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Science 10 Chapter 4.2 Names and Formulas of Ionic Compounds. Ionic Compounds (metal + non-metal {+,-}) Hydrates (water attached) Covalent Compounds (non-metal + non-metal {-,-}) Acids (H + something). Ionic Compounds. Made up of ions (+ & -) Compounds are NEUTRAL - PowerPoint PPT Presentation
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Science 10 Chapter 4.2Names and Formulas of Ionic Compounds Ionic Compounds (metal + non-metal {+,-}) Hydrates (water attached)Covalent Compounds (non-metal + non-metal {-,-}) Acids (H + something)
Ionic Compounds
• Made up of ions (+ & -)• Compounds are NEUTRAL• The sum of (+) ion charges must equal the (-)
ion charges• Opposites attract• Form crystals from
insideout
Salt, NaCl
Ionic Compounds3 rules for chemical formula, given name
1. Write formula for (+) ion first, then (-) ion second
2. Criss-cross the charge numbers on the ions3. Tidy up the formula– Divide evenly by 2 or 3– Omit superscript charges– Omit subscripts of 1– Put brackets around polyatomic ions (PAIs) if
there’s more than 1 *Table of PAI’s pg. 66 of wb
Ionic Compounds - Construct formula given name
Sodium IodideNa+1 I-1 NaI
Calcium OxideCa+2 O-2 CaO
Calcium PhosphateCa+2 PO4
-3 Ca3(PO4)2
Copper (I) OxideCu+1 O-2 Cu2O
Ionic Compounds - Construct name given formula
• Write metal name first, then non-metal ending with “ide”
• E.g., CaCl2 calcium chloride
Ionic Compounds - Construct name given formula
• For PAIs, don’t change their ending
• E.g., CaCrO4
calcium chromate
Ionic Compounds: Construct name given formula
• For multivalent metals reverse criss-cross subscripts to find charges
• Always check charge of non-metal (2nd ion)– If not, multiply both sides by the same # to correct
• Write metal’s charge in roman numerals after name(I, II, III, IV, V, VI, VII)
*On periodic table, most
common ion is listed on top
Ionic Compounds - Construct name given formula
• CuO– Cu can either be 1+ or 2+– Reverse criss-cross = 1+– Check: can oxygen be 1-?– Multiply– Name: copper (II) oxide
Hydrates• Molecules that include water in their crystal
structuresNaming• Find name before water is attached• Add water using a prefix with the word
“hydrate” CoCl2
cobalt (II) chloride hexahydrate CoCl2·6H2O
Prefixes for Hydrates
=Prefix
# water molecules Prefix
# water molecules
Mono 1 Hexa 6
Di 2 Hepta 7
Tri 3 Octa 8
Tetra 4 Nona 9
Penta 5 Deca 10
Name a hydrate!
Name a hydrate
Cr(NO3)3·9H2O
chromium (III) nitrate nonahydrate
Science 10 Quiz Feb 12, 20141. Identify the hydrate(s) in the list belowa) Al(NO3)3 b) H2O2 c) Al(NO3)3·9H2O d) CaCrO4
2. The least/most common ion charge is written above the other ion charges
Devin S.
Anthony T.
Sonia W.
Gabrielle, W.
Alisha Y.
Oliver K Cici L. Aidan M.
Karla M.
Teagan M.
Avery S.
Robert F.
Jordan G.
Jordanne H.
Liam H. Sarah H.
Daniel H.
Sydney H.
Rab H. Rose J. Richard J.
Clayton A.
Brianna B.
Eddie B.
Darian B.
Cara B. Spencer C.
Shea C. Austin C.
Kowisha C.
Stephy C.
Science 10 Quiz Feb 12, 20141. Identify the hydrate(s) in the list belowa) Al(NO3)3 b) H2O2 c) Al(NO3)3·9H2O d) CaCrO4
2. The least/most common ion charge is written above the other ion charges
Chelsea T.
Jacob W.
Amy W.
Mandy H.
Christina L.
Jack L. Michael L.
Lewis M.
Alexander O.
Kyra R. Kaleb S. Ashley S.
Ashen S.
Sam B. Bradley B.
Caleb B.
Jessie C.
Alex C. Emily C.
Rachel C.
Ben E. Connor H.
Danielle H.
Covalent compounds (aka molecules)
• Share electrons• No order in formation (clump as (s), (l), or (g)• Use the same prefixes (mono, di, tri, …)• Made of 2 or more non-metals• Subscripts show actual number of atoms in
molecule
• examples: carbon monoxide, carbon dioxideCO CO2
Naming binary covalent compounds
• Binary = 2 elementsSteps:1. Write the most metallic (left) element first2. Second element gets “ide” ending***Subscripts must be named***
e.g., nitrogen dioxide, dinitrogen dioxideNO2 N2O2
TRAPS
• NH4+ = ammonium
• NH3 = ammonia
• H2O = water
Some Common Acids naming scheme: {H + something} Three Acids:
1. H + Non Metal (found on right side of Periodic table {Halogen})
a) start with “HYDRO b) add non metal c) change ending to IC most times {RIC}d) add word “acid”
Example: HF = hydrofluoric acid HB = HCl =
2. H + Poly atomic ion with a ATE ending a) name P.A.I.b) change ending to “RIC”c) add word “acid”Example: H2SO4 = sulphuric acid
H3PO4 =
H2CrO4 =
3. H + Poly atomic ion with a ITE endinga) name P.A.Ib) change ending to “ROUS”c) add word “acid”Examples: HNO2 = nitrous acid
H2SO3 =
H3PO3 =
1. Silver chloride__________2. Sulphur dioxide__________3. Lead (II) acetate decahydrate_______________4. Silver dichromate__________5. Silicon tetraflouride__________6. Ammonium phosphate __________7. Copper (I) iodide__________8. Iron (II) fluoride nonahydrate_____________9. Zinc hydrogen sulphite______________10. Manganese (IV) monohydrogen phosphate
trihydrate ________________
Name into Formula
Formula into Name
1. NI3 _______________________________
2. Ca(OH)2 _______________________________
3. Fe2(SO4)3.H2O _______________________________
4. (NH4)2C2O4 _______________________________
5. Co3(PO4)2.8H2O_______________________________
6. H3PO4 _______________________________
7. HClO2 _______________________________
8. N3O _______________________________
9. HI _______________________________10. Mg3P2 _______________________________
Science 10 Chapter 4.2Names and Formulas of Ionic Compounds
4 types of compounds CO2
HNO3
CoO Cr(NO3)3·9H2O workbook pages
71, 73 due tomorrow