Is there a difference between the hardness of a small rock and a larger rock? Shockingly there isn’t. A small rock will be comparable in its hardness to the larger rock of the same type. This quality is because of the physical property of the rock. Similarly, everything in nature including compounds like haloalkane and haloarene has some physical properties as well as chemical properties. In this topic, we will understand more about the physical properties of haloalkanes and haloarenes. Physical properties of any compound primarily depend upon The mass of the compound Different forces of attraction including intermolecular and intramolecular forces of attraction. When a hydrogen atom in an aliphatic or aromatic hydrocarbon is replaced by halogen …show more content…
However, bromides and iodides develop color on exposure to light. The reason for the development of color is the decomposition of halogens in presence of light. The reaction to the phenomenon is 2R−I → R−R + I2 Many of the halogen compounds having volatile nature have a sweet smell. Haloarenes are also colorless liquid or crystalline solids that have a characteristic smell. Boiling Point We know there is a large difference in electronegativity between the carbon and halogen atom of any given compound resulting in the development of highly polarized molecules. The polarity of the C-X bond and higher molecular mass in comparison to the actual hydrocarbon results in the development of very strong intermolecular forces of attraction in the derivatives of halogen. The stronger intermolecular forces of attraction are formed due to dipole-dipole and van der Waals interaction. The boiling point of haloalkanes and haloarenes depends upon the intermolecular forces of attraction. Hence, the boiling points of derivatives of chlorides, bromides, and iodides are comparatively higher the hydrocarbons of the similar molecular mass. The size and molecular mass of halogen members increase when we move down the group in the homologous series thereby forming stronger forces of attraction. Hence the boiling point increases as we move down the group in the homologous …show more content…
However, the boiling point decreases with the branching of the compound. This is because branching results in the lesser surface area, thus decreasing the van der Waal’s forces interaction. Moreover, as the branching increases the molecule forms sort of a spherical shape resulting in the decrease in the area of contact and forming weaker intermolecular forces. Derivatives such as methyl chloride, ethyl chloride, methyl bromide and few chlorofluoromethanes are gases at room temperature. However, the higher members of the group are usually solids or
The percent yield of products that was calculated for this reaction was about 81.2%, fairly less pure than the previous product but still decently pure. A carbon NMR and H NMR were produced and used to identify the inequivalent carbons and hydrogens of the product. There were 9 constitutionally inequivalent carbons and potentially 4,5, or 6 constitutionally inequivalent hydrogens. On the H NMR there are 5 peaks, but at a closer inspection of the product, it seems there is only 4 constitutionally inequivalent hydrogens because of the symmetry held by the product and of this H’s. However, expansion of the peaks around the aromatic region on the NMR show 3 peaks, which was suppose to be only 2 peaks. In between the peaks is a peak from the solvent, xylene, that was used, which may account to for this discrepancy in the NMR. Furthermore, the product may have not been fully dissolved or was contaminated, leading to distortion (a splitting) of the peaks. The 2 peaks further down the spectrum were distinguished from two H’s, HF and HE, based off of shielding affects. The HF was closer to the O, so it experienced more of an up field shift than HE. On the C NMR, there are 9 constitutionally inequivalent carbons. A CNMR Peak Position for Typical Functional Group table was consulted to assign the carbons to their corresponding peaks. The carbonyl carbon, C1, is the farthest up field, while the carbons on the benzene ring are in the 120-140 ppm region. The sp3 hybridized carbon, C2 and C3, are the lowest on the spectrum. This reaction verifies the statement, ”Measurements have shown that while naphthalene and benzene both are considered especially stable due to their aromaticity, benzene is significantly more stable than naphthalene.” As seen in the reaction, the benzene ring is left untouched and only the naphthalene is involved in the reaction with maleic
Discussion and Conclusions: Interpreting these results have concluded that relative reactivity of these three anilines in order of most reactive to least reactive go; Aniline > Anisole > Acetanilide. Aniline, has an NH2 , the most active substituent , and adds to any ortho/para position available on the ring. This data is confirmed with the product obtained, (2,4,6 tribromoaniline, mp of 108-110 C). As for anisole, it has a strongly activating group attached, OMe an alkoxy group, and it added in two of the three available spots, both ortho. The results conclude: (2,4-Dibromoanisol mp 55-58 C ). Acetanilide has a strong activating group attached, acylamino group, but this group is large and the ortho positions are somewhat hindered so the majority of the product obtained added at the para position, results conclude: (p-bromoacetanilide mp 160-165 C). Since all the substituents attached to the aromatic rings were activators the only products able to be obtained were ortho/para products.
