NEET Chemistry Questions: Structure of Atom

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The number of electrons that can be accommodated in $d_{xy} $ orbital is




The $d_{xy}$ orbital can accommodate a maximum of 2 electrons with opposite spins, following the Pauli exclusion principle. This is true for all the five d-orbitals ($d_{xy}$, $d_{yz}$, $d_{xz}$, $d_{x^2-y^2}$, and $d_{z^2}$).
The electronic configuration of Mn can be written as




No explanation available.
The total number of electrons present in any main energy level can be calculated from




The total number of electrons present in any main energy level (n) can be calculated from the formula 2n^2. This is based on the Aufbau principle, which states that electrons occupy orbitals in the order of increasing energy.
Which of the following statements about quantum numbers is wrong?




No explanation available.
The two electrons have the following sets of quantum numbers . X: 3, 2, -2, + 1/ 2 Y : 3, 0, 0, + 1/2 What is true of the following?




The two sets of quantum numbers X (3, 2, -2, +1/2) and Y (3, 0, 0, +1/2) have different values for the subsidiary quantum number (l) and the magnetic quantum number (m), indicating that they represent electrons with different energy levels and orientations.
If the value of azimuthal quantum number of an electron is 2, then which of the following values of magnetic quantum numbers is not permissible,




The azimuthal quantum number (l) determines the value of the magnetic quantum number (ml) which can range from -l to +l. For l = 2, the possible values of ml are -2, -1, 0, 1, and 2. Therefore, the value of 3 for ml is not permissible.
The fundamental particles which arc responsible for keeping nucleons together is




Mesons are fundamental particles composed of a quark and an antiquark. They are responsible for the strong nuclear force that binds protons and neutrons together in the nucleus, keeping the nucleons together.
The positron is as heavy as




The positron is the antiparticle of the electron, having the same mass as an electron but with a positive charge. It has the same mass as an electron, which is much less than the masses of a neutron, alpha particle, or proton.
Atoms may be regarded as comprising of protons, electrons and neutrons. If the mass attributed to the neutrons were halved and that attributed to electrons were doubled then atomic mass of would




No explanation available.
How many electrons in an atom with atomic number 105 can have (n +l) = 8 ?




The principal quantum number (n) represents the main shell, and the azimuthal quantum number (l) represents the subshell within that main shell. For (n + l) = 8, the possible combinations are: n = 8, l = 0 (s subshell), which can hold 2 electrons, and n = 7, l = 1 (p subshell), which can hold 6 electrons. Together, these can accommodate 2 + 6 = 8 electrons for an atom with atomic number 105.
The size of the nucleus is approximately




No explanation available.
The line spectrum ot two elements is not identical because .




The line spectrum of two elements is not identical because they have different energy level schemes. The electrons in different elements have different energy levels, and transitions between these levels result in the emission or absorption of specific wavelengths of light, giving rise to unique line spectra.
Bohr’s atomic model can explain the spectrum of




Bohr's atomic model can explain the spectrum of atoms or ions which are uni-electron species, such as hydrogen atoms, singly ionized helium (He+), or doubly ionized lithium (Li2+). The model is limited to systems with only one electron orbiting the nucleus.
An atom has 2 K, 8 L, 11 M, 2 N electrons, the total number of s-electrons will be




The given atom has 2 K-shell electrons (1s), 8 L-shell electrons (2s and 2p), 11 M-shell electrons (3s, 3p, and 3d), and 2 N-shell electrons (4s). The total number of s-electrons, which have the spherical distribution, is 2 (1s) + 2 (2s) + 2 (3s) + 2 (4s) = 8.
For a sub-shell with azimuthal quantum number l, the total values of magnetic quantum number m can be related to l as




No explanation available.