Write a full set of quantum numbers for the following:

Chemistry

1 answer:

bogdanovich [222]10 months ago

8 0

It is known that the maximum value of ml is equal to the value of l. But the minimum value of n is as follows.

n = l + 1

where n = principal quantum number

l = azimuthal quantum number

Values of n can be 1, 2, 3, 4, and so on. Whereas the values of l are 0 for s, 1 for p, 2 for d, 3 for f, and so on.

Also, "m" is known as a magnetic quantum number whose values can be equal to -l and +l.

The electronic configuration of Li is. So here, n = 2, l = 0, m = 0 and s = ±.

Electronic configuration of is. So here, n = 4, l = 1, m = -1, 0, +1, and s = ± .

Electronic configuration of is. So here, n = 5, l = 1, m = -1, 0, +1, and s = ± The electronic configuration of B is. So here, n = 2, l = 1, m = -1, 0, +1, and s = ±.

<h3>What is quantum number?</h3>

Quantum numbers in quantum physics and chemistry explain the values of conserved quantities in a quantum system's dynamics.
Quantum numbers are quantities that can be precisely known at the same time as the system's energy and are related to the eigenvalues of operators that commute with the Hamiltonian and their corresponding eigenspaces.
A base state of a quantum system is fully described by the specification of all of its quantum numbers, which can theoretically be measured collectively.

<h3>What purpose do quantum numbers serve?</h3>

Because they can be used to determine an atom's electron configuration and the likely placement of its electrons, quantum numbers are significant.
The atomic radius and other properties of atoms, such as ionization energy, are also understood using quantum numbers.

Learn more about quantum numbers here:

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If you have a 1500 g aluminum pot, how much heat energy is needed to raise its temperature by 100°C?

Nataly [62]

The heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ.

The heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.

Explanation:

The heat energy required to raise the temperature of any body can be obtained from the specific heat formula. As this formula states that the heat energy required to raise the temperature of the body is directly proportional to the product of mass of the body, specific heat capacity of the material and temperature change experienced by the material.

So in this problem, the mass of the aluminium is given as m = 1500 g, the specific heat of the aluminium is 0.900 J/g °C. Then as it is stated that the temperature is raised by 100 °C, so the pots are heat to increase by 100 °C from its initial temperature. This means the difference in temperature will be 100°C (ΔT = 100°C).

Then, the heat energy required to raise the temperature will be

$q = m*c*del T = 1500 * 0.900 * 100 = 135000 = 135 kJ$

Thus, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100 °C is 135 kJ.

Similarly, the mass of copper pot is given as 1500 g, the specific heat capacity of copper is 0.385 and the difference in temperature is 100 °C.

Then, the heat energy required to raise its temperature will be

$q = m*c*del T = 1500 * 0.385 * 100 = 57750 = 57.75 kJ$

And the heat energy required to raise the temperature of 1500 g of copper pot by 100°C is 57.75 kJ.

So, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ. And the heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.