The Periodic Table- Topic 5 Homework: 1. Read pages 78-83 in RB & complete # 1-29 on separate paper (read carefully) 2. Complete guide pg 4 (use your periodic table and colored pencils/crayons) Click for song SMP, Periodic Table Notes 2014

Mendeleev’s Periodic Table (1869) 6.1 Searching For an Organizing Principle How did Mendeleev organize his periodic table? The Abbreviated History of the Periodic Table for Regents Chemistry Mendeleev’s Periodic Table (1869) SMP, Periodic Table Notes 2014

A. Dmitri Mendeleev (1869, Russian) I. HISTORY A. Dmitri Mendeleev (1869, Russian) Organized elements by increasing ATOMIC MASS. Elements with similar chemical properties were grouped together. There were some discrepancies. SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 B. Henry Moseley ORGANIZED ELEMENTS BY INCREASING ATOMIC NUMBER. Resolved discrepancies in Mendeleev’s arrangement. The modern periodic table known as The Periodic Law SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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. SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 II. ORGANIZATION OF THE ELEMENTS A. Arrangement of Table 1. Horizontal rows Called PERIODS All elements in the same period have the same number of ENERGY LEVELS in their atomic structure 7 periods/energy levels SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 2. Vertical Columns Called GROUPS OR FAMILIES 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. XCl2 Group 2: Be+2 Cl-1 = Mg+2 Cl-1 = When writing formulas, use the criss-cross rule to cancel out oxidation states BeCl2 MgCl2 SMP, Periodic Table Notes 2014

III. Comparing Metals, Nonmetals & Metalloids Elements on the Periodic Table are divided into three subgroups called METALS, NONMETALS and METALLOIDS (semimetals). Nonmetals on the right Metals on the left Metalloids (touch the staircase) Group 18 are Noble Gases SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Record metallic properties i Increase nonmetallic properties Decrease metallic properties Increase metallic properties SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Table J:  Activity Series**                                                    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 (radius gets smaller) have LOW IONIZATION ENERGY (energy needed to remove electrons) Metallic character INCREASES as ionization energy decreases. have a low electronegativity (attraction for electrons) form POSITIVE IONS (cations) when combining with other atoms FRANCIUM most reactive metal: See Table J SMP, Periodic Table Notes 2014

2. Metal Physical Properties good conductors of heat and electricity due to their mobile valence electrons 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) SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Table J:  Activity Series**                                                    B. NONMETALS- located on the right side of the periodic table (except for Noble gases) Chemical properties tend to GAIN electrons to form negative IONS (anions) resulting in a larger radius have high electron affinities (electronegativity) produce COVALENT bonds by SHARING electrons with other nonmetals FLUORINE most reactive nonmetal: see Table J SMP, Periodic Table Notes 2014

Know this definition & examples 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) Know this definition & examples SMP, Periodic Table Notes 2014

Crystal Structure and Unit Cells 13.3 Crystal Structure and Unit Cells Carbon Allotropes Diamond, graphite, and fullerenes are allotropes of carbon. Classifying Based on the arrangements of their atoms, explain why the properties of fullerenes are closer to those of diamond than of graphite?

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 SMP, Periodic Table Notes 2014

Buckminsterfullerene The 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.

Squares in the Periodic Table In this periodic table, the colors of the boxes are used to classify representative elements and transition elements.

Trends in the Periodic Table Many properties of the elements change in a predictable way as you move through the periodic table – these systematic trends are called periodic trends. (use reference Table S for data comparison) SMP, Periodic Table Notes 2014

IONIZATION ENERGY (IE) Energy needed to remove the most loosely bound electron from a neutral gaseous atom X + energy X+ + e- Atoms with a HIGH ionization energy hold onto electrons MORE EASILY and are less likely to give them up. Atoms with a LOW Ionization Energy hold onto electrons LOOSELY and are more likely to LOSE electrons

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

Trends in Ionization Energy

Trends in Ionization Energy First ionization energy tends to increase from left to right across a period and decrease from top to bottom within a group. Predicting Which element would have the larger first ionization energy—an alkali metal in period 2 or an alkali metal in period 4?

Trends in Ionization Energy

SMP, Periodic Table Notes 2014 Atomic Radii one half of the distance between the nuclei of two atoms of the same element when the atoms are joined. SMP, Periodic Table Notes 2014

AR TREND in a period As you move across left to right on a table, values generally DECREASES Why? THE GREATER THE #PROTONS (atomic #), THE STRONGER THE PULL ON THE E’S BRINGING THEM CLOSER INTO THE NUCLEUS

AR TREND GOING DOWN A GROUP OR FAMILY Atomic radii generally INCREASES from the top of the table to the bottom of the table Why? Due to electron shielding –As you move down, YOU ADD ANOTHER NRG LEVEL INCREASING THE SHIELDING (KERNEL E- BLOCK)

IONIC RADIUS (write on the bottom of your page) A LOSS OR GAIN IN ELECTRONS BY AN ATOM WILL CHANGE THE SIZE OF THE RESULTING ION Metals lose e’s resulting in smaller ionic radius Nonmetals gain e’s resulting in larger ionic radius SMP, Periodic Table Notes 2014

Trends: Relative Sizes of Some Atoms and Ions SMP, Periodic Table Notes 2014

COMPARISON OF METALS TO NONMETALS If you generally compare ionic size for metals and nonmetals, metal ionic sizes are SMALLER and nonmetal ionic sizes are BIGGER. This 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).

