Understanding Atomic Structure and Chemical Bonding

The way atoms are built helps us understand how they bond together. Let’s break down some key ideas:

1. Electron Configuration:

   • Electrons, which are tiny particles around the nucleus of an atom, are found in different areas called orbitals.
   • The first orbital can hold up to 2 electrons.
   • The second can hold 8 electrons.
   • The third can hold even more—up to 18 electrons.

2. Valence Electrons:

   • The electrons that matter most for bonding are called valence electrons.
   • These are the electrons on the outermost shell of an atom.
   • For example, elements in Group 1 have 1 valence electron, while elements in Group 17 have 7 valence electrons.

3. Types of Bonds:

   • Ionic Bonds: These are made when electrons move from one atom to another. For example, in table salt (NaCl), sodium (Na) gives away 1 electron to chlorine (Cl).
   • Covalent Bonds: These happen when atoms share electrons. A good example is water (H₂O), where oxygen and hydrogen share electrons.

4. Electronegativity:

   • This term describes how strongly an atom can attract electrons from other atoms when they bond.
   • Electronegativity is measured on a scale created by Pauling, where the lowest is 0.7 (for francium) and the highest is 4.0 (for fluorine).

In summary, learning about atomic structure helps us see how different elements connect with each other and form a variety of substances.