IB Chem stuff we need to memorise AHHHHHHHH

Name the class, functional group name and suffix

Alcohol, hydroxyl, -ol

Name the class, functional group name and suffix

Aldehyde, carboxyl, -anal

Name the class, functional group name and suffix

alkane, n/a, -ane

Name the class, functional group name and suffix

Alkene, alkenyl, -ene

Name the class, functional group name and prefixes

halogenoalkene, halogeno, (flouro, chloro, bromo, iodo)

Name the class, functional group name and suffix

alkyne, alkynyl, -yne

Name the class, functional group name and suffix

amide, amido, -anamide

Name the class, functional group name and suffix

amine, amino, -anamine

Name the class, functional group name and suffix

arene, phenyl, -benzene

Name the class, functional group name and suffix

carboxylic acid, carboxyl (acid), -anoic acid

Name the class, functional group name and suffix

ester, carboxyl (ester), -anoate

Name the class, functional group name and suffix

ether, alkoxy, -oxy[alkane]

Name the class, functional group name and suffix

ketone, carbonyl, -anone

Define First Ionization Energy

Energy required to remove one mole of electrons from one mole of gaseous ions in their ground state.

Define Electron Affinity

energy change that occurs when one mole of electrons is added to one mole of gaseous atoms

Define electronegativity

the ability of an atom to attract electrons in a covalent bond

Define Ligand

A species that uses a lone pair to form a dative/coordinate bond with a metal ion

What is the overall state of ammonium (NH₄)

+1

What is the oxidation state of hydroxide ion (OH)

-1

What is the oxidation state of nitrate ion (NO₃)

-1

What is the oxidation state of hydrogen carbonate (HCO₃)

-1

What is the oxidation state of carbonate ion (CO₃)

-2

What is the oxidation state of sulfate ion (SO₄)

-2

What is the oxidation state of phosphate ion (PO₄)

-3

Formal Charge General Rules?

FC = V - (Sticks + Stones)

Sticks - Bond line

Stone - unbonded electron

Lowest formal charge

negative values for most electronegative

HNMR spectra

Shift ppm - functional group

Integrated Area - Relative Number of Protons in hydrogen environment

Splitting - n + 1 rule → (Total Neighboring H+ ions) +1 of neighboring hydrogen environments

The ratio of split peak heights in HNMR

Pascal’s Triangle

What is TMS, what is its shift and why is it used as a reference for HNMR?

tetramethyl silane, 0ppm, unreactive+non-toxic, volatile so it is easily removed and can be analysed, all protons in TMS are equivalent this produces a strong signal away from other signals

Define Hess’ Law

Enthalpy change for a reaction is independent of the pathway between initial and final states

Define Le Chatelier’s Principle

when a system at equilibrium is subject to a change, it will respond in such a way to minimise the effect of the change

Define lattice enthalpy

the enthalpy change needed to convert 1 mole of solid crystal into its scattered gaseous ions, (HL → it is positive and is proportional to the product of the ionic charges and inversely proportional to the sum of ionic radii)

Fuel Cells vs Conventional Techniques

In Fuel cells, electrical energy is derived directly from a chemical reaction without the need for multiple transformations of energy, highly energy efficient compared to their classic counterparts.

Describe a Fuel Cell

A fuel cell consists of a spontaneous exothermic chemical reaction that is divided in two regions. These two half-reactions are separated by a polymer electrolyte membrane, but connected by a wire. The wire allows for the flow of electrons from one half of the reaction to the other. These electrons released are from an oxidation reaction and are used on the other side. The flow of electrons creates a current.

What reaction takes place on the cathode of a methanol fuel cell? REDCAT (remember state symbols!)

What reaction takes place on the anode of a methanol fuel cell? ANOX (remember state symbols!)

What is the overall reaction of a methanol fuel cell? (remember state symbols!)

Describe the net reaction in a Hydrogen Fuel Cell (remember state symbols!)

What half reaction occurs in the cathode for a hydrogen fuel cell? REDCAT

What half reaction occurs in the anode for a hydrogen fuel cell? ANOX

State the difference between atom economy and % yield

yield: amount of product formed as a % of the maximum mass that could be produced theoretically

atom economy: % of the mass (Mr) of the reactants that becomes the desired product

Define Dynamic Equilibrium (2)

When the macroscopic properties in a system remain constant (concentrations of P and R no change) and the rate of forwards and backward reactions are the same

Transition Metal Properties

variable oxidation states, forms complex ions/compounds, forms coloured compounds/ions, «para»magnetic compounds/ions

why is zinc not a transition metal?

completely filled d-orbital

Classification of Amines (Primary, Secondary vs Tertiary)

Number of Carbons connected to it.

Oxidation state for carbon ions

For each bond,

C-H -1 (Carbon more e.neg than H so it pulls electrons towards)
C-X (where X is more electronegative) +1 (X pulls towards leaving C more +ve)

Classifications of alchohols

how many carbons are 2 away? (1 - primary, 2- secondary, 3- tertiary)

Aldehydes can be synthesised how?

Oxidation of Primary Alchohols
Reagents: Primary Alchohol (E.g. Ethanol), Acidified Potassium Di Cromate K2Cr2O7 (Dilute with H2SO4)
Conditions: Distillation

Specific temperature (any more would result in further oxidation to carboxylic acids being formed)

Carboxylic Acids can be synthesised how?

Oxidation of Primary Alcohols

Reagents: Primary Alchohol, Acidifed Potassium Di Cromate

Conditions: Reflux, we want product to come back done and be oxidised again.

Aldehydes can be synthesised how?

Oxidation of Secondary Alcohols

Reagents: Secondary Alcohol, Acidifed Potassium Di Cromate

(Heat, 1 product only)

Why can't tertiary alcohols be oxidised?

No H atoms bonded to carbon that hydroxyl is bonded to, cannot oxidise without breaking the carbon C-C chain

Quantitative color change for when aldehyde becomes carboxylic acid while being synthesised

Orange → Green

Color change observed when ketones are being synthesised

Orange → Green

delta H using average bond enthalpies

Bonds Broken - Bonds formed (Reactants - Products)

Define electrolyte

A solution (or liquid) that is capable of conducting an electrical charge. The solution in an electrochemical cell.

Define electrode

Conductors of electricity used to make contact with a non-metallic part of a circuit, such as a solution in a cell (the electrolyte).

Electron flow in Voltaic Cell and Electrolytic Cell follow what rule?

A to C, Anode to Cathode

This does not determine charge of each (Anode or Cathode)

Explain polarities of electrodes in voltaic vs electrolytic cells

voltaic - anode negative, cathode positive

electrolytic - anode positive, cathode negative

voltaic - redox reaction causes electron flow, so by ANOX, electrons released from anode so negative sign.

electrolytic - driven by external source, electrons first deposited in cathode so it is negative.

What is the purpose of a salt bridge? How do ions flow? (Voltaic Cells)

Purpose

• physically separates the cathode and anode as there is no mixing of the two solutions. (Contact causes liquid junction potential ions from electrolyte may not be same charge, influencing the overall potential difference in the cell if allowed to move between solutions)

• provides an electrical path for the movement of the cations and anions in the cell

Ion flow

• cation and anions flow to prevent a buildup of charge and allow for continuous electron flow. Cations (+ve) flow to side that loses positive ions in the solution this happens in the cathode as a positive ion is reduced to a neutral ion. Anions flow to solution where positive ions are being released. This happens in anode where oxidation occurs.

How to determine reactivity using standard reduction potentials

Lower, More negative, is more unfavorable to reduce so it is more likely to oxidise