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Chapter 7: Problem 2

Describe two different causes of the force of attraction in a chemical bond.

Short Answer

Expert verified
The force of attraction in chemical bonds can be caused by differences in electronegativity, leading to polar covalent bonds, or by electron transfer, resulting in ionic bonds.

Step by step solution

01

Understanding the Role of Electronegativity

One primary cause of the force of attraction in a chemical bond is the difference in electronegativity between the two atoms involved. Electronegativity describes an atom's tendency to attract electrons towards itself. When two atoms with different electronegativities form a bond, the electrons are more attracted to the more electronegative atom, leading to polarization of charges and formation of a polar covalent bond, creating an attractive force between the atoms.
02

Considering the Concept of Ionicity

Another cause is the complete transfer of electrons between atoms, resulting in ionic bonding. This occurs when there is a significant difference in electronegativity between the two atoms. The more electronegative atom gains one or more electrons from the less electronegative atom, resulting in a positively charged ion and a negatively charged ion. The electrostatic attraction between the oppositely charged ions creates a strong force of attraction, which constitutes the ionic bond.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Electronegativity
Electronegativity is a measure of the tendency of an atom to attract a pair of electrons. It plays a crucial role in determining the type of bond formed between two atoms. The concept of electronegativity was first introduced by Linus Pauling and has become a fundamental aspect of chemical bonding. Here's what you need to remember about electronegativity:
  • Each atom has a specific electronegativity value, which helps predict how it will interact with other atoms.
  • The higher the electronegativity, the greater the atom's ability to attract electrons.
  • This property is influenced by the atomic number and the distance from the nucleus to the valence electrons.
Electronegativity differences between atoms determine how electrons are shared or transferred in a chemical bond. For a balanced understanding of bonding types, consider how these values lead to ionic or polar covalent bonds.
Ionic Bonding
Ionic bonding is an essential concept in chemistry, particularly in understanding how atoms combine to form compounds. This process involves the complete transfer of one or more electrons from one atom to another, resulting in the formation of ions. Let's break down how ionic bonding occurs:
  • If the electronegativity difference between two atoms is large, typically greater than 1.7 on the Pauling scale, ionic bonding is likely to occur.
  • The more electronegative atom gains one or more electrons, becoming a negatively charged ion.
  • The less electronegative atom loses electrons and becomes a positively charged ion.
The electrostatic attraction between these oppositely charged ions creates a strong and stable bond, known as an ionic bond. This type of bonding is commonly found in compounds like sodium chloride (table salt), where sodium donates an electron to chlorine.
Polar Covalent Bond
A polar covalent bond represents a point between pure covalent and ionic bonding. This type of bond forms when atoms with differing electronegativities share electrons, but not equally. Important points about polar covalent bonds include:
  • These bonds occur when the electronegativity difference is between 0.4 to 1.7.
  • The shared electrons are pulled closer to the more electronegative atom, resulting in slight positive and negative charges within the molecule.
  • This partial charge separation creates a dipole, which can affect the molecule's physical properties, such as boiling point and solubility.
Water is a classic example of a molecule with polar covalent bonds. In water (H鈧侽), the oxygen atom is more electronegative than the hydrogen atoms, causing an uneven distribution of electron charge. This results in a molecule with a slight positive charge near the hydrogens and a slight negative charge near the oxygen.

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Most popular questions from this chapter

What are transition elements? (Chapter 6\()\)

An external force easily deforms sodium metal, while sodium chloride shatters when the same amount of force is applied. Why do these two solids behave so differently?

Predict which solid in each pair will have the higher melting point. Explain your answers. $$ \begin{array}{l}{\text { a. } \mathrm{NaCl} \text { or } \mathrm{CsCl}} \\\ {\text { b. Ag or } \mathrm{Cu}} \\ {\text { c. } \mathrm{Na}_{2} \mathrm{O} \text { or } \mathrm{MgO}}\end{array} $$

Name the following compounds. \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\)

What does the term electrically neutral mean when discussing ionic compounds?
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