Download CHAPTER 7 READING GUIDE – IONIC COMPOUNDS AND METALS

Survey
yes no Was this document useful for you?
   Thank you for your participation!

* Your assessment is very important for improving the work of artificial intelligence, which forms the content of this project

Document related concepts

Aromaticity wikipedia, lookup

Auger electron spectroscopy wikipedia, lookup

Degenerate matter wikipedia, lookup

Heat transfer physics wikipedia, lookup

X-ray photoelectron spectroscopy wikipedia, lookup

Atomic orbital wikipedia, lookup

State of matter wikipedia, lookup

Ionization wikipedia, lookup

PH wikipedia, lookup

Stability constants of complexes wikipedia, lookup

Electron scattering wikipedia, lookup

Ion source wikipedia, lookup

Metastable inner-shell molecular state wikipedia, lookup

Electrochemistry wikipedia, lookup

Solid wikipedia, lookup

Ionic liquid wikipedia, lookup

Rutherford backscattering spectrometry wikipedia, lookup

Homoaromaticity wikipedia, lookup

Nanofluidic circuitry wikipedia, lookup

Electron configuration wikipedia, lookup

Chemical bond wikipedia, lookup

Ionic compound wikipedia, lookup

Ion wikipedia, lookup

Transcript
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.