Question
Explain with example $: i. s-s \ \sigma$ overlap $ii. p-p \ \sigma$ overlap $iii. s-p \ \sigma$ overlap
✓
Answer
$i. s-s \ \sigma$ overlap:
$a.$ The overlap between two half$-$filled s orbitals of two different atoms containing unpaired electrons with opposite spins is called $s-s$ overlap.
e.g. Formation of $H_2$ molecule by $s-s$ overlap:
Hydrogen atom $(Z = 1)$ has electronic configuration $: 1s^1.$ The $1s^1$ orbitals of two hydrogen atoms overlap along the internuclear axis to form a $\sigma$ bond between the atoms in $H_2$ molecule.
$b.$ Diagram:
$ii. p-p \ \sigma$ overlap:
$a.$ This type of overlap takes place when two $p$ orbitals from different atoms overlap along the internuclear axis.
e.g. Formation of $F_2$ molecule by $p-p$ overlap:
Fluorine atom $(Z = 9)$ has electronic configuration $1s^2 \ 2s^2 \ 2p2x \ 2p2y \ 2p1z.$
During the formation of $F_2$ molecule, half$-$filled $2p_z$ orbital of one $F$ atom overlaps with similar half$-$filled $2p_z$ orbital containing electron with opposite spin of another $F$ atom axially and a $p-p \ \sigma$ bond is formed.
$b.$ Diagram:
$iii. s-p \ \sigma$ overlap:
$a.$ In this type of overlap one half filled s orbital of one atom and one half filled
$p$ orbital of another orbital overlap along the internuclear axis.
e.g. Formation of $HF$ molecule by $s-p$ overlap:
Hydrogen atom $(Z=1)$ has electronic configuration $: 1 s^1$ and fluorine atom $(Z=9)$ has electronic configuration $1 s^2 \ 2 s^2 \ 2 p_x^2 \ 2 p_y^2 \ 2 p_z^1$.
During the formation of $HF$ molecule, half$-$filled $1 \mathrm{~s}$ orbital of hydrogen atom overlaps coaxially with half$-$filled $2 p_z$ orbital of fluorine atom with opposite electron spin and an $s-p \ \sigma$ bond is formed.
$b.$ Diagram:
$a.$ The overlap between two half$-$filled s orbitals of two different atoms containing unpaired electrons with opposite spins is called $s-s$ overlap.
e.g. Formation of $H_2$ molecule by $s-s$ overlap:
Hydrogen atom $(Z = 1)$ has electronic configuration $: 1s^1.$ The $1s^1$ orbitals of two hydrogen atoms overlap along the internuclear axis to form a $\sigma$ bond between the atoms in $H_2$ molecule.
$b.$ Diagram:
$ii. p-p \ \sigma$ overlap:
$a.$ This type of overlap takes place when two $p$ orbitals from different atoms overlap along the internuclear axis.
e.g. Formation of $F_2$ molecule by $p-p$ overlap:
Fluorine atom $(Z = 9)$ has electronic configuration $1s^2 \ 2s^2 \ 2p2x \ 2p2y \ 2p1z.$
During the formation of $F_2$ molecule, half$-$filled $2p_z$ orbital of one $F$ atom overlaps with similar half$-$filled $2p_z$ orbital containing electron with opposite spin of another $F$ atom axially and a $p-p \ \sigma$ bond is formed.
$b.$ Diagram:
$iii. s-p \ \sigma$ overlap:
$a.$ In this type of overlap one half filled s orbital of one atom and one half filled
$p$ orbital of another orbital overlap along the internuclear axis.
e.g. Formation of $HF$ molecule by $s-p$ overlap:
Hydrogen atom $(Z=1)$ has electronic configuration $: 1 s^1$ and fluorine atom $(Z=9)$ has electronic configuration $1 s^2 \ 2 s^2 \ 2 p_x^2 \ 2 p_y^2 \ 2 p_z^1$.
During the formation of $HF$ molecule, half$-$filled $1 \mathrm{~s}$ orbital of hydrogen atom overlaps coaxially with half$-$filled $2 p_z$ orbital of fluorine atom with opposite electron spin and an $s-p \ \sigma$ bond is formed.
$b.$ Diagram:
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