Here is the detailed analysis for each molecule as requested.<\/p>\n\n\n\n
Analysis of Molecules<\/strong><\/h3>\n\n\n\na) BF\u2083 (Boron trifluoride)<\/strong><\/p>\n\n\n\n\n- Total Valence Electrons:<\/strong>\u00a03 (from B) + 3 \u00d7 7 (from F) =\u00a024<\/strong><\/li>\n\n\n\n
- Lewis Structure:<\/strong>\u00a0Boron is the central atom, forming single bonds with three fluorine atoms. Each fluorine has three lone pairs. This structure has zero formal charges on all atoms. While resonance structures can be drawn giving boron a full octet, they place a positive formal charge on the highly electronegative fluorine atom, making them minor contributors. The dominant structure is the one with an incomplete octet on boron.
:F: | :F \u2014 B \u2014 F:<\/code>content_copydownloadUse code\u00a0<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central boron atom has 3 electron domains (3 single bonds, 0 lone pairs). This corresponds to an AX\u2083 arrangement, resulting in a\u00a0Trigonal Planar<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a03 electron domains require\u00a0sp\u00b2<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0The B-F bonds are polar. However, the molecule’s symmetrical trigonal planar shape causes the individual bond dipoles to cancel each other out perfectly. Therefore, the molecule is\u00a0nonpolar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
b) OSCl\u2082 (Thionyl chloride)<\/strong><\/p>\n\n\n\n\n- Total Valence Electrons:<\/strong>\u00a06 (from O) + 6 (from S) + 2 \u00d7 7 (from Cl) =\u00a026<\/strong><\/li>\n\n\n\n
- Lewis Structure:<\/strong>\u00a0Sulfur is the central atom. The most stable Lewis structure features a double bond between sulfur and oxygen, single bonds between sulfur and each chlorine, and one lone pair on the sulfur atom. This arrangement minimizes formal charges to zero for all atoms.
:O: || :Cl \u2014 S \u2014 Cl: ..<\/code>content_copydownloadUse code\u00a0with caution<\/a>.<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central sulfur atom has 4 electron domains (1 double bond, 2 single bonds, 1 lone pair). This corresponds to an AX\u2083E\u2081 arrangement, resulting in a\u00a0Trigonal Pyramidal<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a04 electron domains require\u00a0sp\u00b3<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0The S-O and S-Cl bonds are polar, and the trigonal pyramidal geometry is asymmetrical. The lone pair and the bond dipoles do not cancel, creating a net dipole moment. The molecule is\u00a0polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
c) SCN\u207b (Thiocyanate ion)<\/strong><\/p>\n\n\n\n\n- Total Valence Electrons:<\/strong>\u00a06 (from S) + 4 (from C) + 5 (from N) + 1 (for the charge) =\u00a016<\/strong><\/li>\n\n\n\n
- Lewis Structure and Resonance:<\/strong>\u00a0Carbon is the central atom. The ion exists as a resonance hybrid of three structures. The most significant contributor places a double bond between S and C, a double bond between C and N, and the negative formal charge on the most electronegative atom, nitrogen. A second important contributor has a single bond between S and C, and a triple bond between C and N, placing the negative charge on sulfur.
[ :S=C=N: ]\u207b <--> [ :S\u2014C\u2261N: ]\u207b <--> [ :S\u2261C\u2014N: ]\u00b2\u207b FC: S=0, C=0, N=-1 FC: S=-1, C=0, N=0 (Major Contributor)<\/code>content_copydownloadUse code\u00a0with caution<\/a>.<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central carbon atom has 2 electron domains in all significant resonance structures. This corresponds to an AX\u2082 arrangement, resulting in a\u00a0Linear<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a02 electron domains require\u00a0sp<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0As an ion, it is charged. The charge distribution within the ion is uneven because sulfur and nitrogen have different electronegativities. The bond dipoles do not cancel, so the ion possesses a permanent dipole moment and is considered\u00a0polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
d) H\u2082CCl\u2082 (Dichloromethane)<\/strong><\/p>\n\n\n\n
- \n
- Total Valence Electrons:<\/strong>\u00a03 (from B) + 3 \u00d7 7 (from F) =\u00a024<\/strong><\/li>\n\n\n\n
- Lewis Structure:<\/strong>\u00a0Boron is the central atom, forming single bonds with three fluorine atoms. Each fluorine has three lone pairs. This structure has zero formal charges on all atoms. While resonance structures can be drawn giving boron a full octet, they place a positive formal charge on the highly electronegative fluorine atom, making them minor contributors. The dominant structure is the one with an incomplete octet on boron.
