Ionic bonds are like a handshake between two atoms. They happen when one atom gives away electrons to another atom. This usually occurs between metals and non-metals. However, this process can be tricky because it takes a lot of energy to make it happen.

1. Difficulty in Electron Transfer:

   • Metals need to lose electrons, which requires them to fight against something called ionization energy.
   • On the other hand, non-metals need to gain electrons, which is a challenge because of electron affinity.
   • It gets even harder if the atoms involved are similar in strength, or electronegativity.

2. Lattice Energy:

   • The strength of ionic bonds also depends on something known as lattice energy. This is affected by two main factors:
     • Charge of Ions: The more electric charge an ion has, the stronger the attraction. For example, $Na^+$ is weaker than $Mg^{2+}$ because $Mg^{2+}$ has a higher charge.
     • Ion Size: Smaller ions can come closer together, which makes them attracted to each other even more. But, figuring out how big the ions are and how that affects the bonds can be complicated.

3. Solvent Effects:

   • Ionic compounds are often studied in liquids. However, the liquid can interact with the ions and weakens the ionic bonds, making it hard to understand just how strong they really are.

To tackle these problems, it's important to have a good grasp of atomic structure and how crystals form. Working through practice problems and using models can really help students understand ionic bonding better. This way, they can feel more confident tackling the twists and turns of ionic bonds.