Electrons can have only specific energy (corresponding to specific levels), but nothing in between. By changing levels they absorb or emitt energy equal to the difference beteen levels. This particular amount of energy can be observed as monochromatic light, that is light of a particular wavelength (color) that looks like a line on a spectrum. Transition between different levels give several lines on a spectrum.
Electrons are only able to possess quanta of energy.
The sharing of electrons in the outer energy levels of two atoms is called bonding.
That electrons can orbit their nucleus in only certain discrete orbits at certain specific levels of energy
Different atoms have a different number of electrons. This is why they show different spectra.
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The simple (and correct) answer to why molecular absorption of radiant energy is more complex than that of atoms is rooted in the fact that there are more possible allowable energy levelsfor electrons to occupy in a molecule than an atom. Let's look at those persnickety electrons and see what's up.In an atom, there are "some" electrons, and they occupy various energy levels. Because of the nature of atomic structure and the behavior of the electron, these electrons have the "opportunity" to move to higher energy levels if they gain extra energy to do so. But it is very important to note that the electrons can move only to specific energy levels dictated by the atomic and the electron structure in a given atom. It's not a free for all. Now focus on the fact that the electrons can only move if they have the exact amount of energy necessary to get to another higher allowable energy level. That quanta of energy must be "just right" for the electron to respond, "grab" the energy, and change energy levels. And, as stated, there are specific allowable energy levels for the electrons in a given atom. But it's different for molecules.A molecule is made up of atoms, and the atoms bring with them their own allowable energy levels. That does not necessarily mean that a given possible energy level in a given atom is possible in a molecule with that atom in it. This is due to "restrictions" placed on electrons because of chemical bonding and the behavior of electrons of atoms which are bonded. But the presence of two or more atoms in a molecule will "open the door" to more allowable energy levels for the electrons of the atoms in that molecule. And the greater number of allowable energy levels can only be seen in the molecule, and cannot be seen in the sum of the individual allowable energy levels in the constituent atoms.
electrons
no, electrons can
The sharing of electrons in the outer energy levels of two atoms is called bonding.
That electrons can orbit their nucleus in only certain discrete orbits at certain specific levels of energy
Niels BohrNiels Bohr proposed the first model of the atom with distinct energy levels with quantized energies. He proposed this theory based on the spectra of atoms and ions.
Different atoms have a different number of electrons. This is why they show different spectra.
Energy levels
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Vibration is related to energy. Or on a more complex level, atoms posses electrons, which in the bohr model, are at different energy "levels"
The simple (and correct) answer to why molecular absorption of radiant energy is more complex than that of atoms is rooted in the fact that there are more possible allowable energy levelsfor electrons to occupy in a molecule than an atom. Let's look at those persnickety electrons and see what's up.In an atom, there are "some" electrons, and they occupy various energy levels. Because of the nature of atomic structure and the behavior of the electron, these electrons have the "opportunity" to move to higher energy levels if they gain extra energy to do so. But it is very important to note that the electrons can move only to specific energy levels dictated by the atomic and the electron structure in a given atom. It's not a free for all. Now focus on the fact that the electrons can only move if they have the exact amount of energy necessary to get to another higher allowable energy level. That quanta of energy must be "just right" for the electron to respond, "grab" the energy, and change energy levels. And, as stated, there are specific allowable energy levels for the electrons in a given atom. But it's different for molecules.A molecule is made up of atoms, and the atoms bring with them their own allowable energy levels. That does not necessarily mean that a given possible energy level in a given atom is possible in a molecule with that atom in it. This is due to "restrictions" placed on electrons because of chemical bonding and the behavior of electrons of atoms which are bonded. But the presence of two or more atoms in a molecule will "open the door" to more allowable energy levels for the electrons of the atoms in that molecule. And the greater number of allowable energy levels can only be seen in the molecule, and cannot be seen in the sum of the individual allowable energy levels in the constituent atoms.
1. Atoms do not have energy levels unlike particles like electrons etc.2. The lowest energy for atoms will be 0 at absolute zero temp of 0 deg Kelvin.3. For electrons in all atoms lowest energy is that of 2 electrons nearest to the nucleus.
Sodium atoms do have electrons that are arranged in energy levels. The electron configuration of sodium is 1s22s22p63s1.