Properties Of Period 3 Elements And Their Oxides Flashcards
(12 cards)
Sodium reaction with water
2Na + 2H2O -> 2NaOH +H2,
Fizzing
Colourless solution
Vigorous
Very exothermic
Magnesium react with water
Mg + 2H2O -> Mg(OH)2 + H2
Slow reaction
Vigorous with steam
Bright white light
White solid formed
Sodium with oxygen
4Na + O2 -> 2Na2O
Yellow flame
White solid
Basic ionic oxide
O2- + H2O -> 2OH-
Magnesium with oxygen
2Mg + O2 -> MgO
White light and white solid
Sparingly soluble
Basic ionic oxide
Aluminium with oxygen
4Al + 3O2 -> 2Al2O3
White solid formed
Ionic amphoteric oxide
Why is aluminium oxide amphoteric
Al2O3 + 6H+ -> 2Al3+ + 3H2O, acid reaction
Al2O3 + 2OH- 3H2O -> 2Al(OH)4-, base reaction
Silicone dioxide
Si + O2 -> SiO2
Covalent acidic oxide
White powder
Insoluble
Phosphorus(v) oxide
P4 + 5O2 -> P4O10
Covalent acidic oxide
White solid
Bright white flame, whitebsmoke
Sulfur oxides
S + O2 -> SO2
2SO2 + O2 -> 2SO3 with vanadium catalyst
Blue flame with misty fumes
Yellow solid S dissolves to form red liquid and burns to form blue flame
Trends in melting point of p3 oxides
Metal oxides: as charge on Metal increases melting point increases, size of Metal ion decreases but charge increases so stronger attraction between oppositely charged ions, MgO> Al2O3 due to covalent character in aluminium
Silicon dioxide- highest meltingnpoint due to macromolecular structure, large amounts of energy required to break the many covalent bonds
Non metals- simple molecular structures, p4o10 has more electrons so stronger van der waals forces
Phosphoric acid
P4O10 + 6H2O -> 4H3PO4
Phosphorus atoms in the acid promote electrons into 3d sub level to form five covalent bonds
Sulfuric acid
SO2 + H2O -> H2SO3
Acid promotes one electron into 3d sub level to form four covalent bonds
Sulfur atom has one lone pair of electrons
SO3 + H2O -> H2SO4
Acid promotes two electrons into 3d sub level to form six covalent bonds