The total pressure of these two layers is the addition of the vapor pressure of each layer. Mixing these two layers results in a higher vapor pressure, which thus results in a lower boiling point than the boiling points of the water and the oil individually. Eugenol oil is the organic layer; therefore it is hydrophobic (afraid of water) and is nonpolar. This causes a boiling temperature that is slightly lower than 100 °C for the eugenol oil. Because eugenol oil has a lower boiling point than water, the molecule of eugenol is more likely to be able to escape into the air than the water, which has a higher boiling point.
The goal of this lab is to exemplify a standard method for making alkyne groups in two main steps: adding bromine to alkene groups, and followed by heating the product with a strong base to eliminate H and Br from C. Then, in order to purify the product obtained, recrystallization method is used with ethanol and water. Lastly, the melting point and IR spectrum are used to determine the purity of diphenylacetylene.
Benzyl bromide, an unknown nucleophile and sodium hydroxide was synthesized to form a benzyl ether product. This product was purified and analyzed to find the unknown in the compound. A condenser and heat reflux was used to prevent reagents from escaping. Then the solid product was vacuum filtered.
The heat makes the molecules in the mixture expand and move slower than when they are in colder temperatures (source 1). The molecules are like people when it comes to how they react to heat and coldness. When the molecules are cold, they like to be very close to one another and the molecules move fast because they are “shivering” (source 2).This is just a one of many examples and comparisons that I am going make throughout this paper. Some of the examples will be very cheesy. I am going to give a warning. When the molecules are hot, they like to be far apart from one another (source 1). They even might start to sweat like humans, too. The molecules have some energy too, but the molecules just do not have as much energy when they are hot. They like to be lazy like many humans do in hot weather (source 1).
The noble gases are group 18 of the periodic table and are chemical elements with similar properties. All of the noble gases have a full outer shell. None of them have color, odor, and all have very low chemical reactivity. There are six of them and they are Helium, neon, argon, krypton, xenon, and radon.
For water at 1 atm, the melting point and boiling point is 0 °C and 100°C respectively. Water reaches the maximum density at 4°C. The density of ice is lower than that of water. The molecules are in constant motion and the strong hydrogen bonding leads to the closed packing of water molecules.
Also, I will know what a chemical and physical property is and I will know how to find them out. Materials = == == ==
Alcohol particles break their bonds when they mix with oxygen. This is known as an exothermic reaction. Boiling points will be increased because energy is needed, bonds can be formed and broken. Breaking bonds need less energy than is needed to form bonds - an exothermic reaction. Bigger molecules use high energy to break down.
Figure 1 compared the change in temperature in Celsius during evaporation for ethanol and 1-propanol over a time period in seconds. Due to its higher molecular mass, 1-propanol (60.09 g/mol) was harder to evaporate than ethanol (46.06 g/mol). Both substances had very low changes in temperature because of their hydrogen bonds and dispersion forces as well as relatively high molecular masses, those factors made it hard to break their bonds and make them evaporate.
Toluene is useful as it dissolves iodine, sulfur, oils, fats, resins, and phosgene. Toluene is important for many industrial uses, the hydrogenation (addition of hydrogen) of toluene yields methyl cyclohexane which is a solvent for waxes, oils, fats, and rubbers. Trinitrotoluene (TNT) is a component of several explosives. Monochlorotoluene is a widely used solvent for synthetic resins and rubbers. Saccharin and chloramine T are both derived from toluene synthesis. Toluene is a valuable chemical in many industries.
There are four different types of hydrocarbons each having a different homologous series (formula for carbon chain). These being an alkane (formula = CnH2n+2), alkene (formula = CnH2n), alkyne (formula = CnH2n-2), and an alkanol which has the same formulae as an alkane only that is has a hydroxide molecule which replaces one of the hydrogen atoms (refer to figure 3 and
molecules its size it would have a boiling point of -75øC and a freezing point of -125øC4.
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.