University:
Seattle Pacific University
Course:
CHM 1211 | General Chemistry I
Academic year:

2020
Views:

397

Pages:

2
Author:

esfredint7qo

Atomic Basics Answer Key Part A: Atomic Structure 1. Draw five protons in the nucleus of the atom. Label them with their charge. 2. Draw six neutrons in the nucleus of the atom. 3. Draw two electrons in the first energy level and label them with their charge. 4. Draw three electrons in the second energy level and label them with their charge. 5. What element is represented by the diagram? BORON Part B: Atomic Calculations 6. Label the information provided in the periodic table. ATOMIC NUMBER 8 O Oxygen 15.999 7. What does the atomic number represent? PROTONS or ELECTRONS SYMBOL 8. What does the atomic mass represent? NAME ATOMIC MASS PROTONS + NEUTRONS 9. How would you figure the number of protons or electrons in an atom? USE THE ATOMIC NUMBER 10. How would you figure the number of neutrons in an atom? SUBTRACT THE ATOMIC NUMBER FROM THE ATOMIC MASS 11. Use your knowledge of atomic calculations to complete the chart. Element Li P Cl Ni K Ag H Si W Ne Atomic Number Atomic Mass Protons Neutrons Electrons 3 15 4 16 18 3 15 17 28 17 59 19 108 1 14 17 10 28 19 47 20 0 28 174 20 47 1 14 17 10 NOTE: The number protons and electrons is equal to the atomic number. To find neutrons, subtract the number of protons from the atomic mass. To find the atomic mass, add the number of protons and neutrons. Part C: Electron Configuration 12. How many electrons can each level hold? 1st = 2 2nd = 8 3rd = 18 13. What term is used for the electrons in the outermost shell or energy level? VALENCE 14. Scientists use two types of diagrams to show the electron configuration for atoms. Follow your teacher’s directions to complete the diagrams. Bohr Diagram Shows all electrons Sulfur Atomic # = 16 Lewis Structure Shows valence electrons Atomic Mass = 32 S Protons = 16 Neutrons = 16 Electron = 16 15. Calculate the missing information and then draw the Bohr Diagram and Lewis Structure for each element. Li Cl Atomic # = 3 Atomic # = 10 Atomic # = 12 Mass # = 7 Mass # = 20 Mass # = 24 # of P = 3 # of P = 10 # of P = 12 # of N = 4 # of N = 10 # of N = 12 # of E = 3 Ne # of E = 10 Mg # of E = 12 Atomic # = 17 Atomic # = 2 Atomic # = 14 Mass # = 35 Mass # = 4 Mass # = 28 # of P = 17 # of P = 2 # of P = 14 # of N = 18 # of N = 2 # of N = 14 # of E = 17 He # of E = 2 Si # of E = 14 16. Answer the questions below based on the elements in question #15. (1) Which elements had a filled outermost shell? He & Ne (2) Which element would be most likely to lose electrons in a chemical bond? Li (Only has 1 valence electron) (3) Which element would be most likely to gain electrons in a chemical bond? Cl (Only needs 1 more electron to fill its outer shell) (4) Which elements are not likely to bond with other elements? He & Ne Why? They have full outer shells.