3/9/2017
BELLRINGER:
BELLRINGER:
How do atoms form
chemical bonds?
2. Describe a metallic bond.
3. What are some properties
of metallic bonds?
4. STOTD
1.
What is an ion?
What are the two types of
ions?
STOTD
1.
2.
3.
CHEMICAL FORMULAS

Chemical Formula




IONIC COMPOUNDS AND
METALLIC BONDS


Unit 4: Chapters 6 and 7
Shows what elements are in a compound
If there is more than 1 atom of an element we add subscripts
to show how many
NaCl
CO2
MgCl2
Na3P
1 Na and 1 Cl
1 C and 2 O
1 Mg and 2 Cl
3 Na and 1 P
end
CHEMICAL FORMULAS

Some compounds have large groups of atoms


Polyatomic Ions


OH-, PO43-, NO3-, NH4+
In your Reference Tables!!!
If there is more than 1 Polyatomic Ion,


Write the group inside ( )
And put a subscripts outside to tell how many
end
ELECTRON CONFIGURATION


***Valence Electrons in the highest energy level***
Electron Dot Diagrams show the number of valence
electrons


Write the symbol
Place LARGE dots to represent each valence electron

1 dot on each side before pairing them up
end
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3/9/2017
ELECTRON CONFIGURATION
Draw diagrams for the following:


Sr

Si

Cl
ELECTRON CONFIGURATION
end
•
FORMATION OF A
Octet Rule
–
–

end
CHEMICAL BOND
Atoms are most stable with 8 valence electrons
•
ns2 np6 (Same as the Nobel Gases)
•
Transition metals are different
FORMATION OF A CHEMICAL BOND

The s- and p-block elements follow this rule



To get 8 valence, atoms will react and either:

Chemical Bond

Ionic
Covalent (covered in the next chapter)
 Metallic


Transfer Electrons:

The force holding two atoms together
3 types:
Lose Electrons to drop an energy level
Gain Electrons till they have 8
Share Electrons with other atoms, so everyone has 8
end
IONIC BONDS
**HONORS**IONIC BONDS



Ionic Bonds
Attraction between positive and negative ions
 Metal and Nonmetal (or Polyatomic Ion)
 Electrons are TRANSFERRED
 Ionic Compounds = Salts
**HONORS**ΔEN > 1.7

end
Identify which are Ionic.

1.
2.
3.
4.
5.
Using the EN chart determine the ΔEN
K2O
MgGe
SrO
AlP
FrF
end
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IONIC BONDS

BELLRINGER:
Ions


Atoms with a charge
Formed by losing/gaining electrons
1.
2.
Positively charged = Lost e- = Cation
 Negatively charged = Gain e- = Anion

3.
4.
What does an ionic bond consist of?
What is a polyatomic ion and where
can you find a list of them?
How many valence electrons do
atoms want to have?
STOTD
end
IONIC BONDS
•
•
•
•
The Periodic Table can predict the charges
The charge is known as the Oxidation Number
–
–
•
IONIC BONDING
There is a PT trend for Oxidation states!
Oxidation States follows the # of Valence Electrons
1 2
+1
1 +2
2
Arranged by Group
Cannot predict a Transition Metal’s charge
Ions will combine so the overall charge = 0
13 14 15 16 17 18
0
+3 +4 -3 -2 -1 8
3 4 5 6 7
end
•
Oxidation States follow the # of Valence Electrons
IONIC BONDS
1
2
13
14
15
16
17
18
# of
1
Valence:
2
3
4
5
6
7
8
+2
+3
±4
-3
-2
-1
0
Oxidation
State:
+1
–
•
Show the transfer of electrons with an Electron Dot
Diagram
sodium chloride (NaCl)
Na
+
Cl

 Draw Electron Dot Diagrams for:
KF
1.
2.
end
ve
end
IONIC BONDS
Group:
Group
Oxidation
3.
[ Na ]+[ Cl ]-
MgO
MgCl2
end
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PROPERTIES OF IONIC COMPOUNDS
PROPERTIES OF IONIC COMPOUNDS


Ionic compounds form a structure of a Crystal
Lattice

Negative ions alternate with positive ions
The strength of Ionic Bonds and Crystal
Structures determine the Physical Properties:



High Melting & Boiling Point
Brittle
Conduct Electricity when dissolved in water or
molten
Lattice Energy- the
energy needed to break
apart the crystal lattice
end
NAMING IONIC COMPOUNDS
•
Naming Ionic Compounds:
•
1.
2.
3.
3 steps
Name the Cation (the metal)
Name the Anion (the nonmetal)
Change the Ending on the anion to –ide
end
NAMING IONIC COMPOUNDS
•
More than 2 elements = POLYATOMIC ION!!!
•
Follow the same steps to name the compound
• Name the following:
1. BaS
–
LOOK AT YOUR REFERENCE TABLE!!!
•
Get the polyatomic’s name from the reference tables!
DON’T change the ending of a polyatomic ion
NaNO3
Sodium Nitrate
Name the following:
1. KOH
•
2. MgF2
2. NaC2H3O2
3. Ca3N2
3. (NH4)2O
4. Sr3(PO4)2
end
BELLRINGER:
Name the following Ionic Salts:
1. BeP
2. Na3N
3. Sr3(PO4)2
4. KOH
5.
–
STOTD
end
NAMING IONIC COMPOUNDS

Polyatomics are given on your Reference Table

But there are 5 you must know WITHOUT LOOKING!!!
Nitrate
Sulfate
Carbonate
Acetate
Ammonium
NO3SO42CO32C2H3O2- or CH3COONH4+
end
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WRITING IONIC FORMULAS
**HONOROS**
NAMING IONIC COMPOUNDS
•
Writing formulas:


1.
Polyatomic Ions
–
2.
If you remember the –ate form you also know 3 other
ions
3.
Per-
–
-ate  + 1 oxygen
-ate
-ite  -1 oxygen
hypo- -ite  -2 oxygens
The charge does not change!!!
Remember: The polyatomic ion IS A GROUP
–
1.
2.
3.
4.

