Chemistry: Bonding Types

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Questions and Answers

What occurs during the formation of an ionic bond?

Ions are formed but do not interact with each other.

The outer shells of atoms remain unchanged.

Electrons are shared between two metals.

Electrons are transferred from one atom to another. (correct)

What type of structure is formed by ionic compounds?

Giant ionic lattice (correct)

Molecular clusters

Covalent network

Amorphous solid

Which of the following ions has a negative charge?

SO42- (correct)

Cl- (correct)

Na+

NH4+

How are covalent bonds primarily formed?

By sharing electrons between two non-metals. Signup and view all the answers

What effect does a lone pair have on the bond angle between covalent bonds?

Reduces the bond angle by 2.5° Signup and view all the answers

What differentiates a dative bond from a standard covalent bond?

One atom supplies both electrons in a dative bond. Signup and view all the answers

Which compound is formed by sodium and chlorine?

Sodium chloride Signup and view all the answers

What is the bond angle for a linear molecule?

180° Signup and view all the answers

In a triangular pyramid shape, how many lone pairs are present?

1 Signup and view all the answers

What is the charge of an ammonium ion?

+1 Signup and view all the answers

How does electronegativity change across a period in the periodic table?

It increases Signup and view all the answers

In covalent bonding, how are multiple bonds represented?

With multiple straight lines indicating the number of shared pairs Signup and view all the answers

What type of bond forms when two atoms with different electronegativities bond together?

Polar bond Signup and view all the answers

What is the bond angle in a trigonal planar molecule?

120° Signup and view all the answers

What happens to the electronegativity of an atom as it moves down a group in the periodic table?

It decreases Signup and view all the answers

What is the bond angle in a tetrahedral molecule?

109.5° Signup and view all the answers

What property makes mercury unique among metals at room temperature?

It is the only liquid metal at room temperature. Signup and view all the answers

Why do simple molecular substances generally have low melting and boiling points?

They consist of weak van der Waals forces. Signup and view all the answers

What characteristic of diamond contributes to its hardness?

Its giant covalent lattice structure. Signup and view all the answers

How does the presence of lone pairs affect molecule shapes?

They create additional repulsive forces that alter bond angles. Signup and view all the answers

Why is water considered unusual among simple molecular substances?

It has a simple structure but high boiling point due to hydrogen bonding. Signup and view all the answers

What allows graphite to conduct electricity effectively?

The availability of free electrons between layers. Signup and view all the answers

What can change the bond angle in a molecule?

The repulsion between electron pairs around the central atom. Signup and view all the answers

What type of structure do macromolecular substances like diamond possess?

A macromolecular giant lattice structure. Signup and view all the answers

What is the main characteristic of metallic bonding?

A lattice of positively charged ions surrounded by delocalised electrons Signup and view all the answers

What effect does a greater charge on the positive ions have in metallic bonding?

It strengthens the attractive force in the lattice Signup and view all the answers

How do the physical properties of ionic substances compare to those of metallic substances?

Ionic substances are brittle, while metallic substances are malleable Signup and view all the answers

What happens to ionic substances when they are molten or in solution?

They conduct electricity as the ions are free to move Signup and view all the answers

Which statement is true about metallic substance conductivity?

They conduct electricity due to the movement of delocalised electrons Signup and view all the answers

Which characteristic of ionic substances contributes to their high melting and boiling points?

Strong electrostatic forces within the ionic lattice Signup and view all the answers

What type of crystal structures have different physical properties based on their bonding?

Ionic, metallic, simple molecular, and macromolecular structures Signup and view all the answers

What factor impacts the strength of metallic bonds in terms of ionic size?

Larger ions produce weaker attraction due to greater atomic radius Signup and view all the answers

What type of intermolecular force is the weakest?

Van der Waals Forces Signup and view all the answers

Which type of molecule experiences stronger van der Waals forces?

Linear molecules Signup and view all the answers

What is necessary for hydrogen bonding to occur?

Lone pairs on electronegative atoms Signup and view all the answers

What effect does hydrogen bonding have on the physical properties of substances?

Increases melting and boiling points Signup and view all the answers

Which regions in a polar molecule attract each other through a permanent dipole?

Negative and positive regions Signup and view all the answers

How does molecular weight (Mr) affect van der Waals forces?

