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.
I only need help with the highlighted ones please :)
![### Phosphate Ion (PO₄³⁻) Structure and Questions
#### Structure Explanation
The structure of the phosphate ion (PO₄³⁻) is depicted with phosphorus (P) at the center, bonded to four oxygen (O) atoms. One of these oxygen atoms is double-bonded to phosphorus, while the other three are single-bonded with three extra electrons shown as dots. The ion carries an overall charge of 3-.
#### Questions
**i. Why can phosphorus have more than 8 electrons?**
Phosphorus can have more than 8 electrons because it is in the third period of the periodic table, where elements are capable of expanding their valence shells using d-orbitals. This allows phosphorus to accommodate more than eight electrons, unlike elements in the second period.
**ii. As drawn, what is the molecular geometry?**
The molecular geometry of the phosphate ion, as drawn, is tetrahedral. This is due to the four regions of electron density around the central phosphorus atom, consisting of one double bond and three single bonds with oxygen atoms.
**iii. Do you predict that all bond angles in the ion are equal? Briefly explain.**
Yes, in a tetrahedral geometry, all bond angles are predicted to be equal, typically around 109.5°. This is due to the symmetrical arrangement of the bonds around the central phosphorus atom.
**iv. Do you predict that all bond lengths in the ion are equal? Briefly explain.**
No, not all bond lengths in the ion are predicted to be equal. The bond with the double-bonded oxygen will be shorter than the bonds with the single-bonded oxygens, due to the stronger double bond which pulls the atoms closer together compared to single bonds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbf5f188-ec82-4083-8d7c-ea618d5be715%2Ff7d80918-15cc-4a9d-9994-6ae721fdd981%2Fr3pdwgb_processed.png&w=3840&q=75)
![](/static/compass_v2/shared-icons/check-mark.png)
Step by step
Solved in 3 steps with 1 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
![Living by Chemistry](https://www.bartleby.com/isbn_cover_images/9781464142314/9781464142314_smallCoverImage.jpg)
![Introductory Chemistry: An Active Learning Approa…](https://www.bartleby.com/isbn_cover_images/9781305079250/9781305079250_smallCoverImage.gif)
![Living by Chemistry](https://www.bartleby.com/isbn_cover_images/9781464142314/9781464142314_smallCoverImage.jpg)
![Introductory Chemistry: An Active Learning Approa…](https://www.bartleby.com/isbn_cover_images/9781305079250/9781305079250_smallCoverImage.gif)
![Chemistry for Today: General, Organic, and Bioche…](https://www.bartleby.com/isbn_cover_images/9781305960060/9781305960060_smallCoverImage.gif)
![Introductory Chemistry: A Foundation](https://www.bartleby.com/isbn_cover_images/9781337399425/9781337399425_smallCoverImage.gif)