Chapter 8 Review:
1. Chemical bonds can be formed in two ways. Two atoms can share electrons to form a covalent bond, or an atom can give or take electrons from another atom to form an ionic bond.2. An positive ion (cation) is formed by removing electrons from an atom or group of atoms. A negative ion (anion) is formed by gaining electrons an atom or group of atoms.
3. An ion is formed when an atom loses or gains electrons so that the number of protons and the number of electrons are different. Halogens only have to gain one electron become negatively charged ion. Alkali metals only have to lose one electron to gain atomic stability. Which is why they are more likely more likely to form ions.
4. Ionization energy is the energy needed to remove an electron from an element, whereas electron affinity is the amount of attraction a substance has for a electron. One is the amount of energy to remove an electron while the other is the likeliness for it to attract an electron.
5. The formation of an Ionic Bond is the transfer of one or more elections from a metal onto a non-metal.
6. The three physical properties are Melting Point, Boiling Point, and Hardness.
7. In order to be electrically neutral, charges of the cations and anions must balance or cancel one another out.
8. You would need the charges of the metallic and non-metallic ions.
9. When two elements combine in a one to one ratio subscripts will be needed in the formulas of Ionic Compounds.
10. You write the name of the metal first then the non-metal.
11. The attraction between a metal cation and the shared electrons that surround it.
12. Malleability means beaten into sheet and ductility means drawn into wires. These properties are due to the non- directional nature of the metallic bond. When any force is applied on the metal the position of kernels is changed without destroying the crystal. The metallic lattice gets deformed due to the slippage of the kernels from one part to another. It doesn't change the environment of the kernels of the kernels. It simply moves the kernel from one lattice to another.
13. Substation Alloys: Where some of the atoms in one metal are replaced by atoms of different metal. Interstitial Alloys: Where small atoms fill in the gaps between larger atoms in metal.
14. Noble gasses will not likely form chemical bonds for their outer levels are full. (Basically they are happy.)
15. a. one b. one c. three d. two e. two
16. Barium, it has two valance electrons, so it becomes a negatively charged ion.
17. An anion is when two atoms of opposite charge attract one another. Nitrogen is negatively charged, and so attracts positively.
18. Neon has eight valance electrons. It doesn't want to bond with anything. Fluorine needs one more electron.
19. a. The most reactive of the three. b. Reactive but not likely. c. Not very Reactive.
20. The iron is usually Fe2+. However, iron has multiple oxidation states. So it is easy for iron to loose 1 more electron to form Fe3+.
3. An ion is formed when an atom loses or gains electrons so that the number of protons and the number of electrons are different. Halogens only have to gain one electron become negatively charged ion. Alkali metals only have to lose one electron to gain atomic stability. Which is why they are more likely more likely to form ions.
4. Ionization energy is the energy needed to remove an electron from an element, whereas electron affinity is the amount of attraction a substance has for a electron. One is the amount of energy to remove an electron while the other is the likeliness for it to attract an electron.
5. The formation of an Ionic Bond is the transfer of one or more elections from a metal onto a non-metal.
6. The three physical properties are Melting Point, Boiling Point, and Hardness.
7. In order to be electrically neutral, charges of the cations and anions must balance or cancel one another out.
8. You would need the charges of the metallic and non-metallic ions.
9. When two elements combine in a one to one ratio subscripts will be needed in the formulas of Ionic Compounds.
10. You write the name of the metal first then the non-metal.
11. The attraction between a metal cation and the shared electrons that surround it.
12. Malleability means beaten into sheet and ductility means drawn into wires. These properties are due to the non- directional nature of the metallic bond. When any force is applied on the metal the position of kernels is changed without destroying the crystal. The metallic lattice gets deformed due to the slippage of the kernels from one part to another. It doesn't change the environment of the kernels of the kernels. It simply moves the kernel from one lattice to another.
13. Substation Alloys: Where some of the atoms in one metal are replaced by atoms of different metal. Interstitial Alloys: Where small atoms fill in the gaps between larger atoms in metal.
14. Noble gasses will not likely form chemical bonds for their outer levels are full. (Basically they are happy.)
15. a. one b. one c. three d. two e. two
16. Barium, it has two valance electrons, so it becomes a negatively charged ion.
17. An anion is when two atoms of opposite charge attract one another. Nitrogen is negatively charged, and so attracts positively.
18. Neon has eight valance electrons. It doesn't want to bond with anything. Fluorine needs one more electron.
19. a. The most reactive of the three. b. Reactive but not likely. c. Not very Reactive.
20. The iron is usually Fe2+. However, iron has multiple oxidation states. So it is easy for iron to loose 1 more electron to form Fe3+.