Innovative and self-directed, EXPERIMENTS IN GENERAL CHEMISTRYFEATURING MEASURENET, 2nd Edition prepares students for the laboratory setting by. Experiments in General Chemistry Featuring MeasureNet Guided Inquiry, Self- Directed, and Capstone Second Edition Bobby Stanton University of Georgia Lin . Innovative and self-directed, EXPERIMENTS IN GENERAL CHEMISTRY: FEATURING MEASURENET, 2nd Edition prepares students for the.

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For example, the oxidation number of Na in sodium metal is zero; the oxidation number of F in F2 is zero. Other editions – View all Experiments in General Gfneral Each line on the cylinder is 0.

For light to be absorbed by a chemical species, the light must have a wavelength, or energy, that exactly matches an energy transition in the absorbing species. Determination of the Specific Heat of a Solid 7. Predicting whether a precipitate will form depends on knowledge of the solubilities of the products. Be sure the stir bar is still turning.

Should you record the two most intense emission lines in the Lab Report for each metal ion in the emission spectra of the known and unknown solutions? When excess NH3aq is added, the precipitate dissolves.

Often chemists must separate the individual fezturing of a mixture to identify and characterize each component.


Place the crucible containing the mixture in the clay triangle as shown in Figure 1. Suspend the crucible and lid inside the clay triangle. Tape the top corners of the paper cylinder together with a 2 cm strip of adhesive tape do not allow the two edges of the paper to touch, see Figure 4. Immediately replace the lid on the calorimeter.

In reality, when the pH has risen by 1. At the University of Georgia, we would like to thank our undergraduate and graduate students in the General Chemistry program. Carefully circle the visible experijents with a pencil.

Rinse the crucible with copious quantities of water. Figure 2 indicates that the equivalence-point occurs when After 15 minutes, the green marker and green food dyes each separated into two components, a yellow component and a blue component. If a student incorrectly calibrated the temperature probe so that all subsequent temperature readings are 2.

The concentration of the metal ion is directly proportional to the intensity brightness of the emitted light.

Experiments in General Chemistry: Featuring MeasureNet

Two stoichiometric factors one the reciprocal of the other express this relationship. How do you determine the molar mass of the metal? If none of these indicators are observed, assume that a chemical reaction did not occur see Note. When there is no longer any detectable loss of mass from the sample after a heating cycle, the reaction has gone to completion and is said to be heated to constant mass.


A student records two potassium emission spectra: Be certain to use a clean Beral pipet for each solution to avoid contamination of the solutions. The original sample is dissolved in a minimum volume of water.

Thoroughly dry the unknown metal with a towel. The moles of NaOH added in the titration and the moles of metal nitrate in the beaker can be calculated using Eq.

Experiments in General Chemistry: Featuring MeasureNet

Repeat the washing process 2—3 times. Should your calculations be included in the Lab Report? Based on your chemiztry from Step 6, indicate whether the compound is a chloride, sulfate, or carbonate compound. For example, S2 has an oxidation number of 2. Washing involves rinsing the precipitate with several small quantities of a volatile electrolyte solution. Add 10—15 mL of 3 M aqueous ammonia to the mL beaker.

Determine the concentration of the limited NH3 solution. Chemistrh lenses are not permitted in the laboratory.