Conclusions At the end of Part A in this experiment‚ it can be determined that Sodium Chloride had the highest amount of conductivity tested by all groups. On the graph above‚ the data shows that NaCl (sodium chloride) held the highest amount of electrical conductivity for all groups and on the table it reads the highest numbers across its row. Also as seen in the data above‚ ethanol had the lowest amount of conductivity with sucrose‚ acetic acid‚ ammonia‚ and MgCl2 following in ascending order
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Before conducting the experiment‚ the online simulation was used to determine which substances were endothermic or exothermic when dissolved in water. According to the simulation‚ sodium chloride and ammonium chloride was observed to be endothermic. Calcium chloride‚ sodium acetate‚ sodium carbonate‚ and lithium chloride was observed to be exothermic. As sodium chloride and ammonium chloride was observed to be endothermic‚ those two salt substrates was not used in the experiment as the goal of the
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Writing Lewis Dot Formula November 8‚ 2013 I. Learning Objectives At the end of the sessions‚ the students of III- 15‚ and III – 10 must be able to: 1. Students will be able to interpret and draw Lewis dot diagrams for individual atoms and both covalent and ionic compounds. II. Subject Matter A. Topic: Chemical Bonding B. References 1. Department of Education‚ Culture and Sports. (1991). Science and Technology III. Quezon City: Book Media Press‚ pp. 273. 2. Estrella‚ Mendoza E. Chemistry
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Elements and compounds are a result of the actions of the valence electrons. There are three types of bonds that I have learned about in the bonding comparison lab. These bonds include ionic‚ polar covalent‚ and non-polar covalent. Each of these bonds and the element compounds connected to them has individual solubility‚ conductivity‚ melting point‚ and volatility levels. The three element compounds that will follow are sodium chloride‚ sucrose‚ and p-dichlorobenzene. Sodium chloride is an ionic
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This molecular orbital model can be used to explain why He2 molecules don’t exist. Combining a pair of helium atoms with 1s2 electron configurations would produce a molecule with a pair of electrons in both the bonding and the * antibonding molecular orbitals. The total energy of an He2 molecule would be essentially the same as the energy of a pair of isolated helium atoms‚ and there would be nothing to hold the helium atoms together to form a molecule. The fact that an He2 molecule is neither
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Chemistry I Chapter 8 Review Problems Part I Using the factor label method‚ neatly and clearly show all work. Answers are to include the unit‚ be in correct number of significant figures. If the answers are less than 1.0 or greater than 10‚ they are to be written in and be in correct scientific notation. Box your final answer. Mass/Mole Problems 1. Determine the molar masses of the following compounds: a. dinitrogen pentoxide c. sodium carbonate b. ammonium
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~ Graded Assignment I) Name: . 1\ \ \ ~o ni-! SC1303A/304A: Chemistry 1Unit 41 Lesson 17: Unit Test I .’ / j ! Graded Assignment Unit Test‚ Part 2 Answer the questions below. You may use the periodic table in the Chemistry: Problems and Solutions book for this test. When you have finished. submit this assignment to your teacher by the due date for full credit. (5 points) 1. You have three elements. A. B. and C. with the following electronegativity values: A = 0.9 B =3.0 C = 3.5 You
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1. Atomic masses are expressed on a scale based on the mass of what? Carbon-12 2. Name the unit used to express atomic masses of individual atoms. Grams or molar mass‚ gmm 3. Define formula mass. Sum of the atomic masses of all atoms in a compound 4. What do we call the number of atoms of an element equal to the number of atoms in exactly 12.0 grams of carbon-12? Mole or Avogadro’s number 5. How many atoms are in a sample of an element whose mass is numerically equal to the atomic
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Identification of a Copper Compound by Percent Mass Unknown Compound: #9 Abstract: The objective of this experiment was to identify the unknown pure copper salt compound of #9. To do this‚ the mass of copper in the unknown was calculated and then divided by the mass of the whole compound to get the percent copper. The molecular weight was also calculated by dividing mass of copper compound used by moles of compound in unknown sample. The percent copper averaged out to 31.6% while the molecular
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Preparation of Calcium Carbonate Lab In this laboratory activity you will attempt to produce 1.00g of calcium carbonate from aqueous solutions of calcium chloride and sodium carbonate. These solutions will be prepared from 2.01 g of calcium chloride and 1.06 g of sodium carbonate . Materials: 3 beakers 100 mL graduated cylinder rubber policeman funnel filter paper Procedure: 1. Put on your safety goggles. 2. Obtain two clean beakers. Rinse the inside of the beakers with a small
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