Take out your interactive notebook and set up an In, Out Through on your next two open pages.

In Activity Why do atoms have a neutral (no) charge?

Ionic Bonding Atoms don’t have an electric charge. They are neutral because the number of positive charges (protons) is always equal to the number of negative charges (electrons)

IONIC CHEMICAL BONDING Atoms connect with other atoms to form chemical bonds.

Types of Chemical Bonds There are four types of chemical bonds: 1.Ionic Bonds 2.Covalent Bonds 3.Metallic Bonds 4.Hydrogen Bonds We will study ionic and covalent bonding.

Ionic Bonding occurs when electron(s) are transferred from one atom to another. (Metals bonding with Nonmetals) LiF Be sure to draw!

Ionic Bonding When electrons are lost or gained the atom becomes an ion (an atom with a charge). Negatively charged ions are attracted to positively charged ions like the opposite poles of a magnet. Li+F- Cation Anion

Ionic Bonding with Sodium (Na) and Chlorine (Cl) results in NaCl or table salt

Ionic Bonding Here is what happens during the reaction between Sodium (Na) and Chlorine (Cl).Here When Sodium loses an electron it has an overall positive charge. This is called a Cation. When Chlorine gains an electron it has an overall negative charge and is called an Anion

Here is another example of Ionic Bonding between Potassium and Fluorine.

In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds. FK

FK

FK

FK

FK

FK

FK

FK + _

FK + _ The compound potassium fluoride consists of potassium (K + ) ions and fluoride (F - ) ions

FK + _ The ionic bond is the attraction between the positive K + ion and the negative F - ion

Out Activity Ionic Bonding Draw the Electron Dot Diagram for Potassium and Iodine. Show how these two will bond in an Ionic Bond. Be sure to use arrows and charge symbols.

Ionic Bonding Notes Complete. Stop at this slide.

Covalent Bonds

So what are covalent bonds? Continue using the Cornell notes you started with Ionic Bonding. Make a new title called “Covalent Bonding” in the through section.

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule).

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair.

In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair

Cl 2 Chlorine forms a covalent bond with itself

Cl How will two chlorine atoms react?

Cl Each chlorine atom wants to gain one electron to achieve an octet

Cl Neither atom will give up an electron – chlorine is highly electronegative. What’s the solution – what can they do to achieve an octet?

Cl

octet

Cl circle the electrons for each atom that completes their octets octet

Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

Cl circle the electrons for each atom that completes their octets This is the bonding pair

Cl circle the electrons for each atom that completes their octets It is a single bonding pair

Cl circle the electrons for each atom that completes their octets It is called a SINGLE BOND

Cl circle the electrons for each atom that completes their octets Single bonds are abbreviated with a dash

Cl circle the electrons for each atom that completes their octets This is the chlorine molecule, Cl 2

O2O2 Oxygen is also one of the diatomic molecules

How will two oxygen atoms bond? OO

OO Each atom has two unpaired electrons

OO

OO

OO

OO

OO

OO

Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

OO

OO

OO

OO

O O Both electron pairs are shared.

6 valence electrons plus 2 shared electrons = full octet O O

6 valence electrons plus 2 shared electrons = full octet O O

two bonding pairs, O O making a double bond

O O = For convenience, the double bond can be shown as two dashes. O O

O O = This is the oxygen molecule, O 2 this is so cool! !