Chapter Review
47. When do chemical bonds form? They may form by the attraction between a positive nucleus and negative electrons or the attraction between a positive ion and negative ion.
48. Why do positive ions and negative ions form? The form to attain a noble gas configuration.
49. Why are halogens and alkali metals likely to form ions? The number of valence electrons helps determine which element will join. For example halogens have 7 and alkai metals only have 1, therefore when join they have a full/happy outshell.
50. Discuss the importance of electrons affinity and ionization energy in the formation of ions. Ionization energy means a atom and lose electrons easily. The electron addinity indicates how much attraction an atom has for electrons. Ions Ions form when an atom loses or gains an electron, these two lead to it and create the attraction between electrons.
51. Discuss the formation of ionic bonds. Ionic bonds form when atoms are going at the speed of light and clash together.
52 Briefly discuss three physical properties of ionic solids that are linked to ionic bonds. Physical properties are crystalline stucture at high melting and boiliong points, room temperature, and exists as solids because of the intermolecular force of attraction.
53. What does the term electrically neutral mean when discussing ionic compounds. It means the charges of the cation and anions must balance or cancel each other out.
54. What information is needed to write a correct chemical formula to represent an ionic compound? The cation, anion and the subscripts are need to do this.
55. What are subscripts used in formulas for ionic compounds? Subscripts are used to show the number of ions of each element in an ionic compound.
56. Discuss how an ionic compound is named. Most have two word names, the first is the name of the cation, and the second is the name of the anion.
57. Describe a metallic bond. A metallic bond is the attraction of metallic cation for decalized electrons.
58. Briefly explain how malleability and ductility of metals are explained by metallic bonding? Metals are malleable,that means they can be hammered thin. They are also ductile which means they can be drawn into wire. Thise hows that mobile particles involved in metallic bonding can be pushed or pulled past each other, making metals malleable and ductile.
59. Compare and contrast the two types of metal alloys. An interstitial alloy is formed when the small holes in a metallic crystal are filled with smaller atoms. A substitutional alloy has atoms of the original metallic sold replace by other metal atoms of similar size.
60. Explain why noble gases are not likely to form chemical bonds. They are unreactive, due to the fact their outersell is happy/full.
61. a. cesium- 1
b. rubidium- 1
c. gallium- 3
d. zinc - 2
e. strontium- 2
62. Discuss the formation of barium ion. Barium is in the 2A group and a metal. Which means that it has two electrons past the noble gas, it can also participate in the metallic bond wher the Ba ions will release the two electrons into the lattice.
63. Explain how an anion of nitrogen forms. It forms due to the face it needs to gain three more lectrons, because electrons are negative, nitrogen is given a -3 charge.
64. The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or florine? Explain.Fluorine has more potential engery, because it still need to become happy/full. Qhile neon is a noble gas and is already happy/full.
65. a. potassium-most reactive
b. fluorine- less reactive
c. neon- nonreactive
66. Discuss the formation of the ion ion that has a 3t oxidation number.The iron ion is a Fe2+, but iron has multiple oxidation states. It is also easy for iron toe lose one more electrons to form Fe3+. Fe2= ions further ozidized when it meets an ozidizing agent. Oxygen will remove one more lectrons from the ion to it Fe3+.
48. Why do positive ions and negative ions form? The form to attain a noble gas configuration.
49. Why are halogens and alkali metals likely to form ions? The number of valence electrons helps determine which element will join. For example halogens have 7 and alkai metals only have 1, therefore when join they have a full/happy outshell.
50. Discuss the importance of electrons affinity and ionization energy in the formation of ions. Ionization energy means a atom and lose electrons easily. The electron addinity indicates how much attraction an atom has for electrons. Ions Ions form when an atom loses or gains an electron, these two lead to it and create the attraction between electrons.
51. Discuss the formation of ionic bonds. Ionic bonds form when atoms are going at the speed of light and clash together.
52 Briefly discuss three physical properties of ionic solids that are linked to ionic bonds. Physical properties are crystalline stucture at high melting and boiliong points, room temperature, and exists as solids because of the intermolecular force of attraction.
53. What does the term electrically neutral mean when discussing ionic compounds. It means the charges of the cation and anions must balance or cancel each other out.
54. What information is needed to write a correct chemical formula to represent an ionic compound? The cation, anion and the subscripts are need to do this.
55. What are subscripts used in formulas for ionic compounds? Subscripts are used to show the number of ions of each element in an ionic compound.
56. Discuss how an ionic compound is named. Most have two word names, the first is the name of the cation, and the second is the name of the anion.
57. Describe a metallic bond. A metallic bond is the attraction of metallic cation for decalized electrons.
58. Briefly explain how malleability and ductility of metals are explained by metallic bonding? Metals are malleable,that means they can be hammered thin. They are also ductile which means they can be drawn into wire. Thise hows that mobile particles involved in metallic bonding can be pushed or pulled past each other, making metals malleable and ductile.
59. Compare and contrast the two types of metal alloys. An interstitial alloy is formed when the small holes in a metallic crystal are filled with smaller atoms. A substitutional alloy has atoms of the original metallic sold replace by other metal atoms of similar size.
60. Explain why noble gases are not likely to form chemical bonds. They are unreactive, due to the fact their outersell is happy/full.
61. a. cesium- 1
b. rubidium- 1
c. gallium- 3
d. zinc - 2
e. strontium- 2
62. Discuss the formation of barium ion. Barium is in the 2A group and a metal. Which means that it has two electrons past the noble gas, it can also participate in the metallic bond wher the Ba ions will release the two electrons into the lattice.
63. Explain how an anion of nitrogen forms. It forms due to the face it needs to gain three more lectrons, because electrons are negative, nitrogen is given a -3 charge.
64. The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or florine? Explain.Fluorine has more potential engery, because it still need to become happy/full. Qhile neon is a noble gas and is already happy/full.
65. a. potassium-most reactive
b. fluorine- less reactive
c. neon- nonreactive
66. Discuss the formation of the ion ion that has a 3t oxidation number.The iron ion is a Fe2+, but iron has multiple oxidation states. It is also easy for iron toe lose one more electrons to form Fe3+. Fe2= ions further ozidized when it meets an ozidizing agent. Oxygen will remove one more lectrons from the ion to it Fe3+.