ionic compounds, lattice energy, and ionization energy Flashcards
ionic bonding
mental and a non metal, electrons transfer from metal to non-metal, + and - charges form. No chemical bond
Ionic compounds
metal and nonmetal/polyatomic, high melting + boiling point, conductive when dissolved in water because they break into ions
Lattice energy
measures the strength of an ionic bond
how to find higher lattice energy?
add the absolute values of the charge of each ion and the greater one wins AND/OR lower ionic radius=larger lattice energy
electronegativity (e-)
the ability of an atom to attract shared electrons
which way on the periodic table does electronegativity increase and decrease
increases right, decreases down
ionic electronegativity
a metal gives an electron to a non metal
covalent electronegativity
2 non metals share an electron
non-polar
electrons are shared equally (symmetrical)
metallic electronegativity
electrons are not associated with a single atom, instead with every atom in a bond (delocalized) (2 metals)
bond polarity
difference between electronegativity (higher e- has negative partial charge, lower has positive) (larger difference is more polar)
which way does the e- arrow point
towards the more electromagnetic atom
if the peak of an intramolecular force graph is <0, is it stable or unstable
stable. when above zero repulsion is strong
how to find the bond energy on a intramolecular force graph?
lowest point on the y axis
what can you determine from the x axis on an intramolecular force graph?
distance between atoms (bond length)
