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Recent questions tagged quantum-mechanical-model
Questions
The hydrogen-like species $Li^{2+}$ is in a spherically symmetric state $S_1$ with one radial node. Upon absorbing light the ion undergoes transition to a state $S_2$ has one radial node and its energy is equal to the ground state energy of hydrogen atom. The orbital angular momentum quantum number of the state $S_2$ is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q200
mock
asked
Feb 10, 2014
by
sharmaaparna1
1
answer
The hydrogen-like species $Li^{2+}$ is in a spherically symmetric state $S_1$ with one radial node. Upon absorbing light the ion undergoes transition to a state $S_2$ has one radial node and its energy is equal to the ground state energy of hydrogen atom. The state $S_1$ is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q198
asked
Feb 10, 2014
by
sharmaaparna1
1
answer
De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. The wavelength of a golf ball weighing 200g and moving at a speed of 5meter/hr is of the order:
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q197
asked
Feb 10, 2014
by
sharmaaparna1
1
answer
De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. If uncertainities in position and momentum of an electron are same , then uncertainity in its velocity can be given by
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q196
asked
Feb 10, 2014
by
sharmaaparna1
1
answer
De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential . The wavelength of helium atom whose speed is equal to its rms speed at $27^{\large\circ}$ C
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q193
asked
Feb 9, 2014
by
sharmaaparna1
1
answer
De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. With what velocity must an electron travel so that its momentum is equal to that of photon of wavelength of $\lambda = 5200A^{\large\circ}$
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q192
asked
Feb 9, 2014
by
sharmaaparna1
1
answer
The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. The number of spherical and angular nodes in 2p orbital are:
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q190
asked
Feb 9, 2014
by
sharmaaparna1
1
answer
The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. The total Magnetic momentum of $Ni^{2+}$ ion is....
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q189
asked
Feb 9, 2014
by
sharmaaparna1
1
answer
The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. Which in each pair is most stable ion: $Cu^+ or Cu^{2+} and Fe^{2+} or Fe^{3+}$
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q188
asked
Feb 9, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. An oil drop has $-6.39\times10^{-19}$ coulomb charge. The number of electrons in this oil drop is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q187
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. An oxide on N has vapour density 46. The total number of electrons in 92g of it are:
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q186
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. What is the minimum energy given out when an electron jumps from one orbit to other form.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q185
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the total number of fundamental particles in $^{14}_6C$ is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q184
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the Non-directional orbital.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q183
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
Rutherford proposed the atomic model after his most striking experiment on $\alpha$– scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the angular momentum of electron in 2p orbital is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q181
asked
Feb 8, 2014
by
sharmaaparna1
1
answer
The total energy of the electron of H-atom in the Second quantum State is $E_2$. The total energy of the ${He^+}$ atom in the third quantum state is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q201
asked
Feb 7, 2014
by
sharmaaparna1
1
answer
When a hydrogen atom emits a photon of energy 12.1eV, the orbital angular momentum changes by
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q176
asked
Feb 7, 2014
by
sharmaaparna1
1
answer
What is energy per mol of photons of FM radiowaves with V=102.5 MHZ ?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q174
asked
Feb 6, 2014
by
sharmaaparna1
1
answer
The dissociation energy of $H_2$ is 430.53KJ. If $H_2$ is exposed to light energy of wavelength 253.7 nm , what $\%$ of light energy will be converted into kinetic energy?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q173
asked
Feb 6, 2014
by
sharmaaparna1
1
answer
Calculate the maximum wavelength in $A^{\large\circ}$ a photon that can initiate the reaction. $Cl_2(g)\rightarrow 2cl(g), \bigtriangleup H = 247$ KJ/mol
sat
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q172
asked
Feb 6, 2014
by
sharmaaparna1
1
answer
Sodium atom emits light with a wavelength of 330nm when an electron moves from a 4p orbital to a 3s orbital. what is the energy difference between the orbitals in KJ/mol?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q171
