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Understanding Different Types of Solids: Crystalline, Ionic, Amorphous, and Metals, Lecture notes of Chemistry

Manipal University Dubai (MUD)Chemistry

An overview of various types of solids, including crystalline solids (ionic, molecular, and atomic), amorphous solids, and metals. Topics covered include the structure of solids, properties of ionic compounds, metallic bonding, and alloys.

Typology: Lecture notes

2021/2022

Uploaded on 09/07/2022

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Types of Solids
Solids
Crystalline Solids- have a regular
repeating arrangement of their
particles.
Salts, Sugars, Metals
Amorphous Solids- have no regular
repeating arrangement of their
molecules
Common glass, several polymers.
Crystalline Structure
Amorphous
Amorphous solids
Amorphous solids, due to a lack of
arrangement of molecules, can
actually flow like a liquid, slowly.
You can also see this effect with silly
putty, and other polymers
Making solids…
Technically, anything can be made
amorphous.
A rapid cooling from liquid to solid
makes it amorphous. The particles
just don’t have time to arrange
themselves in a pattern.
A slower cooling or heat treatment
can make some amorphous solids
crystalline.
Safety Glass
Cars don’t use common glass for their
windshield because it breaks into
dangerous shard when it breaks.
Instead they use a heat strengthened
glass, one that is slowly cooled to a
solid to allow for a better
arrangement of molecules, so that
when it breaks it breaks into less
dangerous “dice”.
Glass Safety Glass
Back to crystalline solids
Crystalline solids can be made up of 3
different things
Ionic Solids –made of ions
Molecular Solids- made of molecules
held together by covalent bonds
Atomic Solids- Made of atoms
pf3

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Download Understanding Different Types of Solids: Crystalline, Ionic, Amorphous, and Metals and more Lecture notes Chemistry in PDF only on Docsity!

Types of Solids

Solids

 Crystalline Solids- have a regular repeating arrangement of their particles.  Salts, Sugars, Metals  Amorphous Solids- have no regular repeating arrangement of their molecules  Common glass, several polymers.

Crystalline Structure

Amorphous

Amorphous solids

 Amorphous solids, due to a lack of arrangement of molecules, can actually flow like a liquid, slowly.  You can also see this effect with silly putty, and other polymers

Making solids…

 Technically, anything can be made amorphous.  A rapid cooling from liquid to solid makes it amorphous. The particles just don’t have time to arrange themselves in a pattern.  A slower cooling or heat treatment can make some amorphous solids crystalline.

Safety Glass

 Cars don’t use common glass for their windshield because it breaks into dangerous shard when it breaks.  Instead they use a heat strengthened glass, one that is slowly cooled to a solid to allow for a better arrangement of molecules, so that when it breaks it breaks into less dangerous “dice”.

Glass Safety Glass

Back to crystalline solids

 Crystalline solids can be made up of 3 different things  Ionic Solids –made of ions  Molecular Solids- made of molecules held together by covalent bonds  Atomic Solids- Made of atoms

Ionic Compounds

 Ionic Compounds have very high melting points.  Sodium Chloride melts at 801oC  That is because every single negative particle is attracted to every single positive particle and vice versa.  This is in essence a very strong intermolecular force.

Ionic Solids

 Ionic solids are brittle. When they break their crystal structure shows, as they break into similar shapes.  NaCl breaks into CaCl 2 into cubes spheres.

Conduction of electricity

 Electricity is a flow of electrons  Anything that allows electrons to easily pass through will be a good conductor of electricity.  While solids, electrons can only jump from ion to ion.  This is a very slow process so solid ionic compounds are not good conductors.

Melts and solutions

 If you melt an ionic compound, then the ions can move. Electrons can now easily move through the substance.  If you dissolve an ionic compound, the ions are also free to move.  Therefore, liquid ionic compounds and ionic solutions are good conductors.

Molecular Compounds

 Molecular Compounds have much lower melting points.  Several are liquids (water) or gases (carbon dioxide) at room temperature.  Molecular compounds are not good conductors of electricity.

Atomic Solids/Elements

 Solid nonmetals and metalloids commonly form very large molecules.  A diamond (any size) could actually be viewed as one molecule of all carbon.  These solids are called network solids.  They have high melting points and don’t conduct electricity.

Allotopes of Carbon

Nonmetal Gases

 Noble gases and diatomic elements (except bromine, and iodine)  These all have only London dispersion forces.  These are very weak intermolecular forces.  They all have very low melting points, obviously since they are gases.  None are good conductors

Bromine and Iodine

 These act the same as the other diatomic elements but since the atoms are larger the London dispersion forces are greater.  That is why they are a liquid (bromine) or a solid (iodine) at room temperature.