All categories

2 years ago

Write an equation that shows the formation of the phosphide ion from a neutral phosphorus atom.

Chemistry

2 answers:

atroni [7]2 years ago

8 0

Answer: $P+3e^-\rightarrow P^{3-}$

Explanation: Phosphorous atom is the element with atomic number 15 and thus contains 15 electrons.

$P:15:1s^22s^22p^63s^23p^3$

Thus it is short of 3 electrons to attain stable noble gas configuration. Thus it gains three electrons and converts to phosphide ion $(P^{3-})$ with 18 electrons.

$P^{3-}:18:1s^22s^22p^63s^23p^6$

Vlad1618 [11]2 years ago

5 0

From reference or science books, we can actually know that the elementary charge of phosphorus is -3. Since it is negative, this means that it has an excess of electrons, which further means that it takes up 3 electrons to become an ion. Therefore the equation can be written as:

P + 3e ---> P3-

You might be interested in

How many grams of antifreeze C2H4(OH)2 would be required per 500 g of water to prevent the water from freezing at a temperature

Wewaii [24]

Answer:

333.7 g.

Explanation:

The depression in freezing point of water (ΔTf) due to adding a solute to it is given by: ΔTf = Kf.m.

Where, ΔTf is the depression in water freezing point (ΔTf = 20.0°C).

Kf is the molal freezing point depression constant of the solvent (Kf = 1.86 °C/m).

m is the molality of the solution.

∴ m = ΔTf/Kf = (20.0°C)/(1.86 °C/m) = 10.75 m.

molaity (m) is the no. of moles of solute per kg of the solvent.

∵ m = (no. of moles of antifreeze C₂H₄(OH)₂)/(mass of water (kg))

∴ no. of moles of antifreeze C₂H₄(OH)₂ = (m)(mass of water (kg)) = (10.75 m)(0.5 kg) = 5.376 mol.

∵ no. of moles = mass/molar mass.

∴ mass of antifreeze C₂H₄(OH)₂ = no. of moles x molar mass = (5.376 mol)(62.07 g/mol) = 333.7 g.

5 0

2 years ago

You are planning to prepare 600 mL of 20% dextrose solution, by mixing your 5% and 50% dextrose solution. How much of each solut

PilotLPTM [1.2K]

Hdjdjejejeuuwuwjwjwjwwjwhwhwhehehehehehdhdhdhdhdhdh

3 0

2 years ago

The electron in a ground-state H atom absorbs a photon of wavelength 97.20 nm. To what energy level does it move?

Lunna [17]

Answer:

E = h v = 6.626 x $10^{-34}$ x 97.20 x $10^{-9}$ = 6.44 x $10^{-41}$ J = 4.01 x $10^{-22}$ eV

n = Energy Level = $-E^{0}$ / E = -13.6 / 4.01 x $10^{-22}$ = 3.39 x $10^{22}$ = 1.84 x $10^{11}$ energy level...

7 0

2 years ago

Cyclohexane has a freezing point of 6.50 ∘C and a Kf of 20.0 ∘C/m. What is the freezing point of a solution made by dissolving 0

ExtremeBDS [4]

Answer:

The freezing point will be $2.9^{0}C$

Explanation:

The depression in freezing point is a colligative property.

It is related to molality as:

$Depressioninfreezing point=K_{f}Xmolality$

Where

Kf= $20\frac{^{0}C}{m}$

the molality is calculated as:

$molality=\frac{moles_{solute}}{mass_{solvent}}$

$moles=\frac{mass}{molarmass}=\frac{0.694}{154}=0.0045mol$

$massofcyclohexane=25g=0.025Kg$

$molarity=\frac{0.0045}{0.025}=0.18m$

Depression in freezing point = $20X0.18=3.6^{0}C$

The new freezing point = $6.5^{0}C-3.6^{0}C=2.9^{0}C$

5 0

2 years ago

An irregularly shaped solid which has a mass of 10.283g was placed in a graduated cylinder containing an inert liquid. The initi

Gwar [14]

Liquid + Solid = 8.89 mL
V ( Solid ) = 8.89 mL - 6.26 mL = 2.63 mL
The density of the solid = m / V = 10.283 g / 2.63 mL =
= 3.9 g/mL = 3.9 g / cm³

3 0

2 years ago