Question

consider dicarbon tetrachloride, c₂cl₄.
the lewis structure has 1 central atoms,
each central atom has 2 single bonds and one double bond,
the number of reds at each central atom is 2.
the bond angles are 3° and the shape at each central atom is 4.
c₂cl₄ is a 5 symmetrical/asymmetrical molecule.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 180 g. 90 h. 120
i. 109.5 j. diatomic k. linear l. planar trigonal m. bent n. pyramidal o. tetrahedral p. symmetrical q. asymmetrical

Explanation:

Step1: Central atoms

In \(C_2Cl_4\), there are 2 carbon atoms which act as central atoms.

Step2: REDs (Region of Electron Density)

Each central carbon atom has 3 regions of electron density (2 single bonds + 1 double bond).

Step3: Bond angles

For a central atom with 3 regions of electron density (sp² hybridized), the bond angle is \(120^{\circ}\).

Step4: Shape

A central atom with 3 regions of electron density (no lone pairs) has a planar - trigonal shape.

Step5: Symmetry

\(C_2Cl_4\) is a symmetrical molecule as the substituents (Cl atoms) are arranged symmetrically around the central carbon - carbon double bond.

Answer:

1. C. 2
2. D. 3
3. H. 120
4. L. planar trigonal
5. P. symmetrical