asked
Feb 6, 2014
by
sharmaaparna1
1
answer
An argon laser emits blue light with a wavelength of 488.0nm. How many photon are emitted by this laser in 2.00 sec,operating a power of 515 milliwatts?(one watt = 1J$S^{-1}$)
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q170
asked
Feb 6, 2014
by
sharmaaparna1
1
answer
The energy required for the ionisation of a certain atom is $3.44\times10^{-18}J$. The absorption of a photon of unknown wavelength ionises the atom and ejects an electron with velocity $1.03\times10^6$ m/sec. Calculate the wavelength of the incident radiation.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q169
asked
Feb 5, 2014
by
sharmaaparna1
1
answer
An electron difraction experiment was performed with a beam of electrons accelerated by a potential difference of 10.0kV.What is the wavelength of the electron beam?(1KV = 1000V = 1000eV for the electron)
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q167
asked
Feb 5, 2014
by
sharmaaparna1
1
answer
A proton is accelerated to one tenth of the velocity of light. Suppose velocity can be measured with a precision of $\pm1\%$, what can be the uncertainity in its position?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q166
asked
Feb 5, 2014
by
sharmaaparna1
1
answer
The speed of a certain proton is $4.5\times10^5m$ If the uncertainity is to be reduced to 0.01percent, what uncertainity in its location must be tolerated?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q165
asked
Feb 5, 2014
by
sharmaaparna1
1
answer
Two particles A and B are in motion . if the wavelength associated with particle A is $5\times10^{-8}$m.Calculate the wavelength associated with particle B if its momentum is half of A.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q164
asked
Feb 5, 2014
by
sharmaaparna1
1
answer
Calculate the wavelength of a helium atom whose speed is equal to root mean square speed at 293 K $(rms = \sqrt{3RT/m})$
sat
chemistry
atomic-structure
jeemain
physical-chemistry
class11
unit2
quantum-mechanical-model
medium
q163
asked
Feb 4, 2014
by
sharmaaparna1
1
answer
The wavelength of $\beta$ line of the Balmer Series is $4815 A^{\large\circ}$. What is the wavelength of $\alpha$ line of balmer Series of the same atom?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q162
asked
Feb 4, 2014
by
sharmaaparna1
1
answer
AIR services on vividh Bharti is transmitted on 219m band.What is its transmission frequency in Hertz.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q161
asked
Feb 4, 2014
by
sharmaaparna1
1
answer
A certain laser transition emits $6.37\times10^{15}$ quants per second per square meter. Calculate the power out put in joule per square metre per second. Given $\lambda$ = 632.8 nm.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
medium
q160
asked
Feb 4, 2014
by
sharmaaparna1
1
answer
A photon of 300nm is absorbed by a gas and then re-emits two photons. One re-emitted photon has wavelength 496nm. Calculate energy of other photon re-emitted out.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
easy
q159
asked
Feb 4, 2014
by
sharmaaparna1
1
answer
The dissociation energy of $H_2$ is 430.53 KJ$mol^{-1}$. If $H_2$ is exposed to radiation energy of wavelength 253.7nm, what % of radiant energy will be converted into kinetic energy ?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q158
asked
Feb 1, 2014
by
sharmaaparna1
1
answer
A certain dye absorbs light of $\lambda = 4530 A^{\large\circ}$ and then fluorescence light of $5080 \;A^{\large\circ}$ Assuming that under given conditions $47\%$ of the absorbed energy is re-emmited out as fluorescence, Calculate the ratio of Quantum emitted out to the no. of quanta absorbed
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q157
asked
Feb 1, 2014
by
sharmaaparna1
1
answer
The photo electric emission requires a threshold frequency $V_o$. For a certain metal $\lambda_1$ = 2200 $\overset{\circ}{A}$ and $\lambda_2$ = 1900 $\overset{\circ}{A}$ produce electrons with a maximum kinetic energy $KE_1$ and $KE_2$. If $KE_2 = 2KE_1$. Calculate $V_o$ and corresponding $\lambda_o$.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q151
asked
Jan 30, 2014
by
sharmaaparna1
1
answer
To what series does the spectral lines of atomic hydrogen belong if its wave number is equal to the difference between the wave numbers of the following two lines of the Balmer series 486.1 and 410.2 nm?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q150
asked
Jan 28, 2014
by
sharmaaparna1
1
answer
A hydrogen like atom (atomic No. Z) is in a higher excited state of quantam number n. This excited atom can make a transition to the first excited state by successively emitting two photons of energies 10.20 eV and 17.00 eV respectively. alternatively the atom from the same excited state can make a transition to the second excited state by successively emitting two photons of energy 4.25eV and 5.95 eV respectively. Determine the values of n and Z.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
difficult
q148
asked
Jan 28, 2014
by
sharmaaparna1
1
answer
A compound of Vanadium has a magnetic moment of 1.73 Bm. Work out the electric configuration of the Vanadium ion in the compound.
