The relative reactivity of the hydrogens H1, H2, H3 , and H4 were 0.37, 1.4, 2.9, and 1.0 respectively. The radical chlorination of 1-chlorobutane follows the radical reaction mechanism. Abstraction of hydrogen from 1-chlorobutane by the chlorine radical occurs in the first part of the propagation step. Depending on which hydrogen is abstracted by the chlorine radical, determines which product is formed. Hydrogens on the alkene have different reactivity which determines which isomer is favored.
Introduction: The radical chlorination of chlorobutane results in the formation of four possible products. These products are formed by substitution reactions, where a halogen atom (chlorine) replaces a hydrogen atom (Wade 2010). The amount of each product formed is based on the relative reactivity of the product. The calculations of the relative reactivity are dependent on the reactivity of the hydrogen atoms, which is influenced by the chloro substituent as well as other factors such as the level of the substituted carbon and the bond dissociation energy. For this lab we want to observe how the chloro substituent has an effect on the reactivity of the possible hydrogen atoms.
2 marks 4 Draw the structural formula of Compound G. 1 mark 5 Using the chemical shift correlation for 13C NMR, predict the number of peaks for Compound G and draw in the position of the peaks on the blank spectrum below, annotating each peak with its corresponding structure. (2 marks) 6 Draw the structural formula for 2-chloro but-2-ene. Below this draw a structural formula of an isomer of 2-chloro but-2-ene and name this substance.
108. Two common sugars, glucose or C6H12O6, and sucrose or C12H22O11, are both carbohydrate4s. Their standard enthalpies of formation are: Glucose = -1273 kJ/mol and Sucrose = -2221 kJ/mol. Using this data: a) Calculate the molar enthalpy of combustion to CO2 (g) and H2O (l). b) Calculate the enthalpy of combustion per gram of each sugar.
in the nucleus of a given atom. The atomic number is the number of protons in an cesium scandium chromium ruthenium 13. Oxygen-18 12. Hydrogen-3 11. Hydrogen-1 Isotope 20 8 1 1 92 65Cu 29 235U 92 Chemistry:
Name___________________________ Period_________________ Chemical Bonds Review Sheet Part one Write the definitions for each of the following terms. Octet rule Cation Anion Ionic compound Monatomic ion Covalent bond Molecular compound Nonpolar covalent bond Polar covalent bond Single bond Double bond Triple bond Part 2 1. Which has a greater potential energy, a noble gas or a metal? Explain your answer. ________________________________________________________________ ________________________________________________________________ ________________________________________________________________ 2.
2.1 Classes of Hydrocarbons: Aliphatic | Aromatic (aka Arenes) | Alkanes, Alkenes, Alkynes | Benzene is an example | Alkanes: All bonds are single bonds Alkenes: Contain at least one C-C double bond Alkynes: Contain at least one C-C triple bond 2.3 Bonding in H2: The Valence Bond Theory Sigma Bond: orbitals overlap along a line connecting the atoms 2.4 Bonding in H2: The Molecular Orbital Model Bonding Orbital and antibonding orbital produced 2.5: Introduction to Alkanes: Methane, Ethane and Propane Alkanes: CnH2n+2 2.6 sp3 Hybridization and Bonding in Methane Sp3 Hybridization 2.7 Bonding in Ethane CH3= Methyl Bonds with sigma bond 2.8 Isomeric Alkanes: The Butanes n-butane: four carbons are joined
Bromination of Arenes This lab demonstrated the application of adding bromine to various arenes, hydrocarbons with alternating single bonds. This process, bromination, is a mechanism which treats hydrogen as a functional group. This being the case, the rate of reaction of certain arenes can be measured and compared to that of other arenes upon the addition of the bromine. The reaction occurs when the bromine radical generates from the halide diatomic molecule, using light energy. The fact that the energy needed to break the necessary bonds falls within the visible light spectrum is the basis on which the experiment is based.
Predict the number of valence electrons for a sulfur atom. a. 4 b. 6 c. 8 d. 16 e. 32 58. Predict the number of valence electrons for a chlorine atom.
If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system.