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Marta_Voda [28]
3 years ago
11

Which 3 elements had complete out shells? (you will probably need to use the periodic table)

Chemistry
1 answer:
wlad13 [49]3 years ago
3 0
The inert gases like neon,argon ,krypton have complete shells
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Elements in the periodic are listed according to
sammy [17]

Answer:

the raising atomic number

Explanation:

Elements are listed on the periodic table according to their atomic number.

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Atoms A and X are fictional atoms. Suppose that the standard potential for the reduction of X^2+ is +0.51 V, and the standard po
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If you are given the standard potential for the reduction of X^2+ is +0.51 V, and the standard potential for the reduction of A^2+ is -0.33, just add the two. The standard potential for an electrochemical cell with the cell is 0.18V

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To show the electron configuration for an atom, when would it be better to use an orbital notation than to use a written configu
VikaD [51]
The answer is <span>D.when the aim is to show electron distributions in shells. This is because there are some instances when elements don't possess a regular or normal electron configuration. There are those who have special electron configurations wherein a lower subshell isn't completely filled before occupying a higher subshell. It is best to visualize such cases using the orbital notation.</span>
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2 years ago
What would happen to a diver who does no exhale while surfacing from a 30 m dive?
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6 0
3 years ago
How many CO2 molecules in 0.0189 mol of CO2?
Blizzard [7]

Answer:

option C is correct = 1.14 × 10²² molecules of  CO₂

Explanation:

Given data:

Number of moles of CO₂ = 0.0189 mol

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Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

For given question:

1 mole of CO₂ =  6.022 × 10²³ molecules of  CO₂

0.0189 mol of CO₂ ×  6.022 × 10²³ molecules of  CO₂ / 1mol

1.14 × 10²² molecules of  CO₂

Thus, option C is correct.

4 0
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