BONDING
UNIT
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)
•Define a bond
•Define ion as well as cation and anion
•Compare and contrast ionic, covalent and
metallic bonding
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.
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
IONIC
BONDING
COVALENT
BONDING
•Involves a transfer of
electrons
•Involves the sharing of
electrons
•The ions are held together by
the electrostatic attraction
between oppositely charged
ions
•The bond is formed by
electrostatic attraction
between the shared pairs of
electrons and the positively
charged nuclei
•The ions are held together in
lattice structures
•Under normal conditions
ionic compounds are usually
solids
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
•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
GROUP 1
•Called Alkali metals
•Form cations with 1+ charge
GROUP 2
GROUP 3
•Called Alkaline Earth
metals
•This family is sometimes referred to as
the Boron family.
•Form cations with a 2+
charge
•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 5
•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
GROUP 7
•The most common oxidation
state is -2, however oxygen
can also exist as -1 in the case
of peroxides .
•Referred to as Halogen. Hal means
“salt” and gen means “to form”
•Sulfur can also exist at a +4
and +6 state and +2, +4, and
+6 oxidation states are
possible for Se, Te, and Po.
•Can share electrons with other atoms
and can have positive oxidation
numbers
•Tend to gain electrons to form 1- anions
•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