Naming & Writing Formulas
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Transcript of Naming & Writing Formulas
Naming Naming &&
Writing FormulasWriting FormulasForFor
Molecular & Ionic CompoundsMolecular & Ionic Compounds
Naming Molecular Compounds
Non-metal + Non-metal
• Step 1: write the element name for the first
non-metal add a prefix ….(if there is more than
one atom)
• Step 2: Write the second element name and
add an ide ending Add a prefix
Exceptions
• DO NOT use any prefixes at all if the first element is hydrogen ……these are acids
Prefixes
1 = 6 =
2 = 7 =
3 = 8 =
4 = 9 =
5 = 10 =
mono
ditri
tetra
penta
hexa
hepta
octa
nona
deca
Examples
• P4O10 tetraphosphorus decaoxide
• bromine heptahydride
• H2S hydrogen sulfide
BrH7
Try the Following
• CO(g)
• CO2(g)
• N3F8
carbon monoxide
carbon dioxide
Trinitrogen octafluoride
Writing Formulas for Molecular Compounds
• Steps: Write each elements symbol Write the subscript number (the prefix)
• E.g. dinitrogen oxide N2O
Sulfur dioxide S20
Try the Following
• oxygen dibromide
• diphosphorus pentasulphide
• carbon tetraiodide
• phosphorus pentachloride
OBr2
P2S5
CI4
PCl5
Molecular Compounds that Must be memorized !!!
ammonia
water
NH3 ( g) =
H2O ( l) =H2S ( g) =
CH4 ( g) =
CH3OH ( l) =C2H6 ( g) =C2H5OH ( l) =
C6H12O6 ( s) =
hydrogen sulphide
methane
methanolethane
ethanol
glucosesucroseC12H22O11 ( s) =
hydrogen peroxideozoneO3 ( g) =
H2O2 ( l) =
Naming Binary Ionic Compounds
Metal + non-metal
• DO NOT USE PREFIXES
• Steps
1.Write the metal 1st
2. Write the non-metal 2nd with an ide ending
E.g. NaF
Na2Ssodium fluoride
sodium sulphide
two sodium ions are bonded with one sulphide ion… this doesn’t matter for naming ionic compound
Try the Following
• LiF
• KCl
• BeS
• Rb3P
• MgF2
• Na2O
• CsBr
lithium fluoride
potassium chloride
beryllium sulphide
rubidium phosphidemagnesium fluoride
sodium oxide
cesium bromide
Try the Following
• KCl
• MgBr2
• Ba3N2
• ScP
potassium chloride
magnesium bromide
barium nitride
scandium phosphide
Writing Formulas for Binary Ionic Compounds
• Steps
1.Look up the symbol for each…& write the metal first
2.Balance the charges (total + charges = total – charges)
3.Use subscripts to show the # of each element
sodium oxide
1+ Charge 2 Charge
1+ 2 = 2+ 2 1 = 2
Na2O
calcium phosphide
2+ Charge 3 Charge
2+ 3 = 6+ 3 2 = 6
Ca3P2
Try the Following
• magnesium chloride
• calcium chloride
• zinc sulphide
• silver sulphide
• germanium oxide
• calcium arsenide
• magnesium nitride
MgCl2
CaCl2
ZnS
Ag2S
GeO2
Ca3As2
Mg3N2
Try the Following
• lithium iodide
• zinc fluoride
• strontium phosphide
• silver oxide
• germanium arsenide
LiI
ZnF2
Sr3P2
Ag2O
Ge3As4
Naming Multivalent Ionic Compounds
• Transition metal ions have more than one possible charge
Cu2+, Cu+, Fe3+, Fe2+
transition metal + non-metal
• Steps
1. Write metal 1st with the charge in roman numerals
2.Write non-metal second
remember the charges have to balance
Roman Numerals (I,II,III,IV,V,VI,VII)
Examples
uranium (VI) fluoride
chromium (III) nitride
cobalt (II) chloride
U6+ F–
Cr3+ N3-
Co2+ Cl-
UF6
CrN
CoCl2
Try the Following
• AuBr
• CrCl2
• Co2O3
• VS2
• PuN2
gold (I) bromide
chromium (II) chloride
cobalt (III) oxide
vanadium (IV) sulphide
plutonium (VI) nitride
Naming Complex Ions
Metal + complex ion
• Steps:
1. Name the metal ion
2. Name the complex ion E.g.) PO43
Note: NH4+ (ammonium ion) is the
only positive complex ion…it will take the place of a metal
Examples
• CaCO3
• Ba(OH)2
• (NH4)3N
• CaCO3
• Ba(OH)2
• (NH4)3N
Solutions
Calcium carbonate
Barium hydroxide
Ammonium nitride
Try the Following
• KIO3
• NaCH3COO
• MgSO3
• NH4NO3
• Ca3(PO4)2
potassium iodate
sodium acetate
magnesium sulphite
ammonium nitrate
calcium phosphate
Writing Formulas For Complex Ions
• Steps:
1. Look up the symbol for each ion
2. Balance the charges
• Note: if you need more than 1 complex ion to balance the charges use brackets
• E.g. Ca(CH3COO)2
2+ 1 -
Try the Following
• aluminum phosphate
• calcium sulphite
• scandium acetate
• ammonium sulphate
• nickel (II) phosphate
• aluminum chlorate
AlPO4
Al(ClO3)3
CaSO3
Sc(CH3COO)3
(NH4)2SO4
Ni3(PO4) 2
SolubilitySolubility
Will the compound dissolve in water?Will the compound dissolve in water?
