The Periodic Table – Chapter 7

1. The Periodic Table – Chapter 7 By Mrs. Shaw

2. Lesson 1: Using the Periodic Table What is the Periodic Table? The Periodic Table is a chart of the elements arranged into rows and columns according to their physical and chemical properties. Columns = Groups Rows = Periods

3. The Development of the Periodic Table The Periodic table of elements was devised to organize the known elements into categories that had similar properties. Dimitri Mendeleev, a Russian chemist, decided to organize the elements in order by atomic mass. When he did that he noticed a repeating pattern appeared of elements with similar properties. Periodic means “repeating pattern”.

4. Mendeleev’s original periodic table Notice the gaps that he allowed for.

5. New discoveries led to new table In 1914 Henry Moseley, a British scientist, determined that rearranging the elements in order of their atomic number actually worked to align the elements based on their similar physical and chemical properties and filled in all the newly discovered elements. Atomic number = # of protons Element Symbol Element Name Atomic mass (average )

6. Arranging the Elements Periods Groups or Families A vertical column of elements is called a group or family. Elements in each group or column usually have similar properties. Each row of elements is called a period.

7. Classification of the Elements Elements in the periodic table are classified into three main groups: metals, nonmetals, and metalloids.

8. Metals ROCK!!! Over 70% of elements are metals They are ductile, malleable, and good CONDUCTORS of electricity. Metals

9. Nonmetals Rule! Nonmetals include the Noble gases. They are brittle and dull and can’t conduct heat or electricity. Nonmetals

10. Metalloids are AWESOME! Metalloids have some of the properties of metals and some of the properties of nonmetals. Metalloids

11. Lesson 2: Metals What are the physical properties of metals? Ductile Metals are elements that are shiny, is easily pulled into wires (ductile) or hammered into thin sheets (malleable) and is a good conductor of electricity and thermal energy. Malleable Shiny (have luster) Good conductivity

12. Other physical properties of metals Density, boiling point, and melting points are greater in metals than of other types of elements. AND Except for Mercury all metals are SOLID at room temperature.

13. Group 1: Alkali Metals Properties Examples Group 1 K + H2O Na Remember elements in the same group (column) have similar properties. Alkali metals are very reactive (they want to chemically bond so are found in compounds) Pure alkali metals are silvery and soft enough to cut with a knife and have the lowest densities of all metals.

14. Group 2: Alkaline Earth Metals Examples Properties Mg React quickly but not as quick as alkali metals. Found as compounds due to their need to react. Soft, silvery with low densities but not as low as alkali metals.

15. Groups 3-12: Transition Metals Transition metals have higher densities, boiling points and greater strength than other types of metals (alkali or alkaline earth). They react less than other metals and some exist as free elements (not as a compound). Examples are: Nickel (Ni), Copper (Cu) and Gold (Au)

16. Lanthanide & Actinide Series Lanthanide series elements are used to make strong magnets. Plutonium is an element in the actinide series that is used as fuel in some nuclear reactors.

17. Pattern in properties of metals Metallic properties increase as you move to the left and down on the periodic table.

18. Did you know that more than 96% of your body’s mass comes from just 4 elements – Oxygen, Carbon, Hydrogen, and Nitrogen and all are Nonmetals. Lesson 3: Nonmetals and Metalloids

19. Properties of Nonmetals Non-metals are brittle, dull, and not good conductors of thermal or electrical energy. Because they are not good conductors they are really good INSULATORS! Many are gases at room temperature.

20. Examples of Insulators The nose cone on the tip of the space shuttles are created using non-metals that insulate against the intense heat of re-entry! Other examples

21. Properties of Metalloids Metalloids are elements that have properties of both metals and nonmetals. Some metalloids are semiconductors or an element that conducts electricity at a high temperature but not a low temperature

22. Valence Electrons Valence electrons are the electrons in the outermost shell that determines a atom’s chemical properties. The amount of electrons in the outer level determine if an atom will likely bond with another – they want to be full so bonding will help that happen.

23. Chemical bonding Chemical bonding is the joining of atoms to form new substances. A chemical bond is an interaction that holds two atoms together. Most atoms form bonds by gaining, losing, or sharing valence electrons until they fill their outer shell to become “happy”.

24. Types of Chemical Bonds There are two types of chemical bonds we will discuss: ionic bonds and covalent bonds.

25. Ionic Bonds Ionic bonds happen when electrons are transferred from one atom to another, causing the atom to become either positively charged or negatively charged. Na + Cl= Na Cl Table Salt

26. Ionic Bond

27. Covalent Bonds Covalent bonds happen when atoms share electrons. For example: Chlorine needs one electron to have a full outer shell so it can share 2 electrons with another Chlorine atom and become stable.

28. Covalent Bonds Another very important covalent bond is H + H + O = H2O