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The energy of 1^{st} orbit in a hydrogen atom __________
The energy of an nth orbit in a hydrogen atom is given by the formula E_{n} = R_{H}/n^{2}, where is the energy of nth orbit and R_{H} is the Rydberg constant. The energy of 1^{st} orbit in a hydrogen atom = 2.18 x 10^{18} J/1 = 2.18 x 10^{18} J.
What’s the radius of 1^{st} orbit of He^{+} atom?
The atomic radius of an atom is given by the formula r_{n} = 52.9n^{2}/Z pm, where r_{n} is the radius of nth orbit of an atom and Z is the atomic number of that atom. For He^{+}, n = 1 and Z =2. Radius = 52.9(1)/2 pm = 0.02645 nm.
Bohr’s model could not explain the ability of atoms to form molecules by ______
Though Bohr’s postulates could explain angular momentum, radius, and energy of an orbit, line spectrum of the hydrogen atom, it also had some drawbacks. Among the drawbacks not able to explain the ability of atoms to form molecules by chemical bonds is also one.
The energy of a hydrogen atom is negative. It means the energy of a hydrogen atom is then that lower than that of a free electron that is at rest. This means the hydrogen atom has negative electronic energy.
We know that linear momentum is given by mv and that angular momentum in Iω; m = mass, v = velocity, r = radius, I = inertia of momentum and w = angular velocity. I =m_{e}r^{2} and ω = v/r and Iω = m_{e}r^{2}v/r = m_{e}vr.
According to Bohr’s postulate, angular momentum is quantized and this is given by the expression m_{e}vr = nh/2π. (n =1, 2, 3….). m_{e}vr is the angular momentum and h is the Planck’s constant. Movement of an electron can only be possible in orbits whose angular momentum is the integral multiple of h/2π
What is the ratio of the atomic radius of the 5^{th} orbit in chlorine atom and 3^{rd} orbit in Helium atom?
The atomic radius of an atom is given by the formula r_{n} = 52.9n^{2}/Z pm, where r_{n} is the radius of nth orbit of an atom and Z is the atomic number of that atom. The ratio of the atomic radius of the 5^{th} orbit in chlorine atom and 3^{rd} orbit in Helium atom is 25/17 : 9/2 = 50 : 153.
Bohr’s model couldn’t explain Zeeman and stark effect.
Yes, it’s a limitation of Bohr’s model that it could not the splitting of spectral lines in the magnetic field that is Zeeman effect and also in the electric field also known as a stark effect. so the above statement is true.
Calculate the wavelength of a photon that traveled from 5^{th} orbit to 2^{nd} orbit.
The energy of an nth orbit in a hydrogen atom is given by the formula E_{n} = R_{H}/n^{2}, where is the energy of nth orbit and R_{H} is the Rydberg constant. E_{5} – E_{2} = 4.58 x 10^{19}J. λ(wavelength) = c(speed of light)h(Planck’s constant)/E = 434nm.
Which of the following is the value for Rydberg constant?
The energy of an nth orbit in a hydrogen atom is given by the formula E_{n} = R_{H}/n^{2}, where is the energy of nth orbit and R_{H} is the Rydberg constant. When experiments were conducted, the product of the energy of nth orbit to the square of n is constant i.e. Rydberg constant.
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