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Name: ______________________________________ Date: _____________________ Ch 6 Notes The Periodic Table 1. The periodic table was organized by Dmitri ____________________________________. He placed known elements in order according to increasing atomic _______________________. 2. When Mendeleev organized the elements he noticed that the elements’ _______________________________ repeated in a regular pattern, or a _______________________________ pattern. 3. Mendeleev placed the known elements in a table, where he arranged elements into _______________________ with similar _____________________________. 4. Although all of the elements were not known, Mendeleev predicted the ___________________________ of several elements that were __________________________ at the time. These predictions were _______________________ and well accepted. 5. The modern periodic table differs from Mendeleev’s periodic table in that: a. _____________________________ found elements were ____________________ b. and, the table was organized by atomic _________________________ rather than atomic _____________________. 6. The horizontal rows on the periodic table are called _______________________.This is because the properties begin to _____________________________ in each new row. 7. The columns on the periodic table are called _______________________(or ___________________) and the elements in the groups have _____________________________ properties. Classification of Elements and Group Names 8. Groups on the periodic table are assigned an A or B notation. The ____________________ group elements can be found in Groups 1A through 8A. The main group elements (Group A elements) are also called _____________________________________ elements. 9. On the other hand, the group B elements are known as the ____________________________________ elements. 10. The elements on the periodic table can be divided into three main categories: a. _________________________ b. ___________________________________ c. _______________________________ 11. Metals have properties that include that they are _______________________ solids, and _____________________ conductors of heat and __________________________. 12. The name of Group 1A is the ____________________________ metals and the name of Group 2A is the ___________________ ___________________ metals. 13. Elements on the right side of the heavy stairstep line are called ________________________. 1 Name: ______________________________________ Date: _____________________ 14. The properties of nonmentals are that they are generally _______________________ or brittle ________________________ at room temperature. 15. Group 7A elements are called ___________________________ and Group 8A elements are called the __________________________ gases. 16. Elements along the stairstep are called ___________________________. Their properties are _________ _____________________________ the properties of metals and nonmetals. 17. Scientists now understand that the repetition of properties of elements occurs because the__________________________ configurations of atoms repeat. 18. For representative elements, the Group Number in front of the A tells the number of ____________________________ electrons in the atoms in the column. 19. Also the period number (or row number) of a __________________________ element tells the __________________________ level of the valence electrons. 20. The periodic table is divided into _____________________ that correspond to the energy _________________________ being filled as you move across a period. a. S-block: Groups ___________________ b. P-block: Groups ___________________ c. D-block: Groups __________________ d. F-block: Rows ________________________________________ Periodic Trends 21. The ________________________ structure of an atom determines many of its ________________________ and ________________________ properties. 22. The atomic ___________________________is a measure of the __________________ of an atom. The larger the radius, the larger the atom. 23. As you move across a ______________________ the atom ________________________ in size. This is due to the ______________________ positive charge of the nucleus while electrons are being added, but the orbitals are close in energy. The increased nuclear charge pulls the outermost electrons ___________________ to the nucleus, making the atom _____________________. 24. As you move down a group, atomic radii __________________________. This is due to the addition of a larger energy ___________________ each time. Electrons in higher levels are located ______________________ from the nucleus than those in the lower energy levels. 25. The driving force that makes reactions happen is ______________ formation. Ions form when atoms gain or lose _______________________. Ions will have either a ___________________________ or __________________________ charge. 26. When atoms lose electrons and form positively charged ions, they become __________________________, and are called _______________________. They become smaller because the loss of the electrons means that the number of protons is ______________________ than the number of electrons. 27. Therefore, the electrons will be pulled more _________________ to the nucleus, and the outer electrons will feel the pull of the nucleus more strongly than before. 2 Name: ______________________________________ Date: _____________________ 28. When atoms gain electrons they form negatively charged ions, called ________________________. The added electron makes the ionic radius ______________________, because of ____________________________ and the weaker pull of the nucleus on each electron. 29. As you move from left to right across the periodic table, your positively forming ions, Groups 1A-4A get _________________________, but Groups 5A- 8A get ___________________________. As you move from top to bottom the ions get larger in each column because of the __________________________ of energy ____________________. 30. To form a positive ion, an __________________________ must be removed from a neutral atom. Removing the electron requires __________________. That energy must overcome the attraction between the positive charge in the nucleus and the negative charge of the electron. 31. This energy, known as __________________________ energy is defined as the energy required to remove an ______________________ from an atom in the gaseous state. 32. The first ionization energy is the amount of energy required to remove the ___________________ electron from the outer shell of the atom. 33. Remember that as you move across a period, you ________________________ atomic number and therefore add more ____________________ charge to the atom. 34. That addition makes it more difficult to _____________________ the electron and therefore more energy is required. 35. For the first ionization energy, as you move across a period, from left to right, the ionization energy _________________________. 36. It is also possible to remove ___________________ after removing the first, or furthermost electron from the electron cloud. However, once you remove the first electron, much more ____________________ is required to remove the second, and third, and fourth, etc. 37. When atoms/ions have __________________ electrons in their outer shell, they are much more __________________. 38. The ____________________ rule says that atoms tend to gain, lose or share electrons in order to acquire a full set of _________________ valence electrons. 39. Use this to predict what kinds of ions will form: elements on the ________________ will form ________________ ions and elements on the _______________ will form _____________________ ions. 40. The __________________________________ of an element tells about its ability to attract electrons in a chemical bond. 41. As you move from top to bottom down a group, electronegativity generally __________________________. As you move from left to right, electronegativity generally _______________________. 3