why do ions emit varying colors when subjected to heat?

Question

why do ions emit varying colors when subjected to heat?
what does it have to do with Neils Bohr's atomic model?

Answer 1

this is because each ions have different energy levels with which the electrons are to be excited, i.e. some has lower excited energy level compared to other as such when the electrons returns to their ground state they will emit the color characteristic of the energy difference of the excited state and the ground state. lower difference means lower energy and the color will be near to red while higher energy means that the energy diffirence is high and that if it is emitted this will corresponds to color near to blue. note that in light spectrum red has the lowest energy while blue has the greatest
with respect to Bohr's model, it only explains that indeed energy is quantized, that is, the energy level has discrete value
see http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

best answer?

Answer 2

The quantum theory was first proposed in 1900 by German physicist Max Planck, to explain the properties of radiation emitted by heated bodies.

As electrons become more "excited" due to an increase in energy, they "jump" to higher energy states. When the electron returns to its "ground state", it gives off a photon of energy. This photon, depending on its frequency and wavelength, is what is responsible for the color generated, and will vary due to a given amount of energy emitted.

The Bohr model of the atom, while easy to understand, is actually quite incorrect as was discovered in the early 20th century. According to the Bohr model, the electrons orbit the nucleus much the same as the planets orbit the sun. The problem with this is that eventually the electrons would run out of energy and crash into the nucleus. Thus was born quantum mechanics in an attempt to derive a more accurate picture.

Simply stated, the electrons travel in a motion that can most easily be represented with an electron density cloud. The highest probability of finding the electron is within the nucleus. As the electron moves further from the nucleus, the probability decreases. Thus, the cloud is darkest in the center and becomes progressively thinner at increasing distances.

Here is a link to an interactive page that you can use to generate electron density clouds.

Answer 3

Rod r has nailed it for you. Also consider than an ion is an atom that has had one or more electrons stripped from it. Atoms of different atomic weights (sum of protons and neutrons in nuclii) have several orbital shells about them some of which man not be full and some of which (at higher energy levels) may be empty. When an atom captures a photon it can kick an electron up to a higher energy orbit; or completely out of all orbits leaving the atom ionized. That is an unstable condition and an electron will enter the atom and in one or more steps move from energetic orbits to the least energetic (rest) orbit and any space that is empty. Each time the electron moves to a less energetic orbit it gives up its excess energy as a photon (moving at the speed of light!). The amount of excess energy that the photon carries establishes its wavelength and thus its color. Short wavelengths (infrared) are less energetic than short wavelengths (ultraviolet and X-rays). Thus a given atom may have many ionized states depending on its temperature and is capable of producing many different colors. A different (larger?) atom will have different sized orbits and states of ionization producing its own unique series of colors (including invisible light!). Therefore spectrometers (special prisims) can be used to analyze light perhaps from a star or our own sun to determine which atoms are there producing light (distinct photons). Helium is named after the sun (Helios) because it was first discovered in the sun's spectrogram (before it was found in gas deposits on earth!).

Answer 4

When any atom, (not just ions), are heated the electrons in the various energy levels are excited. sometimes, the excitation is enough to make them jump from energy level to another higher one. When the electrons jump back down, the photon energy released can be in the optical range. You see it as colours. They are different for different elements. This was first appreciated by Neils Bohr who solved the maths for the Hydrogen atom.

Answer 5

an electron can spring from one potential layer to a diverse, emmiting potential, in form of radiance. this radiance is "seen" to us as shade. in view that each and every electron in each and every atom is unique, any component could supply a diverse flame shade