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161 Cards in this Set
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- Back
- 3rd side (hint)
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What is the enthalpy of formation? |
The enthalpy change when one mole of a compound is formed from its constituent elements, all reactants and products in their standard states under standard conditions |
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Define the enthalpy of atomisation |
Then enthalpy change which accompanies the formation of one mole of gaseous atoms from the element in its standard states under standard conditions |
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What is the First ionisation energy? |
First ionisation energy is the standard enthalpy change when one mole of gaseous atoms is converted into a mole of gaseous ions, each with a single positive charge |
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What is the first electron affinity? |
The first electron affinity is the standard enthalpy change when a mole of gaseous atoms is converted into one mole of gaseous ions, each with a single negative charge |
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What is The second electron affinity? |
The second electron affinity is the enthalpy change when one mole of Electrons is added to one mole of gaseous ions, each with a single negative charge to form ions each with two negative charges |
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What is the lattice formation enthalpy? |
The lattice formation enthalpy is the standard enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions. |
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What is the enthalpy of hydration? |
The enthalpy of hydration is the standard enthalpy change when water molecules surround one mole of gaseous ions. |
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What is the enthalpy of solution? |
The enthalpy of solution is the standard enthalpy change when one mole of solute dissolves completely in sufficient solvent to form a solution in which the molecules or ions are far enough apart to not interact with each other. |
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What is the mean bond enthalpy? |
Mean bond enthalpy is the enthalpy change when one mole of gaseous molecules each breaks a covalent bond to form two free radicals, averaged over a range of compounds |
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What is an exothermic reaction |
A reaction that gives out heat energy. It has a negative delta H |
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What is an endothermic reaction? |
A reaction that takes in heat energy. It has a positive delta H |
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What are standard conditions? |
Pressure of 100kPa and a temperature of 298K |
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When bonds break is it an exothermic or endothermic process? |
Endothermic |
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The second law of thermodynamics says that entropy is always________ |
Increasing |
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The symbol for change in entropy is.... |
Delta S |
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For a reaction to be feasible it has to...... |
Have a positive entropy change |
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What is the equation for gibb's free energy? |
Delta G = delta H - temperature × system entropy change |
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For a reaction to be feasible at any temperature it has to be..... |
Exothermic |
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The temperature in which a reaction is feasible is the.... (Aka delta T =?) |
Enthalpy change divided by the entropy change of a system |
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When the lattice enthalpy of an ionic compound was calculated, the value was somewhat smaller than the theoretical value. Why would this be? |
Because ionic bonds in reality are not purely ionic |
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What period 3 elements react with cold water? |
Sodium, magnesium and chlorine |
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What is the equation of the reaction of sodium with water? Include state symbols |
2Na(s) + 2H2O(l)——> 2NaOH(aq) + H2 (g) |
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What is the pH of the solution formed from sodium and water? |
13-14 |
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What is the reaction of magnesium with water? Include state symbols |
Mg(s) + 2H2O(l) ——> Mg(OH)2(aq) + H2(g) |
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What is the pH of a solution formed from magnesium and cold water? |
~10 |
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Write the reaction of magnesium and steam |
Mg(s) + 2H2O(l) ——> MgO(s) +H2(g) |
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What type of reaction is the reaction between sodium and water? |
Redox |
Oil rig |
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What type of reaction is the reaction between magnesium and water/steam? |
Redox |
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Why is sodium more reactive than magnesium? |
Because it takes less energy for sodium to lose one electron than it does for magnesium to lose two |
Electron loss |
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Write the reaction of sodium with oxygen. Include state symbols |
2Na(s) + 1/2 O2(g)——> Na2O(s) |
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What is an allotrope? |
An element that exists in more than one form |
Carbon is an allotrope |
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Write the reaction of magnesium with oxygen. Include state symbols |
2Mg(s) + O2(g)——> 2MgO(s) |
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What colour does sodium burn with |
A yellow flame |
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How can you distinguish between sodium and aluminium? |
Set the **** on fire. Sodium will burn with a yellow flame and aluminium windows burn with a white flame |
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Write the reaction of aluminium with oxygen. Include state symbols. |
4Al(s) +3O2(g)——>2Al2O3(s) |
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Why does aluminium appear to be unreactive? |
Because it is always coated in a layer of aluminium oxide |
