1. BONDING UNIT TIER 1 Define a bond
TIER 1
Define a bond
Define ion as well as cation and anion
Compare and contrast ionic, covalent and metallic bonding
TIER 2
Deduce which ions form when elements in Groups 1,2 & 3 lose electrons
Deduce which ions form when elements in Groups 5,6, & 7 gain electrons
Explain which ions form when transition metals lose electrons
TIER 3
Apply electronegativity values and the position of two elements on the periodic table to determine the type of dominant bonding that occurs; ionic, polar covalent or nonpolar covalent
Describe the lattice structure of ionic compounds and apply this to explain the physical properties of ionic compounds
Describe the model of metallic bonding and apply this to explain the physical properties of metals
State and explain the relationship between number of bonds, bond length and bond strength.
TIER 4
Deduce the Lewis structures of molecules and ions for up to four electrons pairs on each atom
Predict the shape and bond angles for species with four, three and two negative charge centers on the center atom using the valence shell electron pair repulsion theory (VSEPR)
Analyze the physical properties of covalent compounds resulting from single, double and triple bonds
Describe and compare the structure and bonding in the three allotropes of carbon; diamond, graphite and fullerene.
Describe the structure and bonding of silicon and silicon dioxide
TIER 5
Evaluate the type of intermolecular forces that occurs between covalent molecules based on the structural features of the molecules
Evaluate how the intermolecular forces affect the boiling points of substances
TIER 6
Design a lab that shows a trend in a physical property of substances that are either ionic, covalent or metallic. ( This will be your first official IA lab for IB submission)

2. TIER 1 Define a bond Define ion as well as cation and anion
Compare and contrast ionic, covalent and metallic bonding

3. WHAT IS A BOND?
Any of several forces, especially the ionic bond, covalent bond, and metallic bond, by which atoms or ions are bound in a molecule or crystal.

4. IONS CATION OR ANION
An ion is a charged atom that has either gained or lost electrons
A cation is a positively charged ion that has lost electrons
An anion is a negatively charged ion that has gained electrons
***REMEMBER: The charge is from the uneven distribution of electrons to protons and since electrons are negatively charges and protons are positively charge, if there are more electrons than protons then the ion will be negatively charged and if there are more protons than electrons then the ion will be positively charged. The charge DOES NOT refer to the gain or lose of electron. CHARGE IS NOT A MATHEMATICAL SIGN

5. IONIC, COVALENT OR METALLIC BONDING
Involves a lattice of cations with delocalized electrons
The electrons are free to move within the lattice forming a “sea of electrons”
The strength of the bond depends on the charge of the ions and the radius of the metal ion
IONIC
BONDING
Involves a transfer of electrons
The ions are held together by the electrostatic attraction between oppositely charged ions
The ions are held together in lattice structures
Under normal conditions ionic compounds are usually solids
COVALENT
BONDING
Involves the sharing of electrons
The bond is formed by electrostatic attraction between the shared pairs of electrons and the positively charged nuclei

6. TIER 2
Deduce which ions form when elements in Groups 1,2 & 3 lose electrons
Deduce which ions form when elements in Groups 5,6, & 7 gain electrons
Explain which ions form when transition metals lose electrons

7. GROUPS 1,2 & 3 ELEMENTS GROUP 3 GROUP 1 GROUP 2
This family is sometimes referred to as the Boron family.
This group consist of boron , a metalloid, and the other elements Al to Tl which are metals
All can form 3+ cations.
However, Indium and Thallium can also form 1+ ions. The most common ion for Indium is 3+ but the most common ion for Thallium is 1+ .
GROUP 1
Called Alkali metals
Form cations with 1+ charge
GROUP 2
Called Alkaline Earth metals
Form cations with a 2+ charge

8. GROUP 5,6 & 7 GROUP 5 GROUP 6 GROUP 7
This group contains the nonmetals, Nitrogen and Phosphorus, the metalloids, Arsenic & Antimony and the metal, Bismuth
Both N & P from 3- anions in ionic compounds. There oxidation states can also be 3+ & 5+
Both As & Sb have 3-, 3+ & 5+ oxidation states
Bismuth forms 3+ & 5+ cations
GROUP 6
The most common oxidation state is -2, however oxygen can also exist as -1 in the case of peroxides .
Sulfur can also exist at a +4 and +6 state and +2, +4, and +6 oxidation states are possible for Se, Te, and Po.
GROUP 7
Referred to as Halogen. Hal means “salt” and gen means “to form”
Tend to gain electrons to form 1- anions
Can share electrons with other atoms and can have positive oxidation numbers

9. TRANSITION METALS Referred to as “d block” metals
Also called multivalent metals due to the fact that most will form cations with more than one oxidation number
For example, Iron can either be Fe 2+ or Fe 3+
Zinc, cadmium and silver however are not multivalent. Zn & Cd are 2+ and Ag is 1+
The name of the compound formed by transition metals and nonmetals will have a Roman numeral to designate the charge of the transition cation
Tend to form colored compounds