Bohr’s atomic model, quantum numbers

In accordance with Hund’s rule, Every orbital in the sub level is singly occupied prior to the double occupancy of any orbital in the sub level. In order to maximise total spin, all electrons in a single occupancy orbital must have the same spin as one another. An electron will not pair with another electron […]

Latest: NEET 2024 Paper Analysis Recommended: NEET Rank Predictor 2024 See more: NEET Result 2024 The number of electrons present in each subshell surrounding the nucleus of an atom is represented by its electronic configuration. The orbitals are denoted by the letters s, p, d, and f, and the maximum number of electrons present in these orbitals is

A diagrammatic depiction of the three-dimensional configurations of component particles in a crystal, known as the crystal lattice, in which each constituent particle is shown as a point in space. There is extremely little room between the atoms that make up a crystal lattice because the atoms are packed so closely together in the lattice.

The group 18 elements include helium, argon, krypton, neon, xenon, and radon. In the outermost orbit, the members of the group possess eight electrons. However, helium has only two electrons.  Group 18 elements are chemically unreactive and are gases that do not form compounds. They are located in the extreme right of the periodic table

The azimuthal quantum number is a quantum number that characterises the form of an atomic orbital and defines its orbital angular momentum. The azimuthal quantum number is the second in a series of quantum numbers that describe an electron’s distinct quantum state (the others being the principal quantum number, the magnetic quantum number, and the

Atomic Number Definition An atom consists of protons, neutrons, and electrons. While electrons revolve around the nucleus, protons and neutrons are inside the nucleus. The number of protons in an atom determines its atomic number. Every atom of an element has the same number of protons and hence the same atomic number. In other words,

The p-Block elements of the periodic table have six subgroups. Boron, carbon, nitrogen, oxygen, fluorine and helium are the names of the subgroups. In all of these elements, the shells of three p-orbitals are entered by the last electron. Except for Helium, the general configuration is ns2np1-6. The first element of the group is Boron.

Introduction Bohr adapted the idea of planetary electron mobility in order to make the model match the regular patterns (spectral series) of light emitted by real hydrogen atoms. Bohr was able to explain the series of discrete wavelengths in the hydrogen emission spectrum by restricting the circling electrons to a series of circular orbits with

Electron configuration describes the distribution of electrons within atoms and molecules among various orbitals (including shells and subshells). There are four principle orbitals (s, p, d, and f) that are filled based on the element’s energy level and valence electrons. Each of the four orbitals can accommodate a different number of electrons. The s-orbital can

The electron is less securely bonded to the nucleus as ‘n’ grows. Higher n distances the electron from the nucleus. There are n recognised l (azimuthal) values ranging from 0 to n-1, therefore higher-n electron states are more common. Each n-shell may hold up to 2n2 electrons with two spin states. As seen in the