1. Covalent Bonds Chapter 5 Section 3

2. Covalent Bonds Remember…covalent bonds form between two nonmetals The bonds form when electrons are shared between atoms, not transferred This happens because neither atom will take the electrons from the other, they attract them at the same time.

3. Single Bonds Ionic compounds only form single bonds when there are a pair of electrons between atoms This molecule has 5 single bonds

4. Single and Double/Triple Bonds Covalent (molecular) compounds can form single, double, and triple bonds Each bond has a pair of electrons between atoms

5. Single and Double/Triple Bonds

6. Covalent Bonds The electrons are sometimes shared equally when the same element bonds with itself (BrINClHOF). This is called a nonpolar bond. Sometimes they are shared unequally when one atom is slightly stronger than the other. This is called a polar bond.

7. Covalent Bonds

8. Properties of Molecular Compounds Some form crystal shapes, most do not Low melting points compared to ionic compounds Do not conduct electricity in solution (dissolved in water)

9. Writing Covalent Formulas Use the same procedure as for ionic formulas Example: C Br C 4+ Br 1- CBr 4 Example: N S N 5+ S 2- N 2 S 5

10. Naming Covalent Formulas Use the same procedure as for ionic formulas Add Latin prefix that matches the subscript for the element to each part of formula name 1= mono6= hexa 2= di7= hepta 3= tri8= octa 4= tetra9= nona 5= penta10= deca

11. Naming Covalent Formulas Example: CBr 4 Carbon tetrabromide N 2 S 5 Dinitrogenpentasulfide H 2 O Dihydrogen monoxide CO 2 Carbon dioxide