Term
| In a rate-concentration graph there is a single horizontal flat line, determine the order of the compound |
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Definition
| Zero-order with respect to compound |
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Term
| What is the formula for the rate equation? |
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Definition
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|
Term
| In a two step mechanism what is the name of the first step? |
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Definition
| The rate determining step |
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Term
| What are the reactants in the rate determining step? |
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Definition
| The compounds found in the rate equation |
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Term
Produce a two-step mechanism for this:
H2 + 2ICl -> 2HCl + I2
rate=k[H2][ICl] |
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Definition
H2 + ICl -> HCl + HI
HI + ICl -> HCl + I2 |
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Term
| Define the term lattice enthalpy |
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Definition
| The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions |
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Term
| State the meaning of the term ligand |
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Definition
| Donates an electron to a metal ion / forms a coordinate bond to a metal ion |
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Term
| What is the difference between a strong acid and a weak acid? |
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Definition
| A strong acid completely dissociates and a weak acid partially dissociates |
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Term
| Explain what is meant by the term Bronsted-Lowry base |
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Definition
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Term
| Why is it difficult to predict if the lattice enthalpy of magnesium sulfide would be less/more exothermic than that of sodium oxide? |
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Definition
Mg2+ is smaller and Mg2+ has a greater charge
S2- is larger
But Mg2+ has stronger attraction and S2- has weaker attraction |
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Term
| What is a property of cobalt(II) and cobalt(III) that is typical of transition ions? |
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Definition
| They are catalysts or coloured |
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Term
| CoSO4(aq) reacts with NaOH(aq) what is the transition element species formed? And what type of reaction is it? |
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Definition
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|
Term
| CoSO4(aq) reacts with HCl(aq) what is the transition element species formed? And what type of reaction is it? |
|
Definition
CoCl4^2-
Ligand substitution |
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Term
| Write an expression for Ka of HNO2 |
|
Definition
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Term
| Ca(OH)2(aq) + HNO2(aq) write the overall equation and ionic equation |
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Definition
Ca(OH)2 + 2HNO2 -> Ca(NO2)2 + 2H2O
H+ + OH- -> H2O |
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Term
| How does equilibrium allow a buffer to control pH? |
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Definition
Added alkali reacts with H+
Shifting equilibrium to produce more H+
Added acid reacts with conjugate base(salt)
Equilibrium shifts towards HA |
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Term
| What is needed for testing cell potentials? |
|
Definition
Voltmeter
Salt bridge
Electrode (Pt or metal)
1 mol dm^-3 concentration |
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Term
| What are the three ways being developed to store hydrogen for fuel? |
|
Definition
Absorption in a solution
Adsorption on a solid
Liquid under high pressure |
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Term
| Write the equation that links free energy change with enthalpy change and temperature? |
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Definition
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Term
| Why could an exothermic reaction occur at low temperatures but not at high temperatures? |
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Definition
T/\S is more negative as temperature increases
At high temperature T/\S is more negative than /\H |
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Term
| When is a reaction feasible? |
|
Definition
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|
Term
| What is the formula for Kc? |
|
Definition
| [concentration of product]^mol / [concentration of reactant]^mol |
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Term
| What does pressure, temperature and concentrations do to Kc? |
|
Definition
Pressure and concentrations do not affect Kc
Only temperature affects Kc
The system increase/decreases products and reactants to maintain Kc |
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|
Term
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Definition
| Formation of one mole of an ionic conditions from its gaseous ions under standard conditions |
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|
Term
| Why do ionic compounds differ in melting points? |
|
Definition
There is greater attraction from smaller ions
More (heat) energy to overcome attraction |
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Term
| What happens when there is a decrease in entropy? |
|
Definition
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Term
