22 Periodicity Flashcards by Orla Doyle

Magnesium and cold water

Mg(s) + 2H2O (l) ➡️ Mg(OH)2 (aq) + H2
Reaction slow at room temp

Mg(s) + H2O ➡️ MgO (s) + H2

Both redox reactions

How well did you know this?

Not at all

Perfectly

Sodium and cold water

2Na(s) + 2H2O(l). ➡️ 2NaOH (aq) + H2 (g)

Vigorous
Sodium floats on the surface and fizzes rapidly

How well did you know this?

Not at all

Perfectly

sodium
magnesium
aluminum

metallic
shiny (when freshly exposed to air)
conduct electricity
react with dilute acids to give hydrogen and salts

How well did you know this?

Not at all

Perfectly

silicon

semi-metal (metalloid)
conduct electricity to some extent
semiconductor

How well did you know this?

Not at all

Perfectly

Phosphorus
sulfur
chlorine

non-metals
do not conduct electricity
low melting and boiling points

How well did you know this?

Not at all

Perfectly

argon

chemically unreactive

exists as separate atoms

How well did you know this?

Not at all

Perfectly

sodium and oxygen

burns brightly in air
with a yellow flame (because of sodium peroxide Na2O2)
2Na (s) + 1/2 O2 (g) ➡️ Na2O (s)

How well did you know this?

Not at all

Perfectly

period 3 and oxygen

relativity reactive

reactions are exothermic

How well did you know this?

Not at all

Perfectly

magnesium and oxygen

strip of magnesium ribbon burns in air with a bright white flame
white power produced is magnesium oxide

2Mg (s) + O2(g) ➡️ 2MgO

How well did you know this?

Not at all

Perfectly

aluminium and oxygen

burns brightly

4Al (s) + 3O2(g) ➡️ 2Al2O3

How well did you know this?

Not at all

Perfectly

aluminium

reactive metal but it is always coated with a strongly bonded structure layer of oxide, this protects it from further reaction
so it appears as an unreceptive metal

How well did you know this?

Not at all

Perfectly

silicon and oxygen

Si (s) + O2 (g) ➡️ SiO2 (s)

How well did you know this?

Not at all

Perfectly

red phosphorus and oxygen

has to be heated before it will react with oxygen

4P(s) + 5O2(g) ➡️ P4O10(s)

How well did you know this?

Not at all

Perfectly

white phosphorus and oxygen

spontaneously ignites in air

4P(s) + 5O2(g) ➡️ P4O10(s)

limited supply of oxygen
4P(s) + 5O2(g) ➡️ P2O3(s)

How well did you know this?

Not at all

Perfectly

sulfur and oxygen

when sulfur powder is heated and lowered into a gas jar of oxygen, it burns with a blue flame to form the colourless gas sulfur dioxide

S(s) + O2(g) ➡️ SO2(g)

How well did you know this?

Not at all

Perfectly

sodium oxide
magnesium oxide
aluminum oxide

giant ionic lattices

high melting points

Aluminum oxide

ionic but has some covalent character

small ion with a large positive charge

silicon oxide

ginat covalent (macromolecular) structure
high melting point because many strong covalent bonds must be broken to melt it

phosphorus and sulfur oxide

covalently bonded molecules
intermolecule forces are weak van Der Waals and dipole-dipole forces
relatively low melting points

structure of sodium oxide

giant ionic

structure of magnesium oxide

giant ionic

structure of aluminium oxide

giant ionic

structure of silicon oxide

giant covalent ( macromolecular)

structure of phosphorus oxide

molecular

structure of sulfur oxide

molecular

sodium oxide (basic)

Na2O (s) + H2O (l) ➡️ 2Na+(aq) + 2OH- | pH = 14

Magnesium oxide (basic)

magnesium hydroxide is sparing soluble MgO(s) + H20(l) ➡️ Mg(OH)2(s) Mg(OH)2(s) Mg2+ (aq) + 2OH- (aq) pH = 9

insoluble oxides

aluminium oxide and silicon dioxide are both insoluble in water (silicon dioxide are sand)

phosphorus pentoxide and water (acidic )

phosphorus pentoxide reacts quite violently with water to produce an acid solution of phosphoric acid P4O10(s) + 6H2O(l) ➡️ 4H3PO4(aq) H3PO4(aq) H+(aq) + H2PO4-(aq) pH = 1-2

sulfur dioxide and water (acidic)

sulfur dioxide is fairly soluble in water and reacts to give an acidic solution of sulphuric acid. SO2(g) + H20(l) ➡️ H2SO3 H2SO3 H+ (aq) + HSO3-(aq) pH = 2-3

sulfur trioxide and water (acidic)

sulfur triode reacts violently with water to produce sulphuric acid SO3(g) + H2O(l) ➡️ H2SO4(aq) ➡️ H+(aq) + HSO4-(aq) pH = 0-1

sodium and magnesium oxide and acids

react with an acids to give a salt and water only Na2O(s) + H2SO4(aq) ➡️ Na2SO4(aq) + H2O(l) MgO(s) + 2HCl (aq) ➡️ MgCl2(aq) +H2O

Aluminium oxide and acid

Al2O3(s) + 6HCl(aq) ➡️ 2AlCl3(aq) + 3H2O(l)

Aluminium oxide and alkali

Al2O3(s) + 2NaOH(aq) +3H2O ➡️ 2NaAl(OH)4(aq) NaOH hot and concentrated

silicon dioxide and base

reacts a weak acid with a strong base | SiO2(s) + 2NaOH(aq) ➡️ Na2SiO3(aq) + H2O(l)

iron production

iron is produced in blast furnaces calcium oxide reacts with the impurity silicon dioxide to produce a liquid slag. SiO2(s) + CaO(l) ➡️ CaSiO3(l)

phosphorous pentoxide

reaction of phosphorus pentoxide with an alkali to make phosphorus acid H3PO4(aq) + NaOH(aq) ➡️ NaH2PO4(aq) + H2O(l) NaH2PO4(aq) + NaOH(aq) ➡️ Na2HPO4(aq) + H2O(l) NaHPO4(aq) + NaOH(aq) ➡️ Na3PO4(aq) + H2O(l) 3NaOH(aq) + H3PO4(aq) ➡️ Na3PO4(aq) + 3H2O(l)

sulfur dioxyde and alkali

SO2(aq) + NaOH(aq) ➡️ NaHSO3(aq) NaHSO3(aq) + NaOH(aq) ➡️ Na2SO3(aq) + H2O(l)

calcium sulfite

sulfur dioxide react with base calcium oxide to form calcium sulfite. this is the first step of one of the methods of removing sulfur dioxide from flue gases in power stations CaO(s) + SO2(g) ➡️ CaSO3(s) calcium sulfite is further converted to calcium sulphate and sold as gypsum for plastering