Let the energy of an nth orbit of H atom be -21.76 × 1019/n2 J . What will be the longest wavelength of energy required to remove an electron from the third orbit?

Question

Let the energy of an nth orbit of H atom be -21.76 × 1019/n2 J . What will be the longest wavelength of energy required to remove an electron from the third orbit? (A)  0.628 nm  (B)  1.326 × 10-7 m  (C)  0.798 pm  (D)  0.821 μ m

Tardigrade Admin · Accepted Answer

En=(-21.76×10-19/n2) J For n = 3 En=(-21.76×10-19/(3)2) =-2.42×10-19 J E=(hc/λ) ⇒ λ=(hc/E) =(6.6×10-34×3×108/2.42×10-19) =8.2×10-7 m =0.82×10-6 m =0.82 μ m

Q. Let the energy of an $n^{t h}$ orbit of $H$ atom be $- 21.76 \times 1 0^{19} / n^{2} J$ . What will be the longest wavelength of energy required to remove an electron from the third orbit?

$0.628 nm$

$1.326 \times 1 0^{- 7} m$

$0.798 p m$

$0.821 μ m$

Q. Let the energy of an nth orbit of H atom be −21.76×1019/n2J . What will be the longest wavelength of energy required to remove an electron from the third orbit?

0.628nm

1.326×10−7m

0.798pm

0.821μm

En​=n2−21.76×10−19​J For n=3 En​=(3)2−21.76×10−19​ =−2.42×10−19J E=λhc​ ⇒λ=Ehc​ =2.42×10−196.6×10−34×3×108​ =8.2×10−7m =0.82×10−6m =0.82μm

Q. Let the energy of an $n^{t h}$ orbit of $H$ atom be $- 21.76 \times 1 0^{19} / n^{2} J$ . What will be the longest wavelength of energy required to remove an electron from the third orbit?

$0.628 nm$

$1.326 \times 1 0^{- 7} m$

$0.798 p m$

$0.821 μ m$