Analog electronics ppt on Energy Level by beingtopper.com

1. ENERGY LEVEL
Made By:-
AMAR
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2. Energy levels
• Bigger Orbit = Higher Energy
• Smaller Orbit=Less Energy

5. 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.

6. 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.

8. energy level
n Physics
1. (Physics / General Physics) a
constant value of energy in the
distribution of energies among a
number of atomic particles
2. (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

9. 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