Bond Polarity and Electronegativity
Chemistry ⇒ Chemical Bonding and Structure
Bond Polarity and Electronegativity starts at 10 and continues till grade 12.
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Arrange the following elements in order of increasing electronegativity: O, N, F, C.
Calculate the electronegativity difference for the bond between chlorine (3.16) and sodium (0.93).
Calculate the electronegativity difference for the bond between nitrogen (3.04) and hydrogen (2.20).
Define electronegativity.
Describe how molecular geometry affects the overall polarity of a molecule.
Describe the difference between bond polarity and molecular polarity.
Describe the effect of lone pairs on the polarity of a molecule.
Describe the trend of electronegativity across a period in the periodic table.
Explain why CH4 is a nonpolar molecule even though it contains polar bonds.
Explain why CO2 is a nonpolar molecule even though it contains polar bonds.
Explain why HF has a higher dipole moment than HCl.
Explain why the bond in Cl2 is nonpolar.
Explain why the C–H bond is considered only slightly polar.
Explain why the H–F bond is more polar than the H–Cl bond.
If the electronegativity difference between two atoms is 0, what type of bond is formed?
State the general trend of electronegativity in the periodic table.
State the relationship between bond polarity and dipole moment.
The electronegativity difference between two atoms is 2.1. What type of bond is likely to form?
Which element has the highest electronegativity value according to the Pauling scale?
