Enriched Chemical Bonding Project Combined

 Alexis Jones

Period 3 Enriched

Chemical Bonding Project

Chemical reactions are when elements rearrange, combine, or break apart to create a new substance. These new substances occur due to chemical bonds are formed or broken down. Chemical bonds are either ionic or covalent. These bonds involve valence electrons, which make the bonds more stable. Chemical bonding is when bonds use valence electrons to become more stable, and these bonds use certain elements that have similar or different properties.

Valence electrons are the outer electrons in the outer shell of an atom. Atoms like to gain or lose electrons in order to become more stable. When atoms give away something negative, it is in order to become more positive. When atoms gain something negative, it is in order to become more negative. Valence electrons are represented by Lewis do structures. Lewis dot structures represent valence electrons by having the element symbol in the middle of the number of valence electrons for that element. For example calcium has two valence electrons. To become more stable calcium will lose its two electrons to get a positive charge of two.

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Ionic compounds are the bonding of metals with non-metals. The way ionic bonding works is by losing, or gaining valence electrons in order to become more stable. In ionic bonding cations have a positive charge, and these are the metals. Anions have a negative charge, and these are the non-metals. Ionic bonds form by trading their electrons with other elements. In order to form it first you have to identify that your two, or more elements will make and ionic bond. You do this by identifying your metal and non metal. Then you identify the number of valence electrons each element has. Finally you will take your element with the least valence electrons and draw and arrow from each electron to a lonely electron of the other element. Keep in mind that while doing this you want to keep your elements, and the lonely valence electrons side-by-side. For example potassium (K, metal) has one valence electron, and it gives away its electron to fluorine (F, non-metal) which has seven valence electrons in order to become more stable.

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                Covalent compounds are the bonding of non-metals. The way covalent bonding works is by gaining, or losing valence electrons in order to become more stable just like ionic compounds. In covalent bonds anions are used, which are negative electrons that are non-metals. Unlike ionic compounds which give up electrons, covalent bonds form by sharing electrons. In order to form a covalent bond first you have to identify that the two or more elements you are using are non-metals. Then you will put them side by side, and draw their valence electrons around them. Make sure to keep the lonely electrons and elements side-by-side. Once you have this set up you will draw a solid line to each of the lonely electrons connecting them. For example hydrogen (H, non-metal) has one valence electron, and it shares its electron with Iodine (I, non-metal) which has seven valence electrons. This bond makes both of the elements more stable.

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Periodic trends affect bonding, because of how the elements are arranged on the periodic table. For example elements can be arranged by their electronegative, electron affinity, atomic radius, or ionization energy. Electronegative is the atoms ability to attract other bonded atoms. Electron affinity is an atoms ability to attract another atom. The atomic radius is the radius of an elements atom. Ionization energy is the energy it takes to remove an atom from another atom. Other periodic trends are when the attraction of the atoms for the pair of bonding electrons is different, this is polar covalent bonds. Properties in compounds are used to determine the type of bonding and structure, not just the elements being used. These different properties help group elements to make them either more available or less available for bonding.

Bibliography:

"Electronegativity." Electronegativity. Mar. 2013. Web. 17 Nov. 2013.

Jones, Alexis. Bonding & Nomenclature Learning Guide. 11 Nov 2013.

"Trends in the Periodic Table and Bonding." - Periodicity, Polarity and Properties Education Scotland Foghlam Alba. Web. 17 Nov. 2013.

"Valence Electron." The Free Dictionary. Farlex. Web. 17 Nov. 2013.