Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Ionic bonding and its properties
Ionic bonding and its properties
Differences between Ionic and Covalent Compounds page 123
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Ionic bonding and its properties
How can placing 2 different compounds in water baths with increasing temperatures reveal whether they are ionic or covalent from their melting points?
Hypothesis:
According to what I have learned, I believe that the compound that melts first must be covalent whilst the compound that takes longer to melt will be ionic. This is due to the fact that ionic compounds have higher melting points. This is because the electrostatic connections that hold the compounds together are incredibly strong. This means that the positive and negative charges from the metal and nonmetal are incredibly attracted to one another and form very sturdy bonds that require a lot of energy to break apart. This means that a higher temperature with more energy will be necessary
…show more content…
An ionic compound is defined as “a chemical compound of cations and anions which are held together by ionic bonds in a lattice structure”. This basically means that a compound is formed when the transfers of electrons occur from metal loosing electrons and becoming cations/+ (to achieve a complete outermost shell) and non-metals gaining electrons and becoming anions/- (to complete their outermost shell). These ions of opposite charges are powerfully attracted to one another and form very tight bonds. Covalent compounds are formed when two or more non-metal atoms bond by sharing valence electrons to complete their outermost shell. Valence electrons are the spare electrons on the outermost shell and are always the ones involved in bonding. Atoms share these electrons to achieve the noble gas structure and this is why ionic compounds give/take electrons as well. Some characteristics of ionic compounds would be: that it includes metals bonding with nonmetals, the positive/negative charges, its crystal lattice, the fact that it is non malleable, their high melting points, they conduct electricity (only if molten or dissolved), they are soluble in water and that they are solid at room temperature. Some characteristics of covalent bonds would be: that it occurs between 2 nonmetals; elements share electrons in molecules; low melting points (due to their weak bonds) and the fact that they are usually gases, sometimes liquids and rarely solids at room
Covalent compounds are formed when two or more non-metals react together. The covalent compound is actually made of molecules, and the name given depends on the structure of these molecules. Prefixes, like di- for two, tri- for three, tetra- for four, and so forth, are frequently used. Thus, NO2 is nitrogen dioxide and N2O4 is dinitrogen
Our first goal in Project 7 was to determine what our three unknown solutions were. We did this through a series of tests. Our first test was a series of anion tests. We performed anion tests to determine whether any of the following anions were present in our solution: chloride, sulfate, nitrate, carbonate, and acetate. Our first solution, labeled as B, had only the chloride test come out positive. The next solution, C, tested positive for acetate, as did our last solution, E. We next performed anion tests. These included flame test, as well as an ammonium test. For the flame test, certain cations turn flames different colors, so we used this knowledge to test to see which cations could be present in our solutions. During this test, the only solution that appeared to turn the flame any color was solution C, which turned the flame bright orange, indicating the sodium ion was present. This led us to the conclusion that solution C was sodium acetate. We next performed an ammonium test, which involved mixing our solutions with sodium hydroxide, and smelling the resulting solution in order to detect an ammonia smell. Solution B was identified as smelling like ammonia, indicating the presence of the ammonium cation. From this, we identified solution B as ammonium chloride. We next checked the pH of all three of the solutions, first by using litmus paper. Solution C was slightly basic, solution E and B were both acidic, with a pH around 4. Since we knew that solution E had acetate, and was acidic, and did not turn the flame any color, we determined it was acetic acid, as none of the ions in acetic acid would turn a flame any color.
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
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.
•melting points of the chemical elements displayed on a miniature periodic tableMelting point: 171.6 [or -101.5 °C (-150.7 °F)] K
Electrical conductivity refers to a substances ability to carry moving electrons (conduct electricity). In order to do so, there must be a supply of delocalised electrons. While in a solid state, ionic substances can not conduct electricity as there are no delocalised electrons or free/mobile ions to act as charge carriers. In an aqueous ionic solution, the H2O molecules break apart the crystal lattice structure of the ionic substance into individual ions, surrounding each ion in a jacket of hydration. Below is the equation that describes the dissociation of NaCl when in H2O solvent.
