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FAQs
Unit
2
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Lecture
Questions |
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Help!
I'm reading the study guide and question 12, Unit
2-15, lists a number of compounds and asks whether
they're formed by ionic or covalent bonds, I have
no idea how to determine this! |
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Is
there an atom with a complete outer shell, and
if so, what type of bond does it form with other
atoms of the same type? |
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Why
does an electron leave the outer shell of one
atom and go to another? Is there a greater "attraction"
somewhere? |
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One
Student noted a chemistry resource she found helpful:
Introduction to Chemistry for Biology Students,
7th Edition, by Sackheim: The Benjamin/Cummings
Publishing Company, Inc. This is located in the
bookstore under the ELI BIO 141 section
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Top
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Enzyme
Laboratory Questions |
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During
this experiment, the paper towel did not rise
to the surface on glass 5 (No H2O2). I started
over with new yeast, thinking I had taken too
long and my yeast had "died." I even tried using
different temperatures of water. But got the same
results. Has anyone else had the same results/problem?
|
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How
do I write the chemical equation that shows hydrogen
peroxide breaking down into water and oxygen gas?
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Top
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Help!
I'm reading the study guide and question 12, Unit
2-15, lists a number of compounds and asks whether
they're formed by ionic or covalent bonds, I have
no idea how to determine this!
The video on bonding develops this idea in detail.
Thus, I would first suggest that if at all possible
watch the video. However, here is the short
answer; maybe this will get you on the right
track. If the electron affinities of the atoms
are the same or similar, the bond type in the
molecule is a covalent bond. If the electron
affinities of the two atoms are very different,
the bond type will be ionic. In order to determine
this, you need to know how many electrons are
in the outer shell of each atom.
Ionic
bonds are formed between two atoms when one
of the atoms has a relatively low affinity for
electrons (only 1, 2, or 3 electrons in the
outer shell) and the other has a relatively
high affinity for electrons (5, 6, or 7 electrons
in the outer shell). Thus, the atom type with
a low affinity for electrons will donate electrons
to the atom with a high affinity for electrons.
If the electron affinities of the atoms are
the same or similar, the bond type in the molecule
is a covalent bond.
All
the diatomic molecules (such as O2 and Cl2)
are formed by covalent bonds since the atoms
in the molecule are atoms of the same element
and have exactly the same number of electrons
in their outer shells and hence the same affinity
for electrons. In addition, atoms that have
an intermediate number of electrons in their
outer shells often form covalent bonds with
atoms of other elements. A prime example of
this is carbon that has four electrons in its
outer shell. In this course, we will assume
that any carbon containing compound is formed
by covalent bonds (true in the vast majority
of cases).
When
I try to predict the bond type, I first determine
whether the molecule is a diatomic molecule
(atoms in the molecule are of atoms of the same
element) or is a carbon containing molecule
(assume that if the molecule contains carbon
atoms the bond type is covalent). If either
of these situations is the case, the bond type
is covalent. If that is not the case, then you
must diagram the atoms. One needs to know the
atomic numbers of each atom in order to do this.
If the pattern is atom A with 1, 2, or 3 electrons
in its outer shell and atom B with 5, 6, or
7 electrons in its outer shell, then one would
predict that the atoms are united by an ionic
bond.
Top
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Is
there an atom with a complete outer shell, and if
so, what type of bond does it form with other atoms
of the same type?
Yes, There are atoms with complete outer shells.
Any atom with an atomic number of 2 or 10 has
a complete outer shell for example (He: atomic
number of 2; Ne: atomic number of 10). Remember
there are 2 electrons in the first shell, eight
in the second, eight in the third (able to accommodate
up to 18 but will be stable with 8).
For
a look at all the elements that are nonreactive
(inert) because their outer shell is filled,
look at the periodic table at this site: http://pearl1.lanl.gov/periodic/default.htm
All the atoms of elements in the far right column
are inert. Since these atoms all have a filled
outer shell they don't react with other atoms.
Thus, except for helium (with an atomic number
of 2 and 2 electrons in its outer shell), all
the inert elements have atoms with 8 electrons
in their outer shell. Since these atom types
are nonreactive, they will not play a role in
our study of biochemistry. However, it is important
to understand why the inert atoms are inert
(this idea when turned around helps one understand
why atoms do react -namely to obtain a filled
outer shell). If this idea still doesn't seem
crystal clear to everyone, be sure to watch
videos #1 and #2.