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Write the reaction of silicone and oxygen. Include state symbols |
Si(s) + O2(g)——>SiO2(s) |
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Write the reaction of phosphorus and oxygen. Include state symbols |
4P(s) + 5O2(g) ——>P4O10(s) |
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Write the reaction of sulphur and oxygen including state symbols |
S(s) + O2(g) ——> SO2(g) |
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Why do metal oxides have high melting points? |
Because they form ionic lattices |
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What colour does sulphur burn? |
Blue |
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What does Amphoteric mean? |
That the species can act as both an acid and a base |
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When you react phosphorus pentoxide with 6 water molecules you get what? |
4 phosphoric acid, H3PO4 molecules |
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Sulphur dioxide reacts with water to give what |
H2SO3. A weak acid. |
Not sulphuric acid, but similar |
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Sulphur trioxide reacts with water to give what? |
Sulphuric acid |
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What is the trend with period 3 oxides bonding and acidity? |
The more ionic the solution, the more alkaline. The more covalent, the more acidic. |
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Apart from your mum, what is slag? |
The chemical impurities that have been removed |
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Sodium oxide reacts with sulphuric acid to give what? |
Sodium sulphate, Na2SO4 and water |
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Write the chemical equation for magnesium oxide and hydrochloric acid. Include all state symbols |
MgO(s) + 2HCl(aq) ——> MgCl2(aq) + H2O(l) |
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Aluminium oxide is Amphoteric. Write the reactions between aluminium oxide and both a strong acid and a base. |
Al2O3 + 6HCl ——> 2AlCl3 + 3H2O Al2O3 + 2NaOH + 3H2O ——> 2NaAl(OH)4 |
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Silicon dioxide will react as a______ acid with_______ bases |
Weak, strong |
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What colour, if any, is sodium silicate? |
Colourless |
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Write the equation for the reaction between silicon dioxide and sodium hydroxide |
SiO2(s) + 2NaOH(aq)——>Na2SiO3(aq) + H2O(l) |
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When you react phosphorus pentoxide with aqueous sodium hydroxide, you are really reacting____________ with sodium hydroxide |
Phosphoric acid |
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Write the 3 stages of reaction for phosphorus pentoxide with aqueous sodium hydroxide. Remember the reagents are not what you would think they are. |
H3PO4 + NaOH ——> NaH2PO4 +H2O NaH2PO4 + NaOH ——> NaHPO4 +H2O NaHPO4 + NaOH ——> NaPO4 +H2O The reagent is phosphoric acid because phosphorus pentoxide will react instantly with water to give phosphoric acid. |
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Write the 2 stages of the sulfur dioxide and sodium hydroxide reaction . Include state symbols |
SO2(g) + NaOH(aq) ——> NaHSO3(aq) NaHSO3(aq) +NaOH (aq) ——>NaSO3(aq) + H2O(l) |
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When we connect two electrodes together, the more positive one is being_______Ed and the more negative one is being________Ed |
Oxidised, reduced |
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What is the primary standard electrode? |
The hydrogen electrode |
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In day to day experiments, we don't use the standard electrode. Why is this? |
Because it is very difficult to maintain and set up |
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What is a secondary standard electrode? |
An electrode that has had its potential adjusted to the primary standard electrode |
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Why would we use a secondary electrode? |
Because the hydrogen electrode is quite hard to set up |
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Give an example of a non-rechargable cell |
Zinc/copper cell, the Daniel cell Zinc/carbon cells the leclanchè |
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Why is zinc not a transition metal? |
Because zinc does not form ions with an incomplete d orbitals |
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Why is scandium not a transition metal? |
It forms ions with an empty d orbitals |
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What is the short-handed electronic configuration for chromium? |
[Ar] 3d5 4s1 |
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What is the short-handed electronic configuration for copper |
[Ar] 4s1 3d10 |
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Which transition elements are conducive? |
All of them |
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What colour is the copper 2+(aq) ion? |
Blue |
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What is the coordination number of a transition element? |
The number of coordinate bonds it forms |
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What is a ligand? |
An ion or molecule with a lone pair of Electrons that forms a coordinate bond with a transition metal |
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What shape is an ion with a coordination number 6? |
Octahedral |
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What shape is an ion with coordinate number 4? |
Tetrahedral |
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What is a multidentate ligand? |
A ligand that forms more than one coordinate bond |
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What is a chelate? |
A complex ion with one or more polydentate ligands attached |
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What is a bidentate ligand? |
A ligand that can form 2 coordinate bonds with a transition metal |
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How many coordinate bonds does edta form? |
Up to 6 bonds |
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What is a use for chelates, like edta |
Chelates are used to make metal ions precipitate out. This is used as an antidote for transition metal poisoning. The metal precipitates out and you piss it out. |
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What shape is a complex ion with coordination number 2? |
Linear |
