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- Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.The standard heat of formation of BaBr2BaBr2 is −−764 kJ/molkJ/mol. The first ionization energy of BaBa is 503 kJ/molkJ/mol and its second ionization energy is 965 kJ/molkJ/mol. The heat of sublimation of Ba[Ba(s)→Ba(g)]Ba[Ba(s)→Ba(g)] is 175 kJ/molkJ/mol. The bond energy of Br2Br2 is 193 kJ/molkJ/mol, the heat of vaporization of Br2(l)Br2(l) is 31 kJ/molkJ/mol, and the electron affinity of BrBr is −−325 kJ/molkJ/mol. Calculate the lattice energy of BaBr2BaBr2.B. Show the formation of ionic bonding in the following: MgCl2 CaBr2 Al2S3
- For GaAs the absolute difference in electronegativity and the type of the bond are respectively: Group of answer choices 0.4, polar covalent 3.6, polar covalent 2.0, ionic 3.6, ionic 1.6, polar covalent 2.0, polar covalent 0.4, ionic 0.4, covalent 1.6, covalentNo Plagiarism Please Why do ionic and polar covalent substances conduct electricity and nonpolar molecules are not conductors of electricity? https://www.loom.com/share/58718558d262449c9c9d0d0a5a91652bA. Name the covalent compounds 1. B2Si 2. Cl2O5 3. PCl3 4. Cl2O 5. Si2Br6 6. F2O5 B. Name ionic compounds 1. NH4Cl 2. MgS 3. Fe(NO3)3 4. TiBr3 5. Cu3P 6. SnSe2 7. GaAs 8. Pb(SO4)2 9. Be(HCO3)2 10. Mn2(SO3)3 11. Al(CN)3 C. Using electronegative to determine polarity. (Include the equation and type of compound.)
- 1. Write the chemical formula for a compound containing the following elements: calcium and oxygen; 1:1 A. O2Ca2 B. OCa2 C. OCa D. CaO2 E. Ca2O2 F. O2Ca G. Ca2O H. CaO 2. Calculate ∆En for the following bond and classify it according to type: MgO A. -2.3; ionic B. 2.3; ionic C. -2.3; covalent D. -2.3; polar covalent E. -2.3; nonpolar covalent F. 2.3; polar covalent G. 2.3; covalent H. 2.3; nonpolar covalent I do not undertand how to do this questiosn. Please help These are also the answer chices I have.1. In its Lewis dot symbol, which element would have four (4) dots? Select one: a.Si b.F c.N d.S 2. Which compound is expected to be soluble in a polar solvent? Select one: a.CH4 b.NH3 c.None of these. d.BF3 3. Which compound is nonpolar? Select one: a.CO2 b.None of these. c.HCl d.H2O 4. In HCN, the formal charge on nitrogen is Select one: a.+1 b.0 c.–1 d.None of these. 5. For the carbonate anion, CO3–2, the number of contributing equienergetic resonance structures is Select one: a.3 b.4 c.1 d. 2How can an atom violate the octet rule? Group of answer choices By having fewer than eight valence electrons. By having an odd number of valence electrons. By having more than eight valence electrons. All of the above can happen.
- Explain Vander Waal type of bonding with examples.1)Which type of bond would be expected in molecule of LiF? A)ionic b) polar covalent c)nonpolar covalent b) none of these 2)which of the following contains a metallic bond? A)NaCI b)SO2 c)Cu-Zn Alloy d) K20 3) which of the following contains an ionic bond? A)NACI b) SO2 C) Cu-Zn Alloy d)CO2A nonmetal that would typically gain 2 electrons when forming a compound would be? a. Sulfurb. Nitrogenc. Magnesium d. Fluorinee. Sodium