Studied by 60 people
naming monoatomic cations
Use the element name and add ion at the end (ex. Ag+ : Silver ion)
naming monoatomic anions
Start with the name of the element, drop the ending and add “ide ion” (ex. Cl-: chloride ion)
formation of ions
only form in water
ex. Ag (s) ↔ Ag+ (aq) + e-
ex. Cl2 (g) + 2 e- ↔ 2 Cl- (g)
stock names
IUPAC system (the one we are using)
polyatomic ions
A group of atoms that behaves as a unit with the charge spread over the entire unit. Polyatomic ions are either a cation or an anion. Know common polyatomic ions
oxidation state
total number of electrons that an atom either gains or loses in order to form a chemical bond with another atom. Roman numeral determines how many oxidation states the cation has.
Polyatomic ions
A group of atoms that behaves as a unit with the charge spread over the entire unit. Polyatomic ions are a cation or an anion
type 1 cation
only has one oxidation state. You do not write the roman numeral I
type 2 cation
write roman numeral II after cation to show the multiple oxidation states
Binary Ionic Compounds
Atomic cation and anion
Atomic cation and polyatomic anion
Polyatomic or atomic cation with atomic or polyatomic anion
Cation with multiple oxidation states with atomic or polyatomic anion
know these polyatomics and their charges and formulas!
acetate, ammonium, bicarbonate (hydrogen carbonate), carbonate, chlorate, chromate, cyanide, hydroxide, nitrate, nitrite, perchlorate, permanganate, peroxide, phosphate, sulfate, sulfide
acetate
C2H3O2 (-1)
ammonium
NH4 (+1)
bicarbonate (hydrogen carbonate)
HCO3 (-1)
carbonate
CO3 (-2)
chlorate
ClO3 (-1)
chromate
CrO4 (-2)
cyanide
CN (-1)
hydroxide
OH (-1)
nitrate
NO3 (-1)
nitrite
NO2 (-1)
perchlorate
ClO4 (-1)
permanganate
MnO4 (-1)
peroxide
O2 (-2)
phosphate
PO4 (-3)
sulfate
SO4 (-2)
sulfite
SO3 (-2)
naming molecular compounds
Nonmetal to Nonmetal
Cation first
Atoms name
Polyatomic name (use prefix to define this quantity)
If there is only one cation you don’t use mono for the cation but you do use it for the anion - ex. Carbon monoxide)
Anion second
Atoms end with “ide”
Polyatomic name (use prefix to define the quantity)
Organic compound prefixes
Meth: 1 / Eth: 2 / Prop: 3 / But: 4 / Pent: 5 / Hex: 6 / Hept: 7 / Oct: 8 / Non: 9 / Dec: 10
naming formulas for acids
an acid produced H+ ions
When the anion ends with “ide”
Acid begins with “hydro” + anion + “ic acid”
HF hydrofluoric acid
When the anion ends with “ite”
Anion + “ous acid”
When the anion ends with “ate”
Anion + “ic acid”
common acids
Hydrochloric acid - HCl
Sulfuric acid - H2SO4
Nitric acid - HNO3
Ethanoic acid - HC2H3O2
Phosphoric acid - H3PO4
Carbonic acid - H2CO3
naming formulas for bases
Many bases contain OH group
Ex. NaOH = sodium hydroxide
Use the same naming rules as for type I and II inorganic compounds
Table L NYS Chem Reference Table
Ex. HOH = H2O = Water = Acid
law of definite proportions
A chemical formula tells you, by means of the subscripts, the ratio of atoms of each element in the compound. Ratios of atoms can also be expressed as ratios of masses.
