Nomenclature:
Naming Chemicals
PO43-PO43-
phosphate ionphosphate ion
C2H3O2-C2H3O2-
acetate ionacetate ion
HC2H3O2
Acetic Acid
Before naming….
•Some things you MUST knowto be successful…. You reallyneed to commit these thingsto memory
Ions:
•Atoms or groups of atoms with a _________.
•Cations- ________ions - get by losingelectron(s).
•Anions- ________ ions - get by gainingelectron(s).
•Ionic bonding- held together by the______________ (_____________________).
•Ionic solids are called ________.
•Salts are __________________; they conductelectricity when dissolved in water (aq.)
Metals
•Conductors of heat and electricity
•Make ________ (lose e- to become + charged)
•Malleable (made into ________)
•Ductile (made into ________)
Nonmetals
•Are a ________ _______ or a _______
•Make ________(gain e- to become - charged)
•__________ bond to
each other
Semi-metals (AKA ________)
•Characteristics of _____metals and nonmetals
•More ________ as yougo down PT
________ _____
Common Ions of Elements
Predicting Charges on Monatomic IonsPredicting Charges on Monatomic Ions
KNOW THESE !!!!KNOW THESE !!!!
+1 +2 -3 -2 -1 0
Cd+2
Variable, always +
Polyatomic Ions
•_______ of covalentlybonded atoms thathave a charge.
* NO3- :___________
* NO2- :___________
•Yes, you have tomemorize them.
•Listed in your resourcehandbook: memorizethe required list!!!!
Patterns for Polyatomic Ions
•-ate ion
–_________________________________
•-ate ion plus 1 O same charge, ___- prefix
–_________________________________
•-ate ion minus 1 O same charge, -___suffix
–_________________________________
•-ate ion minus 2 O same charge, ___-prefix, -___ suffix
–_________________________________
Polyatomic Ions
Polyatomic Ions
You can make additional polyatomic ions byadding a __ to the ion!
•CO3 -2 is carbonate:
–HCO3– is ______________________
•PO43- is phosphate:
–HPO42- is ______________________
–H2PO4– is ______________________
•SO42- is sulfate
–HSO4– is ______________________
The 3 types of Chemical Bonds:________, _______ and _________
•Electronegativity and Bond Type
–Bond type can be determined by the difference inelectronegativity (degree of sharing of e-) between theelements involved
–Differences of:
•≥ 2 =_________________
•0.5-1.9 = ______________________
• ≤ 0.4 = ____________________________
•Metals bonded to other metals are___________________ bonded, regardless of thedifference in electronegativity.
Metallic bonds
–The atoms of metalsare held together whenthe atom’s _____________________________________________________________________________________________________________________
–__________________keep everythingtogether
Ionic Bonds
Complete _______ of 1 or moreelectrons from one atom to another(or a _____________________)
one _____ one or more e-, the other____ those e-s
Atoms involved are
______________________________________________________________________________
The cation and anion are attracted to eachother by _______________________
Ionic compounds are neutral
•Ionic compounds are ______________
–That is, they have no __________ charge
•This is because the number of electrons _____________________________________________________________________________________________________________________________
–Formulas reflect this neutrality- the charges onthe individual ions are not written in becausethey ______________________________________________________
CATION +CATION +
ANION --->ANION --->
COMPOUND COMPOUND
CATION +CATION +
ANION --->ANION --->
COMPOUND COMPOUND
A neutral compoundA neutral compound
requiresrequires
A neutral compoundA neutral compound
requiresrequires
COMPOUNDSFORMED FROMIONSCOMPOUNDSFORMED FROMIONS
COMPOUNDSFORMED FROMIONSCOMPOUNDSFORMED FROMIONS
Na+ + Cl- --> NaCl
Covalent Bonds
–________________valence electrons that are______________between atoms
–We are going to name only simple covalent compoundsthat have 2 elements involved
Most bonds are somewhere in betweenionic and covalent
Because not all atoms __________________________
The conventions of naming assume __________________________________in bond types
Metals bonded to nonmetals or polyatomic ions areclassified as having ionic bonds*
Materials made out of all non-metals are classified ashaving covalent bonds*
* _______________________________________________________________________________________________________________________________________________________________________________________.
For more on this, go back to bonding
Naming things:
•If there is only one element present, ____________. Atomic substances do not require “special”naming.
•For anything with more than one element,remember that there is ONE MAIN THING to lookfor:
–Is there a______________________?
So… some general help for naming:
–Look to see if there is a ________ ______inthe formula
–Again, semimetals are not a classification in naming;_______________________________________________________________________________________________________________________________________
•If there are only metals,__________________________
–(metallic bonding; nothing else need be done)
•If ________the first element is a metal, then thecompound is an ________________ compound
•Nonmetals _________ signify a _______ compound
•There is a flow chart in your handbook to help!
