Ionic Compounds

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IonicCompounds
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Metals Vs. NonMetals

• Metals
• Left of steps on Periodic Table
• 80 percent of elements are metals
• Pie chart on page 36
• Properties
• Luster
• Conductivity
• Malleable
• Ductile

• NonMetals
• Right of steps
• 20 percent
• Properties
• May lack luster
• Do not conduct
• Except carbon
• Brittle

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Electron Configuration

• The properties of metals and nonmetals are
  greatly influenced by the electron configurations
  of atoms.

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Ionic Compounds

• Atoms may gain or lose electrons thereby becoming
  ions.
• Cation Positive Charge
• Anion Negative Charge
• Why might a certain Ion gain rather than lose
  electrons?

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Electron Configuration

• Number of electrons in the outermost shell is
  key.
• Few electrons ? Tend to lose them
• Close to full Shell ? Tend to gain
• Tendency towards stability

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Compounds and Ionic Bonding

• A compound is a substance which is made of two or
  more kinds of atoms or ions which have joined
  together.
• Attractive force between positive and negative
  ions creates Ionic Compounds.
• NaCl Na Cl-
• The force of attraction between the positive and
  negative ions is known as an Ionic bond.

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IMPORTANT

• When we talk about stability we are referring to
  the number of electrons in the valence shell.

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Review

• Atom
• Ion
• Cation
• Anion
• Why does an atom lose or gain electrons?
• Predictions
• Fluorine, Potassium, Lithium
• How many Chloride ions bond with Magnesium ions?

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Forming Ionic Compounds (Salts)

• Ionic bonds form between METALS and NONMETALS
  when Electrons are transferred (lost or
  received).
• Columns 1,2,13 may transfer with columns
  15,16,17.

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Forming Ionic Compounds

• Electrons get transferred as a result of energy
  input. This may also occur when materials are
  placed in solution.
• A variety of combinations are possible depending
  on the valence electron number.

Atom gained one electron. It now has a negative
charge.
This atom lost one electron and now has a
positive charge.
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Ionic Bonds

• An ionic bond is the attraction between a
  positively charged cation and a negatively
  charged anion.

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Metals in columns 1, 2, 3 are electron donors.
NonMetals in columns 5, 6, 7 receive Electrons.
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Which Elements form Ionic Bonds?

• The central idea (for the 50th time) is that
  electrons, one or more, are transferred between
  the outer shells of adjacent atoms. This Creates
  Ions/Charged Atoms.
• Metals and NonMetals.
• Certain Elements may donate or receive more than
  one electron. It can therefore bond with
  multiple elements.

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Example 1 Na and Cl

• How many valence electrons does each atom have?
• Which atom will tend to Receive e-? Donate?
• What is the charge on each ion?
• What will the ratio between Na and Cl be?

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Example 1 Na and Cl

• Sodium would lose one electron and become
  positively charged, while Chlorine would gain one
  electron becoming negatively charged.
• The positive/negative charge attraction would
  hold the two ions together.

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Example 2 Mg and O

• How many valence electrons does each atom have?
• Which atom will tend to Donate e-? Receive?
• What is the charge on each ion?
• What will the ratio between Mg and O be?

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Example 2 Mg and O

• The Magnesium would lose two electrons, becoming
  2 charged and the Oxygen would gain the two
  electrons becoming
• -2 charged in the process.
• The negative/positive charge attraction (2/-2)
  (four times as much as 1/-1) would hold the two
  ions together.

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Example 3 Mg and Cl

• How many valence electrons does each atom have?
• Which atom will tend to gain e-? Donate?
• What is the charge on each ion?
• What will the ratio between Mg and Cl be?

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Example 3 Mg and Cl

• The Magnesium would lose two electrons, becoming
  2 charged and two chlorines (not one) would each
  gain one electron, each becoming -1 charged in
  the process.
• The three atoms would bond to each other by the
  positive/negative attraction between the ions.

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Naming Ionic Compounds

• The same as naming individual ions.
• Cation, Electron Donor, or Metal in compound is
  said first.
• Anion name is changed to .ide and said second.

