Micoscale Reactions Explorer Blog

• Draw a Lewis structure for an ionic bond between potassium and iodine.  Draw a Lewis structure for an ionic bond between lead(II) and iodine. Why do they differ?

• [K]+1 [I]-1
• [Pb(II)]+2 [I]2^-2

These differ because when potassium and iodine are combined they are neutral, meaning they have balanced charges. Lead (II) and iodine however,are not balanced and an another idoine atom must be added in order for the elements to be neutral.

• What determines the formula in an ionic compound? (including: what determines the number of ions needed, how do you know how many ions you have in a compound, and why is the formula in that order?)

 The elements charge determines the formula in an ionic compound. The charge can easily be determined by the number of valence electrons the atom gains or loses. The ions are shown in the formula as capital letters,underneath these letters are numbers called subscripts which tell how many there are. The parentheses are an identification that a subscript applies to more than one element in the compound formula. In any compound,the cation (+) is always written before the anion  (-) 

• How are ionic compounds named?  Provide examples.

In order to name an ionic compound first you must identify which element have cations and anions. Then you can use one of two methods,the criss cross method or setting the cation and anions equal to zero. I set the ions equal to zero and if they are neutral than you don't have to change (multiply,add,etc.) the element. If no changes are made there will most likely be no subscripts. If there are changes then,for example,whatever you multiply the ion by will be the subscript of that element. But always keep in mind that cations ALWAYS come first in an ionic compound.

Some examples are:

• Cu(OH)2= Copper(II) Hydroxide
• MgCO3= Magnesium Carbonate
• AgCl= Silver Chloride

Chemical Bonding Lab

1) The types of elements that make up the compounds are:
•Calcium chloride- Where calcium is a metal,and chloride is nonmetal.

•Potassium iodide- Where potassium is a metal,and iodine is nonmetal.

•Sodium chloride- Where sodium is a metal,and chloride is nonmetal.

•Citric acid- Where carbon,hydrogen,and oxygen are nonmetals.

•Phenyl salicylate- Where carbon,hydrogen,and oxygen are nonmetals.

•Sucrose- Where carbon,hydrogen,and oxygen are nonmetals.

2) In terms of the periodic trends,non metals have high electronegativity levels and ionization energies and metals have low electronegativity levels and ionization energies. Potassium iodide,Calcium chloride,and sodium are similar because they are all conductors,and they did not melt. Phenyl salicylate,sucrose,and citric acid are similar because they are non metals and contain carbon,oxygen,and hydrogen.

3) Calcium chloride,potassium iodide,sodium cholride are ionic. Citric acid, phenyl salicylate,and sucrose are covalent. Covalent bonds is the sharing of electron pairs between atoms. Ionic bonding a complete transfer of valence electrons between atoms.

4) My results showed that covalent compounds have low melting points and are soluble in ethanol, and very weak conductors of electricity. This lab also showed that ionic compounds are soluble in water,have high melting points,and are good conductors of electricity.

Metals & Water Explore Lab

● The orders of the metals from most reactive to least reactive are, K-Potassium Na-Sodium Ca-Calcium Mg-Magnesium Cu-Copper.

● Potassium(k) is the most reactive because when the Potassium was placed into the water it sparked a purple flame and moved rapidly across the water and then dissappeared. Sodium(Na) was the second most reactive because when it touched the water it floated across the water rapidly without any spark. Calcium(Ca) was the third most reactive because bubbled and produced a hydrogen gas and it turned the water a magenta color when the phenolphthalein was added. Magnesium(Mg) was the second least reactive because all it did was turn white and when phenolphthalein was added it was a neutral solution. The strip of magnesium also floated to the top of the distilled water. Copper was the least reactive because there was a neutral reaction. Nothing had changed the copper besides when we added the phenolphthalein the water had turned white and there was a little pink.

● Na, atomic #11
    [Ne] 3s1

    Mg, atomic #12
     [Ne] 3s2
 
    K, atomic #19
     [Ar] 4s1

     Ca, atomic #20
      [Ar] 4s1
 
      Cu, atomic #29
       [Ar] 3d10 4s1

● If zinc was added it would be placed after copper and if rubidium was added it would be placed after K, potassium, because in the periodic table the most reactive elements increase down the periodic table and decrease across.

