Edited Invalid date
13.5 The Structures of Ionic Solids -- Part 1
Solids and Modern Materials have the larger fluoride anions occupying all eight of the tetrahedral holes located directly beneath each corner atom.
The cation-to-anion ratio of 1:2 is the same as in the formula of the compound.
PbF2, SrF2, and BaCl2 are included.
There are different colored spheres in this figure.
Network covalent atomic solid are composed of atoms held together by bonds.
Network covalent atomic solid have some of the highest melting points of all substances because of the broken bonds.
In this section, we look at two different families of network atomic solids: carbon and silicates.
In Section 13.1, we talked about the different forms of carbon, including Graphene.
The separation between sheets is 341 pm and there are no bonds between them.
The sheets slide past each other with relative ease, which explains the slippery feel of the material.
There are sheets of carbon atoms arranged in a grid.
The atoms are used for heating elements in the furnace.
The density of the material is 2.2 g. dispersion forces hold the sheets together.
In diamond, pressure rearranges the carbon atoms in graphite to form each carbon atom, forming four covalent bonds to four other carbon atoms.
Carbon is exposed to high pressures deep underground.
The majority of diamond is found in Africa and South Africa.
The first synthetic diamonds were produced using pressures of 50,000 atm and a temperature of 1600 degrees.
There are four carbon atoms at the corners of a tetrahedron.
A diamond crystal can be thought of as a giant molecule, held together by these bonds, because the structure extends throughout the crystal.
Diamond has a very high melting point because of its strong bonds.
The electrons in diamond are not free to move.
Diamonds do not conduct electricity.
Diamond is an excellent conductor of heat.
The largest use of diamonds is for abrasives and cutting tools.
Small diamonds are used at the cutting edge of tools to make the edges harder and give them a longer life.
Natural diamonds are considered gems for their brilliance and relative inertness.
The diamond is denser than the graphite.
It is denser than diamond.
The relative densities of the two substances can't be determined without more information.
A new form of carbon was discovered when researchers aimed a pow erful laser at the surface.
The carbon rings are wrapped into a 20-sided icosahedral structure.
Carbon clusters similar to C60 containing from 36 to over 100 carbon atoms have been identified by researchers.
The individual clusters are held to one another by dispersion forces.
The different types of fullerenes form solutions of different colors.
Tubes with double walls of C6 rings were the first to be discovered.
The ends of the tubes can be opened if they are heated correctly.
In Section 13.1, we talked about how carbon can form long sheets of carbon atoms.
They are 100 times stronger than steel and 116 times dense.
These wires can be used to make tiny electronic devices.
According to geologists, the majority of Earth's crust is composed of sil tetrahedron.
One oxygen atom occupies each corner in a network of covalent structures made of Silicon and oxygen.
A complete octet is obtained by bonding the Silicon atom to four oxygen atoms.
Each oxygen atom is short by one electron.
Each Si atom is surrounded by four O atoms and acts as a bridge connecting the corners of two tetrahedrons.
Section 24.3 has a discussion of silicate structures.
The silicate structures we examined are common in ceramics and are a bridge connecting the corners of cement and glass.
These substances are used in a lot of things.
You are likely to see examples of these materials if you look around.
Each class of materials is examined individually in this section of the chapter.
Review flashcards and saved quizzes
Getting your flashcards
Privacy & Terms