What quality of electrons determine whether or not an electron will either pair up with another or be able to be shared between
covalently bonded atoms
1 answer:
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<u>Answer:</u>
<u>Bohr's Model postulates-</u>
I postulate - The electrons in an atom orbit around the nucleus in definite circular paths called orbits or shells.
II Postulate - Each shell or orbit represents a specific amount of energy.
III Postulate - By emitting or absorbing energy, an electron may shift from one stationary energy orbit to another.
<u>Three main Limitations -</u>
1- It adjusts to the hydrogen atom's spectrum but not to the spectra of other atoms.
2 - In the definition of the electron as a tiny particle that spins around the atomic nucleus, the wave properties of the electron are not described.
3- Bohr is unable to understand why classical electromagnetism is inapplicable to his model. That is why, when electrons are in a stationary orbit, they do not emit electromagnetic radiation.
Explanation:
<u>About Bohr's postulates-</u>
1 - The electron spins in circling circles around the nucleus, emitting no energy. The orbital angular momentum is constant in these orbits.
Only certain radii of orbits, corresponding to certain given energy levels, are required for electrons in an atom.
2- Not every orbit is possible. However, whenever an electron is in a legal orbit, it is in a state of unique and constant energy and does not emit energy (stationary energy orbit).
<u>For example -</u> The energies allowed for electrons in the hydrogen atom are given by the following equation: The Rydberg constant for the hydrogen atom is in this equation, and n = quantum number will range from 1 to ∞. For each of the values of n, the electron energies of a hydrogen atom produced by the above equation are negative. As n rises, the energy becomes less negative and thus rises.
3- By emitting or absorbing energy, an electron may shift from one stationary energy orbit to another.
The energy difference between the two states would be equal to the energy released or consumed. This energy E is in the form of a photon, and it can be measured using the following formula:
E is the energy (absorbed or emitted) in this equation, and h is the Planck constant (its value is ) and v denotes the frequency of light, which is calculated in 1/ s.
Answer:
14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.
Explanation:
The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to Q = m*L, where L is called the latent heat of the substance and depends on the type of phase change.
During the evaporation process, a substance goes from a liquid to a gaseous state and needs to absorb a certain amount of heat from its immediate surroundings, which results in its cooling. The heat absorbed is called the heat of vaporization.
So, it is called "heat of vaporization", the energy required to change 1 gram of substance from a liquid state to a gaseous state at the boiling point.
In this case, being:
- Q=?
- m= 172 g
- L= 84
and replacing in the expression Q = m*L you get:
Q=172 g*84
Q=14,448 J
<u><em>14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.</em></u>