Chemical Bonding: 18 flashcards
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1. What is a chemical bond?
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A chemical bond is the force of attraction that holds atoms or ions together in a chemical species (molecule, ion, etc.).
2. State the octet rule.
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Atoms tend to gain, lose, or share electrons to achieve a stable electronic configuration of eight valence electrons (like noble gases).
3. What is an ionic bond? Give an example.
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An ionic bond is formed by the complete transfer of electrons from one atom to another, resulting in electrostatic attraction between oppositely charged ions. Example: NaCl.
4. Define lattice enthalpy.
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Lattice enthalpy is the amount of energy released when one mole of an ionic compound is formed from its gaseous ions (or the energy required to separate one mole into gaseous ions).
5. What is a covalent bond?
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A covalent bond is formed by the mutual sharing of one or more pairs of electrons between two atoms.
6. What is the difference between a polar covalent bond and a non-polar covalent bond?
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In a non-polar covalent bond, electrons are shared equally (e.g., H₂). In a polar covalent bond, electrons are shared unequally due to electronegativity difference (e.g., HCl).
7. Define electronegativity.
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Electronegativity is the tendency of an atom in a molecule to attract the shared pair of electrons towards itself.
8. What is the VSEPR theory?
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VSEPR (Valence Shell Electron Pair Repulsion) theory states that the shape of a molecule is determined by the repulsion between electron pairs (bonding and lone pairs) in the valence shell of the central atom, which arrange themselves to minimize repulsion.
9. What is the shape of a molecule with 2 bond pairs and 0 lone pairs on the central atom?
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Linear (bond angle 180°). Example: BeCl₂.
10. What is the shape and bond angle of a molecule with 3 bond pairs and 0 lone pairs?
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Trigonal planar, bond angle 120°. Example: BF₃.
11. What is the shape and bond angle of a molecule with 4 bond pairs and 0 lone pairs?
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Tetrahedral, bond angle 109.5°. Example: CH₄.
12. What is the shape of a molecule with 3 bond pairs and 1 lone pair?
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Trigonal pyramidal (bond angle ~107°). Example: NH₃.
13. What is the shape of a molecule with 2 bond pairs and 2 lone pairs?
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Bent or V-shaped (bond angle ~104.5°). Example: H₂O.
14. What is hybridization?
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Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals of equivalent energy, which are used in bonding to explain molecular geometry.
15. What is the hybridization of carbon in CH₄?
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sp³ hybridization (four equivalent sp³ orbitals, tetrahedral geometry).
16. What is the hybridization of boron in BF₃?
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sp² hybridization (three sp² orbitals, trigonal planar).
17. What is the hybridization of beryllium in BeCl₂?
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sp hybridization (two sp orbitals, linear geometry).
18. What is a sigma (σ) bond and a pi (π) bond?
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A sigma bond is formed by head-on overlap of atomic orbitals along the internuclear axis. A pi bond is formed by sidewise overlap of p orbitals, perpendicular to the internuclear axis.
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