Rank the following elements in order of increasing electro negativity (EN): 2. F

Question

Rank the following elements in order of increasing electro negativity (EN): 2. For the two covalent bonds in each of the following pairs, which of the two has a higher polar character? 3. Which two of the following compounds are ionic? 4. How many valence electrons in each of the following atoms? a. Mg b. S c. Br d. P e. C f. Ne 5. Write the Lewis "dot structure' for the following atoms a. Na b. B (boron) c. C d. P e.. f. I (iodine) 6. Write the Lewis structure for the following compounds. Lewis structures must include all 7. Write Lewis structures for the following compounds or ions. Include all bonding and non-bonding electron pairs, and all formal charges as needed. Include resonance structures as needed

Explanation / Answer

1)

I) Of the given elements K and Ca belongs to S-block elements which are having there valence electrons in S shell and which they can easily ionize and get inert gas electronic configuration i.e. octet state. It means these S block elements expected to be more electropositive. In the other words k and Ca are less electronegative among given elements.

K has 1 and Ca have 2 valence shell electrons. It will be easy to ionize 1e than 2 so K expected to be more electropositive i.e. less electronegative than Ca.

Hence we have electronegativity order as K < Ca.

II) Now O, F, S, P elements belong to P block elements.

F have 7 valence shell electrons and hence very quickly it will accept 1e and complete its octet state and attain stability.

O have 6 in 2s shell , S have 6 in 3s shell and P have 5 in 3s 3p shell valence electrons and hence ease of acceptance of electron follows the order,

P < S < O < F

And hence electronegativity order for given elements is ,

(Lowest) K < Ca < P < S < O < F (Highest)

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2)

Polarity of the bond increases as electronegativity difference between bonded atoms increases.

a) Of C-H and C-O

Electronegativity difference between C and O will be more than C and H and hence C-O is more polar than C-H.

C-O has higher polar character.

b) P-Cl and S-Cl

P has less electronegativity than S hence the electronegativity difference between P and Cl will be higher than S and Cl case.

P-Cl has higher polar character.

c) O-F and C-F

C is much less electronegative than O.

Hence electronegativity difference between C and F will be higher than that of between O and F.

C-O bond has more polar character.

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3)

Interblock compound are generally ionic as there is large electronegativity difference

And

Intrablock compounds are polar covalent of non polar generally as electronegativity difference will be less.

Na2S and CaSe are interblock compounds where Na and Ca from S block and S and Se from P block.

Hence Na2S and CaSe are ionic compounds.

SCl2 and SO2 are intragroup compounds and electronegativity difference between bonded atoms is less.

H-F is highly polar but not ionic compound.

Answer : Na2S and CaSe are ionic compounds.

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4) Ground stete electronic configuration (G.S.E.C.) and valence electrons (V.E.)given.

Mg (At. No. 12) G.S.E.C. : [Ne] 3s2    so V.E. = 2

S (At. No 16) G.S.E.C. : [Ne] 3s2 3p4    so V.E. = 6

Br (At.No 35) G.S.E.C. : [Ar] 3s10 4s2 4p5    so V.E. = 7

P (At. No. 15) G.S.E.C. : [Ne] 3s2 3P3    so V.E. = 5

C (At. No 6) G.S.E.C. : 1s22s2 2p2  so V.E. = 4

Ne (at. No) G.S.E.C. : 1s2 2s2 2p6    so V.E. = 0 as octet complete.

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