Chem Chapters 9, 22, 23 Williams

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

1. organic acids

2. alcohols

3. alkenes/alkynes

4. halogens

5. alkane groups

Formula for SATURATED hydrocarbons

NO DOUBLE BONDS

CnH2n+2