# Draw A Lewis Structure For C2H3Cl. Show All Unshared Electron Pairs. None Of The Atoms Bears A Formal Charge, And All Atoms Have Octets (except For Hydrogen Atoms, Which Have Duets). Transcribed Text:
Question: Draw a Lewis structure for C2H3Cl. Show all unshared electron …
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Draw a Lewis structure for C2H3CI. Show all unshared electron pairs. None of the atoms bears a formal charge, and all atoms have octets (except for hydrogen atoms, which have duets).
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General guidance
Concepts and reason A Lewis structure is a structural representation of the molecule including the electron distribution around the atoms. The valence electrons on each atom can be found using the atomic number of each atom.
Fundamentals Lewis structure includes all non-bonded electrons in the structure. Each atom in the molecule should fulfill the octet rule. The dots are used to represent the one pairs or non-bonded pairs of electrons and the dot pairs or a line is used to
Step-by-step
FIRST STEP ALL STEPS ANSWER ONLY
Step 1 of 4 ^
The given molecule is CH3C1
Total number of valence electrons = 2 (4) +3 (1) +1 (7)
= 18 Total number of valance electrons of CH3C1 =18
Explanation Common mistakes Hint for next step Total valance electron is calculated by adding the individual valance electrons of each atom. The valence electrons of individual atoms are given below. Valance electron of carbon is 4. Valance electron of hydrogen is 1. Valance electron of chlorine is 7 There is 1 chlorine, 2 carbons and 3 hydrogen’s present in the given molecule. Hence, the sum is taken for the valence electron for the atom multiplied with the number of respective atoms present.
Step 2 of 4 ^
The skeleton structure for the given molecule is as follows:
Figure 1
Explanation Hint for next step The skeleton structure of C2H3Cl is given in figure 1. This is the only possibility of connectivity of the atoms. All atoms are joined with a line indicating a covalent bond. Each bond contains two electrons. There are five bonds and so ten electrons out of eighteen electrons are used for the bonding structure.
Step 3 of 4 ^
The molecule showing all nonbonding electrons on the respective atoms is as follows:
Н
Figure 2
Explanation Common mistakes Hint for next step Valance electron of chlorine is 7. One electron is used in covalence bonding, and hence, remaining six electrons remain nonbonded on the chlorine atom, that is three pairs of nonbonding electrons. Valance electron of carbon is 4. Three electrons are used in the bonding, and hence, one electron remains nonbonded. Valance electron of hydrogen is 1. One electron is involved in the covalent bonding, and hence, there are no nonbonding electrons on hydrogen.
Step 4 of 4 ^
The Lewis structure is as follows:
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Lewis structure
Figure 2
Lewis structure of C2H3Cl is as follows:
Explanation
A single electron on the atom is not possible for a stable Lewis structure. There is a single electron on adjacent carbons, which is not stable. Hence, they are involved in the covalent bonding to fulfill the octet of carbons.