Test: Structure of Atom - 1 - Grade 10 MCQ

The electronic configuration of Ag in the ground state is [Kr]4d¹⁰5s¹.

From the Law of Conservation of energy, the energy of the absorbed photon is equal to the combined energy of two emitted photons.
E_T = E₁ + E₂ – (1)

Here, E₁ is the Energy of the first emitted photon emitted and E₂ is the Energy of the second emitted photon.

Now, E = (hc)/ (λ) – (2)

Substituting values from (2) in (1) we get

(hc/λ_T) = (hc)/ (λ₁) + (hc)/ (λ₂)

Therefore, on solving the equation, we get λ₂ = 742.77nm

K = 19 = 1s²2s²2p⁶3s²3p⁶s¹

3s²3p⁶ = m-shell

Hence, k has only 8 electrons in the M shell.

Electrons having the same orbital are identified by Spin quantum number. Spin Quantum number has two values +1/2 or -½. Spin quantum number explains the direction through which an electron spins in an orbital. An electron in the same orbitals must have opposite spins. 

For a hydrogen atom, the kinetic energy is the negative of the total energy.
The potential energy is twice the total energy.
The first excited state energy of orbital = -3.4 eV
and kinetic energy of same orbital = -(-3.4 eV) = 3.4 eV
Therefore, the kinetic energy of the same orbit of a hydrogen atom is 3.4 eV.

n = 6, l = 2, therefore 6d will have 5 orbitals.
Hence maximum of 10 electrons can be accommodated as each orbital can have a maximum of 2 electrons.

The representation of the Schrodinger wave function is given by Ψn, l, m. Therefore by comparing Ψn,l,m and Ψ3, 1, 0 we get that n = 3, l = 1, and m=0. Here n, l, and m are principal, azimuthal, and magnetic quantum numbers respectively.

The set of quantum numbers n = 1, l = 2, m = 0, s = 1/2, is not valid because the value of the azimuthal quantum number should lie only in between 0 and n-1, where n is a principal quantum number. So the above set of quantum numbers is not valid.

The magnetic quantum of orbital ranges from -( l–1) to l–1. Its symbol is given by m. For 2p orbital, there are 3 magnetic quantum numbers namely -1, 0, and 1. For 2pz orbital it's 0, taking that z is the internuclear axis.

Isobar is any member of a group of atomic or nuclear species all of which have the same mass number—that is, the same total number of protons and neutrons. Thus, they are isobars.