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Pre AP Chemistry Chapter 7 & 8: Bonding Homework #2 1. List three characteristics of ionic compounds. How do these characteristics differ from that of covalent compounds? 2. Why do ionic compounds conduct electricity when they are molten or dissolved, but they will not conduct when in solid form? 3. Of what kind of elements are ionic compounds composed?________________________ Covalent compounds?___________________________________ Metallic______________________________________________ 4. A B C D Identify the following compounds as ionic, covalent, or metallic NaCl E H2O CH4 F Steel NH3 G CaCl2 Al2(Cr2O2)3 H SO 5. Compound B has a lower melting temperature than compound A. Compound A dissolves readily in water and conducts electricity. Compound B has poor solubility and no conductivity. Which would be the most likely to be a molecular (covalent ) compound? Explain. 6. Decide whether the following element will gain or lose valence electrons in the process of ionization to obtain an octet. State gain or lose and indicate the number of electrons that will change a. strontium____________ b. nitrogen____________ c. zinc__________ d. bromine_____________ 7. Write the appropriate formula for the ion formed by the elements from question 8. Use a + or a minus sign to indicate what charge the ion assume when electrons are gained or lost a. strontium____________ b. nitrogen____________ c. zinc__________ d. bromine_____________ 8. 9. Write the appropriate electrically neutral Ionic formula formed when the following ions bond with each other. a. sodium and selenium________________________________________ b. tin(II) and chlorine___________________________________________ c. tin(IV) and oxygen___________________________________ Why do ionic compounds break when they are struck? Why do metallic compounds bend rather than break? (See figure 7.12 on page221 of your textbook) Explain. 10. Determine the electronegativity difference between the following pairs of atoms. Predict the most likely type of bond that would form between the two atoms. See electronegativity chart on page 191 of textbook. a. Silicon and oxygen b. Hydrogen and oxygen c. Sodium and fluorine 11. Generalize: the larger the difference in electronegativity the more likely that the bond is a(n)__________ bond. 12. Water is a polar molecule in which one atom has more attraction for the shared electrons. Which atom is most likely the atom that has the greatest attractivity for the electrons?____________ Why?