Question

1. chemical name: difluoroethylene formula: c₂h₂f₂ lewis electron - dot structure: (draw two different structures in which a single f is bonded to each c and a single h is bonded to each c and the cs are bound to each other.) perspective drawing with bond angles: structure 1 structure 2 standard electron geometry: c₁: c₂: c₁: c₂: molecular geometry: c₁: c₂: c₁: c₂: hybridization of central atoms: c₁: c₂: c₁: c₂: is the molecule polar or nonpolar?

Explanation:

Step1: Determine Lewis structures

The two possible Lewis - electron dot structures for $C_2H_2F_2$ with a single $F$ and a single $H$ bonded to each $C$ and $C - C$ bond are the cis - and trans - isomers. In the cis - isomer, the two $F$ atoms are on the same side of the $C = C$ double bond, and in the trans - isomer, the two $F$ atoms are on opposite sides of the $C = C$ double bond.

Step2: Analyze electron geometry

Each carbon atom in $C_2H_2F_2$ has 3 electron - groups (2 single bonds and 1 double bond). According to VSEPR theory, the standard electron geometry around each $C$ atom for both structures is trigonal planar.

Step3: Determine molecular geometry

Since there are no lone pairs on the central $C$ atoms and 3 bonding groups around each $C$, the molecular geometry around each $C$ atom is also trigonal planar for both structures.

Step4: Find hybridization

With 3 electron - groups around each $C$ atom, the hybridization of each $C$ atom is $sp^2$ for both structures.

Step5: Check polarity

In the cis - isomer, the bond dipoles of the $C - F$ bonds do not cancel out due to the asymmetric arrangement of the $F$ atoms, so the cis - $C_2H_2F_2$ is polar. In the trans - isomer, the bond dipoles of the $C - F$ bonds are equal in magnitude but opposite in direction, so the trans - $C_2H_2F_2$ is non - polar.

Structure 1 (Cis - isomer)

• Standard electron geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Molecular geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Hybridization of central atoms:
• $C_1$: $sp^2$
• $C_2$: $sp^2$
• Is the molecule polar or non - polar? Polar

Structure 2 (Trans - isomer)

• Standard electron geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Molecular geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Hybridization of central atoms:
• $C_1$: $sp^2$
• $C_2$: $sp^2$
• Is the molecule polar or non - polar? Non - polar

It is not possible to draw the Lewis structures and perspective drawings in this text - based format, but the above text provides the necessary information for filling out the table. For the Lewis structures, in the cis - isomer, the two $F$ atoms are on the same side of the double bond and in the trans - isomer, they are on opposite sides. For the perspective drawing, in a trigonal planar geometry around each $C$ atom, the bond angles are approximately $120^{\circ}$.

Answer:

Step1: Determine Lewis structures

The two possible Lewis - electron dot structures for $C_2H_2F_2$ with a single $F$ and a single $H$ bonded to each $C$ and $C - C$ bond are the cis - and trans - isomers. In the cis - isomer, the two $F$ atoms are on the same side of the $C = C$ double bond, and in the trans - isomer, the two $F$ atoms are on opposite sides of the $C = C$ double bond.

Step2: Analyze electron geometry

Each carbon atom in $C_2H_2F_2$ has 3 electron - groups (2 single bonds and 1 double bond). According to VSEPR theory, the standard electron geometry around each $C$ atom for both structures is trigonal planar.

Step3: Determine molecular geometry

Since there are no lone pairs on the central $C$ atoms and 3 bonding groups around each $C$, the molecular geometry around each $C$ atom is also trigonal planar for both structures.

Step4: Find hybridization

With 3 electron - groups around each $C$ atom, the hybridization of each $C$ atom is $sp^2$ for both structures.

Step5: Check polarity

In the cis - isomer, the bond dipoles of the $C - F$ bonds do not cancel out due to the asymmetric arrangement of the $F$ atoms, so the cis - $C_2H_2F_2$ is polar. In the trans - isomer, the bond dipoles of the $C - F$ bonds are equal in magnitude but opposite in direction, so the trans - $C_2H_2F_2$ is non - polar.

Structure 1 (Cis - isomer)

• Standard electron geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Molecular geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Hybridization of central atoms:
• $C_1$: $sp^2$
• $C_2$: $sp^2$
• Is the molecule polar or non - polar? Polar

Structure 2 (Trans - isomer)

• Standard electron geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Molecular geometry:
• $C_1$: Trigonal planar
• $C_2$: Trigonal planar
• Hybridization of central atoms:
• $C_1$: $sp^2$
• $C_2$: $sp^2$
• Is the molecule polar or non - polar? Non - polar

It is not possible to draw the Lewis structures and perspective drawings in this text - based format, but the above text provides the necessary information for filling out the table. For the Lewis structures, in the cis - isomer, the two $F$ atoms are on the same side of the double bond and in the trans - isomer, they are on opposite sides. For the perspective drawing, in a trigonal planar geometry around each $C$ atom, the bond angles are approximately $120^{\circ}$.