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Chemistry Worksheet : Chs. 7-9 ; Obj. 1-11 Name : Date : A. Read pp. 187 - 216 and answer the following questions : 1. ___________________________________ are the electrons in the highest occupied energy level of an element's atoms. 2. Circle the valence electrons in the following electron configuration of magnesium. 2 2 6 2 1s 2s 2p 3s 3. _____ (T/F) The number of valence electrons is very important in determining the chemical properties of an element. 4. _____ (T/F) The elements of a group have different numbers of valence electrons. 5. _____ (T/F) The representative groups 1A-7A have the same number of valence electrons as their group number. 6. State the number of valence electrons of the following elements : _____ oxygen _____ argon _____ fluorine _____ helium _____ lithium _____ krypton _____ magnesium _____ neon _____ potassium 7. _____ (T/F) Valence electrons are usually the only electrons involved in a chemical bond. 8. _____ (T/F) Electron dot structures show the valence electrons as dots around the symbol of the element. 9. Show the electron dot structures of the following elements : Calcium Ca chlorine Rubidium(Rb - 37) Rb Cl tin (Sn - 50) Sn 10. _____ (T/F) The higher the energy level, the more stable an atom or ion is. 11. _____ (T/F) Stable electron configurations have a low level of energy. 12. State the octet rule and who proposed the octet rule and when. 2 2 6 13. Neon has the following electron configuration : 1s 2s 2p . Answer the following questions true or false based on this electron configuration. _____ Neon has a very stable electron configuration. _____ Neon has a low level of energy. 2 2 6 _____ Magnesium (1s 2s 2p 3s2) needs to lose two electrons to become as stable as neon. _____ Magnesium will have a negative two (2-) charge after it loses two electrons. _____ Fluorine will need to gain one electron to get the electron configuration of neon and will have an ionic charge of 1-. 14. _____ (T/F) Calcium will need to lose two electrons to get the electron configuration of argon. 15. _____ (T/F) All the alkaline earth elements (Group 2A) will need to lose two electrons to obtain a noble gas electron configuration. 16. _____ (T/F) All the elements of the oxygen group (Group 6A) will need to gain two electrons to obtain the electron configuration of a noble gas. 17. _____ (T/F) All the elements of Group 6A are likely to have a 2- ionic charge. 18. _____ (T/F) All the elements of group 3A (aluminum group) will probably gain 5 electrons to get a noble gas electron configuration. 19. __________________________________________ are charged atoms or groups of atoms. 20. __________________________________________ are positively charged ions. 21. __________________________________________ are negatively charged ions. 22. _____ (T/F) Anions are formed by the loss of electrons. 23. _____ (T/F) Cations are formed by the gain of protons. 24. ____________________________ ions are the ions of the halogens and have a 1- charge, 25. _____________________________________ compounds are composed of positive and negative ions. 26. _____ (T/F) A formula unit shows the smallest whole-number ratio of ions in a molecular compound. 27. _____ (T/F) Ionic compounds are composed of nonmetallic elements. 28. _____________________________________ compounds are composed of molecules. 29. _____________________________________ show the kinds and numbers of atoms in the smallest representative unit of a substance. 30. _____________________________________ are neutral groups of atoms that act as a unit. 31. _____ (T/F) Molecular formulas show the number and kinds of atoms present in an ionic compound. 32. _____ (T/F)Molecular compounds are composed of a metal and a nonmetal. 33. Identify the following substances as ionic(I) or molecular(M). _____ H2O _____ C4H8 _____ AlCl3 _____ S2O5 _____ C12H22O11 _____ LiF B. Read pp. 274-275 and answer the following questions : 34. State the law of definite proportions. 35. State the law of multiple proportions. 36. Determine the ratio of oxygen for the two compounds carbon monoxide and carbon dioxide.