Answer: Oxygen usually forms two covalent bonds or a covalent double bond.
Explanation:
A covalent bond is formed by the sharing of 2 electrons, 1 electron from each of the atoms sharing their electrons.
The number of bonds that each element can form depends on the number of valence (outermost) electrons it contains. Oxygen has 6 electrons in its valence shell and needs 2 more electrons thereby forming a double bond.
Wegener used fossil evidence to support his continental drift hypothesis. The fossils of these organisms are found on lands that are now far apart. Grooves and rock deposits left by ancient glaciers are found today on different continents very close to the equator.
Mg 10
fe 24
s 18
i 54
divide by smallest no.
mg1
fe 2.4/2
s 1.8/2
i 5.4/5
if u think this is wrong comment i will fix it
Thanks!
According to the <span> chart represented above, I have determined the pair of atoms which has the greatest polarit and I am pretty sure that it is the first option from the scale :</span>A. Al-Si. I consider this to be correct due to their incredible difference <span>difference in electronegativity.
Hope it helps!</span>
<u>Answer:</u> The activation energy for the reaction is 40.143 kJ/mol
<u>Explanation:</u>
To calculate activation energy of the reaction, we use Arrhenius equation for two different temperatures, which is:
![\ln(\frac{K_{317K}}{K_{278K}})=\frac{E_a}{R}[\frac{1}{T_1}-\frac{1}{T_2}]](https://tex.z-dn.net/?f=%5Cln%28%5Cfrac%7BK_%7B317K%7D%7D%7BK_%7B278K%7D%7D%29%3D%5Cfrac%7BE_a%7D%7BR%7D%5B%5Cfrac%7B1%7D%7BT_1%7D-%5Cfrac%7B1%7D%7BT_2%7D%5D)
where,
= equilibrium constant at 317 K = 
= equilibrium constant at 278 K = 
= Activation energy = ?
R = Gas constant = 8.314 J/mol K
= initial temperature = 278 K
= final temperature = 317 K
Putting values in above equation, we get:
![\ln(\frac{3.050\times 10^8}{3.600\times 10^{7}})=\frac{E_a}{8.314J/mol.K}[\frac{1}{278}-\frac{1}{317}]\\\\E_a=40143.3J/mol=40.143kJ/mol](https://tex.z-dn.net/?f=%5Cln%28%5Cfrac%7B3.050%5Ctimes%2010%5E8%7D%7B3.600%5Ctimes%2010%5E%7B7%7D%7D%29%3D%5Cfrac%7BE_a%7D%7B8.314J%2Fmol.K%7D%5B%5Cfrac%7B1%7D%7B278%7D-%5Cfrac%7B1%7D%7B317%7D%5D%5C%5C%5C%5CE_a%3D40143.3J%2Fmol%3D40.143kJ%2Fmol)
Hence, the activation energy for the reaction is 40.143 kJ/mol
