Upload
henry-hunt
View
236
Download
3
Embed Size (px)
Citation preview
NomenclatureChapter 9
Do Now #1Which statement is true?A. Elements in the same group has the same #
of val. e-B. Elements in the same period has the same #
of val. e-
Write the formula for each of the following compounds.1. Ammonium sulfate2. Vanadium (V) fluoride3. Copper (III) nitrate4. Aluminum oxide
Answers:5. (NH4)2SO4
6. VF5
7. Cu(NO3)3
8. Al2O3
Do Now #2
Do Now #3
What is the difference between CuSO4 and CuNO3?
Answer:Contain different polyatomic anion CuSO4: copper 2+
CuNO3: copper 1+
Name the following compounds:1. CO2. SiO2
3. P4O6
Write the formula for the below compounds:4. Arsenic tribromide
Answer:5. Carbon monoxide6. Silicon dioxide7. Tetraphosphorus hexoxide
Answer: AsBr3
Do Now #4
Types of Chemical BondsIonic Compounds: Formed by the opposite attraction between
cations & anions. (btwn metals & non-metals)
Salt - scientific name given to many different ionic compounds
75102.swf
Transfer of electrons creates ions
Formation of Sodium Chloride
+1 +
2+3
+/-4 -3 -2 -1
0
Hydrogen can be 1+ or 1-, most common is 1+
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+
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+
Fe3+
Fe2+
ANIONS (monoatomic anions all end in –ide)
nitride ______
fluoride _______
oxide ______
chloride _____
iodide _______
phosphide ______
N3-
F1-
O2-
Cl1
-
I1-
P3-
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
Formula writing
Al +3 Cl -1
Al1Cl3 = AlCl3
Sodium chlorideCalcium chloride
Ionic Compound subscripts must be reducedTi+4O-2 Sn+2O-2 Ti2O4 reduces to TiO2 Sn2O2 reduces to
SnO
NaCl
CaCl2
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) nitrideFeCl3 Pb3N2
g. potassium nitride h. tin(IV) oxideK3N SnO2
Ions made up of 2 or more atomsCharge is spread across the group of bonded
atoms
Polyatomic ion
You do not need to memorize them. They will be given to you during the test
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
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
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+
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
Covalent CompoundsFormed when atoms share one or more pairs of electronsBonds between nonmetals
Prefix # of Atoms Prefix # of Atomsmono- 1 hexa- 6di- 2 hepta- 7tri- 3 octa- 8
tetra- 4 nona- 9penta- 5 deca- 10
Examples:SO2 → Sulfur dioxide
SO3 → Sulfur trioxide
NO → Nitrogen monoxide NOT Mononitrogen monooxideN2O5 → Dinitrogen pentoxide NOT dinitrogen pentaoxide
Some compounds are always referred to by their common namesH2O Water
NH3 Ammonia
CH4 Methane
C3Cl6
Si2O7
C5F10
PCl5
Prefix # of Atoms Prefix # of Atomsmono- 1 hexa- 6di- 2 hepta- 7tri- 3 octa- 8
tetra- 4 nona- 9penta- 5 deca- 10
tricarbon hexachloride
Disilicon heptoxide
pentacarbon decafluoride
phosphorous pentachloride
Writing the formula of molecular/covalent compounds:
a) dinitrogen pentaoxide
b) Boron triflouridec) Carbon monoxided) Carbon tetrachloridee) dinitrogen monoxidef) nitrogen dioxideg) dichlorine monoxideh) carbon tetrafluoridei) tetracarbon
octabromide
N2O5
BF3
COCCl4
N2ONO2
Cl2OCF4
C4Br8
BINARY: Contains exactly two elements. (without oxygen)
1. prefix hydro- to name the hydrogen part of the acid
2. add the suffix –ic EXAMPLES:
HCl HBrhydrochloric acid hydrobromic acid
Naming Acids (hint: acids start with “H”)
Naming Acids CONT…
Oxyacids: (contain oxygen) (H & polyatomic ion with O)
1. use the root of the anion2. if it is an –ate anion, use the –ic ending3. if it is an –ite anion, use the –ous ending
H2SO4 HNO3
sulfuric acid nitric acidH2SO3 HNO2
sulfurous acid nitrous acid
FORMULA ANION NAME
H2CO3
HC2H3O2
H2SO3
H3P
H2S
Carbonate Carbonic acid
Acetate Acetic acid
Sulfite Sulfurous acid
Phosphide Hydrophosphoric acid
Sulfide Hydrosulfuric acid
FORMULA ANION NAMEhydronitric acid
nitrous acid
permanganic acid
sulfuric acid
hydrofluoric acid
phosphoric acid
hydrophosphoric acid
H3N N3-
HNO2 NO2-1
HMnO4 MnO4-1
SO4-2H2SO4
HF F1-
PO4-3
P3-
H3PO4
H3P