1. IIIIII 1 The Periodic Table- Topic 5 Click for song Bellwork: Using your RB (pgs 78-83), define the following words in your notebook: family, group, periodic law, period, metal, metalloid, nonmetal

2. Searching For an Organizing Principle Chlorine, bromine, and iodine have very similar chemical properties. 2

3. Mendeleev’s Periodic Table (1869) y How did Mendeleev organize his periodic table? yThe Abbreviated History of the Periodic Table for Regents ChemistryThe Abbreviated History of the Periodic Table for Regents Chemistry 6.1 3

4. Group Work zAll members of the group should be participating ( 1 reader) zUse low voices and work cooperatively zI should hear CHEM Talk!! zLab should be completed by end of the period. zI will be watching and a group grade will be assigned Cooperation and diligence is necessary….. 4

5. 5 A. Dmitri Mendeleev (1869, Russian) z Oz Organized elements by increasing ATOMIC MASS. EElements with similar chemical properties were grouped together. TThere were some discrepancies. I. HISTORY

6. 6 B. Henry Moseley  ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER.  Resolved discrepancies in Mendeleev’s arrangement.

7. The Periodic Law xIn the modern periodic table, elements are arranged in order of increasing atomic number. 6.1 Mendeleev’s original table was according to mass. This was changed when Moseley discovered atomic number. 7

8.  When elements are arranged in order of INCREASING ATOMIC #, elements with similar chemical properties appear at regular intervals.  The properties of the elements within a period change as you move across a period from left to right.  The pattern of properties within a period repeats as you move from one period to the next. 8

9. 9 1. Horizontal rows  Called PERIODS  All elements in the same period have the same number of ENERGY LEVELS in their atomic structure A. Arrangement of Table II. ORGANIZATION OF THE ELEMENTS

10. 10 2. Vertical Columns a)Called GROUPS OR FAMILIES b)All elements in the same group have the same number of VALENCE ELECTRONS, therefore lose or gain the SAME number of electrons, form similar CHEMICAL FORMULAS and have similar CHEMICAL PROPERTIES ex. XCl 2 Group 2: Be +2 Cl -1 = BeCl 2 Mg +2 Cl -1 = MgCl 2 yRemember: When writing formulas, use the criss-cross rule to cancel out oxidation states

11. 11 Elements can be classified by their properties and located on the Periodic Table as metals, nonmetals, metalloids or semimetals Metals on the left Nonmetals on the right Metalloids or semimetals III. Comparing Metals, Nonmetals & Metalloids

12. 12 III. Comparing Metals, Nonmetals & Metalloids Elements on the Periodic Table are divided into three subgroups called METALS, NONMETALS and METALLOIDS (semimetals). Decrease metallic properties Increase metallic properties Increase nonmetallic properties yClick on

13. 13 METALS : located on the LEFT SIDE of the periodic table (except H); MORE THAN 2/3 of all elements 1. Chemical properties  tend to LOSE ELECTRONS EASILY  have LOW IONIZATION ENERGY (energy needed to remove electrons)  Metallic character INCREASES as ionization energy decreases.  have LOW ELECTRON AFFINITY (attraction for electrons)  form POSITIVE IONS when combining with other atoms  FRANCIUM most reactive metal:SeeTableJ

14. 14 2. Metals Physical Properties  good conductors of heat and electricity  LUSTROUS - reflect light, shine when they are polished  MALLEABLE - can be rolled or hammered into sheets  DUCTILE - can be drawn into wires  are SOLIDS at room temperature except for MERCURY (liquid)

15. 15 B. NONMETALS 1.Chemical properties  tend to GAIN electrons to form NEGATIVE IONS  have high electron affinities (electronegativity)  produce COVALENT bonds by SHARING electrons with other nonmetals  FLUORINE most reactive nonmetal: see Table J located on the right side of the periodic table (except for Noble gases)

