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GradeIntroduction To Atom Models

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What atomic model is in use today?

When a hydrogen atom is raised from ground state to excited state.

A) Both K.E. and P.E. increases.

B) Both K.E. and P.E. decreases.

C) The P.E. increases and K.E. decreases.

D) The K.E. decreases and P.E. increases.

A) Both K.E. and P.E. increases.

B) Both K.E. and P.E. decreases.

C) The P.E. increases and K.E. decreases.

D) The K.E. decreases and P.E. increases.

(A) Using Bohr’s second postulate of quantization of orbit angular momentum shows that the circumference of the electron in the nth orbital state in hydrogen atom is n times the de-Broglie wavelength associated with it.

(B) The electron in a hydrogen atom initially in the third excited state. What is the maximum number of spectral lines which can be emitted when it finally moves to the ground state?

(B) The electron in a hydrogen atom initially in the third excited state. What is the maximum number of spectral lines which can be emitted when it finally moves to the ground state?

The kinetic energy of the electron in an orbit of radius $r$ in hydrogen atom is ($e = $ electronic charge)

A. $\dfrac{{{e^2}}}{r}$

B. $\dfrac{{{e^2}}}{{2r}}$

C. $\dfrac{{{e^2}}}{{4r}}$

D. $\dfrac{{{e^2}}}{{2{r^2}}}$

A. $\dfrac{{{e^2}}}{r}$

B. $\dfrac{{{e^2}}}{{2r}}$

C. $\dfrac{{{e^2}}}{{4r}}$

D. $\dfrac{{{e^2}}}{{2{r^2}}}$

Derive the expression for total energy of electron in ${n^{th}}$ Bohr orbit and show that ${E_n} \propto \dfrac{1}{{{n^2}}}$

What are the 6 models of the atom?

How did quarks fit into an atomic model?

Using Rutherford’s model of atom, derive the expression for the total energy of the electron in a hydrogen atom. What is the significance of the total negative energy possessed by the electron?

OR

Using Bohr’s postulates of the atomic model derive the expression for the radius of $ nth $ electron orbit. Hence obtain the expression for Bohr radius.

OR

Using Bohr’s postulates of the atomic model derive the expression for the radius of $ nth $ electron orbit. Hence obtain the expression for Bohr radius.

During normal incidence of light:

A. Angle of incidence is ${{90}^{\circ }}$

B. Angle of incidence is ${{0}^{\circ }}$

C. Sum of angle of incidence and angle of reflection is ${{90}^{\circ }}$

D. Angle of incidence is greater than angle of reflection.

A. Angle of incidence is ${{90}^{\circ }}$

B. Angle of incidence is ${{0}^{\circ }}$

C. Sum of angle of incidence and angle of reflection is ${{90}^{\circ }}$

D. Angle of incidence is greater than angle of reflection.

J.J.Thomson’s cathode ray tube experiment demonstrated that:

A. Cathode rays are streams of negatively charged ions

B. All the mass of an atom is essentially in the nucleus

C. The $\dfrac{e}{m}$ of electrons is much greater than the $\dfrac{e}{m}$ of protons.

D. The $\dfrac{e}{m}$ ratio of the cathode ray particles changes when a different gas is placed in the discharged tube.

A. Cathode rays are streams of negatively charged ions

B. All the mass of an atom is essentially in the nucleus

C. The $\dfrac{e}{m}$ of electrons is much greater than the $\dfrac{e}{m}$ of protons.

D. The $\dfrac{e}{m}$ ratio of the cathode ray particles changes when a different gas is placed in the discharged tube.

The radius of the first orbit of hydrogen is ${{r}_{H}}$, and the energy in the ground state is $-13.6eV$. Considering a $\mu -$ particle with a mass $207{{m}_{e}}$ revolving round a proton as in a Hydrogen atom. The energy and radius of proton and $\mu -$ combination respectively in the first orbit are:

[Assume nucleus to be stationary]

(A). $-13.6\times 207eV,\,207{{r}_{H}}$

(B). $-13.6\times 207eV,\dfrac{{{r}_{H}}}{207}$

(C). $207-13.6eV,\,207{{r}_{H}}$

(D). $207-13.6eV,\,\dfrac{{{r}_{H}}}{207}$

[Assume nucleus to be stationary]

(A). $-13.6\times 207eV,\,207{{r}_{H}}$

(B). $-13.6\times 207eV,\dfrac{{{r}_{H}}}{207}$

(C). $207-13.6eV,\,207{{r}_{H}}$

(D). $207-13.6eV,\,\dfrac{{{r}_{H}}}{207}$

Using Bohr’s atomic model, derive an equation for the radius of orbit of an electron.

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