Term
|
Definition
| Pressure exerted on a liquid when rate of evaporation equals rate of condensation |
|
|
Term
|
Definition
| Pressure exerted on a liquid |
|
|
Term
|
Definition
| Vapour pressure equals atmospheric pressure |
|
|
Term
|
Definition
Acid = electron acceptor
Base = electron donor |
|
|
Term
|
Definition
Acid = proton donor
Base = proton acceptor |
|
|
Term
|
Definition
Acids produce hydrogen ions
Bases produce hydroxide ions |
|
|
Term
|
Definition
| Resistant to changes in pH on the addition of small amounts of acid or alkali |
|
|
Term
| Standard electrode potential |
|
Definition
| Emf generated when the half cell is connected to the standard hydrogen electrode by an external circuit and a salt bridge, under standard conditions. |
|
|
Term
| Standard hydrogen electrode |
|
Definition
298K
Hydrogen gas at 1 atm
Platinum electrode
Solution of 1M H
E=0.00 |
|
|
Term
| Negative electrode potential |
|
Definition
|
|
Term
|
Definition
Always at Anode
Losing electrons |
|
|
Term
|
Definition
Always at Cathode
Gaining |
|
|
Term
| Positive electrode potential |
|
Definition
| Greater tendency to be reduced / gain electrons than hydrogen. |
|
|
Term
| Operations of a mass spectrometer |
|
Definition
Vaporisation
Ionisation: positively ionised so it can be accelerated by electric field. And so it can be deflected.
Acceleration: by oppositely charged plates so they all have the same kinetic energy
Deflection: deflected by magnetic field according to mass: charge ratio
Detection: electronically |
|
|
Term
| Conditions in a mass spectrometer? |
|
Definition
|
|
Term
| The more reactive a metal, the more ... it's electrode potential |
|
Definition
|
|
Term
|
Definition
| Contains an aqueous solution of ions that are enables negative charge to be carried in the opposite direction to that of the electrons (from anode to cathode). |
|
|
Term
| Standard conditions for measuring electrode potentials (5 specs) |
|
Definition
Solutions have a concentration of 1 mol dm-3
All gases have a pressure of 1 atm
All substances used must be pure
Temperature is 298K
If the sol half cell does not use a solid metal then platinum is used as the electrode |
|
|
Term
|
Definition
|
|
Term
| Negative electrode potential |
|
Definition
| Less tendency to be reduced than the hydronium ion. |
|
|
Term
|
Definition
Difference in the tendencies of the half cells to be reduced.
E(where reduction occurred) - E(where oxidation took place). |
|
|
Term
| Gibbs free energy is equal to INCLUDE BOTH EQUATION |
|
Definition
= T - HS
= - Cell potential |
|
|
Term
| Spontaneous reaction G is... |
|
Definition
|
|
Term
|
Definition
| Same molecular formula but with different arrangements of atoms in space. |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Same molecular formula and structural formula but differ in the three dimensional orientation of the atoms in space |
|
|
Term
| Primary alcohol/ halogenolkane |
|
Definition
| Carbon it is attached to is attached to one other carbon |
|
|
Term
| Secondary alcohol/ halogenolkane |
|
Definition
| Carbon it is attached to is attached to two carbon atoms |
|
|
Term
| Tertiary alcohol/ halogenolkane |
|
Definition
| Carbon it is attached to is attached to three carbon atoms |
|
|
Term
|
Definition
| Bulky groups make it difficult for an incoming group to attack the carbon atom |
|
|
Term
|
Definition
|
|
Term
|
Definition
| Bond formed by the sideways overlap of parallel p orbitals |
|
|
Term
|
Definition
| Same molecular formula different structural and geometric formula |
|
|
Term
|
Definition
| Minimum energy needed to remove one mole of electrons from one mole of gaseous atoms in their ground state |
|
|
Term
|
Definition
Sea of delocalised electrons
Lattice of positive ions
Electrostatic attraction |
|
|
Term
|
Definition
| A reaction that releases heat to the surroundings as a results of forming products with stronger bonds than the reactants. |
|
|
Term
|
Definition
| A reaction that absorbs heat from the surroundings as a results of forming products with weaker bonds than the reactants. |
|
|
Term
| Standard enthalpy change of reaction |
|
Definition
| Heat energy transferred during a reaction under standard conditions of temperature (298k) and pressure (1atm) |
|
|
Term
|
Definition
| Energy needed to break one mole of bonds in gaseous molecules under standard conditions (298k |
|
|
Term
|
Definition
| Pure form of the substance under standard conditions of 298k |
|
|
Term
| Standard enthalpy of formation |
|
Definition
Enthalpy change that occurs when one mole of the substance is formed from its elements in their standard states under standard conditions of 298k and
100kpa
Products - reactants |
|
|
Term
| Standard enthalpy change of combustion |
|
Definition
Enthalpy change when one mole of the substance undergoes complete combustion under standard conditions (298k and 100kpa) and where the reactants and products are in their standard states.
