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ORGANIZING THE ELEMENTS

ORGANIZING THE ELEMENTS. Created By: Amy Taylor Hazelwood Central High School To Teacher Page To Activity. Teacher Page. Grade Level: 10 MAP Content Standards: The learner will be able to understand the organization of the periodic table.

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ORGANIZING THE ELEMENTS

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  1. ORGANIZING THE ELEMENTS Created By: Amy Taylor Hazelwood Central High School To Teacher PageTo Activity

  2. Teacher Page • Grade Level: 10 • MAP Content Standards: • The learner will be able to understand the organization of the periodic table. • The learner will be able to show how the periodic table can be utilized to estimate the chemical properties of known and unknown elements. • The learner will be able to show how the periodic table can be utilized to estimate the physical properties of known and unknown elements.

  3. MAP Content Standards Continued.. • The learner will be able to find out the trends for properties of elements in the periodic table as they connect to the physical world. • Tips for Classroom Use: • Preview the activity before using it with your class. • This activity is recommended as an introduction to the organization of the periodic table. You will want to take down or cover any periodic table displayed in your room to encourage creativity.

  4. Tips for Classroom Use, continued... • This activity may take an entire class period to complete effectively. • There are element cards that you will have to print out and copy for your class…one set is recommended for every 3 students. • Journaling: • This activity is intended to be used in conjunction with journaling. • The notebook icon will prompt the students when to journal in their notebooks.

  5. Mass Number = 9 Melting Point (°C) = 1278 Boiling Point (°C) = 2970 # O in oxide = 1 # Cl in chloride = 2 Atomic Radius (nm) = .111 Mass Number = 19 Melting Point (°C) = -220 Boiling Point (°C) = -188 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .072 Mass Number = 20 Melting Point (°C) = -248 Boiling Point (°C) = -246 # O in oxide = n/a # Cl in chloride = n/a Atomic Radius (nm) = .160 Mass Number = 16 Melting Point (°C) = -218 Boiling Point (°C) = -183 # O in oxide = n/a # Cl in chloride = 2 Atomic Radius (nm) = .066

  6. Mass Number = 36 Melting Point (°C) = -101 Boiling Point (°C) = -35 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .099 Mass Number = 7 Melting Point (°C) = 181 Boiling Point (°C) = 1327 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .152 Mass Number = 40 Melting Point (°C) = -189 Boiling Point (°C) = -186 # O in oxide = n/a # Cl in chloride = n/a Atomic Radius (nm) = .191 Mass Number = 27 Melting Point (°C) = 660 Boiling Point (°C) = 2467 # O in oxide = 1.5 # Cl in chloride = 3 Atomic Radius (nm) = .143

  7. Mass Number = 39 Melting Point (°C) = 64 Boiling Point (°C) = 774 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .227 Mass Number = 23 Melting Point (°C) = 98 Boiling Point (°C) = 883 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .192 Mass Number = 32 Melting Point (°C) = 113 Boiling Point (°C) = 445 # O in oxide = 3 # Cl in chloride = 2 Atomic Radius (nm) = .104 Mass Number = 4 Melting Point (°C) = -272 Boiling Point (°C) = -269 # O in oxide = n/a # Cl in chloride = n/a Atomic Radius (nm) = .122

  8. Mass Number = 14 Melting Point (°C) = 210 Boiling Point (°C) = -196 # O in oxide = 2.5 # Cl in chloride = 3 Atomic Radius (nm) = .070 Mass Number = 11 Melting Point (°C) = 2079 Boiling Point (°C) = 3675 # O in oxide = 1.5 # Cl in chloride = 3 Atomic Radius (nm) = .083 Mass Number = 40 Melting Point (°C) = 839 Boiling Point (°C) = 1484 # O in oxide = 1 # Cl in chloride = 2 Atomic Radius (nm) = .197 Mass Number = 12 Melting Point (°C) = 3550 Boiling Point (°C) = 4827 # O in oxide = 2 # Cl in chloride = 4 Atomic Radius (nm) = .077

  9. Mass Number = 28 Melting Point (°C) = 1410 Boiling Point (°C) = 2355 # O in oxide = 2 # Cl in chloride = 4 Atomic Radius (nm) = .117 Mass Number = 31 Melting Point (°C) = 44 Boiling Point (°C) = 280 # O in oxide = 2.5 # Cl in chloride = 3 Atomic Radius (nm) = .115 Mass Number = 1 Melting Point (°C) = -259 Boiling Point (°C) = -253 # O in oxide = 0.5 # Cl in chloride = 1 Atomic Radius (nm) = .053 Mass Number = 24 Melting Point (°C) = 649 Boiling Point (°C) = 1090 # O in oxide = 1 # Cl in chloride = 2 Atomic Radius (nm) = .160

  10. Focus on the process of problem solving with your students…they need to understand not only the facts, but the reasoning behind them. Have them write their thoughts on paper and then discuss them as a class.

  11. An Examination of Elemental Properties • Recall that elements are made up of only one type of atom; thus, all atoms of a given element have the same physical and chemical properties. • Your teacher has provided you with a set of 20 element cards that describe some of these properties for 20 different elements. • Let’s look at the element cards now...

  12. Here’s how each Element Card is organized... • Each card gives • the mass number • the measurements for melting point, boiling point, and atomic radius • the number of atoms of oxygen and chlorine that will combine with one atom of the element to make a compound. Mass Number = ___ Melting Point (°C) = ___ Boiling Point (°C) = ___ # O in oxide = ___ # Cl in chloride = ___ Atomic Radius (nm) = ___

  13. Cut your cards apart and then take some time to look over the properties of the elements. With your group, determine how you feel they are best organized. • Be logical in your organization. • Look for similarities among the elements. • Look for patterns.

  14. In your notebook… • Describe how you chose to place the elements into groups. • How did you place the groups in relation to one another? • Within each group of elements, how did you decide to arrange the elements?

  15. Compare your organization to others in your class. • What were the similarities? • What were the differences? Discuss this with your classmates.

  16. You have, in essence, created your own periodic table. Just as there are many versions of this table around your class, there were many different versions that existed before our current periodic table was adopted.

  17. However, they all had a few things in common: • They all attempted to organize the elements in a user-friendly fashion. • They all grouped elements with similar characteristics together. • They attempted to find patterns to place the elements in a logical way.

  18. Compare and contrast your periodic table to the one displayed in your classroom.

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