Chapter 13: Bonding 1 Flashcards
Valence electrons
eletrons in a shell with the highest n) play a funademental role in bonding
Electrons transfer from one atom to another is called
ionic bonds
When one or more pairs of electrons are shared
A covalent bond
Purpose of sharing electrons
To give each atom a Noble gas configuaration with eight valence electrons, called octet
Determining if a molecule is polar or non-polar is.
Determine the geometry of the molecule if there is symmetry and bond polars cancel each other out (symmetric charge distribution extra lone pairs on one of the molecules leads to unbalance) than they are non-polar, but if they are non-symmetrical then they are polar. You would consider the bonding and lone pair electrons.
When sketching a lewis bond-pair
The total of electrons should match up to the total number of valence electrons to original
Remember when considering the molecular geometry of Lewis structures
That the double bonds don’t add to the total bonds you will need to consider for molecular geometry shape. For example if there is 2 one bond and one 2 bonded pair then it would just count as 3 = trigonal planar
Remember the degrees in geometry.
tetrahedral = 109.5
triagonal planar = 120
Linear = 180
Finding Bonding order
Find the number of bonds in the electron structure and divide it by the number of domains
Ex: NO3^-
How do you find what bond is the most ionic
By electronegativity difference
How do I find what is the most polar bond
By electronegativity difference
dipole moment
There is a separation in charge can occur between two ions in an ionic bond or between two covalent bonds.
Electronegativity differences
less than 0.4 is covalent.
0.5 to 2.0 is polar covalent.
2.0 < is ionic.
Past group 3 past the element of phosphorus means…
This can allow for expanded octects
