The energy difference between the first two levels of hydrogen atom is $10.2 e V$ . For another element of atomic number $10$ and mass number $20$ , the energy difference between the first two levels will be

2040 e V

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2010 e V

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510 e V

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1020 e V

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Solution

The correct option is D $1020 e V$
Given for $H$ - atom

$E_{2} - E_{1} = 10.2 e V$

$E = \frac{- 13.6}{n^{2}} Z^{2}$

For another element given $Z = 10$ ,

$E_{1} = \frac{- 13.6 \times 10^{2}}{1^{2}} = - 1360 e V$

$E_{2} = \frac{- 13.6 \times 10^{2}}{2^{2}} = - 3.4 \times 100 = - 340 e V$

$∴ E_{2} - E_{1} = - 340 - (- 1360) = 1020 e V$

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The energy difference between the first two levels of hydrogen atom is 10.2 eV. For another element of atomic number 10 and mass number 20, the energy difference between the first two levels will be

The correct option is D 1020 eVGiven for H- atom E2−E1=10.2 eV E=−13.6n2Z2 For another element given Z=10, E1=−13.6×10212=−1360 eV E2=−13.6×10222=−3.4×100=−340 eV ∴E2−E1=−340−(−1360)=1020 eV

The energy difference between the first two levels of hydrogen atom is $10.2 e V$ . For another element of atomic number $10$ and mass number $20$ , the energy difference between the first two levels will be