1. Ch. 7-1
Naming Compounds
Names & Formulas

2. POINT > Name and identify the charge of monatomic ions
POINT > Define and determine formulas for binary compounds
POINT > Define and name polyatomic ions

3. POINT > Name and identify the charge of monatomic ions
Metals in Groups 1A, 2A, 3A lose electrons forming (+) charged cations
The atoms lose the number of electrons needed to fulfill the octet rule (Noble gas config)
The cation name is the same as the atom, followed by ion or cation (ex. Na+ = sodium ion)

4. WB CHECK: Write the symbol and name of the ion formed by:
Lithium  Li+ lithium ion
Calcium 
Aluminum 
Potassium 

5. POINT > Name and identify the charge of monatomic ions
Nonmetals gain electrons forming (-) charged anions
The ions gain the number of electrons needed to fulfill the octet rule (Noble gas config)
The name of the anion is the stem of the element name, ending in -ide (ex. O2- = oxide ion)

6. WB CHECK: Write the symbol and name of the ion formed by:
Chlorine  Cl- chloride ion
Phosphorus 
Sulfur 
Nitrogen 

7. POINT > Name and identify the charge of monatomic ions
Many transition metals can form more than one cation, each having a different ionic charge Ex. Iron cation could be Fe2+ or Fe3+ Charge must be determined based on the name or formula of a compound (can’t just use group numbers…)

8. POINT > Name and identify the charge of monatomic ions
Stock system for naming transition metal cations:
Roman numerals after the name indicate the charge
Ex. Iron: Fe2+ written as iron(II) ion
Fe3+ written as iron (III) ion

9. POINT > Name and identify the charge of monatomic ions
Classical system for naming transition metal cations:
Latin (or other) root/suffix indicates the charge:
-ic refers to higher charge, -ous refers to lesser charge
Ex. Iron: Fe2+ written as ferrous ion
Fe3+ written as ferric ion

10. POINT > Define and determine formulas for binary compounds
Binary compounds are composed of two elements
Ex. H2O HCl CO2 NaCl NH3
If the compound is ionic, the cation is written first and the charges of the ions must be balanced

11. POINT > Define and determine formulas for binary compounds
Ex. Determine the name and formula of a compound of iodine and magnesium Iodide ion is I- and magnesium ion is Mg2+ Two I- are needed to balance with one Mg2+ So formula unit would be MgI2 = magnesium iodide

12. WB CHECK: Determine the formula and name of a compound of: oxygen and potassium iron(II) and chlorine sulfur and copper(I) strontium and nitrogen bromine and lithium

13. POINT > Define and determine formulas for binary compounds
Because compounds are electrically neutral, you can determine the formula of an ionic compound this way:
The charge on the cation becomes the subscript on the anion
The charge on the anion becomes the subscript on the cation

14. POINT > Define and determine formulas for binary compounds
If these subscripts are not in the lowest whole-number ratio, divide them by the greatest common factor

15. WB CHECK: What is the formula unit of: calcium flouride zirconium(I) carbide sodium sulfide aluminum oxide barium selenide

16. POINT > Define and determine formulas for binary compounds
All of the examples you just encountered were ionic compounds The charges in an ionic compound must balance, so to name them and determine formulas is straightforward.. Atoms in a binary molecular compound can combine in different ways (ex. CO and CO2, H2O and H2O2)

17. POINT > Define and determine formulas for binary compounds
Atoms in a binary molecular compound can combine in different ways (ex. CO and CO2, H2O and H2O2) To name binary molecular compounds use prefixes to show the number of each type of atom in the compound Ex. CO2 is carbon dioxide CO is carbon monoxide

18. POINT > Define and determine formulas for binary compounds
Rules for naming binary molecular compounds:
Confirm two nonmetals
Name elements in the order of formula
Use prefixes to indicate numbers
“mono” can be left out if it’s the first element Ex. CO2 is carbon dioxide, not monocarbon dioxide

19. POINT > Define and determine formulas for binary compounds
Rules for naming binary molecular compounds:
Second element must end in –ide
Ex. What is the name of N2Cl5?
dinitrogen pentachloride

20. WB CHECK: Write the name of the molecular compound: CO SO3 SO2 N2S3 K3F2

21. POINT > Define and determine formulas for binary compounds
To write the formula of a molecular compound, use the prefixes to identify the subscript of each element
Ex. Hexasulfur tetrachloride would be…
S6Cl4
Remember: Molecular formulas do not get reduced, because they indicate the actual number of atoms present in an actual molecule

22. Write the formula of the molecular compound: Phosphorus trichloride
WB CHECK:
Write the formula of the molecular compound:
Phosphorus trichloride
Dinitrogen tetroxide
Triselenium hexafluoride
Dihydrogen monoxide

23. POINT > Define and name polyatomic ions
Polyatomic ions are groups of atoms covalently bonded together that, as a whole, have a charge Ex. NO3- SO32- PO43- OH- NH4+ These form ionic bonds with other ions: Ex. NaNO3 MgSO3 Li3PO4 KOH NH4Cl Charges must balance, just as with ionic compounds

24. POINT > Define and name polyatomic ions
Most polyatomic ions are negatively charged and most contain oxygen Ex. NO3- SO32- PO43- OH- NH4+ These form ionic bonds with other ions: Ex. NaNO3 MgSO3 Mg3(PO4)2 Mg(OH)2 NH4Cl

25. POINT > Define and name polyatomic ions
Most polyatomic anions end in -ite or -ate -ite indicates fewer oxygen present -ate indicates more oxygen present Ex. SO32- = sulfite ion SO42- = sulfate ion ClO2- = chlorite ion ClO3- = chlorate ion

26. POINT > Define and name polyatomic ions
Sometimes there are more than two possible numbers of oxygen in a “family”
hypo- is added as prefix when fewer oxygen are present (-ite remains as suffix)
ClO-
Hypochlorite

27. POINT > Define and name polyatomic ions
Sometimes there are more than two possible numbers of oxygen in a “family”
per- is added as prefix when more oxygen are present (-ate remains as suffix)
ClO4-
Perchlorate

28. POINT > Define and name polyatomic ions
Note: Adding/removing oxygen does not change the charge of the polyatomic ion Sometimes a hydrogen is a part of the polyatomic ion. If so, the name includes hydrogen and the charge is reduced by 1 Ex. sulfate = SO42- hydrogen sulfate = HSO4-

29. WB CHECK: PO53- PO42- PO33- PO32-
If a phosphate ion, PO43- has a charge of 3- then the formula and charge of a phosphite ion would be
PO53-
PO42-
PO33-
PO32-

30. intermolecular forces hydrogen bonding
WB CHECK:
The atoms within a polyatomic ion are held together by
ionic bonds
covalent bonds
intermolecular forces
hydrogen bonding

31. WB CHECK:
If nitrate is NO3- what is nitrite? If sulfite is SO32- what is sulfate?

32. WB CHECK:
What is the formula of potassium sulfate? What is the formula of magnesium nitrite? What is the name of Na3PO4? What is the name of (NH4)2SO3?

33. Homework: Read pages Practice #1-2 page 211 Practice #1-2 page 213 Practice #1-2 page 215 Practice #1-2 page 217 F.A. #1-5 page 219