bonds Flashcards
ionised meaning
an atom that has lost electrons
ionisation energy
how easy/hard it is to lose electrons from an atom
ionisation energy definition
the energy (enthalpy) required to remove an electron from an isolated (gaseous) atom or ion
electron affinity
the energy cost when an electron is removed to give an isolated (gaseous) atom and an electron
if a closed shell configuration can be obtained then it will happen
Na —–> Na+ + e-
[Ne]3s1 [Ne]
Ca ——-> Ca2+ + 2e-
[Ar]4s2 [Ar]
ionic bonding
a simple electrostatic interaction where “like” charges repel each other and “opposite” charges attract each other
electronegativity
a measure of the ability of an atom in a molecule to draw bonding electrons to itself
electronegativity trends
electronegativity increases left to right of the periodic table and decreases down a group - the most electronegative elements are found at the top right hand corner of the periodic table
difference in electronegativity is 0 or small
covalent bond
difference in electronegativity is large
ionic bond
electronegativity trick
a bond formed by two elements close together in the periodic table is covalent and if far apart are ionic
covalent bonding
when the difference in electronegativity is small, there is no net electron transfer, but electrons are shared between atoms
lewis symbols
these comprise of the element symbol, surrounded by dots or crosses representing valence electrons
stable configuration (noble gas)
would have 8 electrons surrounding the atom
representing an ionic bond
transferring an electron from the least electronegative element to the most electronegative element
