QQuestionChemistry
QuestionChemistry
Which of the following is the correct Lewis structure for carbon dioxide (CO₂)?
A. Central C singly bound to two O atoms, no non-bonding electrons
B. Central C singly bound to two O atoms, double-bonded O with 2 electron pairs
C. C double-bonded to 2 O atoms, each O has 2 lone pairs of electrons
D. One C atom in the center, single-bonded to two O atoms, no other bonds, each O has three lone pairs of electrons
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Answer
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Step 1:: Understand the Lewis structure concept.
A Lewis structure is a graphical representation of the valence electrons around an atom in a molecule, which helps to show the formation of chemical bonds.
Step 2:: Examine the given options for the Lewis structure of CO₂.
Step 3:: Identify the correct Lewis structure.
- Option A suggests a central C atom singly bound to two O atoms, with no non-bonding electrons. This is incorrect because C in CO₂ has a steric number of 2 (two regions of electron density), and it needs to satisfy the octet rule. - Option B suggests a central C atom singly bonded to two O atoms, with one of the O atoms double-bonded and having 2 lone pairs. This is close, but the C atom should be double-bonded to both O atoms to satisfy the octet rule. - Option C suggests a C atom double-bonded to 2 O atoms, with each O atom having 2 lone pairs of electrons. This is the correct Lewis structure for CO₂. - Option D suggests a central C atom single-bonded to two O atoms, with each O atom having three lone pairs of electrons. This is incorrect because it does not satisfy the octet rule for the C atom and the O atoms.
Final Answer
The correct Lewis structure for CO₂ is option C, where the C atom is double-bonded to two O atoms, and each O atom has 2 lone pairs of electrons.
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