Concept explainers
Interpretation:
To analyse whether the given molecules follows octet rule or not.
Concept Introduction:
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Lewis structure of a molecule can be determined as-
- 1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.
If the molecule is an anion, add the same number of electrons as the charge present on the ion.
If it is a cation, subtract the same number of electrons as the charge present on the ion.
2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).
3. Therefore number of bonds formed =
4. Remaining electrons are called as lone pairs.
5. Assign formal charges to atoms.
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Introduction To General, Organic, And Biochemistry
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- 3-66 Why can’t second-row elements have more than eight electrons in their valence shells? That is, why does the octet rule work for second-row elements?arrow_forward3-106 Consider the structure of Penicillin G shown below, an antibiotic used to treat bacterial infections caused by gram-positive organisms, derived from Penicillium fungi: (a) Identify the various types of geometries present in each central atom using VSEPR theory. (b) Determine the various relative bond angles associated with each central atom using VSEPR theory (c) Which is the most poiar bond in Penicillin G? (d) Would you predict Penicillin G to be polar or nonpolar?arrow_forward3-25 Why are carbon and silicon reluctant to form ionic bonds?arrow_forward
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- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning