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Rufina [12.5K]
2 years ago
15

How many electrons can be held in the third orbital?.

Chemistry
2 answers:
Tanzania [10]2 years ago
7 0

Answer:

The third shell can hold <u><em>32 ELETRONS.</em></u> Within the shells, eletrons are further grouped into subshells of four different types, identified as S, P, D and F in order of increasing energy.

Evgen [1.6K]2 years ago
6 0
32 electrons. as the orbitals get father away from the nucleus, they hold more electrons.
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The Earth's mantle is
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Answer:

C. cooler than both the crust and the core

Explanation:

It is observed that at the mantle, temperatures range from estimatedly 200 °C (392 °F) around the upper boundary with the crust to approximately 4,000 °C (7,230 °F) at the core-mantle boundary.

So we can say the mantle is cooler than both the crust and the core.

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3 years ago
Which 3 elements had complete out shells? (you will probably need to use the periodic table)
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The inert gases like neon,argon ,krypton have complete shells
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For lunch today, I ate an apple. What type of carbohydrate did I ingest?
mafiozo [28]

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8 0
3 years ago
Calculate the density of O2(g) at 415 K and 310 bar using the ideal gas and the van der Waals equations of state. Use a numerica
Lera25 [3.4K]

Answer:

Explanation:

From the given information:

The density of O₂ gas = d_{ideal} = \dfrac{P\times M}{RT}

here:

P = pressure of the O₂ gas = 310 bar

= 310 \ bar \times \dfrac{0.987 \ atm}{1 \ bar}

= 305.97 atm

The temperature T = 415 K

The rate R = 0.0821 L.atm/mol.K

molar mass of O₂  gas = 32 g/mol

∴

d_{ideal} = \dfrac{305.97 \ \times 32}{0.0821 \times 415}

d_{ideal} = 287.37 g/L

To find the density using the Van der Waal equation

Recall that:

the Van der Waal constant for O₂ is:

a = 1.382 bar. L²/mol²    &

b = 0.0319  L/mol

The initial step is to determine the volume = Vm

The Van der Waal equation can be represented as:

P =\dfrac{RT}{V-b}-\dfrac{a}{V^2}

where;

R = gas constant (in bar) = 8.314 × 10⁻² L.bar/ K.mol

Replacing our values into the above equation, we have:

310 =\dfrac{0.08314\times 415}{V-0.0319}-\dfrac{1.382}{V^2}

310 =\dfrac{34.5031}{V-0.0319}-\dfrac{1.382}{V^2}

310V^3 -44.389V^2+1.382V-0.044=0

After solving;

V = 0.1152 L

∴

d_{Van \ der \ Waal} = \dfrac{32}{0.1152}

d_{Van \ der \ Waal} = 277.77  g/L

We say that the repulsive part of the interaction potential dominates because the results showcase that the density of the Van der Waals is lesser than the density of ideal gas.

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3 years ago
Which of the following is an isotope of scandium?<br> 40 X 40 X 4X 2X
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688x




Explanation- Your welcome
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