The Buying decision process Essay Example for Free

The Buying decision process Essay Consumer behavior is term used to describe the manner of how an individual buys and assesses a product or service. It also includes the internal or the mental processes and external or social processes that might affect the individual’s conduct (Consumer Behavior 2008). Figure 1. The Buying Decision Process Source: Bowens, Kotler Makens (2003) Purchasing products like buying grocery supplies seems like a mundane activity but a buyer actually foes through several stages of decision making before eventually making the purchase. It will all start with the problem recognition. A problem arises when the current status or condition does not coincide with the preferred one (Marketing Communications 2008). The awareness of this situation can be caused by an internal stimulus, like feeling thirsty and needing to buy a drink, or an external factor, like advertising of a store for a sale (Buyer Behavior 2008). The consumer may or may not continue to the next stage unless there is a strong desire to improve the condition or fulfill the need (Principles of Marketing 2008). Once the consumer decides to fulfill the need, the stage of information search occurs. At this stage the consumer seeks out options to be able to solve the problem at hand. It involves internal and external types. Internal search usually occurs with frequently bought items. The consumer just simple remembers past positive experience with the product (Principles of Marketing 2008). The weakness of this type is when the information stored in the memory is limited or the person is having a hard time remembering, the risk of making an incorrect decision is most likely (Consumer Behavior 2008). On the other hand, the sources for the external types are personal sources like relatives and friends, public sources like reports, commercial sources like ads and lastly experiential sources acquire through experiencing the product (Buyer Behavior 2008). The challenge for any marketing team is to identify how their target audience source product information. After which make sure that the information is always available and can be easily accessed (Principles of Marketing 2008). The information obtained during the second stage will then be evaluated in the alternative evaluation stage. The information will be put into set of options or evoked set (Consumer Decision Process 2008). The evoked set is the set of brands a consumer consider while in the decision process (Marketing Communications 2008). From the second stage the consumer acquired the criteria he/she is looking for and got the brand names that meet those criteria (Consumer Behavior 2008). This process limits the choices for the consumer, making it easier for them to make the final decision of purchasing the product or getting the service. The fourth stage of the process, purchase decision, now involves the actual purchase of the product. Since the consumer now knows what to buy in this stage, he decides where, when and how to purchase the product of choice (Marketing Communications 2008). During this process, three methods of purchase may be used by the consumer: fully-planned, partially planned, and unplanned. Fully-planned purchases are purchases where the customer picks out the merchandise and brand ahead of time. This method is usually used with high risk purchases like buying a house or car. In partial purchase there is a plan to buy a product but to what specific brand is decided later on. Finally, an unplanned purchase is a spur of the moment acquisition (Consumer Decision Process 2008). Although the consumer is already thinking of buying a product, this could still be altered at the point of purchase itself. Factors that could affect it are the store surroundings, time constraint, incentives offered in the store like a sale, product availability, and budget constraint. It is then important for the seller to make sure that these events are anticipated and avoided (Principles of Marketing 2008). Stores could make sure that the stocks are sufficient, the store is clean and the personnel are trained to provide good shopping experience, promotions like sales are position at the right moment, and that products are well organized and can be easily found. Following the purchase will be the consumption of the product and the consumer will enter the last stage of the process which is post-purchase evaluation. In this stage, the consumer will assess if the purchase solved the problem identified in the first stage. He/she will determine if satisfaction was provided by the action (Consumer Behavior 2008). Otherwise, the customer will feel cognitive dissonance, which is an unpleasant feeling or tension produced by thinking about two conflicting ideas. This is a state where the consumer stresses on the thought that the other choice should have been selected (Buyer Behavior 2008). Cognitive dissonance could result to product returns, viewing the product in a negative way or not considering the product as part of the evoked set in the future (Principles of Marketing 2008). Companies can prevent this situation by providing good after sale service to customers. For example. free technical support to electronic device like computers. Other methods are follow-up calls and market research. As shown above the decision making process of consumers is actually a complex process that involves many steps and could be influenced by different factors. The whole process could take a few minutes for simple purchases but could take weeks for important purchases. It is then a good tool for businesses to understand what happens in each stage to be able to present their product favorably to the consumer.