16. 16 2. Nonmetals Physical Properties  exist as gases, molecular solids, or network solids at room temperature except BROMINE (liquid)  BRITTLE - (shatters when struck)  DULL - does not reflect light even when polished  POOR CONDUCTORS of heat and electricity  Allotropes: Different SHAPE & PROPERTIES forms from the same element. Exist in two or more different forms. Therefore they have different crystalline structures and different physical and chemical properties  CARBON: coal; diamond, graphite  OXYGEN: O2; O3 (OZONE)

17. Crystal Structure and Unit Cells Carbon Allotropes y13.3 17

18. Buckminsterfullerene zThe structure of a buckminsterfullerene is a truncated icosahedron made of 20 hexagons and 12 pentagons, with a carbon atom at the vertices of each polygon and a bond along each polygon edge. To become stable, the carbon atom needs 8 electrons in its outer shell, and covalently bonding with 3 other atoms will only make 7 electrons in its outer shell. This means that the one unbonded electron on every carbon atom is free to float around all of the compound's atoms. Electrons carry charge, so this free electron movement means that the buckminsterfullerene can conduct electricity very well. This, because of its size, makes it very useful in nanotechnology.truncated icosahedron 18

19. C. METALLOIDS (semi-metals)  Found lying on the jagged line between metals and nonmetals flatly touching the line (except Al and Po).  B,Si,Ge,As, Sb, & Te  Exhibit properties of both metals and nonmetals  Behave as nonmetals but their conductivity is like metals  SEMICONDUCTORS – Si and Ge 19

20. Squares in the Periodic Table 20

21. 21  Many properties of the elements change in a predictable way as you move through the periodic table – these systematic trends are called periodic trends.. z(use reference Table S for data comparison) Periodic Trends

22. 22 Reference Table S

23. 23 © 1998 LOGAL 1. Atomic Radius y DESCRIPTION: ½ THE DISTANCE BETWEEN 2 ADJACENT NUCLEI

24. Trends in Atomic Size zThe atomic radius is one half of the distance between the nuclei of two atoms of the same element when the atoms are joined.

25. 25 TREND GOING ACROSS A PERIOD yWhat is the ‘trend’ as you move left to right? ATOMIC RADIUS DECREASES yExplanation: ---THE GREATER THE #PROTONS (NUCLEAR CHARGE), THE STRONGER THE PULL ON THE E’S BRINGING THEM CLOSER INTO THE NUCLEUS THEREFORE ATOMIC RADII DECREASES

26. 26 TREND GOING DOWN A GROUP OR FAMILY zWhat is the ‘trend’ as you move down a group? ATOMIC RADIUS INCREASES yExplanation: ----AS EACH ELEMENT GOES DOWN A GROUP, YOU ADD ANOTHER NRG LEVEL INCREASING THE SHIELDING (KERNEL E- BLOCK THE ATTRACTION BETWEEN THE NUCLEUS AND THE VALENCE E-)

27. Ions xPositive and negative ions form when electrons are transferred between atoms. y6. 3 y11p+ y12 n 27

28. Ions xPositive and negative ions form when electrons are transferred between atoms. y6. 3 28

29. Trends in Ionic Size xRelative Sizes of Some Atoms and Ions 29

30. 30 IONIC RADIUS zDescription: A LOSS OR GAIN IN ELECTRONS BY AN ATOM WILL CHANGE THE SIZE OF THE RESULTING ION Ionic Radii Metals Nonmetals

31. 31 COMPARISON OF METALS TO NONMETALS zIf you generally compare ionic size for metals and nonmetals, metal ionic sizes are SMALLER and nonmetal ionic sizes are BIGGER. zThis is because metals tend to LOSE electrons and form CATIONS (and get smaller) while nonmetals tend to GAIN electrons and form ANIONS (and get larger).

