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)

a.) **__LEQ: How can I draw a bond using electrons? How can I name a covalent bond?__** Lewis Dot Structure- element symbol that represents the nucleus, inner electrons, & surrounding dot represent the valence electrons

Electron pairs- two electrons that occupy the same orbital but have different spins

Single bond- Shares two electrons; single bonding pair of electrons

Double bond- shares 4 electrons; two bonding electron pairs

Triple bond- shares 6 electrons; three bonding pairs

Binary covalent- the combination of two elements, usually nonmetals

Bromine has three electron pairs & 1 lone electron; it needs only one more electron to become stable

Chlorine also only needs one more electron to become stable

Aluminum has three lone electrons, so to become stable it needs to bond three different times

Oxygen has two electron pairs & 2 lone pairs; it needs to bond two times to become stable

http://www.ausetute.com.au/lewisstr.html http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/perlewis.html http://misterguch.brinkster.net/covalentcompounds.html

__**LEQ: How can I classify a bond type?**__ Electronegativity- how strong bonds are within a compound

Ionic bond- bonds between metals & non-metals; atoms with large differences in their tendencies to lose or gain electorns

Covalent bond- bonds between nonmetals & non-metals; atoms that have small differences in their tendencies to lose or gain electrons

Metallic bond- bonds between metals & metals; lose their valence electrons but do not gain them, so the electrons "flow" between the atoms (back & forth)

Polar- unequal distribution of electron density, the bond has partial negative & partial positive poles

Non-polar- atoms are identical, bonding pair is share equally

Organic compound- carbon is nearly always bonded to itself and hydrogen & often to other elements

Inorganic compound- any compund that does not contain carbon

Intermolecular force- the atrractive & repulsive forces among patricles in a sample of matter

This is an ionic bond because Na is a metal with only one electron & it bonds with Chlorine, a non-metal, who needs only one more elctron to have a full outershell

This is a covalent bond because they are both non-metals

Electronegativity trends

http://www.chemteam.info/Bonding/Electroneg-Bond-Polarity.html dept.sfcollege.edu/natsci/chem/chm2labs/**BondTypes**.pdf http://staff.jccc.net/pdecell/chemistry/bonds.html

__**LEQ: How can I predict the 3-D shape of molecules?**__ Linear- 0 unbonded pairs around the central element 2 locations bonded to central Hybridization: sp Trigonal Planar- 0 unbonded pairs around central element 3 locations bonded to central Hybridization: sp2 Bent- 2 unbonded paris around central element 2 locations bonded to central Hybridization: sp3 Pyramidal- 1 unbonded pari around central element 3 locations bonded to central Hybridization: sp3 Tetrahedral- 0 unbonded pairs around central element 4 locations bonded to central Hybridization: sp3

Bond angle- the angle formed by the nuclei of two surrounding atoms with nucleus of the central atom at the vertex

VESPR model- predicts the 3-D shape of a molecule http://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/intro3.htm http://library.thinkquest.org/C006669/data/Chem/bonding/shapes.html http://intro.chem.okstate.edu/1314f00/lecture/chapter10/vsepr.html



Tetrahedral: 0 unbonded pairs, 4 bond locations around central element

trigonal planar: 0 unbonded pairs, 3 bond locations around ccentral

bent: 2 bon locations, the unbonded pairs aren't shown