Physical Properties:
Solid at room temperature. ( “Thiocyanate.”)
Boiling point- 146 degrees Celsius +/- 9 degrees. (“Thiocyanate Anion.” )
Typically Colorless ( “Thiocyanate.”)
Flash point- 42.1 +/- 18.7 degrees Celsius (“Thiocyanate Anion.” )
Vapour Pressure- 4.7 +/- .3 mmHg at 25 degrees celsius (“Thiocyanate Anion.” )
This is the lewis dot diagram of Sulfur Cyanide. While this section won’t feature an in depth description of the lewis dot diagram and what it means, the diagram will help to explain Sulfur Cyanide’s state at room temperature and its boiling point. Sulfur Cyanide has a charge of -1 and has ion to ion intermolecular forces. This force is very strong so a lot of energy is required to break apart the intermolecular force and
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One bond is between Carbon and Nitrogen, while the other bond is between Carbon and Sulfur. The bond between Carbon and Nitrogen is more stable than the bond between Carbon and Sulfur. This is the case because there is more attraction between Carbon and Nitrogen along with more shared pairs of electrons. There is a higher attraction between Carbon and Nitrogen than Carbon and Sulfur because of the difference in electronegativity. C and N have an electronegativity difference of .5 while C and S have an electronegativity difference of 0. The higher electronegativity difference leads to more attraction which causes a decrease in potential energy and an increase in stability. C and N also share three pairs of electrons compared to the one pair that C and S share which leads to even more stability on the part of C and N compared to C and …show more content…
It has two bonded regions and zero lone pairs. Sulfur Cyanide has this specific shape because according to VSEPR theory the two bonded regions will repel each other and be as far away from each other as possible. These bonded regions would also be repelled by lone pairs, but since there are none the two bonded regions end up being on opposite ends from each other. This leads to the bond angle being 180 degrees.
Molecular Polarity- Sulfur Cyanide is polar. This is the case because it’s asymmetrical and the electronegativity difference between carbon and nitrogen is .5. The fact that the electronegativity difference is greater than .3 and the molecule is not symmetrical means that the molecule is polar.
Industrial/commercial uses- Sulfur Cyanide is used for agriculture to produce herbicides and fungicides. In the oilfield industry it’s used as a chemical tracer. Sulfur Cyanide is also used as an intermediate for metal Thiocyanates in anti-fouling paints. It’s also used as the starting agent in the synthesis of certain metals and dyes. Alongside all of these things it is also an additive in peroxodisulfates (“Thiocyanate - AkzoNobel.com.”
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
Aspirin is 3.3 g/L soluble in water (3). Aspirin can be soluble in ethanol, DMSO, or water (2). Aspirin has polar groups that when put with polar water molecules can form hydrogen bonds. Aspirin is an asymmetrical molecule. When drawing the Lewis Dot Structure, a person can see that the bonds are polar. There are also dipole moments making the molecule polar. Dipole molecules are composed of a higher electronegative atom pulling electrons towards it (11). It is more soluble in basic solutions than water and acidic solutions (4). The Lewis Structure also reveals that there are many double bonds between the carbons and two double bonds between oxygen and carbon.
- The amount of times the mixture was stirred. We stirred the mixture until the Ammonium Nitrate was dissolved, so the amount of times we stirred after each teaspoon was different.
1-Butanol with intermediate polarity was soluble in both highly polar water and non polar hexane as 1-butanol can be either polar or non polar compound. 1-Butanol was polar based on the general rule of thumb stated that each polar group will allow up to 4 carbons to be soluble in water. Also, 1-butanol can be non polar due to their carbon chains, which are attracted to the non polarity of the hexane.
Chemical warfare is the most terrifying and debilitating way to gain the advantage on your enemy or adversary. The use of chemical warfare dates back to World War I; although it is believed that Spartan and Greek armies used a type of chemical warfare dated back to 82-72 BC. Chemicals were used in combat during World War I. Some of the chemicals being used were chlorine, phosgene, and mustard gas. The Chemical Warfare in World War I began as the Germans used chlorine gas, and threw it into the trenches where the troops and most of the defensive positions were located. Nearly 33% of casualties during World War I resulted from chemical warfare. Only 25% percent were fatalities. At the end of World War I, the casualties resulting from chemical attacks multiplied to a devastating 1,240,853. A total of 91,198 died from injuries sustained from the chemical attacks (Service, 1953). Doctors had no cure or remedy this early in time. Throughout this informative research paper, in this history of I will be breaking down the history and origins of chemical warfare. The history of chemical warfare has changed the world. Our fears of chemical attacks in the future have increased and will continue to get worse.
It is most stable configuration for atom because the outer shell of the atom is completely filled. Minerals that contains covalent bonds are insoluble, stable, brittle and they have high melting points. The elements in the Carbon group like carbon, silicon, tin prefer covalent bonding. For instance, two Carbon atoms bond together with covalent bonding and that is the strongest bond in nature.
... magnetic orbitals on the metal and the valence orbitals of the ligands. In the present case where the nickel centres are bridged by long N-C-N hmt and N-C-N-C-N dca ligands it is reasonable to assume that only minor exchange interactions can be mediate by these bridges and, as observed here, this type of magnetic pathways generally promotes antiferromagnetic interactions [38,45-48]. Nevertheless spin canting is often observed and usually associated with single-ion magnetic anisotropy or antisymmetric exchange interaction. From structural considerations the existence of two crystallographically independent Ni(II) ions with non-collinear anisotropy axes might be at the origin of the suspected canting phenomena. To clearly ascertain for the existence of a spin canting magnetic order, as the data suggests, neutron diffractions measurements are foreseen.
compounds made solely from carbon and hydrogen are generally non-polar and insoluble in water
Ionic compounds, when in the solid state, can be described as ionic lattices whose shapes are dictated by the need to place oppositely charged ions close to each other and similarly charged ions as far apart as possible. Though there is some structural diversity in ionic compounds, covalent compounds present us with a world of structural possibilities. From simple linear molecules like H2 to complex chains of atoms like butane (CH3CH2CH2CH3), covalent molecules can take on many shapes. To help decide which shape a polyatomic molecule might prefer we will use Valence Shell Electron Pair Repulsion theory (VSEPR). VSEPR states that electrons like to stay as far away from one another as possible to provide the lowest energy (i.e. most stable) structure for any bonding arrangement. In this way, VSEPR is a powerful tool for predicting the geometries of covalent molecules.
The next part of the graph is the fingerprint region. In the fingerprint region there are two important peaks. The first of these appears around 750cm-1, and the second at 690cm-1. These two peaks indicate that the benzene ring that we discovered present in the structure is a monosubstituted benzene ring.