Reactants - products |
|
|
Term
|
Definition
| Enthalpy change for any chemical reaction is independent of path provided the starting conditions and final conditions, and reactants and products, are the same. |
|
|
Term
|
Definition
|
|
Term
|
Definition
Differ by CH2
Similar chemical properties
Graduation in physical properties |
|
|
Term
|
Definition
| Non polar therefore do not form hydrogen bonds. Also not polar therefore colloid of water - not soluble. |
|
|
Term
|
Definition
Increase molecular size = increased van der walls = increase boiling point = decrease volatility
Lower men = gases |
|
|
Term
|
Definition
Ammonia =NH3
Ammonium = NH4 |
|
|
Term
| How do hydrogen bonds and dipole to dipole attraction affect volatility of organic compounds? |
|
Definition
| Increase strength of bonding therefore decrease volatility |
|
|
Term
| Volatility of functional groups. Highest volatility first. |
|
Definition
| Alkene - halogenoalkane - aldehyde - ketone - alcohol - carboxylic acid. |
|
|
Term
| Solubility of functional groups. |
|
Definition
Most soluble: alcohol, carboxylic acid, amine (due to hydrogen bonds)
Less soluble: aldehydes, ketones, amine, ester |
|
|
Term
|
Definition
Carbon monoxide / carbon and water.
NEVER HYDROGEN GAS! |
|
|
Term
|
Definition
| High bond enthalpies as bonds are non polar |
|
|
Term
| REACTION MECHANISM: between alkane and halogen. |
|
Definition
| Initiation, termination and propagation steps |
|
|
Term
| Verbally explain reactions mechanism between halogen and alkane |
|
Definition
Homolytic fission: splitting shared pair of electrons equally between two products.
Uv light
Then initiation, propagation and termination |
|
|
Term
| Compete combustion of alcohol produces |
|
Definition
|
|
Term
| Describe using equations the oxidation reactions of primary alcohols. Conditions. |
|
Definition
1. Acidified potassium
Dichromate.
TWO STEP REACTION
2. Alcohol - aldehyde - carboxylic acid. |
|
|
Term
| Oxidising agent for oxidisation of alcohols. |
|
Definition
Acidified potassium dichromate
=
(O) |
|
|
Term
| How do you obtain aldehyde as product? And why is it possible? |
|
Definition
| Distill it as it forms. Possible because aldehydes have lower boiling points. |
|
|
Term
| How do you obtain carboxylic acid in oxidation of primary alcohol? |
|
Definition
| Want aldehyde to remain in contact with oxidising agent for as long as possible. Therefore heat under reflux using reflux condenser. |
|
|
Term
| Are tertiary alcohols oxidised by potassium dichromate? |
|
Definition
| We are going to assume not. |
|
|
Term
| Products formed by oxidation of primary and secondary alcohols. |
|
Definition
Primary alcohol - aldehyde - carboxylic acid
Secondary alcohol - ketone ( under reflux) |
|
|
Term
|
Definition
- use halogen
- substitution reaction
- uv light
RECALL INITIATION, prop
And term |
|
|
Term
|
Definition
- hydrogen
- hydrogenation
- nickel catalyst
- 150 |
|
|
Term
| Alkene to dihalogeno alkane |
|
Definition
- use halogen
- room temp
- loss of colour |
|
|
Term
| Alkene to halogenoalkane. |
|
Definition
Use halide
Room temp
In solution |
|
|
Term
| In Alkene to halogenoalkane which halide reacts most readily- why? |
|
Definition
| HI - weakest bond therefore reacts most readily. |
|
|
Term
|
Definition
Water
Hydration
High pressure with steam
Concentrate sulphuric acid. |
|
|
Term
| Polymerisation - type of reaction and conditions |
|
Definition
- addition reaction
- high pressure
- high temperature
- catalyst |
|
|
Term
| Economic importance of alkenes |
|
Definition
Alkenes used in addition polymerisation to make synthetic plastics and cloth.
