AYL Question Set 4
Lesson 5:
How are ionic and covalent bonding similar? How are they different? You should discuss how they bond and what the major differences are in their nomenclature (the way they are named).
Covalent and ionic are two forms of atomic bonds both of which differ in their structure and properties. Firstly, it should be made clear that an atom’s desire is to achieve stability. Most atoms by nature are not balanced electrically. They achieve balance by sharing or transferring their outermost energy level which contains electrons called valence electrons. The number of valence electrons in an atom mostly determines that atom’s or element’s properties.
Now the octet rule says that an atom likes to achieve stability by ensuring they have eight valence electrons in their outermost level. Atoms lose or gain valence electrons to achieve the full outer level and they do this by bonding with other atoms. Atoms can bond with each other as in the case of O2 or with different atoms as in the case of H2O. (Timberlake) Only Hydrogen (H) and Helium (He) like to only have two valence electrons.
Covalent bonds are formed between two non-metals. Non-metals have low electronegativity (Helmenstine) which means
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they lack the ability to attract electrons from one another. In this case they share the same number of their outermost valence electrons with one other. Covalently bonded atoms tend to have low melting and boiling points, have a definite shape, can be found in liquid or gaseous states at room temperature and can generally be broken apart as they are close by to share one another’s electrons. (Timberlake) Covalent bonds are chemically bonded meaning from an energy standpoint (Electron Sharing…) that they are closer together and have less energy hence are more stable than when separated. Two non-metals forming a covalent bond are named using the name of the first element followed by the second element’s name with its ending changed to IDE. When sub-scripts are used, a pre-fix is used for either and/or both to indicate the number of each element’s atoms in the molecule. MONO is the prefix for one (atom) but if the first element named only has one atom, the mono prefix is left out. Examples include the molecules CO2 carbon dioxide and P2O5 diphosphorus pentaoxide. Ionic bonds are formed between an oppositely charged metal and non-metal in a compound for example methane CH4 made up of carbon and hydrogen and hydrochloric acid HCl hydrogen and chlorine. The non-metal attracts or transfers electrons from the metal very easily creating the bond. The electrostatic or “the forces between particles that are caused by their electric charges”. (Helmenstine) classify the positively charged metal because it has more protons than electrons as a cation and the negatively charged electron-attracting non-metal as an anion. Similar to covalent bonds, elements making up ionic bonds seek balance in their outer most valence electron shell but they do this by transferring the electrons rather than by equally sharing them. Ionic bonds have high melting and boiling points, have no definite shape and are found in the solid state at room temperature. (Timberlake) Ionic bonds have an “electro-negativity” above 1.7 (Covalent Bonds vs Ionic Bonds) which means the higher electronegative atom is strong enough to force transfer of electrons. For example, sodium chloride NaCl made up of sodium with an electro-negativity of 3.16 and chlorine with .900 has a difference between them of 2.26 allowing chlorine to easily attract sodium’s one valence electron creating the ionic bond. (Covalent Bonds vs Ionic Bonds) Ionic bonds are also water-soluble and require much more energy than covalent bonds to be broken. To name an ionic bond you start by naming the positively charged metal (cation) which most of the time consists of a monatomic (single atom) element.
Transition metals can form more than one cation so in cases where they are the first element and need to balance the negatively charged anion, you write the name followed by a Roman numeral in parentheses corresponding to the anion they are combined with and which creates for zero charge balance. An example of this would be Copper (II) Sulfide sulfur has sulfur has a 2 – charge. Once you’ve named the cation now it’s time to name the anion. If the anion is not a polyatomic ion as in the case of sodium chloride NaCl, write the name of the cation changing the ending to IDE just as you do with covalent
ions. Polyatomic ions are ionic compounds usually containing three or more elements, usually non-metals like sulfur, chlorine or fluorine bonded to oxygen forming a cation or anion. (Timberlake) Most polyatomic ions are cations with a negative charge and they are written with ATE for a higher oxidation rate as in sulfate SO4 or ITE at the end of their name for a lower oxidation rate as in sulfite SO3. The prefix HYPO is used for the lowest oxidation rate as in hypochlorite ClO and the prefix PER is used for the very highest oxidation rate as in percholate ClO4. (Bodner) It may seem impossible to name polyatomic atoms but the above rules apply to most. There are a few exceptions in the cases of hydroxide OH, cyanide CN and peroxide O2 as they were once thought to be single atom compounds. Citation List: Bailey, Dr. Kristy M. “Naming Ionic Compounds”. Occc.edu. Oklahoma City Community College. n.d. Web. 2 July 2015. Bodner, Dr. “Nomenclature”. Chemed.chem.purdue.edu. Purdue University, n.d. Web. 2 July 2015. Helmenstine, Ann Marie, PhD. “Electrostatic Forces: Definition”. Chemistry.about.com. About.com, n.d. Web. 2 July 2015. n.a. “Covalent Bonds vs Ionic Bonds”. Diffen.com. Diffen.com, n.d. Web. 2 July 2015. n.a. “Electron Sharing and Covalent Bonds”. Chem.ox.ac.uk. University of Oxford, n.d. Web. 2 July 2015. Timberlake, Karen C. and William. Basic Chemistry. Boston: Pearson Learning Solutions. 2014. Print.
