Covalent+Bonds

__**Directions:**__ a) list and define all vocabulary from the chapter b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.) c) link at least 3 websites for additional resources to help with studying d) develop your own LEQ questions for the section - what did you think were the key points we learned? e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper.) Lewis Dot Structure- are diagrams that show the bonding between atom. Electron Pairs- consists of two electrons that occupy the same orbital but have opposite spins. Single Bond- A covalent bond in which one electron pair is shared by two atoms. Double Bond -is a chemical bond between two chemical elements involving four bonding electrons instead of the usual two. Triple Bond -two chemical elements involving six bonding electrons instead of the usual two in a covalent single bond. Binary Covalent- are compounds made up of only two elements Electronegativity-the tendency of an atom or radical to attract electrons in the formation of an ionic bond Metallic, Ionic & Covalent Bond //-covalent// is usually between a nonmetal and nonmetal and usually isn't as strong as the other //bonds//. Polar-Having electrical or magnetic polarity Nonpolar-he type of bond that is formed when electrons spend as much time orbiting one nucleus as the other; thus, the distribution of charges is symmetrical. Intermolecular Force-are forces that act between stable molecules or between functional groups of macromolecules. Linear-are forces that act between stable molecules or between functional groups of macromolecules. Bent-can be applied to certain molecules to describe their molecular geometry. H2O is an example of a bent molecule. The bond angle between the two hydrogen atoms is approximately 104.45° Trigonal Planar-a molecular geometry model with one atom at the center and three atoms at the corners of a triangle, called peripheral atoms- as unshared pairs, starting with the most electronegative such atom. Pyramidal- is a molecular geometry with one atom at the apex and three atoms at the corners of a trigonal base. Tetrahedral- a central atom is located at the center with four substituents that are located at the corners of a //tetrahedron//. Bond Angle-Angle from a pair of bonded atoms to another atom, one of the bonded pair being the vertex Bond Length-bond length or bond distance is the average distance between nuclei of two bonded atoms in a molecule. Bond Axis- is the imaginary straight line that connects the nuclei of atoms bonded to each other in a molecule. VSEPR Model -The Valence Shell Electron Pair Repulsion (VSEPR) //model//: is based on the number of regions of high electron density around a central atom.

Dinitrogen pentaoxide-N2O5 Boron Trifluoride-BF3 Hypochlorite-HSO4^ -1 Nitrite-NO2^ -1

The elements are listed by which is in the lower group if both elements are in the same group the lower atomic # element is the first of the bond. The second bond will always end in -ide. Prefixes are used to tell how many atoms are in the bond such as mono, bi, and tri. The first element will only have a prefix if there is more than one. LEQ: How do you classify a bond type?

http://academic.brooklyn.cuny.edu/biology/bio4fv/page/covalenb.htm http://sixthsense.osfc.ac.uk/chemistry/bonding/covalent.asp http://www.visionlearning.com/library/module_viewer.php?mid=55