theoretical vs experimental lattic enthalpy Flashcards
what does a large lattice enthalpy suggest
stonger ionic bonds so more enrgy needs to be taken in to overcome the electrostatic forces of attraction
what factors affect the lattice enthalpy
the charge on the ions and the size of the ions
when does enthalpy increase
when the ion gets smaller and the charge increases as when there is a smaller radius the forces of attraction between two ions are stronger
what is the therotical lattice enthalpy
the lattice enthalpy calculated using the perfect ionic model
what is the experimental lattice enthalpy
the enthalpy calculated using the born harber cycle
why do we say that electrons are electron clouds
electrons are not discrete and move around forming an electron density
why is an electron cloud distorted in hcl
the difference in electrnegativity causes the distortion as chlorine more electronegative so pulls the electron towards itself
how does covelent character increase
when the positive ion is small, when the positive ion has multiple charges, when the negative ion is large, when the negative ion contains multiple charges
why does covalent increase with smaller cation
when the cation is smaller it causes a greater extent of polarisation on the anion as greater attraction between the positive nucleas and the electron density
why does covalent character increase when the anion is larger
electrons are held less tightly by the nucleas so the cation can pull the electron density towards itself resulting in polarisation
what is the perfect ionic model
ions are perfect speres with only ionic bonding present
what if the theroertical and experimental lattice enthalpies are the same
100% ionic
why is born harber values usually larger
as the experimental lattice enthalpies take into account the covalent character and the covalent bonds in addition to the ionic bonds so it is stronger and more energy is required
