07]
Solution:
Given equation is x3 + 2x2 + 3x – 4 = 0
Since α, β and γ are the roots of x3 + 2x2 + 3x – 4 = 0 then
α + β + γ = \(\frac{-(-2)}{1}\) = 2
αβ + βγ + γα = \(\frac{3}{1}\) = 3
αβγ = \(\frac{-(-4)}{1}\) = 4
Σα2β2 = α2β2 + β2γ2 + γ2α2
= (αβ + βγ + γα)2 – 2αβγ (α + β + γ)
= 32 – 2 . 4(2)
= 9 – 16 = – 7.

Question 9.
If α, β and γ are the roots of 4x3 – 6x2 + 7x + 3 = 0, then find the value of αβ + βγ + γα. [TS – Mar. 2019]
Solution:
Given equation is 4x3 – 6x2 + 7x + 3 = 0
Comparing this equation with ax3 + bx2 + cx + d = 0
where a = 4; b = – 6; c = 7; d = 3
Since α, β, γ are the roots of 4x3 – 6x2 + 7x + 3 = 0 then
αβ + βγ + γα = S2 = \(\frac{c}{a}=\frac{7}{4}\).

Question 10.
Find the relations between the roots and the coefficients of the cubic equation 3x3 – 10x2 + 7x + 10 = 0.
Solution:
Given cubic equation is 3x3 – 10x2 + 7x + 10 = 0
Comparing this equation with
ax3 + bx2 + cx + d = 0, we get
a = 3, b = – 10, c = 7, d = 10
Let α, β, γ be the roots of given equation
s1 = \(\frac{-b}{a}\)
α + β + γ = \(\frac{-(-10)}{3}=\frac{10}{3}\)
s2 = αβ + βγ + γα
= \(\frac{c}{a}=\frac{7}{3}\)
s3 = αβγ
= \(\frac{-\mathrm{d}}{\mathrm{a}}=\frac{-10}{3}\).

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 11.
Write down the relations between the roots and the coefficients of the biquadratic equation x4 – 2x3 + 4x2 + 6x – 21 = 0.
Solution:
Given biquadratic equation is
x4 – 2x3 + 4x2 + 6x – 21 = 0 ……………… (1)
Comparing this equation with
ax4 + bx3 + cx2 + dx + e = 0,
we get a = 1, b = – 2; c = 4; d = 6; e = – 21
Let α, β, γ, δ are the roots of equation (1) then
i) s1 = α + β + γ + δ
= Σα = \(\frac{-b}{a}=\frac{-(-2)}{1}\) = 2
ii) s2 = Σαβ
= \(\frac{c}{a}=\frac{4}{1}\) = 4
iii) s3 = Σαβγ
= \(\frac{-d}{a}=\frac{-6}{1}\) = – 6
iv) s = Σαβγδ
= \(\frac{\mathrm{e}}{\mathrm{a}}=\frac{-21}{1}\) = – 21

Question 12.
If 1, 2, 3 and 4 are the roots of x4 + ax3+ bx2 + cx + d = 0, then find the values of a, b, c and d. [AP – May 2015]
Solution:
Given that the roots of the polynomial equation are 1, 2, 3 and 4.
Then(x – 1) (x – 2) (x – 3) (x – 4) = 0
(x2 – 3x + 2) (x2 – 7x + 12) = 0
x4 – 7x3 + 12x2 – 3x3 + 21x2 – 36x + 2x2 – 14x + 24 = 0
x4 – 10x3 + 35x2 – 50x + 24 = 0
Now, comparing this equation with
x4 + ax3 + bx2 + cx + d = 0
we get a = – 10; b = 35; c = – 50; d = 24.