sat
chemistry
atomic-structure
jeemain
physical-chemistry
class11
unit2
quantum-mechanical-model
medium
q147
asked
Jan 28, 2014
by
sharmaaparna1
1
answer
If the electron energy is -3.4 eV , Find the principal quantum number of H-atom?
sat
chemistry
atomic-structure
jeemain
physical-chemistry
class11
unit2
quantum-mechanical-model
medium
q146
asked
Jan 24, 2014
by
sharmaaparna1
1
answer
An ion $Mn^{a+}$ has the magnetic moment equal to 4.9bm. What is the value of a ?
sat
chemistry
atomic-structure
jeemain
physical-chemistry
class11
unit2
quantum-mechanical-model
easy
q144
asked
Jan 24, 2014
by
sharmaaparna1
1
answer
Find out the number of angular nodes in the orbital to which the last electron of Cr enter.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q140
medium
asked
Jan 17, 2014
by
sreemathi.v
1
answer
The magnetic moment of a transition metal ion is $\sqrt{15}$BM.Find out the number of unpaired electrons in it
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q137
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
The maximum kinetic energy of photoelectrons ejected from a metal,when it is irradiated with radiation of frequency $2\times 10^{14}s^{-1}$ is $6.63\times 10^{-20}J$.The threshold frequency of metal is
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q127
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
Photoelectrons are liberated by ultraviolet light of wavelength $3000A^{\large\circ}$ from a metallic surface for which the photoelectric threshold is 4000$A^{\large\circ}$.Calculate De-Broglie wavelength of electrons emitted with maximum kinetic energy.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q126
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
The binding energy of electrons in a metal is 250KJ/mol.What is the threshold frequency of metal ?
sat
chemistry
atomic-structure
jeemain
physical-chemistry
class11
unit2
quantum-mechanical-model
q125
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
The minimum energy required to overcome the attractive forces between electron and the surface of Ag metal is $7.52\times 10^{-19}J$.What will be the maximum kinetic energy of electron ejected out from Ag.Which is being exposed to uv light of $\lambda=360A^{\large\circ}$?
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q123
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
Calculate the uncertainty in velocity of a cricket ball (mass=0.15Kg) if its uncertainty in position is of the order of $1A^{\large\circ}$
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q122
medium
asked
Jan 17, 2014
by
sreemathi.v
1
answer
Energy required to stop the ejection of electrons from $Cu$ plate is 0.24eV.Calculate the work function when radiations of $\lambda=253.7nm$ strikes the plate.
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q121
difficult
asked
Jan 17, 2014
by
sreemathi.v
1
answer
An electron has a total energy of 2MeV.Calculate the effective mass of the electron in Kg and its speed .Assume rest mass of electron 0.511MeV
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q120
difficult
asked
Jan 16, 2014
by
sreemathi.v
1
answer
Two hydrogen atoms collide head on and end up with zero kinetic energy.Each atom then emits a photon of wavelength 121.6nm.Which transition leads to this wavelength ?How fast were the hydrogen atoms traveling before collision?$R_H=1.097\times 10^7m^{-1}$ and $m_H=1.67\times 10^{-27}Kg$
jeemain
chemistry
physical-chemistry
class11
unit2
atomic-structure
quantum-mechanical-model
q119
difficult
asked
Jan 16, 2014
by
sreemathi.v
1
answer
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