Naming ionic compounds:
•Remember that those are compounds that have ametal first in the formula*, and then a_______________________________________.
•We can handle these as simple types
–_______________(2 elements) compounds
–___________(more than 2 element) compounds
•Names are always for the smallest whole numberratio of the elements, the ___________
*Two exceptions to this rule:
–Compounds that start with either ammoniums (NH4+) or hydronium (H3O+)
General information for namingionic compounds:
Specifics for binary ionic compounds:
Specifics for binary ionic compounds:
1.Name the cation first, then the anion root withan –ide suffix
2.For CaCl2, the monatomic cation is Ca2+ , calcium,and the monatomic anion is Cl , named chloride.
3. We use chloride because the root for chlorine ischlor, and we use = root + -ide for the secondelement in binary compounds
•CaCl2 = calcium chloride
Example: CaCl2, or calcium chloride
Learning Check
Complete the names of the following binarycompounds:
Na3N
KBr
Al2O3
MgS
If the Metal is a Transition Metal…
__________________________are Type II Cations, and areelements that can have ____________________________________. They MUST have a__________________________________________________________________________________________________
1+ or 2+ 2+ or 3+
Cu+, Cu2+ Fe2+, Fe3+
______________________________________________
________________________________________________
Type II Cations
These elements REQUIRE Roman Numerals because theycan 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+) ____________________
CuCl (Cu+ ) ____________________
SnF4 (Sn4+) ____________________
PbCl2 (Pb2+) ____________________
Fe2S3 (Fe3+) ____________________
You will appreciate this more when we go from names to formulas!
Type II Cations
Some Type II cations have a name using the“old” system as well as the “new system”.
The old system, still widely used, adds to theroot or stem of the Latin name of the metalthe suffixes –ous and –ic. These represent thelower and higher charges respectively.
Examples of Older Names of Cations formed fromTransition Metals(you do not have to memorize these)
Learning Check
Complete the names of the following binarycompounds with variable metal ions:
FeBr2
CuCl
SnBr4
Fe2O3
Hg2S
Writing Formulas for Ionic Compounds fromNames
Formulas of ionic compounds are determined from thecharges on the ions
Na + F Na+ + F- NaF
Sodium atom + fluoride ion sodium fluoride
Charge balance: 1+ + 1- = 0
Neutral, you say?
•Formulas are written to make the compoundhave a _____________________________.
•You do NOT write the charges in the formulabecause they MUST cross out to accuratelyrepresent the compound.
•Ex: NaF2 is INCORRECT for sodium chloridebecause_________________________________________________________________________________________________________________________________________________
Writing the formula…
Write the formula for the barium chloride, thecompound that will form between Ba2+ and Cl.
Solution:
1. Write the ___________, and then the ___________.
2. Balance charge with the number of + and – ions
3. Write the number of ions needed ______________________________________:
So what if the oxidation numbersaren’t even?
•If the oxidation numbers or charges do not balance,you can write the number of ions of each until youget the same number of each charge in total.
•Yes. The “___________ ____________” _________.You take the ______ __________from the_________, and you make it the number of_________ (subscript), and take the charge on theanion, and you make that many cations (subscript).
Is there an easier way?Is there an easier way?
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 oppositeelement, so that there are now ___________ ionsand ___________ions
•This means there were _____ transferred from thelead atoms to the nitrogen atoms; the compound isneutral
Learning Check
Write the correct formula for the compoundscontaining the following ions:
1. Na+ and S2-
a) NaS b) Na2Sc) NaS2
2. Al3+ and Cl-
a) AlCl3 b) AlCl c) Al3Cl
3. Mg2+ and N3-
a) MgN b) Mg2N3c) Mg3N2
Ternary Ionic Compounds:
•Contain at least 3 elements
•There MUST be at least one polyatomic ion
(it helps to ______________)
Examples:
NaNO3____________________________
K2SO4_____________________________
Al(HCO3)3 ______________________________
Specifics for ternary ionic compounds
Specifics for ternary ionic compounds
1.Name the cation first, then polyatomic ion
2.For NaNO3, the monatomic cation is Na+ , sodium,and the polyatomic anion is NO3 , named nitrate.
–NaNO3 is sodium nitrate
3. 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
Learning Check
Match each set with the correct name:
1. Na2CO3a) magnesium sulfite
MgSO3b) magnesium sulfate
MgSO4c) sodium carbonate
2 .Ca(HCO3)2a) calcium carbonate
CaCO3b) calcium phosphate
Ca3(PO4)2 c) calcium bicarbonate
Writing Formulas for Ternary Ionic Compounds
•Write the _______ first, then the _____________.
