Bioscience Assignment

This document provides information on Bioscience Assignment. It covers topics such as equilibrium reactions, Le Chatelier's Principle, hemoglobin and oxygen transport, carbon dioxide transport, and different types of chemical bonding.

Running Head: BIOSCIENCE ASSIGNMENT 1
Bioscience Assignment
Student’s Name
Institutional Affiliation

BIOSCIENCE ASSIGNMENT 2
PART A
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a)
For a reaction at equilibrium, the concentrations/quantities of the reactants and products
is a constant. The rate of forward reaction is equal and opposite to that of backward reaction
(De Nevers, 2012, p. 217). For this to happen, the reaction must take place in a closed
system.
b)
Increasing the quantities of oxygen will shift the reaction to the right.
c)
Increasing the quantities of HbO in the equilibrium will shift the reaction to the left.
d)
The reaction will shift to the right.
e)
Le Chateliers’s Principle.
According to this principle, when a disturbance is created in a reaction in equilibrium, the
reaction will shift in such a manner as to counteract the effect of this disturbance (Pauling, 2014,
p. 409-410). A disturbance can be created by changing the concentrations of either the reactants
or products, change in temperature or pressure.
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Kc= [ HbO ]1
[ Hb ]
1
[ O ]
1

BIOSCIENCE ASSIGNMENT 3
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Kc= [ 6.93× 10−1 ]1
[ 2.27 ×10−8 ]1
[ 9.5 ×10−2 ]1
Kc= [ 6.93× 10−1 ]1
2.1565 ×10−9
Kc=3.21 ×108
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When the value of Kc is very large, it is an indication that the equilibrium
will favor the forward reaction and hence more of the products will be formed.
This type of can be termed as complete. However, when the value of Kc is very
small, it is an indication that the equilibrium will favor reverse reaction and hence
more of the reactants will be formed. Where the value of Kc approaches or is close
to 1, it indicates that the concentrations of both the reactants and products is close
to the same. The reaction may proceed in either way or the other. It’s called a
reversible reaction (Helmenstine, 2019).
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The molecules of the reacting energy must collide with sufficient kinetic
energy so that they can break the bonds between the molecules. Heat can be added
to increase kinetic energy. Additionally, the atoms must collide in the correct
direction/orientation so that the reaction can take place. If this two criteria are met,
a reaction will take place.
PART B
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BIOSCIENCE ASSIGNMENT 4
Hemoglobin is a protein that is contained in the red blood cells. It carries
oxygen from the lungs to the body cells and also carries carbon dioxide from the
cells to the lungs for eventual expulsion from the body (Ronald, 2016, p. 67).
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The ions responsible are iron ions i.e. Fe2+. This is a cation since it has a
positive charge. These irons ions react chemically react with the oxygen. This
reaction reads to the formation of Oxyhemoglobin. These ions can form two bonds
u i.e. they provide the site for the attachment of the oxygen molecules to the
hemoglobin.
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Oxygen has the ability to dissolve in blood. This oxygen can be transport to
various cells in the body for metabolism. However, the percentage of oxygen
transported this way is too small to meet the overall body demand for oxygen. For
this reason, oxygen require a different way of transportation within the body.
Hemoglobin provides the site for the attachment of the oxygen molecules. The iron
ions present in hemoglobin facilitate this process. About 98.5 % of all oxygen is
transported this way.
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Presence concentration of oxygen in the lungs causes hemoglobin in the
blood combines with this oxygen to form oxyhemoglobin. As the concentration of
oxygen increases and pressure increases, the reaction moves to the right with an
aim of establishing an equilibrium by reducing the concentration of oxygen
(Abithira, 2013).

