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Lesson 1 and 2: the History of the Periodic Table Learning Objective • to Understand the History and Significance of the Development of the Periodic Table

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Lesson 1 and 2: the History of the Periodic Table Learning Objective • to Understand the History and Significance of the Development of the Periodic Table Lesson 1 and 2: The History of the Periodic Table Learning Objective • To understand the history and significance of the development of the periodic table. Success Criteria • To produce a timeline showing the development of the periodic table. • To explain the role of Dmitri Mendeleev in developing the periodic table. • To identify a specific element given its group and period. Spot the Difference These are two old versions of the periodic table. What similarities and differences can you spot? Write your answers on paper. Newlands’ periodic table H F Cl Co/Ni Br Pd I Pt/Ir Li Na K Cu Rb Ag Cs Tl G Mg Ca Zn Sr Cd Ba/V Pb Bo Al Cr Y Ce/La U Ta Th C Si Ti In Zn Sn W Hg N P Mn As Di/Mo Sb Nb Bi O S Fe Se Ro/Ru Te Au Os • Answers • Newlands Mendeleev’s periodic table periodic table Group I Group ll Group lll Group IV Group V Group VI Group VII Group VIII doesn’t have H group numbers. • The elements Li Be B C N O F are arranged in Na Mg Al Si P S Cl a different K Ca Ti V Cr Mn Fe Co Ni order. Zn As Se Br • Cu Mendeleev has Rb Sr Y Zr Nb Mo I Ru Rn Pd left gaps in his Ag Cd In Sn Sb Te periodic table. History of the Periodic Table Read the information sheets about the scientists Johann Dobereiner, John Newlands and Dmitri Mendeleev and their contributions to the development of the periodic table. Using the activity sheet, produce a timeline to show the development of the periodic table. History of the Periodic Table Scientist: Johann Dobereiner Date Date Date The Periodic Table Add the following information to your copy of the periodic table. Elements in vertical columns are known as groups. HoriZontal rows are called periods. The group number shows the amount of electrons in the outermost shell. Reactivity Rules: in group 1, the elements become more reactive as you move down the group. Reactivity Rules: in group 7, reactivity decreases as you move down the group. Identifying an Element Given the Group and Period Number Name the element found in (write your answers on paper) : group 4, period 3 Groups 1 2 3 4 5 6 7 0 silicon 1 group 7, period 5 2 3 iodine 4 group 0, period 1 5 Periods 6 helium 7 group 2, period 4 calcium Exam-Style Questions BronZe: The element magnesium has 12 electrons. State magnesium’s groupo number and show how you could prove your answer is correct. (2 marks). Group 2 Because it has 2 electrons in its outer shell. Exam-Style Questions Silver: Part of Mendeleev’s periodic table is shown below. Group I Group ll Group lll Group IV Group V Group VI Group VII Group VIII H o i. Give the symbols of two Li Be B C N O F elements that Na Mg Al Si P S Cl Mendeleev placed in K Ca Ti V Cr Mn Fe Co Ni group 2 which are not Cu Zn As Se Br found in group 2 Rb Sr Y Zr Nb Mo I Ru Rn Pd today.(2 marks) Ag Cd Sn Sb Te In Zn and Cd ii. Name these two elements. (2 marks) zinc and cadmium iii. Mendeleev left gaps in his periodic table. Explain why. (1 mark) For undiscovered elements. iv. How are elements arranged in today’s periodic table? (1 mark) In order of atomic number. Exam-Style Questions Gold: The periodic table, as we know it today, is very different from theo early published periodic tables. Discuss how the periodic table has changed and, where possible, name the scientists involved. Your answer should be in chronological order. (4 marks) Students’ answers may vary. • 1817, Johann Dobereiner and his Law of Triads. Placed elements into groups of 3 based on appearance and similar reactions. • 1864, John Newlands and his Law of Octaves. Arranged elements in order of atomic mass and suggested that each element was similar to the element eight places further on. • 1869, Dmitri Mendeleev. Placed elements in order of atomic mass but left spaces for undiscovered elements. Mendeleev wasn’t afraid to switch elements around in the table. Lesson 3 and 4 : Atomic Structure Learning Objective To understand the structure of atoms and elements. Success Criteria • To define the terms atoms and elements. • To describe the structure of atoms. Atoms: What Do You Know? Can you label the diagram of the atom? Key Terms nucleus proton neutron electron Extension: Can you state the charges of the subatomic particles? Answers The Atom: Some Facts • Atoms are neutral. They have no overall charge because the number of protons and electrons are the same. Particle Relative Mass Relative Charge proton 1 +1 neutron 1 0 electron very small -1 • Atoms have a radius of 0.1 nanometers. Atoms On your activity sheet, define the term atom. Label the diagram of the atom. Complete the table showing the particle’s mass and charge. Elements Elements are made of one type of atom only. They are represented by both a name and a symbol. For example, carbon = C and sodium = Na (notice how the first letter is always shown by a capital and the second is lower case). Elements can be found on the periodic table; there are over 100 of them. Elements Look at your copy of the periodic table. Apart from the element name and symbol, what else do you notice? Mass Number 16 8 Atomic Number O The atomic number is the number of protons each atom contains. The mass number is the total number of protons and neutrons in the atom. Quick Assessment: Exam Question 1. Magnesium is in group 2 and period 3 of the periodic table. Here is a diagram of a magnesium atom. i. What is the mass number of a magnesium atom? ii. What is the charge of a proton? iii. Protons are found in the nucleus. Which other subatomic particle is found in the nucleus? iv. Which particle number is always different for atoms of different elements? 2. The diagram shows the electron arrangement for an element. Give the chemical symbol of the element. Answers 1. Magnesium is in group 2 and period 3 of the periodic table. Here is a diagram of a magnesium atom. i. What is the mass number of a magnesium atom? 24 ii. What is the charge of a proton? positive iii. Protons are found in the nucleus. Which other subatomic particle is found in the nucleus? neutrons iv. Which particle number is always different for atoms of different elements? number of protons 2. The diagram shows the electron arrangement for an element. Give the chemical symbol of the element. N The First 20 Elements: How Many Can You Name? You have one minute to study the name and symbol of the first 20 elements. Start The First 20 Elements: How Many Can You Name? Answers 1. hydrogen H 11. sodium Na 2. helium He 12. magnesium Mg 3. lithium Li 13. aluminium Al 4. beryllium Be 14. silicon Si 5. boron B 15. phosphorous P 6. carbon C 16. sulfur S 7. nitrogen N 17. chlorine Cl 8. oxygen O 18. argon Ar 9. fluorine F 19. potassium K 10. neon Ne 20. calcium Ca.
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