Types of Compounds

Ionic Compounds

Where are we on the Matter Map?

Matter

Pure Substances

Mixtures

Atoms

Compounds

Metallic

Covalent/

Molecular

Ionic

Formula

Units

Molecules

Elements

What is an Ionic Compound?

• Definition: Compounds made from the transfer of an electron from a metal to a nonmetal.

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1. What ionic cpds are made of:

• Formed between a metal and a non-metal

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• Metal becomes a cation (+) b/c it loses an e^-

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• Non-metal becomes an anion (-) b/c it gains an e^-

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2. Charges on ionic cpds

• Hand out new periodic table

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• Overall charge must be zero on elements in their ground state on periodic table.
• Possible charges can be found above the symbol on the periodic table

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• Notice that some only have one possible charge and some have many possible charges

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3. Elements form certain types of ions

• Label on new periodic table:
• Metals lose an e^- to become cations
• Group IA forms +1 cations
• Group IIA forms +2 cations
• Group IIIA forms +3 cations

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• Non-metals gain an e^- to become anions
• Group 5A forms 3^- anions
• Group 6A forms 2^- anions
• Group 7A forms 1^- anions

4. Properties of ionic cpds

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a.) Called “salts” (remember the flame test lab? Those were salts!)

b.) Most are crystalline solids at room temp.

-Ions are arranged in a 3-D repeating pattern

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d.) Salts conduct electricity dissolved in water

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4. Properties of ionic cpds continued...

e.) High melting point (Colligative Property)→ this means that the ionic bond is very strong (What is a practical use for this property?)

In order to properly name ionic compounds...

...we need to know how ALL of the elements react to each other. (Not just Groups 1-8)

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This is called an oxidation state:

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• Often called the oxidation number, is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound.

Oxidation State cont’d...

Some elements have a large number of different ions it can make, like Vanadium.

-Look up Vanadium, how many does it have?

Other elements just have one like these:

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Let’s color it….again!

So, how do you give your periodic table structure?

• Red
• Orange
• Yellow
• Green
• Blue
• Violet

• Pick 3 colored pencils
• Two need to be close to each other in the list
• The third one needs to be as far away from the others as possible
• Example 1 – red, orange, and violet
• Example 2 – orange, blue, and violet

How do you give your periodic table structure?

Let’s color it….again!

• Color that is the farthest apart is for ALL the non-metals.

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• One color of the close two is for metals that only have ONE possible charge (only one digit above the symbol.

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• The other close color is for metals that have more than one possible charge (more than one digit above the symbol.

How are ionic compounds formed?

• It has to do with:

Valence electrons!!!!!

Which are the e^- in the highest energy level or outer shell

What else do valence electron give an element? (Hint: Alkali Metals do what?)

** The valence electrons determine the chemical properties of the element. **

Let’s Practice Electron Dot Structures

• These show valence electrons as dots
• The nucleus and inner electrons are represented by the element symbol

H

Mg

Sr

C

O

Cl

B

Kr

Remember the Octet Rule!!

• Atoms in compounds (ionic or covalent) tend to have 8 electrons in their valence shell.
• And….This is also called the Noble Gas configuration.

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• However, Hydrogen and Helium follow the “duet” rule (why is this so?)

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Octet Rule cont’d

• In order to achieve the octet rule:
• Metals tend to lose electrons
• Non-metals tend to gain electrons

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Chemical Formulas and Bonding

Na → Na¹⁺ + e^-

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Mg → Mg ²⁺ + 2e^-

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Cl + e^- → Cl ^-

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lO + 2e^- → O ^2-

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Reactant → Product

Below are some examples of atoms becoming ions using the Reactant → Product format:

Opposites attract in an Ionic Bond

• The anions and cations have opposite charges, so they attract each other.

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• Now lets write the Reactant → Product format for table salt:

• Na + Cl → Na⁺ Cl ^-

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• Reactants = Sodium and Chlorine
• Product = NaCl (Sodium Chloride)

How are ionic compounds formed again?

