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.
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.
Which of the following best describes a nonpolar covalent bond?
(1) Electrons are transferred from one atom to another.
(2) Electrons are shared unequally between atoms.
(3) Electrons are shared equally between atoms.
(4) There is a large difference in electronegativity.
Which of the following bonds is the least polar?
(1) O–H
(2) N–H
(3) C–H
(4) F–H
Which of the following bonds is the most polar?
(1) H–F
(2) H–Cl
(3) H–Br
(4) H–I
Which of the following has the lowest electronegativity?
(1) Li
(2) Na
(3) K
(4) Cs
The bond in NaCl is considered ________ due to the large difference in electronegativity between Na and Cl.
The difference in electronegativity between hydrogen (2.20) and oxygen (3.44) is ________.
The direction of the dipole moment in a polar bond is from the ________ electronegative atom to the ________ electronegative atom.
The electronegativity of carbon is ________ than that of nitrogen.
True or False: A molecule with polar bonds is always a polar molecule.
True or False: All diatomic molecules with different atoms are polar.
True or False: In a polar covalent bond, electrons are shared equally between the two atoms.
True or False: The electronegativity of an element is a fixed value and does not depend on its chemical environment.
