Define chemical bonding and electro theory of valency

 Chemical Bonding and Electro-Theory of Valency:

• Chemical bonding is the process by which atoms are held together in molecules or ions.
• The electro-theory of valency states that the chemical behavior of an element is determined by the number of electrons in its outermost energy level, or valence shell.
• The number of electrons in the valence shell is referred to as the element's valency.
• Elements with a valency of one or two tend to form ions by losing or gaining electrons, respectively, while elements with a valency of four or more tend to form covalent bonds by sharing electrons.

Define orbit & orbital, shapes of orbitals s,p,d,f

 Orbit and Orbital:

• An orbit is the path that an electron follows as it moves around the nucleus of an atom.
• An orbital is a mathematical representation of an electron's energy and wave-like behavior.
• Orbitals are described by three quantum numbers: n, l, and m, which define the size, shape, and orientation of the orbital, respectively.
• There are four main types of orbitals: s, p, d, and f, which differ in their shapes and energy levels.
• The s orbitals are spherical in shape, while p orbitals are dumbbell-shaped, d orbitals are cloverleaf-shaped, and f orbitals are more complex and less well understood.

 

Describe the electronic configuration elements upto atomic number 30

• The electronic configuration of elements refers to the arrangement of electrons in the energy levels (or shells) surrounding the nucleus of an atom. 
• The number of electrons in each shell is determined by the element's atomic number, which is equal to the number of protons in the nucleus. 
• The first 20 elements have a simple electron configuration, which can be easily predicted using the Aufbau principle.

Electronic Configuration upto 30 Elements

• Hydrogen (1 electron) - 1s1
• Helium (2 electrons) - 1s2
• Lithium (3 electrons) - 1s2 2s1
• Beryllium (4 electrons) - 1s2 2s2
• Boron (5 electrons) - 1s2 2s2 2p1
• Carbon (6 electrons) - 1s2 2s2 2p2
• Nitrogen (7 electrons) - 1s2 2s2 2p3
• Oxygen (8 electrons) - 1s2 2s2 2p4
• Fluorine (9 electrons) - 1s2 2s2 2p5
• Neon (10 electrons) - 1s2 2s2 2p6
• Sodium (11 electrons) - 1s2 2s2 2p6 3s1
• Magnesium (12 electrons) - 1s2 2s2 2p6 3s2
• Aluminum (13 electrons) - 1s2 2s2 2p6 3s2 3p1
• Silicon (14 electrons) - 1s2 2s2 2p6 3s2 3p2
• Phosphorus (15 electrons) - 1s2 2s2 2p6 3s2 3p3
• Sulfur (16 electrons) - 1s2 2s2 2p6 3s2 3p4
• Chlorine (17 electrons) - 1s2 2s2 2p6 3s2 3p5
• Argon (18 electrons) - 1s2 2s2 2p6 3s2 3p6
• Potassium (19 electrons) - 1s2 2s2 2p6 3s2 3p6 4s1
• Calcium (20 electrons) - 1s2 2s2 2p6 3s2 3p6 4s2

 

The electron configuration for elements beyond atomic number 20 becomes more complex and is determined by the filling of the 3d and 4s subshells. Some of the elements and their electron configurations up to atomic number 30 are:

 

• Scandium (21 electrons) - [Ar] 3d1 4s2
• Titanium (22 electrons) - [Ar] 3d2 4s2
• Vanadium (23 electrons) - [Ar] 3d3 4s2
• Chromium (24 electrons) - [Ar] 3d5 4s1
• Manganese (25 electrons) - [Ar] 3d5 4s2
• Iron (26 electrons) - [Ar] 3d6 4s2
• Cobalt (27 electrons) - [Ar] 3d7 4s2
• Nickel (28 electrons) - [Ar] 3d8 4s2
• Copper (29 electrons) - [Ar] 3d10 4s1
• Zinc (30 electrons) - [Ar] 3d10 4s2

 

It is important to note that these electron configurations are only approximate and do not take into account the interactions between electrons, such as spin and electron.