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Examples

• Sodium Chloride
• Magnesium Oxide
• Lithium Nitride
• Potassium Bromide

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Using the correct Name

• K2S 7) SrS
• 2) LiBr 8) Al2O3
• 3) Sr3P2 9) MnO
• 4) BaCl2 10) ZnO
• 5) NaBr 11) ZnCl2
• 6) MgF2 12) Cu2O

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Notation

• Ionic Notation
• 3 Na1
• 1 PO4-3
• Ionic Compound Formula
• NaCl
• CaCl2
• Na3(PO4)

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Formulas

• Rules for Writing Formulas
• Metallic Donor is always written first.
• Nonmetallic Receiver is written second.
• Write the number of atoms required to balance the
  formula as subscripts after the element in
  compound.
• NaCl
• MgO
• MgCl2

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The Ionic Compound
NaCl
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Writing NamingIonic Compounds
Na1 Br-1
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Writing NamingIonic Compounds
Ca2 Br-1
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Writing NamingIonic Compounds
K1 O-2
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Writing NamingIonic Compounds
Li ? N ?
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HW Write the Name of the Compound

• MgS 7) KBr
• 2) Ba3N2 8) FeO
• 3) NaI 9) SrF2
• 4) Li2S 10) CaO
• 5) Na3P 11) Al2O3
• 6) KCl 12) Fe2O3

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HW Write the Correct Formula

• Magnesium Oxide
• 2) Lithium Bromide
• 3) Calcium Nitride
• 4) Sodium Sulfide
• 5) Copper (I) Sulfide
• 6) Copper (II) Sulfide

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Practice Exercise 1

• Which will donate, Which will receive?
• How many will be donated/received?
• Write the Ionic Notation of each.
• Write the formula for each of the following.
• Lithium Oxide
• Potassium Chloride
• Sodium Nitride
• Calcium Chloride
• Magnesium Sulfide
• Barium Nitride
• Aluminum Fluoride
• Aluminum Oxide
• Aluminum Nitride

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Diagramming Ionic Compounds

• Lewis Structures
• Diagram valence shell.
• Place valence electrons around nucleus as they
  would be according to the octet rule

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Diagramming Ionic Compounds
Na
Na
Cl-
Cl
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Practice Exercise 2

• Diagram the following Ionic Compounds
• Lithium Oxide
• Potassium Chloride
• Sodium Nitride
• Calcium Chloride
• Magnesium Sulfide
• Barium Nitride
• Aluminum Fluoride
• Aluminum Oxide
• Aluminum Nitride

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Transition Metals

• d block elements that can form more than one kind
  of ion.
• Lose electrons
• Why can they lose different numbers of electrons?
• Copper
• Cu I or Cu II
• Iron
• Fe II or Fe III

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Implications

• Copper and Iron as well as other transition
  metals can form multiple ionic compounds.

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Polyatomic Ions

• Compound Ions
• A group of COVALENTLY bonded atoms that have a
  net charge (anion or cation)
• Most, but not all are Anions.

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Polyatomics

• SO4-2 Sulfate
• SO3-2 Sulfite
• NO3-1 Nitrate
• NO2-1 Nitrite
• CO3-2 Carbonate
• CN-1 Cyanide
• OH-1 Hydroxide
• NH41 Ammonium

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Na3PO4
Na
P
O
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Phosphate can accept 3 electrons.
PO4-3
O
When it does it has a negative 3 charge.
P
O
O
It is therefore called a..
O
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Sodium Phosphate
O
Na
O
P
O
Na
O
Na3PO4
Na
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Practice Exercise 3

• Give the Ionic Notation and Formula for each.
• Potassium Sulfate
• Magnesium Sulfite
• Aluminum Nitrate
• Sodium Nitrite
• Lithium Carbonate
• Sodium Cyanide
• Barium Hydroxide
• Ammonium Chloride
• Ammonium Hydroxide
• Draw/Diagram Magnesium Sulfite

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Practice Exercise 4

• Write out the Ionic Notation, Formula and Names
  of the following ionic compounds
• Li and F - Na and CO3-2
• Na and S - Li and OH-1
• K and Br - NH41 and Cl
• Rb and O - Ca and SO4-2
• Ca and Cl - NH41 and OH-1
• Mg and SO3-2 - Na and CN-1
• Al and NO3-1 - NH41 and SO4-2