Question 13.
If a, b, c are the roots of x3 – px2 + qx – r = 0 and r ≠ 0, then find \(\frac{1}{a^2}+\frac{1}{b^2}+\frac{1}{c^2}\) in terms of p, q, r.
Solution:
Given equation is x3 – px2 + qx – r = 0
Since a, b and c are the roots of the equation x3 – px2 + qx – r = 0 then
s1 = a + b + c
= \(\frac{-(-p)}{1}\) = p;
s2 = ab + bc + ca
= \(\frac{q}{1}\) = q;
s3 = abc
= \(\frac{-(-r)}{1}\) = r
\(\frac{1}{a^2}+\frac{1}{b^2}+\frac{1}{c^2}=\frac{b^2 c^2+a^2 c^2+a^2 b^2}{a^2 b^2 c^2}\)
= \(\frac{(a b+b c+c a)^2-2 a b c(a+b+c)}{(a b c)^2}\)
= \(\frac{q^2-2 p \cdot r}{r^2}=\frac{q^2-2 p r}{r^2}\).

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 14.
Find the sum of the squares and the sum of the cubes of the roots of the equation x3 – px2 + qx – r = o in terms of p, q, r.
Solution:
Given equation is x3 – px2 + qx – r = 0
Let α, β, γ are the roots of the equation x3 – px2 + qx – r = 0 then
s1 = α + β + γ
= \(\frac{-\mathrm{b}}{\mathrm{a}}=\frac{-(-\dot{\mathrm{p}})}{1}\) = p;
s2 = αβ + βγ + γα
= \(\frac{q}{1}\) = q;
s3 = αβγ
= \(\frac{-(-r)}{1}\) = r
i) The sum of the squares of the roots of the equation = α2 + β2 + γ2
= (α + β + γ)2 – 2(αβ + βγ + γα)
= p2 – 2q
ii) The sum of the cubes of the roots is α3 + β3 + γ3 = (α + β + γ)
2 + β2 + γ2 – αβ – βγ – γα) + 3αβγ
= p(p2 – 2q – q) + 3r
= p3 – 3pq + 3r.

Question 15.
Let α, β, γ be the roots of x3 + px2 + qx + r = 0. Then find Σα3. [March ’03]
Solution:
Given equation is x3 + px2 + qx + r = 0
Since α, β, γ are the roots of the equation x3 + px2 + qx + r = 0 then
s1 = α + β + γ
= \(\frac{-\mathrm{p}}{1}\) = – p;
s2 = αβ + βγ + γα
= \(\frac{q}{1}\) = q;
s3 = αβγ
= \(\frac{-r}{1}\) = – r
Σα3 = α3 + β3 + γ3
= (α + β + γ) (α2 + β2 + γ2 – αβ – βγ – γα) + 3αβγ
= (- p) ((p2 – 2q) – (q)) + 3 (- r)
= – p (p2 – 3q) – 3r
= – p3 + 3pq – 3r

Question 16.
Find s1, s2, s3 and s4 for the equation x4 – 16x3 + 86x2 – 176x + 105 = 0.
Solution:
Given equation is x4 – 16x3 + 86x2 – 176x + 105 = 0
Comparing this equation with ax4 + bx3 + cx2 + dx + e = 0
we get a = 1; b = – 16; c = 86; d = – 176; e = 105
Now, s1 = \(=\frac{-b}{a}=\frac{-(-16)}{1}\) = 16;
s2 = \(\frac{c}{\mathrm{a}}=\frac{86}{1}\) = 86;
s3 = \(\frac{-\mathrm{d}}{\mathrm{a}}=\frac{-(-176)}{1}\) = 176;
s4 = \(\frac{\mathrm{e}}{\mathrm{a}}=\frac{105}{1}\) = 105

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 17.
Find the algebraic equation whose roots are 2 times the roots of x5 – 2x4 + 3x3 – 2x2 + 4x + 3 = 0. [Board Paper]
Solution:
Let f(x) = x5 – 2x4 + 3x3 – 2x2 + 4x + 3 = 0
∴ Required equation is f(\(\frac{x}{2}\)) = 0
⇒ \(\frac{x^5}{32}-\frac{2 x^4}{16}+\frac{3 x^3}{8}-\frac{2 x^2}{4}+\frac{4 x}{2}+3\) = 0
⇒ x5 – 2x4 + 3x3 – 2x2 + 4x + 3 = 0

Question 18.
Find the transformed equation whose roots are the negatives of the roots of x7 + 3x5 + x3 – x2 + 7x + 2 = 0.
Solution:
Let f(x) = x7 + 3x5 + x3 – x2 + 7x + 2 = 0
Required equation is f(- x) = 0
(- x)7 + 3(- x)5 + (- x)3 – (- x)2 + 7(- x) + 2 = 0
x7 + 3x5 + x3 + x2 + 7x – 2 = 0

