22.3 – Writing formulas for Ionic Compounds Part A Focus on what is in PINK.
-
Upload
jeffery-blankenship -
Category
Documents
-
view
212 -
download
0
Transcript of 22.3 – Writing formulas for Ionic Compounds Part A Focus on what is in PINK.
22.3 – Writing formulas for Ionic Compounds
Part A
Focus on what is in PINK
Objectives
Write formulas for ionic compounds
Writing Ionic Formulas
Watch the Tyler DeWitt Video and complete the viewing guide, you will add it to your notes on this chapter
Youtube video
Binary Ionic Compounds
• A compound composed of 2 elements• To write a chemical formula for a
binary compound, you need to know:• which elements are involved• how many electrons they lose or gain to
become stable
Ionic Compounds are NEUTRAL
• Although the individual ions in a compound carry charges, the compound itself is neutral
• A formula must have the right number of positive ions and the right number of negative ions so the charges balance
Oxidation Number
The number of electrons an atom must gain, lose or share to become stable Cations = lose electrons Anions = gain electrons
Oxidation Number
Determined by which group the element is in and how many valence electrons it has
Valence electrons = The BONDING electrons found in the outermost energy level
Oxidation Number
Group 1 = 1 valence electron Loses 1 e- to become stable Ion = +1 charge
Group 2 = 2 valence electron Loses 2 e- to become stable Ion = +2 charge
Group 3 = 3 valence electron Loses 3 e- to become stable Ion = +3 charge
Oxidation Number
Groups 3-12 = Transition metals = variable # of electrons, unpredictable charges
Group 13 = 3 valence electron Loses 3 e- to become stable Ion = +3 charge
Oxidation Number
Group 14 = 4 valence electron Can gain or lose 4e- to become stable Ion = ±4 charge
Group 15 = 5 valence electron Gains 3e- to become stable Ion = -3 charge
Group 16 = 6 valence electron Gains 2e- to become stable Ion = -2 charge
Oxidation Number
Group 17 = 7 valence electron Gains 1e- to become stable Ion = -1 charge
Group 18 = *8 valence electron STABLE No charge, no ions
Oxidation #/Charges of Ions
Write Formulas for these ions
Potassium ion
Magnesium ion
Oxide (oxygen) ion
K+
Mg 2+
O 2-
Transition Elements
• Can have multiple oxidation numbers
• Express using Roman numerals
• For example, the oxidation number of iron in
iron (III) oxide is 3+.
Write Formulas for these ions
Copper (I) ion
Chromium (VI) ion
Mercury (II) ion
Cu 1+
Cr 6+
Hg 2+
Step By Step – Writing Formulas
1. Write the symbol of the element with the positive oxidation number or charge
2. Write the symbol of the element with the negative oxidation number or charge
3. The charge (without the sign) of one ion becomes the subscript of the other ion. • Reduce the subscripts to the smallest whole
numbers that retain the ratio of ions.
Criss-Cross Method
Writing Formulas
Write the formula for calcium chloride. Calcium is Ca+2 Chloride is Cl-1
Ca+2 Cl-1 Cl-1
CaCl2
In-Class Assignment/Homework
PS 22.3 A WKT 1 - Criss Cross practice