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Chapter 4: Problem 1

How many types of chemical bonds are there? What are they?

Short Answer

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Answer: The three primary types of chemical bonds are covalent, ionic, and metallic bonds. Covalent bonds are formed by sharing electrons between two or more atoms with similar electronegativity. Ionic bonds occur when one atom donates electrons to another, creating oppositely charged ions that are attracted to each other. Metallic bonds are formed between metal atoms, where they share a "sea" of electrons that can move freely throughout the metal structure.

Step by step solution

01

Identify the total number of chemical bond types

There are three primary types of chemical bonds that can occur between atoms.
02

Describe the three types of chemical bonds

1. Covalent Bond: A covalent bond is formed by sharing electrons between two or more atoms. In this type of bond, the involved atoms have similar electronegativity, meaning they have a similar pull on the shared electrons. A typical example of a covalent bond is the bond between two hydrogen atoms (H-H) to form a hydrogen molecule (H2). 2. Ionic Bond: An ionic bond occurs when one atom donates one or more electrons to another atom. This creates two ions with opposite charges, which are then attracted to each other. The bond between these oppositely charged ions is called an ionic bond. Ionic bonds usually occur between atoms with a significant difference in electronegativity (e.g., a metal and a non-metal). A common example is the bond between a sodium atom (Na) and a chlorine atom (Cl) to form sodium chloride (NaCl), more commonly known as table salt. 3. Metallic Bond: Metallic bonds are formed between atoms of metals. In this type of bonding, atoms share a "sea" of electrons鈥攖he valence electrons are free to move throughout the entire metal structure instead of being attached to a specific atom. Because of this electron-sharing, metals can conduct electricity and heat well, and they also tend to have high melting and boiling points. Examples include the bonding in copper (Cu), iron (Fe), and many other metals.

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Key Concepts

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

Covalent Bond
When we talk about a covalent bond, we're looking at the partnership between atoms that come together to share electrons. This helps both parties achieve a complete outer shell of electrons, akin to that of noble gases which are known for their stability. To make it even simpler, think of a covalent bond as two friends sharing a pizza evenly so both are satisfied.

The shared electrons are what keep the atoms bonded together. A single bond is formed when one pair of electrons is shared, but you can also find double and triple bonds where two or three pairs of electrons are shared respectively. A prime example of a covalent bond is the molecule of water (H2O), where each hydrogen atom shares an electron with oxygen, forming a bond that gives water its unique properties.
Ionic Bond
Imagine a playground seesaw. An ionic bond is a bit like a seesaw balanced by kids of different sizes 鈥� one child represents a metal atom that has a few extra electrons that it doesn't need while the other, a non-metal atom, just needs a few more to feel complete. To achieve balance, the metal atom donates its extra electrons to the non-metal. This generosity results in the formation of charged ions: a positively charged metal ion and a negatively charged non-metal ion, which are drawn to each other by their opposite charges.

Take table salt (sodium chloride or NaCl) for example. It's formed when sodium, a metal, passes an electron over to chlorine, a non-metal, resulting in a strong attraction between the positively charged sodium ions (Na+) and the negatively charged chloride ions (Cl鈭�), which holds the compound together.
Metallic Bond
A metallic bond is the type of bond we see in metals, and it's what gives them many of their special characteristics 鈥� think of it as a communal potluck where each atom contributes some of its electrons to create a shared pool. In this bond, the valence electrons from the metal atoms are delocalized; they don't belong to any one atom but move freely throughout the entire structure of the metal.

This sharing of mobile electrons across a lattice of metal cations gives rise to properties like electrical conductivity, malleability, and luster. As an example, copper wires conduct electricity because the electrons can move freely within the metallic bond, transporting electric charge from one end of the wire to the other with ease.

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Most popular questions from this chapter

What type of bond formation takes place between (a) a metal and a non-metal and (b) two non-metals?

Draw the Lewis dot formulae for the bond formations in the following compounds. (a) \(\mathrm{NaCl}\) (b) \(\mathrm{CaF}_{2}\) (c) \(\mathrm{H}_{2}\) (d) \(\mathrm{O}_{2}\) (c) \(\mathrm{N}_{2}\) (f) \(\mathrm{H}_{2} \mathrm{O}\) (g) \(\mathrm{NH}_{3}\) (i) \(\mathrm{CH}_{4}\)

Name one solvent in which most of the ionic compounds dissolve.

In a covalent bond, of electrons takes place between the two atoms.

In what type of solvents do the (a) polar compounds and (b) non-polar compounds dissolve?
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