1. Naming Ionic Compounds
NaF -
LiCl -
MgO -

2. Naming Ionic Compounds
Naming Ionic Compounds
NaF- Sodium Ion and Fluoride ion
LiCl- Lithium Ion and Chloride Ion
MgO- Magnesium Ion and Oxide Ion

3. Naming Ionic Compounds
Naming Ionic Compounds
NaF - Sodium Fluoride
LiCl - Lithium Chloride
MgO - Magnesium Oxide

4. More Practice Cd(OH)2 Na2SO4 Cadmium Sodium Sulfate Hydroxide Na2SO3
More Practice
Cd(OH)2
Cadmium
Hydroxide
Ca(ClO)2
Calcium
Hypochlorite
AgCN
Silver Cyanide
Na2SO4
Sodium Sulfate
Na2SO3
Sodium Sulfite
KClO4
Potassium
Perchlorate

5. Ions You Should Know

6. Properties of Molecular & Ionic Compounds

7. Chemical Substances; Formulas and Names
Naming simple compounds
Chemical compounds are classified as organic or inorganic.
Organic compounds are compounds that contain carbon combined with other elements, such as hydrogen, oxygen, and nitrogen; they do not contain metals.
Inorganic compounds are compounds composed of elements other than carbon and usually contain at least one metal atom. 2

8. Chemical Formulas; Molecular Substances
Organic compounds
An important class of molecular substances that contain carbon is the organic compounds.
Organic compounds make up the majority of all known compounds.
The simplest organic compounds are hydrocarbons, or compounds containing only hydrogen and carbon.
Common examples include methane, CH4, ethane, C2H6, and propane, C3H8. 2

9. Naming Covalent Compounds
Naming Covalent Compounds
A covalent compound as we said before is formed by sharing electrons between 2 nonmetals or metalloids.
These compounds are usually molecular and are named using a prefix system.
When naming these compounds name the element further to the left (in the periodic table) first, then the one on the right. 2

10. Naming Covalent Compounds
You name the first element using the exact element name.
Name the second element by writing the root of the element’s name and add the suffix “–ide.”
If there is more than one atom of any given element, you add the Greek prefix denoting how many atoms of that element are present. Table lists the Greek prefixes used.
If only one atom of the second element is present it gets the prefix “mono” 2

11. Naming Covalent Compounds
Here are some examples of prefix names for binary molecular compounds.
PF5 phosphorus pentafluoride
SO2 sulfur dioxide
SF6 sulfur hexafluoride
N2O4 dinitrogen tetroxide
CO carbon monoxide 2

12. Naming Acids
Acids are traditionally defined as compounds that could donate an H+; however, they are acids only in the presence of water. In other words before they enter the liquid they are covalent compounds and they are NOT acids.
There are two main types of acids:
Binary acids consist of a hydrogen ion and any single anion. For example, HCl is hydrochloric acid.
An oxoacid is an acid containing hydrogen, oxygen, and another element. An example is a HNO3, nitric acid. (see Figure 2.23) 2

13. Naming Acids Binary Acids Oxoacids
Start with the prefix “Hydro” which represents the Hydrogen, followed it with the root of the name of the second element and append the ending –oic acid.
Oxoacids
Use the root of the “E” element if the ion taking part in the acid had an ending in –ate to the root append the ending –ic acid, if it ends on –ite then append the ending –ous acid. If the ion had a prefix use the same prefix.

14. Naming Acids Examples: HCl(g) Hydrogen Chloride
HCl(aq) HydroChloric Acid
H2S(g) Dihydrogen Sulfide
H2S(aq) HydroSulfic Acid
H3PO4(aq) Phosphoric Acid
HClO4(aq) Perchloric Acid
HClO(aq) Hypochlorous Acid

15. Ionic Compounds Formulas
Ionic Compounds Formulas
How do we know how many atoms of each ion we need?
A simple crossing of the charges can answer that question about 90% of the time.
Example: Mg2+ and PO43-
Mg3(PO4)2
Check the charges… 3 x (+2) = +6
2 x (-3) = -6
When they combined they cancel to yield a neutral compound.

16. Ionic Compounds Formulas
Ionic Compounds Formulas
The crossing technique does not work if the magnitude of the charges is the same
Example: Mg2+ and CO32-
Mg2(CO3)2
This is incorrect since we want the lowest ratio possible which is 1:1 to yield MgCO3

17. Ionic Compounds Properties
Ionic compounds have properties completely different from their component elements.
Example: Table Salt (NaCl)
Sodium (Na) in the presence of water reacts violently heating up the water and producing hydrogen if the temperature of the water is high enough the hydrogen can ignite explosively.
Chloride (Cl) Green poisonous and corrosive gas. If inhaled will destroy the nasal passages then dissolve in the stomach producing high concentration of hydrochloric acid which will destroy the stomach lining producing ulcers.
Salt (NaCl) posses none of the properties mentioned above.

