ns and the valence shell. Explain why these act differently? P leus and inner-most electron shell. (Note we will be talking m ittle bit of what ozone is and some historic issues about it.)
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
![6. Özone, which is created when three oxygen atoms are bonded in a molecule, is also found in the
atmosphere. Knowing that a single oxygen atom has two electrons in the shell near the nucleus and six in its
valence, please draw a single oxygen, the most common oxygen molecule found in the air we breathe, and an
ozone molecule. Include the valence electrons and the valence shell. Explain why these act differently? Please
just an "O" (for oxygen) to represent the nucleus and inner-most electron shell. (Note we will be talking more
about the atmosphere first, but please do a little bit of what ozone is and some historic issues about it.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81d66944-82c7-4e04-94d5-cc6a0194fa92%2F794bc163-f803-4183-9e2c-0415727eb52d%2Fw58v8np_processed.jpeg&w=3840&q=75)
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