+

Ionic CompoundsWrite down the stuff in red

+Atoms vs. Molecules vs. CompoundsATOMS are the smallest particles of any

element that is still that element Example: an atom of hydrogen (H) or an atom of

calcium (Ca)

MOLECULES are groups of 2 or more atoms

Example: H2 or O2 or H20 or HCl

COMPOUNDS are groups of 2 or more atoms of different elements

Example: H20, HF, NH3 or CH4

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+Forming compounds

When atoms move close together, their valence electrons interact

A bond will form if the electrons become more stable (become an octet)

Electrons become more stable by either:

Losing electrons to other atoms and becoming an CATION

Gaining electrons from other atoms and becoming an ANIONARING electrons

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+Types of bonding

There are two main types of chemical bonding:

IONIC BONDING When atoms gain or lose (transfer) electrons to

other atoms

Example: Na + Cl = NaCl

COVALENT BONDING (We’ll get to this

later) When atoms share electrons with other atoms

Example: H2 + O = H20

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+Ionic bonding

An ionic compound contains a POSITIVE ion (usually a METAL) and a NEGATIVE ion (usually a non-metal)

EX: Na + + Cl- = NaCl

(positive metal) (negative non-metal) ionic compound

In ionic bonding one or more electrons TRANSFERS from each atom of METAL to each atom of NON-METAL

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+Example of an Ionic Compound

• Sodium (Na) has 1 valence electron• Chlorine (Cl) has 7 valence electron• Sodium loses its 1 valence electron and gives it to Chlorine• Sodium has become less negative (more positive) and now

has a +1 charge• Chlorine has become more negative and now have a -1

charge

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+NaCl Ionic Bonding

A

C

B

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+Activity Break!

Girls on the left side of the classroom (near my desk) You are metals

Boys on the right side of the classroom (by the maps) You are non-metals

Wait further instructions!

Mini marshmallows are your electrons. Metals need to find non-metals to give their electrons to in such a way that you both have full valence shells (0 marshmallows or 8)

+Naming Ionic Compounds

Ionic compound names have 2 parts to it, one for each ion in it:

The positive metal ion is always written FIRST

The negative non-metal ion is always written SECOND

The non-metal’s name always ends with the suffix “ide” metal non-metal

+ ion - ion

Example: Potassium Iodide (positive metal) (negative non-metal, ending

with –ide)

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+Names of Ionic Non-Metals

Element Ionic Name Symbol

Flourine Flouride F-

Chlorine Chloride Cl-

Bromine Bromide Br-

Iodine Iodide I-

Oxygen Oxide O2-

Sulfur Sulfide S2-

Selenium Selenide Se2-

Nitrogen Nitride N3-

Phosphorus Phosphide P3-

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+Practice Naming

Write down the proper name of the ionic compound formed from the following ions:

Magnesium + Phosphorus =

Calcium + Bromine =

Aluminum + Oxygen =

Lithium + Nitrogen =

Zinc + Sulfur =

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Magnesium Phosphide

Calcium Bromide

Aluminum Oxide

Lithium Nitride

Zinc Sulfide

+Naming Ionic Compounds from Formulas If you just have the formula, how do you name it?

Example: CaI2

1. Identify and name the metal ion in the compound Ca2+ is the metal. Its name is calcium.

Calcium

2. Identify and name the non-metal ion in the compound I- is the non-metal. Its name is Iodine.

Iodine

3.Change the name of the non-metal so it ends with “ide”Iodide

n Write the two together to name the ionic compoundCalcium Iodide

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+Practice Naming from Formulas

Na3P

1.Name the positive metal ion

2.Name the negative non-metal ion

3.Change the suffix to “ide”

4.Write out the name

5.Bam!

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Sodium

Phosphorus

Phosphide

Sodium Phosphide

+Writing Formulas for Ionic CompoundsExample: Aluminum Flouride

1.Identify the POSITIVE ion and the NEGATIVE ion and list their charges

Aluminum: Al3+

Flouride: F-

2.Figure out how many of each ion you need to balance out the charges

Al3+ : = + 3 F- : -1 -1 -1 = - 3

3.Notice how many of each ion you needed to balance the charges

1 Al3+ ion 3 F- ions

nWrite out the formula by listing the ions. Indicate how many of each ion are there by writing the number in a subscript beside it

AlF3

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+Practice Writing Ionic Formulas

Example: magnesium nitride

1.Identify each ion and list its charge

2.Figure out how many of each ion you need to balance the charges

3.Note how many of each ion you needed

4.Write out the formula and indicate how many of each ions are there with a subscripted number

5.Bam!

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Mg 2+ N3-

Mg 2+ = +2 +2 +2 = +6

N3- = -3 -3 =-6

3 Mg 2+ Ions

2 N3- Ions

Mg 3

N2