18. Ionic Structure Ions form a 3-D lattice.
The coulombic (electrostatic) attraction is so high that in order to separate one ion from the lattice requires a lot of energy (DHlatt).
The lattice energy depends on charge and size of the ions.

19. Lattice Energy
Since the lattice energy is an electrostatic interaction the more separated the charges are the weaker the interaction is.
Bigger ions have lower lattice energies
The higher the charge of the ions the stronger they will attract ions of the opposite charge.
When size and charge point to opposite trends the charge will outweigh the size.
From smallest atom to biggest atom there is only 1.7x factor. From a +1 to +2 that is already a 2x factor.

20. Properties of Ionic Substances
Dues to the charged interaction a blow to a crystal leads to the possibility of splitting the crystal since we will force like charged particles to interact.
Ionic compounds have high melting/boiling points since in order to move the ions from their respective spots it will require breaking the lattice.

21. Ionic Solutions
However, if we do melt an ionic compound it will be able to conduct current.
When ionic compounds are placed in a solvent the produced solution conducts electricity. The higher the number of ions the higher the conductivity.
More when we cover chapter 4.

22. Naming Hydrates
A hydrate is a compound that contains water molecules weakly bound in its crystals.
Hydrates are named from the anhydrous (dry) compound, followed by the word “hydrate” with a Greek prefix to indicate the number of water molecules per formula unit of the compound.
For example, CuSO4. 5H2O is known as copper(II)sulfate pentahydrate. (see Figure 2.24) 2

23. Determining Chemical Formulas
Determining both empirical and molecular formulas of a compound from the percent composition.
The percent composition of a compound leads directly to its empirical formula.
An empirical formula (or simplest formula) for a compound is the formula of the substance written with the smallest integer (whole number) subscripts. 2

24. Determining Chemical Formulas
The percent composition of a compound is the mass percentage of each element in the compound.
We define the mass percentage of “A” as the parts of “A” per hundred parts of the total, by mass. That is, 2

25. Mass Percentages from Formulas
Let’s calculate the percent composition of butane, C4H10.
First, we need the molecular mass of C4H10.
Now, we can calculate the percents. 2

26. Determining Chemical Formulas
Determining the empirical formula from the percent composition.
Benzoic acid is a white, crystalline powder used as a food preservative. The compound contains 68.8% C, 5.0% H, and 26.2% O by mass. What is its empirical formula?
In other words, give the smallest whole-number ratio of the subscripts in the formula
Cx HyOz 2

27. Determining Chemical Formulas
Determining the empirical formula from the percent composition.
For the purposes of this calculation and making calculations simpler, we will assume we have grams of sample benzoic acid.
Then the percentage of each element equals the mass of each element in the sample.
Since x, y, and z in our formula represent mole-mole ratios, we must first convert these masses to moles. 2

28. Determining Chemical Formulas
Determining the empirical formula from the percent composition.
Our grams of benzoic acid would contain:
This isn’t quite a whole number ratio, but if we divide each number by the smallest of the three, a better ratio might emerge. 2

29. Determining Chemical Formulas
Determining the empirical formula from the percent composition.
Our grams of benzoic acid would contain:
now it’s not too difficult to see that the smallest whole number ratio is 7:6:2. The empirical formula is C7H6O2 . 2

30. Determining Chemical Formulas
Determining the “true” molecular formula from the empirical formula.
An empirical formula gives only the smallest whole-number ratio of atoms in a formula.
The “true” molecular formula could be a multiple of the empirical formula (since both would have the same percent composition).
To determine the “true” molecular formula, we must know the “true” molecular weight of the compound. 2

31. Determining Chemical Formulas
Determining the “true” molecular formula from the empirical formula.
For example, suppose the empirical formula of a compound is CH2O and its “true” molecular weight is 60.0 g/mol.
The molar weight of the empirical formula (the “empirical weight”) is only 30.0 g/mol.
This would imply that the “true” molecular formula is actually the empirical formula doubled 2(CH2O) or
C2H4O2 2

32. Molecular and structural formulas and molecular models.
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33. A model of a portion of a Sodium Chloride crystal.
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34. Common Ions of the transition metals
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35. List of Polyatomic Ions
List of Polyatomic Ions
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36. Greek Prefixes for Covalent Compounds Nomenclature
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37. Making and Acid
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38. Molecular model of nitric acid.
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39. Figure 2.24: Copper (II) sulfate. Photo courtesy of James Scherer.
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40. Naming Flow Chart
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41. Naming Flow Chart II
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42. Naming Acids Flow Chart
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