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Chapter 6: Problem 15

What force holds two atoms together in a covalent bond?

Short Answer

Expert verified
The electromagnetic force holds two atoms together in a covalent bond.

Step by step solution

01

Understanding Covalent Bonds

Covalent bonds are a type of chemical bond where atoms share pairs of electrons to achieve a more stable electron configuration. This form of bonding typically occurs between non-metal atoms.
02

Electron Sharing

In a covalent bond, two atoms share one or more pairs of electrons. This sharing allows each atom to attain the electron configuration of a noble gas, which is characterized by a complete outer shell of electrons, providing stability.
03

Role of Electromagnetic Force

The force that holds the two atoms together in a covalent bond is primarily the electromagnetic force. The positively charged nuclei of the atoms are attracted to the shared pair of negatively charged electrons, creating an attractive force that holds the atoms together.

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Key Concepts

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

Understanding Chemical Bonding
Chemical bonding is the process through which atoms combine to form molecules. One common type of chemical bonding is the covalent bond. This occurs when atoms share electrons to achieve stability.

In a covalent bond, non-metal atoms come together and share one or more pairs of electrons. This sharing allows each participating atom to achieve a stable electron arrangement, similar to those found in noble gases.
  • Non-metal atoms often form covalent bonds.
  • Covalent bonds involve electron sharing.
  • This bonding achieves a more stable electron configuration.
Exploring Electron Sharing
Electron sharing is a fundamental concept in covalent bonding. When two atoms approach each other, they may share pairs of electrons to fill their outer shells. This process results in each atom achieving a full valence shell, akin to the electron configuration of noble gases.

The sharing of electrons leads to the formation of a molecule. The number of shared electron pairs can vary, resulting in different types of covalent bonds: single, double, or triple bonds.
  • Single bond: one pair of shared electrons.
  • Double bond: two pairs of shared electrons.
  • Triple bond: three pairs of shared electrons.
These bonds provide the stability needed for the atoms to remain bonded together.
The Role of Electromagnetic Force
In a covalent bond, the electromagnetic force is the key to keeping the atoms together. This force arises due to the attraction between the positively charged nuclei of the atoms and the negatively charged shared electrons.

When atoms share electrons, their nuclei exert an attractive force on these shared electrons. This electromagnetic attraction is what holds the atoms in a strong, stable bond.
  • The positive charge of the nucleus attracts electrons.
  • Electrons are arranged in shared pairs.
  • The electromagnetic force maintains atomic connections.
This force ensures the structural stability and integrity of the molecule, defining the essence of covalent bonding.

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Most popular questions from this chapter

Classify the following bonds as ionic, covalent, or neither \((\mathrm{O}\), atomic number \(8 ; \mathrm{F}\), atomic number 9 ; \(\mathrm{Na}\), atomic number 11; Cl, atomic number 17; \(\mathrm{Ca}\), atomic number 20; U, atomic number 92): \(\mathrm{O}\) with \(\mathrm{F}\). Ca with \(\mathrm{Cl}\) Na with \(\mathrm{Na}\) U with Cl.

Atoms of nonmetallic elements form covalent bonds, but they can also form ionic bonds. How is this possible?

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Which are closer together: the two nuclei within potassium fluoride, KF, or the two nuclei within molecular fluorine, \(\mathrm{F}_{2}\) ?

What is a dipole?
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