Soluble
• Refers to whether or not the compound dissolves in water
• If it is…. the compound is aqueous (aq)
• All acids are soluble
• Some ionic compounds are soluble… the rest are solids
Is It soluble?
• This will apply to ionic compounds (only)
• Steps
1. Find each ion in the boxes across the top
2. if it is soluble it will have (aq) aqueous
3. If it does not dissolve it will have (s) solid.
Determine if the following compounds are soluble in water. Use the proper subscript to indicate the state.
• AgCl• BaCO3
• LiOH• Ca2(PO4)3
• NaCl• CaI2
• Pb(NO3)2
• HMnO4
• AgCl
• BaCO3
• LiOH
• Ca2(PO4)3
• NaCl
• CaI2
• Pb(NO3)2
• HMnO4
(s)
(s)
(aq)
(s)
(aq)
(aq)
(aq)
(aq)
Acids & BasesAcids & Bases
Acids
• They are always soluble in water
• Conduct electricity
• Taste sour
• React with metals to produce hydrogen gas (H2(g))
• Neutralize a base
• they ALWAYS have hydrogen ….usually as the first element
• E.g. HCl(aq) , H3PO4(aq)
• There are three types: Binary Oxo Organic
Binary Acids
• contain only H and one other element (Cl, Br, etc.)
• E.g. HCl (aq)
Oxo Acids
• Contain H and Oxygen
• E.g. H3PO4(aq)
Organic Acids
• Contain C, H, & O
• The H is written at the end
• All have COO-
• E.g. CH3COOH(aq) – acetic acid
C6H5COOH(aq) - benzoic acid
HOOCCOOH(aq) – oxalic acid
Acid Indicators
• Turns blue litmus paper red
• Able to turn bromothymol blue to yellow
• Phenolphthalein remains colorless
• E.g. lemon juice
Bases
• Are usually soluble in water
• Conduct electricity (not weak ones)
• Neutralize acids
• Taste bitter
• Usually solids
• Feel slippery
Base Indicators
• Turns red litmus paper blue
• Bromothymol blue remains blue
• Turns phenolphthalein pink
• E.g. baking soda, Rolaids, soap, Draino crystals
Naming Acids
• Steps:
Hydrogen ____ide becomes hydro____ic acid
Hydrogen ____ate becomes _______ic acid
Hydrogen ____ ite becomes _______ ous acid
Examples
• HF (aq) • H2SO3 (aq)
• H3BO3 (aq)
• HCl (g)
hydrogen fluoride = hydrofluoric acid
hydrogen sulphite = sulphurous acid
hydrogen borate = boric acid
Hydrogen chloride (not an acid)
hydrosulphuric acid phosphorus acid
carbonic acid
hydrogen phosphite H3PO3 (aq)
1+ 3-
hydrogen carbonate H2CO3(aq)
1+ 2-
hydrogen sulphide H2S (aq)
1+ 2-
Try the Following
Writing Acid Formulas• Steps:
1. Use the naming rules in the opposite direction
• Example:
hydrosulphuric acid
hydrogen sulphide H2S(aq)
Try the Following
• carbonic acid
• chlorous acid
hydrogen carbonate
hydrogen chlorite
H2CO3(aq)
HClO2(aq)
Naming Bases
• Steps:
1. Write the metal name 1st
2. Write hydroxide or bicarbonate
E. g. NaOH sodium hydroxide
Try the Following
• KOH
• Ba(OH)2
• NaHCO3
potassium hydroxide
barium hydroxidesodium bicarbonate
Chemical Reactions• Can cause a physical or a chemical
change
• Always results in the formation of a new substance
• Evidence:
1. Temperature change
2. Formation of a precipitate
3. Colour change
4. Gas produces
states states
balancing
Reactants Products
1 H2 (g)+1 ZnCl2(aq)2 HCl(aq)1 Zn(s)+
Energy Changes
• Can occur in the form of heat, light, electrical, or mechanical
• There are two types: Endothermic Exothermic
• Endothermic Energy is absorbed (enters) Reactants + Energy products
• Exothermic Energy is released (leaves) Reactants product + energy
Balancing Equations
• There must be equal numbers of each element on both sides of the equation
Use lowest numbers
Example
____Mg(s) + ___ O2(g) ___ MgO(s)
____ H2O(l) ____H2(g) + ____ O2(g)
• When chemicals react they follow the Law of Conservation of Matter:
Matter can not be created or destroyed it only changes form
• Mass of reactants = mass of products
Counting Practice
• How many of each element are in the following compounds?
1. NaCl 5. NH4CH3COO
2. BaBr2 6. 3 (NH4)2S
3. (NH4)3P 7. 2 CaCl2
4. Ba(OH)2 8. 8 PbI2
9. 4 Zn(CH3COO)2
Balancing Practice
____ Cu(s) + ____ AgNO3(aq) ____ Ag(s) + ___Cu(NO3)2(g)
___ Cl2(g) + ____ NaBr(aq) ____ Br2(l) + ____ NaCl(aq)
____ KI(aq) + ___ Pb(NO3)2(aq) ___ PbI2(s) + ___KNO3(aq)
____ CH4(g) + ____ O2(g) ____ CO2(g) + ____ H2O(g)