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.
general chemistry , please solve question 14 and 15
![11) Which of the following is an isoelectronic series?
A) 02-, F, Ne, Nat
D) F, CI, Br, I-
B) S, a, Ar, K
E) Si2, P2-, 52-, C2-
O B5, Sit, As3, Te2-
12) The Lewis structure of N2H2 shows
A) each nitrogen has two nonbonding electron pairs
C) a nitrogen-nitrogen single bond
E) each nitrogen has one nonbonding electron pair
B) each hydrogen has one nonbonding electron pair
D) a nitrogen-nitrogen triple bond
13) Of the bonds C-C, C-C, and CC, the C-C bond is
A) weakest/shortest
D) intermediate in both strength and length
B) strongest/shortest
E) weakest/longest
14) How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet
strongest/longest
rule on the sulfur atom?
A) 3
B) 2
C)1
D) 5
E) 4
15) Given the electronegativities below, which covalent single bond is most polar?
Element:
H
N
Electronegativity:
2.1
2.5
3.0
3.5
A) O-C
B) 0-H
C)0-N
D) C-H
E) N-H
16) The ground-state electron configuration of the element
is [Kr]5s14d5.
A) Nb
B) Tc
9 Cr
D) Mn
E) Mo
17) The F-B-F bond angle in the BF2 ion is approximately
A) 90°
B) 109.5°
C) 120°
D) 180°
E) 60°
18) There are
o and
n bond(s) in the H2C-CH2 molecule.
A) 3 and 4
B) 5 and 1
C) 3 and 2
D) 2 and 3
E) 4 and 3
19) The molecular geometry of the PF4+ ion is
C) trigonal bipyramidal D) tetrahedral
E) trigonal planar
A) trigonal pyramidal
B) octahedral
orbitals,
20) The hybrid orbitals used for bonding by Xe in the unstable XeF2 molecule are
C) sp2
D) sp3
E) sp3d
A) sp3d2
B) sp](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F32864c0b-8333-426d-96a2-f986604aaa4d%2Fca0ba5d6-2463-4398-86ed-f879d0e6de92%2Fa0h1ahm_processed.jpeg&w=3840&q=75)
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