Nomenclature:
Naming Chemicals
PO43phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
Before naming…. • Some things you MUST know to be successful…. You really need to commit these things to memory Ions: •  Atoms or groups of atoms with a _________. •  CaDons-­‐ ________ions -­‐ get by losing electron(s). •  Anions-­‐ ________ ions -­‐ get by gaining electron(s). •  Ionic bonding-­‐ held together by the ______________ (_____________________). •  Ionic solids are called ________. •  Salts are __________________; they conduct electricity when dissolved in water (aq.) Metals •
•
•
•
Conductors of heat and electricity Make ________ (lose e to become + charged) Malleable (made into ________) DucDle (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 you
go down PT
Common Ions of Elements
________ _____
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Variable, always +
Cd+2
0
Polyatomic Ions •  _______ of covalently bonded atoms that have a charge. * NO3-­‐ :___________ * NO2-­‐ :___________ •  Yes, you have to memorize them. •  Listed in your resource handbook: memorize the required list!!!! PaWerns for Polyatomic Ions •  -­‐ate ion –  _________________________________ •  -­‐ate ion plus 1 O à same charge, ___-­‐ prefix –  _________________________________ •  -­‐ate ion minus 1 O à same charge, -­‐___ suffix –  _________________________________ •  -­‐ate ion minus 2 O à same charge, ___-­‐ prefix, -­‐___ suffix –  _________________________________ Polyatomic Ions You can make additional polyatomic ions by
adding a __ to the ion!"
•  CO3 -2 is carbonate:"
–
– HCO3 is ______________________"
•  PO43- is phosphate:"
– HPO42- is ______________________"
–
– H2PO4 is ______________________"
2-
•  SO4 is sulfate"
–
– HSO4 is ______________________"
The 3 types of Chemical Bonds:
________, _______ and _________!
•  ElectronegaDvity and Bond Type –  Bond type can be determined by the difference in electronegaDvity (degree of sharing of e-­‐) between the elements involved –  Differences of: •  ≥ 2 =_________________ •  0.5-­‐1.9 = ______________________ •  ≤ 0.4 = ____________________________ •  Metals bonded to other metals are ___________________ bonded, regardless of the difference in electronegaDvity. Metallic bonds – The atoms of metals
are held together when
the atom’s _________
__________________
__________________
__________________
__________________
__________________
__________________"
–
__________________
keep everything
together"
Ionic Bonds "
—  Complete _______ of 1 or more
electrons from one atom to another
(or a _____________________)"
—  one _____ one or more e-, the other
____ those e-s"
—  Atoms involved are —
_______________________________________
_______________________________________ —  The caDon and anion are aWracted to each other 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 on the individual ions are not wriWen in because they _________________ _____________________________________ COMPOUNDS
FORMED FROM
IONS CATION +
ANION --->
COMPOUND
Na+ + Cl-­‐ -­‐-­‐> NaCl A neutral compound requires
Covalent Bonds "
–  ________________valence electrons that are
______________between atoms"
–  We are going to name only simple covalent compounds
that have 2 elements involved"
Most bonds are somewhere in between ionic and covalent —  Because not all atoms __________________________ —  The convenDons of naming assume _____________ _____________________in bond types —  Metals 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* —  * _____________________________________________ ______________________________________________ ______________________________________________ ______________________________________________. —  For more on this, go back to bonding •
Naming things: present, ________ If there is only one element ____. 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 ______________________? So… some general help for naming: –  Look to see if there is a ________ ______in the formula –  Again, semimetals are not a classificaDon in naming; _____________________________________________
_____________________________________________
_____________________________________________ •  If there are only metals, __________________________ –  (metallic bonding; nothing else need be done) •  If ________the first element is a metal, then the compound 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 a metal 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 number raDo of the elements, the ___________ *Two excepDons to this rule: –  Compounds that start with either ammoniums (NH4+) or hydronium (H3O+)
General informaDon for naming ionic compounds: Specifics for binary ionic compounds:
Example: CaCl2, or calcium chloride
1.  Name the ca7on first, then the anion root with an –ide suffix 2.  For CaCl2, the monatomic ca7on is Ca2+ , calcium, and the monatomic anion is Cl- , named chloride. 3.  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 Learning Check Complete the names of the following binary compounds: Na3N KBr Al2O3 MgS If the Metal is a TransiDon Metal… __________________________are Type II Ca7ons, and are elements that can have ______________ ______________________. They MUST have a _________________________________________________
_________________________________________________ 1+ or 2+ 2+ or 3+ Cu+, Cu2+ Fe2+, Fe3+ ______________________________________________ ________________________________________________ Type II CaDons These 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: Transi7on metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl3
(Fe3+) ____________________ (Cu+ ) ____________________ CuCl
