1. Nomenclature
Chapter 9

2. Do Now #1 Which statement is true?
Elements in the same group has the same # of val. e-
Elements in the same period has the same # of val. e-

3. Do Now #2 Write the formula for each of the following compounds.
Ammonium sulfate
Vanadium (V) fluoride
Copper (III) nitrate
Aluminum oxide
Answers:
(NH4)2SO4
VF5
Cu(NO3)3
Al2O3

4. Do Now #3
What is the difference between CuSO4 and CuNO3? Answer: Contain different polyatomic anion CuSO4: copper 2+ CuNO3: copper 1+

5. Do Now #4 Name the following compounds: CO SiO2 P4O6
Write the formula for the below compounds:
Arsenic tribromide
Answer:
Carbon monoxide
Silicon dioxide
Tetraphosphorus hexoxide
Answer: AsBr3

6. Types of Chemical Bonds
Ionic Compounds:
Formed by the opposite attraction between cations & anions. (btwn metals & non-metals)
Salt - scientific name given to many different ionic compounds
Transfer of electrons creates ions

7. Formation of Sodium Chloride

8. +1 +2 +3
+/-4 -3 -1 -2
Hydrogen can be 1+ or 1-, most common is 1+

9. CATIONS (alkalai = +1, alkaline earth = +2, aluminum = +3, zinc = +2, silver = +1) sodium ion _______ beryllium ion _______ aluminum ion _____ strontium ion ______ cesium ion _________ silver ion _____
Na 1+
Be 2+
Al 3+
Sr2+
Cs+
Ag+

10. TRANSITION/POST TRANSITION METALS (variable) copper (I) ion _____ copper (II) ion _____ cobalt (II) ion ______ manganese (VII) ion ______ iron (II) ion ______ iron (III) ion _____
Cu+
Cu2+
Co2+
Mn7+
Fe2+
Fe3+

11. ANIONS (monoatomic anions all end in –ide) nitride ______ fluoride _______ oxide ______ chloride _____ iodide _______ phosphide ______
N3-
F1-
O2-
Cl1-
I1-
P3-

13. BINARY IONIC COMPOUNDS (Salts)
Naming rule: Metal name______________ ide (root of non-metal) Ex: AlCl3 = Aluminum Chloride a. Li2O b. MgF2 c. Ca3P2 d. SrI2
Lithium Oxide
Magnesium Fluoride
Calcium Phosphide
Strontium Iodide

14. Formula writing Al +3 Cl -1 Al1Cl3 = AlCl3 Sodium chloride
Calcium chloride
Ionic Compound subscripts must be reduced
Ti+4O Sn+2O-2
Ti2O4 reduces to TiO2 Sn2O2 reduces to SnO
NaCl
CaCl2

15. Write the FORMULA for: a. lithium fluoride b. calcium bromide
LiF CaBr2
c. magnesium phosphide d. barium oxide
Mg3P2 BaO
e. iron(III) chloride f. lead (II) nitride
FeCl3 Pb3N2
g. potassium nitride h. tin(IV) oxide
K3N SnO2

16. Polyatomic ion Ions made up of 2 or more atoms
Charge is spread across the group of bonded atoms
You do not need to memorize them. They will be given to you during the test

17. Write the FORMULA for:
a. lithium sulfate b. calcium hydroxide Li2SO4 Ca(OH)2 c. copper(II) cyanide d. strontium nitrate Cu(CN)2 Sr(NO3)2 e. chromium(III) phosphate f. manganese (IV) carbonate CrPO4 Mn(CO3)2 g. barium chlorate h. aluminum permanganate Ba(ClO3)2 Al(MnO4)3

18. NAME the following compounds:
a. NH4Cl b. Ca(CN)2 Ammonium Chloride Calcium Cyanide c. Na3PO4 d. Al(OH)3 Sodium Phosphate Aluminum Hydroxide e. ZnSO4 f. Cs2CO3 Zinc Sulfate Cesium Carbonate g. KClO3 h. Mg3(PO4)2 Potassium Chlorate Magnesium Phosphate