Explain pauls exclusion principle

 

Pauli's Exclusion Principle:

• The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers.
• This means that each orbital can only hold two electrons, with opposite spins.
• The Pauli exclusion principle helps to explain the stability of atoms and their electronic configurations.
• Without the exclusion principle, electrons would occupy the same orbital and would experience mutual repulsion, leading to an unstable atom.

Describe the concept of Hund's rule

 Hund's Rule:

• Hund's rule states that when there are multiple orbitals of the same energy level, electrons will occupy each orbital with a single electron before any orbital has two electrons.
• This results in an unpaired electron, which is important in determining the magnetic behavior of an atom.
• Hund's rule helps to explain why some elements have unpaired electrons, which can have a significant effect on their chemical behavior.
• Hund's rule is a key principle in understanding the electronic configurations of atoms and the behavior of molecules.

Define the concept of the Bohrs Atomic model

 Bohr's Atomic Model:

• a. The Bohr atomic model was proposed by Niels Bohr in 1913.
• The model proposed that electrons move around the nucleus in defined orbits and that the energy of an electron is proportional to its distance from the nucleus.
• Bohr also proposed that electrons could only exist in specific orbits and that transitions between orbits were associated with the emission or absorption of light.
• The Bohr model was a major step forward in our understanding of the structure of atoms and helped to lay the foundations of quantum mechanics.
• Although the Bohr model is no longer considered to be a complete and accurate description of the atom, it is still useful in introductory chemistry courses.

 

Explain the Aufbau principle with suitable electronic configuration examples

Aufbau Principle:

• The Aufbau principle states that electrons occupy the lowest energy orbitals first, and then successively fill higher energy orbitals.
• This principle is used to predict the electronic configuration of an element.
• Electrons are filled into orbitals in order of increasing energy until all electrons are accounted for.
• For example, the electronic configuration of helium is 1s2, which means that the first two electrons occupy the 1s orbital.
• The Aufbau principle is based on the idea that electrons will occupy the lowest energy available to them.

Define Atomic structure, atomic number, atomic mass number

Atomic structure:

• Atoms are made up of three types of subatomic particles: protons, neutrons, and electrons.
• The nucleus, located at the center of the atom, contains protons and neutrons, while electrons orbit the nucleus in shells or energy levels.
• The arrangement of electrons in an atom's energy levels determines its chemical properties and behavior.

Atomic number:

• Atomic number is the number of protons in the nucleus of an atom.
• The atomic number determines the element to which an atom belongs.
• Elements with the same atomic number have similar chemical properties.

Atomic mass number:

• Atomic mass number is the total number of protons and neutrons in the nucleus of an atom.
• Isotopes of the same element have the same atomic number but different atomic mass numbers.
• The atomic mass of an element listed on the periodic table is an average of the atomic masses of all its isotopes, weighted by their relative abundances.

 

ECET Chemistry: Water Technology

1. Define soft water and hard water
2. Define hardness and causes of hardness
3. Describe different types of hardness
4. What are the disadvantages of hard water in industries
5. Describe the characteristics of drinking water
6. Define the degree of hardness, and its use and units
7. Describe the municipal treatment of water for drinking purpose
8. Describe the processes of osmosis and reverse osmosis
9. What are the advantages and disadvantages of osmosis and reverse osmosis

ECET Chemistry: Corrosion

1. Define Corrosion
2. Factors influencing the rate of corrosion
3. Electrochemical theory of corrosion
4. Define composition, stress, and concentration cells
5. Define rusting of iron and its mechanism
6. Methods of preventing corrosion- a.protective coating, cathodic protection

ECET Chemistry: Electrochemistry

1. Define conductors, insulators, and electrolyte
2. What are the types of conductors
3. Describe electrolysis of fused NACL and aqueous NACL
4. Describe the Arrhenius theory of electrolytic dissociation
5. Define faradays laws of electrolysis
6. Define galvanic cell and its uses
7. Define electrode potential and standard electrode potential
8. Describe the electro-chemical series and its significance
9. Define the concept of emf
10. Working principle and applications of batteries and fuel cell

ECET Chemistry: Principles of Metallurgy

1. Define metal and non-metal, characteristics of metal
2. Define the concept of metallurgy
3. Define the terms- ore, flux, gangue, and slag
4. Describe the principle of concentration of ore by the froth flotation
5. Steps involved in the concentration of ore- roasting, calcination, and smelting
6. Composition and applications of alloys
7. Define alloy and properties of alloy