• The ions are formed by either gaining or losing electrons from the outer shell.

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• The ionic bond is formed by the transfer of these outer shell electrons.

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Naming Ionic Compounds

These rules are used for naming binary ionic compounds where there is

ONLY ONE POSSIBLE CHOICE OF CHARGE

above the symbol on the periodic table

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What color did you color these on your periodic table?

Naming Ionic Compounds I

• Determine that the cpd is a metal and non-metal
• Say the name of the 1^st element (the metal, cation)
• Change the 2^nd element’s name (the non-metal, anion) so that it ends in –ide

examples:

• NaCl
• MgO
• Al₂S₃

sodium chloride

magnesium oxide

aluminum sulfide

Binary Ionic Compound Naming I

• NaBr
• SrO
• ScF₃
• MgCl₂
• La₂O₃
• CsSe₂
• ZnI₂
• Li₃P
• HfO₂
• Ba₃N₂

• Sodium bromide
• Strontium oxide
• Scandium fluoride
• Magnesium chloride
• Lanthanum oxide
• Cesium selenide
• Zinc iodide
• Lithium phosphide
• Halfnium oxide
• Barium nitride

Binary Ionic Compound Naming I

Chemical Formula and Ionic Bonding Worksheet

Naming Ionic Compounds II

<ROMAN NUMERALS or Multi Charges>

• After you know the compound is ionic (a metal + non-metal),
• And you know that the metal has a choice of charge (what color is that for you?)…
• You must look at the total charge on the non-metal
• What is the charge on EACH non-metal?
• Multiply by how many non-metal atoms there are

-Check the next slide for an example of this step:

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Example: CuBr₂

This is an ionic compound (metal + non-metal)

Copper has a choice of charge.

• We need to look at the charge on bromine.
• From the periodic table, Br has a charge of -1
• But there are TWO bromine atoms
• So the total charge on bromine is…
• -2 (because the -1 charge on Br x 2 Br atoms is -2)

CuBr₂

4. Remember that the total charge must be 0, so you can know the total charge on the metal.

• So, take the -2 charge we know & make it positive and give it to Cu. Then divide by # of Metal atoms.

-This gives you the Roman Numeral

• Using what we know already, let’s try to name this ionic compound:

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CuBr₂

-1

-2

+2

+2

b/c -1 x 2 = -2

b/c total charge must = 0

b/c +2 ÷ 1 = +2

So the name of this compound is Copper (II) bromide.

Roman Numerals

• I

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• II

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• III

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• IV

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• V

• VI

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• VII

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• VIII

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• IX

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• X

Binary Ionic Compound Naming II – Roman Numerals Practice

Write in notes and check answers on next slide

• MnO₂
• CuCl₂
• W₃As₅
• OsF₆
• CrN
• Au₂S₃
• Pt₃P₄
• Fe₂O₃
• NiBr₃
• CoP

Binary Ionic Compound Naming II – Roman Numerals

Check Answers Here

• MnO₂
• CuCl₂
• W₃As₅
• OsF₆
• CrN
• Au₂S₃
• Pt₃P₄
• Fe₂O₃
• NiBr₃
• CoP

• Manganese (IV) oxide
• Copper (II) chloride
• Tungsten (V) arsenide
• Osmium (VI) fluoride
• Chromium (III) nitride
• Gold (III) sulfide
• Platinum (IV) phosphide
• Iron (III) oxide
• Nickel (III) bromide
• Cobale (III) phosphide

Binary Ionic Compound Naming III – Mixed Practice (MUST HAND IN!!!)

Write on Separate Sheet and please show work!!

• VCl₅
• CaO
• Ga₂O₃
• Mo₃N₅
• Cs₂S
• BeF₂
• CoN
• Zr₃P₄
• OsO₃
• ScP

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