nomenclature : naming chemicals po 4 3- phosphate ion c 2 h 3 o 2 - acetate ion hc 2 h 3 o 2 acetic...
TRANSCRIPT
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Nomenclature:
Naming Chemicals
POPO443-3-
phosphate ionphosphate ion
CC22HH33OO22--
acetate ionacetate ion
HC2H3O2
Acetic Acid
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Before naming….Some things you MUST know to be successful…. You really need to commit these things to memory
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Ions
Atoms or groups of atoms with a charge.Cations- positive ions - get by losing
electron(s).Anions- negative ions - get by gaining
electron(s).Ionic bonding- held together by the opposite
charges. (usually a metal and a nonmetal)Ionic solids are called salts.Salts are electrolytes; they conduct
electricity when dissolved in water (aq.)
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Conductors of heat and electricity
Make cations (lose e- to become + charged)
Malleable (made into sheets)
Ductile (made into wire)
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Are a brittle solid or a gas Make anions (gain e- to become - charged)
Covalently bond to each other
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•Characteristics of both metals and nonmetals
•More metallic as you go down PT
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Alkali Metals
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Alkaline Earth Metals
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Transition metals
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Inner Transition Metals
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Halogens
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Noble Gases
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+1+2 -1-2-3+/-4+3
Variable, always +
Common Ions of Elements
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Predicting Charges on Monatomic IonsPredicting Charges on Monatomic IonsKNOW THESE !!!!KNOW THESE !!!!
+1 +2 -3 -2 -1 0
Cd+2
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Polyatomic Ions
Groups of covalently bonded atoms that have a charge.* NO3
- :nitrate ion* NO2
- :nitrite ionYes, you have to
memorize them.Listed in your
resource handbook: memorize the required list!!!!
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Patterns for Polyatomic Ions-ate ion
chlorate = ClO3-
-ate ion plus 1 O same charge, per- prefixperchlorate = ClO4
-
-ate ion minus 1 O same charge, -ite suffixchlorite = ClO2
-
-ate ion minus 2 O same charge, hypo- prefix, -ite suffixhypochlorite = ClO-
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Polyatomic IonsPolyatomic IonsYou can make additional polyatomic ions by adding a H+
to the ion!CO3 -2 is carbonate
HCO3– is hydrogen carbonate
PO4 3- is phosphate
HPO4 is hydrogen phosphate
H2PO4 is dihydrogen phosphate
HSO4–2 is hydrogen sulfate
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The 3 types of Chemical Bonds:Ionic, Covalent, & MetallicElectronegativity and Bond type
Bond type can be determined by the difference in electronegativity between the bonds involved.
Differences of:≥ 2 = ionic0.5 – 1.9 = polar covalent ≤ 0.4 = nonpolar covalent
Metals bonded to other metals are metallically bonded, regardless of the difference in electronegativity
..
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Metallic bondsThe atoms of metals
are held together when the atom’s valence electrons float around the nuclei of the metals – the “sea of electrons”
Electrostatic forces keep everything together
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The 3 types of Chemical Bonds:Ionic, Covalent, & Metallic
Ionic—complete transfer of 1 or more electron from one atom to another (or another group)one loses one or more e-, the other gains those
e-
Atoms involved are a metal and either a non-metal or a
polyatomic ionThe cation and anion are attracted to
each other by electrostatic attraction
..
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Ionic compounds are neutralIonic compounds are neutral
That is, they have no overall chargeThis is because the number of electrons that are given up by the metal is the same number of electrons that are gained by the anion for the formula.
Formulas reflect this neutrality- the charges on the individual ions are not written in because they cancel out overall for the compound
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CATIONCATION + + ANIONANION ---> --->
COMPOUNDCOMPOUND
CATIONCATION + + ANIONANION ---> --->
COMPOUNDCOMPOUND
A neutral compound A neutral compound requiresrequires
equal number of + equal number of + and - charges.and - charges.
A neutral compound A neutral compound requiresrequires
equal number of + equal number of + and - charges.and - charges.
COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM IONSIONS
COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM IONSIONS
Na+ + Cl- --> NaCl
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Covalent Bonds2, 4, or 6 valence electrons that are shared
between atomsWe are going to name only simple covalent
compounds that have 2 elements involved
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Most bonds are somewhere in between ionic and covalent
Because not all atoms share e- equallyThe conventions of naming assume absolute
difference in bond typesMetals bonded to nonmetals or polyatomic
ions are classified as having ionic bonds*Materials made out of all non-metals are
classified as having covalent bonds** semimetals are not a classification in
naming; you need to treat the elements that are on the right of the line as non-metals, and those on the left as metals.