Black Americans Essay -- American History

Black Americans Black Americans are those persons in the United States who trace their ancestry to members of the Negroid race in Africa. They have at various times in United States history been referred to as African, coloured, Negro, Afro-American, and African-American, as well as black. The black population of the United States has grown from three-quarters of a million in 1790 to nearly 30 million in 1990. As a percentage of the total population, blacks declined from 19.3 in 1790 to 9.7 in 1930. A modest percentage increase has occurred since that time. Over the past 300 and more years in the United States, considerable racial mixture has taken place between persons of African descent and those with other racial backgrounds, mainly of white European or American Indian ancestry. Shades of skin colour range from dark brown to ivory. In body type black Americans range from short and stocky to tall and lean. Nose shapes vary from aquiline to extremely broad and flat; hair colour from medium brown to brown black; and hair texture from tightly curled to limp and straight. Historically, the predominant attitude toward racial group membership in the United States has been that persons having any black African ancestry are considered to be black. In some parts of the United States, especially in the antebellum South, laws were written to define racial group membership in this way, generally to the detriment of those who were not Caucasian. It is important to note, however, that ancestry and physical characteristics are only part of what has set black Americans apart as a distinct group. The concept of race, as it applies to the black minority in the United States, is as much a social and political concept as a biological one. Blacks Under Slavery: 1600-1865 The first Africans in the New World arrived with Spanish and Portuguese explorers and settlers. By 1600 an estimated 275,000 Africans, both free and slave, were in Central and South America and the Caribbean area. Africans first arrived in the area that became the United States in 1619, when a handful of captives were sold by the captain of a Dutch man-of-war to settlers at JAMESTOWN. Others were brought in increasing numbers to fill the desire for labour in a country where land was plentiful and labour scarce. By the end of the 17th century, approximately 1,300,000 Africans had landed in the New World... ...r education for blacks, and for the first time black students began to appear in colleges that had previously been all white. In the 1970s the percentage of blacks attending college increased markedly, but in the 1980s blacks lost ground. Although desegregation of the public schools in the South proceeded slowly for the first decade after the Brown v. Board of Education decision, by 1969 school districts in every state were at least in token compliance with the 1954 ruling. By that time all forms of de jure segregation had been struck down by the courts. De facto school segregation continued, however, in large part because the communities the schools served were segregated in their residential patterns. This was particularly true in large urban areas and more prevalent in the North than in the South. One method adopted to overcome such segregation was to bus children across school district lines in order to achieve racial balance in the schools. This caused major controversy and led to instances of violent opposition . The overwhelming majority of black children now attend formally integrated schools, although they may have little contact with white pupils even within the schools.

Acquisition of knowledge Essay

Aims: 1. To foster acquisition of knowledge and understanding of terms, concepts, facts, processes, techniques and principles relating to the subject of Chemistry. 2. To develop the ability to apply the knowledge of contents and principles of Chemistry in new or unfamiliar situations. 3. To develop skills in proper handling of apparatus and chemicals. 4. To develop an ability to appreciate achievements in the field of Chemistry and its role in nature and society. 5. To develop an interest in activities involving usage of the knowledge of Chemistry. 6. To develop a scientific attitude through the study of Physical Sciences. 7. To acquaint students with the emerging frontiers and interdisciplinary aspects of the subject. 8. To develop skills relevant to the discipline. 9. To apprise students with interface of Chemistry with other disciplines of Science, such as, Physics, Biology, Geology, Engineering, etc. CLASS XI There will be two papers in the subject. Paper I: Theory- 3 hours Paper II: Practical – 3 hours Project Work Practical File †¦ 70 marks †¦20 marks †¦ 7 marks †¦ 3 marks Main postulates of the theory. Its limitations. Modern atomic theory. Laws of chemical combinations: Law of conservation of mass. Law of definite proportion. Law of multiple proportion. Law of reciprocal proportion. Gay-Lussac’s law of gaseous volumes. Statement, explanation and simple problems based on these laws. (ii) Atomic and isotopic masses. The atomic mass unit is one of the experimentally determined unit. It is equal to 1/12 of the mass of the carbon 12 isotope. (iii) Chemical equivalents, volumetric calculations in terms of normality. C = 12.00 should be taken as a standard for expressing atomic masses. Equivalent weight expresses the combining capacity of the elements with the standard elements such as H, Cl, O, Ag, etc. Variable equivalent weight. Gram equivalent weights, r elationship between gram equivalent weight, gram molecular weight and valency. Determination of equivalent weight of acids, alkalis, salts, oxidising and reducing agents. (experimental details not required). 