1. Review When looking at atoms, what three numbers are the same? How do you find the number of neutrons? What subatomic particles make up the nucleus? Protons, Neutrons, Electrons Practice worksheet

2. The Periodic Table Column = Group or Family 18 columns on the Periodic Table Row = Period 7 rows on the Periodic Table Lanthanides and actinides are printed below the rest of the elements to make the table easier to read.

3. What does the information in the box tell me? 1 H 1.008 Atomic Number = # of protons Atomic Mass = # of protons plus neutrons Elemental Symbol

4. EQ: How does the reactivity of metals change across the periodic table?

5. Identifying the groups Color the alkali metals blue (use pages 132-133) to fill in your periodic table Color the alkaline earth metals light green Color the transition metals yellow Color the metals in the mixed group purple Color the actinides dark green Color the lanthanides orange Put a yellow circle on the metalloids chemical symbol

6. Identifying the groups Outline the boron family in pencil Outline the carbon family members in red Outline the nitrogen family members in light blue Outline the oxygen family members in green Outline the halogen family members in brown Outline the noble gases in dark blue Draw in the stair case in black

7. Metals, Nonmetals, and Semi-metals Metals are to the left of the stair- step Only nonmetal on the metal side Nonmetals are on the right of the stair-step Semi-metals, “metalloids,” touch the stair-step

8. Group 1 – The Alkali Metals –Most reactive metals on the Periodic Table Alkali metals react with other elements by losing one valence electron. Most common Na (Sodium) and K (Potassium) charge is +1 charge is +1

9. Group 2 – Alkaline Earth Metals –Still quite reactive. –Each is fairly hard, gray-white, and a good conductor of electricity. –Most common Mg (Magnesium) and Ca (Calcium) –Like to lose 2 valence electrons –Charge is +2 Video on alkali and alkaline earth metalsVideo on alkali and alkaline earth metalsVideo on alkali and alkaline earth metalsVideo on alkali and alkaline earth metals

10. T he Groups of the Periodic Table Groups 3-12: Transition MetalsGroups 3-12: Transition Metals –Found freely and in compounds in nature –Charge is usually +2 –Transition metal Video Transition metal VideoTransition metal Video Group 13: Boron FamilyGroup 13: Boron Family –Charge is +3 (with 3 valence electrons)

11. Transition Metals The elements in Groups 3 through 12 are called the transition metals. The transition metals include most of the familiar metals, such as iron, copper, nickel, silver, and gold. Most of the transition metals are hard and shiny. All of the transition metals are good conductors of electricity. Many of these metals form colorful compounds.

12. Groups 13-15 (Metals in mixed group, metalloids) Only some of the elements in Groups 13 through 15 of the periodic table are metals. These metals are not nearly as reactive as those on the left side of the table. The most familiar of these metals are aluminum, tin, and lead.

13. Carbon Family Each element in the carbon family has atoms that can gain, lose, or share four electrons (+4 or -4) when reacting with other elements. In Group 14, only carbon is a nonmetal. What makes carbon especially important is its role in the chemistry of life. Carbon is found in all living things.

14. Nitrogen Family Nitrogen is an example of an element that occurs in nature in the form of diatomic molecules, as N 2. A diatomic molecule consists of two atoms. In this form, nitrogen is not very reactive. -3 charge

15. Oxygen Family -2 electrons Like nitrogen, the oxygen you breathe is a diatomic molecule (O 2 ). Oxygen sometimes forms a triatomic (three-atom) molecule, which is called ozone (O 3 ). Highly reactive since it can combine with almost every other element. Most abundant element in Earth’s crust and the second- most abundant element in the atmosphere. (The first is nitrogen.) Group 16

16. Group 17 contains elements are also known as the halogens, which means “salt forming.” The most reactive non-metals. A halogen atom typically has a charge of -1 when it reacts with other elements. Halogen Family Comparing the four halogens video

17. Noble Gases The elements in Group 18 are known as the noble gases. They do not ordinarily form compounds because atoms of noble gases do not usually gain, lose, or share electrons. The noble gases are usually unreactive. Inert Gases

18. Properties of Metals Conductivity –Ability to transfer heat or electricity to another object. Reactivity –The ease and speed that elements combine (or reacts) with other elements and compounds. Corrosion –Destruction of metal or the gradual wearing away of a metal element due to a chemical reaction.

