Covalent Bonding
Chemistry ⇒ Chemical Bonding and Structure
Covalent Bonding starts at 8 and continues till grade 12.
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See sample questions for grade 11
A student draws the Lewis structure for ammonia (NH3). How many bonding pairs and lone pairs are present on the nitrogen atom?
Calculate the bond order of the oxygen molecule (O2).
Describe the difference between sigma (σ) and pi (π) bonds in covalent bonding.
Describe the octet rule and its significance in covalent bonding.
Explain the difference between a polar covalent bond and a nonpolar covalent bond.
Explain why diamond, a covalent network solid, has a very high melting point.
Explain why the H–Cl bond is polar while the H–H bond is nonpolar.
How many total covalent bonds are present in a molecule of ethene (C2H4)?
In the Lewis structure of water (H2O), how many lone pairs of electrons are present on the oxygen atom?
A molecule of carbon monoxide (CO) contains both a triple bond and a coordinate covalent bond. Explain how this is possible, referring to the electron configuration of carbon and oxygen.
Consider the molecule XeF2. Predict its molecular geometry and explain your reasoning based on the VSEPR theory.
Describe the difference between localized and delocalized covalent bonding, providing an example of each.
Explain why the molecule PCl5 is able to form five covalent bonds, even though phosphorus is in period 3 of the periodic table. Discuss the role of d orbitals in your answer.
Given the following data: The bond dissociation energy for a C–C single bond is 348 kJ/mol, for a C=C double bond is 614 kJ/mol, and for a C≡C triple bond is 839 kJ/mol. Calculate the average bond energy per bond for each type and explain the trend observed.
