Ionic and Covalent bonding

1. Ionic and Covalent bonding David A. Katz Pima Community College Tucson, AZ

3. Ionic Bonding Between a metal with low ionization energy ( little energy required to remove an electron) and a non-metal with high electronegativity and electron affinity ( wants to grab an electron towards it)

7. Formation of NaCl

8. • •• 2+ 2- •• Ba O Ba O •• • • • •• •• •• •• Cl •• • •• • 2+ - •• Mg Mg 2 Cl •• • •• •• •• Cl •• • •• Lewis Structures for Ionic Compounds BaO MgCl2

10. Properties of Ionic Compounds • Held together by strong electrostatic forces • Opposite charges attract • High melting points and boiling points • Regular structures – giant ionic lattices • When melted or dissolved ionic compounds conduct electricity

11. Dissolving in Water

12. conductivity

13. Covalent Bond • Between two elements with high ionization energy ( do not give up electrons easily) and high electronegativity ( try to grab the electron to each of them) • Here neither atom is willing to give up its electron • Instead the nuclei share the electrons between them

16. Lewis Structures • Lewis structures are representations of molecules showing all electrons, bonding and non-bonding Example : Li2 O

17. Lewis structures F2 C2H6

18. Multiple Covalent bonds • More than one pair of electrons can be shared between the same atoms O2 N2

20. Properties of Covalent Molecules • Contain non-metals • Weak bonds • Valence electrons are shared between atoms • Polar molecules dissolve in polar solvents • Volatile • Low melting and boiling points • Insoluble in water • Non polar compounds do not conduct electricity; polar compounds can conduct small amounts of electricity