The energy required to excite an electron in hydrogen atom to its first excited state is, the frequency of emitted photon due to the given transition is (h = 6.64 × 10-34 Js, 1 eV = 1.6 × 10-19 J)

Question

The energy required to excite an electron in hydrogen atom to its first excited state is, the frequency of emitted photon due to the given transition is (h = 6.64 × 10-34 Js, 1 eV = 1.6 × 10-19 J) (A) 2.46 × 1010Hz (B) 2.46 × 1012Hz (C) 2.46 × 1015Hz (D) 2.46 × 1018Hz

Tardigrade Admin · Accepted Answer

From Bohrâs third postulate of atomic theory the frequency of emitted photon h upsilon = E2 - E1 = 10.2 eV ∴ upsilon = (10.2/h)eV Here, 10.2 ev = 10.2× 1.6 × 10-19 J, h =6.64 × 10-34 J s ∴ upsilon= (10.2× 1.6× 10-19/6.64× 10-34) = 2.46 × 1015 Hz

Q. The energy required to excite an electron in hydrogen atom to its first excited state is, the frequency of emitted photon due to the given transition is
$(h = 6.64 \times 1 0^{- 34} J s, 1 e V = 1.6 \times 1 0^{- 19} J)$

$2.46 \times 1 0^{10} Hz$

$2.46 \times 1 0^{12} Hz$

$2.46 \times 1 0^{15} Hz$

$2.46 \times 1 0^{18} Hz$

Q. The energy required to excite an electron in hydrogen atom to its first excited state is, the frequency of emitted photon due to the given transition is (h=6.64×10−34Js,1eV=1.6×10−19J)

2.46×1010Hz

2.46×1012Hz

2.46×1015Hz

2.46×1018Hz

From Bohr’s third postulate of atomic theory the frequency of emitted photon hυ=E2​−E1​=10.2eV ∴υ=h10.2​eV Here,10.2ev=10.2×1.6×10−19J, h=6.64×10−34Js ∴υ=6.64×10−3410.2×1.6×10−19​ =2.46×1015Hz

Q. The energy required to excite an electron in hydrogen atom to its first excited state is, the frequency of emitted photon due to the given transition is
$(h = 6.64 \times 1 0^{- 34} J s, 1 e V = 1.6 \times 1 0^{- 19} J)$

$2.46 \times 1 0^{10} Hz$

$2.46 \times 1 0^{12} Hz$

$2.46 \times 1 0^{15} Hz$

$2.46 \times 1 0^{18} Hz$