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2 years ago

How do the bonding and antibonding MOs formed from a given pair of AOs compare to each other with respect to:

1 answer:

6 0

Bonding MO's have lower energy than antibonding MO's. The bonding MO's lower energy, even lower than its constituent atomic orbitals, accounts for the stability of a molecule in relation to its individual atoms. However, the sum of energy of the MO's must equal the sum of energy of the AO's.

<h3>What is atomic orbital?</h3>

An atomic orbital is a function in atomic theory and quantum mechanics that describes the location and wave-like behavior of an electron in an atom. This formula can be used to calculate the likelihood of locating any atom's electron in any given location surrounding the nucleus. The phrase atomic orbital can also refer to the actual region or place where the electron is projected to be present given the orbital's mathematical form.

Each orbital in an atom is defined by a set of values of the three quantum numbers n, l, and ml, which correspond to the energy, angular momentum, and an angular momentum vector component of the electron, respectively (magnetic quantum number).

To learn more about atomic orbital visit:

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Part B When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 22.8 g of carbon were burned in the pres

aksik [14]

<u>Answer:</u> The amount of carbon dioxide gas produced in the reaction is 83.6 grams

<u>Explanation:</u>

As, some amount of oxygen gas is left after the reaction is completed. So, it is present in excess and is considered as an excess reagent.

Thus, carbon is considered as a limiting reagent because it limits the formation of product.

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of carbon = 22.8 g

Molar mass of carbon = 12 g/mol

Putting values in equation 1, we get:

$\text{Moles of carbon}=\frac{22.8g}{12g/mol}=1.9mol$

The chemical equation for the reaction of carbon and oxygen gas follows:

$C+O_2\rightarrow CO_2$

By Stoichiometry of the reaction:

1 mole of carbon produces 1 mole of carbon dioxide gas

So, 1.9 moles of carbon will produce = $\frac{1}{1}\times 1.9=1.9moles$ of carbon dioxide gas

Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 1.9 moles

Putting values in equation 1, we get:

$1.9mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(1.9mol\times 44g/mol)=83.6g$

Hence, the amount of carbon dioxide gas produced in the reaction is 83.6 grams

6 0

3 years ago

Describe the two methods of active transport.

artcher [175]

Cars and bike yesyesyesyesyeyseyeyeyeyey

7 0

3 years ago

Read 2 more answers

Would the amount of solid magnesium increase decrease or stay the same if you added a strong acid to it?

Vlada [557]

Solid Magnesium is considered as active metal so it reacts with strong acids like HCl and H₂SO₄ liberating Hydrogen gas according to the following equations:

Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g)
Mg(s) + H₂SO₄(aq) → MgSO₄(aq) + H₂(g)

so the amount of solid magnesium decrease by addition of strong acid to it.

8 0

3 years ago

A 0.652-g sample of a pure strontium halide reacts with excess sulfuric acid. the solid strontium sulfate formed is separated, d

seraphim [82]

Answer:

The formula of the original halide is SrCl₂.

Explanation:

The balanced equation of this reaction is:

SrX₂ + H₂SO₄ → SrSO₄ + 2 HX, where X is the halide.

From the equation stichiometry, 1.0 mole of strontium halide will result in 1.0 mole of SrSO₄.

The number of moles of SrSO₄ <em>(n = mass/molar mass) </em>= (0.755 g) / (183.68 g/mole) = 4.11 x 10⁻³ mole.

The number of moles of SrX are 4.11 x 10⁻³ moles from the stichiometry of the balanced equation.

n = mass / molar mass, n = 4.11 x 10⁻³ moles and mass = 0.652 g.

The molar mass of SrX₂ = mass / n = (0.652) / (4.11 x 10⁻³ moles) = 158.62 g/mole.

The molar mass of SrX₂ (158.62 g/mole) = Atomic mass of Sr (87.62 g/mole) + (2 x Atomic mass of halide X).

The atomic mass of halide X = (158.62 g/mole) - (87.62 g/mole) / 2 = 71 / 2 g/mole = 35.5 g/mole.

This is the atomic mass of Cl.

<em>So, the formula of the original halide is SrCl₂</em>.

4 0

3 years ago

Which of the following pieces of information about the element lithium describes the atomic number only

vagabundo [1.1K]

The top left corner shows the atomic number which is 3.

6 0

3 years ago