Term
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Definition
mass of substance
__________________
molar mass |
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Term
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Definition
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Term
| In Ionic equations, only the ___________ are involved, for example, C2H4Cl2 + F2 -> C2H4F2 + Cl2 goes to... |
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Definition
reacting particles
F2 + 2Cl- -> 2f- + Cl2 |
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Term
| Number of moles in a solution = |
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Definition
concentration x volume in cm3
__________________________________
1000 |
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Term
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Definition
( Predicted yield )
(_________________) x 100
(Theoretical yield) |
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Term
| The balanced equation tells you the ratio of _______ in a reaction |
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Definition
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Term
There are how many electrons in subshell s
p
d
f |
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Definition
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Term
| Which is lower, the 4s subshell or the 3d? |
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Definition
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Term
| How many blocks are there in the periodic table, what are they called and what do the elements in them have |
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Definition
4, s, p, d, f,
s= outer shell electrons from s1 - s2
p= outer shell electrons from p1 - p6
d= outer shell electrons from d1 - d10
f= outer shell electrons from f1 - f14 |
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Term
An oxidising agent
A reducing agent |
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Definition
accepts electrons and gets reduced
donates electrons and gets oxidised |
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Term
| For oxidation states, all atoms are treated as |
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Definition
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Term
| Uncombined elements, elements bound to the same element and the overall oxidation state for compounds all have an oxidation state of |
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Definition
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Term
| In compounds, or for monatomic atoms, the oxidation state is the same as the |
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Definition
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Term
| Oxygen nearly always has an oxidation state of ______ except in __________ where it is _____, or flourides, where it is |
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Definition
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Term
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Definition
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Term
| Electronegativity increases going to the _______ on periods and _______ on groups |
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Definition
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Term
| Flourine, oxygen, nitrogen and chlorine are the most |
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Definition
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Term
| with a much more electronegative atom on one side the electrons in the bond are ______________ and this makes the molecule a ________ |
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Definition
| pulled to one side, dipole |
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Term
| If there are two equal polar bonds in opposite directions, the molecule ________ as they __________ |
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Definition
| is not a dipole, cancel each other out |
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Term
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Definition
| the electron cloud in one molecule is momentarily more to one side than the other, causing a momentary dipole |
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Term
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Definition
| When a dipole is near another molecule, the charge can attract/repel the electrons in the other molecule, causing a dipole |
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Term
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Definition
| where one atom is much more electronegative than another, pulling the electrons in the bond towards it |
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Term
| Instaneous-Induced dipole bonds |
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Definition
| the weakest intermolecular force, where a temporary dipole induces a dipole in another molecule, leading to them becoming attracted to each other. This can spark off a chain, but they are constantly created and destroyed |
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Term
| Permanent-Permanent dipole bonds |
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Definition
| Where the permanent dipoles attract each other |
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Term
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Definition
| the strongest intermolecular force, only happens when hydrogen is covalently bonded to O, N or F, as they are strongly electronegative. the bond is so polarised that the hydrogen forms weak bonds with the lone pairs of electrons on the F, N or O |
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Term
| First ionisation enthalpy |
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Definition
| the energy required to pull the first electron out of an atom/ molecule |
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Term
| 3 things that affect the ionisation enthalpies and why |
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Definition
Atomic radius - the further away the outer shell electrons are from the nucleus, the less the attraction and lower the enthalpy
Nuclear charge - more proteins in nucleus = higher attraction = higher ionisation enthalpy
Electron shielding - the inner electrons shield the outer electrons from the attraction of the protons, more inner electrons = less attraction = lower ionisation enthalpy |
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Term
| equation for ionisation enthalpies looks like this: |
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Definition
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Term
| Halogens electro-negativity increases __________ and their boiling points increase ________ |
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Definition
| up the group, down the group |
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Term
| Halogens go from ________ for bromine ________ for chlorine __________ for iodine to ____________ when reacting with alkenes |
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Definition
| orange, green, brown, colourless |
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Term
| In hexane, chlorine goes,______, bromine goes __________, iodine goes _______ |
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Definition
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Term
silver nitrate + chlorine
bromine
iodine |
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Definition
white precipitate
cream precipitate
yellow precipitate |
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Term
| Halogens go to the _______ during electrolysis |
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Definition
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Term
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Definition
| toothpaste, sanitising water, HCFC's |
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Term
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Definition
| bleach, sanitising pool water, military weapons |
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Term
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Definition
| medicines, flame retardants, pesticides |
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Term
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Definition
| medicines, essential nutrient, testing for starch |
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Term
| features of continuous process |
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Definition
| products continually enter and leave, lower labour costs, makes large amounts of product, little variation of qualit, but expensive to build, little chance of contamination unless producing more than one product |
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Term
| features of batch process |
