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goldfiish [28.3K]
3 years ago
6

Name the noble gas atom that has the same electron configuration as each ion in the compound rubidium oxide

Chemistry
1 answer:
Zepler [3.9K]3 years ago
3 0
In rubidium oxide - Rb₂O , the ions are Rb⁺ and O²⁻
Rb is a group one element with one valence electron. To become stable it loses its outer electron to gain a complete outer shell.
Electronic configuration of Rb is - 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 5s¹
Once it loses its valence electron the configuration is;
 - 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 
The noble gas with this configuration is Krypton - Kr

Oxygen electron configuration is 1s² 2s² 2p⁴
Once it gains 2 electrons the configuration is  - 1s² 2s² 3p⁶
The noble gas with this configuration is Neon - Ne
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Which statement concerning the hydrated hydrogen ion is incorrect? (a) Although we often represent hydrogen ions as bare protons
Harrizon [31]

Answer:C. The value of n for H+(H2O)n can be calculated for almost all solutions.

Explanation:

An hydrate can be described as a substance that contains water or with an hydrogen bonded water molecule group.

The hydrate group doesn't necessarily have a fixed formula.

5 0
3 years ago
How many moles in 30.0 grams of h3po4
jok3333 [9.3K]
Molar mass H₃PO₄ = 98.0 g/mol

1 mole ----- 98.0 g
? mole ------ 30.0 g

moles = 30.0 * 1 / 98.0

= 0.306 moles

hope this helps!


5 0
3 years ago
Good morning my friend please follow me​
Anna35 [415]
It’s night for me :D
7 0
3 years ago
Can you force the atoms into new configurations by pushing atoms around
marta [7]
<span>No, this is not possible. The reason for this impossibility is that the electrons are not attracted to one another, and thus, would repel. If you were to push the atoms into each other, the electrons would then prevent this from happening. Essentially atoms will bounce off of one another due to the repel of charges.</span>
5 0
3 years ago
If the actual yield of a reaction is 37.6 g while the theoretical yield is 112.8 g what is the percent yield
Zigmanuir [339]
<h2>Hello!</h2>

The answer is:

The percent yield of the reaction is 32.45%

<h2>Why?</h2>

To calculate the percent yield, we have to consider the theoretical yield and the actual yield. The theoretical yield as its name says is the yield expected, however, many times the difference between the theoretical yield and the actual yield is notorious.

We are given that:

ActualYield=37.6g\\TheoreticalYield=112.8g

Now, to calculate the percent yield, we need to divide the actual yield by the theoretical and multiply it by 100.

So, calculating we have:

PercentYield=\frac{ActualYield}{TheoreticalYield}*100\\\\PercentYield=\frac{37.6g}{112.8g}*100=0.3245*100=32.45(percent)

Hence, we have that the percent yield of the reaction is 32.45%.

Have a nice day!

8 0
3 years ago
Read 2 more answers
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