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Recent questions and answers in Atomic Structure

Questions >> JEEMAIN and NEET >> Chemistry >> Atomic Structure

An ion $Mn^{a+}$ has the magnetic moment equal to 4.9bm. What is the value of a ?

answered Jul 30, 2018 by meena.p

1 answer

Calculate the energy emitted when electrons of 1.0g atom of hydrogen under go transition giving the spectral lines of lowest energy in the visible region of its atomic spectra.$R_H=1.1\times 10^7m^{-1},c=3\times 10^8msec^{-1}$ and $h=6.62\times 10^{-34}Jsec$

answered Jul 6, 2016 by mandarkulkarni11

2 answers

If electron, hydrogen, helium and neon nuclei are all moving with the velocity of light, then the wavelengths associated with these particles are in the order

answered Jan 18, 2016 by meena.p

1 answer

STATEMENT-1 : In reaction, $MnO_4^{–}+5Fe^{2+} 8H^{+} Mn^{2+} + 5Fe^{3+} + 4H_2O, MnO_4^{–}$ acts as oxidising agent. STATEMENT-2 : In the above reaction, $Fe^{2+}$ is converted

answered Jan 18, 2016 by meena.p

1 answer

In the cathode ray experiment how low pressure can increase the space between the atoms of the gas?

answered Dec 22, 2014 by vijayalakshmi.r

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 orbital angular momentum quantum number of the state $S_2$ is

answered 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. Energy of the state $S_1$ in units of the hydrogen atom ground state energy is

answered 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

answered 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:

answered 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

answered 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 binding energy of electron in a metal is 250 KJ/mol. The threshold frequency of metal is

answered 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. With what potential should a beam of electron be accelerated So that its wavelength becomes equal to $1.54A^{\large\circ}$

answered 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

answered 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 $\lambda = 5200A^{\large\circ}$

answered Feb 9, 2014 by sharmaaparna1

1 answer

An oil drop has $-6.39\times10^{-19}$ coulomb charge .The number of electrons in this oil drop is

answered 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:

answered 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....

answered 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: $Cu^+ or Cu^{2+} and Fe^{2+} or Fe^{3+}$

answered 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

answered 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:

answered 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.

answered 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

answered 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.

answered 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. Then the volume occupied by the nucleus is about .....times of volume of atom.

answered 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

answered Feb 8, 2014 by sharmaaparna1

1 answer

Calculate the shortest and longest wavelength in H spectrum of Lyman series. $R_H = 109678 cm^{-1}$

answered Feb 7, 2014 by sharmaaparna1

1 answer

If the radius of first Bohr orbit of hydrogen atom is 'x' then de Broglie wavelength of electron in $3^{rd}$ Orbit is nearly

answered Feb 7, 2014 by sharmaaparna1

1 answer

How many times does light travel faster in vaccum than an electron in Bohr first orbit of hydrogen atom?

answered Feb 7, 2014 by sharmaaparna1

1 answer

Imagine an atom made up of proton and a hypothetical particle of double the mass of electron but having the same charge as the electron . Apply the Bohr's atomic model and consider all possible transitions of this hypothetical particle to the first excited level. The largest wavelength photon that will be emitted has wavelength $\lambda$ (given in terms of the Rydberg constant R for the hydrogen atom) equal to.

answered Feb 7, 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

answered Feb 7, 2014 by sharmaaparna1

1 answer

When a hydrogen atom emits a photon of energy 12.1eV, the orbital angular momentum changes by

answered Feb 7, 2014 by sharmaaparna1

1 answer

What is the ratio of the Rydberg constant for helium to hydrogen atom?

answered Feb 6, 2014 by sharmaaparna1

1 answer

What is energy per mol of photons of FM radiowaves with V=102.5 MHZ ?

answered 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?

answered 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

answered 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?

answered 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$S^{-1}$)

answered 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.

answered Feb 5, 2014 by sharmaaparna1

1 answer

Calculate the wavelength of the first line and the series limit for the Lyman series for hydrogen.(Series limit is for the case when $n_2 = \infty)$

answered 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)

answered 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?

answered 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?

answered 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.

answered 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 $(rms = \sqrt{3RT/m})$

answered 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?

answered Feb 4, 2014 by sharmaaparna1

1 answer

AIR services on vividh Bharti is transmitted on 219m band.What is its transmission frequency in Hertz.

answered 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.

answered 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.

answered 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 ?

answered 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

answered Feb 1, 2014 by sharmaaparna1

1 answer

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