Large industry |
|
|
Term
| Alcohol combustion products |
|
Definition
|
|
Term
|
Definition
- primary alcohol
- oxidising agent = acidified potassium dichromate
- distilled |
|
|
Term
| Alcohol to carboxylic acid |
|
Definition
- primary alcohol
- oxidising agent = acidified potassium dichromate
- aldehyde to remain in contact with the oxidising agent for as long as possible therefore
- heat under reflux. |
|
|
Term
|
Definition
NUCLEOPHILIC SUBSTITUTION
AND
ELIMINATION REACTION. |
|
|
Term
| TWO REACTION MECHANISMS: Halogenoalkane to alcohol |
|
Definition
- can be SN2 or SN1 depends upon whether primary or tertiary halogenoalkane
- sodium hydroxide
- SN2 - two reactants on one - transition state - rate determined by both
- SN1: Steric
Hindrance prevents transition state. Carbocation instead.
Warm aqueous
Solution |
|
|
Term
| Rate of Nucleophilic substitution |
|
Definition
Tertiary = fastest
Primary = slowest
Expect flouroalkane to be most as flouro most electeonegative BUT
HI is weakest bond - need to break this bond therefore HI fastest. |
|
|
Term
|
Definition
6 carbon atoms in a ring
C6H6 |
|
|
Term
| Halogenoalkane to alcohol |
|
Definition
Warm reactants in aqueous solution.
Primary halogenoalkane = primary alcohol and so forth |
|
|
Term
| REACTION MECHANISM SN2 only:Halogenoalkane to amine |
|
Definition
Ammonia
Concentrated ammonia solution
High pressure.
Ammonia reacts to form other products therefore increase concentration to decrease other products. |
|
|
Term
REACTION MECHANISM sn2: Halogenoalkane to
Nitrile |
|
Definition
Substitution reaction
Cyanide ion from potassium cyanide.
Heat under reflux in solution of potassium
Cyanide in ethanol. Alcohol = Solent for polar and non
Polar. |
|
|
Term
|
Definition
Hydrogen
Nickel catalyst
Product = primary amine. |
|
|
Term
|
Definition
Introduces unsaturation into molecule.
Remove small molecule from larger molecule. |
|
|
Term
Halogenoalkane to Alkene
DRAW BOTH |
|
Definition
|
|
Term
| What is a condensation reaction? And what must be present in order for it to occur? |
|
Definition
A condensation reaction is when two molecules react to form a product with the loss of a small molecule.
In order for it to occur: must have two functional groups on each side. |
|
|
Term
|
Definition
Carboxylic acid and alcohol = ester and water
Condensation reaction
Warm carboxylic acid and h2so4 (catalyst) |
|
|
Term
|
Definition
Sweet fruity smells
Food flavourings
Perfumes
Plasticisers
Naturally occurring fats and oils.
Solvents |
|
|
Term
|
Definition
Amides
COOH NH2 = CONH(R) H2O |
|
|
Term
Deduce structure made from 1,6 - diamino hexane and hexanedioic acid. Identify repeating unit. How is it
Formed? |
|
Definition
| Polyamide making. Amine carboxylic acid = Amide. |
|
|
Term
| Economic importance of condensation reactions. |
|
Definition
| Make synthetic polymers - large industry. No need for cotton and silk |
|
|
Term
| Describe Geometrical isomerism BOTH CASES! |
|
Definition
Alkene: double bond in alkenes causes restricted rotation as free rotation would cause the pi bond to break.
Cycloalkanes: the ring in cycloalkanes causes restricted rotation due to strained bond angles.