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Definition
| makes a batch at a time, small quantities can be made, can be multi-purpose, labour costs |
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Term
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Definition
(mass of desired product)
(_______________________) x 100
(total mass of reactants) |
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Term
| to make a chloroalkane from an alcohol add _______________ and ______ |
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Definition
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Term
| to purify a chloroalkane made from an alcohol, |
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Definition
| add sodium hydrogencarbonate to neutralise any remaining acid, add distilled water to the product, shake and then run the lower layer off, remove any water by adding anhydrous sodium sulfate, and then distill the mixture |
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Term
| Halogenoalkanes reacting with hydroxide ions is |
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Definition
| nucleophilic substitution |
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Term
| Halogenoalkanes + Ammonia forms |
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Definition
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Term
| why are iodoalkanes the most reactive halogenoalkanes and fluoroalkanes the least? |
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Definition
| they have the weakest bond with the carbon and fluorine has the strongest |
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Term
| What structure does diamond have and why |
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Definition
| giant molecular structure, it forms four covalent bonds with nearby carbon atoms, forming a tetrahedral shape. It cannot conduct electricity as all electrons are held in localised bonds |
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Term
| what structure does Silican oxide have |
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Definition
| tetrahedral, doesnt conduct electricity as all electrons are used for making covalent bonds |
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Term
| A reaction wont take place unless |
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Definition
| two particles collide facing the right way with enough kinetic energy |
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Term
| minimum amount of energy required for a reaction is known as the |
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Definition
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Term
| To increase reaction rates |
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Definition
| increase temperature, pressure, surface area or introduce a catalyst |
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Term
| reversible reactions can produce |
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Definition
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Term
| dynamic equilibrium is the |
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Definition
| forward reaction occuring at the same rate as the backwards one, it can only occur in a closed system |
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Term
| increasing concentration of something in a reversible reaction |
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Definition
| shifts the equilibrium to the other side |
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Term
| increasing pressure in a reversible reaction |
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Definition
| shifts the equilibrium to the side with the fewest particles |
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Term
| Increasing temperature in a reversible reaction |
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Definition
| shifts the equilibrium to the endothermic side |
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Term
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Definition
78% nitrogen
21% oxygen
>1% Argon
0.035% CO2 |
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Term
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Definition
| Radio-Micro-IR-Visible-UV-Xrays-Gamma |
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Term
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Definition
hv
energy = planks constant x frequency in Hz |
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Term
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Definition
| a cation and anion are formed |
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Term
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Definition
| Two radicals with no charge are formed |
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Term
| reaction for creation and destruction of ozone by UV |
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Definition
O3 + hv -> O2 + O.
O2 + O. -> O3 |
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Term
| Reaction for Chlorine and ozone |
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Definition
Cl. + O3 -> O2 + clO.
ClO. +O3 -> 2O2 + Cl. |
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Term
| A reaction is electrophilic addition if |
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Definition
| atoms are added to the carbon atoms |
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Term
| reacting alkenes with ______ using a _________ catalyst makes _________ |
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Definition
| water, sulfuric acid, alcohols |
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Term
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Definition
| double bonded oxygen at the end and are produced through oxidation of primary alcohols |
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Term
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Definition
| double bond anywhere but the middle, produced through oxidation of secondary alcohols |
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Term
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Definition
| double bonded oxygen attaced to the same carbon that a -OH group is attached to, produced by full oxidation of primary oxygens |
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Term
| what are the two ways of dehydrating oxygen and what does it form |
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Definition
| ethanol passed over a hot catalyst of aluminium oxide, reflux ethanol with concentrated sulfuric acid, both form alkenes |
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Term
| To oxidise a primary alcohol |
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Definition
| Heat ethanol with potassium dichromate and sulfuric acid, then heat vigorously under reflex |
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Term
| Hydrogen bonding means that a substance will ___________________- because ______ |
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Definition
| dissolve in water it can form hydrogen bonds with it |
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Term
| addition polymerisation turns _________ into ________ |
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Definition
| alkenes, addition polymers |
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Term
| Thermoplastics ____________ when heated as they have __________ |
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Definition
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Term
| thermosetting polymers ________ when heated as they have ______- |
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Definition
| dont melt, but char, cross links |
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Term
| atoms can _______ around single, but not double bonds |
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Definition
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Term
| E isomers have both groups on the |
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Definition
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Term
| Z isomers have both groups on the |
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Definition
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Term
| Infra-red spectroscopy is where |
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Definition
| a beam of IR radiation is passed through a chemical |
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Term
|
Definition
| what frequencies of IR radiation are absorbed by the bond |
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Term
| The fingerprint region is |
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Definition
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Term
| the fingerprint region shows |
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Definition
| which bonds are present in a sample |
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