Atomic Structure

Atomic Structure

1. Atomic Structure

   • posetively charged nucleus with negatively charged electrons moving around the outside of the nucleus
   • Location, charge in mass of protons, neutrons and electrons in an atom

2. Nucleide notation

   • Nucleide notation is used to show the numberof sub-atomic particles in an atoms or ion
   • I can determin the number of sub-atomic particles in atoms and ions from nucleide notation
   • The atomic number is the number of protons
   • The mass number is the number of protons PLUS neutrons

3. Atoms and Ions

   • In an atom the number of protons and electrons is equal
   • When there is an imbalance in the number of protons and electrons the particles is know as an ion
   • Ions are formed are formed by loss or gain of electrons to achieve a stable electron configuration
   • Metals tend to form positive ions and Non-metals tend to form negative ions

4. Isotopes

   • Same atomic number but different mass numbers
   • same numbers of protons but a different number of neutrons
   • most elements exist as a mixture of isotopes
   • The relative atomic mass is the average mass of the isotopes presents, taking into account their relative proportions
   • Identify the most or least abundant isotopes, or calculate relative atomic mass using a given formula

5. electron arrangement

6. Periodic Table