Harvard Referencing †Citing a Journal Article

Harvard Referencing – Citing a Journal Article Harvard Referencing – Citing a Journal Article The â€Å"Harvard† referencing system – actually a generic term for author-date referencing – is used around the world for citing sources in written work. As such, every college student should know the basics of the Harvard system. In this post, we go over how to cite a journal article using Harvard referencing. However, it’s worth remembering that many institutions have their own in-house versions of this system, so you should always check your style guide before setting to work on a paper! In-Text Citations As the term â€Å"author-date† implies, Harvard citations include the surname of the author and date of publication: Rational reflection need not compromise the status of something as a mystery (Boyer, 2007). If the author is already named in the text, only the year of publication needs to be given: According to Boyer (2007), there are five kinds of mystery. A sixth type of mystery can be found in the mystery spot. [Photo: Sanjay ach]In citations, you also need to give  relevant page numbers when quoting a source directly: Boyer (2007, p. 89) focuses on the metaphysics of how we experience mystery. Multiple Authors When  citing a work with three or more authors, only name the first listed author, followed by â€Å"et al.† (meaning â€Å"and others†). An article by Mark Pagani, Ken Caldeira, and David Archer, for instance, would be cited as: The source of this carbon remains mysterious (Pagani et al., 2006). Reference List All sources cited in your work should be listed in a reference list at the end of your document. This is where you provide full publication information for your reader, with sources listed alphabetically by author surname. For a journal article, the detail required is: Author Surname(s), Initial(s). (Year) Article Title, Full Title of Journal, Volume Number, Issue/Part Number, Page Numbers. The Boyer article used in the example above would therefore appear in a reference list as: Boyer, S. D. (2007). The Logic of Mystery, Religious Studies, vol. 43, no. 1, pp. 89-102. If you’re citing an online version of a journal article, make sure to provide a URL or DOI too, along with a date of last access: Pagani, M., Caldeira, K., and Archer, D. (2006) An Ancient Carbon Mystery, Science, vol. 314, no. 5805, pp. 1556-7. [Online]. Available at jstor.org/stable/20032976 [Accessed 30 March 2016].

Covalent or Molecular Compound Properties

Covalent or Molecular Compound Properties Covalent or  molecular compounds  contain atoms held together by covalent bonds. These bonds form when the atoms share electrons because they have similar electronegativity values. Covalent compounds are a diverse group of molecules, so there are several exceptions to each rule. When looking at a compound and trying to determine whether it is an ionic compound or a covalent compound, its best to examine several properties of the sample.  These are properties of covalent compounds. Properties of Covalent Compounds Most covalent compounds have relatively low melting points and boiling points.While the ions in an ionic compound are strongly attracted to each other, covalent bonds create molecules that can separate from each other when a lower amount of energy is added to them. Therefore, molecular compounds usually have low melting and boiling points.Covalent compounds usually have lower enthalpies of fusion and vaporization than ionic compounds.The enthalpy of fusion is the amount of energy needed, at constant pressure, to melt one mole of a solid substance. The enthalpy of vaporization is the amount of energy, at constant pressure, required to vaporize one mole of a liquid. On average, it takes only 1% to 10% as much heat to change the phase of a molecular compound as it does for an ionic compound.Covalent compounds tend to be soft and relatively flexible.This is largely because covalent bonds are relatively flexible and easy to break. The covalent bonds in molecular compounds cause these comp ounds to take form as gasses, liquids,  and soft solids. As with many properties, there are exceptions, primarily when molecular compounds assume crystalline forms. Covalent compounds tend to be more flammable than ionic compounds.Many flammable substances contain hydrogen and carbon atoms which can undergo combustion, a reaction that releases energy when the compound reacts with oxygen to produce carbon dioxide and water. Carbon and hydrogen have comparable electronegativies so they are found together in many molecular compounds.When dissolved in water, covalent compounds dont conduct electricity.Ions are needed to conduct electricity in an aqueous solution. Molecular compounds dissolve into molecules rather than dissociate into ions, so they typically do not conduct electricity very well when dissolved in water.Many covalent compounds dont dissolve well in water.There are many exceptions to this rule, just as there are many salts (ionic compounds) that dont dissolve well in water. However, many covalent compounds are polar molecules that do dissolve well in a polar solvent, such as water. Examples of molecular compounds that dissolve well in w ater are sugar and ethanol. Examples of molecular compounds that dont dissolve well in water are oil and polymerized plastic. Note that network solids are compounds containing covalent bonds that violate some of these rules. Diamond, for example, consists of carbon atoms held together by covalent bonds in a crystalline structure. Network solids typically are transparent, hard, good insulators and have high melting points. Learn More Do you need to know more? Learn the  difference between an ionic and covalent bond,  get  examples of covalent compounds, and understand how to predict formulas of compounds containing polyatomic ions.