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SI Units - Basic Chemistry in Hindi Part 1

SI Units - Basic Chemistry in Hindi Part 1

SI Units - Basic Chemistry in Hindi Part 1
In this video we learn about SI System of units. We learn about 7 basic SI units, derived units, international system of units. In this video of Basic chemistry we get all information about SI units Which are used in physic and chemistry science experiments.
Watch this video below or at YouTube Link : https://youtu.be/eR6SCVLrVPE
by- www.ChemistryNotesInfo.com

SI System

7 SI Base Units

Base physical quantity
Symbol for quantity
SI units name
SI units symbol
Length
l
Metre
m
Mass
m
Kilogram
Kg
Time
t
Second
s
Current
I
Ampere
A
Temperature
T
Kelvin
K
Amount of substance
n
Mole
Mol
Luminous intensity
Iv
candela
Cd

Prefixes for SI Units

Multiple
Prefix
Symbol
 10-24
Yocto
y
10-21
Zepto
z
10-18
Atto
a
10-15
Femto
f
10-12
Pico
p
10-9
Nano
n
10-6
Micro
m
10-3
Milli
m
10-2
Centi
c
10-1
Deci
d
10
Deca
da
102
Hecto
h
103
Kilo
k
106
Mega
M
109
Giga
G
1012
Tera
T
1015
Peta
P
1018
Exa
E
1021
Zeta
Z
1024
yotto
Y


Heat and Temperature

What is Heat?

The exchange of energy due to difference in temperature is called heat. But as a noun we can say that the Heat is the quality of being hot or high temperature and to understand easily we can say that feeling of hot or warm is heat.

Heat

The exchange of energy due to difference in temperature is called heat. We may also explain as, heat is the form of the energy that is moved between two substances at different temperatures. Means if two substances are in contact and one has 200K temperature and other have 100K temperature then the direction of energy flow is from the substance at the higher temperature to the substance of lower temperature. Means in above case heat flows from substance having 200k temperature to substance having 100K temperature.
Heat is a form of energy so heat is measured in units of energy, commonly calories or joules.

What is Temperature?

Temperature is the quantity of hotness or coldness of any substance. Simply we can say that Temperature is the measurement of how much an object is hot or cold.

Temperature

Temperature is the quantity of hotness or coldness. Also in scientific way, temperature is explained as the average kinetic energy per molecule of a substance. Heat and Temperature (Temp, T) are two different terms and have different meanings so don’t get confuse between them.  Heat is energy while temperature is not energy. Heat is measured in Joules while temperature is measured in Celsius (C), Fahrenheit (F) or Kelvin (K). Symbol used for heat is Q while symbol used for temperature is T. SI unit of heat is Joule while SI unit of temperature is Kelvin.

Heat VS Temperature

Heat is the flow of energy from hot object to cold object while temperature is the measurement of how much an object is hot or cold. Heat is energy while temperature is not energy. Heat is measured in Joules while temperature is measured in Celsius (C), Fahrenheit (F) or Kelvin (K). Symbol used for heat is Q while symbol used for temperature is T. SI unit of heat is Joule while SI unit of temperature is Kelvin.


Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Chemistry Formulas for Nuclear Chemistry (Radioactivity)

Empirical relationship between size of nucleus and its mass number is
            R = R0A1/3
Where,                       
            R = radius of nucleus,
            A = mass number,
            R0 = contestant = 1.4x10-13cm

Rate of Decayof radioactive substance

Where,
            K = decay constant,
            N = No. of atoms,
            t = time of decay,
            dN = small fraction of N,
            dt = small fraction of t

Value of Decay Constant

            
Where,
            N0 = No. of atoms originally present,
            N = No. of atoms present after time t

Half Life Time (t1/2)

            t1/2 = 0.693/K
Where,
            K = decay constant

Average Life Time (T)

            Average life time (T) =Sum of the lives of the nuclei/ Total number of nuclei
            T = 1/K 
Also,
            Average life time (T) = 1.44 x Half-life (T1/2)
Where,
            K = decay constant
            T = Average Life Time
            T1/2 = Half Life

Specific Activity

            Specific Activity = Rate of decay/m
                                      = KN/m
                                      = K x Avogadro Number/ Atomic Mass in gram
Where,
            N = Number of Radioactive nuclei that undergoes disintegration

Units of Radioactivity

            Standard unit of radioactivity is curie (c).
            1c = Activity of 1gram Ra226 = 3.7 x 1010dps
Where,
            dps = disintegrations per second
millicurie (mc) = 3.7 x 107dps
microcurie (µc) = 3.7 x 104dps
Other units of radioactivity are Rutherford (rd) and Becquerel (Bq).