A result of restricted rotation (must mention phrase).
CIs = xx, yy
Trans = xy, yx |
|
|
Term
| Physical and chemical properties of CIs isomers |
|
Definition
Higher coiling point than Trans as has dipole
Lower boiling point than Trans as
Cannot pack together as well.
Fairly similar chemical properties
Except |
|
|
Term
| CIs and Trans -1,2-dichloroethene |
|
Definition
|
|
Term
| CIs and tran but-2-ene-1,4-dioc acid. Explain difference in bonding and therefore difference in melting points and solubility. What happens when heated |
|
Definition
Cis: forma intramolecular hydrogen bonds (draw and you will see) therefore lower melting and boiling point. Less soluble.
Trans: intermolecular hydrogen bonds. Higher melting boiling point. More soluble.
Sublimes = Trans.
CIs = anhydride |
|
|
Term
| Explain geometrical isomerism in cycloalkanes |
|
Definition
| Ring prevents rotation. Therefore can be CIs and Trans. |
|
|
Term
|
Definition
| Asymmetric or chiral carbon = 4 diff groups. |
|
|
Term
|
Definition
Two superimposible forms of an
Optical isomer. |
|
|
Term
|
Definition
| A mixture containing two equal amounts of the two Enantiomers. Is not optically active |
|
|
Term
| Physical and chemical properties of the Enantiomers . |
|
Definition
Identical except for optical activity: rotate plane of polarisation in equal and opposite directions.
Reactivity with other chiral molecules: React to produce two very different and distinct products. Two Enantiomers react same with non chiral molecules. |
|
|
Term
|
Definition
| Rotate the plane of polarisation. |
|
|
Term
| Uses of radioisotopes. Give the THREE EXAMPLES! |
|
Definition
Carbon 14: dating - relative abundance is constant. Carbon 14 is always present in living things. Upon death don't absorb carbon 14. Level of carbon 14 falls - use of half life can give estimate of relative date of object.
Cobalt 60: radiotherapy. Treat cancer with ionising radiation. Knocks off electrons from cells = damaged. normal recover cancerous cannot recover. Penetrating gamma radiation
Iodine131: emits beta and gamma. Thyroid cancer. Iodine 125: prostate cancer. Medical tracer - detect radiation levels. |
|
|
Term
| Radioisotopes chemical properties compared to parent atom |
|
Definition
| Isotopes of elements that undergo radioactive decay. Radioisotopes share same chemical properties as atoms and have same role in body as their parent element. |
|
|
Term
|
Definition
| AVERAGE mass of an atom of the element taking into account all it's isotopes and their relative abundance, compared to one atom of carbon 12. |
|
|
Term
| Continuous v line spectrum |
|
Definition
Continuous = mixture of all wavelengths
Line: specific wavelength |
|
|
Term
| How are lines in H emission spectrum related to energy levels? |
|
Definition
Energy of photo = hf therefore different energy level transitions correspond to different wavelength of light.
8-3 = infra
7-2 = visible
6-1= ultraviolet |
|
|
Term
| Thinking about electrons in ground state - lowest energy level = |
|
Definition
| Nearest to nucleus as least potential energy |
|
|
Term
| The lines in the visible emission spectrum of hydrogen atoms converge at |
|
Definition
| Higher energy levels = 8 = furthest away from nucleus |
|
|
Term
|
Definition
| Number of ions that surround a given ion in the lattice |
|
|
Term
|
Definition
| Measuring the hydrogen ion concentration. Dont measure electron transfer regardless of lewis theory |
|
|
Term
Outline characteristics of state of
Equilibrium |
|
Definition
Concentration does not change.
Dynamic: forward and backward reaction happen at the same rate.
Closed system: no exchange of matter with surroundings.