The ratio of H2O is only expressed as water, nothing else.
law of multiple proportions
Whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other elements are in the ratio of small whole numbers
Hydrogen and oxygen don’t only form water, they form other compounds (that have different ratios)
naming straight hydrocarbon compounds
Count the number of carbons in the longest continuous chain
Use table P to determine the prefix
Use table Q to determine the ending of the name
Generic formula: C2H2n+2
If a molecule follows this equation, it is a simple straight chain hydrocarbon
methods for drawing hydrocarbons
Molecular formula: (ex. C4H10)
Complete structural formula: draw structure of molecule with correct orientations
Condensed structural formula: only “draw” bonds between carbon - write others as a sort of molecular formula variation
Could also leave out C bonds
Or all bonds understood - used for long chain molecules
Carbon skeleton
Line angle formula: carbons are located at each intersection and at ends of lines
rule for STRAIGHT chain hydrocarbons
*When naming a Hydrocarbon compound, pay attention to the straight chain alkanes!! Something is not hexane just because it has 6 carbons - it has to be 6 continuous carbons - cannot go backwards - if it ends at 5 carbons, you call it methyl - pentane.
naming branched chain hydrocarbons
Count the number of carbons in the longest continuous chain
Use table P to determine the prefix
Use table Q to determine the ending of the name
Identify the carbon where the branch starts
Use the smallest integer
Name the branch
Drop the ending and add “yl”
Methane = methyl, ethane = ethyl, propane = propyl
naming branched chain hydrocarbons with multiple branches
For multiple branches, identify each carbon when the branch begins
Use the smallest integer value and work up, name all (ie. 3,5 dimethyl heptane)
NOTE: be very careful when determining the longest continuous carbon chain
Can name alphabetical or numerical (ex. 2 - methyl 4 ethyl heptane OR 4 ethyl 2 methyl heptane EITHER ONE)
IF there are two of the same branches (ex. Two methyl) add a “di” to become “dimethyl”
naming unsaturated hydrocarbon Compounds
The hydrocarbon contains a double or triple bond
Naming: change ending
Double bond = “ene”
Triple bond = “yne”
Identify where the double or triple is located - if it starts at second, “2 - pentene” 3rd, “3 - pentene
Look for configuration that makes the prefix number as low as possible (ex. 1 - pentene > 2 - pentene)
Why are unsaturated fats better for weight control than saturated fats?
Unsaturated fats have double and triple bonds, storing more energy. Your body uses more energy to break these down, “burning” more food calories
naming cyclic hydrocarbon compounds
Count the number of carbons in the longest chain
Select the prefix and suffix
Add “cyclo” before the prefix
Modify ending if double or triple bonds present, add branches
naming aromatic hydrocarbons
this is when you can shift the placement of double/triple bonds and it is still the same molecule and name - naming stays the same as normal cyclic hydrocarbon compounds
when a molecule is the chain vs branch
When benzene is the “chain” 1, 3 - dimethyl - benzene When benzene is the “branch” 3 - phenyl - octane Phenyl used when benzene is the branch
naming halocarbons
Halogens
Name the hydrocarbon per the rules
Determine the location of the halogen
Use carbon number plus abbreviated halogen name
Cl = Chloro, Br = Bromo
If you need to pick a more “busy” side starting carbon chain and both look the same, do it alphabetically
naming alcohol compounds
OH attached to carbon = alcohol
Name the hydrocarbon per the rules
Determine the location of the OH group
Use carbon number to locate OH group
Drop the “e” on the alkane name and ad “ol”
Primary alcohol
OH attached to carbon, that carbon is attached to one other carbon
Secondary alcohol
OH attached to carbon, that carbon is attached to two other carbons
Tertiary alcohol
OH attached to carbon, that carbon attached to three other carbons
naming organic acid compounds
Name the hydrocarbon per the rules
The organic acid functional group is always located on carbon #1
Drop the “e” on the alkane name and add “oic acid”
O double bonded to C bonded to OH = carboxyl group
Can be written -COOH or -CO2H
order of preference for naming
anything that changes the ENDING takes precedent - so you start naming on that end
organic acids
alcohols
alkenes/alkynes
halogens
alkane groups
Formula for SATURATED hydrocarbons
NO DOUBLE BONDS
CnH2n+2
Note 
Flashcard (32)