More on this when we talk about bonding
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Naming things:If there is only one element present,
name it. Atomic substances do not require “special” naming.
For anything with more than one element, remember that there is ONE MAIN THING to look for:
Is there a metal first?
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So…Look to see if there is a metal first in
the formula Again, semimetals are not a classification in
naming; you need to treat the elements that are on the right of the line as non-metals, and those on the left as metals.
If there are only metals, name both metals (metallic bonding; nothing else need be done)
If ONLY the first element is a metal, then the compound is an ionic compound
Nonmetals only signify a covalent compound
There is a flow chart in your handbook to help!
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Naming ionic compounds:Remember that those are compounds
that have a metal first in the formula*, and then a nonmetal or a polyatomic ion.
*Two exceptions to this rule: Compounds that start with either ammoniums (NH4
+) or hydronium (H3O+)We can handle these as simple binary (2
element) and ternary (more than two element) compounds
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General information for naming ionic compoundsIf the cation is monatomic- Name the
metal (cation). Use Roman Numerals for transition
metals (ONLY) after the metal If the cation is polyatomic- name it.If the anion is monatomic- name it
but change the ending to –ide. If the anion is poly atomic- just name
itPractice.
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Name the cation first, then the anion root with an –ide suffix
For CaCl2, the monatomic cation is Ca2+ , calcium, and the monatomic anion is Cl , named chloride.
We use chloride because the root for chlorine is chlor, and we use = root + -ide for the second element in binary compounds
CaCl2 = calcium chloride
Example: CaCl2, or calcium chloride
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Practice Naming Binary Ionic Compounds
Examples:
NaCl
ZnI2
Al2O3
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Learning Check Complete the names of the following binary compounds:Na3N
KBr
Al2O3
MgS
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If the Metal is a Transition Metal…Transition metals are Type II Cations, and
are elements that can have more than one
possible charge. They MUST have a
Roman Numeral to indicate the charge on
the individual ion.
1+ or 2+ 2+ or 3+
Cu+, Cu2+ Fe2+, Fe3+
copper(I) ion iron(II) ion copper (II) ion iron(III) ion
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Type II CationsThese elements REQUIRE Roman Numerals because they can have more than one possible charge:anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3 (Fe3+) iron (III) chlorideCuCl (Cu+ ) copper (I) chlorideSnF4 (Sn4+) tin (IV) fluoridePbCl2 (Pb2+) lead (II) chloride
Fe2S3 (Fe3+) iron (III) sulfide
You will appreciate this more when we go from names to formulas!
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Type II CationsSome Type II cations have a name
using the “old” system as well as the “new system”.
The old system, still widely used, adds to the root or stem of the Latin name of the metal the suffixes –ous and –ic. These represent the lower and higher charges respectively.
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Learning Check Complete the names of the following binary compounds with variable metal ions:
FeBr2
CuCl
SnBr4
Fe2O3
Hg2S
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Writing Formulas for Ionic Compounds from NamesFormulas of ionic compounds are determined
from the charges on the ions
Na + F Na+ + F- NaF
Sodium atom + fluorine atom sodium fluoride
Charge balance: 1+ + 1- = 0
Remember that all ionic compounds have no net charge, and that the charges are not written in! Ever. Nope.
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Neutral, you say?Formulas are written to make the
compound have a neutral charge overall.
You do NOT write the charges in the formula because they MUST cross out to accurately represent the compound.
Ex: NaF2 is INCORRECT for sodium chloride because Na has an oxidation state of +1, and F of -1. There is a one to one ratio of Na+ to F- to make a neutral ionic compound.
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Writing the formula…Write the formula for the barium chloride, the compound that will form between Ba2+ and Cl-.
Solution:1. Write the cation, and then the anion2. Balance charge with the number of +
and – ions
3. Write the number of ions needed as
subscripts:
BaBa++++ Cl- Cl- Think: Think: Cl-Cl- Why is ClWhy is Cl written twice? written twice?
BaClBaCl22
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So what if the oxidation numbers aren’t even?If the oxidation numbers or charges do
not balance, you can write the number of ions of each until you get the same number of each charge in total.
Yes. The “Criss Cross” method. You take the charge number from the cation, and you make it the number of anions, and take the charge on the anion, and you make that many cations.
Is there an easier way?Is there an easier way?
