How to Read the Periodic Table

1. How to Read the Periodic Table

2. Understanding the Periodic Table • Now that we know we have Atoms that make up matter. • Each atom has a nucleus and an electron cloud. • Each Nucleus had Protons and/or Neutrons. • Each Atom has an atomic weight.

3. Understanding the Periodic Table • The table is arranged so each element is listed by it’s increasing atomic number. • Also, by Groups. These are columns that run up and down. There are 18. • Groups tell us how many valence electrons each element has in that outer orbital.

4. Groups • The group number of a non-transition metal indicates the number of valence electrons. • Group 1: 1 Valence electron • Group 2: 2 Valence electrons • Group 13: 3 Valence electrons • Group 14: 4 Valence electrons • Group 15: 5 Valence electrons • Group 16: 6 Valence electrons • Group 17: 7 Valence electrons • Group 18: 8 Valence electrons • Except for Helium, It has 2

5. Groups • There are some exceptions to the order when you look at the transition elements, but you get the general idea. • Transition elements start to add electrons to the second-to-last shell.

6. Groups • Knowing valence electrons helps when doing the Lewis Dot diagram. • These diagrams give you a visual picture when working with bonding elements.

7. Periods • Each of the rows is considered to be a different period. • Hint: PERIODic table • All of the elements in a period have the same number of atomic orbitals.

8. Periods • Every element in the top row (the first period) has one orbital for its electrons. • All of the elements in the second row (the second period) have two orbitals. • It goes down the periodic table like that. • the maximum number of electron orbitals or shells for any element is seven.

9. Two at the Top • Hydrogen (H) and helium (He) are special elements. • Hydrogen can have the talents and electrons of two groups: one and seven. • Helium is different from all of the other elements. It can only have two electrons in its outer shell.

10. Metals • I wanted to give you a big overview of metals before we get into details about specific families. • Almost 75% of all elements are classified as metals.

11. How Do You Identify A Metal? • 1. Good conductor of electricity. • 2. Good conductor of heat. • 3. Lustrous or shiny in appearance • 4. Malleable and ductile.

12. Non Metals • the elements on the right side of the periodic table. • Many are gases at room temperature, dull surfaces on the solid nonmetals, cannot be shaped by ductility or malleability.

13. How Do You Identify A Nonmetal? • 1. They are dull in appearance. • They are poor conductors of heat. • They are poor conductors of electricity. • They are brittle.

14. Metalloids • Have properties of both metals and nonmetals • Located on either side of the zigzag line separating metals and nonmetals • Most common is Silicon • Some can conduct heat and electricity but not as good as metals.

15. Families • There are not just columns and rows of the periodic table. There are also other, less specific, groups. • Families of elements by their chemical properties. • Each family reacts in a different way with the outside world.

16. Families • Metals behave differently than gases, and there are even different types of metals. • Some elements don't react, while others are very reactive, and some are good conductors of electricity.

17. Families • Examples of Families • - Alkali Metals- Alkaline Earth Metals- Transition Metals- Halogen Gases- Noble Gases

18. Families • Examples of Physical Properties • - Density- Boiling Point- Melting Point- Conductivity- Heat Capacity Examples of Chemical Properties • - Valence- Reactivity- Radioactivity

19. Alkali Metals • Group 1 • The members of the family include: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr). • They are very reactive. • They all have one electrons in their outer shell. • That's one electron away from being happy (full shells).

20. Alkali Metals • When you are that close to having a full shell, you want to bond with other elements and lose that electron. • An increased desire to bond means you are more reactive. • In fact, when you put some of these pure elements in water (H2O), they can cause huge explosions.

21. Alkali Metals • The alkali metals are also metals. • Characteristics are assigned by the way elements look. • Alkali group is shiny and light in weight. • Their light weight and physical properties separate them from other metals.

22. Alkali Metals • They are malleable (bendable) and sometimes soft enough to be cut with a dull knife. Alkali metals are not the type of metals you would use for coins or houses. • These are Hydrogen(H), lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr).

23. Alkali Metals • They are very reactive. Why? • They all have one electrons in their outer shell. That's one electron away from being happy (full shells). • When you are that close to having a full shell, you want to bond with other elements and lose that electron. • An increased desire to bond means you are more reactive. • Batteries need lithium to work. • Potassium is one of the many elements found in fireworks and pyrotechnics of all kinds.

24. Alkaline Earth Metals • Group 2 • This is the second most reactive family of elements in the periodic table. • Why they are called alkaline is because when these compounds are mixed in solutions, they are likely to form solutions with a pH greater than 7.

25. Alkaline Earth Metals • The members of this Family include: beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). • They bond very easily. • Each of them has two electrons in their outer shell. • They are ready to give up those two electrons in electrovalent/ionic bonds.

26. Alkaline Earth Metals • It's all about giving up those electrons to have a full outer shell. • Beryllium is a very light metal. That's why NASA uses it in the Space Shuttle. • As you get to the bottom of the list, you will find the radioactiveradium.