19. TRANSITION/POST TRANSITION METALS (charge varies)
WHAT ABOUT THE METALS THAT HAVE MORE THAN ONE OXIDATION # (CHARGE)? a. Write in the charges for the ions you are sure of (anion) b. Work backwards to find the charge of the metal ion (cation) Which metals DO NOT need Roman Numerals? Column I (alkali) Column II (alkaline earth) Silver (always +1): Ag+ Zinc (always +2): Zn2+ Aluminum (always +3): Al3+

21. NAME the following compounds (Roman numerals shows the charge of the metal)
a. CuS b. FeP copper (II) sulfide iron (III) phosphide c. FeSO4 d. CuNO3 iron (II) sulfate copper (I) nitrate e. NiI3 f. Cr(MnO4)4 nickel (III) iodide chromium (IV) permanganate g. Pb(NO3)2 h. Pb(SO4)2 lead (II) nitrate lead (IV) sulfate i. Sn(CO3)2 j Sn(NO3)2 tin (IV) carbonate tin (II) nitrate k. Cu3(PO4)2 l. Cu3PO4 copper (II) phosphate copper (I) phosphate

22. Covalent Compounds
Formed when atoms share one or more pairs of electrons
Bonds between nonmetals

23. NO → Nitrogen monoxide NOT Mononitrogen monooxide
Prefix
# of Atoms
mono- 1
hexa- 6
di- 2
hepta- 7
tri- 3
octa- 8
tetra- 4
nona- 9
penta- 5
deca- 10
Examples:
SO → Sulfur dioxide
SO → Sulfur trioxide
NO → Nitrogen monoxide NOT Mononitrogen monooxide
N2O5 → Dinitrogen pentoxide NOT dinitrogen pentaoxide
Some compounds are always referred to by their common names
H2O Water
NH3 Ammonia
CH4 Methane

24. C3Cl6 Si2O7 C5F10 PCl5 tricarbon hexachloride Disilicon heptoxide
Prefix
# of Atoms
mono- 1
hexa- 6
di- 2
hepta- 7
tri- 3
octa- 8
tetra- 4
nona- 9
penta- 5
deca- 10
tricarbon hexachloride
C3Cl6 Si2O7 C5F10 PCl5
Disilicon heptoxide
pentacarbon decafluoride
phosphorous pentachloride

25. Writing the formula of molecular/covalent compounds:
N2O5
BF3 CO
CCl4
N2O
NO2
Cl2O
CF4
C4Br8
a) dinitrogen pentaoxide b) Boron triflouride c) Carbon monoxide d) Carbon tetrachloride e) dinitrogen monoxide f) nitrogen dioxide g) dichlorine monoxide h) carbon tetrafluoride i) tetracarbon octabromide

26. Naming Acids (hint: acids start with “H”)
BINARY: Contains exactly two elements.
(without oxygen)
prefix hydro- to name the hydrogen part of the acid
add the suffix –ic
EXAMPLES:
HCl HBr
hydrochloric acid hydrobromic acid

27. Naming Acids CONT…
Oxyacids: (contain oxygen) (H & polyatomic ion with O)
use the root of the anion
if it is an –ate anion, use the –ic ending
if it is an –ite anion, use the –ous ending
H2SO4 HNO3
sulfuric acid nitric acid
H2SO3 HNO2
sulfurous acid nitrous acid

28. FORMULA ANION NAME H2CO3 HC2H3O2 H2SO3 H3P H2S Carbonic acid Carbonate
Acetate
Acetic acid
Sulfite
Sulfurous acid
Phosphide
Hydrophosphoric acid
Sulfide
Hydrosulfuric acid

29. FORMULA ANION NAME hydronitric acid nitrous acid permanganic acid
sulfuric acid
hydrofluoric acid
phosphoric acid
hydrophosphoric acid
H3N
N3-
HNO2
NO2-1
HMnO4
MnO4-1
H2SO4
SO4-2 HF
F1-
H3PO4
PO4-3
H3P
P3-