Recent questions tagged atomic-structure

Which one of the following statements are always true for neutral atoms

asked Jul 18, 2018 by swapnarajan1982

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A 1 MeV proton is sent against a gold leaf (Z = 79). Calculate the distance of closest approach for head on collision.

asked Jul 18, 2018 by swapnarajan1982

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Calculate the ratio of K.E and P.E of an electron in an orbit?

asked Jul 18, 2018 by swapnarajan1982

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An orbital may never be occupied by

asked Jul 17, 2018 by swapnarajan1982

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The sublevel that can be occupied by a maximum of 10 electrons is identified by the letter

asked Jul 17, 2018 by swapnarajan1982

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The sublevel that has only one orbital is identified by the letter

asked Jul 17, 2018 by swapnarajan1982

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The lowest principal quantum number that an electron can have is

asked Jul 17, 2018 by swapnarajan1982

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The two main regions of an atom are the

asked Jul 17, 2018 by swapnarajan1982

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Discovery of the nucleus of an atom was due to the experiment carried out by

asked Jul 17, 2018 by swapnarajan1982

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The ratio of the energy of a photon of 2000A wavelength radiation to that of 4000A radiation is

asked Jul 17, 2018 by swapnarajan1982

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Atoms consists of protons, neutrons and electrons. If the mass of neutrons and electrons were made half and two times respectively to their actual masses, then the atomic mass of ${_6}C^{12}$

asked Jul 17, 2018 by swapnarajan1982

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What is the wavelength associated with 150 eV electron

asked Jul 17, 2018 by swapnarajan1982

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In an alpha scattering experiment, few alpha particles rebounded because

asked Jul 17, 2018 by sharmaaparna1

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Which of the following ions will have maximum magnetic moment

asked Jul 17, 2018 by sharmaaparna1

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Find Atomic number of element that has electron configuration lasting with $6p^2$

asked Jul 17, 2018 by sharmaaparna1

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Calculate the de Broglie wavelength of an electron moving with a velocity of $5.0\times10^5ms^{–1}$

asked Jul 17, 2018 by swapnarajan1982

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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

asked Jan 18, 2016 by meena.p

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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

asked Jan 18, 2016 by meena.p

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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

asked Feb 10, 2014 by sharmaaparna1

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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

asked Feb 10, 2014 by sharmaaparna1

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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

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:

asked Feb 10, 2014 by sharmaaparna1

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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

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

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

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

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

asked 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

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:

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....

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

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

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:

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.

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

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.

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

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

asked Feb 8, 2014 by sharmaaparna1

1 answer

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

asked 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

asked Feb 7, 2014 by sharmaaparna1

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

asked 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.

asked Feb 7, 2014 by sharmaaparna1

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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

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

asked Feb 7, 2014 by sharmaaparna1

1 answer

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

asked Feb 6, 2014 by sharmaaparna1

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

asked Feb 6, 2014 by sharmaaparna1

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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?

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

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?

asked Feb 6, 2014 by sharmaaparna1

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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$S^{-1}$)

asked Feb 6, 2014 by sharmaaparna1

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