Questions and Answers
What type of orbital overlap forms the bond in a fluorine molecule?
Which of the following compounds has a carbon-carbon sigma bond formed by overlapping sp orbitals?
What is the formula for calculating the percentage of ionic character in a compound?
How many sigma and pi bonds are present in vinyl alcohol?
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Which carbon-carbon bond has the highest bond energy?
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Which of the following compounds is an ionic compound?
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Which of the following statements about bond angles is true?
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Which of the following is NOT a factor that affects the bond energy of a covalent bond?
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Which of the following compounds exhibits a dipole-dipole interaction?
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Study Notes
Chemical Bonding
- The exact value of the angle in BF3 is 120°.
- Molecules with non-planar geometry include CH4, NH4+, MnO4-, and NF3.
- Sigma bonds are formed when two partially filled atomic orbitals overlap in such a way that the probability of finding the electron is maximum around the line joining the two nuclei.
- The angle between un-hybridized p-orbital and three sp2 hybrid orbitals of each carbon atom is 120°.
- Fe will form the most ionic bond with F-.
- AB4 type molecules with no lone pairs enable the formation of a regular tetrahedral shape.
- The compound with the greatest difference of electronegativity is HF.
- The bond formed by overlapping of sp2 and p orbitals is found in BF3.
- During the formation of a chemical bond, energy decreases.
- Hydrogen bonds are not primary bonds.
- Non-planar molecules include SO2, C2H4, and BF3.
- Ionic bonds have the least electronegativity difference between bonding atoms.
- The element with the lowest first ionization energy is N.
- The percentage of ionic and covalent character in HF is 43% and 57%, respectively.
Molecular Geometry
- The compromised distance between two hydrogen atoms in a hydrogen molecule is 74 pm.
- The radius of an atom cannot be measured precisely because the atom has no sharp boundary, and the size of the atom changes from one compound to another.
- Covalent radius is half of the bond distance between two similar atoms covalently bonded in a molecule.
- The energy gap between 2nd ionization energy and 3rd ionization energy is very large for elements with Z values belonging to I-A, II-A, III-A, and IV-A.
- The central atom of AB4 molecules carries bond pair-bond pair repulsions only.
- The percentage of s-character in hybrid orbitals indicating the longest bond length is 25%.
- The hybridization of carbon number 1 in 1-Propene is sp2.
- The molecular geometry of a species with 3 bond pairs and 1 lone pair is trigonal pyramidal.
- The shape of the carbonate ion is trigonal planar.
Electronegativity and Ionization Energy
- The element with the highest electronegativity is F.
- The high value of the first ionization energy of nitrogen compared to oxygen is due to its half-filled p-subshell.
- Electronegativity of elements increases from left to right along a period.
- Ionic character in a compound can be calculated by (ionic μ / observed μ) × 100.
- The bond energy depends on electronegativity difference, bond length, and atomic radius.
Bonds and Hybridization
- The bond between carbon and oxygen in CO2 is a covalent bond.
- The strength of a bond between two atoms depends on electronegativity difference, bond length, and atomic radius.
- The shortening of bonds is due to the predominant participation of s-orbital in hybridization.
- The carbon-carbon sigma bond in ethyne molecule is formed by overlapping between sp-orbitals of carbon atoms.
- The bond in fluorine molecule is formed by the overlapping of p-orbitals on each atom of fluorine.
Miscellaneous
- Ammonia (NH3) can form a bond with boron trifluoride (BF3) by supplying electrons.
- The bond between carbon and oxygen in CO2 is a covalent bond.
- The specie with the highest ionic character is CsF.
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Description
Chemical Bonding questions for MDCAT Unit-6, covering topics like bond angles and molecular geometry.