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Chapter 7: Q16E (page 391)

From its position in the periodic table, determine which atom in each pair is more electronegative: (a)\({\rm{N or P}}\)(b)\({\rm{N or Ge}}\)(c)\({\rm{S or F}}\)(d)\({\rm{Cl or S}}\)(e)\({\rm{H or C}}\)(f)\({\rm{Se or P}}\)(g)\({\rm{C or Si}}\).

Short Answer

Expert verified
  1. Nitrogen is more electronegative.
  2. Nitrogen is more electronegative.
  3. Fluorine is more electronegative.
  4. Chlorine is more electronegative.
  5. Carbon is more electronegative.
  6. Phosphorus is more electronegative.
  7. Carbon is more electronegative.

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Explanation

As, the addition of a proton has a greater effect than the addition of an electron, the size of the atom decreases as you travel from left to right in the periodic table. Because of the strong force of the nucleus, it will be able to receive electrons more easily as its size decreases.

According to the foregoing argument, electronegativity rises as one moves from left to right in the periodic table.

As you progress from top to bottom in a group, the size of the group grows due to the addition of fresh energy shells. Because the force of attraction of the nucleus is no longer able to attract additional electrons as the size of the nucleus rises, electronegativity will drop as the group size decreases.

03

Determining which atom in each pair is more electronegative?

a. Due to nitrogen is heavier than phosphorus, it is more electronegative.

Therefore, nitrogen is more electronegative.

04

Determining which atom in each pair is more electronegative?

b. Nitrogen is more electronegative than Germanium since it is located to the right of it.

Therefore, nitrogen is more electronegative.

05

Determining which atom in each pair is more electronegative?

c. As, Fluorine is heavier than Sulfur, it is more electronegative.

Therefore, Fluorine is more electronegative.

06

Determining which atom in each pair is more electronegative?

d. The Chlorine is in front of Sulfur, it is more electronegative.

Therefore, Chlorine is more electronegative.

07

Determining which atom in each pair is more electronegative?

e. As, Carbon is located above and to the right of Hydrogen, it is more electronegative.

08

Determining which atom in each pair is more electronegative?

f. Due to phosphorus is located to the right and above \({\rm{Se}}\), \({\rm{P}}\) is more electronegative.

Therefore, phosphorus is more electronegative.

09

Determining which atom in each pair is more electronegative?

g. As, the value of carbon is to the right and above sillicon, it is more electronegative.

Therefore, carbon is more electronegative.

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Most popular questions from this chapter

Predict the electron pair geometry and the molecular structure of each of the following:

  1. \({\rm{IO}}{{\rm{F}}_{\rm{5}}}\)(I is the central atom)
  2. \({\rm{POC}}{{\rm{l}}_{\rm{3}}}\)(P is the central atom)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SeO}}\)(Se is the central atom)
  4. \({\rm{ClS}}{{\rm{O}}^{\rm{ + }}}\)(S is the central atom)
  5. \({{\rm{F}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  6. \({\rm{N}}{{\rm{O}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{SiO}}_{\rm{4}}^{{\rm{4 - }}}\)

Question: Use principles of atomic structure to answer each of the following:

(a) The radius of the \({\rm{Ca}}\) atom is \({\rm{197 pm}}\); the radius of the \({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}\) ion is \({\rm{99 pm}}\). Account for the difference.

(b) The lattice energy of \({\rm{CaO(s)}}\) is \({\rm{ - 3460 kJ/mol}}\); the lattice energy of \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) is \({\rm{ - 2240 kJ/mol}}\). Account for the difference.

(c) Given these ionization values, explain the difference between \({\rm{Ca}}\) and \({\rm{K}}\) with regard to their first and second ionization energies.

(d) The first ionization energy of \({\rm{Mg}}\) is \({\rm{738 kJ/mol}}\) and that of \({\rm{Al}}\) is \({\rm{578 kJ/mol}}\). Account for this difference.

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Two arrangements of atoms are possible for a compound with a molar mass of about\({\rm{45 g/mol}}\)that contains\({\rm{52}}{\rm{.2 \% C, 13}}{\rm{.1 \% H}}\), and\({\rm{34}}{\rm{.7 \% O}}\)by mass. Write the Lewis structures for the two molecules.

The arrangement of atoms in several biologically important molecules is given here. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms.
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