128 PAPER I –THEORY – 70 Marks There will be one paper of 3 hours duration divided into 2 parts. Part I (20 marks) will consist of compulsory short  answer questions, testing knowledge, application and skills relating to elementary/fundamental aspects of the entire syllabus. Part II (50 marks) will be divided into 3 Sections, A, B and C. Candidates are required to answer two out of three questions from Section A (each carrying 10 marks), two out of three questions from Section B (each carrying 5 marks) and two out of three questions from Section C (each carrying 10 marks). Therefore, a total of six questions are to be answered in Part II. SECTION A 1. Atoms and Molecules (i) The concept of atoms having fixed properties in explaining the laws of chemical combination. The study about the atoms. Dalton’s atomic theory: Terms used in volumetric calculations such as percentage (w/w and w/v), normality, molarity, molality, mole fraction, etc. should be discussed. Students are required to know the formulae. Simple calculations on the above topics. (iv) Relative molecular mass and mole. The following methods may be considered for the determination of relative molecular masses for the gases: the molar volume method; Victor Meyer’s method (experimental details not required). Numerical problems based on the above method and Victor Meyer’s method. Mole concept, Avogadro’s number and numerical problems on mole concept. Gram molecular volume. (v) Chemical Reaction calculations based mass-volume and relationships. Self explanatory. 2. Atomic Structure (i) Electrons, Protons and Neutrons as fundamental particles, their charges and masses. Concept of indivisibility of atom as proposed by Dalton does not exist. The atom consists of subatomic fundamental particles. Production of cathode rays and their properties. Production of anode rays and their properties. Chadwick’s experiment for the discovery of neutron and properties of neutron. (ii) Rutherford’s nuclear model based on the scattering experiment. Rutherford’s nuclear model of atom. Rutherford’s scattering experiment. Discovery of nucleus. Defects of Rutherford model. (iii) Bohr’s atomic model. 1. Postulates of Bohr’s theory – based on Planck’s quantum theory. 2. Numericals on Bohr’s atomic radii, velocity and energy of orbits (derivation not required). 129 – Stoichiometric on mass-mass, volume-volume 3. Defects in the Bohr’s Model. (iv) Atomic structure: wave mechanical model-  a simple mathematical treatment. Quantum numbers; shape, size and orientation of s and p orbitals only. Hund’s rule of maximum multiplicity. Pauli’s exclusion principle, Aufbau principle, electronic configuration of elements in terms of s, p, d, f subshells. †¢ Wave mechanical model – experimental verification of wave nature of electron. †¢ de Broglie’s equation. Numericals. †¢ Heisenberg’s Numericals. uncertainity principle. †¢ Quantum numbers – types of quantum numbers, information obtained in terms of distance of electron from the nucleus, energy of electron, number of electrons present in an orbit and an orbital. †¢ Pauli’s exclusion principle. Shape, size and orientation of the s and p subshells. †¢ Hund’s rule of maximum multiplicity. †¢ Aufbau principle, (n+l) rule. †¢ Electronic configuration of elements in terms of s, p, d, f subshells. 3. Periodic Table (i) Atomic number (Proton number) as the basis for classification of the elements in the Periodic Table. IUPAC nomenclature for elements with Z> 100. Mendeleev’s periodic law, defects in the Mendeleev’s periodic table. Advantages and disadvantages. Modern periodic law (atomic number taken as the basis of classification of the elements). Extended and long form of periodic table. General characteristics of groups and periods. Division of periodic table as s, p, d and f blocks. (ii) Extra nuclear structure as the basis of periodicity. Some idea of the following: ionisation enthalpy, electron gain enthalpy, atomic radius, atomic volume, electronegativity, etc must be given. The periodicity of electronic structure leading to the periodicity of elements e.g the relative ease of ionisation of elements. †¢ Periodic properties such as valence electrons, atomic volume, atomic and ionic radii and their variation in groups and periods. †¢ The idea of ionisation enthalpy, electron gain enthalpy and electronegativity must be given and their variation in groups and periods may be discussed. †¢ The factors (atomic number, atomic volume and shielding effect, the number of electrons in the outermost orbit) which affect these periodic properties and their variation in groups and periods. (iii) Periodicity of elements with reference to s, p, d and f block elements. Classification of elements on the basis of s, p, d, f block elements and also on the basis of their complete and incomplete electron shells. Study of the periodicity of properties  mentioned in point (ii) in terms of s, p, d, f blocks and the governing factors in terms of the block characteristics. 