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.
A student draws the Lewis structure for ammonia (NH3). How many bonding pairs and lone pairs are present on the nitrogen atom?
Consider the molecule XeF2. Predict its molecular geometry and explain your reasoning based on the VSEPR theory.
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.
Which molecule contains a triple covalent bond?
(1) O2
(2) N2
(3) H2O
(4) CO2
Which of the following best describes a coordinate covalent bond?
(1) Both atoms contribute one electron each to the bond
(2) One atom donates both electrons to the shared pair
(3) Electrons are transferred from one atom to another
(4) The bond is formed by delocalized electrons
Which of the following best describes a covalent bond?
(1) The transfer of electrons from one atom to another
(2) The sharing of electron pairs between atoms
(3) The attraction between oppositely charged ions
(4) The delocalization of electrons across a metal lattice
Which of the following best explains why O2 is a diatomic molecule?
(1) Oxygen atoms are unstable alone and share two pairs of electrons to achieve stability
(2) Oxygen atoms transfer electrons to each other
(3) Oxygen atoms form ionic bonds with each other
(4) Oxygen atoms do not form bonds with each other
A single covalent bond involves the sharing of _______ pair(s) of electrons.
Fill in the blank: In a polar covalent bond, the atom with higher electronegativity acquires a partial _______ charge.
Fill in the blank: The ability of an atom to attract shared electrons in a covalent bond is called _______.
Fill in the blank: The molecule BF3 is an example of a molecule that does not obey the _______ rule.
True or False: Covalent bonds are generally formed between two nonmetal atoms.
True or False: Covalent bonds can only be single bonds.
True or False: The bond between the carbon and oxygen atoms in carbon dioxide (CO2) is a double covalent bond.
True or False: The bond order of a molecule is defined as the number of bonds between two atoms divided by the number of bond groups between those atoms.
