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Bell Work

Bell Work. Pretend you work for Jeopardy ! Come up with a category W rite three questions Assign each question a value ( e.g . 100, 200 and 300 ) Briefly explain the reasoning for your category , questions and values. The Periodic Table. Unit 2.

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Bell Work

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  1. Bell Work Pretendyouwork for Jeopardy! • Come up witha category • Writethreequestions • Assigneach question a value (e.g. 100, 200 and 300) • Brieflyexplain the reasoning for yourcategory, questions and values

  2. The Periodic Table Unit 2

  3. Write these down! We’ll answer with the following video… • What scientists contributed to the periodic table we have today? • How did Dimitri Mendeleev organize the periodic table?

  4. The Current Periodic Table • Mendeleev wasn’t too far off. • Now the elements are put in rows by increasing ATOMIC NUMBER!! • The horizontal rows are called periods and are labeled from 1 to 7. • The vertical columns are called groups are labeled from 1 to 18.

  5. Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! • (Mendeleev did that on purpose.) • Why?? • They have the same number of valence electrons. • They will form the same kinds of ions.

  6. Metals, Non-Metals & Metalloids Metals Metalloids Non-metals

  7. Families on the Periodic Table • Columns are also grouped into families. • Families may be one column, or several columns put together. • Families have names rather than numbers. (Just like your family has a common last name.)

  8. Hydrogen • Hydrogen belongs to a family of its own. • Hydrogen is a diatomic, reactive gas. • Hydrogen was involved in the explosion of the Hindenberg. • Hydrogen is promising as an alternative fuel source for automobiles

  9. Alkali Metals • 1st column on the periodic table (Group 1/IA) not including hydrogen. • Very reactive metals, always combined with something else in nature (like in salt). • Soft enough to cut with a butter knife

  10. Alkaline Earth Metals • Second column on the periodic table. (Group 2/IIA) • Reactive metals that are always combined with nonmetals in nature. • Several of these elements are important mineral nutrients (such as Mg and Ca

  11. Transition Metals • Elements in groups 3-12 (group B elements) • Less reactive harder metals • Includes metals used in jewelry, coins and construction. • Metals used “as metal.”

  12. Boron Family • Elements in group 13 (IIIA) • Aluminum metal was once rare and expensive, not a “disposable metal.”

  13. Carbon Family • Elements in group 14 (IVA) • Contains elements important to life and computers. • Carbon is the basis for an entire branch of chemistry (organic). • Silicon and Germanium are important semiconductors.

  14. Nitrogen Family • Elements in group 15 (VA) • Nitrogen makes up over ¾ of the atmosphere. • Nitrogen and phosphorus are both important in living things. • Most of the world’s nitrogen is not available to living things. • The red stuff on the tip of matches is phosphorus.

  15. Oxygen Family or Chalcogens • Elements in group 16 (VIA) • Oxygen is necessary for respiration. • Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

  16. Halogens • Elements in group 17 (VIIA) • Very reactive, volatile, diatomic, nonmetals • Always found combined with another element in nature . • Used as disinfectants and to strengthen teeth.

  17. The Noble Gases

  18. The Noble Gases • Elements in group 18 (VIIIA) • VERY unreactive, monatomic gases • Used in lighted “neon” signs • Used in blimps to fix the Hindenberg problem. • Have a full valence shell.

  19. Inner Transition Elements • Pulled “out” of the periodic table • Uranium is part of `these which is used in nuclear reactions. • MOST are: • radioactive • synthetically made

  20. Write these down! We’ll answer with the following video… • What are isotopes? • Why is the atomic number referred to as “the fingerprint of the element?” • Why are atomic masses decimals?

  21. Atomic Number(Z) – the number of protons in the nucleus of each atom • Mass Number – the total number* of protons and neutrons of an isotope (e.g. for He = 4) *Rounded to the nearest whole number

  22. Cations (Positive Ions) • Groups 1(IA), 2(IIA), 13(IIIA) form ions by removing the electrons in the outermost shell

  23. This is equal to the group number. Na group IA lose 1 e- Na+ Ca group IIA lose 2 e- Ca2+ Al group IIIA lose 3 e- Al3+

  24. Naming cations • Monatomic cations are identified simply by the element’s name: • Na1+ sodium • Mg2+ magnesium • Al3+ aluminum • Transition elements are a little different and will be discussed later.

  25. Anions (Negative Ions) • Groups 15(VA), 16(VIA), 17(VIIA) form ions by adding electrons to the outermost shell to make a full octet (8).

  26. This is the number of electrons that when added to the group number give eight N group VA add 3 e- N3- O group VIA add 2 e- O2- Cl group VIIA add 1 e-Cl-

  27. Naming anions • Monatomic anions are named by changing the ending to ~ide: F fluorine fluoride F- O oxygen oxide O2- N nitrogen nitride N3-

  28. What ion is formed from: Sulfide Rubidium group VIIA add 1 e- Cl- Cl No ion is formed….element name only Argon Chloride group II A subtract 2 e- Mg2+ Mg S2- S group VI A add 2 e- Magnesium Rb1+ Rb group I A subtract 1 e- has 8e- Ar Ar group VIIIA

  29. Predicting Ionic Charges Group1(IA): Lose 1 electron to form 1+ ions H+ Li+ Na+ K+

  30. Group 2 (IIA): Loses 2 electrons to form 2+ ions Be2+ Mg2+ Ca2+ Ba2+ Sr2+

  31. Group 13 (IIIA): B3+ Al3+ Ga3+ Loses 3 electrons to form 3+ions

  32. Group 14 (IVA): Gain or lose 4 electrons

  33. Group 15 (VA): Gains 3 electrons to form 3- ions N3- P3- As3-

  34. Group 16 (VIA): Gains 2 electrons to form 2- ions O2- S2- Se2-

  35. Group 17 (VIIA): Gains 1 electron to form 1- ions F1- Cl1- Br1- I1-

  36. Group 18(VIIIA): Noble gases are stable and DO NOTform ions!

  37. Label Your Periodic Table as follows: 1+ 2+ 3+ 3- 2- 1-

  38. Label Your Periodic Table as follows: 1+ 2+ What about these? 3+ 3- 2- 1-

  39. Groups 3 - 12: Most transition elements have more than one possible charge. Iron(II) = Fe2+ Iron(III) = Fe3+

  40. Groups 3 - 12: Most transition elements have more than one possible charge. Copper(I) = Cu1+ Copper(II) = Cu2+

  41. Groups 3 - 12: Some transition elements have only one possible charge. Zinc = Zn2+ Silver = Ag+ These two need to be memorized

  42. Other Metals Will have more than one possible charge.

  43. Other Metals Will have more than one possible charge. Tin = Sn2+ Tin = Sn4+ This needs to be memorized

  44. Other Metals Will have more than one possible charge. Lead = Pb2+ Lead = Pb4+ This needs to be memorized

  45. Writing Binary Ionic Compound Formulas Example: lithium and chlorine 1. Write the formulas for the cation and anion, including CHARGES! Li+ Cl- +1 + -1 = 0 charges cancel 2. Check to see if charges will cancel each other. LiCl 3. Rewrite formula WITHOUT charges. Notice “1” is not written in the formula.

  46. Naming Binary Ionic Compounds LiCl • Write the name of the cation • Write the name of the anion lithium chloride

  47. Writing Ionic Compound Formulas Example: aluminum and sulfur 1. Write the formulas for the cation and anion, including CHARGES! Al3+ S2- 2. Check to see if charges will cancel. +3 + -2 ≠ 0 3. Check to see if charges will reduce. +3 and -2 do NOT reduce

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