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Artist 52 [7]
3 years ago
9

1. For each of the molecules below, determine the electron geometry, molecule geometry, and bond

Chemistry
1 answer:
Alexxx [7]3 years ago
8 0

Answer:

CCl4- tetrahedral bond angle 109°

PF3 - trigonal pyramidal bond angles less than 109°

OF2- Bent with bond angle much less than 109°

I3 - linear with bond angles = 180°

A molecule with two double bonds and no lone pairs - linear molecule with bond angle =180°

Explanation:

Valence shell electron-pair repulsion theory (VSEPR theory) helps us to predict the molecular shape, including bond angles around a central atom, of a molecule by examination of the number of bonds and lone electron pairs in its Lewis structure. The VSEPR model assumes that electron pairs in the valence shell of a central atom will adopt an arrangement which tends to minimize repulsions between these electron pairs by maximizing the distance between them. The electrons in the valence shell of a central atom are either bonding pairs of electrons, located primarily between bonded atoms, or lone pairs. The electrostatic repulsion of these electrons is reduced when the various regions of high electron density assume positions as far apart from each other as possible.

Lone pairs and multiple bonds are known to cause more repulsion than single bonds and bond pairs. Hence the presence of lone pairs or multiple bonds tend to distort the molecular geometry geometry away from that predicted on the basis of VSEPR theory. For instance CCl4 is tetrahedral with no lone pair and four regions of electron density around the central atom. This is the expected geometry. However OF2 also has four regions of electron density but has a bent structure. The molecule has four regions of electron density but two of them are lone pairs causing more repulsion. Hence the observed bond angle is less than 109°.

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C3H8 + 5O2 → 3CO2+ 4H2O, if 5.75L of oxygen are consumed in the above reaction, how many L of carbon dioxide are produced?
anzhelika [568]

Answer: 3.45 L carbon dioxide are produced

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number 6.023\times 10^{23} of particles.

To calculate the moles, we use the equation:

\text{Number of moles}=\frac{\text{Given volume}}{\text {Molar volume}}=\frac{5.75L}{22.4L}=0.257moles

C_3H_8+5O_2(g)\rightarrow 3CO_2+4H_2O  

According to stoichiometry :

5 moles of O_2 produce =  3 moles of CO_2

Thus 0.257 moles of O_2 will produce=\frac{3}{5}\times 0.257=0.154moles  of CO_2  

Volume of CO_2=moles\times {\text {Molar volume}}=0.154moles\times 22.4L/mol=3.45

Thus 3.45 L carbon dioxide are produced

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Answer:

Diagram 1

Explanation:

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I think it’s B not quite sure ! Sorry
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What mass of sucrose c12h22o11 is needed to make 300 ml of a 0.50m solution?
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