Experiment 12- Molecular Geometries of Covalent Molecules: Lewis Structures and the VSEPR Model Flashcards

Set Details Share
created 6 years ago by brianquintero1
updated 6 years ago by brianquintero1
show moreless
Page to share:
Embed this setcancel
code changes based on your size selection

Purpose of Experiment 12

become familiar with:

1. Lewis structures

2. principles of the VSEPR model

3. the three-dimensional structures of covalent molecules


chemical bond

when atoms or ions are strongly attached to one another


Three types of chemical bonds

1. ionic

2. covalent

3. metallic


Ionic bond

- electrostatic forces btwn ions of opposite charge

- formed by transfer of one or more electrons

- from atom of low ionization energy to atom of high ionization energy

usu metals with nonmetals (except noble gases)


Covalent bond

sharing of electrons between two atoms

More familiar exs= bonds among nonmetallic elements


Metallic bonds

found in metals like gold, iron, magnesium

each atom is bonded to several neighboring atoms

give rise to high electrical and thermal conductivity

b/c in m bonds electrons are relatively free to move throughout the 3D shapes of mc's


Which electrons are involved in bonding

valence electrons (reside in incomplete outer shell of an atom)


creator of Lewis Dot structure

G.N. Lewis, American chemist


Lewis symbol consists of:

chemical abbreviation for the element

and a dot for each valence electron

each side accommodates up to two electrons


What can atoms do to achieve noble gas config?

gain, lose, or share electrons


octet rule

atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons

octet of electrons= full s and p subshells


Properties of ionic substances

(most substances do not have these characteristics)

usually brittle

high melting point

crystalline solids w/ well-formed faces

- characteristics result from electrostatic forces that maintain ions in a rigid, well-defined, 3D arrangement


Example of how H2 forms a bond

- the nuclei and electrons cause electron density to concentrate btwn the nuclei

- the shared pair of electrons acts as a kind of "glue" holding the atoms together


single bond

double bond

sharing of one pair of electrons

sharing of two pairs of electrons

- triple bond is the sharing of three pairs of electrons


Steps for drawing Lewis dot structures

1. Sum the number of valence e-

a. add electrons for negative charges

b. subtract electrons for positive charges

2. Decide the central atom (least electronegative excluding H)

3. Assign leftover electrons to the terminal atoms until all octet

4. Assign any leftover e- to the central atom (if central atom doesn't have octet, create multiple bonds)


Why formal charge?

sometimes can draw several diff Lewis structures that all obey the octet rule

formal charge helps decide the structure that is the most reasonable


formal charge (of an atom)

the charge that an atom in a molecule or ion would have if all atoms had the same elcectronegativity


equation for formal charge

(regular valence e-) - (valence e- found in the molecule)

* remember to count only one of the two bonded molecules for each bonded atom


Most bonds btwn two diff kinds of atoms are usually...



Why are most bonds of two diff atoms usu polar?

b/c diff atoms have diff electronegativities (so electrons are not shared equally by the two bonded atoms)