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lavenderhound360Lv1

6 Oct 2020

Fluorine reacts with sulphur to form several covalent compounds. Three of these compounds are SF2, SF4, and SF6. Draw the Lewis structures for these compounds, and predict the molecular structures (including bond angles). Would you expect OF4 to be a stable compound?

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Iris MandiaLv9

17 Nov 2020

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Consider the following compounds: These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each. What is the molecular structure of each of the compounds? What are the bond angles and the polarity of each? (a polar molecule has a net dipole moment when a nonmolecule does not.)

pinkporpoise652

Please answer a and b for these two compounds:[Ni(CN)5]3- and MnO4-

a,) For the following transition metal compounds first draw theLewis structure in 100% ionic form and assign the metal oxidationstate, then draw the 100% covalent form with all single bonds. Ifappropriate, draw additional resonance structures with multiplemetal Lewis base covelant bonds. Be sure to include all formalcharges in the covalent forms.

b.) For compounds that you identify as having partially ionicsingle bonds, use Pauling's electroneutrality principle to estimatethe % covalency of the metal Lewis base bonds. For compounds thatyou identify as having resonance structures with multiple covalentbonds, use Pauling's electroneutrality principle to identifyresonance form(s) likely to be most stable.

You are encouraged to make educated guesses, provided they areaccompanied with reasoned arguments.

Experiment 1:

Molecular Models of Neutral Molecules

In this experiment, you will predict the three-dimensional geometry of a series of neutral molecules using the VSEPR theory.

Procedures

Part 1: Use your Periodic Table of Elements to determine the elemental symbol, group number and valence electrons for the elements listed in Table 1.

Table 1: Lewis Dot Structures

Element	Symbol	Group Number	Valence Electrons	Lewis Dot Structure
Hydrogen	H
Carbon	C
Chlorine	Cl
Aluminum
Oxygen	O
Fluorine	F
Neon	Ne
Nitrogen	N

Part 2: Construct the three-dimensional geometry for the molecules listed in Table 2.

Table 2: Molecular Models

Molecule (central atom is underlined)	Shape Name Bond Angle	Bond Angles (more than one may be possible)
CO2	Linear
AlCl3	Trigonal Planar
H2O	Bent
NH3	Trigonal pyramidal
CCl4	Tetrahedral
PCl5	Trigonal bipyramidal
SF6	Octahedral

Post-Lab Questions:

1. What is the molecular geometry (shape) of the methane molecule (CH4)? Explain completely why all the bond angles in methane are equal.

2. What is the molecular geometry (shape) of the chloromethane molecule (CH3Cl)? Explain completely why NOT all of the bond angles in chloromethane are equal.

3. Chloromethane can be thought of as resulting from methane via the replacement of one Hydrogen atom with a Chlorine atom. Subsequent replacements of H with Cl yield dichloromethane (CH2Cl2), trichlormethane (CHCl3) and tetrachlormethane (CCl4). Which of these three previous molecules will have all bond angles equal to each other? Explain completely.

4. Sketch the molecular shape of the compounds in the table below. Be sure to identify the bond angles. H₂ Cl₂ SO₂ NH₃ MoF₆