In Year 10 Chemistry, it's important to understand how the physical and chemical properties of elements change across the periodic table. Let’s explore some key trends!

1. Atomic Radius:

   • As you go from left to right across a row in the periodic table, the atomic radius usually gets smaller. This happens because the nucleus of the atom, which has a positive charge, pulls the electrons closer. So, the atom becomes smaller. For example, sodium (Na) is bigger than chlorine (Cl), which means Cl has a smaller atomic radius.

2. Electronegativity:

   • Electronegativity is a way to measure how well an atom can attract electrons. When you move from left to right, electronegativity usually increases. For instance, fluorine (F) has a high electronegativity, while sodium (Na) has a much lower electronegativity. This trend is important for understanding how atoms bond with each other.

3. Ionisation Energy:

   • Ionisation energy is the energy needed to remove an electron from an atom. Like electronegativity, ionisation energy tends to increase as you move across a period. This means that atoms hold onto their electrons more tightly as you go from left to right.

These trends show how the periodic table is set up in a way that affects the properties of different elements. Understanding these patterns helps us learn more about chemistry!