<span>109.5°.
VESPR helps predict the bond angles with the electrons being the most out. By looking that the structure of the molecule, one Si and four H, the Si atom can be seen as the center and the four H atoms can be seen around it. Now think about how the H atoms would be placed, ideally they would be placed the farthest distance from each other equidistant. So in this case it would be 109.5°.</span>
<u>Answer:</u> The percentage abundance of 
and 
isotopes are 75.77% and 24.23% respectively
<u>Explanation:</u>
Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.
Formula used to calculate average atomic mass follows:
.....(1)
Let the fractional abundance of isotope be 'x'. So, fractional abundance of isotope will be '1 - x'
- <u>For isotope:</u>
Mass of isotope = 62.9396 amu
Fractional abundance of isotope = x
- <u>For isotope:</u>
Mass of isotope = 64.9278 amu
Fractional abundance of isotope = 1 - x
- Average atomic mass of copper = 63.546 amu
Putting values in equation 1, we get:
![63.546=[(62.9396\times x)+(64.9278\times (1-x))]\\\\x=0.6950](https://tex.z-dn.net/?f=63.546%3D%5B%2862.9396%5Ctimes%20x%29%2B%2864.9278%5Ctimes%20%281-x%29%29%5D%5C%5C%5C%5Cx%3D0.6950)
Percentage abundance of isotope = 
Percentage abundance of isotope = 
Hence, the percentage abundance of and isotopes are 69.50% and 30.50% respectively.
Answer:
33 Neutrons
Explanation:
Atomic Mass = # of Protons + # of Neutrons
Atomic Number = Proton count
Atomic Mass of Co = 27 Protons + x Neutrons
60 = 27 + x
x = 33
The answer is <span>Fluorine my dude
</span>
The limiting reactant between the reaction of 6 moles of oxygen and 12 moles of mercury is mercury (Hg)
<h3>Balanced equation </h3>
4Hg + O₂ —> 2Hg₂O
From the balanced equation above,
4 moles of Hg reacted with 1 mole of O₂
<h3>How to determine the limiting reactant</h3>
From the balanced equation above,
4 moles of Hg reacted with 1 mole of O₂
Therefore,
12 moles of Hg will react with = 12 / 4 = 3 moles of O₂
From the above calculation, we can see that only 3 moles of O₂ out of 6 moles given is required to react completely with 12 moles of Hg.
Thus, Hg is the limiting reactant and O₂ is the excess reactant .
Learn more about stoichiometry:
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