Covalent and Ionic Virtual lab 2021-2022 PDF

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Chemistry: Ionic & Covalent Chemical Bonding Virtual Lab Name: Marcia Murillo Grade/Section: 10A Pre-Virtual Lab Questions: Answer these before going to the website to begin the virtual lab. 1. Metals are located on the right/left (circle one) of the periodic table. Non-metals are located right/left (circle one) on the periodic table? 2. What subatomic particle(s) participate in chemical bonding? _electrons______________________________ 3. In your own words, define valence electrons. It’s the number of electrons that will be in the outermost energy level. Virtual Lab Procedure: Go to the website http://www.teachchemistry.org/bonding (located also on my website). Once you get to the website, you should see a picture of the Periodic Table on your screen.

Part I: Ionic Bonding 1. Choose Sodium (Na). a. What type of element is it? Metal b. How many valence electrons does it have? _1 2. Choose Fluorine (F). a. What type of element is it? non metal b. How many valence electrons does it have? 7 3. Answer the question on the screen, “What type of bond is this combination likely to form?”

a. Circle: Ionic or Covalent?

b. Choose the appropriate number of atoms to make the bond. Record the number of each atom below: #Na atoms 1

#F atoms 1

4. Watch the final animation closely (it will play continuously). a. Describe the change in the number of valence electrons in the atoms as the bond is successfully formed: The sodium is left with zero valence electrons and a positive charge, while the fluorine now has 8 valence electrons and a negative charge.

b. What does the positive (+) charge indicate (mention specific subatomic particles in your answer)? It indicates that the atom gave away electrons. c. What does the negative (-) charge indicate (mention specific subatomic particles in your answer)? It indicates that all the atoms received electrons. d. What is the final overall charge of the compound? neutral e. What is the name and formula for the compound formed? Sodium Fluoride NaF 5. Reset the selected data using the Reset symbol (arrow that looks like an “undo” button) 6. Choose Calcium (Ca). a. What type of element is it? metal b. How many valence electrons does it have? 2 7. Choose Chlorine (Cl). a. What type of element is it? non metal b. How many valence electrons does it have? 7 8. Answer the question on the screen, “What type of bond is this combination likely to form?” a. Circle: Ionic or Covalent? b. Choose the appropriate number of atoms to make the bond. #Ca atoms 1 #Cl atoms 2

9. Watch the final animation closely (it will play continuously). a. Why were more than 2 total atoms needed to create this compound? Because it will be complete with more than 2 atoms Explain what happened to the valence electrons in each atom. Calcium had two valence electrons, and chlorine just needed another for a total of eight, so you combine two calcium atoms into two different chlorine atoms, giving each chlorine approximately eight valence electrons. b. What is the final overall charge? neutral c. What is the name AND formula for the compound formed? Calcium Chloride CaCl2

10. Reset the selected data using the Reset symbol (arrow that looks like an “undo” button)

11. Using a Periodic Table, complete the chart below. Then, use the simulation to check your answers by clicking on the appropriate elements to make each compound.

Atom #1

# Valence

Ion

Atom #2

# Valence

Ion

Na

Electrons 1

Charge 1

O

electrons 6

Charge -2

K

1

1

F

7

Mg

2

2

Cl

Ca

2

2

Al

3

3

Formul

Name

a Na2O

Sodium Oxide

-1

KF

Potassium Fluoride

7

-1

MgCl2

Magnesium Chloride

N

5

-3

Ca3N2

Calcium Nitride

S

6

-2

Al2S3

Aluminum Sulfide

Part II: Covalent Bonding

1. Now, you will investigate diatomic molecules, those that are made up of two of the same type of atom. Select 2 fluorine atoms. a. How many valence electrons are in each fluorine atom? 7 b. Is a fluorine atom a metal or a non-metal? nonmetal c. Did the combination of these atoms create a covalent or ionic bond? covalent bond d. How are the valence electrons organized to form a bond between these atoms? They share 1 electron each to add up to 8 on the atoms. e. How is this different from the ionic bonds formed in the previous part of the activity? In this case, the atoms are linked electrons, resulting in both having eight valence electrons, whereas in ionic bonds, one atom gives electrons to another, leaving just one with eight valence electrons.

2. Select 2 oxygen atoms.

a. How many valence electrons are in each oxygen atom? 6 b. Is an oxygen atom a metal or a non-metal? nonmetal c. Did the combination of these atoms create a covalent or ionic bond? Covalent bond d. How are the valence electrons organized to form a bond between the atoms? They share four electrons, allowing them to each have eight valence electrons. How is this bond different from the bond in the fluorine molecule in question 1? Both atoms share two electrons in this link, giving each of them eight valence electrons, whereas in the fluorine molecule bond, just one electron from each atom was shared.

Part III: Post Lab Questions

1. What are the differences between ionic and covalent bonds? Be sure to refer to valence electrons in your response. An atom sends its valence electrons to another atom in an ionic bond, resulting in one of the atoms having eight valence electrons. In a covalent bond, both atoms share their valence electrons, allowing them to have a total of 8 valence electrons. 2. How is the naming of ionic and covalent compounds different? In ionic compounds you only add -ide to the ending of the nonmetal, and in covalent compounds you change the ending of the element to -ide and if necessary add a prefix....