1. Chapter 5
Types of Compounds

2. Section 5.1
Ionic Compounds

3. Binary Compounds A compound that contains only two elements. Example:
Sodium chloride (NaCl)
Potassium Iodide (KI)
Calcium fluoride (CaF2)

4. Naming Binary Compounds
First write the name of the positively charged ion (metal)
Then add the name of the negatively charged ion, (nonmetal)
Change the ending of the nonmetal’s name to include “ide”
Example:
NaCl (sodium chlorine)
sodium chloride
(The metal is always written first)

5. (don’t worry about the subscripts for now)
Check Point
Complete the names of the following binary compounds:
Na3N sodium ________________
MgBr2 magnesium ________________
Al2O3 aluminum ________________
CaS _________ _______________
(don’t worry about the subscripts for now)

6. Binary Compound Formulas
Compounds are electrically neutral.
The sum of the charges in an ionic compound are neutral.
Example:
In the compound NaCl
One Na+ balances out one Cl -

7. Formula Unit
The lowest whole number ratio of ions in an ionic compound.
Ionic compounds do not form molecules.

8. Predicting Charges
A neutral atom becomes “charged” when it has lost or gained valence electrons.
All elements in a group have the same number of valence electrons so they must lose or gain the same number of electrons to achieve stability.
Charges on an ion are known as its oxidation number.
Group numbers can be used to predict charges.

9. Charges for Groups

10. Predict the charges of the following elements:
Check Point
Predict the charges of the following elements:
Mg _________
S _________
Li _________
Al _________

11. The Criss-Cross Method
1. Write the element’s symbol for the metal (cation) and the nonmetal (anion).
Al S
2. Use a superscript for the charge (+/-) of each ion.
Al S - 2

12. 3. Criss-cross the superscript of the cation to the subscript position of the anion (disregard the positive sign).
4. Criss-cross the superscript of the anion to the subscript position of the cation (disregard the negative sign).

13. 4. Rewrite your final answer. 5
4. Rewrite your final answer. 5. If possible, divide the subscripts by their greatest common factor to reduce to simplest whole ratio. Example: Ni4O2 Ni2O

14. Write the formula for the following compounds:
Check Point
Write the formula for the following compounds:
Sodium and Sulfur _________
Magnesium and Bromine _________
Aluminum and Oxygen _________

15. Polyatomic Ions An ion that has two or more different elements.
The group of atoms has an overall charge.
The names and formulas for these ions are found on the back of your periodic table.
The ending of polyatomic ions does not get changed.

16. Polyatomics

17. Formulas w/ Polyatomic ions
Treat the polyatomic ion as if it was a single element by keeping it together as a unit (that includes its subscripts).
Multiples of a polyatomic ion in a formula can be indicated by placing parentheses around the entire ion (including its subscripts) and then writing a new subscript outside of the parentheses to show the number of polyatomic ions.

18. Practice Write the formula for aluminum sulfate:
Criss-Cross (don’t touch the ”4” subscript in the sulfate).
Use parentheses in your final answer.

19. Write the formula for the following compounds:
Check Point
Write the formula for the following compounds:
Sodium and carbonate _________
Magnesium and hydroxide _________

20. Transition Metals & Charges
Many transition metals may have more than one charge.
Since many transition metals can have more than one possible charge they MUST have a Roman Numeral to indicate the charge on the individual ion.
Example:
Fe2+ iron(II) ion
Fe3+ iron(III) ion

21. Roman Numerals Number Roman Numeral 1 I 2 II 3 III 4 IV 5 V 6 VI 7 Vii8
Viii 9 IX 10 X

22. Check Point Indicate the charge on the following:
Copper (II) _________
Iron (III) _________
Indicate the name of the following:
Ni _________
Pb _________

23. Lead (II) chloride _________ Iron (III) oxide _________
Check Point
Write the formula:
Lead (II) chloride _________
Iron (III) oxide _________
Copper(I) sulfite _________

24. Write the names of the following compounds:
Check Point
Write the names of the following compounds:
FeBr2 _________
Fe2O3 _________
CuCl _________

25. Hydrates
A hydrate is a compound in which there is a specific ratio of water to the ionic compound.
Water molecules are chemically bonded to the ionic compound.

