ENERGY LEVEL

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Energy levels

• Bigger Orbit = Higher Energy• Smaller Orbit=Less Energy

Electrons in atoms can occupy many different energy levels. The further away an energy level is from the nucleus, the higher its energy. So an electron occupying energy level E4 in this picture, would have a higher energy than an electron occupying any of the other three energy levels.

When an electron moves from a higher energy level to a lower energy level, a

photon (particle of light) is emitted. Light emitted this way (from movement of

charged particles) is called radiation. A photon of light is depicted as a squiggly

line with an arrow on one end, as in this picture.

When an electron moves from a higher energy level to a lower energy level, a photon (particle of light) is emitted. Light emitted this way (from movement of charged particles) is called radiation. A photon of light is depicted as a squiggly line with an arrow on one end.

energy leveln Physics1. (Physics / General Physics) a constant value of energy in the distribution of energies among a number of atomic particles2. (Physics / General Physics) the energy of a quantum state of a system. The terms energy level and energy state are often used loosely to mean quantum state. This is avoided in precise communication

Electrons in an atom are contained in specific energy levels (1, 2, 3, and so on) that are different distances from the nucleus. The larger the number of the energy level, the farther it is from the nucleus. Electrons that are in the highest energy level are called valence electrons. Within each energy level is a volume of space where specific electrons are likely to be located. These spaces, called orbitals, are of different shapes, denoted by a letter (s, p, d, f, g). (In most cases, only the electrons contained in the s and p orbitals are considered valence electrons.) Electrons seek the lowest energy level possible.

The following electron-filling pattern indicates how the electrons fill into the energy levels. Knowing this pattern is useful in many aspects of chemistry, including predicting the bonding situation of a particular atom and in the prediction of the geometry of a covalent compound.

Electron filling pattern: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f