Strengthens the forces with higher Mr Signup and view all the answers

Which of the following molecules is most likely to exhibit hydrogen bonding?

Water (H2O) Signup and view all the answers

How can a molecule with an induced dipole generate attractions?

By influencing other charged particles Signup and view all the answers

Study Notes

Ionic Bonding

Occurs between a metal and a non-metal
Electrons are transferred from the metal to the non-metal
Creates charged particles called ions
Oppositely charged ions attract through electrostatic forces to form a giant ionic lattice
Common compound ions include sulfate, hydroxide, nitrate, carbonate and ammonium

Covalent and Dative Bonding

Covalent bonds form between two non-metals
Electrons are shared between the two outer shells
Multiple electron pairs can be shared, which produces multiple covalent bonds
Dative bonds form when both electrons in the shared pair are supplied from a single atom
Once a dative bond has formed, it is a standard covalent bond and reacts the same way

Metallic Bonding

Metallic bonding consists of a lattice of positively charged ions surrounded by a sea of delocalised electrons
This produces a very strong electrostatic force of attraction between these oppositely charged particles
The greater the charge on the positive ion, the stronger the attraction (more electrons are released)
Larger ions produce a weaker attraction due to their greater atomic radius

Bonding and Physical Properties

Physical properties include boiling point, melting point, solubility and conductivity
They are different depending on the type of bonding and crystal structure
Crystal structures include ionic, metallic, simple molecular and macromolecular

Crystal Structures

Ionic

Ionic substances have high melting and boiling points
This is because the electrostatic forces holding the ionic lattice together are strong and require a lot of energy to overcome
When molten or in solution, ionic substances can conduct electricity because the ions separate and are no longer held in a lattice
Ionic substances are often brittle materials

Metallic

Substances with metallic structure are often good conductors
Metals are also malleable as the layers of positive ions are able to slide over one another
The delocalised electrons prevent fragmentation as they can move around the lattice
Metallic substances have high melting points and are nearly always solid at room temperature

Simple Molecular

Simple molecular structures consist of covalently bonded molecules held together with weak van der waals forces
These are a type of intermolecular force that acts between molecules
Simple molecular substances have low melting and boiling points
Simple molecular substances are very poor conductors as their structure contains no charged particles

Macromolecular

Macromolecular structures are covalently bonded into a giant lattice structure
Each atom has multiple covalent bonds, which are very strong, giving the substance a very high melting point
The strength of the covalent lattice makes macromolecular substances rigid

Shapes of Molecules

The shape of a molecule is determined by the number of electron pairs around the central atom
Each electron pair naturally repels each other so that the largest bond angle possible exists between the covalent bonds
Any lone pairs present around the central atom provide additional repulsive forces, which changes the bond angle
Lone pairs around the central atom reduce the bond angle by 2.5 degrees

Bond Polarity

The negative charge around a covalent bond is not evenly spread around the orbitals of the bonded atoms
Every atom has electronegativity, which is its power to attract negative charge towards itself within a covalent bond
Electronegativity increases along a period and decreases down a group
If the two atoms that are bonded have different electronegativities, a polar bond forms
The more electronegative atom draws more of the negative charge towards itself, producing a ∂- region and a ∂+ region

Intermolecular Forces

There are three main types of intermolecular forces
Each one differs in strength and what it acts between

Van Der Waals Forces

This is the weakest type of intermolecular force
It acts as an induced dipole between molecules
The strength of van der waals forces varies depending on the Mr of the molecule and its shape
The larger the Mr of a molecule, the stronger the intermolecular forces

Permanent Dipole

This type of intermolecular force acts between molecules with a polar bond
The ∂+ and ∂- regions attract each other and hold the molecules together in a lattice like structure
This force is stronger than Van der Waals forces

Hydrogen Bonding

Hydrogen bonds only form between hydrogen and the three most electronegative atoms: nitrogen, oxygen and fluorine
The lone pair on these atoms forms a bond with a hydrogen atom from another molecule
It is the strongest type of intermolecular force
Molecules held together with hydrogen bonds have much higher melting and boiling points compared to similar molecules without hydrogen bonding

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Description

Explore the different types of chemical bonding, including ionic, covalent, and metallic bonding. Understand how electrons are transferred or shared between atoms, and how this leads to the formation of various compounds. This quiz will test your knowledge of key concepts and ion characteristics.