26. Hydrates
Hygroscopic : A compound that easily absorbs water from the air.
Deliquescent: A substance that is so hygroscopic that it takes up enough water from the air to dissolve completely and form a liquid solution.

27. Hydrates
Anhydrous: A compound in which all of the water has been removed.
Heating hydrates can remove the water in the compound.
These compounds may become a different color than when it was a hydrate.
TEXTBOOK PAGE 165

28. Hydrate Formula
Because water is part of a hydrate (not just surrounding it) the formula is written in a special way.
The name for the compound is written and then a “dot” is placed followed by the number of water molecules in the compound.
The dot in the formula represents a ratio of compound formula units to water molecules.

29. Hydrate Formula
To name a hydrate, first write the name of the regular compound.
Then add a prefix to the word hydrate to indicate the number of water molecules present.
Example :
CuSO4•5H2O
copper(II) sulfate pentahydrate

30. Hydrate Prefixes

31. Check Point Write the names of the following hydrates:
BaCl2•2H2O _________
Na2CO3•H2O _________
Write the formula for the following hydrates:
Calcium sulfate dihydrate _________
nickel(II) sulfate hexahydrate _________

32. Section 5.2 Covalent Compounds

33. Distillation A method of separating substances.
A solid may be separated from a liquid.
One liquid may be separated from another liquid.

34. Molecular Element
A molecule that forms when atoms of the same element bond together.
These atoms bond together to achieve stability.

35. Hydrogen Oxygen Nitrogen Cl (chlorine) Bromine Iodine Fluorine
7 Diatomic Molecules
Hydrogen Oxygen Nitrogen Cl (chlorine) Bromine Iodine Fluorine
H2 O2 N2 Cl2 Br2 I2 F2

37. Allotropes of Phosphorus
Molecules of a single element that differ in crystalline or molecular structure.
The properties of allotropes are usually different even though they contain the same element.
Structure can be more important than composition in determining the properties of molecules.
Allotropes of Phosphorus

38. Got Carbon? Organic Compound: Compounds that contain carbon.
Inorganic Compound: Compounds that do not contain carbon.

39. Naming Covalent Compounds
Write out the name of the first nonmetal.
Write the name of the second nonmetal changing its ending to “ide”.
Add a prefix to the name of each element to indicate how many atoms of each element are present.

40. Naming Covalent Compounds
Write the element that is farther to the left in the periodic table first.
If both elements are in the same group, name the element that is closer to the bottom of the table first.
If there is only one atom of the first element listed , the prefix mono is omitted.
If there are vowel combinations such as o-o or a-o next to each other in the name, the first vowel is omitted to simplify pronunciation.
Example: mononitrogen monoxide

41. PREFIXES ARE ONLY USED WITH COVALENT COMPOUNDS
(NOT IONICS)

42. Check Point Write the names of the following : CCl4 _________
N2O _________
Write the formula for the following :
sulfur hexafluoride _________
tetraphosphorus decoxide _________

43. Common Acids
TEXTBOOK PAGE 180

44. Naming Acids Acids Examples: Compounds that form H+ in water.
Formulas usually begin with ‘H’.
Examples:
HCl (aq) – hydrochloric acid
HNO3 – nitric acid
H2SO4 – sulfuric acid

45. Naming Acids “An easy way to remember which goes with which…
No Oxygen
w/Oxygen
“An easy way to remember which goes with which…
In the cafeteria, you ATE something ICky”

46. Acid Nomenclature Flowchart

47. Acid Nomenclature HBr (aq)  hydrobromic acid H2CO3 H2SO3
 carbonic acid
Has oxygen, -ate
Has oxygen, -ite
 sulfurous acid

48. Naming Acids hydrofluoric acid sulfuric acid nitrous acid  H+ F-
2 elements
 H+ F-
 HF (aq)
3 elements, -ic
 H+ SO42-
 H2SO4
3 elements, -ous
 H+ NO2-
 HNO2

49. Check Point HI (aq) __________ HCl __________ H2SO3 __________
Name the following acids:
HI (aq) __________
HCl __________
H2SO __________
HNO __________

50. Check Point Hydrobromic acid _______ Nitrous acid _______
Write the formula for the following acids:
Hydrobromic acid _______
Nitrous acid _______
Carbonic acid _______
Phosphoric acid _______

51. Hydrocarbons
TEXTBOOK PAGE 180