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Chapter 14: Q14.95P (page 623)

Question: Assuming acid strength relates directly to the electronegativity of the central atom, rank H3PO4,HNO3 , and H3ASO4 in order of increasing acid strength.

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01

Definition of Electronegativity

Electronegativity of an atom is defined as the tendency of an atom to attack the electrons.

In the periodic table as we move from right to left in a period electronegativity goes on increasing. While in a group as we move downward electronegativity is decreases. This is the general trend found in the periodic table. The relation of acidic character with electronegativity is as follows;

Electronegativity 伪acidic character

02

Acidic strength of given acid

The relation of acidic character with electronegativity is as follows;

Electronegativity鈭� acidic character

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Most popular questions from this chapter

One similarity between B and Si is the explosive combustion of their hydrides in air. Write balanced equations for the combustion ofB2H6 androle="math" localid="1653907272447" Si4H10 .

(a) What is the range of oxidation states shown by the elements of Group 5A (15) as you move down the group?

(b) How does this range illustrate the general rule for the range of oxidation states in groups on the right side of the periodic table?

Draw Lewis structures for the following compounds and predict which member of each pair will form hydrogen bonds:

(a) NH3 or AsH3

(b) CH4 or H2O

An important starting material for the manufacture of polyphosphazene is the cyclic molecule (NPCl2)3. The molecule has a symmetrical six-membered ring of alternating N and P atoms, with the Cl atoms bonded to the P atoms. The nitrogen phosphorus bond length is significantly less than that expected for an NP single bond.

(a) Draw a likely Lewis structure for the molecule.

(b) How many lone pairs of electrons do the ring atoms have?

(c) What is the order of the nitrogen-phosphorus bond?

In addition to those in Table 14.3, other less stable nitrogen oxides exist. Draw a Lewis structure for each of the following:

(a) N2O2, a dimer of nitrogen monoxide with an N-Nbond.

(b) N2O2, a dimer of nitrogen monoxide with no N-Nbond.

(c) N2O3with no N-Nbond.

(d) NO+ and NO3鈭� , products of the ionization of liquid N2O4.

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