Notes 

Chemistry Chapter 7 Notes(p.165-194)

Read page 191 for the five facts.

Chemical bond:

the force that holds two or more atoms together

Cation:

positively charged ion

Anion:

negatively charged ion

Ionic bond:

electrostatic force that holds oppositely charged particles together in an ionic compound

Ionic compounds: (Formula Units)

compounds that contain ionic bonds

Crystal lattice:

a three-dimensional geometric arrangement of particles

Electrolyte:

an ionic compound whose aqueous solution conducts an electric current

Lattice energy:

the energy required to separate 1 mol of the ions of an ionic compound

Turn to page 179. 

What do you notice about the lattice energy?

Why do they have different lattice energies?  Think about electronegativities!

Formula unit:

represents the simplest ratio of the ions involved

Monoatomic ion:

a one-atom ion

Oxidation number (oxidation state): the charge of a monatomic ion

Polyatomic ions:

ions that are made up of more than one atom

Oxyanion:

a polyatomic ion composed of an element , usually a nonmetal, bonded to one or more oxygen atoms

Electron sea model:

proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons

Delocalized electrons:

free to move electrons

Metallic bond:

the attraction of a metallic cation for delocalized electrons

Alloy:

 a mixture of elements into the metallic properties (A metal plus something else.)

A) Substitutional Alloys=

Results as atoms of one metal are replaced with another element.

B) Interstitial Alloys=

Results when the spaces between metal atoms are filled with other atoms.

Things to remember

Ending –ide think negative and right side of periodic table.

Ending –ate  and –ite think negative and common polyatomic ion.

If the first element is a metal, use the formula unit naming method.

(Do not use the term for the subscript.)

If there are more than two different types of elements, use the common polyatomic ion chart. (p. 183)

Naming Formula Units:(Metals from the Shell S and P)

1.Write the name of the first element.

2. Write the name of the second element with the ide ending.

Ex.  CaCl2

Calcium Chloride

Naming Formula Units:(Metals from the Shell d)

1. Write the name of the first element.

2. Write the charge in Roman numerals.

3. Write the name of the second element with the ide ending.

Example

CuO

Copper(II) Oxide

Naming Formula Units:(With S and P metals and polyatomic ions)

1. Write the name of the first element.(Follow the rules based on the location of the metal.)

2. Write the name of the polyatomic ion.

K2HPO4

Potassium Hydrogen Phosphate

Naming Formula Units:(With d metals and polyatomic ions)

1. Write the name of the first element.

2. Write the charge in Roman numerals.

3. Write the name of the polyatomic ion.

Fe(NO3) 2

Fe   NO3-1

  +2 -2=0

 Iron(II) Nitrate

Extra information

Only two different # of Oxygen atoms that are bonded

-ite Less Oxygen atoms

-ate  More Oxygen atoms

If there are four different # of Oxygen atoms bonded to another element:

Hypo  (less than)  Lowest # of O

-ite Second lowest # of O

-ate  Third lowest # of O

per (more than) Highest # of O