•Overall charge must equal ____________.•Overall charge must equal ____________.
–If charges cancel–If charges cancel, just write symbols.
–If not, use ________________ to balance charges.
•Use parentheses to__________________________________________________________________________.
•Use ______________________ to indicate theion’s charge when needed (transition metals)
•Remember that the final formula should __________________________________written in.
Writing Formulas, cont’d
Example:
Cr2+ PO43-*the charges do not balance
Cr2+ PO43- ______________
The polyatomic ions is in parentheses_____________________________________________________.
This is so that we know to count anumber of those groups!
Learning Check
1. aluminum nitrate
a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3b) Cu(NO3)2c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOHb) Fe3OHc) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)
Ternary Ionic Nomenclature:
You Criss-cross these, too.
Sodium Sulfate
Iron (III) hydroxide
Ammonium carbonate
Write the Formula:
Copper (II) chlorate
Calcium nitride
Aluminum carbonate
Potassium bromide
Barium fluoride
Cesium hydroxide
General naming rules forcovalent (molecular) compounds
•Names are _______________,__________________.
–Prefixes tell you________________________.
•First element whole name with theappropriate prefix
–***NEVER use ______ for the first element!
•For the second element, use the_________ _____________ and the -ideending with appropriate prefix for thatmany.
never
You NEVER
.
Since you are sharing electrons, rather than giving them away/picking them up, the charges _______________________________.
Covalent Naming Prefixes:
PREFIX
NUMBER
1
2
3
4
5
6
7
8
9
10
Specifics for binary covalent compounds
Specifics for binary covalent compounds
1.Name the first element, using a prefix if there ismore than one atom of the element present
2.Name the second element, using the appropriateprefix in all cases
3. CO2 is carbon dioxide because there is onecarbon (no prefix when there is only one atom ofthe element,) and two oxygens (di- prefix)
Example: Example: CO2 is carbon dioxide
Learning Check
1.P2O5a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.Cl2O7a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3. Cl2a) chlorine
b) dichlorine
c) dichloride
Learning Check
Give the names of following covalent compounds:
CO
CO2
PCl3
CCl4
N2O
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
More Covalent Examples
Hydrates: Ionic Compounds·Water
•Some salts trap water crystals when theyform crystals.
–Ex: CuSO4· ___H2O
•These are ______________.
•Both the name and the formula needs toindicate _____________________________.
•In the name we add the word hydrate with aprefix that tells us how many watermolecules.
•____________________________________
Hydrates
•In the formula ____________________________________________________________.
•_____________________________________
•_____________________________________
Acid Nomenclature
•Acids
–Compounds that_________________________________
–Formulasusually_________________________________
–In order to be an acid instead of a gaseous covalentcompound, it___________________________________
•Meaning dissolved in water; symbolized by _______
–Ternary acids are ALL aqueous
–Two types:
•____________________
•____________________
Naming acids: Non-oxy acids
If the acid ________________________
•add the prefix ____________-
•change the suffix -________________
HCl_______________________
H2S _______________________
HCN _______________________
Naming acids: Oxyacids
If the formula has oxygen in it
•write the name of the ___________, but change:
•_____________________________
•_____________________________
•Watch out for sulfuric and sulfurous!
H2CrO4
HMnO4
HNO2
____________________
____________________
___________________
Acid Nomenclature Flowchart
Specifics: Acid Nomenclature
Binary Binary
TernaryTernary
An easy way to remember which goes withwhich…An easy way to remember which goes withwhich…
“In the cafeteria, you ATE something ICky”“In the cafeteria, you ATE something ICky”
HBr (aq)
H2CO3 (aq)
H2CO2 (aq)
Acid Nomenclature
Acid
Name
HNO3
HNO2
H2SO4
H2SO3
H3PO4
HC2H3O2
Name ‘Em!
•HI (aq)
•HCl (aq)
•H2SO3 (aq)
•HMnO4 (aq)
•HIO4 (aq)
Formulas of Acids
•Backwards from names.
•If it has hydro- in the name:
–_____________________________
–Anion ends in ____________
•No hydro, anion ends in ____________
–Write anion and add ______________________________________
Write the Formula!
•Hydrobromic acid
•Hydrosulfic acid
•Carbonic acid
•Phosphoric acid
•Hydrotelluric acid
Common Names
•A lot of chemicals have common namesas well as the proper IUPAC name.
•Chemicals that should always be namedby common name and never named bythe IUPAC method are:
–H2O___________________________________________________________
–NH3_______________________________________________________________