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

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

Periodic Trends Summary (use reference Table S for data comparison) Across a period Down a group Ionization energy increases decreases Electronegativity Atomic radii Metallic properties Click on for video clip SMP, Periodic Table Notes 2014

Class/Home work - Trends Class work: Complete guide pg 8: Only collect trend data for groups 1 and 7, and periods 2 and 4 Complete pgs 10-11 in guide Visit my website for on-line practice with the trends and the PT vocabulary Trends Quiz Friday Bring Review books to class tomorrow SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 IV. Classification Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble Gases Click for song SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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) SMP, Periodic Table Notes 2014

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 SMP, Periodic Table Notes 2014

Groups 3-11: Transition Metals multiple positive oxidation states Lose electrons from two outermost energy levels Ions form colored solutions Ex. CuSO4 (due to the Cu 2+ ion) SMP, Periodic Table Notes 2014

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 SMP, Periodic Table Notes 2014

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 O2 and O3 (it is an allotrope) Polonium is radioactive SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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) SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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 SMP, Periodic Table Notes 2014

TODAY: PT Day 1 1. Check HW answers on the side board. Record correct answers in RB & turn in HW. 2. Jigsaw Report to your colored groups and BEGIN your PT teachback. Present (teach) your information to the group FIRST! This NOT a silent lesson – use your “6 inch” voices to teach the other members. Complete the section of notes cooperatively. Ask your questions to ascertain clarity. By Day 2, everyone in the group should have the Teachback WS completed and the follow-upo questions started. Cooperation and diligence is necessary….. I will be watching and listening. SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Today: PT Day 2 Continue with your group teach back then proceed to answer/check questions #46-90. Transfer answers to the sheet provided. Answers to the outline are on my website for YOU to review this evening. Transfer #’s 46-74 to the scantron. On the scantron write Periodic Table Teachback Due Thursday: BOTH the answer sheet, scantron, and each member’s research notes. Group Quiz THURSDAY SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Today: PT Day 3 Transfer #’s 46-74 to the scantron beginning with # 46 on the scantron. Record all group members names in the name section. In the subject area, write PT Teachback. Group quiz – each member should record his/her answers on their own quiz paper. I will collect one random quiz to score. Work together. Transfer quiz responses 1-21 to the same scantron. Submit the following: Answer sheet Scantron (#1-21 and #46-74 recorded) Each member’s research notes. SMP, Periodic Table Notes 2014

TEACHBACK PROJECT REVIEW Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble Gases Click for song SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 video 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 LOWER IONIZATION ENERGIES SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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: Y2O 9. What is the most reactive metal in this group? FRANCIUM SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 video 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 A GREATER IE SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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 ZCl2 Oxide: ZO SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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 SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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 (O2 and O3) 5. What type of element is Polonium? RADIOCATIVE METAL How can you tell it is radioactive? IT’S ATOMIC NUMBER IS GREATER THAN 83 SMP, Periodic Table Notes 2014

TRANSITION ELEMENTS (groups 3B-12) 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 SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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? MgX2 SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 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 ) SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 GROUP 18 The name of this group is called NOBLE GASES. What type of molecules do these gases form? (monatomic or diatomic) MONATOMIC Describe the electron arrangement in the outermost energy level of all these elements. STABLE OCTECT – INERT GAS STRUCTURE Which element has only two electrons? HELIUM Describe the reactivity of the elements in this group. THEY ARE UNREACTIVE (Kr and Xe can be forced to react with F in lab settings) SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 Topic 5 RB ANSWERS #46-90 46) _2_ 47) _1_ 48) _4_ 49) _1_ 50) _1_ 56) _2__ 57) _3__ 58) _3__ 59) _2_ 60) _1__ 66) _1_ 67) _2_ 68) _2_ 69) _4_ 70) _1_ 61) _3_ 62) _3_ 63) _1_ 64) _1_ 65) _3_ 51)_ 2_ 52) _4_ 53)_4_ 54) _3_ 55) _2_ 71) _1_ 72) _3_ 73) _1_ 74) _2_ SMP, Periodic Table Notes 2014

SMP, Periodic Table Notes 2014 79) They both follow the octet rule (8 valence e’s) 80) Bromine: MBr3 Oxygen: M2O3 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) MCl2 88) MgX2 89) X2O SMP, Periodic Table Notes 2014