11. Consider the VSEPR structure shown to the right. What is the molecular geometry depicted? And what is the hybridization of the central atom? a. trigonal pyramidal; sp³ b. T-shaped; sp³ d. trigonal planar; sp² e. trigonal bipyramidal; sp³d c. tetrahedral; spª SZIPLE
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.
![11. Consider the VSEPR structure shown to the right. What is the molecular geometry depicted?
And what is the hybridization of the central atom?
a. trigonal pyramidal; sp³
b. T-shaped; sp³
d. trigonal planar; sp²
e. trigonal bipyramidal; sp³d
12. Consider Lewis structures for the following species: CO32, CO₂ and CO. Which of the following statements is true?
The average bond order in the carbonate ion (CO3²-) is.
The carbon-oxygen bond in carbon monoxide (CO) is the shortest
The carbon in CO₂ is sp hybridized.
It is possible to draw 3 equivalent resonance structures (i.e. same formal charge distribution) for the carbonate ion.
All of these are true.
a.
b.
C.
d.
e.
13. Which one of the following relationships is not correct?
a. atomic radius of P> atomic radius of Cl
c. ionic radius of S2-> ionic radius of Cl-
e. atomic radius of Rb> ionic radius of Rb+
c. tetrahedral; sp4
d. an s orbital with an s orbital
Svad ludolom bill dail
b. ionic radius of Cl-> atomic radius of Cl
d. atomic radius of Ca> atomic radius of K
14. Which of the following types of orbital overlap can result in the formaiton of a pi (r) bond?
a. an s orbital with a p orbital
b. an p orbital with a hybrid orbital c. a p orbital with a p orbital
e. all of these could form a π bond](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fee870430-32a2-499a-9e83-c784fd8c6eea%2Fca7d8e23-35a1-44f2-bda6-ab2a49797059%2F9z6w8tc_processed.jpeg&w=3840&q=75)
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