ECET Chemistry: Acids and Bases

1. Define acid and base
2. Describe Arrhenius's theory of acids and bases
3. Describe Bronsted Lowry's theory of acids and bases
4. Define the ionic product of water and the concept of ph
5. describe the lewis theory
6. Describes strong and weak acid bases
7. Define buffer and types of buffer, a.acid buffer, b.basic buffer
8. Application of Buffer Solution

ECET Chemistry: Solutions and Colloids

1. Define solution, solute, and solvent
2. Classification of solutions based on the physical state
3. Define the mole concept
4. Define molecular weight and equivalent weight
5. MW & EW of acid, base, and salt
6. Define mole and the concept of molarity and normality
7. Applications of colloids
8. Define colloids and their types- a.iyophillic, b.iyophobic

ECET: Fundamentals of Chemistry

1. Define Atomic structure, atomic number, atomic mass number
2. Explain the Aufbau principle with suitable electronic configuration examples
3. Define the concept of the Bohrs Atomic model
4. Describe the concept of Hund's rule
5. Explain pauls exclusion principle
6. Describe the electronic configuration elements upto atomic number 30
7. Define orbit & orbital, shapes of orbitals s,p,d,f
8. Define chemical bonding and electro theory of valency
9. Types of chemical bonds with characteristics, a.ionic bond, b.covalent bond, c.coordinate covalent bond
10. Explaint the concept of oxidation and reduction

ECET: Modern Physics

1. Define photo electric effect
2. Define Threshold frequency,Threshold wavelength,Work function, Stopping potential
3. Laws of photo electric effect & applications of photo electric effect
4. Einstein photo electric equation & Critical angle
5. Concept of total internal reflection
6. Super conductors and conductivity & Application and properties of super conductors
7. Optical fibre its principal, and its applications

ECET Physics: Elements of Vectors

S.No.	Topic
1	Define Scalar, Vector, Tensor with examples
2	Representation of Scalar and Vector
3	Types of vectors
4	Vector Additional Rules
5	Resolution of vectors
6	Laws used for determining resultant of vector
7	Pseudo vectors and equal vectors
8	Scalar product or dot product
9	Vector Product or cross product

ECET Physics: Heat and Thermodynamics

1. Define - Heat, temperature, critical temperature, scales of temperature, celsius, fahrenheit, kelvin scale or absolute scale
2. Relation between different scales
3. Boyles law and Charles law | its validity
4. Ideal gas and ideal gas equation
5. Gas constant, universal gas constant, SI units of UGS, value of UGS
6. Charles law in terms of absolute temperature, gas equation in terms of density
7. Daltons law of partial pressure
8. Define thermodynamics & laws of thermodynamics
9. Isothermal and adiabatic process
10. specific heat of substance, SH of gas at cp & cv
11. Molar specific heat of gas, MSH of gas at cp & cv
12. Ratio of cp&cv, derivation of relation | cp-cv=R
13. Define manometric and diatomic gas and its cp cv r(gama=cp/cv) values relations

ECET Physics: Units and Dimensions

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1 Define physical quantity

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2 Fundamental and derived physical quantity with examples

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3 Define the Unit & characteristics of the unit

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4 Base, Supplementary & special units

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5 Define Multiples and sub-multiples of units

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6 Define SI units, their advantages & disadvantages

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7 Define dimension, dimensional formulas, and their uses

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8 Dimensional constants & dimensionless quantities

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9 Principal of homogeneity of dimensions

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10 Limitations of dimensional analysis

ECET Physics: Kinematics

1. Define rest & motion, speed & velocity, displacement & distance, uniform & non-uniform speed & velocity, instantaneous velocity, acceleration
2. Equation of motion of a body moving with constant acceleration along straight line
3. Motion under gravity and equations of motion under gravity
4. Equations of vertical, horizontal and oblique projection
5. Average velocities with variation in S,V
6. Equations of motion in special case
7. Equations of projectile,trajectory Position after time t, velocity after time t