4 - Ionic Compounds SNC2D Chemistry Chemical Reactions

4 - Ionic Compounds SNC2D – Chemistry – Chemical Reactions

Date: ______

Ionic Compounds

  • Most elements are ______
  • They achieve stability by ______
  • Bonds are electron ______that fill or complete the outer (______) shell to maximum for each element involved
  • In some of these bonds, changes will occur in order to achieve stability
  • What are the elements in an ionic bond?
  • ______

  • How are electrons involved?
  • Electrons (e-) are ______from the ______to the ______
  • Metals become ______
  • Non-metals become ______
  • Ions are held together by the ______attraction (remember grade 9)
  • Example: Sodium (metal) and Chlorine (non-metal)
  • Both are ______elements if consumed
  • Sodium
  • ______
  • Chlorine
  • ______

  • Let’s look at the Bohr Rutherford Diagrams

Lewis Dot Structures

  • The kernel consists of the ______and the ______
  • A kernel is denoted by using the ______for the element
  • The valence electrons are shown as ______
  • Square _____ brackets are used to separate ions and the ______on the ion is shown on the outside of the brackets
  • Recall that atoms are most stable when they have a ______(______) shell
  • How can the requirements of Na solve the requirements of Cl in stability achievement?
  • They form an ionic compound called sodium chloride (table salt)
  • It would appear that bond formation changes ______of elements

Draw Lewis Dot Diagrams for the following compound:

Ca and O Mg and Cl Li and S

Crystal Lattice

  • Ionic compounds do not exist as ______, but rather in large complexes called crystal lattices


Formulae for Ionic Compounds

  • In ionic bonds we looked at the ______of the atoms involved in the compound
  • To create a compound, we take the charge of the ions involved and use the ______rule
  • Since compounds need to be neutral, we can determine the proper ______of the cations and anions to create a neutral compound
  • Subscripts are used to denote the ratio in ______

Ionic Bonds

  • Since you know the charge on each ion, you can “______” the charges to write the chemical formula

Use the criss-cross rule:

Ca and F Li and I Mg and O Na and S


Polyatomic Ions

  • Some ions are made up of ______atoms
  • The entire unit carries a ______

Examples

OH1- NO31- CH3COO1-

  • When working with polyatomic ions, you can follow the criss-cross rule to write the chemical formula

Use the criss-cross rule:

Ca and SO42- Li and CO32- Mg and NO3- Na and ClO3-

Multivalent Metals

  • Some metal atoms can have more than ______
  • These metal cations are listed with ______to indicate what the charge on the ion is

Examples:

______

Use the criss-cross rule:

Cu1+ and SO42- Cu2+ and SO42- Sn2+ and NO3- Sn4+ and NO3-


Naming Ionic Compounds

  • Binary Compounds
  • Binary means _____
  • The general rule is that the metal gets named first
  • Non-metal has an “______” ending
  • Examples:
  • NaCl is ______

MgCl2 Na2O Ca3P2 Al2S3

Polyatomic Ions

  • List of common polyatomic ions

NH4+ Ammonium CH3COO- Acetate

OH- Hydroxide SO42- Sulfate

ClO3- Chlorate CO32- Carbonate

NO3- Nitrate CrO42- Chromate

CN- Cyanide PO43- Phosphate

  • To name a compound with a polyatomic ion, name the metal first, followed by the polyatomic ion
  • Example: NaNO3

KNO3 NH4Cl Ca3(PO4)2 Al2(SO4)3

  • There is a pattern to the naming of polyatomic ions
  • In all the following changes, the charge of the polyatomic ion ______
  • The base name for a polyatomic ion ends with “-ate”
  • If we add a single oxygen, we add “______” to the front of the name of the polyatomic ion
  • Removing an oxygen changes the “-ate” to “_____”
  • Removing 2 oxygen atoms adds a “______” to the front of the name, while the ending is “______”

ClO- ClO2- ClO3- ClO4-

More Examples:

MgClO NaNO2 CuSO3 (Ba)3(PO3)2

  • Sometimes polyatomic ions with a valence (charge) of two or greater can have one or more hydrogen atoms
  • When naming these polyatomic ions, “______” is added in front of the polyatomic ion name
  • The overall charge is changed on the root polyatomic ion by ___ for every hydrogen that is added

HCO3- H2PO42- hydrogen sulfite

Multivalent Metals

  • When naming ionic compounds containing multivalent metals, we add in ______to tell us the charge on the metal
  • Example: PbCl2 ______

FeO Fe2O3 Cu3PO4 Cu3(PO4)2

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