Question 19.
Find the polynomial equation whose roots are the reciprocals of the roots of x4 – 3x3 + 7x2 + 5x – 2 = 0. [March ’11] [TS – Mar. 2015]
Solution:
Let f(x) = x4 – 3x3 + 7x2 + 5x – 2 = 0
The required equation is f(\(\frac{1}{x}\)) = 0
⇒ \(\frac{1}{x^4}-\frac{3}{x^3}+\frac{7}{x^2}+\frac{5}{x}-2\) = 0
⇒ 1 – 3x + 7x2 + 5x3 – 2x4 = 0
⇒ 2x4 – 5x3 – 7x2 + 3x – 1 = 0

Question 20.
Form the polynomial equation whose roots are the squares of the roots of x3 + 3x2 – 7x + 6 = 0. [May ’02]
Solution:
Let f(x) = x3 + 3x2 – 7x + 6 = 0
The required equation is f(√x) = 0
(√x)3 + 3 (√x)2 – 7√x +6 = 0
⇒ x√x + 3x – 7√x + 6 = 0
⇒ 3x + 6 = – √x (x – 7)
Squaring on both sides
9x2 + 36 + 36x = x (x2 + 49 – 14x)
= x3 + 49x – 14x2
x3 – 23x2 + 13x – 36 = 0.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 21.
Form the polynomial equation whose roots are the cubes of the roots of x3 + 3x2 + 2 = 0.
Solution:
Let f(x) = x3 + 3x2 + 2 = 0
The required equation is f(\(\sqrt[3]{x}\))= 0
\((\sqrt[3]{x})^3+3(\sqrt[3]{x})^2\) + 2 = 0
⇒ x + 3 . x2/3 + 2 = 0
x + 2 = – 3x2/3
Cubing on both sides (x + 2)3 = – 27x2
⇒ x3 + 8 + 6x2 + 12x + 8 = – 27x2
x3 + 33x2 + 12x + 8 = 0

Question 22.
If α, β, γ are the roots of x3 + px2 + qx + r = 0 then find
i) Σα2
ii) Σα3
iii) Σ \(\frac{1}{\alpha}\)
Solution:
Given equation is x3 + px2 + qx + r = 0
Since α, β, γ are the roots of the equation x3 + px2 + qx + r = 0 then
s1 = α + β + γ = \(\frac{-\mathrm{p}}{1}\) = – p;
s2 = αβ + βγ + γα = \(\frac{q}{1}\) = q;
s3 = αβγ = \(\frac{-r}{1}\) = – r.

i) Σα2 = α2 + β2 + γ2
= (α + β + γ)2 – 2(αβ + βγ + γα)
= (- p)2 – 2(q)
= p2 – 2q

ii) Σα3 = α3 + β3 + γ3
= (α + β + γ) (α2 + β2 + γ2 – αβ – βγ – γα) + 3αβγ
= (- p) ((p2 – 2q) – (+ q)) + 3(- r)
= – p (p2 – 2q – q) – 3r
= – p3 + 3pq – 3r

iii) \(\Sigma \frac{1}{\alpha}=\frac{1}{\alpha}+\frac{1}{\beta}+\frac{1}{\gamma}\)
= \(\frac{\beta \gamma+\alpha \gamma+\alpha \beta}{\alpha \beta \gamma}=\frac{q}{-r}=\frac{-q}{r}\)

Question 23.
Form the polynomial equation of the lowest degree with roots as 0, 0, 2, 2, – 2, – 2.
Solution:
The polynomial equation whose roots are 0, 0, 2, 2, – 2, – 2 is
(x – 0) (x – 0) (x – 2) (x – 2) (x + 2) (x + 2) = 0
⇒ x2 (x – 2)2 (x + 2)2 = 0
⇒ x2 (x2 + 4 – 4x) (x2 + 4 + 4x) = 0
⇒ x2 [(x2 + 4)2 – (4x)2] = 0
⇒ x2 (x4 + 16 + 8x2 – 16x2) = 0
⇒ x2 (x4 – 8x2 + 16) = 0
⇒ x6 – 8x4 + 16x2 = 0.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 24.
Form the monic polynomial equation of degree 3 whose roots are 2, 3 and 6. [May ’14, March ’02]
Solution:
x3 – 11x2 + 36x – 36 = 0