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Give an example of a linear complex ion |
Silver something |
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Write the half equation for the reduction of tollens reagent. |
[Ag(NH3)2]+ e- ——> Ag +2NH3 |
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Why are transition metals coloured? |
Transition metals have part filled d orbitals. This allows their Electrons to move from one d orbital to another. Because each d orbital has a slightly different energy in a compound, the Electrons absorb light in the visible spectrum to move to higher energy orbitals. Because they only absorb certain wavelengths, the wavelengths that they do not absorb we see as the colour of the transition metal. |
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When you connect two electrodes together, do the electrons go from the more positive to negative, or vice-versa? |
Goes from more negative to positive |
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When do you use a platinum electrode, apart from the standard electrode? |
When going from an ion to another ion. |
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Electrodes are always in equilibrium. This means they are affected by ____, _____ and _______ |
Temperature, pressure and concentration |
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What concentration is an electrode solution, when measuring electrode potentials? |
1moldm-³ |
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The standard electrode potential of a half cell is... |
The voltage measured under standard conditions when the half cell is connected to a standard hydrogen electrode |
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The more reactive a metal is the more ______ its electro potential is |
Negative |
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The more reactive a non-metal is, the more _____ its electro potential |
Positive |
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What are the advantages of non rechargeable cells? |
They are cheaper Longer lifetime |
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What are the disadvantages of non rechargeable batteries? |
Can't deliver the power of a rechargeable Toxic as **** Bit of a waste |
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what is the common oxidation state(s) for scandium? |
3+ |
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what is the common oxidation state(s) for titanium |
4+ |
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what is the common oxidation state(s) for vanadium |
4+ and 5+ |
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What are the 3 common oxidation states for chromium? |
2+, 3+, 6+ |
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What is the common oxidation state(s) for manganese? |
2+, 4+ and 7+ |
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Give the variable oxidation states of Fe |
2+,3+ |
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What is the oxidation state(s) cobalt can be in? |
2+,3+ |
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What is nickels common oxidation state(s) |
2+ |
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Copper can exist in what oxidation state(s) |
1+, 2+ |
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Zinc exists in what oxidation state(s) |
2+ |
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What are the steps for forming a redox equation |
1. Write both half equations 2. Balance the oxygens with waters 3. Balance hydrogens with H+ 4. Multiply each half equation by the number of electrons in the other 5. Add them together to cancel the species |
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What happens when a charged complex ion is oxidised or reduced to a neutral complex? |
It precipitates out |
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A positive complex ion tends to be acid or alkaline? |
Acid |
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A negative complex ion tends to be acid or alkaline? |
Alkaline |
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What is the colour of Cr (II) |
Blue |
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What colour is Cr(III) |
Green |
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What colour is Cr(VI)? |
Yellowish orange |
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What is useful about chromium in the VI oxidation state? |
It can used as an oxidising agent in organic chemistry (acidified potassium dichromate) |
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What is the equilibrium equation for the dichromate ion? |
2CrO4²- (aq) + 2H+ (aq) <----> Cr2O7²-(aq) + H2O(l) |
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In a perfect world, catalysts should last forever, why doesn't it? |
Because there is some **** in solutions and stuff which make it impure, and these react with the catalysts and poison them |
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Write the haber process equilibrium reaction, along with what catalyst it uses |
N2(g) + 3H2(g) <-----> 2NH3(g) Fe catalyst |
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What is the contact process? |
The process used to produce sulfur trioxide, used to make sulfuric acid |
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Name the catalyst for the contact process(a step in sulfuric acid manufacture) and state the chemical formula |
Vanadium oxide, V2O5 |
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What is synthesis gas? |
A mixture of carbon monoxide and hydrogen |
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What do we use synthesis gas (CO + 2H2) for? |
The production of methanol |
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What is autocatalysis? |
The process in which a reaction is catalysed by its own products. Aka it speeds up as it goes |
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What is the lewis definition of an acid? |
An electron pair acceptor. (You can remember the lewis stuff as the opposite of the bronsted Lowry **** as they say an acid is a proton DONOR) |
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What are aqua ions? |
Ions dissolved in water or transition metals with water ligands. E.g. [Fe(H2O)6]³+ |
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Which is the stronger acid? Fe3+ or Fe2+? Think about charge densities. |
Fe3+ |
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How can you tell the difference between a 2+ and 3+ transition metal ion?