Rutherford (rd)

1rd = 106dps

Becquerel (Bq)

            Becquerel (Bq) is the SI unit of radioactivity.
                        1Bq = 1 disintegrations per second
                        1 Bq = 1 dps

Radioactive Equilibrium

            A ----à B ----à C
            At steady state,
                        NA/NB = KB/KA = TA/TB
Where,
            KA = radioactivity constant for the process A---àB
            KB = radioactivity constant for the process B---àC
            TA = average life period of A
            TB = average life period of B
Radioactive Equilibrium in terms of half-life periods,
            NA/NB = (T1/2)A/ (T1/2)B

Chemistry Formulas for Structure of Atom Part 1

Chemistry Formulas of Structure of Atom

Chemistry Formulas from Rutherford Atomic Model

·         Radius of Nucleus, rn = r0 × A1/3
Where, A = Mass Number,
               r0 = Proportionality Constant = 1.4 × 10-13 cm
·         Volume of the nucleus = Approx. 10-39 cm3
·         Volume of the atom = Approx. 10-24 cm3
·         Density of the nucleus = 1014 g cm-3
Or,

Important Characteristics of Three Fundamental Particles
1.      Electron
·         Charge on an Electron = -1.602×10-19 coulombs.
·         Mass of an Electron = 9.11×10-28 g
·         Specific Charge (e/m ratio) of electrons (cathode rays) = 1.76×108 coulombs/gram
·         Radius of the electron = 10-15 cm
·         Density of the electron = 2.17×1017g/cc
·         Mass of one mole of the electrons = Approx. 0.55mg
·         Charge on one mole of the electrons = 96500 Coulombs = 1 Faraday
2.      Proton
·         Mass of Proton = 1.672×10-24g
·         Charge on Proton = 1.602×10-19 Coulombs
·         Specific Charge of Proton = 9.58×104 Coulombs/gram
·         Mass of one mole of proton = 1.007 gram
·         Charge on one mole of proton = 96500 Coulombs = 1 Faraday
·         Volume of Proton = Approx. 1.5×10-38cm3
3.      Neutron
·         Mass of Neutron = 1.675×10-24g
·         Specific Charge on Neutron = 0
·         Density of Neutron = 1.5×1014g/cc
·         Mass of one mole of neutron = 1.008g
4.      Other Sub-Atomic Particles of Atom
·         Positrons
·         Neutrions
·         Mesons
Chemistry Formulas of Atomic Number (Z) and Mass Number (A)
·         General Symbol for an Atom of Element (E) indicating its Atomic Number (Z) and Mass Number (A)
ZEA
·         Atomic Number (Z) = Number of Protons = Number of Electrons
·         Mass Number (A) = Number of Protons + Number of Neutrons
·         No. of Neutrons = A – Z

Famous Scientists and their Inventions

Scientists and Their Important Research in the Field of Chemistry

chemist, chemistry, chemistry experiments, chemistry scientists, famous chemists, famous scientists, great scientists, list of scientists, names of scientists, scientific name, scientist names,
Given below is the list of scientists and their important research and inventions. These famous scientists or chemists perform many science and chemistry experiments which help in the development of Chemistry and Science. 

 List of Famous Scientists and their Inventions

List of Scientists
Research and Inventions
Ernest Rutherford
Bombardment of Atoms by alpha-particles
J. J. Thompson
Discovery of Electron, e/m of Electron
Eugen Goldstein
Discovery of Proton
James Chadwick
Discovery of Neutron
Louis De-Broglie
Wave Equation
Niels Henrik David Bohr
Atomic Model, Long Form of Periodic Table
Albert Einstein
Photoelectric Effect
Niels Bohr, Wolfgang Pauli and Friedrich Hund
Distribution of electrons
Heisenberg Principle
Uncertainty Principle
Becquerel
Radioactivity
Marie Curie
Radium
Francis William Aston
Mass Spectrograph
Dmitri Ivanovich Mendeleev
Periodic Law, Periodic Table
Sidwick and Powell
Theory of Hybridisation
Louis Allred and Eugene George Rochow
Electronegativity
Robert Sanderson Mulliken
Electronegativity
Robert Boyle
Boyle’s Law, Relation Between P and V
Jacques Alexandre César Charles
Charle’s Law, Relation Between T and V
Lorenzo Romano Amedeo Carlo Avogadro
Avogadro’s Law, Relation Between V and number of molecules (n)
John Dalton
Dalton’s Law, Relation Between the Total Pressure and Partial Pressure of Individual Gases
Thomas Graham
Graham’s Law, Relation Between the Rate of Diffusion and Density (or Molecular Weight) of Gases
François Marie Raoult
Raoult’s Law, Relation Between Partial Vapour Pressure and Mole Fraction
Harold Clayton Urey
Heavy Water
Henry Louis Le Chatelier
Le Chatelier Principle, Effect of P, T and Concentration of Reactants on the System in Equilibrium


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