Electron Configurations

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Electron Configurations


Lecture number:
2
Pages:
3
Type:
Lecture Note
School:
North Carolina State University
Course:
Ch 220 - Introductory Organic Chemistry
Edition:
1

Unformatted text preview:

CH 220 1st Edition Lecture 2 Outline of Current Lecture I. Electron configurations II. Types of bonding in compounds III. Lewis symbols of elements & Lewis structures IV. Shapes of molecules V. Hybridization Current Lecture I. Electron configurations a. In neutral atoms the number of protons is equal to the number of electrons b. Valence electrons are involved in chemical bonding & reactions, as well as achieving a noble gas configuration c. Core electrons are not involved in chemical bonding or reactions d. Atoms are more stable in compounds that as isolated atoms e. The metals lose electrons from their valence shell f. Non-metals gain electrons to complete their valence shell II. Types of bonding in compounds a. Organic chemistry focuses on nonmetal-nonmetal bonding, known as covalent bonding b. Covalently bonded compounds share electrons to achieve their octet c. Hydrogen is the exception – as it wants to complete its duet d. Na+ is a cation and is isoelectronic with Ne (it loses an electron so that it has the same amount of electrons as Ne) e. Cl- is an anion and is isoelectronic with Ar (it gains an electron so that it has the same amount of electrons as Ar) f. In a covalent bond, the nuclei are attracted to the electron density between atoms, which forms a directional bond g. Bond energy is the same to make a bond as it is to break a bond III. Lewis symbols of elements a. Bars represent bonded pairs b. Dots represent lone valence electrons that are non-bonding c. Methane is the smallest organic molecule d. Examples of the amount of bonds and lone pairs are shown below: These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.



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