Atomic and ionic radius

Which one has the largest radius?

• Lithium (Li, atomic #3)
• Boron (B, atomic #5)
• Neon (Ne, atomic #10)
• Nitrogen (N, atomic #7)

What is meant by isolectronic?

• Group of atoms or ions that have the same electronic configuration

• Group of atoms or ions that have the same protonic configuration

• Group of atoms or ions that have the same electrical properties

• Group of atoms or ions that have the same electron charge

What is the example of species that are isolectronic?

• Na⁺ and Si⁴⁺

• Na⁺ and Cl^-

• Mg²⁺ and Al ⁺

• S^2- and O^2-

Arrange these species in increasing order of size.

Cl^- , Ca²⁺ , S^2- , Ar , K⁺

• Ca²⁺ > K⁺ > Ar > Cl^- > S^2-

• S^2- > Cl^- > Ar > K⁺ > Ca²⁺

• Ca²⁺ < K⁺ < Ar < Cl^- < S^2-

• S^2- < Cl^- < Ar < K⁺ < Ca²⁺

Ionization energy is...

• the energy required to add an electron to a specific atom
• how much energy it takes to remove an electron from an atom
• the energy required to shield the outer electrons from the nucleus
• a measure of the ability of an atom to attract electrons

Ionization energy __________ as you do across a period

• has no pattern

• stays the same

• decreases

• increases

Which has the highest ionization energy?

• Arsenic

• Iron

• ZInc

• Cobalt

Going down the group, the atomic radius of elements increases. Why is that so?

• the number of shell (n) increases

• Shielding effect increases

• Nucleus attraction towards valence electrons weaker

• All of the above

Which is larger... P or P^3- ? … and why?

• P^3- because it gains an energy level

• P^3- due to extra electron repulsion

• P because it loses an energy level

• P because of extra electron repulsion

Na⁺ and Al³⁺ are isoelectronic species (1s² 2s² 2p⁶). Which of these ion is smaller?

• Na⁺

• Al³⁺

• I'm not sure

• They have the same size