1. IIIIII SMB, Periodic Table Notes 20111 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. 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. SMB, Periodic Table Notes 20113 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

4. SMB, Periodic Table Notes 20114 B. Henry Moseley  ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER.  Resolved discrepancies in Mendeleev’s arrangement.

5. 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.

6.  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.

7. SMB, Periodic Table Notes 20117 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

8. SMB, Periodic Table Notes 20118 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

9. SMB, Periodic Table Notes 20119 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

10. SMB, Periodic Table Notes 201110 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

11. SMB, Periodic Table Notes 201111 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: See Table J http://castlelearning.com/review/reference/chem%20table%20j.htm http://castlelearning.com/review/reference/chem%20table%20j.htm

12. SMB, Periodic Table Notes 201112 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)

13. SMB, Periodic Table Notes 201113 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)

14. SMB, Periodic Table Notes 201114 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.  CARBON: coal; diamond, graphite  OXYGEN: O2; O3 (OZONE)

15. 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

16. SMB, Periodic Table Notes 201116  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

17. SMB, Periodic Table Notes 201117 Reference Table S

18. SMB, Periodic Table Notes 201118 © 1998 LOGAL 1. Atomic Radius y DESCRIPTION: ½ THE DISTANCE BETWEEN 2 ADJACENT NUCLEI

19. SMB, Periodic Table Notes 201119 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 (SHIELDING)

20. SMB, Periodic Table Notes 201120 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

21. SMB, Periodic Table Notes 201121 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).

22. SMB, Periodic Table Notes 201122 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

23. SMB, Periodic Table Notes 201123 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

24. SMB, Periodic Table Notes 201124 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

25. SMB, Periodic Table Notes 201125 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

26. SMB, Periodic Table Notes 201126 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

27. SMB, Periodic Table Notes 201127 IV. Classification  Alkali Metals  Alkaline Earth Metals  Transition Metals  Halogens  Noble Gases Click for song

28. SMB, Periodic Table Notes 201128 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)

29. SMB, Periodic Table Notes 201129 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

30. SMB, Periodic Table Notes 201130 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)

31. SMB, Periodic Table Notes 201131 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

32. SMB, Periodic Table Notes 201132 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

33. SMB, Periodic Table Notes 201133 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)

34. SMB, Periodic Table Notes 201134 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

35. SMB, Periodic Table Notes 201135 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.

36. SMB, Periodic Table Notes 201136 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.

37. SMB, Periodic Table Notes 201137 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.

38. SMB, Periodic Table Notes 201138 TEACHBACK PROJECT REVIEW  Alkali Metals  Alkaline Earth Metals  Transition Metals  Halogens  Noble Gases Click for song

39. SMB, Periodic Table Notes 201139 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

40. SMB, Periodic Table Notes 201140 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

41. SMB, Periodic Table Notes 201141 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) DECREASES 5. Are they (more or less) LESS reactive than all of the elements in Group 1 and why? THEY HAVE GREATER IE video

42. SMB, Periodic Table Notes 201142 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

43. SMB, Periodic Table Notes 201143 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

44. SMB, Periodic Table Notes 201144 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

45. SMB, Periodic Table Notes 201145 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

46. SMB, Periodic Table Notes 201146 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

47. SMB, Periodic Table Notes 201147 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 )

48. SMB, Periodic Table Notes 201148 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)

49. SMB, Periodic Table Notes 201149 Topic 5 RB ANSWERS #46-90 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_

50. SMB, Periodic Table Notes 201150 79) They both follow the octet rule (8 valence e’s) 80) Bromine: MBr 3 Oxygen: M 2 O 3 Why? Group 13 has 3 valence e’s and will form a 3+ charge 81) Hydrogen is a NM & doens’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