1. Each element has a symbol Each square on the periodic table contains information about the element Atomic number Chemical symbol Name Atomic mass An international committee of scientists is responsible for approving the names and chemical symbols of the elements.

2. Chemical symbol Usually consists of 1 or 2 letters First letter is always capitalized Second letter is always lower case

3. Rows are called periods Period= each horizontal row of elements from left to right The physical and chemical properties of the elements are different, the number of electrons in the outer level of atoms are different, and the elements change gradually from metallic to non-metallic Elements at the left= metallic Elements at the right= non-metallic

4. Columns are called groups Group= a column (from top to bottom) on the periodic table Elements in the same group often have similar chemical and physical properties Sometimes call a group a family Same number of outer electrons

5. Review questions 1.Compare a period and a group on the periodic table. 2.How are the elements arranged in the modern periodic table? 3.Compare metals, non-metals, and metalloids in terms of their electrical conductivity.

6. Grouping the elements Elements in a group share similar properties since the atoms of the elements have the same number of electrons in their outer energy level

7. Groups 1 & 2: very reactive metals Highly Reactive= Give away electrons very easily!! Only found combined with other elements in nature or in ionic form

8. Group 1: Alkali Metals 1 electron in the outer level Very reactive – their atoms can easily give away a single electron Soft, silver-colored, shiny Usually stored in oil to prevent them from reacting with water and the atmosphere Examples of compounds formed with alkali metals: Sodium chloride (table salt) Sodium hydroxide (unclogs drains) Potassium bromide (photography)

9. Group 2: Alkaline-Earth Metals 2 electrons in their outer shell Very reactive, but less reactive than alkali metals in group 1 since they need to give 2 electrons away Silver colored Examples of alkaline earth metals or compounds: Magnesium (airplanes) Calcium (cement, plaster, chalk, and YOU!)

10. Groups 3-12: Transition Metals 1 or 2 electrons in the outer level Do not give their electrons away as easily Shared properties of shiny, good conductors, higher densities and melting points than that of groups 1 & 2 Form colored solutions Examples: Mercury (thermometers, barometers) Gold (jewelry) Titanium (artificial limbs) Iron (steel towers)

11. Lanthanides & Actinides Some transition metals from periods 6 & 7 are placed at the bottom of the periodic table to keep the table from being too wide! Lanthanides= follow lanthanum in the periodic table Shiny, reactive metals Actinides= follow actinium in the periodic table Radioactive, unstable= can change atoms into different elements

12. Review Questions! 1.What are the 2 properties of the alkali metals? 2.What causes the properties of elements in a group to be similar? 3.Why are neither the alkali metals nor the alkaline-earth metals found uncombined in nature?