1.Rank the following ions in order of decreasing radius: F,Cl,Br,I, and At. Use

Question

1.Rank the following ions in order of decreasing radius: F,Cl,Br,I, and At. Use the periodic table as necessary.Rank from largest to smallest radius. To rank items as equivalent, overlap them.

At-, F-, Br-, I-, Cl-

2.The following ions contain the same number of electrons. Rank them in order of decreasing ionic radii.

Rank from largest to smallest radius. To rank items as equivalent, overlap them.

Cl-, P3-, S2-, Ca2+, Sc3+, K+

3. Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Ei1.

Rank the elements from highest to lowest ionization energy. .

Na, F, Li, N, B, O

Explanation / Answer

1) All the ions belong to the same group VII A of the periodic table.

As we move down the group from top to bottom, one new shell is introduced and thus the atomic and ionic radii increase down the group.

thus order of decreasing a ionic radii is

At- > I- > Br- > Cl- >F-

2) Among the isoelectronci series (having same electrons, the higher the number of protons the smaller is the size of ion/species.

Thus the decreasing order of size is P-3(z= 15) > S-2(z=16) > Cl- (z=17) > K+(z=19) > Ca+2(z=20) > Sc+3(z=21)

3)Across a period , as we move from left to right the atomic radii decreases and from top to bottom in a group the atomic raddii increases. Thus the first ionizationeenergy increases along the period and decreases along a group.

However this trend is not followed in case of N and O as N has exactly half -filled configuration of 2s22p3 so its first higher ionisation energy is greater than O with 2s2 2p4 configuration.

Thus the order is

F > N > O > B . Li > Na

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