CHEMISTRY
CHAPTER 10 (THE MOLE) READING GUIDE
Pp.319-357
1.Chemist created the(atom/molecule) counting unit called the _______ because atoms are so small and too
numerous to count directly.
2.a)The mole is the SI (metric) unit used to measure ______________________.b) What is its
abbreviation?
C) One mole is defined as the number of ________ atoms in exactly _____ g of pure
__________. d) A mole of anything contains 6.02 x 1023 representative particles, which is called
_______________ ____________. e) A representative particle is any kind of particle such as an _____,
a molecule, a formula unit, an __________, or an ________.
3. Study fig 10.2; the representative particle(rep part) in a mole of water is the water ___________, the rep
part in a mole of copper is the copper _______, and the rep part in a mole of sodium chloride(NaCl) is the
NaCl _________ ________.
4. To convert from moles to particles and particles to moles, we will use ______________ analysis; if you
remember properly, a ______________ factor, which is a ratio of equalities, is used in the conversion.
5. Fill in the blanks with the two conversion factors that can be used _________________________ and
_______________________. Remember that the unit you want to cancel will be at the bottom of the ratio.
6. Copy the example in the book that shows how to convert from moles to particles(molecules, atoms, ions,
etc); *see bottom of p.322* 3.50 mol sucrose x ______________________= 2.11 x 1024 molecules sucrose
7. The next page shows how to convert particles to moles; (fill in properly written just like you did above)
2.11 x 1024 molecules sucrose x ___________________________ = 3.50 mol sucrose
*8. Class work practice problems (p323)- #1-3 & study ex prob 10.1 on p324; practice problems#5,6.
9.a) Define molar mass –
b) The molar mass of any element is numerically equal to its ________ _______ and has the units
___________.(atomic mass unit”amu” from periodic table)
10. What is the conversion factor used to convert moles to mass?
11.Copy the example at the bottom of page 327; 3.00 moles of Cu x ____________________=191g Cu
*12.Study ex prob 10.2- class work practice problems (p328)#15,16
13. What is the conversion factor used to convert mass to moles?
*14.Study ex prob 10.3-class work practice problems(p329)#17,18
15. To convert mass to atoms or atoms to mass, the first step, of the two- step problem, is to convert the given
to ___________ , in the words(see fig 10.8)the ________ is at the center of the conversion problems.
*16. Study ex prob 10.4 & 10.5* Class work practice problems(p331)#19-21
17. Study fig 10.9; Given one molecule of ‘CCl2F2’ (usually called Freon);a) how many atoms of each element are
in the formula?
C___, Cl___, F____.b)what is its atomic ratio?
*18. In the ex prob 10.6, the ratio between the moles of a __________ and the moles of individual ______ is
necessary for calculations. *Class work practice problems(p335)#29-32
19. The mass of a mole of a compound equals the _______ of the masses of all the _____________ that
make up the compound. *study the book’s breakdown of the mass of potassium chromate*
*20. Class work practice problems(p335)#34-36; (p336)#37,38; (p337)#40
21. Study ex prob 10.7 & 10.8-mole to mass and mass to mole conversion problems.
22. To convert the mass of a compound to the number of particles you must first convert to ________ first.
*study ex prob 10.9
*23. Class work practice problems(p338)#42-45
24. Read fig 10.11; this flow chart shows that the _______ is in the central position in the diagram. *FYI-there
is another flow chart called the mole road b/c the mole is at the central crossroad of the diagram.
25. a) Define percent compositionb)Write the equation for percent by mass = ________________________________
26.Read fig 10.12- What is the difference between a synthetic chemist and an analytical chemist?
*27. Study ex prob 10.10; class work practice problems (p344)#54-57
28.a) Define empirical formula b) The empirical formula may or may not be the actual ___________ formula.c) Fig 10.13 shows that
you can always assume that you have a _____g sample of a compound, therefore 40.05% becomes 40.05g.
*29. Study ex prob 10.11; class work practice problems(p346)#58-61
30. Define molecular formula31. Compare/contrast acetylene and benzene.
32.a)To convert empirical formula to __________ formula, you must multiply the coefficients in an empirical
formula times ‘n’.b) Finish the equation; n = ___________________________.* Study fig 10.15
*33. Study ex prob 10.12 & 10.13; *class work practice problems(p350)#62-64
34. a) What is a hydrate?
B)The usual coloring of an opal gemstone is the result of _________________________.
35. How is an anhydrous compound formed?
36. What are the 2 major uses of hydrates?