:F: | :F \u2014 B \u2014 F:<\/code>content_copydownloadUse code\u00a0<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central boron atom has 3 electron domains (3 single bonds, 0 lone pairs). This corresponds to an AX\u2083 arrangement, resulting in a\u00a0Trigonal Planar<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a03 electron domains require\u00a0sp\u00b2<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0The B-F bonds are polar. However, the molecule’s symmetrical trigonal planar shape causes the individual bond dipoles to cancel each other out perfectly. Therefore, the molecule is\u00a0nonpolar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
b) OSCl\u2082 (Thionyl chloride)<\/strong><\/p>\n\n\n\n
- \n
- Total Valence Electrons:<\/strong>\u00a06 (from O) + 6 (from S) + 2 \u00d7 7 (from Cl) =\u00a026<\/strong><\/li>\n\n\n\n
- Lewis Structure:<\/strong>\u00a0Sulfur is the central atom. The most stable Lewis structure features a double bond between sulfur and oxygen, single bonds between sulfur and each chlorine, and one lone pair on the sulfur atom. This arrangement minimizes formal charges to zero for all atoms.
:O: || :Cl \u2014 S \u2014 Cl: ..<\/code>content_copydownloadUse code\u00a0with caution<\/a>.<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central sulfur atom has 4 electron domains (1 double bond, 2 single bonds, 1 lone pair). This corresponds to an AX\u2083E\u2081 arrangement, resulting in a\u00a0Trigonal Pyramidal<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a04 electron domains require\u00a0sp\u00b3<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0The S-O and S-Cl bonds are polar, and the trigonal pyramidal geometry is asymmetrical. The lone pair and the bond dipoles do not cancel, creating a net dipole moment. The molecule is\u00a0polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
c) SCN\u207b (Thiocyanate ion)<\/strong><\/p>\n\n\n\n
- \n
- Total Valence Electrons:<\/strong>\u00a06 (from S) + 4 (from C) + 5 (from N) + 1 (for the charge) =\u00a016<\/strong><\/li>\n\n\n\n
- Lewis Structure and Resonance:<\/strong>\u00a0Carbon is the central atom. The ion exists as a resonance hybrid of three structures. The most significant contributor places a double bond between S and C, a double bond between C and N, and the negative formal charge on the most electronegative atom, nitrogen. A second important contributor has a single bond between S and C, and a triple bond between C and N, placing the negative charge on sulfur.
[ :S=C=N: ]\u207b <--> [ :S\u2014C\u2261N: ]\u207b <--> [ :S\u2261C\u2014N: ]\u00b2\u207b FC: S=0, C=0, N=-1 FC: S=-1, C=0, N=0 (Major Contributor)<\/code>content_copydownloadUse code\u00a0with caution<\/a>.<\/li>\n\n\n\n- VSEPR Molecular Geometry:<\/strong>\u00a0The central carbon atom has 2 electron domains in all significant resonance structures. This corresponds to an AX\u2082 arrangement, resulting in a\u00a0Linear<\/strong>\u00a0geometry.<\/li>\n\n\n\n
- Hybridization of Central Atom:<\/strong>\u00a02 electron domains require\u00a0sp<\/strong>\u00a0hybridization.<\/li>\n\n\n\n
- Polarity:<\/strong>\u00a0As an ion, it is charged. The charge distribution within the ion is uneven because sulfur and nitrogen have different electronegativities. The bond dipoles do not cancel, so the ion possesses a permanent dipole moment and is considered\u00a0polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n
d) H\u2082CCl\u2082 (Dichloromethane)<\/strong><\/p>\n\n\n\n
- Lewis Structure and Resonance:<\/strong>\u00a0Carbon is the central atom. The ion exists as a resonance hybrid of three structures. The most significant contributor places a double bond between S and C, a double bond between C and N, and the negative formal charge on the most electronegative atom, nitrogen. A second important contributor has a single bond between S and C, and a triple bond between C and N, placing the negative charge on sulfur.
- Lewis Structure:<\/strong>\u00a0Sulfur is the central atom. The most stable Lewis structure features a double bond between sulfur and oxygen, single bonds between sulfur and each chlorine, and one lone pair on the sulfur atom. This arrangement minimizes formal charges to zero for all atoms.
- Lewis Structure:<\/strong>\u00a0Boron is the central atom, forming single bonds with three fluorine atoms. Each fluorine has three lone pairs. This structure has zero formal charges on all atoms. While resonance structures can be drawn giving boron a full octet, they place a positive formal charge on the highly electronegative fluorine atom, making them minor contributors. The dominant structure is the one with an incomplete octet on boron.
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