19. Special Rows on the PT Lanthanides Actinides

20. Lanthanides Two rows of elements are placed below the main part of the periodic table. The elements in the top row are called the lanthanides (lan thuh nydz). Lanthanides are soft, malleable, shiny metals with high conductivity. They are mixed with more common metals to make alloys. An alloy is a mixture of a metal with at least one other element, usually another metal.

21. Actinides The elements below the lanthanides are called actinides (ak tuh nydz). All of the elements after uranium in the periodic table were created artificially in laboratories. (Synthetic) –The nuclei of these elements are very unstable, meaning that they break apart very quickly into smaller nuclei. In fact, many of these elements are so unstable that they last for only a fraction of a second after they are made. Element 117 video

22. Hydrogen The element with the simplest and smallest atoms. Each hydrogen atom has one proton and one electron. Some hydrogen atoms also have neutrons. Because the chemical properties of hydrogen differ very much from those of the other elements, it really cannot be grouped into a family. Hydrogen is rarely found on Earth as a pure element. Most hydrogen is combined with oxygen in water (H 2 O). +1 charge

23. Metalloids Along the border between the metals and the nonmetals are eight elements called metalloids. The metalloids have some characteristics of both metals and nonmetals. –All are solids at room temperature. –They are brittle, hard, and somewhat reactive. The most common metalloid is silicon (Si). Silicon combines with oxygen to form silicon dioxide (SiO 2 ). Ordinary sand, which is mostly SiO 2, is the main component of glass.

24. Metalloids Continued The most useful property of the metalloids is their varying ability to conduct electricity. Whether or not a metalloid conducts electricity can depend on temperature, exposure to light, or the presence of small amounts of impurities. Metalloids such as silicon, germanium (Ge), and arsenic (As) are used to make semiconductors. Semiconductors are substances that can conduct electricity under some conditions but not under other conditions. Semiconductors are used to make computer chips, transistors, and lasers.

25. Electrons (e-) Electrons move within a sphere-shaped region surrounding the nucleus. Scientists depict this region as a cloud of negative charge because electrons may be anywhere within it. –Electrons with lower energy usually move in the space near the atom’s nucleus. –Electrons with higher energy move within the space farther from the nucleus. Most of an atom’s volume is the space in which electrons move. That space is huge compared to the space taken up by the nucleus.

26. Light and the Atom  Atoms absorb and then emit energy with their electrons  When the energy emitted falls within the visible spectrum we see it as light

27. Mendeleev Father of the periodic table Arranged his periodic table by atomic mass Today it is arranged by atomic number Mosley later discovered that the periodic nature of the elements was associated with atomic number and not atomic mass.

28. Isotopes See Isotopes ppt

29. CaCl 2 + NaHCO 3  ?

30. What are the reactants? Calcium chloride: ice melt or driveway “heat” CaCl 2 Sodium bicarbonate: baking soda NaHCO 3

31. CaCl 2 + NaHCO 3  NaCl + CaCO 3 + H 2 CO 3 H 2 CO 3  H 2 O + CO 2 heat

32. What are the products? Sodium chloride: table salt NaCl Calcium carbonate: chalk CaCO 3 Carbonic acid: found in cola H 2 CO 3

33. Obeying the law of conservation of mass For a completely correct model, we must be sure that there are equal numbers of each type of atom on left and right side.

34. CaCl 2 + NaHCO 3  NaCl + CaCO 3 + H 2 CO 3 H 2 CO 3  H 2 O + CO 2 heat Need to balance equation