32. 32 zMETALS: TREND GOING ACROSS A PERIOD yTrend: As you move left to right for METALS, ionic size DECREASES yExplanation: METALS LOSE ELECTRONS FROM THEIR OUTERMOST SHELL zMETALS: TREND GOING DOWN A GROUP yTrend: As you move down a group for METALS, ionic size INCREASES yExplanation: AS YOU MOVE DOWN A GROUP, YOU ADD ANOTHER ENERGY LEVEL THEREBY INCREASING THE SIZE DUE TO THE INCREASED # OF ELECTRONS

33. 33 NONMETALS: TREND GOING ACROSS A PERIOD yTrend: As you move left to right for NONMETALS, ionic size decreases. yExplanation: NONMETALS GAIN ELECTRONS WHICH ARE ATTRACTED TO THE PROTONS IN THE NUCLEUS NONMETALS : TREND GOING DOWN A GROUP yTrend: As you move down a group for NONMETALS, ionic size INCREASES. y Explanation: AS YOU MOVE DOWN A GROUP, YOU ADD ANOTHER ENERGY LEVEL THEREBY INCREASING THE SIZE DUE TO THE INCREASED # OF ELECTRONS © 2002 Prentice-Hall, Inc.

34. 34 IONIZATION ENERGY (IE) zDescription: AMOUNT OF ENERGY NEEDED TO REMOVE AN E- FROM AN ATOM. yAtoms with a HIGH ionization energy hold onto electrons MORE EASILY and are less likely to give them up. yAtoms with a LOW Ionization Energy hold onto electrons LOOSELY and are more likely to LOSE electrons

35. Ionization Energy zEnergy needed to remove the most loosely bound electron from a neutral gaseous atom zX + energy X + + e- 35

36. Trends in Ionization Energy 36

37. Trends in Ionization Energy 37

38. 38 TREND GOING ACROSS A PERIOD zWhat is the ‘trend’ as you move left to right? IE INCREASES zExplanation: AS THE #PROTONS (AKA: NUCLEAR CHARGE) INCREASES, THERE IS A GREATER PULL ON THE E’S REQUIRING MORE NRG TO REMOVE THEM TREND GOING DOWN A GROUP OR FAMILY zWhat is the ‘trend’ as you move top to bottom? IE DECREASES zExplanation: Atom size increases making the outermost electron farther away from the nucleus therefore making it easier to remove zShielding increases INCREASES DECREASES

39. Trends in Ionization Energy 39

40. 40 ELECTRONEGATIVITY (EN) zDescription: MEASURE OF AN ATOM’S ABILITY TO ATTRACT ELECTRONS zAtoms with a HIGH Electronegativity have a STRONGER attraction for bonded electrons zAtoms with a LOW Electronegativity have a WEAKER attraction for bonded electrons zBased on a scale of 4, Fluorine has the greatest EN

41. 41 TREND ACROSS A PERIOD zWhat is the ‘trend’ as you move left to right? EN INCREASES zExplanation: THERE ARE MORE PROTONS (INCREASED ATOMIC NUMBER) WHICH INCREASES THE ELECTRONS ATTRACTION TREND GOING DOWN A GROUP OR FAMILY y What is the ‘trend’ as you move top to bottom? EN DECREASES y Explanation: AS YOU GO DOWN A GROUP THERE ARE MORE ELECTRONS AND MORE NRG LEVELS SO THE ATTRACTION GETS WEAKER

42. 42 Periodic Trends Summary (use reference Table S for data comparison) Trend Across a period Down a group Ionization energyincreasesdecreases Electronegativityincreasesdecreases Atomic radiidecreasesincreases Metallic propertiesdecreasesincreases yClick on for video clipClick on for video clip

43. 43 IV. Classification  Alkali Metals  Alkaline Earth Metals  Transition Metals  Halogens  Noble Gases Click for song

44. 44 Group 1: Alkali Metals  extremely reactive (not found free in nature)  form stable ionic compounds  react with water to form a base  react with air to form oxides  react with acids to form salts Click on for video clip (2:56 min)

45. 45 Group 2: Alkaline Earth Metals  reactive (not found free in nature) - form stable ionic compounds  react with water to form a base  react with air to form oxides  react with acids to form salts Click on for video clip

46. 46 Groups 3-11: Transition Metals  multiple positive oxidation states  Lose electrons from two outermost energy levels  Ions form colored solutions  Ex. CuSO 4 (due to the Cu 2+ ion)

