ionic bonding part i
DESCRIPTION
Ionic Bonding Part I. An Elemental Love Story. Demo. Burning string demo Clean string vs Sugar soaked string vs Salt soaked string Any difference?. Research Mission. For this week, you will read articles about: Iodine deficiency disorder Pros and cons of fluoride - PowerPoint PPT PresentationTRANSCRIPT
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Ionic Bonding Part I
An Elemental Love Story
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Demo
Burning string demo Clean string vs Sugar soaked string vs Salt
soaked string Any difference?
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Research Mission
For this week, you will read articles about: Iodine deficiency disorder Pros and cons of fluoride The importance of potassium The dangers of chromium
After gathering information, your group will present what you learned and how it relates to ions and ionic bonding.
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Before we dive in
What is a chemical bond? What are three main different types of
bonds? Why do elements form ions? What is a cation? What is an anion?
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Q: How do elements combine to form compounds?
A: Compounds have different forces that hold groups of atoms together and make them function as a unit called bonds.
Bonds
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Bonds
Bonds come in three main varieties:
1. Metallic bonds – when metal cations bond they share a sea of delocalized electrons.
2. Ionic bonds – transfer of electrons between metals and non metals
3. Covalent bonds – sharing of electrons between two nonmetals
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Metallic Bonding
Strong forces of attraction are responsible for the high melting point of most metals.
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Metallic Bonding The chemical bonding that
results from the attraction between metal cations and the surrounding sea of electrons
Vacant p and d orbitals in metal's outer energy levels overlap, and allow outer electrons to move freely throughout the metal
Valence electrons do not belong to any one atom
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Properties of Metals
Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster
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Metal Alloys Alloys: some metal atoms replaced by
others of similar size.
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Ionic bonding
Ionic compounds bond in repeating 3-dimensional patterns with alternating positive and negative ionscalled crystal lattice.
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Ionic Crystal Lattice Shapes
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Ionic bondingAll salts are ionic compounds and form crystals.
NaCl forms the simplest cubic structure
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Properties of Ionic Compounds
Structure: Crystalline solids
Melting point:
Generally high
Boiling Point:
Generally high
Electrical Conductivity:
Excellent conductors, molten and aqueous
Solubility in water:
Generally soluble
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Properties of Ionic Compounds
Lab! We will be examining the properties of ionic
compounds next double with a lab. In the meantime, we will move onto how and
why ions bond.
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Great BBC video on ions
http://www.bbc.co.uk/schools/gcsebitesize/science/add_aqa_pre_2011/atomic/ionicact.shtml
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Know our ions inside and out
In order to be successful with ionic bonding, you need to know what ion each element in the s and p block will form.
Practice on the Ion worksheet grid in the packet
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The Octet Rule – Ionic Compounds
Ionic compounds form so that each atom, by gaining or losing electrons, has an octet of electrons in its highest occupied energy level.
Ionic bonds form between metals and nonmetals!
• Metals lose electrons to form positively-charged cations
• Nonmetals gains electrons to form negatively-charged anions
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Ionic Bonding:Sodium Chloride Example
Sodium has 1 valence electron
Cl: 1s22s22p63s23p5
Na: 1s22s22p63s1
Chlorine has 7 valence electrons
An electron transferred gives each an octet
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Ionic Bonding
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Cl- 1s22s22p63s23p6
Na+ 1s22s22p6
This transfer forms ions, each with an octet:
Ionic Bonding:Sodium Chloride Example
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Cl- Na+
The resulting ions come together due to electrostatic attraction (opposites attract):
The net charge on the compound must equal zero
Ionic Bonding:Sodium Chloride Example
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Writing Ionic Compounds with Electron Dot Diagrams
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Drawing Ionic compounds
How would these elements bond?
Li F K Br
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Drawing Ionic Compounds
Not all relationships are 1:1 with sharing of valence electrons.
Sometimes you need more of one element than the other to make a neutral compound
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Drawing Ionic Compounds
How would these elements bond?
Mg Br
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Draw the ionic compounds
How about
K S
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Criss Cross method!
Example: Aluminum sulfide
1. Write the formulas for cation and anion, including CHARGES!
2. Do charges balance?3. If not, use criss-cross
method to balance subscripts.