| If enthalpy and entropy are both negative how will feasibility change as temperature increases? |
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Definition
Reaction becomes less feasible
/\G increases
T/\S becomes more negative |
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Term
| How can you work out entropy? |
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Definition
| Entropy of products - entropy of reactants |
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|
Term
| What is the equation for /\G? |
|
Definition
|
|
Term
| When does a reaction become feasible? |
|
Definition
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Term
| Write an expression of Kc for 2CH4->C2H2 + 3H2 |
|
Definition
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|
Term
| What happens to the initial rate when temperature is increased? |
|
Definition
|
|
Term
| What happens to the initial rate when pressure is increased? |
|
Definition
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|
Term
| What happens to the initial rate a catalyst is added? |
|
Definition
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|
Term
| Give two examples of large-scale uses of hydrogen |
|
Definition
Fuel cells
Manufacture of margarine
Making ammonia
Making HCl
Making methanol |
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|
Term
| Why would a reaction take place in multiple steps? |
|
Definition
Stoichiometry in rate equation does not match stoichiometry in overall equation
Collision unlikely with more than 2 ions |
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|
Term
| Draw a rate concentration graph of something that is first order |
|
Definition
|
|
Term
| Draw a rate concentration graph of something that is second order |
|
Definition
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|
Term
| How do convert pKa to Ka? |
|
Definition
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|
Term
| What are the two general equation for Ka of a weak acid? |
|
Definition
| Ka= ([H+][A-])/[HA] OR [H+]^2/[HA] |
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|
Term
| What is the equation for pH? |
|
Definition
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|
Term
| Why are Sc and Zn not transition elements? |
|
Definition
A transition element has an ion with an incomplete d-orbital
Sc and Zn are not transition element
Sc3+ is 1s2 2s2 2p6 3s2 3p6
Zn2+ is 1s2 2s2 2p6 3s2 3p6 3d10
Sc3+ d-orbital is empty
Zn2+ d-orbital is full |
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Term
| How does H2NCH2CH2NH2 act as a bidentate ligand? |
|
Definition
Electron lone pair of N
Donates two electron lone pairs to a metal ion |
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Term
| What would make a compound have stronger ionic bonds? |
|
Definition
Greater ionic charge
Smaller ionic size |
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|
Term
| What does a y=x rate-concentration graph show? |
|
Definition
|
|
Term
| What is the formula for rate equation and what is k? |
|
Definition
rate=k[]^order
k is the rate constant |
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|
Term
| How can weak acid be proved by a single pH test? |
|
Definition
|
|
Term
| What is the acid dissociation constant? |
|
Definition
|
|
Term
| What is the formula for Ka of a weak acid? |
|
Definition
|
|
Term
| What is the relation between the concentration of H+ and pH? |
|
Definition
|
|
Term
| What is the equation for Kw? |
|
Definition
|
|
Term
| What is a buffer formed from? |
|
Definition
| A weak acid and a salt of the weak acid |
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|
Term
| What happens when acid is added to a buffer? |
|
Definition
Conjugate base reacts with added acid
Equilibrium shifts to restore conjugate base (usually left) |
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|
Term
| What happens when alkali is added to a buffer? |
|
Definition
Weak acid reacts with added alkali
Equilibrium shifts to restore acid (usually right) |
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|
Term
| What is needed to set up an electrochemical cell? |
|
Definition
Voltmeter
Salt bridge
Electrodes
1 mol dm-3 solutions in each |
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|
Term
| What reaction is on the right hand side of the electrochemical cell? |
|
Definition
|
|
Term
| How is cell potential worked out? |
|
Definition
| E(positive terminal (left))-E(negative terminal (right)) |
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|
Term
| What carries the charge through the wire of an electrochemical cell? |
|
Definition
|
|
Term
| What carries the charge through the solution of an electrochemical cell? |
|
Definition
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|
Term
| What is the main difference between an electrochemical cell and a fuel cell? |
|
Definition
| A fuel cell converts energy from the reaction of a fuel with oxygen into a voltage |
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|
Term
| What is the overall reaction in a fuel cell? |
|
Definition
|
|
Term
| What are the ways to store hydrogen? |
|
Definition
Under pressure as a liquid
Adsorbed on solid
Absorbed within solid |
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|
Term
| Why is the use of hydrogen for fuel considered the same as fossil fuels? |
|
Definition
| Energy is needed to make the hydrogen |
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|
Term
| What is the expression for Kc? |
|
Definition
| Kc=([products]^mol/[reactant]^mol[reactant]^mol) |
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|
Term
| What side does equilibrium favour when pressure is increased? |
|
Definition
| The side with the least moles |
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|
Term
| When pressure increases what happens to Kc? |
|
Definition
Kc does not change
