The Atom and the Periodic Table

1. The Atom and the Periodic Table Chapter 10 and Chapter 11

2. Objectives • SPI 0807.9.1 Recognize that all matter consists of atoms • I can: • I can recognize that all matter is made of atoms. • I can identify the parts of an atom. • I can identify the charge and location of each particle in an atom. • Explain how an atom can be neutral and how the atom can become charged.

3. I can recognize that all matter is made of atoms. History of Atomic Theory • Democritus – Greek philosopher 400 BCE • Thought you could eventually end up with a particle that could not be cut in half – he called this particle an atom. • From Greek word “atomos” meaning “not able to be divided” • Most people did not believe this to be true including Aristotle. • Did not perform experiments to prove theory, it was just an idea • Democritus was right: matter is made of particles called atoms – the smallest particle into which an element can be divided and still be the same substance

4. I can recognize that all matter is made of atoms. Dalton’s Atomic Theory • John Dalton – British chemist and schoolteacher • Published his theory in 1803 • All substances are made of atoms. Atoms are small particles that cannot be created, divided, or destroyed. • Atoms of the same element are exactly alike and atoms of different elements are different. • Atoms join with other atoms to make new substances.

5. I can recognize that all matter is made of atoms. I can identify the charge and location of electrons in an atom. Thomson’s Discovery of Electrons • J. J. Thomson(1897) – British scientist (awarded Nobel Prize in 1906) • Proved Dalton’s theory had a mistake: atoms can be divided into smaller parts. • Discovered electrons (e-) – subatomic particle that has a negative charge • Plum-pudding model • Electrons were mixed throughout an atom

6. I can recognize that all matter is made of atoms. I can identify the parts of an atom. Rutherford’s Theory • Ernest Rutherford (1911)– student of Thomson (awarded Nobel Prize in 1908) • Proposed that the center of the atom is the nucleus – tiny, extremely dense positively charged part of the atom

7. I can recognize that all matter is made of atoms. I can identify the particles that make up an atom. Bohr’s Model • Niels Bohr (1913) – Danish scientist, worked with Rutherford (awarded Nobel Prize in 1922) • Proposed that electrons move around the nucleus in certain paths or energy levels. • Electrons can jump from one level to another level but do not occupy the space between the energy levels.

8. I can recognize that all matter is made of atoms. I can identify the location of each particle in an atom. The Modern Atomic Theory • Erwin Schrodinger – Austrian physicist (awarded Nobel Prize in 1933) • Werner Heisenberg – German physicist (awarded Nobel Prize in 1932) • Electrons travel in regions around the nucleus of an atom where they are likely to be found called electron clouds

9. I can recognize that all matter is made of atoms.

10. Objectives • SPI 0807.9.1 Recognize that all matter consists of atoms. • SPI 0807.12.5 Determine the relationship among the mass of objects, the distance between these objects, and the amount of gravitational attraction. • I can: • I can recognize that all matter is made of atoms. • I can identify the parts of an atom. • I can identify the charge and location of each particle in an atom. • Explain how an atom can be neutral and how the atom can become charged. • Explain how gravity is affected by the mass of an object and the distance between objects.

11. I can recognize that all matter is made of atoms. The Atom • Extremely small • One penny contains 2 x 1022 atoms • One Al atom has a diameter of 0.00000003 cm • Al foil is 50,000 atoms thick

12. I can identify the parts of an atom. I can identify the charge and location of each particle in an atom. The Atom • Nucleus – small, dense, positively charged center of the atom • Contains most of the atom’s mass • Protons (p+)– positively charged particle in the nucleus • Mass of one proton is 1.7 x 10-24 g = 1 amu (atomic mass unit) • Neutrons (n0)– particles in the nucleus that has no charge. • Mass = 1 amu • Electrons – negatively charged particles of an atom • Found outside the nucleus in electron clouds • Mass of one electron is almost zero • 1,800 electrons = mass of 1 proton

13. I can identify the parts of an atom. I can identify the charge and location of each particle in an atom.

14. I can identify the parts of an atom. I can identify the charge and location of each particle in an atom.

15. Explain how an atom can be neutral and how the atom can become charged. The Atom • # of protons = #of electrons • The charges cancel out, so the atom has an overall neutral charge • If protons ≠ electrons, then the atom becomes charged • Ion – charged particle • Lose electron → lose negative → positive ion • Gain electron → gain negative → negative ion

