explain why a s bond formed by overlap of an s orbital with an sp3 orbital of carbon is stronger than a sbond formed by overlap
1 answer:
orbital have less electron density than p orbital. Therefore on overlap of s orbital with
less repulsion take place than overlapping of sp3 orbital.
Electronegativity depends on s character.
In there is hybridization between one s and 3 p orbital. Therefore,
have 25% of s character .
In p orbital , there is no s orbital present. Therefore s character is p orbital is % .
Higher the electronegativity means higher tendency to attract electron.
Thus, bond form by overlap of and
will be stronger than bond formed by overlap of
with
.
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Answer:
yes the Bohr model predicts their spectra accurately
Explanation:
The Bohr model based on one electron system
The atom H has a single atom and the ion Be+3 has a single atom as well and this proves that the Bohr model predicts their spectra accurately .
also apply the equation model to further explain
E =
z = atomic number
for H the value of z = 1
for Be+3 the value of z = 4
when this values are substituted into the equation above
E = , E =
this results show that the energy level of Be+3 is higher than the energy level of H by a factor of 16 , and this shows that their line patterns are similar