|:8–2–6: The electron-pair geometry around the CI atom in CIO₂ is There are A. The Lewis diagram for CIO₂ is: lone pair(s) around the central atom, so the geometry of CIO₂ is B. The Lewis diagram for PCI4+ is: :CI: :CI-P-CI: CI: The electron-pair geometry around the P atom in PCI4+ is There are lone pair(s) around the central atom, so the geometry of PCI4+ is
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.
The diagram shows a central chlorine atom (Cl) bonded to two oxygen atoms (O) with single bonds. There is one lone pair of electrons on Cl and each O has three lone pairs. The entire diagram is enclosed in brackets with a negative charge indicated outside the bracket.
The **electron-pair geometry** around the Cl atom in \( \text{ClO}_2^- \) is [Blank].
There are [Blank] lone pair(s) around the central atom, so the geometry of \( \text{ClO}_2^- \) is [Blank].
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**B. The Lewis diagram for \( \text{PCl}_4^+ \) is:**
The diagram features a central phosphorus atom (P) bonded to four chlorine atoms (Cl) with single bonds. Each chlorine atom has three lone pairs. The entire diagram is enclosed in brackets with a positive charge indicated outside the bracket.
The **electron-pair geometry** around the P atom in \( \text{PCl}_4^+ \) is [Blank].
There are [Blank] lone pair(s) around the central atom, so the geometry of \( \text{PCl}_4^+ \) is [Blank].
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