The balanced molecular equation is: Na2S(aq) + ZnCl2(aq) = ZnS(s) +2NaCl(aq). The ionic and net ionic equations are: Ionic: 2Na(aq) + S2(aq) + Zn2(aq) + 2Cl(aq) ZnS(s) +2Na(aq) + 2Cl(aq), and net ionic: Zn2(aq) + S2 (aq)+ ZnS(s). Chemical reaction occurred from the ammonium dichromate(Decomposition) was exothermic reactions. In a double displacement reaction two compounds exchange bonds or ions in order to form different compounds. An example of a double displacement reaction occurred between zinc chloride and sodium sulfide to form zinc sulfide and sodium chloride.
It is a sandwich of two [C2B9H11]2- (dicarbollide)clusters with a metal ion in the center. A broad range of interactions can be formed between metallacarboranes and their neighboring molecules. Metallacarboranes can be of two types, namely endo- and exo-metallacarboranes. A metal fragment is linked to the periphery of the carborane skeleton in exo-metallacarboranes, through B–H…M interactions. Metallacarboranes are artificial structures with distinct physicochemical properties, such as delocalization of cluster charge, high rigidity of the skeleton, lipophilicity and the ability to form so-called dihydrogen bonds.
Another category of chemical reactions is single-replacement. In a single-replacement reaction, a molecule composed of a cation, or atom with a positive charge, and an anion, or atom with a negative charge, is introduced to a pure element. When mixed together, the anion from the reactant molecule will transfer over to the pure element, causing the original cation to become a pure element. When magnesium metal is placed in hydrochloric acid: Mg + 2HCl --> MgCl2 + H2. Here, it can be seen that the chlorine anion that was a part of the hydrochloric acid is transferred to the pure magnesium, leaving behind hydrogen.
Reactivity of Metals in Single-Replacement Reactions A lab was conducted to test the reactivity of metals in single-replacement reactions. This lab was done to solve the problem of which metals will replace each other in single-replacement reactions. A single replacement reaction is a type of oxidation-reduction chemical reaction when an element or ion moves out of one compound and into another. It was presumed before the experiment that the location of the metal on the Activity Series chart would thus determine the reactivity of the metal. Copper, magnesium, iron, and zinc were all tested in the same five solution compounds; which included hydrochloric acid, sulfate, magnesium chloride, iron chloride, and zinc chloride.
Ionic bonding is the chemical bonding in which 2 or more ions are linked by virtue of its opposite charge 3. Ionic compound is a collection of atoms of 2 or more elements that have become lined through ionic bonding 2.4 The Hydrogen
The goal of the experiment is to synthesize a bromohexane compound from 1-hexene and HBr(aq) under reflux conditions and use the silver nitrate and sodium iodide tests to determine if the product is a primary or secondary hydrocarbon. The heterogeneous reaction mixture contains 1-hexene, 48% HBr(aq), and tetrabutylammonium bromide and was heated to under reflux conditions. Heating under reflux means that the reaction mixture is heated at its boiling point so that the reaction can proceed at a faster rate. The attached reflux condenser allows volatile substances to return to the reaction flask so that no material is lost. Since alkenes are immiscible with concentrated HBr, tetrabutylammonium bromide is used as a phase-transfer catalyst.
This element is a transition metal in group 12. Zinc is a family of cadmium (Cd), mercury (Hg), and copernicium (Cn), even though they are found in same row and they have things in common they also have different properties. Zinc’s mass is 65. some of the colors are bluish-silver, white, and bluish-green Zinc has many use. Zinc is used for metal coating rust protection, nickel , steel iron and many other things.The zinc layer helps the metal from rusting. Zinc,copper and iron is combined to make nickel.
Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, definitions of each relating factor were researched, leading to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound is formed when two or more nonmetal atoms share valence electrons; covalent compounds are also categorized into two sections: polar covalent and nonpolar covalent. Furthermore, polar covalent compounds dissolve in water, while nonpolar covalent compounds do not. Dissolving is the process in which a solvent and a solute interact with each other and form a solution.
The NAD+ and FAD each pick up hydrogen and electrons, turning them into NADH and FADH2. Each Pyruvate can yield 3 NADH and 1 FADH2 per cycle. The purpose of the Krebs cycle is to create these for the next stage, Oxidative Phosphorylation. Oxidative Phosphorylation (the electron transport chain) The FADH and NADH that were created in the Krebs cycle use their electrons to provide energy to electron transport chain that moves proteins along the inner membrane of the mitochondria. These proteins swap the electrons to send hydrogen protons from the inside of the mitochondria to the outside.
Objective #1 Compare the differences between ionic and covalent bonding and how molecules are formed by either ionic or covalent bonds. IONIC BONDING: Ionic Bonding is the complete transferring of valence electrons between two atoms. This type of chemical bonding results in two oppositely charged ions, a cation and an anion In ionic bonding the electrostatic attraction between the charged ions holds the compound together. Example: Bonding of Sodium and chlorine. 1s2 2s2 2p6 3s1 Fig.1 to show the electronic configuration of sodium along with its atomic mass and atomic number The above diagram shows the atom, sodium.