4. Chemical Bonding Electrovalent Bond (i) Electrovalent or ionic bond e.g formation of NaCl, Li2O, MgO, CaO, MgF2, and Na2 S. Cause of chemical combination, Octet rule, types of chemical bonds. Electrovalent formation of NaCl, Li2O, MgO, CaO, MgF2, and Na2S. Properties of ionic compounds. Electron dot structure of the following ionic compounds: NaCl, Li2O, MgO, CaO, MgF2, and Na2S must be taught in detail. (ii) Factors influencing the formation of ionic bond, e.g electron gain enthalpy, ionisation enthalpy, lattice energy and electronegativity. The conditions necessary for the formation of ionic bonds such as: low ionisation enthalpy of metals. high electron gain enthalpy of non-metals. high lattice energy. All these points must be discussed in detail. (iii) The relation between the ionic bonding and Periodic Table. The relationship between the formation of cations and anions of the atoms and their positions in the periodic table should be discussed. Correlate the periodic property and the position of the elements in the periodic table to show the ease of formation of anions and cations and electrovalent and covalent compounds. (iv) Variable electrovalency and its causes. Variable electrovalency; reasons for variable electrovalency i.e, due to inert electron pair effect, by using suitable examples. Covalent Bond (i) Covalent bond, sigma and pi bonds e.g. formation of ammonia, nitrogen, ethene, ethyne, and carbon dioxide. Resonance. Definition of covalent bonding, conditions for formation of covalent bonds, types of covalent bonds i.e single, double and triple bonds. Sigma and pi bonds. H2, O2, N2. Classification of covalent bonds based on electronegativity of atoms – polar and non polar covalent bond, dipole moment, formation of CH4, H2O, NH3, ethane, ethene, ethyne and CO2, etc. and their electron dot structure or Lewis structure. Characteristics of covalent compounds. Comparison in electrovalency and covalency. Resonance in simple inorganic molecules like ozone, carbon dioxide, carbonate ion and nitrate  ion. (ii) Variable valency: chlorine exhibits the valency of 1,3,5 & 7 respectively. Variable valency, cause of variable covalency e.g. chlorine exhibits the valency 1, 3, 5 and 7 respectively. Discuss in terms of atomic structure. Variable covalency of phosphorus and sulphur may be discussed. Discuss in terms of atomic structure. (iii) Deviation from Octet rule and Fajan’s rules. Definition of Octet rule. Failure of Octet rule, due to either incomplete octet or exceeding of Octet with suitable examples. Fajan’s rules: Statements. Conditions for electrovalency and covalency must be discussed. Polar and non polar bonds should be correlated with Fajan’s rules. (viii) Molecular orbital theory, Qualitative treatment of homonuclear diatomic molecules of first two periods. Energy level diagrams, bonding, antibonding molecular orbitals, bond order, paramagnetism of O2 molecule. Relative stabilities of O2, O2-, O2- – , O2+, O2++ Self-explanatory. 5. The Gaseous State (i) The gas laws, qualitatively. kinetic theory treated (iv) Co-ordinate or dative covalent bond, e.g.  formation of oxy-acids of chlorine. Co-ordinate or dative covalent bonding: definition, formation of hypochlorous acid, chloric acid, perchloric acid, ammonium ion, hydronium ion, nitric acid, ozone – structural formulae of the above molecules based on co-ordinate bonding. (v) Hydrogen bonding: its essential requirements, the examples of hydrogen fluoride, water (ice), alcohol, etc may be considered. H-bonding – definition, types, condition for hydrogen bond formation, examples of inter-molecular hydrogen bonding in detail taking hydrogen fluoride, water and ice and ethanol into account. Intramolecular hydrogen bonding. (vi) Metallic bonding, Van der Waals’ forces. Metallic bonding – Electron sea model and band model. Explanation of metallic properties in terms of metallic bonding. Van der Waals’ forces and its types. (vii)Valence Shell Electron Pair Repulsion Theory; Hybridisation and shapes of molecules: hybridisation involving s, p and d orbitals only; sigma and pi bonds. Concept of electron-pair repulsion and shapes of  molecules taking methane, ammonia and water as examples. Hybridisation and molecular shapes – definition, hybridization of orbitals involving s, p and d orbitals (examples: ethane, ethene, ethyne, PCl5 and SF6). Characteristics of gases, comparison between solid, liquid and gas. Properties of gases on the basis of kinetic theory of gases. Laws of gases – Boyle’s Law, Charles’ Law, Absolute Temperature, Pressure Temperature Law, Avogadro’s Law. Simple numerical problems based on the above laws. Postulates of Kinetic Theory must be discussed to explain gas laws. (ii) PV = nRT or PV= (w/M)RT and the application of this equation of state. Ideal gas equation PV = nRT; its application in calculation of relative molecular mass and in the calculation of the value of R. (iii) Non ideal behaviour of gases and Van der Waals’ equation. Non ideal behaviour of gases i.e. deviation from gas laws may be discussed at low and at high temperature and pressure. Van der Waals’ equation (P + a/V2) (V-b) = RT for one mole of a gas. The pressure correction and volume correction may be explained. (iv) Dalton’s law, the Avogadro constant, the mole, Graham’s law of diffusion, simple numerical problems on the above. †¢ Dalton’s Law of partial pressure. †¢ Application of Dalton’s Law. †¢ Numerical problems based on the above law. †¢ Avogadro’s constant. †¢ Relationship between the mole and Avogadro number. Graham’s Law of diffusion and its application. †¢ Simple numerical problems on the above. 