Top
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Why
does an electron leave the outer shell of one
atom and go to another? Is there a greater "attraction"
somewhere?
Atoms
that donate electron(s) donate because they
have a relatively low affinity for electron(s)
compared to the atom that "steals" the electron
away. Atoms with 1, 2, or 3 electrons in their
outer shell tend to be electron donors to atoms
with 5, 6, or 7 electrons in their outer shell.
The general rule: An atom with low electron
affinity loses its electron(s) to atom types
with a high electron affinity. Again, videos
#1 and #2 deal with this in detail. Also, study
sections 2.6 through 2.8 in your text and steps
43-50 in the inorganic program in the Study
Guiide (pages Unit 2 - 8 and 9).
I
don't understand how to determine the location
in which atoms are bonding within structural
formula. For example: In the structural formula
for Glucose, the first carbon is double bonded
to oxygen and the third carbon has the hydrogen
and hydroxyl opposite the other carbons. How
is this determined? In question 15 of Unit 2-21,
you noted that fructose differs from glucose
only because the second carbon is double bonded
rather than the first carbon. Again, I don't
understand how to determine this.
You
do not need to memorize the structural formula
for glucose - it will be given to you; you just
need to be able to recognize that it is glucose
and to understand what the lines represent in
a structural formula (a pair of shared electrons).
You would not be required to determine that
fructose is structurally different from glucose
because of the position of the double bonded
oxygen on the carbon chain. This was pointed
out to emphasize the importance of structural
formulas in biochemistry - subtle differences
in molecular configuration can result in totally
different compounds. You should be able to look
at a structural formula and determine if it
is possible, i.e., carbon always shares 4 pairs
of electrons so note that four lines (represents
4 covalent bonds) always comes away from carbon.
Also, you should know that oxygen in organic
compounds will share two pairs of electrons
(hence 2 lines) and hydrogen 1 pair. Objectives
15 and 16 discuss the differences between molecular
and structural formulas and why structural formulas
are important in biochemistry. As you continue
in biochemistry, you will find out that it is
the SHAPE of a molecule that often dictates
its function (a great example of that in this
unit is enzyme activity).
Top
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One
Student noted a chemistry resource she found helpful:
Introduction to Chemistry for Biology Students,
7th Edition, by Sackheim: The Benjamin/Cummings
Publishing Company, Inc.
This
is located in the bookstore under the ELI BIO
141 section.
Yes, some students do find it helpful. I would
suggest viewing the tapes before purchasing
more books however - the tapes will help to
focus your attention on the points that are
essential in this course. Basically, you don't
need to become a biochemist for this course;
you just need enough biochemistry so that the
cell physiology you encounter later in the course
is understandable! If after viewing the tapes,
you are still confused, call me at ELI or, if
possible, make an appointment to discuss the
points you are having difficulty with. Also,
all students that are taking a course at ELI
can use the campus tutoring service. Call the
campus nearest you to find out more about tutoring
if you think you need a tutor.
Top
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.
During this experiment, the paper towel did not
rise to the surface on glass 5 (No H2O2). I started
over with new yeast, thinking I had taken too long
and my yeast had "died." I even tried using different
temperatures of water. But got the same results.
Has anyone else had the same results/problem?
One
would NOT expect the towel to rise in the glass
that lacked hydrogen peroxide. Why? Think about
why the towel is rising in the glasses where
it does rise. Reread the last paragraph on page
Lab 3-5. Underline the last three sentences
in the paragraph and reread them. Why did you
do an experiment that lacked hydrogen peroxide??
Who can answer this?
Top
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How
do I write the chemical equation that shows hydrogen
peroxide breaking down into water and oxygen gas?
In
a chemical reaction the reactants (starting
materials) are on the left side of the ARROW
(not an = sign) and the products (what is obtained
at the end of the reaction) are on the right
side of the arrow. Thus, the reactant, hydrogen
peroxide, is on the left side of the arrow and
the products, oxygen gas and water, are on the
right side of the arrow. The enzyme, catalase,
is written on top of the arrow. This indicates
that the enzyme is not changed by the reaction.
Note that the yeast cells are the SOURCE of
the catalase. The equation for this reaction
is written in the blanks on Exercise IIIA#4
and Exercise IV#1.
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