CHAPTER 7 READING GUIDE – IONIC COMPOUNDS AND METALS
1. A ______bond is the force that holds two atoms together.
2. Chemical bonds can form by the attraction between the ______nucleus of one atom and the ______electrons of another atom, or by the attraction between positive ______and negative ______.
3. An ______-______structure is a type of diagram used to keep track of ______electrons.
4. A ______ion forms when an atom loses one or more valence electrons in order to attain a ______gas configuration.
5. By losing an ______, the sodium atom acquires the stable outer-electron configuration of ______.
6. It is important to understand that although ______now has the electron configuration of ______, it is not neon.
7. ______atoms are reactive because they lose valence electrons easily.
8. The group ______and ______metals are the most reactive metals on the periodic table.
9. Although the formation of an ______is the most stable electron configuration, other electron configurations can provide some ______.
10. ______, which are located on the right side of the periodic table, easily gain ______to attain a stable outer electron configuration.
11. An ______is a negatively charged ion.
12. The ______force that holds oppositely charged particles together in an ionic compound is referred to as an ______bond.
13. Many ionic compounds are ______, which means that they contain only two different elements.
14. The ______bonds in a compound determine many of its ______.
15. The strong attractions among the ______ions and the ______ions in an ______compound result in the formation of a ______lattice.
16. ______point, ______point, and ______are physical properties of matter that depend on how strongly the particles that make up the matter are ______to one another.
17. ______are charged particles, so whether they are free to move determines whether an ionic compound conducts ______.
18. Both ______compounds in solution and in the liquid state are excellent conductors of ______.
19. An ionic compound whose aqueous solution conducts an electric current is called an ______.
20. Ionic crystals have ______melting points and ______boiling points.
21. During every chemical reaction, energy is either ______or ______.
22. If energy is absorbed during a chemical reaction, the reaction is ______. If energy is released, it is ______.
23. Because chemists around the world need to be able to communicate with one another, they have developed a set of rules for ______compounds.
24. A ______ion is a one-atom ion such as ______or ______.
25. The charge of a monatomic ion is known as its ______number, or oxidation state.
26. The ______number of an element in an ionic compound equals the number of ______transferred from the atom to form the ion.
27. In the chemical formula for an ionic compound, the symbol of the ______is always written first, followed by the symbol of the ______.
28. ______, which are small numbers to the lower right of a symbol, represent the number of ______of each element in an ionic compound.
29. Many ionic compounds contain ______ions, which are ions made up of more than one atom.
30. Because a polyatomic ion exists as a unit, never change ______of the atoms within the ion.
31. If more than one polyatomic ion is needed, place ______around the ion and write the appropriate subscript outside the parenthesis.
32. ______often form lattices in the solid state.
33. The ______sea model proposes that all the metal atoms in a metallic solid contribute their ______electrons to form a sea of electrons.
34. A ______bond is the attraction of a metallic cation for delocalized electrons.
35. In general, ______have moderately high melting points and high boiling points.
36. Metal are ______, which means they can be hammered into sheets, and they are ______, which means they can be drawn into wire.
37. The movement of mobile ______around positive metallic cations makes the metals good ______.
38. An ______is a mixture of elements that has metallic properties.
39. ______steel, ______, and cast ______are a few of the many useful alloys.