Chapter 8 Review
47. When do chemical bonds form?
Chemical bonds can be formed in two ways. Two atoms can share electrons to form a covalent bond, or an atom can give/take electrons from another atom to form an ionic bond.
48. Why do positive ions and negative ions form?
A positive ions is formed from removing the electron's from an atom, and a negative ion is formed from gaining electron from an atom. Both positive and negative ions are formed by the transfer of electrons, the negative icon are repelled for the earth.
49. Why are halogens and alkali metals likely to form ions?
The number of valance electrons helps in determining which elements will join, halogens have 7, alkali metals 1 thus a joined a full 8 in the valance shell.
50. Discuss the importance of electron affinity and ionization energy in the formation of ions.
Electron affinity varies directly with the ionization energy, so these will affect the formation of ions by decreasing or increasing the size of the ion.
51. Discuss the formation of ionic bonds.
Ionic bonds are formed by atoms going the speed of light and clashing together to form these bonds.
52. Briefly discuss three physical properties of ionic solids that are linked to ionic bonds.
An ionic bond exists when one element donates its electrons to the other element in the bond. It is not a true bond but rather an electrostatic attraction (the + of one is attracted to the - of the other) Ionic bonds occur if there is a great difference in electronegativity (greater than 1.7 in the pauling scale). Usually they will occur with a alkaline metal (1A element - very low electronegativity) and a halogen (7A - very electronegative.) Some properties are that they disassociate in water (depressing the freezing point raising the boiling point and making the liquid conductive). They form crystal complexes and do not truly exist as a molecule rather as an ionic solid with no definable beginning or end. They therefore do not have a molecular formula but rather just an empirical formula representing their ratio.
53. What does the term electrically neutral mean when discussing ionic compounds?
The positive ion and the negative ion have charges that are equal opposites. For example. Oxygen O has a -2 charge. Hydrogen H has a +1 charge. H2O has a neutral charge. While the ions are held together by their electronegativities, overall, the molecule has no charge.
54. What information is needed to write a correct chemical formula to represent an ionic compound?
The elements involved. The specific number of each element in the molecule.
55. When are subscripts used in formulas for ionic compounds?
When two elements combine in a one to one ratio subscripts will be needed in the formulas for ionic compounds.
56. Discuss how an ionic compound is named.
The cation's name (positive ion) is written out first, then the anion's name (negative ion) is named with the ending "ide" instead of its regular ending unless it is a polyatomic ion or an ion with different charges.
57. Describe a metallic bond.
A metallic bond happens when electrons overlap in continuous atoms of a metal. When this happens, it seems like the electrons belong to the whole sample instead of singular atoms.
58. Briefly explain how malleability and ductility of metals are explained by metallic bonding.
In metallic bonding the atoms donate their electrons to a shared pool of electrons and the positively charged ions are then attracted to that negatively charged common pool of electrons. This means the metals can be easily deformed or manipulated without breaking, it also means it can easily conduct an electric current.
59. Compare and contrast the two types of metal alloys.
Substitution alloys: where some of the atoms in one metal are replaced by atoms of a different metal.
Interstitial alloys: where small atoms fill in the gaps between larger atoms in a metal.
60. Explain why noble gases are not likely to form chemical bonds.
The noble gases are chemically inert - and not likely to form chemical bonds - because their atoms are in a state of low energy.
61. Give the number of valence electrons in an atom of each of the following:
Cesium: 1 Rubidium: 1 Gallium: 13 Zinc: 12 Strontium: 2
62. Discuss the formation of the barium ion.
Barium is a member of group 2A and a metal. That means that it has two electrons beyond the noble gas and tha the only thing it will ever do is lose those two electrons and become the 2+ ion with the previous noble gas configuration. It can also participate in the metallic bond where the Ba ion will release the two electrons into the lattice.
63. Explain how an anion of nitrogen forms.
All element what to become noble gases, so in order for Nitrogen to become the closest noble gas which is ,Neon it needs to gain 3 electrons. So because electrons are negative, nitrogen is given a 3- change. it will look like thhis, N 3-, except the three and the minus sign will be like an exponent in the corner.
64. The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or fluorine?
Flourine. Neon already has 8 valence electrons. It doesn't want to bond with anything. Flourine needs one more electron.
65. Predict the reactivity of the following atoms based on their electron configurations.
Potassium: More reactive than fluorine. Fluorine: More reactive than neon. Neon: Is unreactive.
66. Discuss the formation of the iron ion that has a 3+ oxidation number.
The iron ion is usually Fe2+. However, iron has multiple oxidation sates. Hence, it is also easy for iron to lose 1 more electron to form Fe3+. Fe2+ ions further oxidized when it meets an oxidizing agent. Oxygen will remove 1 more electron from the ion to make it Fe3+.