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Add carbonate. The 3+ ion makes CO2 bubbles and the 2+ doesnt |
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Write the equation for aluminium hydroxide and HCl |
Al(H2O)3(OH)3 + 3HCl ---------> [Al(H2O)6]3+ + 3Cl- |
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Al(H2O)3(OH)3 + OH- gives what? |
[Al(OH)4]- and 3 waters |
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Why do aqueous transition metals even react? |
Because water is a **** ligand so basically everything forces it out the complex |
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What is the colour of aqueous iron 2+? |
Pale green |
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Name the colour of cobalt 2+ aqueous |
Pink |
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[Cu(H2O)6]2+ is what colour? |
Pale blue |
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What colour is Fe³+(aq) |
Purple/yellow/brown I'm sorry but how the **** can something be purple yellow and ******* brown?! |
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What colour is aqueous aluminium? |
Colourless |
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What is the colour of chromium 3+? |
Green |
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Fe2+(AQ) reacts with a little OH- to give what? State the colour |
Green gelatineous precipitate, Fe(OH)2(H2O)4 |
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Fe2+ and excess hydroxide gives what? State the colour as well. |
Green gelatineous precipitate of Fe(H2O)4(OH)2 |
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Aqueous iron (II) and a little ammonia gives what? Give the colour |
Green gelatineous precipitate, Fe(OH)2(H2O)4 |
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What does an excess of ammonia and aqueous iron 2+ give? Give the colour |
Green gelatineous precipitate, Fe(OH)2(H2O)4 |
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When you react iron 2+ with a carbonate what do you get? And the colour. |
FeCO3 ppt. Green. |
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What do you get when reacting Co2+ with OH-? Give the colour of the product. |
Blue ppt. Of Co(H2O)4(OH)2 |
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What do you get when reacting Co2+ with excess OH-? Give the colour of the product. |
Blue ppt. Of Co(H2O)4(OH)2 |
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What do you get when reacting Co2+ with NH3? Give the colour of the product. |
Blue ppt. Of Co(H2O)4(OH)2 |
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What do you get when reacting Co2+ with excess NH3? Give the colour of the product. |
Pale yellow-brown solution of [Co(NH3)6]2+ |
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What do you get when reacting Co2+ with carbonate? Give the colour of the product. |
Pink precipitate of CoCO3 |
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What do you get when reacting Copper 2+ with OH-? Give the colour of the product. |
Pale blue precipitate of Cu(H2O)4(OH)2 |
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What do you get when reacting Copper 2+ with excess OH-? Give the colour of the product. |
Pale blue precipitate of Cu(H2O)4(OH)2 |
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What do you get when reacting Copper 2+ with NH3? Give the colour of the product. |
Pale blue precipitate of Cu(H2O)4(OH)2 |
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What do you get when reacting Copper 2+ with excess NH3? Give the colour of the product. |
Deep blue [Cu(NH3)4(H2O)2]2+ |
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What do you get when reacting Copper 2+ with carbonate? Give the colour of the product. |
Blue/green precipitate of CuCO3 |
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What do you get when reacting iron 3+ with OH-? Give the colour of the product. |
Brown gelatineous precipitate of Fe(H2O)3(OH)3 |
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What do you get when reacting iron 3+ with excess OH-? Give the colour of the product. |
Brown gelatineous precipitate of Fe(H2O)3(OH)3 |
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What do you get when reacting iron 3+ with NH3? Give the colour of the product. |
Brown gelatineous precipitate of Fe(H2O)3(OH)3 |
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What do you get when reacting iron 3+ with excess NH3? Give the colour of the product. |
Brown gelatineous precipitate of Fe(H2O)3(OH)3 |
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What do you get when reacting aluminium 3+ with OH-? Give the colour of the product. |
White precipitate of Al(H2O)3(OH)3 |
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What do you get when reacting aluminium 3+ with excess OH-? Give the colour of the product. |
Colourless solution of [Al(OH)4]- |
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What do you get when reacting aluminium 3+ with NH3? Give the colour of the product. |
White precipitate of Al(H2O)3(OH)3 |
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What do you get when reacting aluminium 3+ with excess NH3? Give the colour of the product. |
White precipitate of Al(H2O)3(OH)3 |
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What do you get when reacting aluminium 3+ with carbonate? Give the colour of the product. |
White precipitate of Al(H2O)3(OH)3 and bubbles |
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What do you get when reacting iron 3+ with carbonate? Give the colour of the product. |
Brown gelatineous precipitate of Fe (H2O)3(OH)3 and Bubbles |
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What do you get when reacting chromium 3+ with OH-? Give the colour of the product. |
Green precipitate of Cr(H2O)3(OH)3 |
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What do you get when reacting chromium 3+ with excess OH-? Give the colour of the product. |
Green solution of [Cr(OH)6]3- |
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What do you get when reacting chromium 3+ with NH3? Give the colour of the product. |
Green precipitate of Cr(H2O)3(OH)3 |
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What do you get when reacting chromium 3+ with excess NH3? Give the colour of the product. |
Purple solution of [Cr(NH3)6]3+ |
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What do you get when reacting chromium 3+ with carbonate? Give the colour of the product. |
Green precipitate of Cr(OH)3 and CO2 bubbles |
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When do we use the lewis definition for acids? |
Transition metal chemistry |
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When do we use the bronsted Lowry definition? |
When hydrogen's get involved |
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