By Satyajit D Sarker; Lutfun Nahar, Ph. D
ISBN-10: 0470017805
ISBN-13: 9780470017807
ISBN-10: 0470017813
ISBN-13: 9780470017814
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This stable configuration of electrons is called an octet. Except for hydrogen and helium, a filled valence shell contains eight electrons. Lewis structures help us to track the valence electrons and predict the types of bond. The number of valence electrons present in each of the elements is to be considered first. The number of valence electrons determines the number of electrons needed to complete the octet of eight electrons. Simple ions are atoms that have gained or lost electrons to satisfy the octet rule.
In a double bond they share two pairs of electrons and form a s bond and a p bond. In a triple bond two atoms share three pairs of electrons and form a s bond and two p bonds. Sodium (Na) loses a single electron from its 3s orbital to attain a more stable neon gas configuration (1s2 2s2 2p6) with no electron in the outer shell. An atom having a filled valence shell is said to have a closed shell configuration. The total number of electrons in the valence shell of each atom can be determined from its group number in the periodic table.
For example, the hydronium ion (H3Oþ) is positively charged and the oxygen atom has a formal charge of þ1. + .. H O H H Assigned 5 valence electrons: formal charge of +1 So; formal charge ¼ ðgroup numberÞ À ðnonbonding electronsÞ À 1=2 ðshared electronsÞ ¼ 6 À 2 À 1=2ð6Þ ¼ 1: An uncharged oxygen atom must have six electrons in its valence shell. In the hydronium ion, oxygen bonds with three hydrogen atoms. So, only five electrons effectively belong to oxygen, which is one less than the valence electrons.
Chemistry for pharmacy students : general, organic and natural product chemistry by Satyajit D Sarker; Lutfun Nahar, Ph. D
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