Chemical bonds can be formed in two ways. Two atoms can share electrons to form a covalent bond, or an atom can give/take electrons from another atom to form an ionic bond.
48. Why do positive ions and negative ions form?
A positive ions is formed from removing the electron's from an atom, and a negative ion is formed from gaining electron from an atom. Both positive and negative ions are formed by the transfer of electrons, the negative icon are repelled for the earth.
49. Why are halogens and alkali metals likely to form ions?
The number of valance electrons helps in determining which elements will join, halogens have 7, alkali metals 1 thus a joined a full 8 in the valance shell.
50. Discuss the importance of electron affinity and ionization energy in the formation of ions.
Electron affinity varies directly with the ionization energy, so these will affect the formation of ions by decreasing or increasing the size of the ion.
51. Discuss the formation of ionic bonds.
Ionic bonds are formed by atoms going the speed of light and clashing together to form these bonds.
52. Briefly discuss three physical properties of ionic solids that are linked to ionic bonds.
An ionic bond exists when one element donates its electrons to the other element in the bond. It is not a true bond but rather an electrostatic attraction (the + of one is attracted to the - of the other) Ionic bonds occur if there is a great difference in electronegativity (greater than 1.7 in the pauling scale). Usually they will occur with a alkaline metal (1A element - very low electronegativity) and a halogen (7A - very electronegative.) Some properties are that they disassociate in water (depressing the freezing point raising the boiling point and making the liquid conductive). They form crystal complexes and do not truly exist as a molecule rather as an ionic solid with no definable beginning or end. They therefore do not have a molecular formula but rather just an empirical formula representing their ratio.
53. What does the term electrically neutral mean when discussing ionic compounds?
The positive ion and the negative ion have charges that are equal opposites. For example. Oxygen O has a -2 charge. Hydrogen H has a +1 charge. H2O has a neutral charge. While the ions are held together by their electronegativities, overall, the molecule has no charge.
54. What information is needed to write a correct chemical formula to represent an ionic compound?
The elements involved. The specific number of each element in the molecule.
55. When are subscripts used in formulas for ionic compounds?
When two elements combine in a one to one ratio subscripts will be needed in the formulas for ionic compounds.
56. Discuss how an ionic compound is named.
The cation's name (positive ion) is written out first, then the anion's name (negative ion) is named with the ending "ide" instead of its regular ending unless it is a polyatomic ion or an ion with different charges.
57. Describe a metallic bond.
A metallic bond happens when electrons overlap in continuous atoms of a metal. When this happens, it seems like the electrons belong to the whole sample instead of singular atoms.
58. Briefly explain how malleability and ductility of metals are explained by metallic bonding.
In metallic bonding the atoms donate their electrons to a shared pool of electrons and the positively charged ions are then attracted to that negatively charged common pool of electrons. This means the metals can be easily deformed or manipulated without breaking, it also means it can easily conduct an electric current.
59. Compare and contrast the two types of metal alloys.
Substitution alloys: where some of the atoms in one metal are replaced by atoms of a different metal.
Interstitial alloys: where small atoms fill in the gaps between larger atoms in a metal.
60. Explain why noble gases are not likely to form chemical bonds.
The noble gases are chemically inert - and not likely to form chemical bonds - because their atoms are in a state of low energy.
61. Give the number of valence electrons in an atom of each of the following:
Cesium: 1 Rubidium: 1 Gallium: 13 Zinc: 12 Strontium: 2
62. Discuss the formation of the barium ion.
Barium is a member of group 2A and a metal. That means that it has two electrons beyond the noble gas and tha the only thing it will ever do is lose those two electrons and become the 2+ ion with the previous noble gas configuration. It can also participate in the metallic bond where the Ba ion will release the two electrons into the lattice.
63. Explain how an anion of nitrogen forms.
All element what to become noble gases, so in order for Nitrogen to become the closest noble gas which is ,Neon it needs to gain 3 electrons. So because electrons are negative, nitrogen is given a 3- change. it will look like thhis, N 3-, except the three and the minus sign will be like an exponent in the corner.
64. The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or fluorine?
Flourine. Neon already has 8 valence electrons. It doesn't want to bond with anything. Flourine needs one more electron.
65. Predict the reactivity of the following atoms based on their electron configurations.
Potassium: More reactive than fluorine. Fluorine: More reactive than neon. Neon: Is unreactive.
66. Discuss the formation of the iron ion that has a 3+ oxidation number.
The iron ion is usually Fe2+. However, iron has multiple oxidation sates. Hence, it is also easy for iron to lose 1 more electron to form Fe3+. Fe2+ ions further oxidized when it meets an oxidizing agent. Oxygen will remove 1 more electron from the ion to make it Fe3+.