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: 1.I can recognize that all matter is made of atoms. 2.I can identify the parts of an atom. 3.I can identify the charge and location of each particle in an atom. 4.Explain how an atom can be neutral and how the atom can become charged.

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

4. Dalton’s Atomic Theory John Dalton – British chemist and schoolteacher ▫Published his theory in 1803 1.All substances are made of atoms. Atoms are small particles that cannot be created, divided, or destroyed. 2.Atoms of the same element are exactly alike and atoms of different elements are different. 3.Atoms join with other atoms to make new substances. I can recognize that all matter is made of atoms.

5. 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 I can recognize that all matter is made of atoms. I can identify the charge and location of electrons in an atom.

6. 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 I can recognize that all matter is made of atoms. I can identify the parts of an atom.

7. 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. I can recognize that all matter is made of atoms. I can identify the particles that make up an atom.

8. 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 I can recognize that all matter is made of atoms. I can identify the location of each particle in an atom.

9. Modern Atomic Theory (20 th century) Schrodinger, Heisenberg Electron clouds-regions electrons likely found Bohr (1913) Energy levels-paths in which electrons travel Rutherford (1911) Nucleus-central region of atom that has positive charge Thomson (1897) Discovered electrons-negative particlePlum-pudding model Dalton (1803) All substances made of atomsAtoms can join to make new substances Democritus Atom – smallest particle that cannot be divided 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: 1.I can recognize that all matter is made of atoms. 2.I can identify the parts of an atom. 3.I can identify the charge and location of each particle in an atom. 4.Explain how an atom can be neutral and how the atom can become charged. 5.Explain how gravity is affected by the mass of an object and the distance between objects.

11. The Atom Extremely small ▫One penny contains 2 x 10 22 atoms ▫One Al atom has a diameter of 0.00000003 cm ▫Al foil is 50,000 atoms thick I can recognize that all matter is made of atoms.

12. The Atom Nucleus – small, dense, positively charged center of the atom ▫Contains most of the atom’s mass 1.Protons (p+)– positively charged particle in the nucleus  Mass of one proton is 1.7 x 10 -24 g = 1 amu (atomic mass unit) 2.Neutrons (n 0 )– 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 I can identify the parts of an atom. I can identify the charge and location of each particle in an atom.

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. 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 Explain how an atom can be neutral and how the atom can become charged.

16. Forces in Atoms 1.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 I can explain how gravity is affected by the mass of an object and the distance between objects.

17. Forces in Atoms 2.Electromagnetic Force ▫Same charge repels ▫Opposite charges attract ▫Protons and electrons attract ▫Holds electrons around the nucleus I can explain how gravity is affected by the mass of an object and the distance between objects.

18. Forces in Atoms 3.Strong force ▫Holds protons together in the nucleus ▫Greater than EM force I can explain how gravity is affected by the mass of an object and the distance between objects.

19. Forces in Atoms 4.Weak force ▫Found in radioactive elements (unstable atoms that spontaneously fall apart over time) ▫Allows a neutron to change into a proton or electron I can explain how gravity is affected by the mass of an object and the distance between objects.

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: 1.Identify the parts of an atom. 2.Identify the charge and location of each particle in an atom. 3.Identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

21. Building Atoms 1.Determine atomic number for the element ▫Top number on periodic table  Number of protons and electrons for that element 2.Determine atomic mass for the element ▫Bottom number (rounded) on periodic table 3.Subtract atomic # from atomic mass ▫Number of neutrons 4.Draw the atom with the correct number of protons and neutrons in the nucleus 5.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 I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

22. Carbon 1.Atomic number = 6 ▫# of protons = # of electrons = 6 2.Atomic mass = 12.01 =12 3.Atomic mass – atomic # = # of neutrons ▫12 – 6 = 6 neutrons I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

23. Aluminum 1.Atomic number = 13 ▫# of protons = # of electrons = 13 2.Atomic mass = 26.98154 =27 ▫Atomic mass – atomic # = # of neutrons 3.27 – 13 = 14 neutrons I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

24. 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 2,670 known isotopes 38 isotopes of tin I can identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

25. Naming Isotopes 1.Write the name of the element 2.Followed by a hyphen (-) 3.Followed by the mass # of the isotope Hydrogen-1 Lithium-5 Cobalt-60 Gallium-71 I c an identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

26. Boron Boron-10Boron-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 I c an identify the atomic number, atomic mass, number of protons, neutrons, and electrons in an atom using the periodic table.

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: 1.Explain how the periodic table was first arranged and how it is arranged today. 2.Identify each element as a metal, nonmetal, or metalloid using the zigzag line as a reference. 3.Identify an element by its chemical symbol. 4.Identify the groups and periods of the periodic table. 5.Describe how chemical properties of elements are similar in the same group. 6.Label each group by name (ex: alkali metals, halogens, noble gases, etc.) 7.Identify similar properties for each group. 8.Explain which groups are likely to react together.

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

30. Germanium Mendeleev’s prediction Actual Properties Atomic mass7072.6 Density5.55.3 AppearanceDark gray metalGray metal Melting PointHigh melting point 937 ◦C I can explain how the periodic table was first arranged and how it is arranged today.

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

33. Decoding the Periodic Table 1.Metals, Nonmetals, Metalloids a.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 b.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 c.Metalloids  Along zigzag line  Half of a complete set of electrons in outer energy level  Semiconductors  Properties of both metals and nonmetals I can identify each element as a metal, nonmetal, or metalloid using the zigzag line as a reference.

35. Decoding the Periodic Table 2.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 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. Decoding the Periodic Table 3.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 4.Groups (Family) ▫Vertical columns of elements (top to bottom) ▫Similar chemical and physical properties ▫Eighteen groups I can identify the groups and periods of the periodic table.

39. Reading the Periodic Table 1.What information is given in each square on the periodic table? ▫AN, AM, symbol, name, state, protons, electrons 2.How many elements are liquid at RT? Which ones? ▫2▫2 ▫Hg, Br 3.How many are gas at RT? ▫11 4.How many are metals? ▫88 5.How many are nonmetals? ▫18 6.How many are metalloids? ▫6▫6 7.How many groups? ▫18 8.How many periods? ▫7▫7 9.List elements whose symbols do not seem to come from their English names? ▫Sn, Hg, Pb, Sb, W, K, Na 10.What elements are in the same group as oxygen? ▫S, Se, Te, Po

40. 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 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

41. Group 1: Alkali Metals All metals 1 electron in outer energy level Very reactive Soft Silver Shiny Low density 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

42. 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 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

43. 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) 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

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. LanthanidesActinides Period 6 Shiny reactive Period 7 Radioactive Elements after 94 (plutonium) are made in laboratories 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

46. 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 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

47. Group 14: Carbon Group 2 metals, one nonmetal, two metalloids 4 electrons in OEL Solids at RT 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

48. Group 15: Nitrogen Group 1 metals, 2 metalloids, 2 nonmetals 5 electrons in OEL Solids at RT Nitrogen makes up to 80% of air 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

49. 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 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

50. 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 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

51. Group 18: Noble Gases Nonmetals 8 electrons in OEL (except helium which has 2) Complete set of electrons in OEL Unreactive Colorless, odorless gases at RT 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

52. Hydrogen 1 electron in OEL Reactive Colorless, odorless gas Low density Explosive reactions with oxygen Most abundant element in the universe 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