When you cross charges, the subscript applies to the
WHOLE GROUP
Use ( )
• Write the formula for the
following:
Calcium Phosphate
Aluminum Acetate
Barium Chromate
Ammonium Sulfate
Do NOT put the “+” or “-”
end
WRITING IONIC FORMULAS
–

• Write the formulas for the following:
1. Beryllium Phosphide
2. Calcium Fluoride
3. Strontium Sulfide
4. Lithium chloride
5. Magnesium fluoride
6. Calcium oxide
7. Potassium nitride
8. Aluminum phosphide
end
•
3 steps:
Write the positive ion, with charge
Write the negative ion, with charge
Cross the charges to get subscripts
1.
2.
3.
4.
5. Lithium nitrate
6. Potassium carbonate
7. Magnesium phosphate
8. Ammonium chloride
5.
6.
7.
8.
Write the formula for the following:
Calcium Phosphate
Aluminum Acetate
Barium Chromate
Ammonium Sulfate
Lithium nitrate
Potassium carbonate
Magnesium phosphate
Ammonium chloride
end
BELLRINGER:
1.
2.
3.
What is the name of SrO?
Write the formula for
potassium sulfate.
STOTD
TRANSITION METALS
•
Transition Metals have 2 valence electrons
–
But they have Many Oxidation States
–
Exception:
–
–
Ag is +1, Zn is always +2
Sn & Pb have two oxidation states: +2 and +4
end
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TRANSITION METALS
•
•
TRANSITION METALS
Follow the same steps to write the formula
The metal's charge/oxidation state is the Roman
Numeral
1.
2.
3.
Vanadium (III) Sulfide
4.
Iron (III) chloride
Vanadium (II) oxide
Indium (III) carbonate
Tin (IV) nitride
Metal's Charge
V3+
V2S3
S2-
Write formulas for the following:
1. Osmium (V) Fluoride
2. Silver (I) Nitride
3. Technetium (VII) Phosphate
end
TRANSITION METALS
•
•
When naming you MUST put the charge as a Roman
Numeral!
To figure out the charge, uncross the subscripts!
Fe2O3
Fe3+ O2iron (III) oxide
•
4.
Name the following:
1. HgF2
2. Hf2S5
3. YP
5.
BELLRINGER:
NUMBER YOUR PAPER 1-5 AND SEE IF YOU CAN DETERMINE WHAT
THE FOLLOWING MAGNIFIED PHOTOS ARE.
2.
4.
2.
3.
end
1.
1.
Practice
Silver (I) oxide
Copper (I)
bromide
Copper (II)
bromide
Iron (II) oxide
Iron (III)
oxide
1.
2.
3.
4.
5.
CrCl2
CrCl3
HgI
MnO
Mo2S3
THE ANSWERS:
3.
5.
6
3/9/2017
THIS WEEK
REVIEW OF IONIC BONDS
Monday: Finish Unit 4: Ionic Bonds
Tuesday: Ionic vs Covalent Bonding Lab
 Wednesday: Review Day (Games and Index Card
Cheat Sheet)
 Thursday: Unit 4 Ionic Bonding Test
 Friday: Start Unit 5: Covalent Bonds
Types of Chemical Bonds
Electron Dot Diagrams, Octet Rule
 Oxidation States
 Properties of Ionic Bonds
 Names and Formulas
 Transition Metals




REVIEW!!
NAMING ACIDS


Types of Chemical Bonds
You need to memorize the names & formulas for these 4
acids:
Hydrochloric Acid
HCl
Nitric Acid
HNO3
Sulfuric Acid
H2SO4
Acetic Acid
HC2H3O2 or CH3COOH
end
NAMING ACIDS **HONORS**

Oxyacids


Hydrogen + Oxygen + other element (Polyatomic Ion)
Naming follows polyatomic names
per- -ate 
-ate 
-ite 
hypo- -ite 
1. H3PO4
2. HNO3
3. H2CO3
4. HClO3
5. HClO2
per- -ic acid
-ic acid
-ous acid
hypo- -ous acid
end

METALLIC BONDS
Metallic Bond


Between metals
Valence e- shared between ALL of the atoms

Metal Cation + a “sea of electrons”
end
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METALLIC BONDS


More Valence Electrons Shared = Stronger Bond
The “sea of electrons” determines the metals
properties:





High Melting and Boiling Points
Conductivity
Malleability and Ductility
Luster
Alloy


A Metal MIXED with another element.
Gives different properties when mixed in different amounts
BELLRINGER:
Name the following acids:
a) HBr
b) H2SO3
c) HNO3
2. Why do metallic bonds conduct
electricity so well?
3. STOTD
1.
end
BELLRINGER:
 ON
A SEPARATE SHEET OF PAPER
a moment to reflect on what you
have learned in this class so far. Write a
short paragraph for your reflection.
Consider these questions:
 Take




What do I like about this class?
What do I not like about this class?
How can my teacher help me learn?
What material (class topics) sticks out to me
the most?
 Why?
8