Chapter 6 Review.
Vocabulary
Section 6.3
Match each word to the sentence where it best
fits.
Section 6.1
supernova
macronutrients
trace amounts
trace element
electronegativity
periodic
ionization energy
atomic radius
1. You’ll need a significant amount of
_____________ if you want to stay healthy.
2. In a _____________ most of the elements in
your body were created.
3. While necessary for life, too much of any one
_____________ can be toxic.
4. Almost every element on the periodic table
can be found in our bodies in ________.
5. The changing of the seasons is an example of
a _____________ shift in weather patterns.
6. There is a phenomena called the photoelectric
effect in which shining a light with high
energy photons on a metal can cause the metal
to eject electrons. Those photons must have
energy equal to or greater than the
____________ of the atoms of that metal.
7. If I want to find an element which will strip
electrons from another element during a
chemical reaction, then I want one with a high
_______________.
8. The _____________ of an atom is a result of
the size of the largest orbital occupied by its
electrons.
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electron configuration
Lewis dot diagrams
valence electrons
9. By knowing the ________, it gives us deeper
knowledge of the structure of the atom.
10. You find ________ at the highest principle
energy level of an atom.
11. When trying to figure out a chemical formula,
it is helpful to use ________, a visual
representation of the outermost electrons.
Conceptual Questions
Section 6.1
12. What were the two most abundant elements
created in the Big Bang?
13. If only two elements were created in the Big
Bang (with trace amounts of two other
elements), where did the rest of the elements
on the periodic table come from?
14. Describe the distribution of metals, nonmetals, and metalloids on the periodic table.
15. All elements higher than atomic number 92
are not found mineral ores, because they don’t
have any stable isotopes. Without a supernova
here on Earth to create heavier elements, how
were these elements discovered?
16. Explain what is meant by the phrase: “You are
made from star dust.”
17. Which element in your body was most likely
created early in the birth of our universe?
a. hydrogen
b. oxygen
c. carbon
d. nitrogen
A NATURAL APPROACH TO CHEMISTRY
18. Describe what is meant by an “essential
element.”
19. If you don’t eat a well rounded diet, it may be
necessary for you to take mineral supplements
often found in multi-vitamins. These can help
provide you with, necessary trace elements
that may be missing from your diet. Explain
why it would not be good to take too many
multi-vitamins at one time.
20. Name two functions performed by essential
elements in your body.
Section 6.2
26. One of the most dangerous radioactive
isotopes to get into your body would be some
radioactive version of strontium. Strontium
tends to be incorporated into your bones and
teeth, instead of passing through your system
quickly. Why does it make sense that
strontium would be captured by your bones
and teeth given the family of elements
strontium belongs to?
27. Chlorine gas was once used as a chemical
weapon. Using the periodic table suggest
another gaseous element that may also be
dangerous and explain why you chose this
element.
28. Explain the difference between
electronegativity and ionization energy.
21. Given the collection of objects above, come
up with at least one table that organizes them
according to their properties of shape, size,
and color - a periodic table of objects.
22. There are three missing objects that would
complete your table. Describe the properties
of size, shape, and color for these missing
objects.
23. How did density and reaction patterns help
Mendeleev to create the first periodic table?
24. When Mendeleev first started looking for
patterns in elements, he arranged the elements
first in order of increasing atomic mass. How
is this different from how we would order
elements today?
25. What makes a group of elements a “family?”
29. Compare and contrast the periodic properties
of atomic radius, electronegativity, and
ionization energy. What is similar and what is
different in how these properties map to
elements on the periodic table?
Section 6.3
30. Which sub-atomic particle most directly
affects the properties of an atom or molecule?
a. proton
b. neutron
c. electron
31. Explain the reasoning behind your choice for
the question above.
32. If the primary energy levels for electrons are
represented by numbers such as 1, 2, 3, 4, etc.,
what letters are used to describe the energy
sublevels (or orbitals) within these primary
levels?
33. What are two differences between a 1s and 2s
orbital? How about a 2p and 3p orbital?
A NATURAL APPROACH TO CHEMISTRY
193
Chapter 6 Review.
34. In what order will the electrons fill up the
orbitals?
a. They will fill the lowest energy ones first.
b. They will fill the highest energy ones first.
c. The orbitals are filled in a random order.
Quantitative Problems
35. Fill in the table below to show which type of
orbital is being filled by the highest energy
electron in each of the large block of elements.
41. Of the 4.40 x 1028 atoms in a typical person,
3.96 x 1027 of them are nitrogen. What
percent of a typical person’s atoms are
nitrogen?
Section 6.1
40. If a carbon-12 atom fused with a helium-4
atom, what would the resulting new atom be?
42. Of the 4.40 x 1028 atoms in a typical person,
8.80 x 1020 of them are iodine. Why is iodine
considered to be found in “trace amounts”
when the typical person has 880 billion billion
atoms of iodine in his or her body?
36. Of all the electrons surrounding the nucleus,
why are the valence electrons considered to be
the most important?
37. What is the best predictor of an element’s
chemical properties?
a. Atomic radius.
b. Density.
c. Number of valence electrons.
d. Its full electron configuration.
38. What is the relationship between the size of an
orbital and the energy level of electrons found
in that orbital?
43. Place the following elements in the
appropriate place on the periodic table outline
shown below.
a. Hydrogen
b. Helium,
c. Potassium,
d. Krypton,
e. Copper
f. Boron,
g. Calcium,
h. Phosphorus
i. Iron,
39. Carbon can form the following two
compounds: carbon dioxide (CO2) and
methane (CH4). This means that:
a. The number of valence electrons on
carbon atoms can vary.
b. The number of valence electrons of
hydrogen and oxygen must be different.
c. Carbon always has the same number of
valence electrons.
d. Both b and c are true.
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A NATURAL APPROACH TO CHEMISTRY
44. Which of the following atoms has the biggest
radius?
a. H or He
b. Li or Be
c. He or Ne
d. Na or Mg
e. O or S
49. Given the graph below, what would you
estimate would be the melting point of
titanium (Ti)?
Section 6.2
45. How many electrons can fit in an orbital?
46. Write the electron configuration for the
following elements.
a. Nitrogen (N),
b. Neon (Ne),
c. Sodium (Na),
d. Boron (B),
e. Iron (Fe),
f. Chlorine (Cl).
47. Give electron configurations both the full and
short version for each of the following
elements:
a. Silicon (Si),
b. Molybdenum (Mo),
c. Cesium (Cs),
d. Uranium (U).
48. What are the similarities and the differences in
the electron configurations of the following
pair of atoms?
a. Ne and Kr
b. F and Cl
c. Li and Na
d. O and N
e. C and Si
A NATURAL APPROACH TO CHEMISTRY
Section 6.3
50. How many electrons can be at primary energy
level 3? Explain why.
51. How many valence electrons does each of the
following elements have?
a. Kr,
b. F,
c. Na,
d. Al,
e. Br,
f. Zn.
52. Draw a Lewis dot structure for each of the
following elements:
a. N,
b. Ne,
c. Kr,
d. Na,
e. O
f. Be,
g. Xe,
h. F,
i. Li
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