Al3+ S2-
Not balanced!
2 3
Now balanced.
= Al2S3
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Criss Cross Method!Example: Beryllium chloride
1. Write the formulas for cation and anion, including CHARGES!
Be2+Cl-
2. Do charges balance?
3. Balance charges, if necessary, using subscripts. Use criss-cross method to balance subscripts.
Not balanced!
2Now balanced.
= BeCl2
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Mg Cl
Na O
Magnesium chloride: Magnesium loses two electrons and each chlorine gains one electron
Sodium oxide: Each sodium loses one electron and the oxygen gains two electrons
Al SAluminum sulfide: Each aluminum loses two electrons (six total) and each sulfur gains two electrons (six total)
Try the criss cross method
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Naming Ionic Compounds
You may have noticed that the name of the nonmetal in the previous compounds sounded different (chloride instead of chlorine, oxygen inside of oxide) Can you think of what might be a naming rule for
ionic compounds? What’s the order we use? Do any of the names change?
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Naming Ionic Compounds
Name the cation first and then the anion
Cations – use the name of the element
Anions – use the name of the nonmetal but change the ending to an –ide
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Metal Monatomic Cations
Ion name
Lithium Li+ LithiumSodium Na+ SodiumPotassium K+ PotassiumMagnesium Mg2+ Magnesiu
mCalcium Ca2+ CalciumBarium Ba2+ BariumAluminum Al3+ Aluminum
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Nonmetal Monatomic Anions
Ion Name
Fluorine F- Fluoride
Chlorine Cl- Chloride
Bromine Br- Bromide
Iodine I- Iodide
Oxygen O2- Oxide
Sulfur S2- Sulfide
Nitrogen N3- Nitride
Phosphorus P3- Phosphide
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Practice!
Let’s try writing our predicting ion charges and and writing ionic compounds using the criss cross method
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Ionic Bonding Wrinkles
Polyatomic molecules and
METALS WITH MULTIPLE IONS
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Polyatomic ions
Many ionic compounds contain polyatomic ions which are ions made up of more than one atom.
Polyatomic ions are atoms that are covalently bonded together and act as an individual ion.
Because it exists as a unit, DO NOT change the subscripts within the ion.
In Ionic Compounds, you put ( ) around them
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Polyatomic ions
You will not be asked to memorize the polyatomic ions, but…
You do need to be able to recognize them And use a resource to determine its ionic
charge So that you can balance and write ionic
compounds! http://www.youtube.com/watch?v=MJZeZvDx
cx8
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Polyatomic Ion Names
CO3 2- carbonate OH – hydroxide SO4 2- sulfate
PO4 3- phosphate
NO3– nitrate
ClO3– chlorate
NH4 + ammonium
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Writing Ionic Compound with polyatomics
Example: Zinc hydroxide
1. Write the formulas for cation and anion, including CHARGES!
Zn2+ OH-
2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
( )2
Now balanced.
= Zn(OH)2
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Example: Barium nitrate
1. Write the formulas for cation and anion, including CHARGES!
Ba2+ NO3-2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
( ) 2Now balanced.
= Ba(NO3)2
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Writing Ionic Compound with polyatomic molecules
Example: Ammonium sulfate (note the 2 word name)
NH4+ SO4
2-
2. Do charges balance? Not balanced!
( )2
Now balanced.
= (NH4)2SO43. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
1. Write the formulas for cation and anion, including CHARGES!
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METALS WITH MULTIPLE IONS
Up until now, we’ve only been working with ions from the s and p block and ignoring d-block
This is because d-block metals as well as other metals can often form more than one type of ion
Again, you will not have to memorize these ions, but be able to use a resource to write ionic compounds with them.
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METALS WITH MULTIPLE IONS
For those metals it is important to represent which ion it is with a roman numeral.
If it is +1 you put a (I) after the name of the metal If it is +2 it is a (II) after the name of the metal If it is a +3, you put a (III) after the name of the
metal You include this roman numeral in the name
ONLY for metals that form multiple ions!
For example: NiBr2 would be Nickel (II) Bromide
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Roman numeral review!
VI II III
IV VII II
I III V
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Practice!
Now, let’s practice writing ionic compounds with either polyatomic ions or METALS WITH MULTIPLE IONS