(a)
Interpretation:
The element Na needs to be classified as molecular, network covalent, ionic or metallic.
Concept introduction:
In order to identify the structure of a material/compound, one often looks at what types of bonds hold the constituent particles together. For example, molecular solids refer to a substance where the constituent particle i.e. molecules are held together by van der Waal forces. Similarly, metals contain metallic ions surrounded by a sea of delocalized electrons that ultimately form the lattice structure. Each type of bonding provides a set of unique characteristics to the substance. Moreover, the nature of inter-particle bonding is more important in determining the nature of substance.
(b)
Interpretation:
The compound
Concept introduction:
In order to identify the structure of a material/compound, one often looks at what types of bonds hold the constituent particles together. For example, molecular solids refer to a substance where the constituent particle i.e. molecules are held together by van der Waal forces. Similarly, metals contain metallic ions surrounded by a sea of delocalized electrons that ultimately form the lattice structure. Each type of bonding provides a set of unique characteristics to the substance. Moreover, the nature of inter-particle bonding is more important in determining the nature of substance.
(c)
Interpretation:
The benzene
Concept introduction:
In order to identify the structure of a material/compound, one often looks at what types of bonds hold the constituent particles together. For example, molecular solids refer to a substance where the constituent particle i.e. molecules are held together by van der Waal forces. Similarly, metals contain metallic ions surrounded by a sea of delocalized electrons that ultimately form the lattice structure. Each type of bonding provides a set of unique characteristics to the substance. Moreover, the nature of inter-particle bonding is more important in determining the nature of substance.
(d)
Interpretation:
The carbon-60 or
Concept introduction:
In order to identify the structure of a material/compound, one often looks at what types of bonds hold the constituent particles together. For example, molecular solids refer to a substance where the constituent particle i.e. molecules are held together by van der Waal forces. Similarly, metals contain metallic ions surrounded by a sea of delocalized electrons that ultimately form the lattice structure. Each type of bonding provides a set of unique characteristics to the substance. Moreover, the nature of inter-particle bonding is more important in determining the nature of substance.
(e)
Interpretation:
The aqueous solution of
Concept introduction:
In order to identify the structure of a material/compound, one often looks at what types of bonds hold the constituent particles together. For example, molecular solids refer to a substance where the constituent particle i.e. molecules are held together by van der Waal forces. Similarly, metals contain metallic ions surrounded by a sea of delocalized electrons that ultimately form the lattice structure. Each type of bonding provides a set of unique characteristics to the substance. Moreover, the nature of inter-particle bonding is more important in determining the nature of substance.
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Chapter 9 Solutions
Chemistry: Principles and Reactions
- Use principles of atomic structure to answer each of the following: (1] (a) The radius of the Ca atom is 197 pm; the radius of the Ca2* ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K20 is –2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First lonization Energy (kJ/mol) Second lonization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.arrow_forwardAmmonium chloride, NH4Cl, is a very soluble salt in water.(a) Draw the Lewis structures of the ammonium and chlorideions. (b) Is there an N—Cl bond in solid ammonium chloride?(c) If you dissolve 14 g of ammonium chloride in 500.0 mLof water, what is the molar concentration of the solution?(d) How many grams of silver nitrate do you need to add tothe solution in part (c) to precipitate all of the chloride as silverchloride?arrow_forwardDraw a Lewis structure for(a) The cyclic silicate ion Si₄O₁₂⁸⁻(b) A cyclic hydrocarbon with formula C₄H₈arrow_forward
- Draw a Lewis structure for each of the following molecules and ions. In each case, the atoms can be connected in only one way. (a) Br2 (b) H2S (c) N2H4 (d) N2H2 (e) CN- (f) NH4+ (g) N2 (h) O2arrow_forward(a) Determine the number of sodium ions in the chemicalformula of albite, NaxAlSi3O8. (b) Determine the numberof hydroxide ions in the chemical formula of tremolite,Ca2Mg5(Si4O11)2(OH)x.arrow_forwardMixing SbCl3 and GaCl3 in a 1;1 molar ratio (usingliquid sulfur dioxide as a solvent) gives a solid ioniccompound of empirical formula GaSbCl6. A controversyarises over whether this compound is ( ) SbCl2 + ( ) GaCl 4 - or( ) GaCl+ 2 ( ) SbCl 4 -(a) Predict the molecular structures of the two anions.(b) It is learned that the cation in the compound has abent structure. Based on this fact, which formulationis more likely to be correct?arrow_forward
- Consider the lattice energies of the following Group 2Acompounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol;CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol.(a) What is the oxidation number of H in these compounds?(b) Assuming that all of these compounds have the samethree-dimensional arrangement of ions in the solid, whichof these compounds has the shortest cation–anion distance?(c) Consider BeH2. Does it require 3205 kJ of energyto break one mole of the solid into its ions, or does breakingup one mole of solid into its ions release 3205 kJ of energy?(d) The lattice energy of ZnH2 is 2870 kJ/mol. Consideringthe trend in lattice enthalpies in the Group 2A compounds,predict which Group 2A element is most similar in ionic radiusto the Zn2+ ion.arrow_forwardCan you assist #74 ?arrow_forwardThe elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forward
- Write a Lewis structure for each of the following molecules and ions:(a) (CH3)3SiH(b) SiO44−(c) Si2H6(d) Si(OH)4(e) SiF62−arrow_forwardCompare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 220 pm (b) Mn²+ and O²- separated by a distance of 431 pmarrow_forwardChlorine dioxide gas (ClO2) is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (a)What is the Lewis structure for ClO2? (b) Why do you thinkthat ClO2 is reduced so readily? (c) When a ClO2 moleculegains an electron, the chlorite ion, ClO2-, forms. Draw theLewis structure for ClO2-. (d) Predict the O—Cl—O bondangle in the ClO2- ion. (e) One method of preparing ClO2is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s)------>2 ClO2(g) + 2 NaCl(s)If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorinegas at a pressure of 1.50 atm at 21 °C, how many gramsof ClO2 can be prepared?arrow_forward
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