SnF4 (Sn4+) ____________________ PbCl2 (Pb2+) ____________________ Fe2S3 (Fe3+) ____________________ You will appreciate this more when we go from names to formulas! Type II CaDons Some Type II caDons have a name using the “old” system as well as the “new system”. The old system, sDll widely used, adds to the root or stem of the LaDn name of the metal the suffixes –ous and –ic. These represent the lower and higher charges respecDvely. Examples of Older Names of CaDons formed from TransiDon Metals (you do not have to memorize these) Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 CuCl SnBr4 Fe2O3 Hg2S WriDng Formulas for Ionic Compounds from Names Formulas of ionic compounds are determined from the c
harges o
n t
he i
ons
Na + F à Na+ + F-­‐ à NaF Sodium atom + fluoride ion sodium fluoride Charge balance: 1+ + 1-­‐ = 0 Neutral, you say? •  Formulas are wriWen to make the compound have a _____________________________. •  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_______________________________
______________________________________
______________________________________
______________________________________ WriDng the formula… Write the formula for the barium chloride, the compound that will form between Ba2+ and Cl-­‐. Solu7on: 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 oxidaDon numbers aren’t even? •  If the oxidaDon numbers or charges do not balance, you can write the number of ions of each unDl you get the same number of each charge in total. Is there an easier way? •  Yes. The “___________ ____________” _________. You take the ______ __________from the _________, and you make it the number of _________ (subscript), and take the charge on the anion, and you make that many caDons (subscript). Criss-­‐Crossing in acDon: 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 ___________ ions and ___________ions •  This means there were _____ transferred from the lead atoms to the nitrogen atoms; the compound is neutral 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 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 Examples: NaNO3, and Co(NO3)2
1.  Name the ca7on first, then polyatomic ion 2.  For NaNO3, the monatomic ca7on is Na+ , sodium, and the polyatomic anion is NO3- , named nitrate. –  NaNO3 is sodium nitrate 3.  For Co(NO3)2, the monatomic ca7on is Co+2, cobalt (II) and the polyatomic anion is NO3- , named nitrate. –  Co(NO3)2 is cobalt (II) nitrate 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 WriDng Formulas for Ternary Ionic Compounds •  Write the _______ first, then the _____________. •  Overall charge must equal ____________. – If charges cancel, just write symbols. – If not, use ________________ to balance charges. •  Use parentheses to ____________________________ _________________________________________
_____. •  Use ______________________ to indicate the ion’s charge when needed (transiDon metals) •  Remember that the final formula should ________ __________________________wriWen in. WriDng 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 a number of those groups! 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
4. Tin(IV) hydroxide c) Fe(OH)3 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 for covalent (molecular) compounds •  Names are _______________, __________________. – Prefixes tell you________________________. •  First element whole name with the appropriate prefix – ***NEVER use ______ for the first element! •  For the second element, use the _________ _____________ and the -­‐ide ending with appropriate prefix for that many. NEVER never You . 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
Example: CO2 is carbon dioxide
1.  Name the first element, using a prefix if there is more than one atom of the element present 2.  Name the second element, using the appropriate prefix in all cases 3.  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) Learning Check 1. P2O5
2. Cl2O7
3. Cl2 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide a) chlorine b) dichlorine c) dichloride Learning Check Give the names of following covalent compounds: CO CO2 PCl3 CCl4 N2O More Covalent Examples §  arsenic trichloride
§  dinitrogen pentoxide
§  tetraphosphorus decoxide
Hydrates: Ionic Compounds·∙Water •  Some salts trap water crystals when they form crystals. – Ex: CuSO4·∙ ___H2O •  These are ______________. •  Both the name and the formula needs to indicate _____________________________. •  In the name we add the word hydrate with a prefix that tells us how many water molecules. •  ____________________________________ Hydrates •  In the formula ________________________ ____________________________________. •  _____________________________________
•  _____________________________________ Acid Nomenclature •  Acids – Compounds that _________________________________ – Formulas usually_________________________________ – In order to be an acid instead of a gaseous covalent compound, 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 ACIDS
start with 'H'
2 elements
3 elements
hydro- prefix
-ic ending
no hydro- prefix
-ate ending
becomes
-ic ending
-ite ending
becomes
-ous ending
Specifics: Acid Nomenclature Anion
Ending
Binary à
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
Ternary
An easy way to remember which goes with
which…
“In the cafeteria, you ATE something ICky”
Acid Nomenclature §  HBr (aq)
§  H2CO3 (aq)
§  H2CO2 (aq)
Acid
HNO3
HNO2
H2SO4
H2SO3
H3PO4
HC2H3O2
Name
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 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 _________________________ _______________________________
___ –  NH3 _____________________________ _______________________________
___