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Forming Chemical Bonds
• Objectives– Define chemical bond– Relate chemical bond formation to
electron configuration– Describe the formation of positive and
negative ions
Electron Dot structure
• Recall them…– Do some on board
• Recall “ion”
• Write electron configurations for potassium and argon– What’s the difference?– Why is argon so stable?– How could potassium achieve stability?
Ions
• How do atoms become ions?
• Positive ions– They always want to achieve the most
stable state…8 valence electrons– Look at Ne and Na’s configurations– Ionization energy is key…
Negative Ions
• Look at argon and chlorine– Anions gain electrons in bonding to
achieve noble gas configuration
Formation of Ionic Bond
• Objectives– Describe the formation of ionic bonds– Account for many of the physical
properties of an ionic compound– Discuss the energy involved in the
formation of an ionic bond
Ionic Bonding
• Atoms transfer electrons from one to another forming a bond between two ions.
• The electrostatic force that holds oppositely charged particles together in an ionic compound is referred to as an ionic bond
• Ionic bonds are extremely strong bonds
Ionic Bonds
• Binary compounds– Contains two different elements– Ex: MgO
• Is CaSO4 a binary compound?
• Polyatomic ion: an ion that contains more than one element– SO4-
– OH-
Properties of Ionic Compounds
• Ions packed into regular repeating patterns called crystals (crystal lattice)
Crystals
• High-energy bonds
• Melting point, boiling point and hardness all depend on strength of bond– Stronger = higher boiling and melting pts.
Properties
• High melting and boiling points - Ionic bonds are very strong - a lot of energy is needed to break them. ...
• Conductive when aqueous - Ions are charged particles, but ionic compounds can only conduct electricity if their ions are free to move.
Electrolyte
• An ionic compound whose aqueous solution conducts an electric current– NaCl, MgCl2, KF
Energy and Ionic Bond
• Lattice energy:– The energy required to separate one
mole of the ions of an ionic compound– Higher energy bonds = higher lattice
energy