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 bonds in order of increasing polarity: C–H, O–H, N–H.
Define electronegativity.
Describe how the concept of electronegativity is useful in predicting the type of bond formed between two atoms.
Describe the relationship between bond polarity and molecular polarity.
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 the C–Cl bond is more polar than the C–H bond.
Explain why the H–Cl bond is polar.
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 least polar bond?
(1) H–F
(2) H–Cl
(3) H–Br
(4) H–I
Which of the following molecules has a net dipole moment?
(1) BF3
(2) CH4
(3) H2O
(4) CCl4
Which of the following molecules is expected to have the highest dipole moment?
(1) H2O
(2) CO2
(3) CH4
(4) CCl4
A bond between two identical atoms is always ________ (polar/nonpolar).
If the electronegativity difference between two atoms is greater than 1.7, the bond is usually considered ________.
In the molecule NH3, the nitrogen atom has a ________ (partial positive/partial negative) charge.
The bond in O2 is ________ (polar/nonpolar).
State whether the following statement is true or false: The polarity of a molecule depends only on the polarity of its bonds.
True or False: A molecule with polar bonds is always polar.
True or False: The greater the difference in electronegativity between two bonded atoms, the more polar the bond.
