The color of an object, the atom releasing the photon back I have a question about why the color of an object is as it is. This is something I am wondering about after watching episode 5 of the tv-series Cosmos from 2014.
From what I understand a blue object abosrbs all the colors except blue?
Also from what I understand when an atom absorbs electromagnetic waves (or a photon) with a certain wavelength the electron moves to a higher energy level. But after a while the electron moves back to the lower energy level and when that happens a photon that corresponds to that energy level is released?
So why do we for example on a blue object see only the color that is reflected? Shouldn't we also see the absorbed colors that are released when the electron moves back to the lower energy level?
 A: 
From what I understand a blue object abosrbs all the colors except blue?

Yes, or at least it reflects a range of wavelengths with a strong peak centered around blue.

But after a while the electron moves back to the lower energy level and when that happens a photon that corresponds to that energy level is released?

It emits some form of EM radiation - quite possibly visible light (depends on the atom and energy levels), but the intensity of the radiation is completely drowned out by other light so you can't see it.
If you put a substance that does this in a light-tight box and a light detector (i.e. photomultiplier tube) in it, you will detect the visible light from these atomic transitions. This is called a scintillating detector
A: When an electron moves from a higher energy state to a lower energy state it loses energy in the form of electromagnetic waves.
All objects emit electromagnetic radiation which depend on the body’s temperature. This is called blackbody radiation.
When the temperature of an object is increased it begins to glow ( first red and orange then white and blue as the temperature is progressively increased).
When a body is cool and when we do not see a glow at all it is still constantly emitting radiation that is mostly in the infrared region.
Night vision equipment allows us to see objects in the dark as they are emitting radiation in the infrared zone.
In short the radiation emitted may consist of various components having different wavelengths.
The spectrum of waves obtained might not all be in the visible range.
EDIT:
While getting excited the electron absorbs only one quantum of energy and gets excited to a higher energy level depending upon the energy of absorbed quanta.
While de excitation the electron eventually reaches the ground state it may do so series and take paths involving intermediate orbits.
Taking these different paths will lead to release of energy or light that is not in the visible spectrum.
For example: An electron de exciting from n=3 or more to n=1 it may get de excited directly to n=1 or it may choose to get de excited in steps like going to n=2 and then to n=1.
Here n is orbit number and n=1 is the ground state. (Check the graph of emission spectrum of hydrogen involving Lyman balmer paschen brackett and pfund series which correspond to ultraviolet, visible and infrared(x3) respectively.)
This de excitation in intermediate steps is probably the reason why we don’t see the red light which you mentioned even after the electron gets de excited to lower states as the energy must be conserved and this may happen when done in steps.
