7. Each of the following statements about the properties of matter are false. Choose two statements and explain the fallacy. a. Aluminum conducts electricity because it allows electrons to flow between covalent bonds between atoms in the crystal lattice. b. The bonding within H,O molecules explains why water has a high boiling point. The geometry of an ionic compound determines if it's polar or non-polar. с.

7. Each of the following statements about the properties of matter are false. Choose two statements and explain the fallacy. a. Aluminum conducts electricity because it allows electrons to flow between covalent bonds between atoms in the crystal lattice. b. The bonding within H,O molecules explains why water has a high boiling point. The geometry of an ionic compound determines if it's polar or non-polar. с.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 3A

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Similar questions

What is the geometric sanctum of the ammonia molecule? How many pairs of electrons surround the nitrogen atom in NH3? What is the approximate HNHbond angle in ammonia?
hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?
Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (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 K2O 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 Ionization Energy (kJ/mol) Second Ionization 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.
Hydrogen gas and oxygen gas react violently to form water. When this occurs, a very loud noise is heard. Draw the Lewis structures for hydrogen gas, oxygen gas, and water. State whether each molecule is polar or nonpolar and why. Explain how the polarity of these molecules is related to hydrogen and oxygen existing in the gas phase at room temperature and water existing in the liquid phase at room temperature. Which is lower in energy for this reaction a mixture of hydrogen and oxygen gases or water? How do you know this is true?
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Describe the molecular structure around the indicated atom or atoms: (a) the sulfur atom in sulfuric acid, H2SO4[(HO)2SO2] (b) the chlorine atom in chloric acid, HClO3[HOClO2] (c) the oxygen atom in hydrogen peroxide, HNO3[HONO2] (d) the nitrogen atom in nitric acid, HNO3[HONO2] (e) the oxygen atom in the OH group in nitric acid, HNO3[HONO2] (f) the central oxygen atom in the ozone molecule, O3 (g) each of the carbon atoms in propyne, CH3CCH (h) the carbon atom in Freon, CCl2F2 (i) each of the carbon atoms in aliene, H2CCH2
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The molecules NH3andBF3have the same general formula (AB3)but different shapes. Find the shape of each of the above molecules. Provide more examples of real molecules that have the same general formulas but different shapes.
Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
a) What types of elements are bonded together to make an ionic compound? Give three examples of ionic compounds. Identify the types of elements that make up the compound in each example. B) Describe how the physical state of a substance at room temperature depends on the strength of the intermolecular forces between the particles of the substance.