Determine the Elements Electron Configuration Exercise by use of a Periodic Table

Module 05 Lab 02 – Unknown Strong Acid Lab/Questions and Concept Test

Instructions for Virtual Lab: Record all observations and take screenshots of your work.

Go to lab page: http://chemcollective.org/acid-base

  1. Strong Acid
    1. Determine the concentration of the unknown strong acid          
    2. 3 lab questions dealing with the Acid Lab (below)
      1. Briefly describe the equivalence point in a titration. What species are present?
      2. Phenolphthalein is an indicator that will change color at pH close to 8. Why would we use phenolphthalein to determine when the equivalence point is reached?
      3. At what point do you know that you have added enough base from the buret into the acid solution? What happens to your calculations for the concentration of the acid if you accidentally add in more base than you need to?
    3. Concept test (note: you will need to record the answers separately)

Click on the words “Unknown Acid Problem” (on the right side just above Work Bench 1), which will further explain the lab problem within this assignment.

The lab will center on:

  • Determining the concentration of the acid (showing math steps and auto graded answer)
  • 3 lab questions
  • Concept test

Submit a zip file of all screenshots and answers for this lab activity.

For assistance taking a screenshot, refer to the following guide

Submit a zip file of all screenshots and answers for this lab activity.

For assistance taking a screenshot, refer to the following guide.

For assistance zipping files together, refer to the following guide.

Submit your completed assignment by following the directions linked below. Please check

PARTS 2

Module 05 Lab 03 – Equilibrium Simulation

Instructions for Virtual Lab: Record all observations and take screenshots of your work.

Go to lab page: http://chemcollective.org/equilib

  1. LeChatiler’s Principle
    1. Chemical Equilibrium Lab and Concept Test (take screen shots of answers)
  2. Common Ion Effect
    1. Solubility and Common Ion Effect (take screen shots of answers)
  3. 3 lab questions
    1. Based on the colors of the reactants and products, which do you think is in a higher concentration in the flask of 0.1M cobalt chloride?
    2. Describe what happens when you add concentrated HCl to the flask of cobalt chloride. Did you add a product or reactant when you added the HCl?
    3. Describe what happens when you add silver nitrate to the blue cobalt chloride solution. What does adding the silver nitrate do to the reaction?

Click on the words “Cobalt Lab” (on the right side just above Workbench 1), which will further explain the lab problem within this assignment.

The lab will center on:

  • Predicting the effect of removing Chloride Ions
  • Predicting the effect of adding HCl
  • Determining if the reaction is endothermic or exothermic
  • Determining the new K value at the new temperature
  • Common Ion Effect (test does not have to be taken)
  • Answering the 3 lab questions

Submit a zip file of all screenshots and answers for this lab activity.

For assistance taking a screenshot, refer to the following guide.

For assistance zipping files together, refer to the following guide.

Submit your completed assignment by following the directions linked below. Please check the Course Calendar for specific due dates.

The name of the file should be your first initial and last name, followed by an underscore and the name of the assignment, and an underscor

Parts 3

odule 02 Lab 03 – Periodic Table

Purpose of Experiment: To use the periodic and determine the electron configuration.

Instructions: For this lab, the instructor will assign you 10 different elements. Using the periodic table, identify the group name, element name, element symbol, atomic number, atomic weight and electron configuration for each element. Organize the information gathered for all ten elements into one document for submission.

Submit your completed assignment by following the directions linked below. Please check the Course Calendar for specific due dates.

The name of the file should be your first initial and last name, followed by an underscore and the name of the assignment, and an underscore and the date. An example is shown below:

Module Five Assignment

Name:

Chemical Equations

Instructions: Solve the following chemical equations.

  1. For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts.
  2. For the following reaction, calculate how many moles of each product are formed when 0.356 moles of PbS completely react. Assume there is an excess of oxygen.
  3. For the following reaction, calculate how many moles of each product are formed when 4.05 g of water is used.
  4. Determine the theoretical yield of P2O5, when 3.07 g of P reacts with 6.09 g of oxygen in the following chemical equation
  5. Determine the percent yield of the following reaction when 2.80 g of P reacts with excess oxygen. The actual yield of this reaction is determined to by 4.89 g of P2O5.

