Explanation
Electronegativity is the property of attracting electrons by an atom in a molecule. Electron affinity is the amount of energy librated when an electron is added to an isolated gaseous atom.
Al and Ga have approximately equal ionisation potential. Ionisation energy increases with decrease in atomic size and decrease in shielding effect.
BeO is most acidic in nature as acidity of oxides decreases wit increases in electropositive character of central atom.
Order of first ionoisation potential
K<Na<Be
First ionisation potential decreases down a group and increases from left to right in a period.
Ionisation energy increases with an increase in penetration power and thus the order of screening effect is
S>p>d>f.
Chlorine has highest electron affinity among F, u, S and O
Low value of electron affinity of fluorine than chlorine is due to small size of F atom.
The tendency of an atom in a compound to attract a pair of bonded electron toward itself is known as electronegativity of an atom. Flourine is most electronegativity element.
Order of electron affinity is
F<U>Br>I
Electron affinity decreases down the group. Chlorine has higher electron affinity than fluorine because of small size of fluorine.
Order of ionization enthalapy
B<S<P<F
Ionisation enthalapy decreases down the group and increases along a period.
Sulphur has six valence electrons as it belongs to VI group of periodic table. Hence it has maximum valency.
Fluorine never shows positive oxidation state, it is most electronegative element.
Lithium is not amphoteric in nature. It is basic in nature.
Ionization energy of N is greater than that of 0 due to its more stable configuration. Nitrogen has half filled orbital.
Ionisation energy of Sn is less than that of Pb because due to presence of 4f electrons which screen the nucleus more effectively than 6p electrons causing the effective nuclear charge to be very high. Hence Sn has the lowest value of IE1 among all the given elements.
The elements with atomic number 9, 17, 35, 53 and 85 are respectively F, Cl, Br, I and At. These are VII A group elements which is also known as halogens.
Be has maximum ionization potential. Ionisation potential increases in a period on moving left to right in a period and decreases down a group.
The energy required by an atom to lose their valence electron is called ionization potential. The noble gases have fully filled orbitals. So, large amount of energy required to remove a valence electron their ionization potential is very high.
In the periodic table atomic radii decreases from left to right hence fluorine has a very less atomic radii. Noble gases are the monoatomic gases, hence their covalent atomic radii cannot be found out. Their calculated atomic radii is vander waal’s radii which is almost double to covalent radii, hence the vander waal’s radius of neon is about 1.60 Å
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