Part I: Line Bond Structures Instructions: After looking at the examples on page 2 and 3, complete the tables on each of the pages thereafter by drawing Line Bond Structures of the molecules given. When you are finished with all of the line bond structures, re-draw your structures on this first page and bring it to me to check. After I check your line bond structures, proceed to the Part II: Molecular Shape section. NH3 Br₂ H-N-H H Last 4 Line Bond Structures and Molecular Geometry H₂S H H HCI H-cl OF 2 NI3 I-N-I H-N-H 14 C-C-C-C HHH 14 H-CI: H :Ï: :I-N-I: 2-methylbutane (CsH12) - see page 14 6. Br-Br Br-Bri CC14 CI .c-cl Cí C-C1-C-C 1 CI (S₂ S-S SO₂ S= S. a CS₂ S-C-S :ci: S=C = S Acetone (C3H6O) - see page 15 HO H H-c-c-6-H C-C-C
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.
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