Question

question 1 (2 points)
true or false.
1 a molecule with a single polar covalent bond will be polar because it is asymmetrical.
2 a molecule with more than one polar covalent bond will be polar if it is asymmetrical.
3 a molecule with more than one polar covalent bond will be nonpolar if it is symmetrical.
4 symmetrical molecules are always nonpolar.
5 asymmetrical molecules are always polar.
a. true b. false

Explanation:

• 1: A single polar covalent bond makes the molecule asymmetrical in terms of electron - charge distribution, so it is polar.
• 2: When a molecule has more than one polar covalent bond and is asymmetrical, the bond dipoles do not cancel out, resulting in a net dipole moment (polar).
• 3: If a molecule with more than one polar covalent bond is symmetrical, the bond dipoles cancel each other (e.g., \(CO_2\) has two \(C = O\) polar bonds but is linear and non - polar).
• 4: Symmetrical molecules (e.g., \(CH_4\) with tetrahedral symmetry and \(C - H\) bonds that are slightly polar) have bond dipoles that cancel out, making them non - polar.
• 5: Asymmetrical molecules (e.g., \(H_2O\) with a bent shape and \(O - H\) polar bonds) have bond dipoles that do not cancel, so they are polar.

Answer:

1. A. True
2. A. True
3. A. True
4. A. True
5. A. True