Stone Thrower Wales ( Stw ) Defect

Figure 6.9. SEM micrographs showing the existence of structural pores in SC-CNCs, indicating the porous nature of (a) NC-1, (b) NC-2, and (c) NC-3.

Carbon has six total electrons; two of the electrons it has are in its first electron shell while the other four are its valence electrons. Due to its four valence electrons, it rarely gains and/or loses electrons and/or form ionic bonds due to the fact it would have to give away or take four other electrons. In order to complete its outer shell, carbons shares its valence electrons with other atoms by having four separate covalent bonds. The carbon atom then becomes the crossing point where each molecule branches off into four separate directions.Carbon’s electron configuration allows it to bond frequently with oxygen, hydrogen, nitrogen, and phosphorus. If the carbon atom forms only a single covalent bond, The electrons form so that its bonds angle towards an imaginary tetrahedron.

Monday - I was out in the lab working on copper swage flare #1 cutting the pieces and flaring them Tuesday- I finished up readying the pieces for assembly then I started assembling it and soldering it and brazing the end of it Wednesday- I finished assembling it then I cleaned it up and I had to heat it back up and wipe more solder off Thursday- I finished up cleaning my project up and I put it on the tester which it didn't leak but it wasn't clean enough so i spent the rest of the day cleaning it

The peaks around 3000 cm-1 and 2920 cm-1 show the stretching of carbon-hydrogen bonds in both sp2 and sp3 hybridized carbons respectively. The peak around 1620 cm-1 shows the stretching of carbon-carbon double bonds, and lastly, the peak around 1495 cm-1 signifies the bending of a sp3 carbon-hydrogen bond. The significant peaks are sharp and fit the strength categories that are on the IR chart

The ChemMagic software program was used for this experiment. The compounds were tested one at a time. First was the compound butane. The draw tab was chosen on the program. Butane was then drawn in the program and the model was loaded. A 3D butane compound was projected on the screen and the optimize tab was selected. Next, the rotate bond tab was selected so that the C2-C3 bond would rotate. After the bond was selected, the bonds were then moved to rotate in intervals of 10 starting with 0 degrees. After the bond was rotated in the desired increment, the energy tab was selected and the angle and energy level was then recorded. These steps were followed for every compound each being rotated in intervals of 10 until 360 degrees was reached.

When Crick found flaw in V Vand’s proposed theory of X-ray diffraction by helices, he consulted his Cavendish colleague Bill Cochran. Both of the men, came up with a solution independently with different methods and the result agreed with X-ray diffraction diagram’s obtained Max Perutz during his research (Page 36). This development further increased the knowledge and application of the theory of how helices were supposed to look in X-ray photographs for Watson and Crick coalition. Watson not able to follow the mathematical expertise required to understand the theory, however, became well acquainted with the physical manifestation of helices on X-photographs of crystalline

During the increase of temperature from 294K to 980K where α-β transition happens, the unit cell structure is trigon α-FePO4 with Fe in the 3a sites, P at the 3b sites and O in the 6c sites (x, y, z). Looking at the structures between trigon α-FePO4 and hexagonal β-FePO4, they have similar symmetry and their symmetrical relationship structure is similar when compared according to the correct respective axes. From 980K to 1073K, the unit cell structure is hexagonal β-FePO4 with Fe in the 3d sites, P at the 3c sites and O in the 12k sites(x, y, z). In hexagonal unit structure, the lattice parameter recordings are as follows: a = b ≠ c with α = β = 90° and γ = 120°. From the graphs, we note that the tetrahedral tilt angle decrease drastically as the transition temperature is reached.

value of 0.087 micro g. These results support and expand our understanding of the mechanisms

Lonsdaleite is a hexagonal diamond named after famous crystallographer Dame Kathleen Lonsdale. In nature, this diamond is only found at meteorite impact sites such as Canyon Diablo in the United States. The discovery that lonsdaleite can be synthetically produced in a controlled laboratory setting presents a scientific breakthrough in terms of creating hexagonal diamonds. Making the stronger diamond was a team led by associate professor Jodie Bradby and her colleagues from the ANU, University of Sydney, RMIT University, and the United States. The team also included ANU doctoral student Thomas Shiell.

Graphene synthesis usually utilise a method called exfoliation, which is defined as taking the outermost layer of graphite. There are three major types of exfoliation: chemical, mechanical, and thermal. The paper mainly focuses on chemical and mechanical exfoliation for graphene synthesis, which are the methods with highest number of experiments done.

As Wenner data can be analyzed directly (see Figure 4). In addition, layer 1’s thickness and resistivity increased. Layer 2 and 3’s thickness and resistivity values were decreased. We may interpret these as variations at depth. The curve segments follow a specific pattern of overlaps, which is clearly illustrated in Figure 5.

The purpose of this experiment was to determine the rotation constant, vibration-rotation interaction constant, moment of inertia, and bond lengths for Acetylene(C2H2) and Deuterated Acetylene(C2D2) synthesized in the lab. Using Fourier Transform Infrared (FTIR), an absorption spectrum for C2H2 and C2D2 was generated and using the peaks and values given by the FTIR, the bond length between C≡C and C-H ultimately determined.

* Lim Peng Chew, Lim Ching Chai, Nexus Bestari Physics, Sasbadi Sdn. Bhd. , 2013, Pg 18,19

Graphene is a form of carbon which has recently been receiving a great deal of attention. Some have come to call it “the wonder material” due to its many extraordinary properties. Although isolated in 2004, graphene's properties had been calculated decades earlier. It consists of a single layer of carbon atoms arranged in a hexagonal lattice. A single sheet of graphene is stronger than steel and yet remains very flexible, retaining all of its properties despite being bent and unbent multiple times. It is able to sustain extremely high electric current densities, is impermeable to all gasses, has a thermal conductivity double that of diamond and a very high electron mobility at room temperature. It is also easily chemically functionalized,

Ring contraction occurs through rearrangement of carbon atoms to form a smaller ring structure. Two