The radius of the second Bohr orbit for hydrogen atom is-Planck-s constant h - 6-6262 - 10-34 Js- mass of an electron - 9-1091 - 10-31 kg- charge of an electrone - 1-60210 - 10-19 C- permittivity of vacuum -8-854185 - 10-12 kg-1 m-3 A2

R_n=0.53n^2/Z∘A n=2 Z=1 r_2=0.53 × 4∘A=2.12 ∘A ...

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Byju's Answer

Standard XI

Chemistry

Bohr's Model of a Hydrogen Atom

The radius of...

Question

The radius of the second Bohr orbit for hydrogen atom is:
(Planck’s constant $h = 6.6262 \times 10^{- 34} J s$ ; mass of an electron $= 9.1091 \times 10^{- 31} k g$ ; charge of an electron
$e = 1.60210 \times 10^{- 19} C$ ; permittivity of vacuum $ϵ_{ϕ} = 8.854185 \times 10^{- 12} k g^{- 1} m^{- 3} A^{2})$

4.76 \circ A

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0.529 \circ A

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2.12 \circ A

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1.65 \circ A

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Solution

The correct option is C $2.12 \circ A$
$r_{n} = \frac{0.53 n^{2}}{Z} \circ A$

$n = 2$

$Z = 1$

$r_{2} = 0.53 \times 4 \circ A = 2.12 \circ A$

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Q. The radius of the second Bohr orbit for hydrogen atom is:
(Planck’s constant

h = 6.6262 \times 10^{- 34} J s

; mass of an electron

= 9.1091 \times 10^{- 31} k g

; charge of an electron

e = 1.60210 \times 10^{- 19} C

; permittivity of vacuum

ϵ_{ϕ} = 8.854185 \times 10^{- 12} k g^{- 1} m^{- 3} A^{2})

The radius of the second Bohr orbit for hydrogen atom is:
(Plank’s const. H = 6.6262 x $10^{- 34}$ Js; mass of electron = 9.1091 x $10^{- 31}$ kg; charge of electron e = 1.60210 x $10^{- 19}$ C; permittivity of vaccum $ϵ_{0} = 8.854185 \times 10^{- 12} k g^{- 1} m^{- 3} A^{2})$