1. Atomic Structure and Bonding The Structure of Atoms

2. Specific Learning Outcomes Describe or label a diagram of a model of an atom using the terms protons, neutrons, electrons and nucleus. Define atomic number (Z) Define mass number (A) Define and give examples of isotopes. Calculate the number of electrons, protons and neutrons in any named atom. Write electron configurations of the first 20 elements using 2,8,8 notation.

3. A little Atomic History In 1806 John Dalton reintroduced the idea of an atom. His theory suggested that all elements were made up of atoms. These atoms were unique to the element and could not be created or destroyed. When atoms from different elements joint together they would form compounds. Amedeo Avogrado 1811 Discovered that some elements existed in combinations atoms like Cl 2 or O 2 Jons Berzelius 1813 Devised the “Chemical Symbol” First letter uppercase, second letter lower case. J J Thomson 1897 Discovered electrons. Ernest Rutherford 1911 Discovered a lot more about atomic structure – like polarity and density. Henry Moseley 1914 Learnt how to count the positive charges in an atom and how electrons were arranged.

4. The Structure of Atoms Electron (Negative Charge) Neutron (No Charge) Proton (Positive Charge) Nucleus There are three pieces to an atom. There are electrons, protons, and neutrons. As you know, there are over 100 elements in the periodic table. The thing that makes each of those elements different is the number of electrons, protons, and neutrons. The protons and neutrons are always in the centre of the atom. Scientists call the centre of the atom the nucleus. The electrons are always found whizzing around the centre in areas called orbitals. Energy Level

5. Atomic Number and Mass Number Chemists have a symbolic way of representing atoms which enables them to quickly see how many protons, neutrons and electrons an atom has… Mass Number Element Symbol Atomic Number Atomic Number = Number of protons in the nucleus or Number of electrons outside of the nucleus Atomic Number = Number of protons in the nucleus or Number of electrons outside of the nucleus Mass Number = Number of protons plus neutrons in the nucleus Mass Number = Number of protons plus neutrons in the nucleus

6. Isotopes Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, with two neutrons. HydrogenDeuteriumTritium

7. Atomic Number and Mass Number Activities The Structure of Atoms (page 44) Complete Table Level 2 Chemistry Practical Workbook What's the most important thing to learn in chemistry? Never lick the spoon.

8. Electron Configuration An electron configuration of an atom is a description of the number of electrons in each energy level. Nucleu s 1 st Level 2 nd Level 3 rd Level 4 th Level For example for the element calcium where Z = 20, the electron configuration would be as 2,8,8,2. To complete an electron configuration take the atomic number (Z) and spread it out through the levels – each level has a maximum number of electrons that it will hold as demonstrated above. Whatev er is left over

9. Electron Configuration Activities Electron Configurations of the First 20 Elements (page 10) Complete Question 1 (a, c, e, g & i) Complete Question 2 (b, d, f, h, & j) Complete Question 3 Complete Question 4 (a & b) Level 2 Chemistry Theory Workbook