No change in macroscopic properties |
|
|
Term
| Strong base examples (LBNK) |
|
Definition
|
|
Term
|
Definition
| Ammonia (NH3) ethylamine (C2H5NH2) |
|
|
Term
|
Definition
|
|
Term
|
Definition
Ethanoic acid (CH3COOH)
Carbonic acid (H2CO3)
Phosphoric acid (H3PO4) |
|
|
Term
|
Definition
Concentration of water =
Constant at specific temp therefore
Combine with kc = Kc[H2O] = Kw |
|
|
Term
|
Definition
Base disassociation constant
Kc[H2O] |
|
|
Term
|
Definition
| Ability of an atom to attract electrons in a covalent bond. |
|
|
Term
Atomic radii Trends
- group
- period 3 |
|
Definition
1. Atomic radii increases as no of occupied shells increases.
2. Decrease as increase in CHARGE DENSITY (atomic no) greater attraction |
|
|
Term
Ionic radii trends
- group
- period 3 |
|
Definition
1. Increases down a
Group
2. Across a period = decrease till group 4 ( increase in nuclear charge)
= 4:7 decrease due to increase in nuclear charge
3. Postive ions are smaller
Than negative ions |
|
|
Term
Melting point
- alkaline metals
- halogens |
|
Definition
- decrease down group 1 increased distance between lattice and electrons
- increase down group 7 = increase in no of electrons = stronger van der waals. |
|
|
Term
First ionisation energy trends
- period
- group |
|
Definition
Increase across period. -Increase atomic no.
Decrease down a group - effective nuclear charge remains constant while increased shielding from inner electrons.
Provides evidence of sub levels
- |
|
|
Term
Electronegativity
- period
- group |
|
Definition
Increases across a period
Decreases down a group |
|
|
Term
|
Definition
| Unimolecular Nucleophilic substitution |
|
|
Term
|
Definition
| Bimolecular Nucleophilic substitution |
|
|
Term
| Characteristic properties of transition metals |
|
Definition
| Variable oxidation number, complex ion formation, existence of coloured compounds, catalytic properties , partially filled d sub shells |
|
|
Term
| Why are scandium and zn not considered to be transition elements? |
|
Definition
Scandium - does not have partially filled d
Sub shell as an ion.
Zinc : does not have partially filled d subshell |
|
|
Term
Explain why there are variable oxidation numbers in transition metal IONS!
Oxidation states of Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn |
|
Definition
| Oxidation states of Ti , V, Cr, Mn, Fe, Co, Ni, Cu, Zn |
|
|
Term
|
Definition
| Species that uses a lone pair of electrons to form a dative covalent bond with a metal ion. |
|
|
Term
| Why are some complexes of d blocks coloured. |
|
Definition
Electric field due to lone pair of electrons splits d sub shell.
Different energy levels. Electrons absorb energy and moves between energy LEVELS.
Frequency of light absorbed means complementary colour is transmitted. |
|
|
Term
| State examples of the catalytic action of transition elements and their compounds. 4 examples requires |
|
Definition
MnO2 in decomp of hydrogen peroxide
V2O5 in contact process
Fe in haber process
Ni in conversion of Alkenes to alkanes
Co in via b
Pd and pt in catalytic converters |
|
|
Term
| Economic significance of catalysts in contact and haber process |
|
Definition
|
|
Term
Chemical and
Physical properties of nobles |
|
Definition
Mono atomic
Unreactive
Colourless
Gases |
|
|
Term
| Chemical and physical properties of group 1 |
|
Definition
Highly reactive
Good conductors of electricity
Low density
Grey shiny surfaces
Form ionic compounds |
|
|
Term
| Chemical and physical properties of group 7 |
|
Definition
Coloured
Gradual change from gases to liquid
Very reactive
Reactivity decreases down the group
Form ionic compounds
Or covalents |
|
|
Term
|
Definition
| Electrostatic attraction between oppositely charged ions. |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Electrostatic attraction between a pair of electrons and positively charged nuclei |
|
|
Term
3 charge centres
1 lone pair |
|
Definition
|
|
Term
4 charge centres
0 lone pair |
|
Definition
|
|
Term
4 charge centres
1 lone pair |
|
Definition
|
|
Term
4 charge centres
2 lone pair |
|
Definition
|
|
Term
5 charge centres
0 lone pair |
|
Definition
Triangular bipyramidal
180, 120, 90 |
|
|
Term
5 charge centres
1 lone pair |
|
Definition
|
|
Term
5 charge centres
2 lone pair |
|
Definition
|
|
Term
5 charge centres
3 lone pair |
|
Definition
|
|
Term
6 charge centres
0 lone pair |
|
Definition
|
|
Term
6 charge centres
1 lone pair |
|
Definition
|
|
Term
6 charge centres
2 lone pair |
|
Definition
|
|
Term
Diamond structure
And bonding |
|
Definition
1 carbon attached to four other carbon atoms
Sp3
Tetrahedral |
|
|
Term
| C60 - fullerene mention 4 things. |
|
Definition
Sp2 hybridised
60 atoms in a sphere
Accepts electrons to form negative ions - semiconductor
1 carbon bonded to three other carbons |
|
|
Term
|
Definition
1 carbon to three other carbon atoms
Delocalised electrons
Conducts
Sp2 |
|
|
Term
|
Definition
One silicon atom to four other silicon atoms. Tetrahedral arrangement.
