Problem: Part B. Using the given table of electronegativity values, determine whether each bond is nonpolar covalent, polar covalent, or ionic.Drag the appropriate items to their respective bins.Bond polarity results from two bonded atoms having differing electronegativity values. Covalent bonds exist when the two atoms involved in the bond share the electrons. These electrons are shared either evenly or unevenly to a degree depending on the electronegativity differences between the two atoms. Ionic bonds exist when the two atoms transfer electrons. These electrons are so strongly attracted to the more electronegative atom that there is virtually no sharing of electrons and the atoms are simply attracted to another by having opposite charges.The difference in electronegativity values can be used to predict the type of bond formed between two atoms.Nonpolar covalent: Bonds between atoms with electronegativity differences of 0.4 and under are generally considered nonpolar covalent bonds since the electrons are shared relatively evenly. This is true even if there are two different atoms in the bond, such as a Cl−Br bond.Polar covalent: Bonds between atoms with electronegativity differences between 0.4 and 2.0 are generally considered polar covalent since the electrons are shared unevenly.Ionic: Bonds between atoms with electronegativity differences greater than 2.0 are generally considered ionic since the electrons are localized on the more electronegative atom.

FREE Expert Solution
79% (282 ratings)
Problem Details

Part B. Using the given table of electronegativity values, determine whether each bond is nonpolar covalent, polar covalent, or ionic.


Drag the appropriate items to their respective bins.


Bond polarity results from two bonded atoms having differing electronegativity values. Covalent bonds exist when the two atoms involved in the bond share the electrons. These electrons are shared either evenly or unevenly to a degree depending on the electronegativity differences between the two atoms. Ionic bonds exist when the two atoms transfer electrons. These electrons are so strongly attracted to the more electronegative atom that there is virtually no sharing of electrons and the atoms are simply attracted to another by having opposite charges.

The difference in electronegativity values can be used to predict the type of bond formed between two atoms.

  • Nonpolar covalent: Bonds between atoms with electronegativity differences of 0.4 and under are generally considered nonpolar covalent bonds since the electrons are shared relatively evenly. This is true even if there are two different atoms in the bond, such as a Cl−Br bond.
  • Polar covalent: Bonds between atoms with electronegativity differences between 0.4 and 2.0 are generally considered polar covalent since the electrons are shared unevenly.
  • Ionic: Bonds between atoms with electronegativity differences greater than 2.0 are generally considered ionic since the electrons are localized on the more electronegative atom.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Chemical Bonds concept. You can view video lessons to learn Chemical Bonds. Or if you need more Chemical Bonds practice, you can also practice Chemical Bonds practice problems.