Title | Activity - Molecule polarity demonstration-1 |
---|---|
Author | Nidhi Karavadra |
Course | middle english literature |
Institution | Virtual High School |
Pages | 3 |
File Size | 122.6 KB |
File Type | |
Total Downloads | 53 |
Total Views | 160 |
HI THIS IS A NICE DOCUMENT ITS ABOUT ENGLISH...
Molecule Polarity Simulation Visit the Molecule Polarity simulator. 1. Select the “Real Molecules” simulation option (click on the “Real Molecules Only in Java” link; you will then be prompted to download the simulation). Once you download the simulation to your device, open the simulation and begin the activity. Set 1: HF vs. H2 For each molecule be sure to have the “Atom Labels” and “Atom Electronegativies” button selected. Use the “Bond Dipoles” and “Molecular Dipoles” buttons to determine if these dipoles are present when instructed below. (a) Use the simulation to determine if bond dipoles are present on each molecule. (b) Use the simulation to determine if a molecular dipole is present on each molecule. (c) Use the simulation “Electrostatic Potential” option to map the electron density on each molecule. Molecule
H2
Electronegativit y Difference between atoms 2.1 – 2.1 = 0
Bond Dipoles Molecular Present? Dipole Present? (yes or no) (yes or no) no no
HF
4.0 – 2.1 = 1.9
yes
Sketch/describe the Electrostatic Potential
yes
Question 1: Using what you learned from Set 1, predict what properties of the molecule determine if a molecular dipole is present or not. - Molecules with non-polar bonds will be non-polar. Molecules with polar bonds might be polar. Set 2: Repeat the data collection carried out in Set 1 for each set molecules below. Be sure to have the “Atom Labels” “Atom Electronegativies” button selected. Use the “Bond Dipoles” and “Molecular Dipoles” buttons to determine if these dipoles are present when instructed below. (a) Use the simulation to determine if bond dipoles are present on each molecule. (b) Use the simulation to determine if a molecular dipole is present on each molecule. (c) Use the simulation “Electrostatic Potential” option to map the electron density on each molecule. Molecul e BF3
Electronegativit y Difference between atoms 4.0 – 2.0 = 2.0
Bond Dipoles Molecular Present? Dipole Present? (yes or no) (yes or no) Yes No
Sketch/describe the Electrostatic Potential
NH3
3.0 – 2.1 = 0.9
Yes
Molecul e H2O
Electronegativit y Difference between atoms 3.5 – 2.1 = 1.4
Bond Dipoles Molecular Present? Dipole Present? (yes or no) (yes or no) Yes Yes
CO2
3.5 – 2.5 = 1.0
Yes
No
Molecul e
Electronegativit y Difference between atoms 2.5 – 2.1 – 0.4
Bond Dipoles Present? (yes or no) Yes
Molecular Dipole Present? (yes or no) No
CH3F
C-H 2.5 – 2.1 = 0.4 C-F 4.0 – 2.5 = 1.5
Yes
Yes
Molecul e H2O
Electronegativit y Difference between atoms 3.5 – 2.1 = 1.4
Bond Dipoles Molecular Present? Dipole Present? (yes or no) (yes or no) Yes Yes
NH3
3.0 – 2.1 = 0.9
Yes
Molecul e
Electronegativit y Difference between atoms C-H 2.5 – 2.1 = 0.4 C-F 4.0 – 2.5 = 1.5 C-H 2.5 – 2.1 = 0.4 C-F 4.0 – 2.5 = 1.5
Bond Dipoles Molecular Present? Dipole Present? (yes or no) (yes or no) Yes Yes
CH4
CH3F
CHF3
Yes
Yes Sketch/describe the Electrostatic Potential
Sketch/describe the Electrostatic Potential
Sketch/describe the Electrostatic Potential
Yes
Sketch/describe the Electrostatic Potential
Yes
Analyze and Evaluate: (a) Compare the molecules that have a net molecular dipole and those that do not. What are the common features for the molecules that have net molecular dipoles? - Molecules with net dipoles have polar bonds and asymmetrical shapes.
(b) Compare the molecules that have a net molecular dipole and those that do not. What are the common features for the molecules that DO NOT have net molecular dipoles? - Molecules with no net dipoles either have non-polar bonds, or have polar bonds and symmetrical shapes. (c) Create a general statement that summarizes how you can predict if a molecule will polar or not (i.e., create a statement that begins “A molecule will have a net molecular dipole if…”). - A molecule will have a net molecular dipole if it has polar bonds and a VSEPR shape that is asymmetrical....