Which of the following electron-dot formulas (or Lewis structures) is wrong? A Br- B C D COA OD O :F-CI: :K-CI: :I-a: O 64°F Cloudy B ci: (Lewis structure for BrCI) Cl: U (Lewis structure for CIF) (Lewis structure for KCI) (Lewis structure for ICI)
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![**Question:**
Which of the following electron-dot formulas (or Lewis structures) is wrong?
**Options:**
A. \[\mathrm{Br} - \mathrm{Cl}\] (Lewis structure for BrCl)
B. \[\mathrm{F} - \mathrm{Cl}\] (Lewis structure for ClF)
C. \[\mathrm{K} - \mathrm{Cl}\] (Lewis structure for KCl)
D. \[\mathrm{I} - \mathrm{Cl}\] (Lewis structure for ICl)
**Answer Choices:**
- A
- B
- C
- D
**Explanation:**
- Each option represents a Lewis structure with dots indicating valence electrons around the elements.
- Option A shows bromine (Br) and chlorine (Cl) bonded together.
- Option B shows fluorine (F) and chlorine (Cl) bonded together.
- Option C shows potassium (K) and chlorine (Cl) bonded together. This is incorrect as KCl is an ionic compound, not a covalent one, so there should not be a line (covalent bond) between them.
- Option D shows iodine (I) and chlorine (Cl) bonded together.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F551637be-7a52-44bd-9b06-307a09d9ac69%2F325477f6-5744-4d83-ae26-3fbb2375bef7%2Flr50oe_processed.jpeg&w=3840&q=75)
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