Periodic Table Summary

What is the electronic configuration of element M (Z=15)?

• 1s² 2s² 2p⁶ 3s² 3p³

• 1s² 2s² 2p⁶ 3s² 3p⁵

• 1s² 2s² 2p⁶ 3s¹ 3p³

What is the electronic configuration of element Q (Z=17)?

• 1s² 2s² 2p⁶ 3s² 3p⁴

• 1s² 2s² 2p⁶ 3s² 3p⁵

• 1s² 2s² 2p⁶ 3s² 3p⁶

Locate element M (Z=15) in the Periodic Table.

• Period 2 Group 13

• Period 3 Group 18

• Period 3 Group 15

• Period 2 Group 15

Where element Q (Z=17) would be located in the Periodic Table?

• Period 2 Group 17

• Period 3 Group 17

• Period 3 Group 15

• Period 2 Group 15

Which block would element M and Q located in Periodic Table?

• s-block and p-block respectively

• both elements are in p-block

• both elements are in d-block

• both elements are in s-block

Between elements ₁₅M and ₁₇Q, which element has the larger atomic radius?

• Element M

• Element Q

Between elements ₁₅M and ₁₇Q, Choose a correct reason why element M is larger than Q.

• effective nuclear charge of M is higher than Q

• number of inner electrons of Q is bigger than M

• Element M has weaker attraction between nucleus and valence electron compared to element Q

Answer explanation

the number of proton Q is larger than M but the number of inner electrons remain constant. Z_eff in M is lower than Q

Element ₁₇Q has higher electronegativity than element ₁₅M because attraction between nucleus and valence electrons in Q is weaker than M.

• True

• False

Between elements ₁₇Q and ₁₅M, Which element would have higher first ionisation energy?

• Element Q

• Element M

Why does Element ₁₇Q has higher first ionisation energy than element ₁₅M?

• Element Q has larger atomic radius than element M

• Element Q has lower number of valence electrons than element M

• Element Q has weaker attraction between the nucleus and outer electrons

• Element Q has smaller atomic radius so more energy needed to remove the first valence electron