Energy level
The nucleus has a width on the order of 10^(-15) meters, while an electron is (on average) a distance of 10^(-10) meters from the nucleus. If you were to magnify the nucleus to the size of a baseball, the electrons would be orbiting at a distance of around 1000 meters. That is, there are about 50,000-100,000 nucleus diameters to the electron's average radius.
shell
Because if the radius is big, then the large distance affects the strenght of the electron with the nucleus. This also increases reactivity in non metals since it will be easier to take away the electron :)
As an electron moves farther from the nucleus, its energy increases. This increase in energy results in the electron being in a higher energy level or orbital. The electron's increasing distance from the nucleus leads to decreased attraction, causing it to have more potential energy.
Nucleus exerts a force on every electron revolving around it. This force is inversely proportional to the distance between the nucleus and the electron. Therefore the electrons in outermost orbit (or shell) have the least nucleic forceacting upon them in comparison to the inner electrons. Therefore they are the most easily removable electrons.They are called valence electrons.
The force between the nucleus and the outermost electron in a large atom is primarily governed by the attraction between the positively charged nucleus and the negatively charged electron. This force is known as the electrostatic force of attraction and is directly proportional to the product of the charges and inversely proportional to the square of the distance between the nucleus and the electron.
It would not depend on the direction with respect to the nucleus. The direction of the electron has no effect on the distance of the electron from the nucleus.
The approximate distance an electron is located from the nucleus is measured by the concept of electron cloud or electron probability density. This concept is utilized in quantum mechanics to describe the distribution of the electron's probable locations within an atom.
The nucleus has a width on the order of 10^(-15) meters, while an electron is (on average) a distance of 10^(-10) meters from the nucleus. If you were to magnify the nucleus to the size of a baseball, the electrons would be orbiting at a distance of around 1000 meters. That is, there are about 50,000-100,000 nucleus diameters to the electron's average radius.
In an s orbital, the probability of finding an electron at a particular distance from the nucleus does not depend on the direction in which the distance is measured or the orientation of the orbital. This is because s orbitals are spherically symmetric, meaning the electron has an equal likelihood of being found at any distance from the nucleus in all directions.
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The path of a given electron's orbit around a nucleus, marked by a constant distance from the nucleus.
The electron shell is an energy level represented as the distance of an electron from the nucleus of the atom
The distance of the electron cloud from the nucleus affects the atom's stability. When the electron cloud is closer to the nucleus, the atom is more stable. This is because the positively charged nucleus and negatively charged electrons are closer together, creating a stronger attraction. Conversely, if the electron cloud is further from the nucleus, the atom is less stable as the attraction between the nucleus and electrons is weaker.