7. Explain the trend as you move across a row of the pelotic case for each of sel properties using your understanding of effective nude change a. Atomic radius b. lonization energy/electronegativity
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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**7. Explain the trend as you move across a row of the periodic table for each of the following atomic properties using your understanding of effective nuclear charge.**
a. **Atomic radius**
b. **Ionization energy/electronegativity**
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### Explanation
When discussing the trends in atomic properties across a row of the periodic table, it is essential to understand the concept of effective nuclear charge (Z_eff). Effective nuclear charge is the net positive charge experienced by valence electrons in an atom.
#### a. **Atomic Radius**
As you move from left to right across a period of the periodic table, the atomic radius generally decreases. This trend occurs because:
1. **Increasing Protons:** The number of protons in the nucleus increases, which results in a higher positive charge.
2. **Higher Effective Nuclear Charge:** The increased positive charge pulls the electrons closer to the nucleus.
3. **Same Energy Level:** Electrons are added to the same principal energy level, ensuring they do not shield each other effectively from the nucleus's increasing pull.
Thus, atoms become smaller as the effective nuclear charge increases across a period.
#### b. **Ionization Energy/Electronegativity**
Ionization energy and electronegativity both generally increase as you move from left to right across a period. This trend can be explained by considering the following points:
- **Ionization Energy:** The energy required to remove an electron from an atom in its gaseous state. As you move across the period, the effective nuclear charge increases, making it more difficult to remove an electron due to the stronger attraction between the electrons and the nucleus.
- **Electronegativity:** The tendency of an atom to attract electrons towards itself in a chemical bond. With an increasing effective nuclear charge, atoms more strongly attract bonding electrons.
By understanding these trends, one can predict and rationalize the chemical behavior of different elements in the periodic table.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F31367867-84a4-4184-a2ca-45c4adf73bec%2Fa310d27c-0b43-4070-8505-ccd5a7101587%2F87citc_processed.jpeg&w=3840&q=75)
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