47. 47 Group 15 – unique features  Members range from typical nonmetals (nitrogen and phosphorus) through metalloids (arsenic and antimony) to metals (bismuth)  Nitrogen  Forms stable diatomic molecules with a triple bond  Component of protein  Forms some unstable compounds that are used as explosives  Phosphorus  Component of nucleic acids (DNA, RNA)  More reactive than nitrogen at room temperature

48. 48 Group 16 – unique Features  Members range from typical nonmetals (oxygen and sulfur) through metalloids (selenium and tellurium) to metals (polonium)  Solids except oxygen  Oxygen can exist as O 2 and O 3 (it is an allotrope)  Polonium is radioactive

49. 49 Group 17: Halogens  very reactive nonmetals - high electronegativity  not found free in nature  form diatomic molecules when free  react with metals to form salts (halides)  Found in all three phases (s, l, g) due to differences in Van der Waals forces (these are weak)

50. 50 Group 18: Noble Gases  Have complete outer shells  Almost inert (not reactive); stable  Krypton, xenon, and radon form compounds with oxygen and fluorine  Referred to as monatomic gases

51. 51 TODAY…….. 1. Using a pencil, transfer your RB answers to your scantron form –  In the green box, write “RB Topic 5 #1-45”.  Turn in BOTH the scantron and your written work.

52. 52 2. Assemble into NEW groups according to the number on your card from yesterday (refer to your sheet). Take your notes and 5 questions with you. Using your notes, discuss & complete the Teachback WS questions pertaining to your group.  Use the post-it notes for any questions you may have THAT MAY NEED ANSWERING  Folks who did the Noble gases will need to meet briefly for a few moments.

53. 53 3. Return BACK to your original groups and BEGIN your teachback. This NOT a silent lesson – use your “6 inch” voices to teach the other members. Ask your questions to ascertain clarity. At the end of this session, everyone in the group should have the Teachback WS completed.  Use the post-it notes for any questions you may have THAT NEED ANSWERING..  Once finished, begin RB questions 46-90. Cooperation and diligence is necessary….. I will be watching and listening.

54. 54 TEACHBACK PROJECT REVIEW  Alkali Metals  Alkaline Earth Metals  Transition Metals  Halogens  Noble Gases Click for song

55. 55 GROUP 1 1. The name of this group is ALKALI METALS 2. Does this group contain metals or nonmetals? METALS 3. Alkali metals (lose or gain)l LOSE electrons becoming (positive or negative) ions? POSITIVE 4. Describe the reactivity of the elements in this group as the atomic number increases. INCREASES 5. Are they (more or less) MORE reactive than all of the elements in Group 2 and why? THEY HAVE LOW IONIZATION ENERGIES video

56. 56 Group 1 continued: 6. Can these compounds be found in nature in the elemental or combined state? COMBINED STATE IN THE FORM OF A SALT 7. What type of compounds do they normally form (ionic or covalent)? IONIC (M + NM) 8. If element Y represents an alkali metal, what is it’s general formula for the reaction with a: Chloride: YCl Oxide: Y 2 O 9. What is the most reactive metal in this group? FRANCIUM

57. 57 GROUP 2 1. The name of this group is ALKALINE EARTH METALS. 2. Does this group contain metals or nonmetals? METALS 3. They (lose or gain) LOSE electrons & form (positive or negative) ions POSITIVE ? 4. Describe the reactivity of the elements in this group as the atomic number increases (increases or decreases) INCREASES 5. Are they (more or less) LESS reactive than all of the elements in Group 1 and why? THEY HAVE GREATER IE video

58. 58 Group 2 continued: 6. Can these compounds be found in nature in the elemental or combined state? COMBINED STATE IN THE FORM OF A SALT 7. What type of compounds do they normally form (ionic or covalent)? IONIC (M + NM) 8. If element Z represents an alkaline earth metal, what is it’s general formula for the reaction with a: Chloride ZCl 2 Oxide: ZO

59. 59 GROUP 15 1. What is this group referred to as? NITROGEN GROUP 2. Name the diatomic element in this group? NITROGEN 3. Classify each element in this group as a metal, non-metal or semi- metal (metalloid). metals: ANTIMONY, BISMUTH nonmetals: NITROGEN, PHOSPHORUS semi-metal: ARSENIC 4. Explain what happens to the reactivity of a non-metal as the atomic number increases. DECREASES. 5. Which is the most reactive non-metal in this group? PHOSPHORUS 6. Is nitrogen a (diatomic or monatomic) DIATOMIC molecule & what type of bond is found in nitrogen? TRIPLE COVALENT

