2.14.2: Answers Ions, Molecules, and Compounds (Exercises)
- Page ID
- 290660
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Two Types of Bonding Answers
1. The octet rule is the concept that atoms tend to have eight electrons in their valence electron shell.
2. Ionic bonds are formed by the attraction between oppositely charged ions.
3. Positive charges repel each other, so an ionic compound is not likely between two positively charged ions.
4. Negative charges repel each other also.
5. Ca atom is more likely to lose two electrons. It will become Ca2+ ion.
6. An Al atom is more likely to lose three electrons. It will become Al3+ ion.
7. Selenium is more likely to gain two electrons. It will become Se2− ion.
8. Iodine is more likely to gain one electron. It will become I− ion.
Ions & Bonding Answers
| Nuclear Symbol | Atomic Number | Mass Number | Number of Protons | Number of Electrons | Number of Neutrons | Charge |
| \(\mathrm{^{40}_{18}Ar}\) | 18 | 40 | 18 | 18 | 22 | 0 |
| \(\mathrm{^{39}_{19}K^+}\) | 19 | 39 | 19 | 18 | 20 | +1 |
| \(\mathrm{^{36}_{16}S^{2-}}\) | 16 | 36 | 16 | 18 | 20 | -2 |
2.
- a. MG, Group 2, metal, +2
- b. MG, Group 17, nonmetal, -1
- c. TM, +6
- d. MG, Group 15, nonmetal, -3
- e. MG, Group 13, metalloid, +3
- f. ITM, +6
- g. MG, Group 14, metal, +4
- h. TM, +2
3. Group 1 = alkali metals; Group 2 = alkaline earth metals; Group 17 = halogens; Group 18 = noble gases.
- Elements: \(\ce{O2}\), \(\ce{N2}\), \(\ce{Cl2}\), or any other diatomic element. Compounds: \(\ce{CO2}\), \(\ce{H2O}\), \(\ce{NH3}\), or any other covalent compound.
5.
- a. positive, +1
- b. positive, +2
- c. negative, -1
- d. negative, -2
- e. positive, +1
Nomenclature Answers
1.
- a. covalent, dinitrogen oxide or dinitrogen monoxide
- b. ionic, potassium oxide
- c. covalent, phosphorus trichloride
- d. ionic, aluminum phosphate
- e. covalent, hydrochloric acid
- f. ionic, ammonium fluoride
- g. ionic, lead(II) nitrite
- h. covalent, sulfurous acid
2.
- a. calcium carbonate
- b. zinc sulfide
- c. copper(I) hydroxide
- d. magnesium perchlorate
3.
- a. \(\ce{K3PO4}\)
- b. \(\ce{(NH4)2SO4}\)
- c. \(\ce{Co(OH)2}\)
- d. \(\ce{FeN}\)
4.
- a. \(\ce{PI3}\)
- b. \(\ce{N2O5}\)
- c. \(\ce{HClO3}\)