Chapter 9: Problem 17

How do covalent bonds differ from hydrogen bonds? Define base complementarity.

Short Answer

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Answer: Covalent bonds are strong chemical bonds formed by sharing electron pairs between atoms, whereas hydrogen bonds are weaker electrostatic interactions occurring between a hydrogen atom and a highly electronegative atom. Covalent bonds provide the basic structure of molecules, while hydrogen bonds contribute to the three-dimensional structures and functions of biomolecules. Base complementarity refers to the specific pairing of nucleotide bases in nucleic acids, such as DNA and RNA, through hydrogen bonding. This pairing ensures accurate replication of genetic information and allows the formation of double-stranded structures.

Step by step solution

Understand and define covalent bonds

Covalent bonds are a type of chemical bond formed when two atoms share a pair of electrons. This sharing of electrons allows both atoms to achieve a more stable electron configuration. Covalent bonds are strong and generally involve non-metal elements bonding with one another.

Understand and define hydrogen bonds

Hydrogen bonds are a type of weak electrostatic interaction that occurs between a hydrogen atom (H) and a highly electronegative atom, such as nitrogen (N), oxygen (O), or fluorine (F). The hydrogen atom is usually covalently bonded to one electronegative atom, while the other electronegative atom interacts with the hydrogen atom through the hydrogen bond. Hydrogen bonds are weaker than covalent bonds but play an essential role in the structures and functions of biomolecules, like DNA and proteins.

Compare covalent and hydrogen bonds

The major differences between covalent and hydrogen bonds are as follows: 1. Covalent bonds involve the sharing of electron pairs between atoms, while hydrogen bonds are electrostatic interactions between a hydrogen atom and a highly electronegative atom. 2. Covalent bonds are stronger and more stable than hydrogen bonds. 3. Covalent bonds involve non-metal elements, while hydrogen bonds specifically involve hydrogen and a highly electronegative element (usually N, O, or F). 4. Covalent bonds form the basic structure of molecules, while hydrogen bonds contribute to the three-dimensional structures and functions of biomolecules.

Define base complementarity

Base complementarity refers to the specific pairing of nucleotide bases in nucleic acids, such as DNA and RNA. In DNA, adenine (A) always pairs with thymine (T), and guanine (G) always pairs with cytosine (C) through hydrogen bonding. In RNA, adenine (A) pairs with uracil (U) instead of thymine. This base pairing ensures accurate replication of genetic information and allows the formation of double-stranded structures, such as the famous double helix of DNA. Base complementarity is crucial for various biological processes, including DNA replication, transcription, and translation.

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How do covalent bonds differ from hydrogen bonds? Define base complementarity.

Short Answer

Step by step solution

Understand and define covalent bonds

Understand and define hydrogen bonds

Compare covalent and hydrogen bonds

Define base complementarity

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