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CHXI02:STRUCTURE OF ATOM

307134 An electron in hydrogen like species jumps in such a way that its kinetic energy changes from x to $\frac{x}{4} .$ The change in potential energy will be:

1

+ \frac{3}{2} x

2

- \frac{3}{8} x

3

+ \frac{3}{4} x

4

- \frac{3}{4} x

Explanation:

$∵ PE = - 2K .E .$
When, $K . E . = x, P . E . = - 2 x$
and when, $K . E . = \frac{x}{4}, P . E . = - 2 (\frac{x}{4})$
$= - \frac{x}{2}$
$∴$ Change in $P . E . = - \frac{x}{2} - (- 2 x)$
$= \frac{3}{2} x$

CHXI02:STRUCTURE OF ATOM

307135 The energy of an electron in first Bohr orbit of H-atom is 13.6 eV. The energy value of electron in the excited state of $L i^{2 +}$ is:

1

- 27 .2 e V

2

30 .6 e V

3

- 30 .6 e V

4

27 .2 e V

Explanation:

For $L i^{2 +}$ ion,
$E = - 13 .6 \times \frac{Z^{2}}{n^{2}} = - 13 .6 \times \frac{{(3)}^{2}}{{(2)}^{2}} = \frac{- 13 .6 \times 9}{4}$
$= - 30 .6 e V$

JEE - 2014

CHXI02:STRUCTURE OF ATOM

307136 The energy of an electron in the first Bohr orbit of hydrogen atom is $- 2.18 \times 10^{- 18} J$ . Its energy in the third Bohr orbit is

1

\frac{1}{27}

of this value

2

\frac{1}{9}

of this value

3 three times of this value

4 one third of this value

Explanation:

$E_{n} = - \frac{2.18 \times 10^{- 18}}{n^{2}}$ Joule
For $3^{rd}$ orbit, $E_{3} = - \frac{2.18 \times 10^{- 18}}{(3)^{2}} = - \frac{2.18 \times 10^{- 18}}{9} = \frac{E_{1}}{9}$

JEE - 2023

CHXI02:STRUCTURE OF ATOM

307137 The ground state energy of hydrogen atom is -13.6 eV . The energy of first excited state of ${Li}^{2 +}$ ion in eV is

1

-

3.4 eV

2

-

13.6 eV

3

-

25 eV

4

-

30.60 eV

Explanation:

$En = - 13.6 \times \frac{Z^{2}}{n^{2}} eV$
$= - 13.6 \times \frac{3^{2}}{{(2)}^{2}} e V$
$= \frac{- 13.6 \times 9}{4} eV = - 30.60 eV$

CHXI02:STRUCTURE OF ATOM

307134 An electron in hydrogen like species jumps in such a way that its kinetic energy changes from x to $\frac{x}{4} .$ The change in potential energy will be:

1

+ \frac{3}{2} x

2

- \frac{3}{8} x

3

+ \frac{3}{4} x

4

- \frac{3}{4} x

Explanation:

$∵ PE = - 2K .E .$
When, $K . E . = x, P . E . = - 2 x$
and when, $K . E . = \frac{x}{4}, P . E . = - 2 (\frac{x}{4})$
$= - \frac{x}{2}$
$∴$ Change in $P . E . = - \frac{x}{2} - (- 2 x)$
$= \frac{3}{2} x$

CHXI02:STRUCTURE OF ATOM

307135 The energy of an electron in first Bohr orbit of H-atom is 13.6 eV. The energy value of electron in the excited state of $L i^{2 +}$ is:

1

- 27 .2 e V

2

30 .6 e V

3

- 30 .6 e V

4

27 .2 e V

Explanation:

For $L i^{2 +}$ ion,
$E = - 13 .6 \times \frac{Z^{2}}{n^{2}} = - 13 .6 \times \frac{{(3)}^{2}}{{(2)}^{2}} = \frac{- 13 .6 \times 9}{4}$
$= - 30 .6 e V$

JEE - 2014

CHXI02:STRUCTURE OF ATOM

307136 The energy of an electron in the first Bohr orbit of hydrogen atom is $- 2.18 \times 10^{- 18} J$ . Its energy in the third Bohr orbit is

1

\frac{1}{27}

of this value

2

\frac{1}{9}

of this value

3 three times of this value

4 one third of this value

Explanation:

$E_{n} = - \frac{2.18 \times 10^{- 18}}{n^{2}}$ Joule
For $3^{rd}$ orbit, $E_{3} = - \frac{2.18 \times 10^{- 18}}{(3)^{2}} = - \frac{2.18 \times 10^{- 18}}{9} = \frac{E_{1}}{9}$

JEE - 2023

CHXI02:STRUCTURE OF ATOM

307137 The ground state energy of hydrogen atom is -13.6 eV . The energy of first excited state of ${Li}^{2 +}$ ion in eV is

1

-

3.4 eV

2

-

13.6 eV

3

-

25 eV

4

-

30.60 eV

Explanation:

$En = - 13.6 \times \frac{Z^{2}}{n^{2}} eV$
$= - 13.6 \times \frac{3^{2}}{{(2)}^{2}} e V$
$= \frac{- 13.6 \times 9}{4} eV = - 30.60 eV$