16. I can explain how gravity is affected by the mass of an object and the distance between objects. Forces in Atoms • Gravitational forces • Acts on all objects all the time • Pulls objects toward one another • Depends on mass and distance between particles • Greater mass has greater gravitational pull • Closer distance has greater gravitational pull • Very small in atoms

17. I can explain how gravity is affected by the mass of an object and the distance between objects. Forces in Atoms • Electromagnetic Force • Same charge repels • Opposite charges attract • Protons and electrons attract • Holds electrons around the nucleus

18. I can explain how gravity is affected by the mass of an object and the distance between objects. Forces in Atoms • Strong force • Holds protons together in the nucleus • Greater than EM force

19. I can explain how gravity is affected by the mass of an object and the distance between objects. Forces in Atoms • Weak force • Found in radioactive elements (unstable atoms that spontaneously fall apart over time) • Allows a neutron to change into a proton or electron

20. Objectives • SPI 0807.9.1 Recognize that all matter consists of atoms. • SPI 0807.9.9 Use the periodic table to determine the properties of an element. • I can: • Identify the parts of an atom. • Identify the charge and location of each particle in an atom. • Identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

21. I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. Building Atoms • Determine atomic number for the element • Top number on periodic table • Number of protons and electrons for that element • Determine atomic mass for the element • Bottom number (rounded) on periodic table • Subtract atomic # from atomic mass • Number of neutrons • Draw the atom with the correct number of protons and neutrons in the nucleus • Place electrons in electron clouds around the nucleus • Only 2 electrons go in the first energy level, only 8 in the second, 18 in the third, 32 in the fourth, 50 in the fifth, 72 in the sixth

22. I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. Carbon • Atomic number = 6 • # of protons = # of electrons = 6 • Atomic mass = 12.01 =12 • Atomic mass – atomic # = # of neutrons • 12 – 6 = 6 neutrons

23. I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. Aluminum • Atomic number = 13 • # of protons = # of electrons = 13 • Atomic mass = 26.98154 =27 • Atomic mass – atomic # = # of neutrons • 27 – 13 = 14 neutrons

24. I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. 2,670 known isotopes 38 isotopes of tin Isotopes • Atoms that have a different number of neutrons, but the same number of protons • Isotopes are still the same element, because they have the same number of protons • The number of protons determine which element you have • If you change the # of protons, then the element changes • Isotopes have the same chemical properties and most physical properties

25. I c an identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. Naming Isotopes • Write the name of the element • Followed by a hyphen (-) • Followed by the mass # of the isotope • Hydrogen-1 • Lithium-5 • Cobalt-60 • Gallium-71

26. I c an identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table. Boron Boron-10 Boron-11 • Atomic # = 5 • #of protons =# of electrons = 5 • Mass number = 10 • Mass # - atomic # = # neutrons • 10-5 = 5 neutrons • Atomic # = 5 • #of protons =# of electrons = 5 • Mass number = 11 • Mass # - atomic # = # neutrons • 11-5 = 6 neutrons

27. The Periodic Table Chapter 11

28. Objectives • SPI 0807.9.9 Use the periodic table to determine the properties of an element. • I can: • Explain how the periodic table was first arranged and how it is arranged today. • Identify each element as a metal, nonmetal, or metalloid using the zigzag line as a reference. • Identify an element by its chemical symbol. • Identify the groups and periods of the periodic table. • Describe how chemical properties of elements are similar in the same group. • Label each group by name (ex: alkali metals, halogens, noble gases, etc.) • Identify similar properties for each group. • Explain which groups are likely to react together .

29. I can explain how the periodic table was first arranged and how it is arranged today. The Pattern • Dmitri Mendeleev, Russian chemist • Discovered pattern in 1896 (63 elements has been discovered by this time) • Wrote the names and properties of each element on cards and arranged the cards by properties, density, appearance, and melting point – no pattern • Arranged by increasing atomic mass – pattern appeared • Pattern was periodic – repeats at regular intervals • Mendeleev named his table the Periodic Table of elements • Mendeleev predicted properties of missing elements not yet found

30. I can explain how the periodic table was first arranged and how it is arranged today. Germanium

31. I can explain how the periodic table was first arranged and how it is arranged today. Changing the Arrangement • Henry Moseley, British scientist • 1914 - Determined the atomic number for each element • Rearranged the PT by increasing atomic number • All elements follow periodic law – the repeating chemical and physical properties of elements change periodically with the elements’ atomic numbers

