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between H₂S and H₂Se why does H₂Se have a higher boiling point even though it has a weaker dipole-dipole?

405169322

What is the chemical formula for Bisethylenediaminediiodomanganese (IV) ion?

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What is the chemical formula for Pentaamminenitritonickel(III)?

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yes, because HOCl is more stable. Mainly because the O–H bond in HOI is stronger than the O–H bond in HOCl. Making HOCl more likely to donate a proton.

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what is the chemical formula for Triamminetriaquachromium (III) chloride?

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What is the name of this compound? [Cr(ox)(Cl)₃]-

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Thanks!

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What is the name of the compound? K₂[Ni(CN)₄]

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The Cisplatin bonds with two guanine molecules in DNA which prevents the DNA from functioning. Also if it was transplatin it would only make one bond and would not be effective.

I hope this helps :0

lol

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The soapy feel is associated with the base's ability to dissolve oils and fatty acids on your skin which removes friction, leading to a slippery/soapy feel.

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The transition metal does not have a suffix so it should go later the name. I hope that helps.

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Shouldn't the number of ligands be given?

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This website covers in detail all common molecular shapes with angles. It also gives examples of these molecules with lone pairs and multiple lone pairs. http://web.gccaz.edu/~rob2108739/Geomet ... Tables.pdf

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The orbital that have head-on overlap leads to a sigma bond which is is a strong bond. Especially when compared to a pi bond; formed with two atoms with overlapping p orbitals.

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I believe at its base, stronger bonds would increase boiling point. However, the strength of the bonds in the molecule could be entirely based off the molecular structure. It's a combination of both that controls the boiling point, viscosity, etc.

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Q: What did one angry water molecule say to the other water molecule?
A: Get bent!

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If the molecule in question is completely symmetric than the dipole moment will cancel itself out.

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I believe the two lone pairs on the top of the oxygen, creating the bent shape, is because of the overall polarity of the molecule. The two hydrogen atoms both have a partial positive helps maintain the polarity and therefore would repulse the two lone pairs. Not certain but I hope that helps.

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4.11 Using Lewis structures and VSEPR, give the VSEPR formula for each of the following species and predict its shape:
(a) sulfur tetrachloride;
(b) iodine trichloride;
(c) IF4-;
(d) xenon trioxide.

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4.3 Draw the structures and name the shapes of the following
molecules: (a) HCN; (b) CH2F2.

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Using this equation: E(photon) - E(removed e-) = E(kinetic). you can solve for the difference in energy for kinetic.

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Hello! The criteria "1 atm and 25 degrees Celsius" is called Standard State: "conditions specifies 1 atm of pressure, that liquids and gases be pure, and that solutions be at 1 M concentration. Temperature is not specified, although most tables compile data at 25°C (298 K)."( htt...

CHEMISTRY COMMUNITY

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churro 38

churro 32

churro 31

Re: HOCl vs HOI

churro 30

churro 29

Re: churro 27

churro 27

Re: Cisplatin

Re: “Soapy” feel of bases

Re: Transition Metal in naming

Re: Ligands

Re: Shapes

Re: Orbital Overlap

Re: Bonds vs Shapes [ENDORSED]

Re: Post All Chemistry Jokes Here

Re: Dipole moments

Re: Position of Lone Pairs in H20

4.11 6th Edition

4.3 Draw the structures and name the shapes of the following molecules: (a) HCN; (b) CH2F2.

Re: Light Intensity

Re: Limting Reactant Calculations