60. 60 GROUP 16 1. Classify each element in this group as a metal, non-metal or semi-metal. metals: POLONIUM nonmetals: OXYGEN, SULFUR, SELENIUM semi-metal: TELLERIUM 2. Name the diatomic element in this group. OXYGEN 3. Define an allotrope? DIFFERENT FORMS OF AN ELEMENT IN THE SAME PHASE WITH HAVING DIFF CHEM & PHYSICAL PROPERTIES 4. Which element(s) in this group is an allotrope? SULFUR, OXYGEN (O 2 and O 3 ) 5. What type of element is Polonium? RADIOCATIVE METAL How can you tell it is radioactive? IT’S ATOMIC NUMBER IS GREATER THAN 83

61. 61 TRANSITION ELEMENTS (groups 3B-12) 1.Which element is a liquid at room temperature? 1.Which element is a liquid at room temperature? MERCURY (Hg) 2. What are the four main characteristic chemical properties of transition elements?  MULTIPLE POSITIVE OXIDATION STATES  IONS FORM COLORED SOLUTIONS  LOSE ELECTRONS FROM TWO OUTERMOST ENERGY LEVELS  UNFILLED D ORBITALS

62. 62 GROUP 17 1. The name of this group is HALOGENS 2. Name and classify the elements in this group: METALS: At NONMETALS F, Cl, Br, I 3. Halogens (lose or gain) GAIN electrons becoming (positive or negative) ions? NEGATIVE 4. Why is astatine not included much in these discussions? NOT ENOUGH AVAILABLE TO STUDY 5. What would the general formula of a Group 17 element (represented by X) combined with magnesium of group 2? MgX 2

63. 63 6. What is the most reactive element in this group? FLUORINE 7. Can these compounds be found in nature in the elemental or combined state? COMBINED STATE AS SALTS 8. What type of salts do these elements form? HALIDES 9. For each state of matter, list the element(s) in this group. solid: IODINE liquid: BROMINE gas: CHLORINE, FLUORINE 10. What type of forces of attractions account for the different states of matter that exist and the high MP’s and BP’s as you go down the group? VAN DER WAALS FORCES (weak forces that get stronger as you go down the group )

64. 64 GROUP 18 zThe name of this group is called NOBLE GASES. zWhat type of molecules do these gases form? (monatomic or diatomic) MONATOMIC zDescribe the electron arrangement in the outermost energy level of all these elements. STABLE OCTECT – INERT GAS STRUCTURE zWhich element has only two electrons? HELIUM zDescribe the reactivity of the elements in this group. THEY ARE UNREACTIVE (Kr and Xe can be forced to react with F in lab settings)

65. 65 Topic 5 RB ANSWERS #43-90 71) _1_ 72) _3_ 73) _1_ 74) _2_ 56) _2__ 57) _3__ 58) _3__ 59) _2_ 60) _1__ 46) _2_ 47) _1_ 48) _4_ 49) _1_ 50) _1_ 51)_ 2_ 52) _4_ 53)_4_ 54) _3_ 55) _2_ 61) _3_ 62) _3_ 63) _1_ 64) _1_ 65) _3_ 66) _1_ 67) _2_ 68) _2_ 69) _4_ 70) _1_ 43) 4 44) 2 45) 1

66. 66 79) They both follow the octet rule (8 valence e’s) 81) Hydrogen is a NM & doesn't have the characteristics of other group 1 members other than one valence e 82) LARGEST: aluminum SMALLEST: carbon HIGHEST IE: carbon LOWEST IE: aluminum 83) Same number of valence e’s 84) Metals have fewer valence e’s. As you move to the right of the PT, there are more val e’s. Once the orbitals are full, a noble gas configuration is met (8 val e’s) 85) Metals become positive ions 87) MCl 2 88) MgX 2 89) X 2 O