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Criss-Crossing in action:Example: Lead (II) nitrate
Pb2+ N3- *the charges do not balance
Pb2+ N3- Pb3N2
The 2 and the 3 are brought down to the opposite element, so that there are now 3 Pb2+ ions and 2 N3- ions
This means there were 6e- transferred from the lead atoms to the nitrogen atoms; the compound is neutral
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Learning Check Write the correct formula for the compounds containing the following ions:1. Na+ and S2-
a) NaS b) Na2S c) NaS2
2. Al3+ and Cl-
a) AlCl3 b) AlCl c) Al3Cl
3. Mg2+ and N3-
a) MgN b) Mg2N3 c) Mg3N2
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Ternary Ionic Compounds:Contain at least 3 elementsThere MUST be at least one polyatomic ion
(it helps to circle the ions)Examples:NaNO3 Sodium nitrate
K2SO4 Potassium sulfate
Al(HCO3)3 Aluminum bicarbonate(Aluminum hydrogen
carbonate)
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Name the cation first, then polyatomic ion
For NaNO3, the monatomic cation is Na+ , sodium, and the polyatomic anion is NO3
, named nitrate.
• NaNO3 is sodium nitrate
For Co(NO3)2, the monatomic cation is Co+2, cobalt (II) and the polyatomic anion is NO3
, named nitrate.
• Co(NO3)2 is cobalt (II) nitrate
Examples: Examples: NaNO3, and Co(NO3)2
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Learning Check Match each set with the correct name:1. Na2CO3 a) magnesium sulfite
MgSO3 b) magnesium sulfate
MgSO4 c) sodium carbonate
2 . Ca(HCO3)2 a) calcium carbonate
CaCO3 b) calcium phosphate
Ca3(PO4)2 c) calcium bicarbonate
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Writing Formulas for Ternary Ionic CompoundsWrite the cation first, then the anion. Overall charge must equal Overall charge must equal zerozero..
If charges cancelIf charges cancel, just write symbols.If not, use subscripts to balance charges.
Use parentheses to show more than one of a particular polyatomic ion.
Use Roman numerals indicate the ion’s charge when needed (transition metals)
Remember that the final formula should not have charges written in.
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Writing Formulas with Polyatomic IonsExample:
Cr2+ PO43- *the charges do not balance
Cr2+ PO43- Cr3(PO4)2
The polyatomic ions is in parentheses whenever a subscript is added
This is so that we know to count a number of those groups!
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Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH b) Fe3OH c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)
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Ternary Ionic Nomenclature:You Criss-cross these, too.
Sodium Sulfate
Iron (III) hydroxide
Ammonium carbonate
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Ternary Ionic Nomenclature:You Criss-cross these, too.
Sodium SulfateNa+ and SO4 -2
Na2SO4
Iron (III) hydroxideFe+3 and OH-
Fe(OH)3
Ammonium carbonateNH4
+ and CO3 –2
(NH4)2CO3
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Write the Formula:
Copper (II) chlorate Calcium nitrideAluminum carbonatePotassium bromideBarium fluorideCesium hydroxide
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General naming rules for covalent compoundsNames are two words, with prefixes.Prefixes tell you how many.First element whole name with the
appropriate prefix, except mono.Second element, -ide ending with
appropriate prefix.Practice
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neverYou NEVER criss-cross charges with covalent compounds.
Since you are sharing electrons, rather than giving them away/ picking them up, the charges are not relevant.
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Covalent Naming Prefixes:
PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-
NUMBER123456789
10
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Name the first element, using a prefix if there is more than one atom of the element present
Name the second element, using the appropriate prefix in all cases
CO2 is carbon dioxide because there is one carbon (no prefix when there is only one atom of the element,) and two oxygens (di- prefix)
Example: Example: CO2 is carbon dioxide
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Learning Check 1. P2O5 a) phosphorus oxide
b) phosphorus pentoxidec) diphosphorus pentoxide
2. Cl2O7 a) dichlorine heptoxide
b) dichlorine oxidec) chlorine heptoxide
3. Cl2 a) chlorineb) dichlorinec) dichloride
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Learning Check Give the names of following covalent
compounds:
CO
CO2
PCl3
CCl4
N2O
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CCl4
N2O5
SF6
Covalent Naming Examples
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arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
More Molecular Examples
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Hydrates: Ionic Compounds·WaterSome salts trap water crystals when
they form crystals. Ex: CuSO4·5H2OThese are hydrates.Both the name and the formula
needs to indicate how many water molecules are trapped.
In the name we add the word hydrate with a prefix that tells us how many water molecules.
CuSO4·5H2O is copper (II) sulfate pentahydrate
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HydratesIn the formula you put a dot and
then write the number of molecules.
Calcium chloride dihydrate = CaCl22
Chromium (III) nitrate hexahydrate = Cr(NO3)3 6H2O
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Acid NomenclatureAcids
Compounds that form H+ in water.
Formulas usually begin with ‘H ’.
