Exam 2 Study Guide Fall 23-24 PDF

Exam 2 Study Guide 1. What are the three subatomic particles of the atom? What happens when you change any of these particles? 2. What are the two types of ions that can form? What are the names, charges, and overall electron balance? 3. What are the approximate sizes of the three subatomic...

Exam 2 Study Guide 1. What are the three subatomic particles of the atom? What happens when you change any of these particles? 2. What are the two types of ions that can form? What are the names, charges, and overall electron balance? 3. What are the approximate sizes of the three subatomic particles? 4. How do you calculate the atomic mass of an atom? 5. Determine the mass and numbers of protons, neutrons, and electrons in the following: a. Mg-25 b. Mg2+ c. Chlorine d. Al3+ e. Carbon-14 6. How is the atomic mass shown on the periodic table calculated? 7. Refer to the last three examples in the isotope simulator assignment for how to calculate average atomic mass from given isotopes, or how to calculate the percent abundances when give known masses. 8. What elements make up the metalloids? 9. What are the columns and rows called on the periodic table? 10. If given a periodic table, you should know how to identify the following: a. Metals b. Non-metals c. Alkali metals d. Alkaline earth metals e. Halogens f. Nobel gases g. Transition metals 11. Predict the charge of the monatomic (single atom) ions formed by the main group elements. 12. What units does Avogadro’s number help to convert between? 13. What units does molar mass help to convert between? 14. What is Avogadro’s number? 15. Conversion practice using molar mass and Avogadro’s number: a. How many atoms are in 3.0 grams of lithium? b. How many moles are in 3.0 grams of beryllium? c. How many grams are in 4.0 x 1024 atoms of argon? 16. What is the valence shell of an atom? What are the valence electrons? Why are they important to distinguish from other electrons around the atom? 17. How many electrons can the first four principal (main) energy shells contain in an atom? 18. What does the Bohr model show? 19. Know the number of valence electrons in the main group elements. For example: a. Magnesium b. Calcium c. Helium  d. Hydrogen e. Aluminum 20. What is the octet rule? What number of electrons do the main group elements want in their outermost shell to be stable? 21. Write the electron configuration for any given element. Be able to write the regular (long) notation or the noble gas (short) notation. 22. Explain why the noble gases are so stable in nature. 23. Explain why group 1 and 17 elements are so reactive in nature. 24. Draw the Bohr model for any of the main group elements. 25. What is the different between absorption and emission in atoms? 26. What does it mean when an electron becomes “excited”? What is the “non-excited” state of an electron called? 27. How can the flame test help determine the wavelength emitted by an excited electron?