Chem Chapters 9, 22, 23 Williams

Use the element name and add ion at the end (ex. Ag+ : Silver ion)

Start with the name of the element, drop the ending and add “ide ion” (ex. Cl-: chloride ion)

only form in water

ex. Ag (s) ↔ Ag+ (aq) + e-

ex. Cl2 (g)  + 2 e-  ↔ 2 Cl- (g)

IUPAC system (the one we are using)

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

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.

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

only has one oxidation state. You do not write the roman numeral I

write roman numeral II after cation to show the multiple oxidation states

• 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

acetate, ammonium, bicarbonate (hydrogen carbonate), carbonate, chlorate, chromate, cyanide, hydroxide, nitrate, nitrite, perchlorate, permanganate, peroxide, phosphate, sulfate, sulfide

C2H3O2 (-1)

NH4 (+1)

HCO3 (-1)

CO3 (-2)

ClO3 (-1)

CrO4 (-2)

CN (-1)

OH (-1)

NO3 (-1)

NO2 (-1)

ClO4 (-1)

MnO4 (-1)

O2 (-2)

PO4 (-3)

SO4 (-2)

SO3 (-2)

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)

Meth: 1 / Eth: 2 / Prop: 3 / But: 4 / Pent: 5 / Hex: 6 / Hept: 7 / Oct: 8 / Non: 9 / Dec: 10

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”

• Hydrochloric acid - HCl

• Sulfuric acid - H2SO4

• Nitric acid - HNO3

• Ethanoic acid - HC2H3O2

• Phosphoric acid - H3PO4

• Carbonic acid - H2CO3

• 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

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.

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)

• 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

• 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

*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.

• 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

• 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”

• 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)

• Unsaturated fats have double and triple bonds, storing more energy. Your body uses more energy to break these down, “burning” more food calories

• 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

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 benzene is the “chain” 1, 3 - dimethyl - benzene When benzene is the “branch” 3 - phenyl - octane Phenyl used when benzene is the branch

• 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

• 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”

OH attached to carbon, that carbon is attached to one other carbon

OH attached to carbon, that carbon is attached to two other carbons

OH attached to carbon, that carbon attached to three other carbons

• 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

anything that changes the ENDING takes precedent - so you start naming on that end

1. organic acids

2. alcohols

3. alkenes/alkynes

4. halogens

5. alkane groups

NO DOUBLE BONDS

CnH2n+2