Giant covalent. |
|
|
Term
|
Definition
Giant covalent structure
Each si is bonded to four oxygen atoms
Each O bonded to two
Si atoms |
|
|
Term
|
Definition
| Mixing of atomic orbitals to form new orbitals for bonding |
|
|
Term
|
Definition
| Change in concentration of reactants per unit time |
|
|
Term
|
Definition
| Minimum kinetic energy particles must have before they are able to react |
|
|
Term
| Rate of reaction depends on: 6 |
|
Definition
Temperature
Concentration
Particle size
Pressure
Catalyst
Geometry of atoms |
|
|
Term
| Maxwell Boltzmann energy distribution curve. |
|
Definition
Number of particles with kinetic energy = y
Kinetic energy
= x |
|
|
Term
| Does temperature affect the rate constant? |
|
Definition
| Yes an increase in temperature increases the rate constant. |
|
|
Term
| What MUST you remember when doing buffer calculations?? |
|
Definition
1. Disassociation of weak acid is so small = 0
Therefore concentration at eq = initial
2. Salt is fully disassociated |
|
|
Term
| Standard states of period 3 elements |
|
Definition
|
|
Term
| Period 3 oxides and standard states |
|
Definition
Na : Na2O (solid)
Mg: MgO (solid)
Al: 2Al2O3 (solid)
Si: SiO2 (solid)
P: P4O10 P4O6 (solid)
S: SO2 (solid) SO3 (liquid)
Cl: Cl2O7 (g) Cl2O (g) |
|
|
Term
| Electrical conductivity and bonding of period 3 oxides in molten state |
|
Definition
Na: high, Giant ionic
Mg: high, Giant ionic
Al2O3: high, Giant ionic
SiO2: very low, giant covalent
P4O10/P4O6: none, molecular covalent
SO3/SO2: none, molecular
covalent
Cl2O7/ Cl2O: none, molecular covalent |
|
|
Term
Period 3 oxides
Water ( only need to do Na2O, MgO, P4O10, SO3). Do Al2O3 and SiO2 react? Therefore period acid/base nature |
|
Definition
NaOH aq
Mg(OH)2 aq
H3PO4 (aq)
H2SO4 (aq)
No they do not react with water. |
|
|
Term
| Period 3 chlorides and their standard states |
|
Definition
Na : NaCl solid
Mg: MgCl2 solid
Al: AlCl3 solid AlCl6 gas
Si: SiCl4 liquid
P: PCl3 liquidPCl5 solid
S: S2Cl2 liquid
Cl: Cl2 gas |
|
|
Term
Period 3 chlorides and chlorine
water. Therefore determine acid base nature |
|
Definition
Chlorine
Water ~ HCl HOCl
NaCl: hydrated into ions - neutral
MgCl2: hydrated into ions - weakly acid
AlCl3: Al(OH)3 3HCl
SiCl4:SiO2 4HCl
PCl3 |
|
|
Term
| Difference between AlCl3 and Al2Cl6 |
|
Definition
AlCl3 = solid
Al2Cl6 = liquid. Dimer because of two dative covalent bonds from Cl to al |
|
|
Term
| Electrical conductivity of period 3 chlorides and bonding |
|
Definition
Na: highly conductive
Mg: highly conductive
Al: poor conductor
Rest = no conductivity |
|
|
Term
|
Definition
|
|
Term
| Explain how a redox reaction is used to produce electricity in a voltaic cell. |
|
Definition
| In diagram. Separate a spontaneous redox reaction into two half cells and allow electrons to transfer between by an external circuit. |
|
|
Term
| Essential components of voltaic cell. |
|
Definition
Voltmeter
Salt bridge
Two half cells |
|
|
Term
| Essential components of electrolytic cell. |
|
Definition
Battery/ cell
Electrolyte
Electrodes |
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Term
| In voltaic cell where does oxidation occur? And where does the current flow from and to? |
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Definition
Anode = oxidation
From cathode to abode |
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Term
| In electrolytic cell where does oxidation take place and where does current flow and to? |
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Definition
Anode = oxidation
From anode to cathode |
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Term
| Ions present in electrolysis of molten salts |
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Definition
| Only ions present are from salt. |
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Term
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Definition
Electrons to balance oxidation numbers.