Question 25.
Form the monic polynomial equation of degree 4 whose roots are 4 + √3, 4 – √3, 2 + i and 2 – i.
Solution:
x4 – 12x3 + 50x2 – 92x + 65 = 0

Question 26.
Find s1, s2, s3 and s4 for the equation 8x4 – 2x3 – 27x2 – 6x + 9 = 0.
Solution:
s1 = \(\frac{1}{4}\),
s2 = \(\frac{-27}{8}\),
s3 = \(\frac{3}{4}\),
s4 = \(\frac{9}{8}\)

Question 27.
Find the algebraic equation whose roots are 3 times the roots of x3 + 2x2 – 4x + 1 = 0.
Solution:
x3 + 6x2 – 36x + 27 = 0

Question 28.
Find an algebraic equation of degree 4 whose roots are 3 times the roots of the equation 6x4 – 7x3 + 8x2 – 7x + 2 = 0. [March ’09]
Solution:
6x4 – 21x3 + 72x2 – 189x + 162 = 0.

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 29.
Find the transformed equation whose roots are the negatives of the roots of x4 + 5x3 + 11x + 3 = 0. [AP – Mar. 2015]
Solution:
x4 – 5x3 – 11x + 3 = 0

Question 30.
Find the polynomial equation of degree 4 whose roots are the negatives of the roots of x4 – 6x3 + 7x2 – 2x + 1 = 0.
Solution:
x4 + 6x3 + 7x2 + 2x + 1 = 0

Question 31.
Find the polynomial equation whose roots are the reciprocals of the roots of x5 + 11x4 + x3 + 4x2 – 13x + 6 = 0.
Solution:
6x5 – 13x4 + 4x3 + x2 + 11x + 1 = 0

Question 32.
Find the polynomial equation whose roots are the reciprocals of the roots of the equation x4 + 3x3 – 6x2 + 2x – 4 = 0.
Solution:
4x4 – 2x3 + 6x2 – 3x – 1 = 0

TS Inter Second Year Maths 2A Theory of Equations Important Questions Very Short Answer Type

Question 33.
Find the polynomial equation whose roots are the squares of the roots of x4 + x3 + 2x2 + x + 1 = 0.
Solution:
x4 + 3x3 + 4x2 + 3x + 1 = 0

Question 34.
Find the polynomial equation whose roots are the squares of the roots of x3 – x2 + 8x – 6 = 0.
Solution:
x3 + 15x2 + 52x – 36 = 0

TS Inter 1st Year Chemistry Notes Chapter 8 Hydrogen and its Compounds

Here students can locate TS Inter 1st Year Chemistry Notes 8th Lesson Hydrogen and its Compounds to prepare for their exam.

TS Inter 1st Year Chemistry Notes 8th Lesson Hydrogen and its Compounds

→ The only element that is placed in different groups of long form of periodic table is Hydrogen. The groups are IA, VIIA, etc.

→ Oxides of IA groupware basic while oxides of VIIA group are acidic. But water is practically neutral.

→ In non-metal hydrides, hydrogen exhibits +1 oxidation state while in metal hydrides hydrogen exhibits – 1 oxidation state.

→ Atoms of the same element with different mass numbers are called Isotopes.

→ Protium, Deuterium and Tritium are the three isotopes of Hydrogen.

→ Tritium is the lightest radioactive isotope. It decays by beta emission.

→ Hydrogen is a potential fuel. It has many industrial applications and is a source for atomic energy.

→ Water which does not produce lather readily with soap is called Hard water.

TS Inter 1st Year Chemistry Notes Chapter 8 Hydrogen and its Compounds

→ The reason for the hardness of water is the presence of dissolved salts of Ca+2 and Mg+2 ions.

→ Hardness of water can be removed by boiling, Clark’s process, Soda process, Calgon Process, Permutit process and use of Ion- exchange resins.

