And then, explain why you chose your answer.
B) measure the temperature at noon everyday
P.S This is Science
Decrease, increase and increase I think this is correct
B)the smallest unit of p4
C)the smallest unit of NH3
D)the smallest unit of H2O
Answer:
Explanation:
During an exothermic reaction bonds break and new bonds form and protons and electrons go from a structure of higher potential energy to lower potential energy. During this change, potential energy is converted to kinetic energy, which is the heat released in reactions. In an endothermic reaction the opposite occurs.
B electrons move to higher energy levels
** C electrons are gained by an atom in
D. člectrons fall bàok to lower energy levels
Answer:
option d= electrons fall back to the lower energy levels
Explanation:
Excitation:
When the energy is provided to the atom the electrons by absorbing the energy jump to the higher energy levels. This process is called excitation. The amount of energy absorbed by the electron is exactly equal to the energy difference of orbits.
De-excitation:
When the excited electron fall back to the lower energy levels the energy is released in the form of radiations. this energy is exactly equal to the energy difference between the orbits. The characteristics bright colors are due to the these emitted radiations. These emitted radiations can be seen if they are fall in the visible region of spectrum.
Fluorescence:
In fluorescence the energy is absorbed by the electron having shorter wavelength and high energy usually of U.V region. The process of absorbing the light occur in a very short period of time i.e. 10 ∧-15 sec. During the fluorescence the spin of electron not changed.
The electron is then de-excited by emitting the light in visible and IR region. This process of de-excitation occur in a time period of 10∧-9 sec.
Phosphorescence:
In phosphorescence the electron also goes to the excitation to the higher level by absorbing the U.V radiations. In case of Phosphorescence the transition back to the lower energy level occur very slowly and the spin pf electron also change.
The characteristic color (spectrum) of an element is produced when its electrons fall back to lower energy levels. They absorb energy to jump to a higher level, then emit it in the form of light of a specific wavelength when returning to their original or lower level.
The characteristic bright-line spectrum (color) of an element is produced when electrons fall back to lower energy levels (Option D). This process is part of the quantum mechanical model of the atom, particularly in the field of spectroscopy. Each element possesses unique energy levels. When an electron in an atom absorbs energy, it jumps to a higher energy level. When the electron returns to its original or lower energy level, it emits energy in the form of light of a specific wavelength. This is viewed as a unique color in the spectrum.
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