Chapter 11 Study Guide
Chemical Bonds: The Formation 
of Compounds From Atoms

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1. Define each of the following:
        a) dipole
        b) polar molecule
        c) valence electrons
        d) ionic bond
        e) covalent bond
        f) polyatomic ion
        g) anion
        h) cation

2. Why does covalent atomic radius increase within a family of elements as atomic number increases?

3. What type of element is an element most likely to be if it has both a high ionization energy and a high electronegativity?

4. Which of the following would have the highest ionization energy in Period 4?
        an alkali metal 
        an alkaline metal
        a chalcogen 
        a halogen

5. How does the Br ^- ion differ from the Br atom in terms of radius and number of electrons?

6. How does an atom of potassium (K) and an atom of seleneium (Se) compare in terms of covalent atomic radius, ionization energy, electronegativity, and metallic properties?

7. Where are the metals with the lowest ionization energy found on the periodic table? Where are those with the highest found?

8. Which of the following has the strongest metallic character?
        B     C     Si     Al

9. What are the periodic properties of the elements?

10. What happens an electron is removed from an sodium (Na) atom?

11. Is transfer of electrons associated with ions or molecules?

12. Where are the nonmetals with the highest electronegativities found in the periodic table?

13. What type of bonds are contained in Al₂(SO₄)₃?

14. How are chemical bonds formed?

15. What kind of elements would form an ionic bond with chlorine?

16. Why is the bond between two nitrogen atoms considered to be 100% covalent?

17. What happens to the energy of the system when a chemical bond is formed between two fluorine atoms?

18. Are shared pairs of electrons found in molecules or polyatomic ions?

19. What type of atoms will form a covalent bond?

20. How many lone pairs of electrons are contained in H₂S?

21. Which of the following would contain a nonpolar covalent bond?
            HF         F₂         Br₂O         PH₃

22. How many valence electrons do each of the following have?
            Br     Fe     K     Mg     N     Se

23. How can you tell by looking at a chemical formula whether it has ionic bonding?

24. When there is a reaction between radium atoms and oxygen atoms, what happens to the radium atoms?

25. How many valence electrons in each of the following?
            H₃PO₄             Cr₂O₇ ^2- 

26. During the formation of an ionic bond, which atom will transfer its valence electron(s) to another atom?

27. If the metal loses 2 electrons, what is its new formula?

28. What happens to the radius of a potassium atom when it becomes an ion?

29. What is the relationship between the radius of a positive ion and its parent atom?

30. What is the relationship between the radius of a negative ion and its parent atom?


31. Draw the Lewis Structure for each of the following. 

            P₂                    Cl₂        

            O                    CO₃ ^2- 

            K ⁺                 O ^2-
 
            H₂O                 SiS₂

            SeO₂