3 question blog

The tasks I have completed  lately include the flipped 3.2 and 3.3 notes and also the Electron configuration POGIL. Recently, I have learned how to calculate wavelength, light, and frequency as well as how to do electron configurations based off Pauli's, Huns, and Aufban's rules and principles. According to Pauli's rule, no two electrons in the same atom can have the same energy. Hund's rule states that electrons can not double up in an orbital until it's necessary. Aufban's principle states that electrons have a specific order. Next, I plan on completing the Ch4 practice questions and take the chapter 3 test.

Flame test lab

1. The elements can be distinguished based off the color of the flame. My results showed that Lithium (Li) was red, Sodium (Na) was orange, Potassium (K) was lavender, Calcium (Ca) was a red orange, Strontium (Sr) was a lighter red, Barium (Ba) was yellow, and Copper (Cu) was green.

2. My group and I were able to identify the unknowns. Unknown #1 was calcium. Unknown #2 was lithium. We identified these based off the color of the flame that was shown while it burned.

3. Cesium was not an element that was used because none of the colors in the second clip resembled the color of cesium.

4. The element loses energy as it is heated and put into the fire. The flame gains energy from the color the element made as it burned in the flame.

3 Question Blog

The tasks I have completed lately include the isotope abundance lab, the notes over the structure of the atom and the history behind it. Also, the unit 2 test. Recently, I've learned how to calculate the average atomic mass and how to differentiate the charges of electrons, protons, and neutrons. Electrons have a negative charge, protons have a positive charge, and neutrons have no charge. I've also learned how to count subatomic particles and nucleons. Also, how to identify everything within the elements including the atomic number, the mass number and so forth. Next I am planning to complete the placement #1 and the electron JiTT assignments.

3 question Blog

So far, I have completed every task that has been given to me. Such as the conclusions and calculations for the labs in Chemistry. Its been tough but I'm doing my best to finish everything when it's due. I have learned many things such as how useful significant digits are, and also the different properties of matter and much more. The notes help me to get a better understanding of everything which makes it easier to follow. Now, I'm preparing myself for the chemical and physical properties lab by listing the chemicals and other materials that will be used. Also reading and writing the safety precautions for this lab which is extremely important.

Interactions of Powder/ Identifying White Powders

Today we combined liquids and white powders! The liquids we used were Vinegar, DI H2O, and Iodine. The Powders we used consisted of Baking Soda, Corn Starch, and Baking Powder. We combined Corn starch with Iodine, then with Baking Powder, and also with Baking soda. We combined Vinegar and DI H2O also with all the powders. In which all were seperated. My partner and I were able to distinguish the Powders by looking at them and seeing how they reacted. For example, Iodine and Corn Starch changed colors and so did Iodine and Baking powder and also, Iodine and Baking Soda. Vinegar and Baking Powder bubbled, as did Vinegar and Baking Soda, and DI H2O also bubbled when it was mixed with Baking Soda and also, Baking Powder. DI H2O and Cornstarch Dissolved as well as Vinegar and Cornstarch. We were given results that would allow us to identify a unknown powder, in which we did! We noticed that the powder bubbled with DI H2O and Vinegar and also changed colors when we added iodine, so the powder must've been Baking Soda! It was a fun and interesting lab!!

Accuracy and Precision in the Food Industry

Today we determined if we actually received what we pay for with food, using chips. The answer is no! The bags of chips were not accurate. We calculated the acceptable range to determine the accuracy. Using the bags net weight that was provided, we added 0.10 grams to the initial bag net weight to find the highest range and subtracted 0.10 to find the lowest range. We then took the chips out, and ate them... thats why the bag is empty in the picture below. Yum! We ended up weighing the empty bag  which is known as the tare weight. The weight of the bag moved two decimal places because it no longer included the chips. Regardless if you moved the decimal more places it wouldn't have impacted the precision or accuracy because it would have been outside out the range. Precision and accuracy are similar but somewhat different. Precision is the closeness of two or more measurements. Accuracy is the true value.

Bouncy Ball Explore Blog

Hello everyone! We made our own bouncy balls out of glue and borox. We learned that the less amount of glue used, the higher the ball will bounce. Of course my partner and I learned that from experience. As you can see in the picture below, we used way to much glue! In this experiment, the glue was the independent variable and the borox was the dependent variable since the glue was being hardened by the borox. It would be slightly difficult for someone to duplicate the exact size and weight of the bouncy ball I created because I forgot to write how much of each material I used! Oops! Anyways, trial and error is science because without it, it would be difficult to prove if something is true or false without testing your theory.