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Nomenclature Chapter 9.

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Presentation on theme: "Nomenclature Chapter 9."— Presentation transcript:

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-


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

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-

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