c. Why was his arrangement so ingenious (give two reasons)? d. His arrangement produced some anomalies. Give an example. Chapter 5: The Periodic Table

Transcription

1 Chapter 5: The Periodic Table Atomic Radius decreases lonization Energy increases Electron Affin ity i ncreases Electronegativity increases Atomic Radius increases lonization Energy decreases Electron Affin ity decreases E lectronegativity decreases SHORT ANSWER: 'J". Who came up with the first useable Periodic Table? How did he arrange the elements? c. Why was his arrangement so ingenious (give two reasons)? i. ii. d. His arrangement produced some anomalies. Give an example. 2. How did Moseley arrange the elements? 3. How did Moseley determine the atomic number? Explain in detail (hint: hieh speed electrons, X- rays, metals).

2 4. How did Dobereiner arrange the elements? Explain. 5. Why was Newlands ridiculed for this version of the Periodic Table? 6. Name each of the following groups: Group L4: Group 2A: c. Group 7A: d. Group 34: e. Group 44: f. Group 5A: 7. Where are the transition metals on the periodic table (what orbitals do these atoms fill)? 8. List the elements in the Lanthanide series: 9. List the elements in the Actinide series: 10. Elements of the same group have the same number of electrons. 11. The chemical and physical properties of the elements are periodic functions of their, Elements with similar properties occur at 1-2. Define atomic radius: L3. t4. Moving down a group, the atomic radius discovered most of the Noble gases. 15. Moving left to right across a period, atomic radius why? 16. Metals tend to have why?

3 17. Nonmetals tend to have 18. Noble gases have 19. Moving down a group, ionization energy 24. Moving left to right across a period, ionization energy 21-. What is electron affinity? Which group(s) has the highest electron affinity (most negative number)? c. Which group(s) have the lowest electron affinity (positive numbers)? 22. Define electronegativity. 23. What element has the highest electronegativity? 24. Where are metals located on the periodic tables? 25. List 3 characteristics of metals:

4 26. Where are nonmetals located on the periodic table? 27. List three characteristics of nonmetals: c. 28. List the metalloids: 29. What properties do metalloids have? 30. An element undergoes several ionizations as follows: First: 740 kj Second: 1450 kj Third: 7730 kj Fourth: 9500 kj How many valence electrons does the atom have? What group does it belong to? 31. Moving left to right in period 6, the electrons enter which sublevels (see electron configuration)? MULTIPLE CHOICE: L The relationship in which the physical and chemical properties of elements show a periodic pattern when elements are arranged by increasing atomic number is called the periodic law c. Mendeleev's law the law of octaves d. Meyer's periodicity 2. Who classified the elements into triads? Mendeleev c. Newlands Moseley d. Dobereiner 3. The scientist who observed a pattern of properties that repeated every eight elements was Mendeleev c. Newlands Moseley d. Dobereiner 4. Mendeleev arranged the elements in the periodic table in order of increasing atomic number c. ionization energy mass number d. atomic mass

5 5. ln the periodic table, the periods are vertical columns c. chemicalfamilies horizontal rows d. blocks of elements 6. How many elements are in the first period of the periodic table? 7 2 c. 18 d. L09 7. The elements in Group 14 of the periodic table are called the halogens alkali metals 8. The elements in Group 2A of the periodic table are called the halogens alkalimetals 9. What are the elements in Group 7A of the periodic table called? halogens alkali metals 10. Those electrons that are largely responsible for an atom's chemical behavior are called core electrons valence electrons 1L. The second period of the periodic table contains s-block elements c.s, p, and d-block elements s and p-block elements d. p block elements L2. Asystematicvariationinthepropertiesof elementsgoingdownagrouporacrossaperiodis called a blockcharacteristic periodic law 1-3. When an atom loses an electron, it collapses loses protons remains the same size 1-5. A positively charged ion is called a cation gluon L6. A negatively charged ion is called a cation down quark high energy electrons c. stable electrons c. periodic trend d. triad configuration c. becomes smaller becomes negatively charged d. becomes larger 14. When an atom becomes a negative ion, it c. becomes larger d. becomes smaller c. anion d. quark c. anion d. quark 1-7. Thefirstelectron removed from an tin (Sn) atom is (see electron figuration)? 3p 4d c. 5s d. 5p