rons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between the cations and delocalized electron. These interactions are called “metallic bonds” and the model is termed as “sea of electrons model”. Ionic crystals. Made of ions (cations and anions) which form strong electrostatic interactions that hold the crystal lattice together. The electrostatic attractions are numerous and extend throughout the crystal since each ion is surrounded by several ions of opposite charge, making ionic crystals hard and of high melting points. Molecular crystals. Made up of atoms, such as noble gases, or mol
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
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FOUR TYPES OF CRYSTALS (SOLID)
- Metallic crystals. Made of atoms that readily lose electrons to form positive ions (cations) but no atom in the crystal would readily gain electrons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between the cations and delocalized electron. These interactions are called “metallic bonds” and the model is termed as “sea of electrons model”.
- Ionic crystals. Made of ions (cations and anions) which form strong electrostatic interactions that hold the crystal lattice together. The electrostatic attractions are numerous and extend throughout the crystal since each ion is surrounded by several ions of opposite charge, making ionic crystals hard and of high melting points.
- Molecular crystals. Made up of atoms, such as noble gases, or molecules such as sugar, iodine and naphthalene. The atoms or molecules are held together by a mix hydrogen bonding/dipole-dipole and dispersion forces, and these are the attractive forces that are broken when crystal melts.
- Covalent network crystals. Made of atoms in which atom is covalently bonded to its nearest neighbors. The atoms can be made of one type of atom or made ofcan be made of different atoms. There are no individual molecules and the entire crystal mat be considered one very large molecule. The valence electrons of the atoms in the crystal are all used to form covalent bonds because there are no delocalized electrons, covalent network solids do not conduct electricity. Covalent bonds are the only type of attractive bond between atoms in network solid.
|
Type of Solid |
Form of Unit Particle |
Forces Between Particle |
Properties |
Example |
|
Molecular |
Atoms/molecules |
London Dispersion
Dipole-dipole forces
Hydrogen Bonds |
|
Argon, Methane |
|
Covalent Network |
Atoms in a network of covalent bonds |
Covalent Bonds |
|
Diamond, quarts |
|
Ionic |
Positive and negative ion |
Electrostatic Attraction/Ionic Bonds |
|
Typical salts, Sodium Chloride, Potassium Chloride, Calcium Nitrate |
|
Metallic |
Atoms |
Metallic Bonds |
|
All metallic elments. |
Activity:
Research and describe the properties for each crystals. Use the following as bases of property comparison.
- Strength or hardness
- Melting point
- Electrical conductibility
- Heat conductibility
- Brittleness
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