Saturday, July 3, 2021
Suppose 10–17 J of light energy is needed by the interior of the human eye to see an object. How many photons of green light (wavelength =550 nm) are needed to generate this minimum amount of energy?
(1) The ionization energy of He+ is 19.6 10^-18 J
atom^-1. The energy of the first stationary state of Li+2 will be :
(2) Show that the wavelength of a 150 g rubber ball
moving with a velocity 50 m sec^-1 is short enough to be observed ..
(3) If an electron is present in n = 6 level. How many
spectral lines would be observed in case of H atom ...
(4) Speed of helium atom at 300K is 2.40 x10^2 meter per
sec. What is its wave length. (mass number of helium is 4)..
(5) K.E. of the electron is 4.55 x 10^-25 J. Its de
Broglie wave length is ...
(6) The wavelength associated with a golf ball weighing
200g and moving at a speed of 5m/h is of the order.
(7) The ratio of wave length of photon corresponding to
the alpha-line of Lyman series in H-atom and Beta-line of Balmer series in He+
is
(8) shortest wavelength of He+ ion in Balmer series
is x, then longest wavelength in the Paschene series of Li+2 is
(9) The ratio of difference in wavelengths of 1st and 2nd
lines of Lyman series in H like atom to difference in wavelength for 2nd and
3rd lines of same series is:
(10) If H+ (ion) is accelerated to a final velocity of
6.62×10+6 meter per second and error in velocity is 1% then find uncertainty in
position is?
(11) What is the relation between Total energy (TE),
Kinetic energy (KE) and Potential energy (PE) of Bohr's orbits?
(12) How to calculate energy of Bohr's orbits in term of
Rydberg's constant
Calculate the energy per mole of photon of electromagnetic radiations of wavelength 4000Å.
Related Questions:
(1) On the basis of Heisenbergs uncertainty principle,
show that the electron cannot exist within the nucleus.
(2) Atomic radius is the order of 10^-8 cm. and nuclear
radius is the order of 10^--13 cm. Calculate what fraction of atom is occupied
by nucleus
(3) Electromagnetic radiations of wavelength 242 nm is
just sufficient to ionise sodium atom. Calculate the ionisation energy of
sodium in kJ mol^-1.
(4) The shortest wave length in H spectrum of Lymen
series when Rh = 109678 cm^1 is
(5) An electron beam can undergo diffraction by crystals.
Through what potential should a beam of electrons be accelerated so that its
wavelength becomes equal to 1.54 A
(6) The mass charge ratio for A+ ion is 1.97x10^-7 kg
C^-1. Calculate the mass of A atom.
(7) AIR service on Vividh Bharati is transmitted on 219 m
band. What is its transmission frequency in Hertz?
(8) Calculate the number of photon emitted in 10 hours by
a 60 W sodium lamp (lemda or photon = 5893 A")
(9) Calculate the longest wavelength which can remove the
electron from first Bohrs orbit. Given E1 = 13.6 eV .
(10) Calculate momentum of radiations of wavelength 0.33
nm.
The quantum theory assumes that energy changes are not continuous. Why do not we notice this effect in our everyday activities?
In everyday activities, we deal with macroscopic particles such as our bodies, or cars which gains and loss total amount of energy much larger than a quantum. The gain and loss of the relatively miniscule quantum of energy is unnoticed.
Related Questions:
What is the difference between 2p and 3p orbitals?
Why are 2p orbitals higher in energy than 2s?
Does 2s and 2p have the same energy?
Calculate radial and angular node for 2p-orbitals.
What are the difference between "Nodal surface" and "Nodal plane"?
What are Zeeman and Stark effects? Were they
explained by the Bohr’s theory?
Which of the Hydrogen spectrum series found in
visible range of spectrum?
What are difference between "Isoelectronic"
and "Isosters" species?
What are the difference between "Kernel" and
"Core" ?
Thursday, July 1, 2021
Sunday, June 27, 2021
General Inorganic Chemistry (Interactive mechanism of inorganic reactions):
(1)-Classification
of Elements & Periodicity in properties
(2) Structure of atom and Electronic configuration
(3)-Chemical bonding
& Molecular Structures
3.1 Chemical Bonds
3.2 Ionic Bond
3.3 Covalent bond (sigma and pi Bond)
3.4 Coordinate bond
3.5 Valence Bond Theory
3.5 Hybridization
3.6 VSEPR Theory
3.6 MOT
(4)-General Inorganic
Chemistry (G.Ino.C)
3.1 Dipole Moment
3.2 Fajan’s Rule
3.3 Resonance
3.4 D-Orbital resonance
3.5 Bent’s rule of hybridization
3.6 Drago’s rule: No need of hybridization
3.7 Back bond
3.8 Bridge Bond: Multi-centered Bond
3.9 Vander Waal’s force
3.10 Hydrogen Bond
3.11 Metallic Bond
5-Acid-Base Concepts/theories
4.1 Arrhenius Acid–Base concept
4.2 Bronsted Lowery Acid-base concept:
4.3 Lewis Acid-Base concepts:
4.4 The Solvent System (Self or Auto Ionization of Solvent):
4.5 The Lux-Flood Acids-base concepts:
4.6 The Usanovich Acid-base concepts:
6-Oxides (Acid
anhydrides)
5.1 Classification of oxides: (On the Basis of oxygen content):
5.2 Classification of oxides: (On the basis of Acid-Base Interaction):
7-Oxy acids and its Salts
6.1 Oxy acids of Boron:
6.2 Oxy acids of Silicon:
6.3 Oxy acids of Nitrogen:
6.4 Oxy acids of Phosphorous:
6.5 Oxy acids of Sulphur:
6.6 Oxy acids of Chlorine:
(8)-Type of
inorganic reactions
(9)-Hydrolysis
Mechanism
8.1 Hydrolysis of Halides of 13th group:
8.2 Hydrolysis of Halides of 14th group:
8.3 Hydrolysis of Halides of 15th group:
8.4 Hydrolysis of Halides of 16th group:
8.5 Hydrolysis of Interhalogen compounds:
8.6 Hydrolysis of Halides of 18th group:
8.7 Hydrolysis of peroxy acids:
8.8 Hydrolysis of Oxides:
8.9 Hydrolysis of Carbides:
8.10 Hydrolysis of Nitrides:
8.11 Hydrolysis of Hydrides:
8.12 Hydrolysis of phosphides:
8.13 Hydrolysis of sulphides:
8.14 Hydrolysis of Silicides:
8.15 Hydrolysis of Borides:
8.16 Hydrolysis of Phosphides:
(10)-Effect of heat on compounds (acids, bases and Salts)
9.1 Thermal stability of salts
9.2 Thermal Decomposition Reactions
(11)- The
Coordination compounds
(12)- Quantitive Analysis (Salts Analysis):
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