Increase in pressure causes the system to no longer be in equilibrium
So top of Kc expression increases and bottom decreases until Kc is reached |
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|
Term
| What is another method other than using fossil fuels to produce hydrogen? |
|
Definition
|
|
Term
| What is needed for a reaction to be feasible? |
|
Definition
|
|
Term
| What is the expression for /\G? |
|
Definition
|
|
Term
| What is the expression for /\S? |
|
Definition
| /\S = (sum of products) - (sum of reactants) |
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|
Term
| If T/\S is negative why would an increase in temperature cause a reaction to not be feasible? |
|
Definition
As temperature increases T/\S becomes more negative
Eventually /\G becomes positive |
|
|
Term
| What are the two transitional metals with a partially filled 4s sub-shell? |
|
Definition
|
|
Term
| What electrons get lost first in transitional metals? |
|
Definition
|
|
Term
|
Definition
| A molecule that donates an electron pair to a metal ion to form a coordinate bond |
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|
Term
| How can a molecule act as a bidente ligand? |
|
Definition
Lone pairs on two atoms
Donates two electron pairs
Forms two coordinate bonds |
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|
Term
| What are the three ways to follow the rate of reaction? |
|
Definition
Record gas volume
Observe colour changes
Electrical conductivity changes |
|
|
Term
| What is the reaction rate? |
|
Definition
| Change in amount of compounds per unit time |
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|
Term
|
Definition
| The time its takes for half of the reactant to be used up |
|
|
Term
| What has a constant half life? |
|
Definition
|
|
Term
| What is a clock reaction? |
|
Definition
| A reaction where you can easily measure the time before a product is formed |
|
|
Term
| What affects the rate constant (k)? |
|
Definition
|
|
Term
| A higher temperature does what to the rate constant (k)? |
|
Definition
|
|
Term
| How is equilibrium formed? |
|
Definition
As reactants get used up forward reaction slows down
As more product is formed the reverse reaction speeds up
Till the rate of the forward reaction is the same as the reverse reaction |
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|
Term
| What are the two main things needed for dynamic equilibrium? |
|
Definition
A closed system
A constant temperature |
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|
Term
| What is the only thing that affects Kc? |
|
Definition
|
|
Term
| Why does temperature affect Kc? |
|
Definition
Change means more product is formed
Kc will increase |
|
|
Term
| What do cells use as a buffer solution? |
|
Definition
H2PO4- <-> H+ + HPO4^2-
Dihydrogen phosphate ions and Hydrogen phosphate ions |
|
|
Term
| What does the blood use as a buffer solution? |
|
Definition
H2CO3 <-> H+ + HCO3-
Carbonic acid |
|
|
Term
| Whats a strong acid/strong alkali titration graph look like? |
|
Definition
|
|
Term
| Whats a strong acid/weak alkali titration graph look like? |
|
Definition
|
|
Term
| Whats a weak acid/strong alkali titration graph look like? |
|
Definition
|
|
Term
| Whats a weak acid/weak alkali titration graph look like? |
|
Definition
|
|
Term
| The horizontal line of a titration curve indicates? |
|
Definition
Equivalence point
Neutralised |
|
|
Term
| What is methyl oranges pH of colour change? and what is the colour change? |
|
Definition
|
|
Term
| What is phenolphthalein pH of colour change? and what is the colour change? |
|
Definition
|
|
Term
| What are the properties of transition metals? |
|
Definition
Form complex ions
Variable oxidation states
Coloured compounds
Good catalysts |
|
|
Term
What is the colour change that accompanies
Cu2+ + 2OH- -> Cu(OH)2 |
|
Definition
| Pale blue to blue precipitate |
|
|
Term
What is the colour change that accompanies
Co2+ + 2OH- -> Co(OH)2 |
|
Definition
| Pink to blue precipitate that goes back to pink |
|
|
Term
What is the colour change that accompanies
Fe2+ + 2OH- -> Fe(OH)2 |
|
Definition
| Pale green to dark green precipitate |
|
|
Term
What is the colour change that accompanies
Fe3+ + 3OH- -> Fe(OH)3 |
|
Definition
| Yellow to dark orange/brown precipitate |
|
|
Term
| What is a transition element? |
|
Definition
| Forms a stable ion with an incomplete d sub shell |
|
|
Term
|
Definition
| A transition metal coordinately bonded to one or more ligands |
|
|
Term
| What is a coordinate bond? |
|
Definition
| Dative covalent bond where a shared pair of electrons come from the same atom |
|
|
Term
|
Definition
| A molecule that can donate a pair of electrons to form a coordinate bond |
|
|
Term
| What do you call a ligand with two lone pairs? |
|
Definition
|
|
Term
| What is the structure for platin? |
|
Definition
|
|
Term
| How is cis-platin used to treat cancer? |
|
Definition
Binds to DNA of cancer cell
Prevents reproduction |
|
|
Term
| What is the reaction and colour change of aqueous copper(II) ions and ammonia? |
|
Definition
[Cu(H2O)6]2+ + 4NH3 <-> [Cu(NH3)4(H2O)2]2+ + 4H2O
Pale blue to deep blue |
|
|
Term
| What is the reaction and colour change of aqueous copper(II) ions and chloride? |
|
Definition
[Cu(H2O)6]2+ + 4Cl- <-> [CuCl4]2- + 6H2O
Pale blue to yellow |
|
|
Term
| What is the reaction and colour change of aqueous cobalt(II) ions and chloride? |
|
Definition
[Co(H2O)6]2+ + 4Cl- <-> [CoCl4]2- + 6H2O
Pink to blue |
|
|
Term
| What is the reaction and colour change of aqueous cobalt(II) ions and ammonia? |
|
Definition
[Co(H2O)6]2+ + 6NH3 <-> [Co(NH3)6]2+ + 6H2O
Pink to brown |
|
|
Term
| What does a larger Kstab mean? |
|
Definition
|
|
Term
| What is meant by stability constant? |
|
Definition
| Equilibrium constant for the formation of a complex ions from it constituent ions |
|
|
Term
| Draw the structure of haemoglobin |
|
Definition
|
|
