1. explain the relevance of the conductivity lab to the relevance of the subject of chemistry. - 2. using the periodic table, discuss the importance of the unique group and period location of sodium and chlorine. classify each element as either a metal or a non-metal, and use these classifications to explain their likely behavior for losing or gaining electrons, in terms of their ionization energy or electronegativity, forming cations or anions respectively. - 3. using the aeld, illustrate the atomic structure of the sodium and chlorine atoms, displaying the number of protons and neutrons comprising the nucleus, as well as the placement of electrons on the various energy levels, according to bohr’s atomic theory. provide an explanation of these diagrams, especially accounting for the number of protons and neutrons comprising the nucleus as well as the arrangement of electrons on the energy levels. 4. using the electron-dot notation, illustrate the number and arrangement of the valence electrons for sodium and chlorine. explain the significance of the number of valence electrons of sodium and chlorine relative to their periodic table group number, as well as the arrangement of their valence electrons according to their energy level, sublevel, and orbitals. 5. using orbital notation, illustrate the arrangement of the electrons for sodium and chlorine in the various energy levels, sublevels, and orbitals. explain the arrangement of electrons based upon the “aufbau” principal, hunds rule, and the pauli exclusion principal. 6. write the electron configurations for the sodium and chlorine atoms. write the outer configuration for each atom, and explain their significance relative to the number of bonds each element would be predicted to form. 7. using the concepts of ionization energy and electronegativity, explain why metals like sodium tend to give up electrons, and nonmetals like chlorine tend to gain electrons to form ionic bonds. 8. using the aeld, illustrate and explain the transfer of an electron from sodium to chlorine, forming an ionic bond. 9. using the electron-dot notation, illustrate and explain the transfer of an electron from sodium to chlorine, forming an ionic bond. explain the force of attraction between the sodium and chloride ions. 10. using orbital notation, illustrate and explain the transfer of an electron from sodium to chlorine, forming an ionic bond.    11. explain why the bond between sodium and chlorine is classified as an ionic bond based upon electronegativity values. 12. write the electron configuration of the sodium ion (na+1) and the chloride ion (cl-1). 13. write the balanced oxidation half-reaction for the sodium atom. 14. write the balanced reduction half-reaction for the chlorine atom. 15. write a balanced chemical equation for the direct combination reaction between sodium and chlorine forming sodium chloride. write the name of all the reactants and products, as well as their states of matter. classify each of the substances according to the paperclip atom lab. 16. explain how the balanced chemical equation between sodium and chlorine supports the law of conservation of mass. 17. recalling the videotaped demonstration of the reaction between sodium and chorine, describe the reaction as presented on the videotape in terms of the states of matter of sodium and chlorine, their appearance as reactants, the appearance of the reaction as it proceeds, the appearance of sodium chloride as a product and the forms of energy released from the reaction.