unit learning goal attraction and repulsion between electric charges at the atomic scale explain...
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Bonding and Nomentclature UNit
Unit Learning Goal Attraction and repulsion between ele
ctric charges at the atomic scale explain the structure, properties, and transformations of matter, as well as the classification of the matter.
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Bonding-1
Valence Electrons and the Octet Rule
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Valence Electrons and Bonding
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Valence Electrons and Bonding
Valence Electrons What are they?▪ Outer Shell Electrons
These electrons make all bonds happen.
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Octet Rule
All atoms “want” to obtain the electron configuration of a noble gas
Usually this is 8 outer shell electrons
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Lewis Dot
Dots to indicate the number of electrons in the outer shell
Na Ca O
N F Si
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12 3 4 5 6 7
8NUMBER OF VALENCE ELECTRONS
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Octet Rule: How Achieved
Achieve Noble Gas Give & Take of
Electrons▪ =Ionic Bond
Sharing Electrons▪ =Covalent Bond
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Bonding-2Ionic Bonding
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Ionic Bonds
Ionic bonds occur because of a Transfer of Electrons
These two atoms are NOT happy: How can we help them out?
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The atom with the extra electrons gives them to the one who “wants” electrons
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+2 -2
Note that after the transfer of electrons the atoms acquire a charge: +2 and -2
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oxidation number
The oxidation number of an element indicates the number of electrons lost, gained, or shared as a result of chemical bonding. It is the charge of atoms after they have their complete octet.
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What Causes the Ions to be attracted?
Ions are always attracted to each other due to the attraction between opposite electrical charges.
Positive and negative charged ions attract each other till the total charge is ZERO.
1 Na+ + 1 Cl- = NaCl no charge (balanced)
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Ionic Bonds
Definitions Salt
Ionic compounds are often referred to as salts. Crystal Lattice▪ A repetitive arrangement of atoms in an ionic
compound
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A large Salt Crystal
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Crystal Lattice
One Na for every one Cl
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Crystal Lattice Explained
Formula is a ratio: NaCl does not mean one Na connected to one Cl
It means Na1,000,000Cl1,000,000
So it looks like…
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Ionic Bonds
Property Reason
High melting point Due to strong bonds
Do not conduct electricity when solid
Electrons can’t move
Solids at room temp. Strong bonds
Good conductors when dissolved or liquid
Ions are free to move
Brittle and hard Strong bonds
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Compound with Polyatomic ions Polyatomic Ions are ions that have more
than one atom. Often these ions can include nonmetal atoms.
Polyatomic ions are groups of atoms that act together as one unit
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Transition Metals
Transition Metals are always cations just like all metals.
Transition Metals often have more than one possible charge. It is necessary to check for possible charges when we make our ionic compounds.
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Common Transition elements with more than one ion formation
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Ionic Bonding Lewis Dot Example
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Polyatomic Ions
We must consider these ions as groups that always travel together.
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Iron Oxides
Iron II Oxide ` Iron III Oxide
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Nomenclature
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THE NAME OF COMPOUNDS ARE VERY IMPORTANT!
Because they tell you what is in that compound!
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How do I know the ion formed by various elements?
The periodic table group numbers signify the number of valence electrons members of that group each have.
The valence electron number will indicate whether or not that element/group will lose or gain electrons, and how many Groups 1-3 and the transition elements lose
electrons to become positive ions Groups 5-7 gain electrons to become negative ions Group 4 and 8 do not readily form ions
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The periodic table as a useful tool
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Naming Basics: Ionic Compounds
Ionic compounds are formed between a metal and a nonmetal Metals: groups 1, 2, 3, & the transition
metals (short rows) Nonmetals: primarily groups 5, 6, & 7
To name them: Cation + (Anion + ide) Cation: positive ion Anion: negative ion Na + Cl = Sodium Chloride
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Determining the molecular formula of an ionic compound
Compounds are by definition neutral. When combining ions to form an ionic compound, the overall charge of the compound must equal zero
Subscripts are used to indicate the number of each element needed in order to have a neutral compound
For example: Na + Cl = NaCl (+1, -1 equals zero) Mg + Br = MgBr2 (+2, -1, -1 equals zero)
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Compounds with Polyatomic ions
When naming compounds with polyatomic ions, use the name of the polyatomic ion with no –ide suffix
For example: K2S = Potassium sulfide while K3PO4 = Potassium phosphate
In the example above, the rules for determining subscripts remains the same: the goal is for the compound to be neutral (no electrical charge)
K = +1 charge, PO4 = -3 charge and so I will need three K+ ions to bond with one PO4 polyatomic ion in order to reach an electrical charge of zero (neutral
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Compounds with elements that form more than one type of Ion (multiple charges)
When naming a compound containing an element that can form more than one type of ion, a Roman numeral is used to indicate the charge of that ion in that particular compound
Copper (II) Oxide: Copper has a +2 charge, and therefore the formula will be CuO
Copper (I) Oxide: Copper has a +1 charge and therefore the formula will be Cu2O
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Common Transition elements with more than one ion formation
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Naming compounds containing only nonmetals
When nonmetals combine, the naming system is different. Because you cannot necessarily use the charge to
indicate the quantities of each atom in the compound, the name must indicate the amounts using standard prefixes: mono, di, tri, tetra, penta, hexa, hepta, octa, nona, and deca
The only time a prefix is not used is for the first element of the name when there is only one of that element in the compound. CO carbon monoxide N2O4 dinitrogen tetraoxide