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Organic chemistry - Coggle Diagram
Organic chemistry
Hydrocarbons
Alcyclic
(closed rings)
Saturated
single bonds
CYCLOALKANES
Unsaturated
double bond
CYCLOALKENES
triple bond
CYCLOALKYNES
Aromatics
(unique 6C ring)
Benzene
intermediate between single and bond bones due to delocalised elections
Stable despite being desaturated
C6H6
Alphatic
(open carbon chains)
Saturated
= max amt of atoms attached to a singular atom
MUST BE SINGLE BONDS
C - C
ALK
ANES
Unsaturated
= less than max amt of attached to carbon bond. has at least one multiple bond
TRIPLE BOND
ALK
YNES
C ≡ C
DOUBLE BOND
ALK
ENES
C = C
Reactivity of Hydrocarbons
Combustion
all hydrocarbons are involved.
Format
: molecular formula → inorganic product
types of combustion
incomplete combustion
adequate amount of O2
CO2 (g) + H2O (g)
releases large amounts of energy
complete combustion
limited amount of CO2
CO (g) + H2O (g)
Substitution
halogenation (single bonds)
alkanes
react with halogens
NEED UV LIGHT
carbon - hydrogen bond is broken
replaced with carbon - halogen bond
condensed form
Alkane + halogen → haloalkane + hydrogen halide
*if there is enough halogen it can replace even more hydrogen cis and trans is only for alkenes
Halogenation
alkene + halogen → haloalkane
condensed structure
Addition (alkenes)
Hydrogenation
alkene + Hydrogen gas → Alkane
needs metal catalyst bc reaction is non-sponaneous
Hydrohalogenation
alkene + hydrogen halide → haloalkane
H-atom is more likely to attach to the carbon atom with the most Hydrogen atoms
Hydration
alkene + H2O → alcohol
needs acid medium
"ol" at the end
energy changes
Requirements
Activation energy
must collide with enough energy to break bonds
represented as Ea
collision theory
must collide with the appropriate orientation that facilitates the formation of new bonds
Endothermic
reaction
absorbs heat from the environment
transition state
Exothermic
reaction
releases heat from the system and into the environment
combustion
Enthalpy
measured in kj mol-1
refers to stored chemical energy
Systems
reactants + product
takes or gives energy to the surroundings
Surrounding
everything else outside the system
takes or gives energy to systems
energy conversions (joules)
kilojoules = 1 thousand J
mega joules = 1 million J
giga joules = 10^9 J
terajoules = 10^12 J
THERMOCHEMICAL QUESTIONS
includes
heat
in the equation
CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H20 (g) + 890kj mol-1
CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H20 (g) △H = 890 kj mol-1
fuels
fractional distillation
uses heat to separate the mixture into different factions
crude oil
carbon based compound made up of fossil fuels
layers of liquid filled trays that have bubble caps that stop the movement of gas.
when vapour matches the temperature of the tray the bubble cap prevents movement and condenses the vapour into liquid
types of fuels
: has special stored energy that is easy to release therefore releases more energy
fossil fuels
: non renewable energy
pros
: short term solution, faster
cons
: SUSTAINABILITY, global warming since it releases more carbon and other pollutant when it is burned
types
coal
crude oil
natural gas
biofuels
: renewable
Pros
: made with indirect sources of carbon, constantly replenished
cons
: net impact of carbon is larger
types
biogas
bioethanol
Biodiseal
renewable vs non-renewable
energy content
E / ( N x heat of combustion (△Hn))
heat of combustion is the energy released from combustion of fuels (is given in test)