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PtichkaEL [24]
3 years ago
13

White phosphorus is composed of tetrahedral molecules of P4 in which every P atom is connected to three other P atoms. In the Le

wis structure of P4, there are 1. 6 bonding pairs and 4 lone pairs of electrons. 2. 6 bonding pairs and no lone pairs of electrons. 3. 5 bonding pairs and 4 lone pairs of electrons. 4. 3 bonding pairs and 4 lone pairs of electrons. 5. 6 bonding pairs and 2 lone pairs of electrons.

Chemistry
1 answer:
Dmitrij [34]3 years ago
4 0

Answer:

In the Lewis structure of P4 there are 6 bonding pairs and 4 lone pairs of electrons.

Explanation:

The structure of tetrahedral molecule of P4 is provided below.

Each phosphorus atom has 5 valence electrons out of which 3 electrons involve in bonding and the rest 2 electrons exist as a lone pair that does not involve in bonding.Hence each phosphorus atom has one lone pair.In P4 molecule there are phosphorus atoms and hence 4 lone pairs in total.

As you can see in the figure, each phosphorus atom is bonded to the other three atoms.A bond is formed when two atoms share one electron each and the pair is called bonding pair.

From the figure we can see that there are 6 bonds in total.Each bond consist of one bonding pair of electrons and hence in total there are 6 bonding pairs of electrons.

Hence in a P4 molecule there are six bonding pairs and 4 lone pairs of electrons.

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Explanation:

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3 years ago
Given the reaction _K(s) +_ Cl2(g) → _KCl(s) what is the amount of K, in grams, needed to completely react with 2 moles of Cl2(g
damaskus [11]

Answer:

156.4g K

Explanation:

I'm not sure if it is correct but I think it should be this

What do we know so far?: 2K + 1Cl2 -> 2KCl, 2 mol of Cl2

What are we looking for?: #g of K

What is the ratio of K to Cl2?: 2:1

Set up equation: 2molCl2 x \frac{2mol K}{1 mol Cl2}

Cancel unwanted units: 2 x \frac{2mol K}{1}

Answer we got: 2 x 2mol K = 4mol K

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2 years ago
Which is heavier? 30kg or 60lb?
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3 years ago
Wastewater discharged into a stream by a sugar refinery contains 3.40 g of sucrose (C12H22O11) per liter. A government-industry
Ipatiy [6.2K]

<u>Answer:</u> The pressure that must be applied to the apparatus is 0.239 atm

<u>Explanation:</u>

To calculate the osmotic pressure, we use the equation for osmotic pressure, which is:

\pi=iMRT

or,

\pi=i\times \frac{m_{solute}}{M_{solute}\times V_{solution}\text{ (in L)}}}\times RT

where,

\pi = osmotic pressure of the solution

i = Van't hoff factor = 1 (for non-electrolytes)

m_{solute} = mass of sucrose = 3.40 g

M_{solute} = molar mass of sucrose = 342.3 g/mol

V_{solution} = Volume of solution = 1 L

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature of the solution = 20^oC=[20+273]K=293K

Putting values in above equation, we get:

\pi =1\times \frac{3.40g}{342.3g/mol\times 1}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 293K\\\\\pi =0.239atm

Hence, the pressure that must be applied to the apparatus is 0.239 atm

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3 years ago
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