→ Deuterium oxide is also called Heavy water.

→ Heavy water is prepared by the exhaustive electrolysis of N/2 NaOH solution.

→ Heavy water is used as moderator in nuclear reactor for slowing down the speed of neutrons.

→ The structural unit in a peroxide is O2-2 and has the O-O bond, called peroxy bond.

→ H2O2 molecule has open book structure.

→ 30% solution of H2O2 is called perhydrol.

TS Inter 1st Year Chemistry Notes Chapter 9 s-Block Elements

Here students can locate TS Inter 1st Year Chemistry Notes 9th Lesson s-Block Elements to prepare for their exam.

TS Inter 1st Year Chemistry Notes 9th Lesson s-Block Elements

→ Lithium, Sodium, Potassium, Rubidium, Caesium and Francium are the six elements present in IA group.

→ Elements of IA group are called alkali metals. Their hydroxides are water soluble and the solutions are basic.

→ The general electronic configurations of IA group elements is ns1.

→ Alkalj metals are highly electropositive and good reductants.

→ Common oxidation state of alkali metals is +1 and they usually form ionic compounds.

→ Sodium is prepared by the electrolysis of fused NaOH in Castner’s process. In Down’s process, it is prepared by the electrolysis of fused NaCl.

→ Sodium hydroxide is called caustic soda. It can be prepared by the electrolytic process in Nelson cell (or) Castner-Kellner cell.

→ Na2CO3.10H2O is called washing soda. Na2CO3 is called soda ash and NaHCO3 is called baking soda.

→ Na2CO3 is prepared on a large scale by Solvay – Ammonia Soda process.

TS Inter 1st Year Chemistry Notes Chapter 9 s-Block Elements

→ Elements of IIA group are called alkaline earth metals.

→ The general electronic configuration of IIA group elements is ns .

→ The common oxidation state of alkaline earth metals is + 2.

→ Magnesium is extracted by the electroly-sis of fused MgCl2.

→ Alkyl Magnesium Halides are known as Grignard reagents.

→ Magnesium sulphate heptahydrate (MgSO4) 7H2O is called Epsom salt.

→ Quick lime is calcium oxide.

→ When CO2 is passed through lime water, a milky white ppt. of CaCO3 is formed, which dissolves in -excess of CO2.

→ Mortar is a mixture of lime, sand and water.

→ The function of sand in mortar is to make the mass, porous.

→ Gypsum is calcium sulphate dihydrate CaSO4.2H2O.

→ Plaster of Paris is calcium sulphate hemihydrate CaSO4. \(\frac{1}{2}\)H2O. It is prepared by heating gypsum at 120°C.

TS Inter 1st Year Chemistry Notes Chapter 10 p-Block Elements: Group 13

Here students can locate TS Inter 1st Year Chemistry Notes 10th Lesson p-Block Elements: Group 13 to prepare for their exam.

TS Inter 1st Year Chemistry Notes 10th Lesson p-Block Elements: Group 13

→ Boron, Aluminium, Gallium, Indium and Thallium are the five elements of group III A.

→ III A group is also known as Boron – Aluminium family. They belong to p – block.

→ The general outer electronic configuration of IIIA group elements is ns2np1.

→ The valency of IIIA group elements is 3 and their common oxidation states are – 3, + 1 and +3.

→ The reluctance of outer s – electron pair (ns electrons) to unpair and participate in bond formation is called inert pair effect.

→ Boron is a non-metal and is a rare element.

→ Aluminium is the most abundant metal in earth’s crust.

→ The oxide of Boron is acidic and aluminium oxide is amphoteric.

TS Inter 1st Year Chemistry Notes Chapter 10 p-Block Elements: Group 13

→ Important minerals of ‘Al’ are Bauxite (Al2O3 . 2H2O), Cryolite (Na3AlF6).

→ Aluminium metal is extracted by the electrolysis of Bauxite dissolved in cryolite.

→ Crude ‘Al’ metal is purified by Hoope’s process.

→ A mixture of ‘Al’ powder and ammonium nitrate is called ammonal’ and is used as explosive.

→ A 1 : 3 mixture of ‘Al’ powder and Ferric oxide is called ‘thermite mixture’.

