Chem 2

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  • Created by: chloe_32
  • Created on: 08-05-15 16:02
Minimum energy required for a reaction to occur
activation energy
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structural modifications to a element
allotropes
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the number of protons in the nucleus
atomic number
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fuel produced from renewable plant material
biofuel
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enthalpy change for breaking a covalent bond
dissociation
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apparatus used to measure heat change
calorimeter
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a carbon with a positive charge
carbocation
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a process with no change of co2 in the atmosphere
carbon neutral
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a substance altering the rate of reaction without being used up
catalyst
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process manufacturing sulfuric acid
contact process
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reaction when a species is oxidised and reduced
disproportionation
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reaction simultaneously in both directions
dynamic
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when no energy is lost in a collision
elastic
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the power of an atom to attract the electron density in a covalent bond towards itself
electronegativity
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when a c=c becomes saturated
electrophilic addition
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unsaturated compound is formed by removing a small molecule
elimination
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heat energy is taken in
endothermic
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amount of heat energy released when a change occurs at constant pressure
enthalpy change
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heat energy is given out
exothermic
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blue solution which when added to aldehydes forms a brick red ppt
fehlings
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region below 1500cm-1 in a infra-red spectrum
fingerprint region
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enthalpy change depends on initial and final states and is independent of the routeby which the reaction occurs
hess's law
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formation of radicals when a bond breaks equally
homolytic fission
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a system at equilibrium will respond to oppose any change imposed upon it
le chateliers principle
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average of several values of the bond dissociation enthalpy taken from a range of compounds
mean bond enthalpy
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steps by which a reaction occurs
mechanism
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unique entire infra-red spectrum of an organic compound
molecular fingerprint
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electron loss
oxidation
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substance formed in a reaction
product
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change in concentration of a substance in unit time
rate of reaction
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substance consumed in a reaction
reactant
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reactions involved oxidation and reduction
redox
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process of electron gain
reduction
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process in which a mixture is heated in a flask fitted with a condenser to prevent loss of volatile substances
reflux
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a reaction which does not go to completion
reversible
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taken as 100kPa, 298K, and standard states
standard conditions
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enthalpy change under standard conditions when 1 mol of a substance is burned completely in oxygen with all reactants and products in standard states
standard enthalpy of combustion
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enthalpy change under standard conditions when 1 mol of a compound is formed from its constituent elements with all reactants and products in standard states
standard enthalpy of formation
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compounds with the same structural formula but whose atoms are arranged differently in space
stereoisomers
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contains (Ag(NH3)2)+ which with aldehydes forms a silver mirror
tollens
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heat energy q=
mct
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ethanol is produced by the _______ of ethene
hydration
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the ending 'ate' gives what charge
negative
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NaX gives
fumes
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Cl- soluble in dilute NH3 forms
white ppt
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Br- insoluble in NH3 forms
cream ppt
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I- insoluble in concentrated NH3 forms
yellow ppt
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group 2 hydroxides _________ solubility down the group
increase
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is used as a antacid and laxative
magnesium hydroxide
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is used to reduce soil acidity
calcium hydroxide
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group 2 sulfates _________ solubility down the group
decrease
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CFCs replacement
HFCs
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Z
same
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E
opposite
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in elimination OH- acts as a
base
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o=c-h
aldehyde
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-oh
alcohol
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c=o
ketone
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ho-c=o
carboxylic acid
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when yeast forms ethanol
fermentation
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when ethanol is formed using steam a phosphoric acid catalyst, 300c, 6.5x10^3kPa
direct hydration
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Other cards in this set

Card 2

Front

structural modifications to a element

Back

allotropes

Card 3

Front

the number of protons in the nucleus

Back

Preview of the front of card 3

Card 4

Front

fuel produced from renewable plant material

Back

Preview of the front of card 4

Card 5

Front

enthalpy change for breaking a covalent bond

Back

Preview of the front of card 5
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