part c: electron configuration\n12. how many electrons can each level hold? 1st = ____ 2nd = ____ 3rd =…

part c: electron configuration\n12. how many electrons can each level hold? 1st = ____ 2nd = ____ 3rd = ____\n13. what term is used for the electrons in the outermost shell or energy level? ____\n14. scientists use two types of diagrams to show the electron - configuration for atoms. follow your teacher’s directions to complete the diagrams.\n sulfur\n atomic # = 16\n atomic mass = 32\n protons = ____\n neutrons = ____\n electron = ____\n bohr diagram\n shows all electrons\n lewis structure\n shows valence electrons\n s\n15. calculate the missing information and then draw the bohr diagram and lewis structure for each element.\n li\n atomic # = 3\n mass # = 7\n # of p = ____\n # of n = ____\n # of e = ____\n ne\n atomic # = 10\n mass # = 20\n # of p = ____\n # of n = ____\n # of e = ____\n mg\n atomic # = 12\n mass # = 24\n # of p = ____\n # of n = ____\n # of e = ____\n cl\n atomic # = 17\n mass # = 35\n # of p = ____\n # of n = ____\n # of e = ____\n he\n atomic # = 2\n mass # = 4\n # of p = ____\n # of n = ____\n # of e = ____\n si\n atomic # = 14\n mass # = 28\n # of p = ____\n # of n = ____\n # of e = ____\n(1) which elements had a filled outermost shell? ____\n(2) which element would be most likely to lose electrons in a chemical bond? ____\n(3) which element would be most likely to gain electrons in a chemical bond? ____\n(4) which elements are not likely to bond with other elements? ____ why?

part c: electron configuration\n12. how many electrons can each level hold? 1st = ____ 2nd = ____ 3rd = ____\n13. what term is used for the electrons in the outermost shell or energy level? ____\n14. scientists use two types of diagrams to show the electron - configuration for atoms. follow your teacher’s directions to complete the diagrams.\n sulfur\n atomic # = 16\n atomic mass = 32\n protons = ____\n neutrons = ____\n electron = ____\n bohr diagram\n shows all electrons\n lewis structure\n shows valence electrons\n s\n15. calculate the missing information and then draw the bohr diagram and lewis structure for each element.\n li\n atomic # = 3\n mass # = 7\n # of p = ____\n # of n = ____\n # of e = ____\n ne\n atomic # = 10\n mass # = 20\n # of p = ____\n # of n = ____\n # of e = ____\n mg\n atomic # = 12\n mass # = 24\n # of p = ____\n # of n = ____\n # of e = ____\n cl\n atomic # = 17\n mass # = 35\n # of p = ____\n # of n = ____\n # of e = ____\n he\n atomic # = 2\n mass # = 4\n # of p = ____\n # of n = ____\n # of e = ____\n si\n atomic # = 14\n mass # = 28\n # of p = ____\n # of n = ____\n # of e = ____\n(1) which elements had a filled outermost shell? ____\n(2) which element would be most likely to lose electrons in a chemical bond? ____\n(3) which element would be most likely to gain electrons in a chemical bond? ____\n(4) which elements are not likely to bond with other elements? ____ why?

Answer

Explanation:

Step1: Recall atomic number properties

The number of protons (P) is equal to the atomic number. The number of electrons (E) is equal to the number of protons in a neutral atom. The number of neutrons (N) = Mass number - Atomic number.

Step2: For Sulfur (S)

Atomic number = 16. So, Protons = 16, Electrons = 16. Mass number = 32, Neutrons = 32 - 16=16.

Step3: For Lithium (Li)

Atomic number = 3. Protons = 3, Electrons = 3. Mass number = 7, Neutrons = 7 - 3 = 4.

Step4: For Neon (Ne)

Atomic number = 10. Protons = 10, Electrons = 10. Mass number = 20, Neutrons = 20 - 10 = 10.

Step5: For Magnesium (Mg)

Atomic number = 12. Protons = 12, Electrons = 12. Mass number = 24, Neutrons = 24 - 12 = 12.

Step6: For Chlorine (Cl)

Atomic number = 17. Protons = 17, Electrons = 17. Mass number = 35, Neutrons = 35 - 17 = 18.

Step7: For Helium (He)

Atomic number = 2. Protons = 2, Electrons = 2. Mass number = 4, Neutrons = 4 - 2 = 2.

Step8: For Silicon (Si)

Atomic number = 14. Protons = 14, Electrons = 14. Mass number = 28, Neutrons = 28 - 14 = 14.

Step9: Answer questions about bonding

(1) Elements with filled outermost shell: Ne, He. They have a stable electron - configuration (2 for He and 8 for Ne in the outermost shell). (2) Element most likely to lose electrons: Li. It has 1 valence electron and wants to achieve a stable configuration by losing it. (3) Element most likely to gain electrons: Cl. It has 7 valence electrons and wants to gain 1 electron to have a stable octet. (4) Elements not likely to bond: Ne, He. They have a full outermost shell and are chemically stable.

Answer:

For Sulfur: Protons = 16, Neutrons = 16, Electrons = 16. For Lithium: Protons = 3, Neutrons = 4, Electrons = 3. For Neon: Protons = 10, Neutrons = 10, Electrons = 10. For Magnesium: Protons = 12, Neutrons = 12, Electrons = 12. For Chlorine: Protons = 17, Neutrons = 18, Electrons = 17. For Helium: Protons = 2, Neutrons = 2, Electrons = 2. For Silicon: Protons = 14, Neutrons = 14, Electrons = 14. (1) Ne, He (2) Li (3) Cl (4) Ne, He; They have a full outermost shell and are chemically stable.