The degree of polarity of a bond is indicated by
1) ionization energy difference
2) the shape of the molecule
3) electronegativity difference
4) the charge on the kernel
c is the answer to the question but be careful. Electronegativity difference is what makes the BOND polar but the MOLECULE still may not be a dipole due to the three dimensional shape.
okay thank you so much
The degree of polarity of a bond is indicated by the electronegativity difference between the atoms involved in the bond. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. The greater the electronegativity difference between two atoms bonded together, the more polar the bond between them.
To find the answer to this question, you need to understand the concept of electronegativity and its relationship to bond polarity:
1) Ionization energy difference: Ionization energy refers to the energy required to remove an electron from an atom. While ionization energy is a property that can be used to understand the reactivity and stability of atoms, it is not directly related to bond polarity.
2) Shape of the molecule: The shape of a molecule, also known as its molecular geometry, can influence the overall polarity of the molecule, but not specifically the polarity of a single bond.
3) Electronegativity difference: This is the correct answer. As mentioned earlier, the difference in electronegativity between two atoms bonded together determines the degree of polarity in the bond. The greater the difference, the more polar the bond.
4) Charge on the kernel: The charge on the kernel, or the nucleus, of an atom (usually referred to as the atomic charge) is not a direct indicator of bond polarity.
Therefore, the correct answer to the question is option 3) electronegativity difference.