CHXI02:STRUCTURE OF ATOM

307134 An electron in hydrogen like species jumps in such a way that its kinetic energy changes from x to $\frac{x}{4} .$ The change in potential energy will be:

1

+ \frac{3}{2} x

2

- \frac{3}{8} x

3

+ \frac{3}{4} x

4

- \frac{3}{4} x

Explanation:

$∵ PE = - 2K .E .$
When, $K . E . = x, P . E . = - 2 x$
and when, $K . E . = \frac{x}{4}, P . E . = - 2 (\frac{x}{4})$
$= - \frac{x}{2}$
$∴$ Change in $P . E . = - \frac{x}{2} - (- 2 x)$
$= \frac{3}{2} x$

CHXI02:STRUCTURE OF ATOM

307135 The energy of an electron in first Bohr orbit of H-atom is 13.6 eV. The energy value of electron in the excited state of $L i^{2 +}$ is:

1

- 27 .2 e V

2

30 .6 e V

3

- 30 .6 e V

4

27 .2 e V

Explanation:

For $L i^{2 +}$ ion,
$E = - 13 .6 \times \frac{Z^{2}}{n^{2}} = - 13 .6 \times \frac{{(3)}^{2}}{{(2)}^{2}} = \frac{- 13 .6 \times 9}{4}$
$= - 30 .6 e V$

JEE - 2014

CHXI02:STRUCTURE OF ATOM

307136 The energy of an electron in the first Bohr orbit of hydrogen atom is $- 2.18 \times 10^{- 18} J$ . Its energy in the third Bohr orbit is

1

\frac{1}{27}

of this value

2

\frac{1}{9}

of this value

3 three times of this value

4 one third of this value

Explanation:

$E_{n} = - \frac{2.18 \times 10^{- 18}}{n^{2}}$ Joule
For $3^{rd}$ orbit, $E_{3} = - \frac{2.18 \times 10^{- 18}}{(3)^{2}} = - \frac{2.18 \times 10^{- 18}}{9} = \frac{E_{1}}{9}$

JEE - 2023

CHXI02:STRUCTURE OF ATOM

307137 The ground state energy of hydrogen atom is -13.6 eV . The energy of first excited state of ${Li}^{2 +}$ ion in eV is

1

-

3.4 eV

2

-

13.6 eV

3

-

25 eV

4

-

30.60 eV

Explanation:

$En = - 13.6 \times \frac{Z^{2}}{n^{2}} eV$
$= - 13.6 \times \frac{3^{2}}{{(2)}^{2}} e V$
$= \frac{- 13.6 \times 9}{4} eV = - 30.60 eV$

CHXI02:STRUCTURE OF ATOM

307134 An electron in hydrogen like species jumps in such a way that its kinetic energy changes from x to $\frac{x}{4} .$ The change in potential energy will be:

1

+ \frac{3}{2} x

2

- \frac{3}{8} x

3

+ \frac{3}{4} x

4

- \frac{3}{4} x

Explanation:

$∵ PE = - 2K .E .$
When, $K . E . = x, P . E . = - 2 x$
and when, $K . E . = \frac{x}{4}, P . E . = - 2 (\frac{x}{4})$
$= - \frac{x}{2}$
$∴$ Change in $P . E . = - \frac{x}{2} - (- 2 x)$
$= \frac{3}{2} x$

CHXI02:STRUCTURE OF ATOM

307135 The energy of an electron in first Bohr orbit of H-atom is 13.6 eV. The energy value of electron in the excited state of $L i^{2 +}$ is:

1

- 27 .2 e V

2

30 .6 e V

3

- 30 .6 e V

4

27 .2 e V

Explanation:

For $L i^{2 +}$ ion,
$E = - 13 .6 \times \frac{Z^{2}}{n^{2}} = - 13 .6 \times \frac{{(3)}^{2}}{{(2)}^{2}} = \frac{- 13 .6 \times 9}{4}$
$= - 30 .6 e V$

JEE - 2014

CHXI02:STRUCTURE OF ATOM

307136 The energy of an electron in the first Bohr orbit of hydrogen atom is $- 2.18 \times 10^{- 18} J$ . Its energy in the third Bohr orbit is

1

\frac{1}{27}

of this value

2

\frac{1}{9}

of this value

3 three times of this value

4 one third of this value

Explanation:

$E_{n} = - \frac{2.18 \times 10^{- 18}}{n^{2}}$ Joule
For $3^{rd}$ orbit, $E_{3} = - \frac{2.18 \times 10^{- 18}}{(3)^{2}} = - \frac{2.18 \times 10^{- 18}}{9} = \frac{E_{1}}{9}$

JEE - 2023

CHXI02:STRUCTURE OF ATOM

307137 The ground state energy of hydrogen atom is -13.6 eV . The energy of first excited state of ${Li}^{2 +}$ ion in eV is

1

-

3.4 eV

2

-

13.6 eV

3

-

25 eV

4

-

30.60 eV

Explanation:

$En = - 13.6 \times \frac{Z^{2}}{n^{2}} eV$
$= - 13.6 \times \frac{3^{2}}{{(2)}^{2}} e V$
$= \frac{- 13.6 \times 9}{4} eV = - 30.60 eV$