This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed.
However, the atoms are arranged a little differently. Two molecules that have this type of relationship are called isomers.
An atom, by definition, is the smallest part of any substance. The atom has three main components that make it up: protons, neutrons, and electrons. The protons and neutrons are within the nucleus in the center of the atom. The electrons revolve around the nucleus in many orbitals. These orbitals consist of many different shapes, including circular, spiral, and many others. Protons are positively charged and electrons are negatively charged. Protons and electrons both have charge of equal magnitude (i.e. 1.602x10-19 coulombs). Neutrons have a neutral charge, and they, along with protons, are the majority of mass in an atom. Electron mass, though, is negligible. When an atom has a neutral charge, it is stable.
Atoms are electrically neutral; the electrons that bear the negative charge are equal in number to the protons in the nucleus
1. What is the difference between Introduction 2. What is the difference between History 3. What is the difference between a's Planning / Preparation 4.
Because they repel they are as far from each other as possible. The two electrons in each of the oxygen-hydrogen bond are not shared equally. They are more strongly attracted to the oxygen. The bond is polar, it has a 'negative part' (the oxygen) and a 'positive part' (the hydrogen).The hydrogen bond is very weak, about ten times weaker than a single covalent bond.
Constitution; one of the main and most noticeable differences between the two documents is that which is known as the Bill of Rights. The Bill of Rights have given the people their own form of freedom. In the Articles of Confederation they solely focused on the people of higher order and the states as separate beings, but in the U.S. Constitution they catered mainly towards the freedom of the people while still establishing law and order. Under the Articles of Confederation, the national government could not impose taxes on the states, the states had to themselves impose the taxes. This however caused the United States to become poor and when the Constitution was written the national government started taxing the states instead of independent taxing in order to increase funds. Lastly, the United States could not impose their own war unless they had authorization from the states to whisk of their own soldiers, they had to ask the states if they could send their men to war, but if the states did not want to send the soldiers there would be no one to defend the nation. In the Constitution, the nation would have only one army where they could wish to send anyone enlisted to
While all atoms of the same element have the same number of protons, it is possible for atoms of one element to have different numbers of neutrons. Atoms of the same element with different numbers of neutrons are called isotopes . For example, all atoms of the element carbon have 6 protons, but while most carbon atoms have 6 neutrons, some have 7 or 8. Isotopes are named by giving the name of the element followed by the sum of the neutrons and protons in the isotope's nucl...
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
This law states that, “when elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties” (textbook). From that, the modern periodic table was born; “each new horizontal row of the table corresponds to the beginning of a new period because a new principal energy level is being filled with electrons” (textbook).
From these properties of bonds we will see that there are two fundamental types of bonds--covalent and ionic. Covalent bonding represents a situation of about equal sharing of the electrons between nuclei in the bond. Covalent bonds are formed between atoms of approximately equal electronegativity. Because each atom has near equal pull for the electrons in the bond, the electrons are not completely transferred from one atom to another. When the difference in electronegativity between the two atoms in a bond is large, the more electronegative atom can strip an electron off of the less electronegative one to form a negatively charged anion and a positively charged cation. The two ions are held together in an ionic bond because the oppositely charged ions attract each other as described by Coulomb's Law.
Examples of positively charged ions are Na+ and Li+ and examples of negatively charged ions are Cl- and F-. The positive ions are called cations and the negative ions are called anions. Highly charged molecules are reflected by their melting point such NaCl which has a melting point of 801◦C. The melting point of sodium chloride is lower than the melting point of magnesium oxide which is 2852◦ C. This is because the magnesium chloride has a higher charge and therefore requires more energy to break there ionic bonds than sodium chloride. This could also be due to the molecules having higher intermolecular forces than the other which causes it to require more energy to break there
Bonds have a number of characteristics that differentiate one issue from another. We are going to define and describe a number of characteristics in detail below.
To start off, learning the Bohr-Rutherford diagrams in grade nine was a very big confusion for me. I had never fully understood how many shells should go around the nucleus nor did I know how to do the many calculations. As I progressed into grade ten, the teachings became easier. The review shows an example such as in the the bohr diagram, a nucleus is in the center, which is a little circle, and following that there are shells surrounding it containing electrons. Each ring can only hold a certain amount of electrons, and so the first shell around the nucleus can hold a maximum of 2 electrons, the next shell is able to hold a maximum of 8 electro...