Properties of Liquids and Solids

Instructions: Answer the following questions using the following information: ∆Hfus=6.02 kJ/mol; ∆Hvap= 40.7 kJ/mol; specific heat of water is 4.184 J/g∙˚C; specific heat of ice is 2.06 J/g∙˚C; specific heat of water vapor is 2.03 J/g∙˚C.

  1. How much heat is required to vaporize 30 g of water at 100˚C?
  2. How much heat is required to convert 29 g of ice at -4.0 ˚C to water vapor at 105 ˚C (report your answer to three significant figures)? Answer all five parts, showing your detailed calculations:

i) Heat to warm ice from -4.0 to 0 oC:

ii) Heat to convert ice to liquid:

iii) Heat to warm liquid to boiling:

iv) Heat to convert liquid to gas:

v) Heat to warm gas from 100 to 105 oC:

  1. An ice cube at 0.00 ˚C with a mass of 8.32 g is placed into 55 g of water, initially at 25 ˚C. If no heat is lost to the surroundings, what is the final temperature of the entire water sample after all the ice is melted (report your answer to three significant figures)?

Mixtures and Solutions

word image Instructions: Use the following image to answer the following questions. Circle your answers and/or show your calculations.

  1. A solution contains 40 g of NaCl per 100 g of water at 100˚C. Is the solution unsaturated, saturated or supersaturated?

unsaturated, saturated or supersaturated?

  1. A solution contains 50 g of KCl per 100 g of water at 25˚C. Is the solution unsaturated, saturated or supersaturated?

unsaturated, saturated or supersaturated?

  1. A solution contains 10 g of KNO3 per 100 g of water at 30˚C. Is the solution unsaturated, saturated or supersaturated?

Solubility Graph [Online Image]. Retrieved November 12, 2018 from https://socratic.org/chemistry/solutions-and-their-behavior/solubility-graphs

unsaturated, saturated or supersaturated?

  1. An 8 oz bottle of Dr. Pepper made with imperial cane sugar (C12H22O11) contains 27 g of sugar in 266.6 mL of water. What is the molarity of the solution with respect to cane sugar?
  2. Calculate the mass of NaCl in a 55 mL sample of a 3.5 M saline solution.
  3. What volume of water should be added to 2.6 g of KCl to make a 4 M solution?

Acid/Base: The Water Constant and pH

Instructions: Determine if each solution is acidic, basic, or neutral. Circle your answers.

Acidic Basic Neutral

  1. [H3O+] = 1 x 10-10 M; [OH-] = 1 x 10-4 M

Acidic Basic Neutral

  1. [H3O+] = 1 x 10-7 M; [OH-] = 1 x 10-7 M

Acidic Basic Neutral

  1. [H3O+] = 1 x 10-1 M; [OH-] = 1 x 10-13 M

Acidic Basic Neutral

  1. [H3O+] = 1 x 10-13 M; [OH-] = 1 x 10-1 M

Instructions: Calculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic.

[OH-] = Acidic Basic Neutral

  1. [H3O+] = 2.6 x 10-3 M

[OH-] = Acidic Basic Neutral

  1. [H3O+] = 2.6 x 10-8 M

[OH-] = Acidic Basic Neutral

  1. [H3O+] = 3.6 x 10-2 M

[OH-] = Acidic Basic Neutral

  1. [H3O+] = 4.3 x 10-3 M

Instructions: Calculate the [H3O+] of solutions a and b; calculate the [OH-] solutions c and d.

  1. pH = 2.76
  2. pH = 3.65
  3. pOH = 3.65
  4. pOH = 5.87

Equilibrium and Le Chateleir’s Principal

Instructions: Write the equilibrium expression for each chemical equation.

  1.  

Oxidation-Reduction Reactions

Instructions: Assign an oxidation state to each element, ion, or molecule.

  1. Cl
  2. Br2
  3. S-2
  4. Ca2+

Instructions: Assign an oxidation state to each atom in each compound.

  1.  
  2.  
  3.  
  4.  

Instructions: Assign an oxidation state to each atom in each polyatomic ion.

  1.  
  2.  
  3.  
  4.  

Instructions: Identify the oxidation state of P in each ion.

  1.  
  2.  
  3.  
  4.  
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