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Chapter 2: Problem 4

Which of the following statements about covalent bonds is not true? a. A covalent bond is stronger than a hydrogen bond. b. A covalent bond can form between atoms of the same element. c. Only a single covalent bond can form between two atoms. d. A covalent bond results from the sharing of electrons by two atoms. e. A covalent bond can form between atoms of different elements.

Short Answer

Expert verified
Statement c is not true.

Step by step solution

01

Understanding Covalent Bonds

Covalent bonds are chemical bonds formed by the sharing of electron pairs between atoms. These bonds are strong and can occur between atoms of the same or different elements.
02

Analyzing Statement a

Statement a claims that a covalent bond is stronger than a hydrogen bond. This is generally true, as covalent bonds involve the sharing of electrons whereas hydrogen bonds are weaker and arise due to dipole interactions.
03

Analyzing Statement b

Statement b proposes that a covalent bond can form between atoms of the same element. This is true; an example is the bond between two hydrogen atoms in a hydrogen molecule (H鈧�).
04

Analyzing Statement c

Statement c suggests that only a single covalent bond can form between two atoms. This is not true, as atoms can form single, double, or even triple covalent bonds, like in oxygen (O鈧�) forming a double bond.
05

Analyzing Statement d

Statement d indicates that a covalent bond results from the sharing of electrons between two atoms. This accurately describes the nature of covalent bonds and is true.
06

Analyzing Statement e

Statement e claims that a covalent bond can form between atoms of different elements. This is true, as seen in the formation of water (H鈧侽), where hydrogen and oxygen form covalent bonds.
07

Conclusion: Identify the False Statement

Analyzing all statements, the false statement is c, which incorrectly asserts that only a single covalent bond can form between two atoms.

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Key Concepts

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

Chemical Bonding
Chemical bonding is a fundamental concept in chemistry that explains how atoms come together to form molecules. There are several types of chemical bonds, but the most common ones are covalent, ionic, and metallic bonds. Covalent bonds are characterized by the sharing of electron pairs between atoms, providing a stable balance of attractive and repulsive forces.
  • Covalent Bonds: These involve the sharing of electrons between two atoms, allowing each to achieve a full outer electron shell, which is often more stable. Covalent bonds are strong and are the most common type of bond in organic chemistry.
  • Ionic Bonds: These occur when one atom donates an electron to another, creating positive and negative ions that attract each other.
  • Metallic Bonds: These involve the pooling of electrons shared among a group of metal atoms, allowing electrons to move freely between them, giving rise to properties like conductivity and malleability.
Understanding these bonding types is crucial for predicting the behavior, reactivity, and properties of different molecules and compounds. Covalent bonds can form between atoms of the same or different elements, as we often see in both small molecules, like water, and large complex structures like proteins.
Electron Sharing
Electron sharing is the process at the heart of covalent bonding. When two atoms share electrons, they both gain greater stability by filling their valence electron shells. Covalent compounds form because the energy state of shared electrons is lower than that of separate atoms. This sharing creates a strong bond, tying the atoms together effectively.
  • Single Bonds: Involve one pair of shared electrons. For example, hydrogen gas (H鈧�) forms with a single covalent bond between two hydrogen atoms.
  • Double Bonds: Involve two pairs of shared electrons. An example is the oxygen molecule (O鈧�), which has a double bond.
  • Triple Bonds: Involve three pairs of shared electrons, like the bond in nitrogen gas (N鈧�).
The number of shared electron pairs affects the strength and length of the bond. Generally, more shared pairs mean stronger, shorter bonds. Understanding how atoms share electrons helps in comprehending the molecular structure and properties, such as reactivity and boiling points of substances.
Molecular Structure
Molecular structure refers to the arrangement of atoms within a molecule. The way atoms bond and the specific arrangement in space determine the properties and functions of the molecule. Covalent bonds bring atoms together to form molecules with specific geometries. These geometries result from the spatial distribution of atom pairs and the repulsion between electrons.
  • Linear: Molecules like carbon dioxide (CO鈧�) have a linear structure, where atoms are arranged in a straight line.
  • Trigonal Planar: In molecules like boron trifluoride (BF鈧�), the atoms form a flat triangular shape.
  • Tetrahedral: Methane (CH鈧�) is an example where the central carbon atom forms a tetrahedral shape with hydrogen atoms.
The molecular structure is crucial because it influences molecular properties, including polarity, state of matter, and reactivity. Understanding molecular structures helps explain the diversity of materials and their chemical behaviors in various environments.

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Most popular questions from this chapter

Would you expect the elemental composition of Earth's crust to be the same as that of the human body?

Which of the following statements about the isotopes of an element is not true? a. They all have the same atomic number. b. They all have the same number of protons. c. They all have the same number of neutrons. d. They all have the same number of electrons. e. They all have identical chemical properties.

Which of the following statements about water is not true? a. It releases a large amount of heat when changing from liquid into vapor. b. Its solid form is less dense than its liquid form. c. It is the most effective solvent for polar molecules. d. It is typically the most abundant substance in a living organism. e. It takes part in some important chemical reactions.

The mass number of an element a. equals the number of neutrons in an atom. b. equals the number of protons in an atom. c. equals the number of electrons in an atom. d. equals the number of neutrons plus the number of protons. e. depends on the relative abundances of its electrons and neutrons.

The atomic number of an element a. equals the number of neutrons in an atom. b. equals the number of protons in an atom. c. equals the number of protons minus the number of neutrons. d. equals the number of neutrons plus the number of protons. e. depends on the isotope.
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