10-2 Intensive Chemistry Review for Test covering Chapters 3 - 4.2 (UPDATE: 4.3 WILL NOT
BE INCLUDED ON THIS TEST)
Look carefully over your notes, handouts, and the text. Work through the summaries and end-ofchapter problems and test prep (noting in the study guide which concepts you may skip.)
3.1
1.You are not responsible for the law of definite proportions or the law of multiple proportions.
2. You should be able to describe in your own words, and apply to related situations (a) the law of
conservation of mass, and (b)Dalton's atomic theory.
3. You should be able to outline Dalton's atomic theory and identify how our understanding of the atom
has changed since his time. Which parts are no longer accepted as correct? What discoveries contradict
those parts of Dalton's theory?
4. What is atomic mass? What unit is it measured in? What is 1 atomic mass unit defined as being
exactly equal to? (hint: see figure 3-8)
5. What is a mole? How is it used? How big is it? (What is the value of Avogadro's number?) Could
you hold a mole of grains of salt in your hand? How about a mole of cells? A mole of water molecules?
3.2
6. Look at figure 3-12 (p. 83). What discovery came out of the cathode ray experiment? How did the
discovery of cathode rays affect Dalton's atomic theory?
7. Look at figure 3-14 (p. 84). What did scientists learn about the atom from the gold foil experiment?
8. How does the size of the nucleus compare to the size of the electron cloud (and the overall size of the
atom)? How does the mass of the nucleus compare to the mass of the overall atom?
9. For protons, neutrons and electrons, identify their location in an atom, symbol, charge (+1,0,-1),
approximate mass in amu (1 or 1/2000). (See table 3-2).
10. Compare atomic mass and atomic number. What does each measure?
11. Coulomb's law describes the relationship between the strength of the attraction (or repulsion)
between 2 charged objects. What happens to the strength of attraction as two oppositely charged objects
are moved closer to one another? How does the repulsion of a +1 ion and a +1 ion compare to that of a
+2 ion and a +2 ion at the same distance apart?
12. What is an isotope? Is every atom of a given element an isotope of that element? How do the mass
and structure of two different isotopes of carbon differ from one another? (ex: carbon-12 and
carbon-13)
13. What is a radioisotope? How is it different from other isotopes?
3.3
14. Visible light is only one small part of the electromagnetic spectrum. Given a diagram like the one
shown in fig 3-20 (p. 92), identify which has a longer wavelength – infrared or microwaves? Which has
more energy – red light or blue light? Which type of electromagnetic radiation shown has the highest
energy?
15. Study fig 3-22 and 3-23 on pp. 94-95. The light is produced by a hydrogen lamp. Why are there
only very specific wavelengths of light being emitted? What does this mean? If a white light were
shined through the device (3-22), what would the would the pattern of light look like?
16. What is meant by “ground state” and “excited state” when referring to electrons?
16. You are NOT responsible for knowing or using the equation on p. 95 for the energy of electrons.
17. What is meant by the statement that each electron has a unique 4-part quantum address around a
nucleus? (You do NOT need to memorize table 3-4 on p. 97)
18. The principle quantum number (n level) is essentially like the “rings” of the earlier atomic models.
It typically is numbered between 1 and 7 for the ground state of any electron. Each increase in levels
(from 1 to 2 to 3...) leads to an increase in the number of sublevels. The first 4 sublevels are named
___, ____, ____, ____.
19. How many orbits can be in each sublevel?
How many electrons can be in any orbital?
What must be true for two electrons to be in the same orbital?
20. Review rules for filling the electron orbitals (filling in orbital filling diagrams and electron
configurations). (pp. 98-100, plus “Hog Hotel”)
Pauli exclusion principle:
Aufbau principle:
Hund's rule:
How can you use the periodic table to figure out an electron configuration?
How do you use the “Noble gas shortcut” for writing an electron configuration?
Chapter 4.1
21. Several people were working to organize the known elements into some sort of structure at the
same time (mid-1800s). Why is Mendeleev given the major credit for discovering the periodic table?
(What did he do that was so special – even audacious?!)
22. What is the periodic law? What does it mean?
23. Mendeleev ordered the elements by increasing ______________, while the modern periodic table is
organized by increasing _________________.
24. Know the following terms and locations relating to the periodic table: group, family, period,
transition metals, main group elements, metalloids, active metals, non-metals, rare earth metals, alkali
metals, halogens, noble gases, alkaline earth metals, hydrogen.
25. Why is hydrogen often considered to be in a family by itself?
Chapter 4.2
26. List several common characteristics of metals, compared to non-metals. What is the most
significant characteristic of metals?
27. What must an electron be able to do in order for a material to be considered conductive? Why are
some electrons in metals so much more able to do this than electrons around non-metals?
28. You are NOT responsible for the discussion of metal crystals (pp. 129-131) or of super conductors
(132-133).
UPDATE (1/23): QUESTIONS 28-30 WILL NOT BE INCLUDED ON THE TEST
28. What is meant by a periodic trend? (Remember back to the periodic law?)
29. What are the 2 major processes going on within and between atoms that are the major causes of
many periodic trends? How does this relate back to Coulomb's law?
30. What is meant by “electron shielding”?
30. Describe and explain the major reasons for each of the following trends:
- atomic radii
- ionization energy
- electron affinity
(You do NOT need to explain the boiling point/melting point trends)