6. Colloidal Solutions Preparation and properties of colloids, both lyophilic and lyophobic colloids. Precipitation as evidence that the colloidal particles are charged. Idea of gold number is required, but application of gold number is not required. The importance of large surface area in adsorption should also be appreciated. †¢ †¢ †¢ †¢ †¢ Thomas Graham classified the substances as crystalloid and colloid. Classification of substances on the basis of the particle size i.e. true solution, sol and suspension. Colloidal system is heterogeneous. Lyophilic and lyophobic colloids. Classification of colloidal solutions as micro, macro and associated colloids. Preparation of lyophilic colloids. Preparation of  lyophobic colloids by colloid mill, peptisation, Bredig’s arc method (procedural details not required) by oxidation, reduction, double decomposition and exchange of solvent method should be discussed. Purification of colloids (dialysis, ultra filtration, and ultracentrifugation). Properties of colloidal solutions such as Brownian movement, Tyndall effect, coagulation and protection (protective colloids), should be discussed. Gold number and Hardy Schulze rule. Application of colloids in life. Electrophoresis (movement of dispersed phase). Emulsions, surfactants, micelles (only definition and examples). 8. Chemical Energetics (i) Introduction. (a) Scope of thermodynamics- characteristics of thermodynamics. (b) Types of system – ideal system, real system, isolated system, closed system, open system. (c) Meaning of surrounding. (d) Properties of the system: macroscopic, intensive and extensive properties of the system. (e) State of the system. (f) Main processes the system undergoes: reversible, irreversible, adiabatic, isothermal, isobaric, isochoric, cyclic. (g) Meaning of thermodynamic equilibrium. (h) Meaning of thermodynamic process. (ii) First law of Thermodynamics mathematical statement. and its (a) Idea of conservation of energy – total energy of the system and the surrounding. (b) Meaning of internal energy of the system and change in internal energy of the system. (c) Meaning of work done by the system and by the surrounding at constant temperature. (d) Meaning of heat absorbed by the system and by the surrounding at constant temperature. (e) The sign convention for change in internal energy, heat given out or gained, work done by the system or by the surrounding. (f) State function and path function- meaning with examples. (g) Internal energy change, work done and heat absorbed in a cyclic process. (h) Internal energy change in an isolated system and in non isolated system. 7. Chemical Kinetics Rate of a chemical reaction, basic idea of order and molecularity of a reaction. Rate of a chemical reaction; Relation between order and the stoichiometric coefficients in the balanced equation; Meaning of molecularity. Differences between the order and molecularity of the reaction. Physical significance of entropy State function and not path function. Relationship between adiabatic change and entropy. Entropy change of the universe and a reversible isothermal process. Entropy change of the universe and irreversible process. Meaning of thermal death. Meaning of energy content and work content (free energy) of the system – thermodynamic quantity – state function. Types of work and meaning of the two types of work. Meaning of Helmholtz’s Free energy and Gibb’s free energy and the change in Gibb’s and Helmholtz’s free energy. Relationship between Gibb’s free energy and Helmholtz’s free energy. Simple calculation on the change in Gibb’s free energy and Helmholtz’s free energy. Relationship between change in Gibb’s free energy and equilibrium constant of a chemical reaction. Change in Gibb’s free energy in reversible, irreversible, isobaric and isochoric processes. Based on change in Gibb’s free energy, defining the criteria for the spontaneity of a change in terms of entropy and enthalpy; defining the limits for reversible chemical reactions. (k) Chemical change and internal energy. (l) Need for enthalpy – constant pressure or open vessel processes. (m) Enthalpy a thermodynamic property – state function. (n) Mathematical form constant pressure. (iii) Ideas about Heat, Work and Energy. Heat – the energy in transit.  Condition for the transfer of heat. Limitation in conversion of heat into work. Condition at which heat transfer ceases. Unit of heat. Meaning of energy – capacity to do work. Meaning of work – intensity factor and capacity factor. Types of work. Mathematical form of reversible work. Mathematical form of irreversible work. Difference between the reversible and irreversible work done – graphically. Adiabatic reversible expansion. Relationship between Cv and internal energy change.

