a. what happens on a molecular level that allows an analyte to absorb light at a...
a. what happens on a molecular level that allows an analyte to absorb light at a certain wavelength?
b. why are you using a specific wavelength of light to record absorbance measurements for the dye
(i.e., why won't every wavelength of light be absorbed by the analyte)?
Homework Answers
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a. what happens on a molecular level that allows an analyte to
absorb light at a...
1: What happens in a molecular level that allows an analyze to absorb light at a...
1: What happens in a molecular level that allows an analyze to absorb light at a certain wavelength. 2: Why are you using a specific wavelength of light to record absorbance measurements for the dye (i.e., why non't every wavelength of light be absorbed by the analyte) I need this answer ASAP please. Thank you
Which of the following best explains what happens as photons of visible light are absorbed by...
Which of the following best explains what happens as photons of visible light are absorbed by dye molecules? Certain electrons in the dye molecule move to a higher energy level, with the difference in energy between the lower and higher energy levels being the same as the energy of the absorbed photons Certain chemical bonds in the dye molecules begin to bend and stretch with the difference in energy between the lower and higher vibrational states being the same as...
1. (2pt) Explain the mechanism by which atoms absorb light, i.e. what happens when an atom...
1. (2pt) Explain the mechanism by which atoms absorb light, i.e. what happens when an atom absorbs a photon. 2. (2pt) Why do atomic emission spectra come in the form of lines instead of broad bands that span whole regions of the electromagnetic spectrum?
Answer QUESTION 5 Describe what happens at the molecular level once equilibrium is reached--that is, once...
Answer QUESTION 5
Describe what happens at the molecular level once equilibrium is reached--that is, once the solution is saturated with Cu(IO_3)_2. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? Describe how you are going to calculate the [Cu^2+] for the saturated solution of copper iodate once you know the absorbance value of the copper ion. How will you use this concentration to find the K_sp value for...
A- B- C- In Part C students will make the standard solutions to find a calibration...
A-
B-
C-
In Part C students will make the standard solutions to find a calibration curve. The experiment's Standard 1 consists of 0.13 M CuSO4. What will be the concentration of Standard 2 if it is prepared by combining 10.0 mL of Standard 1 with 10.0 mL deionized water? How should you set up the spectrophotometer? Make sure your cuvettes are clean and dry before use. Turn it on as soon as you can so it can warm up....
Can you please answer question 3,4&5. Using crystal field theory, sketch the energy level diagram for...
Can you please answer question 3,4&5.
Using crystal field theory, sketch the energy level diagram for complex ion nNwhich is classified as low-spin. 4. Find the wavelength and frequency of lig ht that could be absorbed by a complex-ion for which ? is 3.82 x 10-19 Joules. 5. Which complex-ion, Coci or Coclwill absorb light with the longer kavelength of maximum absorbance. Explain your choice
Using picture and words, describe your understanding of what happens on the molecular level when SALT...
Using picture and words, describe your understanding of what happens on the molecular level when SALT (NaCl) dissolves in water. Using picture and words, describe your understanding of what happens on the molecular level when SUGER (C12H22O11) dissolves in water.
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the...
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the ground state. What happens to the light and to the electron? Group of answer choices a. The light is not absorbed and the final energy of the electron is -1312 kJ/mol. b.. The light is absorbed and the final energy of the electron is −328 kJ/mol. c.. The light is not absorbed and the final energy of the electron is −1050 kJ/mol. d.. The...
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red...
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red dye, blue dye, yellow dye. 2. Obtain a spectrum for each dye according to the provided directions (water is the blank). 3. For each of the three dyes (red, yellow, and blue) record the wavelength for the largest peak in the visible range (380 nm to 750 nm), Record this in the data table below. Save the red dye for part B. 4. Identify...
Modified TRUE-FALSE. Write true if the statement is correct and if incorrect, change the underlined word...
Modified TRUE-FALSE. Write true if the statement is correct and if incorrect, change the underlined word to make the statement correct. IR spectra show absorption bands that enable to determine if certain functional groups are present in a molecule. IR spectra are expressed in wave number. Transmitted light have greater absorbance. (Emission) Absorption spectrum is the light of specific wavelength that is emitted when the atoms relax. When atoms absorb light of specific wavelength that causes the electrons to go...
Which of the following best explains what happens as photons of visible light are absorbed by dye molecules? Certain electrons in the dye molecule move to a higher energy level, with the difference in energy between the lower and higher energy levels being the same as the energy of the absorbed photons Certain chemical bonds in the dye molecules begin to bend and stretch with the difference in energy between the lower and higher vibrational states being the same as...
1. (2pt) Explain the mechanism by which atoms absorb light, i.e. what happens when an atom absorbs a photon. 2. (2pt) Why do atomic emission spectra come in the form of lines instead of broad bands that span whole regions of the electromagnetic spectrum?
Answer QUESTION 5
Describe what happens at the molecular level once equilibrium is reached--that is, once the solution is saturated with Cu(IO_3)_2. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? Describe how you are going to calculate the [Cu^2+] for the saturated solution of copper iodate once you know the absorbance value of the copper ion. How will you use this concentration to find the K_sp value for...
A-
B-
C-
In Part C students will make the standard solutions to find a calibration curve. The experiment's Standard 1 consists of 0.13 M CuSO4. What will be the concentration of Standard 2 if it is prepared by combining 10.0 mL of Standard 1 with 10.0 mL deionized water? How should you set up the spectrophotometer? Make sure your cuvettes are clean and dry before use. Turn it on as soon as you can so it can warm up....
Can you please answer question 3,4&5.
Using crystal field theory, sketch the energy level diagram for complex ion nNwhich is classified as low-spin. 4. Find the wavelength and frequency of lig ht that could be absorbed by a complex-ion for which ? is 3.82 x 10-19 Joules. 5. Which complex-ion, Coci or Coclwill absorb light with the longer kavelength of maximum absorbance. Explain your choice
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red dye, blue dye, yellow dye. 2. Obtain a spectrum for each dye according to the provided directions (water is the blank). 3. For each of the three dyes (red, yellow, and blue) record the wavelength for the largest peak in the visible range (380 nm to 750 nm), Record this in the data table below. Save the red dye for part B. 4. Identify...
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