classify each orbital diagram for ground-state electron configurations by the rule or principle it violates.

Answers

Answer 1

Answer: The correct answer for the question that is being presented above is this one: see attached picture. Each orbital diagram for ground-state electron configurations by the rule or principle it violates: Aufbau violation, Hand violation, Pauli violation.

Assume that the arrangement as 1 - 5, then
Aufbau Violation = 5 & 2
Hand Violation = 3 & 4
Pauli Violation = 1

Answer 2

Answer: The question is incomplete:
Complete question is attached below:
.......................................................................................................................
Answer 1:
In the first case, two electrons in the 1st 2p sub-shell has both the electrons with same electron spin. This is a violation of Pauli's exclusion principle, according to which, orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.

Answer 2:
In the second case, 3s and 3p orbital is incompletely filled. This is a violation of Hund's rule. According to Aufbau Principle, orbitals of lower energy get filled first and than orbital of higher energy. Hence, in present case, 3s orbital must be completely filled first and then electron must 3p orbital.

Answer 3:
In the 3rd case, the first sub-shell of 2p orbital has two electrons, while all other sub-shell is empty. This is a violation of Hund's rule, according to which all orbitals will be singly occupied before any is doubly occupied. Hence, in present case, there should be one electron present in each sub-shell of 2p orbital.

Answer 4:
In the forth case, 4s and 4p orbital are filled first and 3d orbital is filled. This is a violation of Aufbua principle. Because, according to Aufbua principle orbital of lower energy are filled first. In present case, 3d orbital has lower energy as compared to 4s and 4p orbital.

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What is the Mr of Pb(C2H3O2)4

Answers

Answer:

Element Symbol Atomic Mass # of Atoms Mass Percent

Lead Pb 207.2 1 46.732%

Explanation:

What causes the colors observed during a flame test

Answers

By using flame test we can identify the elements because colors which are given by elements with flame test are unique.

During the flame test, the electrons of the atom which are in ground state absorb energy and go to upper level. This is called electron excitation. Excited electrons are unstable. Hence, they come back to the ground state by emitting the energy as photons.If that released energy has a frequency which belongs to visual light, then that wave gives a color.

The colors observed during a flame test are caused by the presence of certain metal ions. When these metal ions are heated by a flame, the electrons in their outer energy level get excited and move to higher energy levels. As they return to their original energy levels, they release energy in the form of light, which we perceive as different colors.

During a flame test, the colors observed are caused by the presence of certain metal ions. When these metal ions are heated by a flame, the electrons in their outer energy level get excited and move to higher energy levels. As they return to their original energy levels, they release energy in the form of light, which we perceive as different colors.

For example, when a copper compound is heated, it emits a green color. This is because copper ions are responsible for this color. Different metal ions will emit different colors, allowing us to identify them by their characteristic flame color.

Therefore, the colors observed during a flame test are a result of the specific metal ions present in the substance being tested.

Learn more about causes of colors in flame test here:

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The gases listed are at standard temperature and pressure: · 1 mol of CO2 gas · 1 mol of N2 gas · 2 mol of O2 gas Which statement is correct? The volume of 1 mol of CO2 is greater than that of 2 mol of O2 . The volume of 1 mol of CO2 is greater than that of 1 mol of N2 . The volumes of 2 mol of O2 and 1 mol of N2 gases are the same. **The volumes of 1 mol of CO2 and 1 mol of N2 gases are the same.**

Answers

Answer : The volume of 1 mole of $CO_(2)$ and $N_(2)$ gases are the same.

Solution: Given,

Moles of $CO_(2)$ = 1 mole

Moles of $N_(2)$ = 1 mole

Moles of $O_(2)$ = 2 mole

Formula used for ideal gas is :

P V = n R T

According to the question, the gases are at standard temperature and pressure. So, the volume of gases only depends on the number of moles. This means that the higher the number of moles, higher will be the volume of gas.

The moles of $O_(2)$ are more than the moles of $CO_(2)$ and $N_(2)$ . So, the volume of $O_(2)$ will be more.

And the moles of $CO_(2)$ and $N_(2)$ are equal. Therefore, their volumes are also equal.

Therefore, the best option is the volume of 1 mole of $CO_(2)$ and $N_(2)$ gases are the same.

The right answer for the question that is being asked and shown above is that: "The volumes of 1 mol of CO2 and 1 mol of N2 gases are the same." The statement that is correct as far as the gases listed are at standard temperature and pressure is concerned is that the volumes of 1 mol of CO2 and 1 mol of N2 gases are the same

seawater contains % (by mass) of potassium. how many grams of potassium are there in 2.86 l of seawater? the density of seawater is 1.025 .