IONIC BONDS

IONIC Interactions between ions Ions satisfy octet rule by loss or gain of e- to reach noble gas state

Na+ has + charge overall as Cl- has – charge overall This causes attraction of opposites Charges evenly distributed on each atom Complete transfer of electron (s) NON-DIRECTIONAL

Result is a crystal lattice Repeated pattern of + and – charges due to electrostatic attraction One of 4 universal forces, remember? (Gravity, electrostatic/weak nuclear force, electromagnetic and strong nuclear force)

LAB IONIC Compounds: High electrostatic charge Dull Hard Brittle High mp and bp temps NO electrical conductivity as solid or molten

Continued.. Most soluble in water Conductivity in solution DO NOT exist as single unit like molecule PACKED as solid in crystal each part of crystal separate entity but all held as one

Formula is NaCl BUT bonded by six neighbors Na 32 Cl 32 also accurate Write/record lowest ratio or simplest ratio of ions Called empirical formula (not really a molecule ratio same # varies)

LAB IONIC Compounds: High electrostatic charge Dull –no free e- Hard- strong electrostatic charge Brittle- shatter region of attraction-no bending-cleavage occurs- breaks on planes-repulsion between like ions High mp and bp temps- strong electrostatic charge NO electrical conductivity as solid or molten- no free electrons moving-charged particles locked

Continued.. Most soluble in water-polarity of water pulls at each charge region Conductivity in solution- ions free and moving DO NOT exist as single unit like molecule PACKED as solid in crystal each part of crystal separate entity but all held as one

Ionic Compound Nomenclature Each corner of symbol has reserved value mass charge Ca z=atomic # # of atoms

Using ion chart, name of compound is combined names of cation and anion Numbers of each are not stated Numbers of each ion implied in formula when + and – charges = 0