Chemical Bonding printable pdf download

Chemical Bonding

Unit #8

Regents Chemistry

1. Electronegativity is a measure of an element’s attraction for electrons.

2. Energy is released when a chemical bond forms. The more energy that is

released, the more stable the bond is.

3. The last digit of an element’s group number is equal to its number of valence

electrons.

4. Draw one dot for each valence electron when drawing an element’s or ion’s Lewis

diagram.

5. The kernel of an atom includes everything in an atom except the atom’s valence

electrons.

6. Metallic bonds can be thought of as a crystalline lattice of kernels surrounded by

a “sea” of mobile valence electrons.

7. Atoms are most stable when they have 8 valence electrons (an octet) and tend to

form ions to obtain such a configuration of electrons.

8. Covalent bonds form when two atoms share a pair of electrons.

9. Ionic bonds form when one atom transfers an electron to another atom when

forming a bond with it.

10. Nonpolar covalent bonds form when two atoms of the same element bond

together.

11. Polar covalent bonds form when the electronegativity difference between two

bonding atoms is between 0.4 and 1.7.

12. Ionic bonds form when the electronegativity difference between two bonding

atoms is greater than 1.7.

13. Substances containing mostly covalent bonds are called molecular substances.

14. Substances containing mostly ionic bonds are called ionic compounds.

15. Memorize this table.

Substance Type

Properties

Hard

Ionic

High melting and boiling points

Conduct electricity when molten or

when aqueous

Soft

Covalent (Molecular)

Low melting and boiling points

Do not conduct electricity (insulators)

16. Hydrogen bonds form when hydrogen bonds to the elements N, O, or F and

gives the compound unusually high melting and boiling points.

USE THE REFERENCE TABLES!!!

Chemical Bonding