Phidias - Free Essay Example

Sample details Pages: 2 Words: 585 Downloads: 3 Date added: 2017/09/23 Category Advertising Essay Type Narrative essay Did you like this example? Andrew Reyes Ancient Humanities Professor Hubbs July 22, 2010 Phidias The name Phidias will be remembered for the rest of time. Phidias was a sculptor born around 490 BC. Phidias is often recognized as a the most renown ancient Greek sculptors. While there are no originals of his work remaining, his reputation has been made well known through various writings. Most of the writings give praise to Phidias. His two greatest contributions came from sculptures; one of Athena, and the other of Zeus. Phidias was a man recognized for his talents, it is a shame that this generation or generations to come will never get to see his work first hand. Phidias’ work on Athena was marveled upon for centuries. Phidias’ colossal statue of Athena was housed in the Parthenon and was displayed the symbol of Athens. It is believed that the statue was damaged in several fires and eventually was burned beyond repair around the fifth century. The statue was believed to be of great st ature and heavy in gold. The sculpture was assembled on a wooden core, covered with shaped bronze plates covered in turn with removable gold plates, save for the ivory surfaces of the goddesss face and arms; the gold weighed 44 talents, the equivalent of about 2,500 pounds (1,100 kg); the Athena Parthenos embodied a sizeable part of the treasury of Athens (Phidias, 2010). † The Second contribution was similar to Athena. Zeus was erected in the temple of Zeus in approximately 432 BC. Similar to Athena it was a chryselephantine, meaning that is was both gold and ivory. At one point Zeus’ statue was considered one of the Seven Wonders of the World. In 1954 a great discovery was found; the location of Phidias’ workshop was found in Olympia. â€Å"Tools, terracotta moulds and a cup inscribed ‘I belong to Phidias’†¦ This has enabled archaeologists to re-create the techniques used to make the great work and confirm its date. (Phidias, 2010)† Phidias’s hard work and dedication to the gods allowed the statue to be well regarded throughout all of Greece. Phidias was not limited to the two sculptures; he also helped create other works of art. Phidias directed and supervised the construction of the temple [Parthenon] over a period of more than ten years†¦ (Fiero, 2006). † The Parthenon is where the statue of Athena was erected, and is believed to have been a remarkable site to see when it was intact. Phidias also contributed a tribute to Marathon. Marathon ran 26 miles to Athens to tell of Greece’s win over the Persians. â€Å"Fragments remain of his [Phidias] work on the Parthenon friezes and commemorative works of the battle of marathon (Sheldon, 2010). Phidias works have helped shape architecture to what it is today. Even in the earliest of times Phidias was able to construct marvels such as the Parthenon, the Statue of Athena, and the Statue of Zeus. His sculpture skills and architecture abiliti es have led him to be one of the most influential artists to have ever walked the face of the earth. It would be hard to say that there is an architect or an artist today that has not been influenced in some way by the great Phidias. ? Bibliography Eddy, S. (1977). The Gold in the Athena Parthenos . American Journal of Archaeology , 107-111. Fiero, G. K. (2006). The Humanistic Tradition. New York: Mcgraw-Hill. Phidias. (2010). Retrieved July 22, 2010, from Wikipedia: https://en. wikipedia. org/wiki/Statue_of_Zeus_at_Olympia Sheldon, N. (2010, June 28). Phidias: The Most Famous Scupltor of Ancient Greece. Retrieved July 22, 2010, from Suite101. com: https://archaeology. suite101. com/article. cfm/phidias-the-most-famous-sculptor-of-ancient-greece Don’t waste time! Our writers will create an original "Phidias" essay for you Create order