1. Topic #12: The Periodic Table of Elements

2. Valence electrons - outermost electrons of an atom, which are important in determining how the atom reacts chemically with other atoms. Ion-atom or molecule where the total number of electrons is not equal to the total number of protons, giving it a net positive or negative electrical charge. Cation – positively charged ion Anion – negatively charged ion Oxidation Number-is equal to the charge on the ion

4. The Modern Periodic Table --- continued Period ( rows on the periodic table) The periodic table consists of rows called Periods (There are a total of 7 rows or periods, beginning with hydrogen) These rows also designate the energy level where electrons are found (more about this when we talk about electron configuration).

5. The Modern Periodic Table Groups (sometimes called Families) are columns numbered from 1-8, followed by a letter “A” or “B”. The groups designated with a letter “A” (1A to 8A) are often referred as the main group or the “REPRESENTATIVE ELEMENTS”. The groups designated with a “B” (1B through 8B) are referred to as the “TRANSITION ELEMENTS”. A more recent numbering system, which uses the numbers 1 through 18, also appears above each group.

6. The Modern Periodic Table --- Classifying the Elements Metals --- elements that are generally shiny when smooth and clean, solid at room temperature, good conductors of heat and electricity. Most metals are ductile (drawn into wires) and malleable (moldable). Metals are in green

7. The Modern Periodic Table --- Classifying the Elements Nonmetals --- elements that are generally gases or brittle, dull-looking solids. They are poor conductors of electricity. The only nonmetal that is a liquid at room temperature is Bromine. Non metals are in orange

8. The Modern Periodic Table --- Classifying the Elements Metalloids --- elements with physical and chemical properties of both metals and nonmetals. Silicon and Germanium are two of the most important metalloids, as they are used extensively in computer chips and solar cells. Metalloids are in purple

9. THE REPRESENTATIVE ELEMENTS Group 1A – The Alkali Metals Elements in this family have 1 valence electron. Lose their valence electron to form a +1 charged ion. Belong to the s-block in the periodic table.

10. THE REPRESENTATIVE ELEMENTS Group 2A – The Alkaline Earth Metals Elements in this family have 2 valence electrons. Lose their valence electrons to form a +2 charged ion. Belong to the s-block in the periodic table.

11. THE REPRESENTATIVE ELEMENTS Group 3A – The Boron Group Is named for the metalloid Boron Elements in this family have 3 valence electrons Lose their valence electrons to form a +3 charged ion. Belong to the p-block in the periodic table

12. THE REPRESENTATIVE ELEMENTS Group 4A – The Carbon Group Is named for the nonmetal Carbon Elements in this family have 4 valence electrons Lose their valence electrons to form a +4 charged ion OR can gain 4 electrons and form a –4 charged ion. Belong to the p-block in the periodic table.

13. THE REPRESENTATIVE ELEMENTS Group 5A – The Nitrogen Group Is named for the nonmetal Nitrogen Elements in this family have 5 valence electrons Gain 3 electrons to form a -3 charged ion. Except Bismuth, which can lose 3 electrons and form ions with a +3 charge.

14. THE REPRESENTATIVE ELEMENTS Group 6A – The Oxygen Group Is named for the nonmetal Oxygen. Elements in this family have 6 valence electrons. Gain 2 electrons to form a -2 charged ion. Polonium is the most metallic member of this family; it was discovered by Marie & Pierre Curie and named after there native land Poland; it is rare, radioactive & extremely toxic. Contains all three classifications: oxygen and sulfur are nonmetals, selenium & tellurium are metalloids, and polonium is a metal. Belong to the p-block in the periodic table.

15. THE REPRESENTATIVE ELEMENTS Group 7A – The Halogens Are named for their ability to form compounds with all metals. Because these compounds are called salts, Group 7A are called “salt formers,” or Halogens Elements in this family have 7 valence electrons. Gain 1 electron to form a -1 charged ion. Fluorine is a gas & the most reactive of all halogens. Belong to the p-block in the periodic table.

16. THE REPRESENTATIVE ELEMENTS Group 8A – The Noble Gases Were among the last naturally occurring elements to be discovered because they are colorless and unreactive. Elements in this family have 8 valence electrons. This means they have the maximum number of electrons in their outermost energy level, 8, except for helium, which has two. Belong to the p-block in the periodic table.

17. THE TRANSITION METALS Groups 1B- 8B (or more commonly referred to as Groups 3-12) Most are hard solids with high melting & boiling points. Transition metals can lose 2 s electrons and form an ion with a +2 charge Because unpaired electrons can move to the outer energy level, these elements can form ions with a +3 charge or higher, as well. Transition metals belong to the d-block in the periodic table

18. THE INNER TRANSITION METALS -- The Lanthanide Series (Period 6 on the Periodic Table) Silvery metals with relatively high melting points. Because there is very little variation in properties among the inner transition metals, they are found mixed together in nature and are extremely difficult to separate. Belong to the f-block in the periodic table

19. THE INNER TRANSITION METALS -- The Actinide Series (Period 7 on the Periodic Table) Actinides are radioactive elements. Belong to the f-block in the periodic table

20. The atomic radius of a chemical element is a measure of the size of its atoms.

21. Electronegativity, is a chemical property that describes the ability of an atom to attract electrons towards itself.

22. The Electron affinity of a molecule or atom is the energy change when an electron is added to the neutral species to form a negative ion.

23. The ionization energy (EI) of an atom is the minimal energy required to remove electrons from atoms.

24. Electronegativity