BIOSCIENCE ASSIGNMENT 5
The reverse reaction takes place in the tissue cells. Here, the concentration
of oxygen is at a reduced level and pressure is low. Due to this factor,
oxyhemoglobin is decomposed with an aim of re-establishing the equilibrium
(Abithira, 2013). This results in more of the reactants being formed and hence
oxygen is transferred to the tissue cells for use in metabolism.
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Carbon dioxide can dissolve into the blood plasma and be transported this
way. About 7% of it is transported this way. Carbon dioxide can also be
transported by binding on to the hemoglobin protein. The compound formed is
called carbaminohemoglobin (Feher, 2018, p. 427-438). This reaction is reversible.
When this compound reaches the lungs, the reverse reaction is favored resulting
into the formation of carbon dioxide and hemoglobin. Lastly, carbon dioxide can
be transported as a bicarbonate ion. A majority of the oxygen is transported this
way. Carbon dioxide is converted into carbonic acid which decomposes into
bicarbonate ions and is transported this way (Feher, 2018, p. 427-438).
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CO2 (g) + H2O (aq)  H2CO3 (aq)  H+(aq) + HCO3-(aq)
The carbonic acid formed is very unstable. It immediately decomposes to
bicarbonate a hydrogen ions. This rapid process creates a concentration gradient
for the absorption of more carbon dioxide. This process allows for the
transportation of carbon dioxide with little PH change in the blood. Additionally,
it helps regulate carbon dioxide when pressure changes due to altitude hence
maintaining body PH.
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BIOSCIENCE ASSIGNMENT 6
An increase in the levels of carbon dioxide favors the forward reaction as
the system tries re-establish the equilibrium. More of the Carbonic acid is therefore
formed. Consequently, due to the rapid decomposition of the carbonic acid results
into the release of hydrogen ions above the normal rate. Since not all hydrogen
ions will bond to the hemoglobin, the increased concentration of hydrogen ions in
the blood above the normal will lowers the PH of the blood i.e. it becomes acidic.
This will alter the metabolic rate in the body tissue cells resulting to a persons
health deteriorating rapidly, causing injury and in severe cases, death can occur
(Lumen Learning, n.d.).
PART C
1.
In solids, particles are closely pack to each other and the intermolecular force of
attraction is very high. The result is that solids have a definite shape and volume.
When heated, the particles close to the source of heat vibrate and the kinetic energy
increases. These particles collide with those close to then hence transferring the
kinetic energy. If the heat supplied is large enough, resulting kinetic energy may
reduce the effective force of attraction between particles resulting in a change of
state to liquid. This is called melting. In liquids, particles are further away from
each other as compared to solid but lesser compared to gases. The force of
attraction between particles is low. When heated sufficiently, the kinetic energy
developed leads to the weakening of the force of attraction and the particles are
held even further away. In this state a gas is formed. The force of attraction
between particles in gases is very lower and particles are in constant motion. When
heated, they particles are spread further apart resulting in an increase in volume
(Seager & Slabaugh, 2011).
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BIOSCIENCE ASSIGNMENT 7
Ionic bonding takes place when the valence electrons of an atom are
transferred to another atom. The electron donor becomes positively charges and the
acceptor negatively charged (Frederick & Ladd, 2016, p. 215-226). Occur between
metals and non metal compounds. Covalent bonds on the other hand occur when
the valence electrons are shared between two or more atoms.
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Ionic: Sodium Chloride, NaCl.
Giant Ionic bond
Covalent: Hydrogen Molecule, H2
Giant covalent bond
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Polar covalent bonds occurs when an electro pair is not shared equally
between atoms. An example is a water molecule. Electrons are attracted more to
one atom than the other due to greater electronegativity (Frost, Deal & Timberlake,
2011, p. 186-192). Nonpolar covalent bonds occur when two atoms share their pair
of electrons together e.g. in a hydrogen molecule.
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Polar; Water, H2O
Nonpolar; Hydrogen molecule, H2
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London dispersion forces are the weakest force of attraction. This force of
attraction is temporary. It occurs when electrons in two adjacent atoms form a
temporary dipole. They are Van der Wall forces. The forces are altered with

BIOSCIENCE ASSIGNMENT 8
change in temperature. For nonpolar compounds, when temperature is reduced,
they cause them to either condense or freeze (Purdue, n.d.).
Dipole-dipole forces occur when there is temporary charge formation within
molecules. The positive end of a molecule is attracted to the negatively charged
end of another molecule. Are intermolecular forces of attraction and occur in polar
molecules.
Hydrogen bonds is a temporary electrostatic force. It’s a dipole-dipole force
of attraction. Occurs when hydrogen is attracted to strong electronegative elements
such as nitrogen (Ivar, 2017, p. 111-119). The donor is the more electronegative
atom while hydrogen is the acceptor. Are strong intermolecular forces of attraction.
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In our example, we chose a water molecule as a type of a polar compound.
These types of molecules experience the dipole-dipole force of attraction. Water
molecules form dipoles due to induction of charges resulting in the molecules align
in such a way that the negatively charges end of one water molecule is attracted to
the positively charged end of another water molecule.
For the non-polar molecule, we chose the hydrogen molecule. These type of
molecules experience London dispersion forces. The hydrogen atoms in a
hydrogen molecule are covalently bonded. This is intramolecular. Hydrogen atoms
develop temporary dipoles which create an intramolecular force of attraction i.e.
London dispersion forces, which is weak.
References

BIOSCIENCE ASSIGNMENT 9
Abithira. (2013, May 07). Grade 12U Chemistry-Sysytems and Equilibrium. Retrieved from
Grade 12U Chemistry Website:
https://fmss12ucheme.wordpress.com/2013/05/07/hemoglobin-equilibrium-2/
De Nevers, N. (2012). Physical and Chemical Equilibrium for Chemical Engineers. Hoboken,
New Jersey: John Wiley & Sons, 217.
Feher, J. J. (2018). Quantitative Human Physiology: An Introduction. Academic Press, 427-438.
Frederick, M., & Ladd, C. (2016). Bonding, Structure and Solid-state Chemistry. Oxford: Oxford
University Press, 215-226.
Frost, L. D., Deal, S. T., & Timberlake, K. C. (2011). General, Organic, and Biological
Chemistry: An Integrated Approach. New York: Pearson, 186-192.
Helmenstine, A. M. (2019, January 26). Equilibrium Constant Kc and How to Calculate It.
Retrieved from ThoughtCo. Website: https://www.thoughtco.com/equilibrium-constant-
606794
Ivar, O. (2017). Wonders of Water: The Hydrogen Bond in Action. Hackensack: World Scientific
Publishing, 111-119.
Lumen Learning. (n.d.). Transport of Carbon Dioxide in the Blood. Retrieved from Lumen
Learning Website: https://courses.lumenlearning.com/wm-biology2/chapter/transport-of-
carbon-dioxide-in-the-blood/
Pauling, L. (2014). General Chemistry. New York: Dover Publications, 409-410.
Purdue. (n.d.). London Dispersion Forces. Retrieved from Chem Purdue:
https://www.chem.purdue.edu/gchelp/liquids/disperse.html
Ronald, P. N. (2016). Regulation of Tissue Oxygenation (2nd ed.). Princeton: Biota Publishing,
67.
Seager, S. L., & Slabaugh, M. R. (2011). Introductory Chemistry for Today. Belmont: Cengage
Learning Inc.

BIOSCIENCE ASSIGNMENT
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