Log in
HomeTextbook Notes300,000US110,000

CH-1010 Chapter Notes - Chapter 4: Electronegativity, Single Bond, Double Bond

29 views3 pages
School
Clemson University
Department
Chemistry
Course
CH-1010
Professor
Mycia Cox

For unlimited access to Textbook Notes, a Class+ subscription is required.

Document Summary

Valence: the capacity of the atoms of an element to form chemical bonds. Ionic bond: a bond resulting from the electrostatic attraction of a cation for an anion. Lattice energy (u): the energy released when 1 mole of an ionic compound forms from its free ions in the gas phase. Crystal lattice: an ordered three-dimensional array of particles. Covalent bond: a bond created by two atoms sharing one or more pairs of electrons. Bond length: the distance between the nuclear centers of two atoms joined together in a bond. Bond energy: the energy needed to break 1 mole of a particular covalent bond in a molecule or polyatomic ion in the gas phase; also called bond strength. Metallic bond: a bond consisting of the nuclei of metal atoms surrounded by a sea of shared electrons. Polyatomic ion: a charged group of more than one kind of atom joined together by covalent bonds.

Get access

Grade+
$40 USD/m
Billed monthly
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
10 Verified Answers
Class+
$30 USD/m
Billed monthly
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
7 Verified Answers

Related Documents

CH-1010 Lecture Notes - Lecture 2: Atomic Number, Oxyanion, Electric Potential Energy
erindog825
CH-1010 Chapter Notes - Chapter 4: Oxyanion, Ionic Compound, Ionic Radius
lavenderantelope86
CH-1010 Lecture Notes - Lecture 3: Lattice Energy, Covalent Bond, Bond-Dissociation Energy
emeraldmammoth217

Related Questions

1. True or False. a. A positively charged ion is called an anion. b. If an atom gives up an electron, it creates negatively charged ion. c. Valence electrons are the electrons that are available for bonding and located in the shells closest to the nucleus. d. An ionic bond is the result of electron sharing. e. When atoms gain, lose, or share electrons they do so in order to have an electron configuration of a noble gas. f. As you go across the periodic table left to right, electronegativity will increase. g. The number of valence electrons an atom has is equal to the atomic number. h. Fluorine cannot be the central atom due to the fact that is can only accept 2 electrons. i. When a covalent bond occurs, the atoms overlap one another to create a new orbital. The more overlapping, the stronger the bond. j. A triple bond is considered to be a weak bond.