Chemistry: Bonding Concepts

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Questions and Answers

What is the effect of increasing electronegativity across a period on bonding?

It results in a non-polar bond.

It decreases the strength of the bond.

It causes electrons to equally share between atoms.

It increases the attraction of bonding electrons to the nucleus. (correct)

Which atom is the most electronegative?

Chlorine

Nitrogen

Fluorine (correct)

Oxygen

What occurs in a polar covalent bond?

One atom develops a δ+ charge and the other a δ- charge. (correct)

The bond becomes ionic in nature.

Electrons are equally shared between the two atoms.

There is no difference in electronegativity between the atoms.

Why does electronegativity decrease down a group?

Distance between bonding electrons and the nucleus increases. Signup and view all the answers

How does the polarity of water relate to its molecular structure?

Oxygen is more electronegative than hydrogen, leading to a polar structure. Signup and view all the answers

What characterizes a polar bond?

Unequal sharing of electrons due to differing electronegativities. Signup and view all the answers

What creates bond polarity in covalent bonds?

The difference in electronegativities of the bonded atoms Signup and view all the answers

What is a covalent bond primarily characterized by?

The sharing of electron pairs between two non-metal atoms Signup and view all the answers

What describes the relationship between ionic and covalent bonding?

They fall on a continuum of bonding types. Signup and view all the answers

Which statement accurately describes a coordinate bond?

Both electrons in the shared pair are supplied by one atom Signup and view all the answers

What happens to the electrons in a covalent bond between atoms of different electronegativities?

They are attracted more strongly to the atom with higher electronegativity. Signup and view all the answers

What type of bond is formed between a metal and a non-metal?

Ionic bond Signup and view all the answers

Which of the following pairs exemplifies a covalent bond?

I2 Signup and view all the answers

Which of the following statements about metallic bonding is true?

It is the attraction between positive ions and delocalized electrons Signup and view all the answers

In the context of bonding, what does a lone pair refer to?

A pair of electrons that are not shared with any atom Signup and view all the answers

Which type of bond does NOT typically result in a noble gas structure?

Metallic bonds Signup and view all the answers

What type of bond is characterized by the sharing of electrons between two non-metal atoms?

Covalent bond Signup and view all the answers

Which molecule is an example of a substance that violates the octet rule?

SF6 Signup and view all the answers

What results when atoms with significantly different electronegativities bond together?

Ionic bonding Signup and view all the answers

Which of the following correctly defines electronegativity?

The ability of an atom to attract electrons in a chemical bond Signup and view all the answers

In the context of ionic bonding, what occurs to the electrons of the metal atom?

They are transferred to the non-metal atom Signup and view all the answers

Study Notes

Bonding

Ionic bonding is the electrostatic attraction between oppositely charged ions formed by electron transfer.
Covalent bonding is the electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
A lone pair is an unshared pair of electrons in the outer shell of an atom.
A coordinate bond (dative bond) is a shared pair of electrons with both electrons supplied by one atom.
The octet rule states that atoms tend to gain, lose, or share electrons to achieve eight electrons in their outer shell, but there are exceptions.
Electronegativity is the extent to which an atom attracts the bonding electrons in a covalent bond. Electronegativity increases across periods and decreases down groups.
A polar bond is a covalent bond with unequal sharing of bonding electrons, indicated by partial charges (δ+ and δ−). Bond polarity arises from differences in electronegativity.
Metallic bonding is the attraction between positive ions and delocalized electrons in a lattice.
Delocalized electrons are outer, mobile electrons that don't stay fixed to one atom but move freely throughout the metal.

Types of Bonding

Ionic bonds occur between a metal and a non-metal.
Covalent bonds occur between two non-metals.
Metallic bonds occur between metal atoms.

Dot and Cross Diagrams

Dot and cross diagrams illustrate the sharing or transfer of electrons in chemical bonds. They illustrate the outer electrons only.

Revision Questions

There are revision questions included in the text, covering various aspects of bonding. These are not summarized here.

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Description

This quiz covers key concepts of bonding in chemistry, including ionic, covalent, and metallic bonds. It also explores electronegativity, the octet rule, and the characteristics of polar bonds. Test your understanding of these essential topics in chemical bonding.