27. Alkaline Earth Metals • Radium is not found around your house anymore, it used to be an ingredient in glow-in-the-dark paints. • These elements are found in fireworks, batteries, flashbulbs, and special alloys. • Calcium helps build your bones.

28. The Boron Family • These Elements are: Boron (B) Aluminum (Al) Gallium (Ga) Indium (In) Thallium (Ti) • They all have 3 valence electrons • Group 13. • They are metallic (except boron, which is a solid metalloid)

29. The Boron Family • Boron is used in detergents (borax or boric acid) • Aluminum is used in airplanes, tin cans, foil, etc… • Scientists use boron when they make fiberglass.

30. The Carbon Family • Group 14 • This family contains: carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb) • These all have 4 valence electrons. • Silicon is the 2 most abundant element on Earth. • Lead can be poisonous to us but used as a sheild against x-rays.

31. The Nitrogen Family • Group 15 • All of the elements of this family have 5 electrons in their outermost energy level. • This group has: Nitrogen(N) Phosphorus(P) Arsenic(As) Antimony(Sb) Bismuth(Bi)

32. The Nitrogen Family • This group is divided into nonmetals, semimetals, and metals by characteristic. • Nitrogen and phosphorus are nonmetals. Arsenic and antimony are metalloids. Bismuth is a metal. • Nitrogen is essential in most of the compounds that allow life to exist. • almost eighty percent of Earth's atmosphere is made of nitrogen gas.

33. The Nitrogen Family • Scientists use phosphorus to make baking powder • Phosphorus is a very important element in fertilizers. Plants need small amounts of phosphorus to grow up healthy. People also need phosphorus and they get it by eating plants.

34. The Oxygen Family • The elements of this family include: • •Oxygen (O) • •Sulfur (S) • •Selenium (Se) • •Tellurium (Te) • •Polonium (Po) • All of the outer rings have 6 valence electrons • This is group 16 • Breathable Air

35. The Oxygen Family • MedicineSulfur is an important element in medicines. • Sulfur in matches that sparks and starts the flames. • Selenium is an element used in photocopiers. • Large amounts of selenium will act as a poison but you need trace amounts of this mineral to survive.

36. The Halogen Family • Group Seventeen • These elements have 7 valence electrons. • The elements included are fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). • They are all just one electron shy of having full shells. Because they are so close to being happy, they have the trait of combining with many different elements.

37. The Halogen Family • Fluorine is used in rocket fuels. Fluorine is a very reactive element which makes it good for very explosive reactions. • Inside that tube of toothpaste is fluorine. • People put chlorine in the pool to kill bacteria and disease. • The salt on your table is made with chlorine.

38. The Noble Gases • This family has the happiest elements of all. • Why Are They Happy? • All of the noble gases have full outer shells with eight electrons. • Oh Wait!!! helium (He) is at the top with a shell that is full with only two electrons. • The facts that the outer shells are full means they are quite happy and don't need to react with other elements.

39. The Noble Gases • Scientists take neon and pump it into glass tubes. When they plug those tubes into the wall and turn on the electricity the neon glows very brightly. • Neon is also used in lasers. • Argon and krypton are great when it comes to getting lights to glow. Over time, krypton has been used in the fluorescent lights. They are probably buzzing over your head right now. • Because krypton is one of those non-reactive gases, you might find it used in lasers.

40. Transition Metals • There are a lot of elements that are considered transition metals. • The transition metals are21 (Scandium) through 29 (Copper)39 (Yttrium) through 47 (Silver)57 (Lanthanum) through 79 (Gold)89 (Actinium) and all higher numbers.

41. Transition Metals • What Makes Them So Special? • Its all has to do with their shells/orbitals. • They have a lot of electrons and distribute them in different ways. • Transition metals are able to put more than eight electrons in the shell that is one in from the outermost shell.

42. Transition Metals • The transition metals are able to put up to 32 electrons in their second-to-last shell. • Like gold (Au), with an atomic number of 79, has an organization of 2-8-18-32-18-1. • Transition metals can use the two outermost shells/orbitals to bond with other elements.

43. The Lanthanide Family • Sometimes called lanthanides, some say rare-earth metals, and some say inner-transition elements. • The lanthanide family is comprised of fifteen elements starting with lanthanum (La) at atomic number 57 and finishing up with lutetium (Lu) at number 71

44. The Lanthanide Family • The lanthanide series can be found naturally on Earth. • You might find some of these elements in superconductors, glass production, or lasers.

45. The Actinide Family • They are all radioactive and some are not found in nature. • Some of the elements with higher atomic numbers have only been made in labs. • The actinide family is comprised of fifteen elements that start with actinium (Ac) at atomic number 89 and finish up with lawrencium (Lr) at number 103.

46. The Actinide Family • There are special laboratories across the world that specialize in experimenting on elements. • Some of these particle accelerators have pounded atomic particles into elements with lower atomic numbers. • The buildup of additional parts creates short-lived, high atomic number elements.

47. The Actinide Family • You have probably heard of plutonium (Pu), since it was used in atomic bombs. Uranium (U) is also well known for its radioactivity. • They aren't all used to blow up the world. • Some of them help us out every day. You can find americium (Am) is some metal detectors.