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Ionization energy, luttice energy, force of attraction between posetively and negatively charged ions are some of the factors that affect the formation of ionic compounds.
Ionic strength doesn't affect pH
Charge an ion has, temperature, polarity of solutes and solvents and pressure.
No, an ionic bond is an intramolecular force, as it holds atoms within a molecule together.
the force of attraction the force of attraction
Ionization energy, luttice energy, force of attraction between posetively and negatively charged ions are some of the factors that affect the formation of ionic compounds.
Ionic strength doesn't affect pH
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy
Charge an ion has, temperature, polarity of solutes and solvents and pressure.
By simply afecting the bonds ( hbonds . ionic bonds and hydrophobic interactions )
5mM
In ionic bonding electrons are transferred from one element to another and are localised and not shared. the force of attraction in ionic bonding is electrostatic. In covalent bonding electrons are shared, or in some cases delocalised as in benzene. The source of the strength of a covalent bond is a quantum effect.
No, an ionic bond is an intramolecular force, as it holds atoms within a molecule together.
the force of attraction the force of attraction
an ionic compound
the word strength is too broad to pinpoint the complete answer but i persume magnesium oxide's strength refers to the physical state of the ionic bond. the word strength is too broad to pinpoint the complete answer but i persume magnesium oxide's strength refers to the physical state of the ionic bond.
Ionic bonds are formed due to electrostatic force of attraction and Ionic compounds exist as the crystal lattice, (combination of billions of ions), so ionic bond is very strong bond and requires high amount of heat for decomposition.But in water ionic bonds are weak and easily decompose into ions.Example.NaCl ------------ 801 0C----------> Na1+ + Cl1-NaCl--- water + room temp.---->Na1+ + Cl1-