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Electronic structure of atoms
The periodic table
12 other sections not shown
adding agent alkali aluminium ammonia anions aqueous atoms basic become beryllium bismuth boron bromide carbon cations charge chloride combination complexes compounds concentrated configuration containing coordination copper corresponding covalent bond decreases difference dioxide dissolves electrical electrons elements energy enthalpy example excess exist fluorine formation give greater group 1A halides halogens heating higher hydrated hydrides hydrogen hydroxide important increase indicate involves iodide iodine ionic ionisation enthalpy iron(II known lattice ligands lithium lone pair magnesium manganese(II melting metal molecule negative nitrogen non-metal obtained occurs orbitals outer oxide oxidising oxygen pairs periodic phosphorus positive possess potassium potential powerful precipitate prepared presence produce properties reaction reactive readily reducing relatively represents respectively salts shell similar sodium solid soluble solution species stable standard structure sulphide sulphuric acid Table temperature tion transition valency zinc