IB Chemistry SL 4.1 - Ionic Bonding and Structure
4.1.1 - Ionic Bonding
Ionic Bonding - Bonds where one atom donates electrons to another; the atom that loses an electron becomes a cation and the other becomes an anion
Cation - An ion with a positive electric charge
Anion - An ion with a negative electric charge
Ionic Bonds are the result of the electrostatic attraction between ions
Ionic Compounds - Usually form between a metal and a nonmetal (easy way to find them)
Atoms use ionic bonding to reach full valence shells that satisfy the octet rule (the tendency of most atoms to want 8 electrons in their valence shells)
Ionic compounds arrange themselves into a crystal/lattice structure (in other words, a regular pattern of repeating structures of atoms)
The ratio of elements in a crystal structure is used to give the chemical formula (ex. In NaCl, there is one sodium atom for every chlorine, thus their ratio is 1:1 and the formula is NaCl)
Ionic bonding is non-directional (force occurs on an atom from all sides)
Coordination Number - gives the # of atoms another atom of a compound is in contact with
Both coordination numbers define how a compound is coordinated (ex. In NaCl, each sodium atom is bonded to 6 chlorine atoms and the same goes for chlorine, so its coordination is 6:6)
Note that many compounds contain bonds with both ionic and covalent properties
4.1.2 - Formulae of Ionic Bonds
Groups 1, 2, and 13 have ionic charges of 1+, 2+, and 3+ respectively
Groups 15, 16, and 17 have ionic charges of 3-, 2-, and 1- respectively
Polyatomic Ions - ions made of multiple atoms bonded covalently
The charges of ionic compounds must cancel out (the sum of the charges of the atoms within it must be 0)
4.1.3 - The physical Properties of Ionic Compounds
Strong electrostatic forces between ions lead to a high boiling/melting point
Melting point depends on ionic charge and radius
Melting point tends to increase when ionic charge increases
Melting point tends to decrease when ionic radius increases
Ionic compounds have low volatility (they do not change state easily)
Most ionic compounds are soluble in water
The first step in dissolution in water is a breaking of the lattice structure
Then water surround the ions that have broken off (hydration)
Water is polar (more on that later)
Non-polar solvents have limited solubility with ionic compounds while polar solvents tend to dissolve ionic compounds very effectively
Ionic compounds have a low electrical conductivity when they are solid because of the lack of free (delocalized) electrons
Ionic compounds are good electric conductors when they are molten or dissolved
Ionic compounds tend to be brittle as they fracture along an entire plane when ions are misaligned
IB Chemistry SL 4.2 - Covalent Bonding
4.2.1 - Nature of the Covalent Bond
Covalent bonding usually occurs between elements with a difference in electronegativity (EN) less than 1.8 units
Non-metals form covalent structures
Covalent Bonding - An electrostatic attraction between positive nuclei and shared pairs of electrons
Each pair helps each atom fill its valence shell (octet rule)
Single pairs contain 2 electrons, double pairs contain 4, triple pairs contain 6
Bond Length - The distance between bonded atoms
Bond Strength - The amount of energy needed to break a bond
More bonds lead to a decrease in length but an increase in strength
Coordinate covalent bond - A covalent bond where both electrons in a pair are given by one atom
Electron Deficient (lacking electrons) atoms are able to form covalent bonds
Dimer - Molecule formed by two identical smaller molecules linked by coordinate covalent bonds or hydrogen bonds
Bond Order - # of bonds between a pair of atoms
To calculate the bond order of a multi-atom molecule, sum the individual bond orders and divide by the number of bonds
4.2.2 - Polarity of Covalent Bonds
The following table gives the polarity ranges of types of bonds:
Difference in EN | Type of Bond |
>=1.8 | Ionic |
0.5-1.7 | Polar covalent |
0.1-0.4 | Non-Polar Covalent |
0 | Pure Covalent |
Notice that most bonds are a mixture of ionic and covalent bonds
An increase in EN leads to an increase in polaitry and ioinc character
In a pure covalent bond, electrons are shared equally
Polar-covalent bonds have properties between ionic and covalent bonds
Electrons are unequally shared and form a bond dipole (one side is partially positive and the other is partially negative, more on this later)
The existence of polar bonds is a requisite for a polar molecule
IB Chemistry 4.1 - 4.2
IB Chemistry SL 4.1 - Ionic Bonding and Structure
4.1.1 - Ionic Bonding
4.1.2 - Formulae of Ionic Bonds
4.1.3 - The physical Properties of Ionic Compounds
IB Chemistry SL 4.2 - Covalent Bonding
4.2.1 - Nature of the Covalent Bond
4.2.2 - Polarity of Covalent Bonds
Difference in EN | Type of Bond |
>=1.8 | Ionic |
0.5-1.7 | Polar covalent |
0.1-0.4 | Non-Polar Covalent |
0 | Pure Covalent |