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Ionic Compounds Ionic Compounds
Chapter 5
Chapter 5 2
Classification of Compounds
Chapter 5 3
Chemical Nomenclature
- The term “nomenclature” come from the Latin word meaning
“calling by name”.
- Chemical Nomenclature is a system for naming chemical
compounds.
- In this chapter we will learn a system for naming compounds
from their formula and writing the chemical formula from the
name.
- You will have to memorize some things (polyatomic ions for
example), but if you learn the system, you will be able to name
numerous chemical compounds by only seeing the formula.
- Do be successful you must LEARN THE SYSTEM!!!
Chapter 5 4
Valence Electrons
- When an atom undergoes a chemical reaction, only the outermost electrons are involved.
- These electrons are of the highest energy and are furthest away from the nucleus. These are the valence electrons.
- The valence electrons are the s and p electrons beyond the noble gas core.
Chapter 5 5
Predicting Valence Electrons
- The Group number indicates the number of
valence electrons.
Chapter 5 6
Electron Dot Formulas
- An electron dot formula of an elements shows the symbol
of the element surrounded by its valence electrons.
- We use one dot for each valence electron.
- Consider phosphorous, P, which has 5 valence electrons.
Here is the method for writing the electron dot formula.
Chapter 5 10
Monoatomic Cations
- Metals form cations with octets by losing all of their valence electrons
- These cations have the same electron configuration as the nearest noble gas (the one at the end of the row above!)
- Cations have fewer electrons than protons
Group 1A metals ⎯→ ion 1+ Group 2A metals ⎯→ ion 2+ Group 3A metals ⎯→ ion 3+
- Cations are named for the parent metal followed by the word “ion”
Na +^ is the Sodium Ion
Ca 2+^ is the Calcium Ion
Chapter 5 11
- Some of the transition metals can form more than one cation
- These cations are named for the parent, followed by the charge
in Roman numerals in parentheses followed by the word “ion”.
Fe 2+^ is the iron(II) ion Fe 3+^ is the iron(III) ion
- This is called the Stock system of naming cations.
- Silver ion (Ag +^ ), Zinc ion (Zn 2+^ ), Nickel ion (Ni2+^ ) and
Cadmium ion (Cd2+^ ) are exceptions because they only form
one ion! Memorize these!
- You will always be able to determine the charge of a transition
metal from its name or formula!
Metals That Form Multiple Cations
Chapter 5 12
Monoatomic Anions
- Nonmetals form anions with full octets by gaining electrons
- These anions have the same electron configuration as the nearest noble gas (the one at the end of the row they are in!)
- Anions have more electrons than protons
Group 7A nonmetals ⎯→ ion 1- Group 6A nonmetals ⎯→ ion 2- Group 5A nonmetals ⎯→ ion 3-
- Monoatomic anions are named by dropping the end of the element name and adding the suffix – ide.
Br-^ is the bromide ion
O 2-^ is the oxide ion
N 3-^ is the nitride ion
Chapter 5 13
Polyatomic Ions
- A Polyatomic Ions are a group of atoms that has an overall
charge
- These ions are generally anions and contain one or more
elements combined with oxygen
Chapter 5 14
Common Polyatomic Ions
You need to memorize the ones above!!
C 2 H 3 O 2 - Acetate Also look at Table 5.8 in Chapter 5!!
HCO 3 - Hydrogen Carbonate H 3 O+ Hydronium
CO 3 2- Carbonate NH 4 + Ammonium
PO 4 3- Phosphate CrO 4 2- Chromate
CN - Cyanide Cr 2 O 7 2- Dichromate
SO 3 2- Sulfite MnO 4 - Permanganate
SO 4 2- Sulfate OH- Hydroxide
NO 2 - Nitrite ClO 3 - Chlorate
NO 3 - Nitrate ClO 4 - Perchlorate
Symbol Name Symbol Name
Chapter 5 15
Ionic Compounds
- Ionic compounds consist of positive and negative ions.
- An ionic bond is an attraction between the positive and
negative charges.
- In an ionic formula, the total charge of the positive ions is
equal to the total charge of the negative ions.
total positive charge = total negative charge
Chapter 5 19
Naming Binary Ionic Compounds
Chapter 5 20
Naming Binary Ionic Compounds:
Transition Metals
Reverse the criss-cross!
Fe
O
Fe
O
Chapter 5 21
Practice, Practice, Practice!!!!
Silver permanganate _________________
Cadmium sulfide ______________________
Cobalt (III) iodide _________________
Zinc sulfate _________________
Barium fluoride _________________
Sodium acetate _________________