In order to be an acid instead of a gaseous covalent compound, it must be aqueous
Meaning dissolved in water; symbolized by (aq)
Ternary acids are ALL aqueous
Two types: Oxyacids Non-oxyacids
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Naming acids
If the acid doesn’t have oxygenadd the prefix hydro-change the suffix -ide to -ic acid
HCl Hydrochloric acidH2S Hydrosulfic acid
HCN Hydrocyanic acid
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Naming acidsIf the formula has oxygen in itwrite the name of the anion, but change
ate to -ic acidite to -ous acid
Watch out for sulfuric and sulfurous!
H2CrO4
HMnO4
HNO2
Chromic acid
Manganic acid
Nitrous acid
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Acid Nomenclature Flowchart
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Anion Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Acid Nomenclature
Binary Binary
Ternary Ternary
An easy way to remember which goes with which…An easy way to remember which goes with which…
““In the cafeteria, you In the cafeteria, you ATEATE something something ICICkyky””
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HBr (aq)
H2CO3 (aq)
H2SO3 (aq)
Acid Nomenclature
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HBr (aq)
H2CO3 (aq)
H2SO3 (aq)
2 elements, -ide
3 elements, -ate
3 elements, -ite
hydrobromic acid
carbonic acid
sulfurous acid
Acid Nomenclature
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Acid Name
HNO3 Nitric acid
HNO2 Nitrous acid
H2SO4 Sulfuric acid
H2SO3 Sulfurous acid
H3PO4 Phosphoric acid
HC2H3O2 Acetic Acid
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Name ‘Em!HI (aq)
H2C2O4
(aq)
H2S2O3
(aq)
HIO4 (aq)
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Formulas for acidsBackwards from names.If it has hydro- in the name it has no oxygen
Anion ends in -ideNo hydro, anion ends in -ate or -iteWrite anion and add enough H to balance the charges.
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hydrofluoric acid
phosphorus acid
nitrous acid
Acid Nomenclature
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hydrofluoric acid
sulfuric acid
nitrous acid
2 elements
3 elements, -ic
3 elements, -ous
Acid Nomenclature
H+ F-
H+ SO42-
H+ NO2-
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hydrofluoric acid
sulfuric acid
nitrous acid
2 elements
3 elements, -ic
3 elements, -ous
HF (aq)
H2SO4 (aq)
HNO2(aq)
Acid Nomenclature
H+ F-
H+ SO42-
H+ NO2-
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Write the Formula!Hydrobromic acid
Boric acid
Carbonic acid
Phosphoric acid
Hydrotelluric acid
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Write the Formula!Hydrobromic acid
Boric acid
Carbonic acid
Phosphoric acid
Hydrotelluric acid
HBr(aq)
H3BO3(aq)
H2CO3(aq)
H3PO4(aq)
H2Te(aq)
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Common NamesA lot of chemicals have
common names as well as the proper IUPAC name.
Chemicals that should always be named by common name and never named by the IUPAC method are:H2O water, not dihydrogen
monoxideNH3 ammonia, not nitrogen
trihydride
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Mixed Practice1. Dinitrogen monoxide2. Potassium sulfide3. Copper (II) nitrate4. Dichlorine heptoxide5. Chromium (III)
sulfate6. Iron (III) sulfite7. Calcium oxide8. Barium carbonate9. Iodine monochloride
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Match each set with the correct name:
Na2CO3 a) sodium carbonate
MgSO3 b) magnesium sulfite
MgSO4 c) magnesium sulfate
Ca(HCO3)2 a) calcium bicarbonate
CaCO3 b) calcium carbonate
Ca3(PO4)2 c) calcium phosphate
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Mixed Review Name the following compounds:1. CaO
a) calcium oxide b) calcium(I) oxide
c) calcium (II) oxide d) calcium monoxide
2. SnCl4
a) tin tetrachloride b) tin(II) chloride
c) tin(IV) chloride
3. N2O3
a) nitrogen oxide b) dinitrogen trioxidec) nitrogen trioxide
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Mixed Practice1. BaI2
2. P4S3
3. Ca(OH)2
4. FeCO3
5. Na2Cr2O7
6. I2O5
7. Cu(ClO4)2
8. CS2
9. B2Cl4
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DONE!Now it is time to study!
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Rainbow Matrix GameLink on Chemistry Geek.com on
Chemistry I pagehttp://chemistrygeek.com/rainbow
Use [ ] to represent subscripts since you can’t enter subscripts into the computer
So H2O would be H[2]OAnd Al2(SO4)3 would be Al[2](SO[4])[3]
Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!)
Borate = BO3 -3 ; Silicate = SiO4 -4 ;Manganate = MnO4 -2 (permanganate is -1)