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Chapter 9: Q58P (page 375)

Using the periodic table only, arrange the elements in each set in order of increasing EN: (a) I, Br, N; (b) Ca, H, F

Short Answer

Expert verified

Electronegativity is defined as an atom's proclivity to attract the shared pair of electrons between the bonded atoms.

Step by step solution

01

Electronegativity between I, Br, N

N is in the second period, Br is in the fourth period, and 'I' is in the fifth period in the given elements. As a result, the atomic size increases from N to Iodine. As the atomic radius increases, so decreases electronegativity.

I<Br<N

02

Increasing order of Electronegativity between Ca, H, F

H is in the first period, F is in the second period, and Ca is in the third period in the given elements. As a result, the atomic size increases from N to Iodine. As the atomic radius increases, so decreases electronegativity.

Ca<F<H

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Most popular questions from this chapter

Even though so much energy is required to form a metal cation with a 2+ charge, the alkaline earth metals form halides with general formula

MX2, rather than MX.

(a) Use the following data to calculate the of MgCl:

Mg(s) Mg(g) = 148 kJ

Cl2(g) 2Cl(g) -243 kJ

Mg(g) (g) + e- =738 kJ

Cl(g) + (g) = -349 kJ

of MgCl = 783.5 kJ/mol.

(b) Is MgCl favoured energetically relative to Mg and ? Explain.

(c) Use Hess’s law to calculate ∆H° for the conversion of MgCl to and Mg ( of = -641.6 kJ/mol).

(d) Is MgCl favoured energetically relative to ? Explain.

Geologists have a rule of thumb: when molten rock cools and solidifies, crystals of compounds with the smallest lattice energies appear at the bottom of the mass. Suggest a reason for this.

Used condensed electron configuration to predict the relative hardness and melting points of Rubidium (Z=37), Vanadium (Z=23) and Cadmium (Z= 48).

Is the H-O bond in water nonpolar covalent, polar-covalent, or ionic? Define each term, and explain your choice.

The average C-H bond energy in CH4 is 415kJ/mol. Use table 9.2(p. 353) and the following to calculate the average C-H bond energy in ethane(C2H6;C-C bond), in ethene (C2H4;C=C bond), and ethyne (C2H2;C≡C):

C2H6(g)+H2(g)→2CH4(g)                           ΔHo=-65.07kJ/molC2H4(g)+2H2(g)→2CH4(g)                         ΔHo=-202kJ/molC2H2(g)+3H2(g)→2CH4(g)                         ΔHo=-376.74kJ/mol
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