Protons to balance charge
Add h20 to balance O2
Eliminate electrons by making them on opposite sides and equalising the magnitude |
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Term
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Definition
| charge density not just charge |
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Term
| Strong acid weak base titration point is |
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Definition
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Term
| What happens at titration point weak acid strong base? Why is titration point above 7ph? |
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Definition
| At titration point all acid is used up. Resulting ph is dependent on poh as only base from partial disassociation of weak acid left. No strong base or partial disassociation of weak acid. Therefore higher than 7 ph |
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Term
| Titration point on graph = |
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Definition
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Term
| State hasselbalch henderson equation |
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Definition
| Ph = pka log [partial disassociated acid or base]\[HA] |
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Term
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Definition
Secondary alcohol
Acidified potassium dichromate
Heat under reflux
Sec alcohol [O] ~ ketone water |
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Term
Alcohol to
Aldehyde and then carboxylic acid equations |
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Definition
Alcohol [O] ~ aldehyde water
Aldehyde [O] ~ carboxylic acid water |
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Term
| Equivalence point in strong acid and base |
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Definition
Strong base completely neutralises strong acid.
HCL ~ Cl and h
Cl is not base = neutral therefore neutral ph at 7 |
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Term
| State relationship between HA and A- or BOH and B at half equivalence point |
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Definition
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Term
| A buffer is most effective at... |
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Definition
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Term
| High concentration of NaCl in aqueous solution. What is produced at each electrode. |
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Definition
When concentrated = Cl and h2
Low concentration= O2 and h2 |
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Term
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Definition
Electrolyte of ions to be deposited.
Cathode = metal to be plated.
Anode = inert electrode.
Obs: cathode getting plated, possible loss of colour if Cu2 = blue |
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Term
| Observations alkali metals added to water. |
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Definition
Hydrogen gas evolved.
Temp of water increases.
Clear, colourless solution is formed. |
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Term
| Properties of alkali metals |
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Definition
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Term
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Definition
Four oxygen to one si .
Both oxygen and si are sp3 hybridise. Each oxygen connected to two si |
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Term
| When describing emission spectra must mention |
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Definition
| Convergence at higher energy levels |
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Term
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Definition
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Term
| Choosing indicator look at pH at ... |
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Definition
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Term
| Enthalpy change of atomisation . |
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Definition
| Heat change that occurs when one mole of gaseous atoms are formed from the element in its standard state. |
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Term
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Definition
| enthalpy change when one mole of gaseous atoms attracts one mole of electrons. |
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Term
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Definition
| enthalpy change when one mole of gaseous negatively charged ions attract one mole of electrons. |
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Term
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Definition
| Enthalpy change that occurs when one mole of a solid ionic compound is separated into gaseous ions under standard conditions. |
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Term
| Kc and rate constant only change for |
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Definition
| Temperature. Does not change with pressure, concentration etc |
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Term
| Difference in conditions between Nucleophilic substitution and elimination. |
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Definition
Sub: dilute solution, aqueous, warm
Elim: concentrated, ethanolic, hot |
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Term
| Region of em spectrum used in HNMR spectroscopy. |
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Definition
Radio waves
Provide energy needed to flip nuclei. |
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Term
| Sub level with highest energy |
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Definition
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