→ Potash alum is called common alum, with chemical formula K2SO4. Al2(SO4)3.24H2O.

→ Diborane (B2H6) is prepared by the reduction of Boron trichloride.

→ Diborane is electron deficient molecule and has two three – centered – 2 – electron bonds.

→ Borazole is called inorganic benzene and has the chemical formula B3N3H6.

TS Inter 1st Year Chemistry Notes Chapter 11 p-Block Elements: Group 14

Here students can locate TS Inter 1st Year Chemistry Notes 11th Lesson p-Block Elements: Group 14 to prepare for their exam.

TS Inter 1st Year Chemistry Notes 11th Lesson p-Block Elements: Group 14

→ Carbon, Silicon, Germanium, Tin and Lead are the five elements present in group 14 .

→ The general outer electronic configuration of elements of group IV A is ns2np2.

→ Carbon and Silicon are non-metals. Tin and Lead are metals.

→ Germanium is a metalloid.

→ The general oxidation states of group IV A elements are – 4, + 2, and +4.

→ The +4 state exhibited by lead is less stable due to inert pair effect’.

→ The property of self-linkage among the atoms of the same element to form long chains and rings is called catenation.

→ Existence of an element in two or more physical forms is called allotropy.

→ The crystalline allotropic forms of carbon are Diamond, Graphite and Fullerenes.

→ Silicon is the second most abundant element in earth’s crust.

→ Silicon carbide is called carborundum.

→ Silicon dioxide has a three-dimensional network structure.

TS Inter 1st Year Chemistry Notes Chapter 11 p-Block Elements: Group 14

→ Silicon dioxide is called silica. Pure silica is called Quartz.

→ A mixture of silicates of sodium and calcium is called glass.

→ CO is formed by the partial combustion of carbon in oxygen.

→ CO2 is formed by the complete combustion of carbon in oxygen.

→ Gases which burn and produce heat energy are called fuel gases.

→ A mixture of CO and N2 is called Producer gas.

→ A mixture of CO and H2 is called Water gas or Blue gas.

→ Semi water gas is a mixture of CO, N2 and H2.

→ Natural gas mainly contains methane, along with ethane and propane.

TS Inter 1st Year Chemistry Notes Chapter 12 Environmental Chemistry

Here students can locate TS Inter 1st Year Chemistry Notes 12th Lesson Environmental Chemistry to prepare for their exam.

TS Inter 1st Year Chemistry Notes 12th Lesson Environmental Chemistry

→ The surroundings in which we live is called environment.

→ The protective blanket of gases surrounding the earth is called atmosphere.

→ Environment can be divided into four segments

  • Atmosphere
  • Hydrosphere
  • Lithosphere and
  • Biosphere.

→ An unwanted chemical substance released into environment which adversely affects the environment is called a pollutant.

→ A substance which is not present in nature, but released during human activity and adversely affects the environment is called a contaminant.

→ The medium which is affected by a pollutant is called a receptor.

→ The medium which retains and interacts with the pollutant is called sink.

→ The oxygen content present in the dis¬solved state in water is called Dissolved Oxygen (DO).

→ The amount of oxygen required to oxidise organic substances present in polluted water is called Chemical Oxygen Demand (COD).

TS Inter 1st Year Chemistry Notes Chapter 12 Environmental Chemistry

→ The amount of oxygen used by the micro-organisms present in the water for five days at 20°C is called Biochemical Oxygen Demand (BOD).

→ The permissible level of toxic pollutant in the atmosphere to which a healthy industrial worker is exposed during an 8 hour day without any adverse effect is called Threshold Limit Value (TLV).

→ The phenomenon of heating up of the sur¬face of the earth due to accumulation of CO2 and other greenhouse gases such as CH4, CFCs, O3, N2O, H2O is called Greenhouse effect or global warming.

→ Ozone in the stratosphere acts as protec¬tive layer but harmful if it is present in the troposphere.

→ Compounds containing carbon, fluorine and chlorine are called chlorofluorocarbons. They are also known as freons.

→ Freons are used as refrigerants and aerosols.

→ The active chlorine catalyses the decomposition of ozone to oxygen. This is called depletion of ozone layer.