A2 Inorganic Flashcards
Reaction of sodium and water
2Na + 2H2O –> 2NaOH +H2
Product of magnesiums reaction with water at room temperature
Magnesium hydroxide
Product of heated magnesium and steam reaction
Magnesium oxide
two allotropes of phosphorus, and define allotrope
red and white, the same element with the atoms arranged differently
two products of the reaction of sulfur and oxygen
sulfur dioxide, trioxide
Which period 3 metal oxide has a polarised bond, partly covalent
aluminium oxide
product of the reaction of sodium oxide and water
sodium hydroxide
product of the reaction of magnesium oxide and water
magnesium hydroxide
the two period 3 elements that do not react with water
aluminium oxide, silicon dioxide
product of reaction of phosphorus with water
phosphoric acid, H3PO4
product of reaction of sulfur dioxide with water
sulfurous acid, H2SO3
product of reaction of sulfur trioxide with water
sulfuric acid, H2SO4
which period three oxide is amphoteric
aluminium oxide
reaction of sodium oxide and sulfuric acid
Na2O + H2SO4 –> Na2SO4 +H2O
Product of the reaction of silicon dioxide and sodium hydroxide
sodium silicate, Na2SiO3
product of Reaction of phosphoric acid and sodium hydroxide
Sodium phosphate, Na3PO4
The two transition metals that do not have full 4S orbitals
Chromium and copper
Which two d-block metals are not technically transition metals and why
scandium and zinc. They form Sc3+ and Zn2+. Neither of these have “part full” D-orbitals. Sc3+ has 3d0, Zn2+ has 3d10
What are the four properties of transition metals
variable oxidation states
colour
catalysis
complex ion formation
How are complex ions formed?
ligands form coordinate bonds with transition metals
Complex ions that are formed from dissolving a salt of a transition metal in water
aqua ions
two examples of bidentate ligands
ethane - 1,2 - diamine, ethanedioate
the name given to complex ions with polydentate ligands
chelates
Describe the chelate effect
mulitdentate ligands replace monodentate ligands due to the increase in entropy
the two types of isomerism seen in complex ions
cis-trans (or E-Z), optical
Why are transition metals coloured?
Transition metals have electrons in d- orbitals. The d- orbitals split when ligands attach. When electrons move from one orbital to the next, they absorb energy from a particular wavelength of light. The colour is missing from the spectrum, so we see the colours that are not absorbed.
what are the equations for the contact process
SO2 + V2O5 –> SO3 + V2O4
2V2O4 + O2 –> 2V2O5
Why is the reaction between S2O8- and I- so slow without a catalyst?
Both ions are negative, so they repel each other. This causes a high activation energy
Explain autocatalysis
one of the products of the reaction is the catalyst for the reaction
Why are more charged ions more acidic when dissolved in water
The higher positive charge causes electrons to be pulled closer to the nucleus as they are more polarising. As this happens to the oxygen atoms, there is less attraction for the hydrogen atoms, so they dissociate more easily
explain how adding a base to a metal aqua ion solution eventually causes the formation of an insoluble precipitate
[M(H20)6]3+ +H2O ⇌ [M(H2O)5(OH)]2+ +H3O+
Adding a base shifts the equilibrium of this reaction to the right, as the base reacts with the H3O+ ions, taking them out of solution. Therefore, the reaction attaches more OH- ligands to the aqua ion, reducing the aqua ions charge. Eventually the aqua ion has neutral charge, so becomes insoluble.
What metal aqua ion is amphoteric
aluminium hydroxide
[Al(H2O)3(OH)3]
What happens when you add excess ammonia to a metal aqua ion
ligand substitution reaction, NH3 ligand replaces H2O
What happens when you add carbonate ions to an M2+ metal aqua ion?
carbonate displaces the ligand, so a metal carbonate is formed with 6 H2O
What happens when you add carbonate ions to an M3+ metal aqua ion?
M3+ is more acidic, so the carbonate ions react with the extra H3O+ ions, shifting the equilibrium to the right, until an insoluble precipitate is formed - [M(H2O)3(OH)3]
Give the reaction of metal aqua ions that produces fizzing
carbonate with metal 3+ aqua ion