Hydrogen sulphide has a boiling point of -82 degrees Celsius and a melting point of -60 degrees Celsius. There are 2 hydrogen and 1 sulphide molecule. Simple molecule’s which are covalent have lower melting and boiling points as they do not need too much energy to separate the bonds because they are as polarised as water. In hydrogen sulphide the intermolecular forces are known as Dipole-Dipole forces which are less powerful than hydrogen bonding which is in water therefore water has the strongest bond compared to hydrogen chloride and hydrogen sulphide. Water is more electronegative than hydrogen chloride and hydrogen sulphide because there are more molecules in water which are drawn together however in hydrogen sulphide there are less molecules
CHEMTUTOR ACIDS AND BASES. (n.d.). CHEMTUTOR ACIDS AND BASES. Retrieved February 16, 2014, from http://www.chemtutor.com/acid.htm
The Periodic Table is based around the Atomic Theory. Firstly people believed that everything was made up the four elements Earth, Fire, Wind, and Water. This theory evolved into everything being made up of atoms. Breakthroughs throughout history such as the discoveries of the nucleus, protons, neutrons and electrons have pushed this theory forward to where it is today.
In the other hand, Sucrose (C12H22O11) and Dextrose (C6H12O6) are covalent bonds because they were not hard, they were not conductors and they also had a very low melting point. The data indicates that Sodium Chloride (NaCl) and Sodium Sulfate (Na2SO4) are ionic bonds, whereas Sucrose (C12H22O11) and Dextrose (C6H12O6) are covalent bonds because of their properties. As a result of the ionic compound properties, we determined that NaCl has has a high conductivity than C12H22O11, because NaCl is ionic compound meaning that it can light up the light bulb. Because we know the properties of each bonds, we can determine what Unknown 1 and 2 is. Unknown 1 resulted as not hard, not a conductor, and had a low melting point. Because of this, we can tell that is a covalent bond because it has the properties of it. Unknown 2 also resulted as not hard, is a conductor, and has a high melting point. With this data, we know that it is a ionic covalent because the properties match with the given. One source of error may have been that we might added a lot of water into the beaker. This error would have affected our data because it would have given us the wrong results when doing the conductivity test. For example, we accidently put too much water, so Sodium Sulfate (Na2SO4) turned out as not a conductor, when it has to be a
The alkaline earth metals form many compounds that are commonly found in nature. The ionic bonds these metals form with the halogen family are called metal halides. These bonds are not solely ionic; they can be a covalent bond in the case of beryllium. Additionally, all of the alkaline metals, except beryllium, can react with water to form alkaline hydroxides, compounds containing the hydroxide ion. However,...
When we place two objects with different temperatures in contact with each other, the heat from the hotter object will immediately and automatically flow to the colder object. This is known as conduction. Some objects make excellent conductors of heat while others make poor conductors of heat or excellent insulators. Silver, copper, and gold make excellent conductors of heat. Foams and plastics make good insulators of heat but make poor conductors. Last night for dinner, I made myself a grilled cheese sandwich and a bowl of tomato soup. I heated the soup faster than I cooked the sandwich so I poured the hot soup into a bowl and finished cooking the sandwich. Once I was done cooking, I gabbed the soup bowl and burned my hand. The heat from the soup made the bowl hot. This is an example of conduction.
Heterocyclic chemistry is the branch of chemistry dealing with the synthesis, properties and applications of heterocycles. The name comes from the greek word “heteros” which means “different”. Any of a class of organic compounds whose molecules contain one or more rings of atoms with at least one atom (the heteroatom) being an element other than carbon, most frequently oxygen, nitrogen, or sulfur [1].
The periodic table, used worldwide by scientists, teachers and students, for quick location of information about elements. The periodic table did not come by overnight though, the periodic table is a table formed from years of work, on the atomic structure. It all started years back with Democritus and his discovery of the atom. This was followed up by John Dalton many years down the track, after elements had been discovered Dalton attempted to create a way to make the elements easier to remember. 84 years later, JJ Thomson discovered electrons, which were key to the periodic table, and in 1889, Dmitri Mendeleev invented the periodic table. Years later Henry Moseley worked out how to measure atomic numbers of elements, and just 9 years after Neil Bohr explained the structure of the atom which further explained why Mendeleev had placed each element in a specific row or column. Finally James Chadwick discovered the neutron in 1922.
For centuries, many scientists and researchers have pondered on the idea of combining two or more substances together to create something new. These explorations have led to the idea of what kind of reactions would occur when diverse elements are combined. This is a concept known as chemistry, a part of science that corresponds with how matter is created from different properties and the process it goes through to create a new substance. Chemistry is a scientific concept that is used in everyday life and is a crucial part in the development of new technology and substances that allow today’s quality of life. The use of chemistry branches off into many different routes, including medical related fields, agriculture, and even in weapons of