32. I can explain how the periodic table was first arranged and how it is arranged today.

33. I can identify each element as a metal, nonmetal, or metalloid using the zigzag line as a reference. Decoding the Periodic Table • Metals, Nonmetals, Metalloids • Metals • Left of zigzag line • Few electrons in outer energy level • Most are solid at RT • Shiny, malleable, ductile, good conductors of heat and electricity • Nonmetals • Right of zigzag line • Almost complete set of electrons in outer energy level • Noble gases (group 18) have complete set of electrons • Most are gases at RT • Not shiny, not malleable, not ductile, poor conductors, brittle • Metalloids • Along zigzag line • Half of a complete set of electrons in outer energy level • Semiconductors • Properties of both metals and nonmetals

34. I can identify each element as a metal, nonmetal, or metalloid using the zigzag line as a reference.

35. I can identify an element by its chemical symbol. Decoding the Periodic Table • Chemical Symbol • Names come from scientists, places • Mendelevium, californium • Symbols are the same worldwide • Consists of one or two letters • First letter is ALWAYS capitalized • Second letter is ALWAYS lowercase • Newer elements have 3 letters

36. I can identify an element by its chemical symbol.

37. I can recognize that all matter is made of atoms. I can identify an element by its chemical symbol.

38. I can identify the groups and periods of the periodic table. Decoding the Periodic Table • Periods • Horizontal rows of elements (left to right) • Follow periodic pattern across a period • Becomes less metallic as you go to the right on the PT • Seven periods • Groups (Family) • Vertical columns of elements (top to bottom) • Similar chemical and physical properties • Eighteen groups

39. Reading the Periodic Table • What information is given in each square on the periodic table? • AN, AM, symbol, name, state, protons, electrons • How many elements are liquid at RT? Which ones? • 2 • Hg, Br • How many are gas at RT? • 11 • How many are metals? • 88 • How many are nonmetals? • 18 • How many are metalloids? • 6 • How many groups? • 18 • How many periods? • 7 • List elements whose symbols do not seem to come from their English names? • Sn, Hg, Pb, Sb, W, K, Na • What elements are in the same group as oxygen? • S, Se, Te, Po

40. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Grouping the Elements • Properties are similar in groups • Atoms in each group have the same number of electrons in their outer energy level • Atoms will gain, lose, or share electrons with other atoms to obtain a complete set of electrons in their outer energy level • These atoms will form compounds

41. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 1: Alkali Metals • All metals • 1 electron in outer energy level • Very reactive • Soft • Silver • Shiny • Low density

42. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 2: Alkaline-Earth Metals • Metals • 2 electrons in outer energy level • Very reactive but less than alkali metals • Silver • Low density but higher than alkali metals

43. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Groups 3-12: Transition Metals • Metals • 1 or 2 electrons in outer energy level • Less reactive than alkaline-earth metals • Shiny • Good conductors of thermal energy and electric current • Higher densities and melting points than elements in groups 1 and 2 (except mercury)

44. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together

45. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Lanthanides Actinides • Period 6 • Shiny • reactive • Period 7 • Radioactive • Elements after 94 (plutonium) are made in laboratories

46. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 13: Boron Group • One metalloid, 4 metals • 3 electrons in OEL • Reactive • Solids at room temperature • Aluminum (Al) is the most abundant element on Earth

47. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 14: Carbon Group • 2 metals, one nonmetal, two metalloids • 4 electrons in OEL • Solids at RT

48. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 15: Nitrogen Group • 1 metals, 2 metalloids, 2 nonmetals • 5 electrons in OEL • Solids at RT • Nitrogen makes up to 80% of air

49. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 16: Oxygen Group • 1 metal, 1 metalloid, 3 nonmetals • 6 electrons in OEL • All solids except oxygen (gas) • Reactive • Oxygen makes up about 20% of air

50. I can describe how chemical properties of elements are similar in the same group. I can label each group by name (ex: alkali metals, halogens, noble gases, etc.) I can identify similar properties for each group. I can explain which groups are likely to react together Group 17: Halogens • Nonmetals • 7 electrons in OEL (only need to gain 1 electron for complete outer level) • Very reactive • Poor conductors of electric current • React with alkali metals (group 1) to form salts