Covalent Bonding
Chemistry ⇒ Chemical Bonding and Structure
Covalent Bonding starts at 8 and continues till grade 12.
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Describe the difference between a coordinate (dative) covalent bond and a regular covalent bond.
Describe the octet rule and its significance in covalent bonding.
Describe the role of lone pairs in determining the shape of a covalent molecule.
Explain the difference between a polar covalent bond and a nonpolar covalent bond.
Explain why covalent compounds do not conduct electricity in the solid or liquid state.
Explain why the bond length decreases as the number of shared electron pairs increases.
Explain why the H–F bond is more polar than the H–Cl bond.
In the context of covalent bonding, what is meant by 'resonance'?
The bond in a Cl₂ molecule is best described as:
(1) Ionic
(2) Polar covalent
(3) Nonpolar covalent
(4) Metallic
Which molecule contains a triple covalent bond?
(1) O₂
(2) N₂
(3) H₂O
(4) CO₂
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 describes the electron domain geometry of carbon dioxide (CO₂)?
(1) Linear
(2) Trigonal planar
(3) Tetrahedral
(4) Bent
A single covalent bond involves the sharing of _______ pair(s) of electrons.
In the molecule carbon dioxide (CO₂), the carbon atom forms _______ double bonds.
In the molecule SF₆, the central sulfur atom forms _______ covalent bonds.
The bond angle in a water (H₂O) molecule is approximately _______ degrees.
True or False: A double covalent bond consists of two shared pairs of electrons.
True or False: All diatomic molecules are nonpolar.
True or False: Covalent bonds are generally formed between two nonmetal atoms.
True or False: Covalent compounds generally have high melting and boiling points.
