Question

what are shells, subshells, and orbitals in an atom? (explain with the diagram)

Answer 1

The Bohr model is useful to explain the reactivity and chemical bonding of many elements, but it actually doesn’t give a very accurate description of how electrons are distributed in space around the nucleus. Specifically, electrons don’t really circle the nucleus, but rather spend most of their time in sometimes-complex-shaped regions of space around the nucleus, known as electron orbitals. We can’t actually know where an electron is at any given moment in time, but we can mathematically determine the volume of space in which it is most likely to be found—say, the volume of space in which it will spend 90% of its time. This high-probability region makes up an orbital, and each orbital can hold up to two electrons.

So, how do these mathematically defined orbitals fit in with the electron shells we saw in the Bohr model? We can break each electron shell down into one or more subshells, which are simply sets of one or more orbitals. Subshells are designated by the letters  Most of organic chemistry—the chemistry of carbon-containing compounds, which are central to biology—involves interactions between electrons in s and p subshells, so these are the most important subshell types to be familiar with. However, atoms with many electrons may place some of their electrons in d and AND FSHELL Subshells. Subshells d and FSHELL Have more complex shapes and contain five and seven orbitals, respectively.

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