For each molecule, specify the polarity of the bonds and the overall polarity of the molecule. i- Be CI : CI bonds molecule Answer Bank nonpolar HO :O: polar bonds H molecule
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.
![### Understanding Polarity for Molecules
In the image, there are two molecules presented for analysis: beryllium chloride (BeCl₂) and water (H₂O). For each molecule, we will specify the polarity of the bonds and the overall polarity of the molecule.
### Molecule 1: Beryllium Chloride (BeCl₂)
- **Lewis Structure**:
- The central atom is Be (Beryllium), which forms two bonds with two Cl (Chlorine) atoms.
- Each Cl atom has three pairs of lone electrons (represented by dots) and one bonding pair with Be.
- **Polarity of Bonds**:
- Analyze the bonds between Be and Cl. Chlorine is more electronegative than Beryllium, making the Be-Cl bonds polar.
- **Overall Polarity of the Molecule**:
- Consider the molecular geometry. BeCl₂ has a linear structure with bonded Cl atoms on opposite sides of Be.
- The dipoles cancel each other out, making the overall molecule nonpolar.
### Molecule 2: Water (H₂O)
- **Lewis Structure**:
- The central atom is O (Oxygen), which forms two bonds with two H (Hydrogen) atoms.
- Oxygen has two pairs of lone electrons (represented by dots) and two bonding pairs with H.
- **Polarity of Bonds**:
- Analyze the bonds between O and H. Oxygen is more electronegative than Hydrogen, making the O-H bonds polar.
- **Overall Polarity of the Molecule**:
- Consider the molecular geometry. H₂O has a bent shape due to the two lone pairs on Oxygen.
- The dipole moments do not cancel out due to the bent shape, making the overall molecule polar.
### Summary
- **BeCl₂**:
- Bonds: Polar
- Molecule: Nonpolar
- **H₂O**:
- Bonds: Polar
- Molecule: Polar
### Answer Bank
- Options provided:
- Nonpolar
- Polar](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e3f76e7-3e2b-4631-a85d-ebd3274410fe%2F2646d7db-752b-40b6-b8c2-ae2058e830b3%2F1owokm_processed.png&w=3840&q=75)
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