Solids are characterized by their definite shape and also their considerable mechanical strength and rigidity. The particles that compose a solid material(with few exceptions), whether ionic, molecular, covalent or metallic, are held in place by strong attractive forces between them.
Definite Volume
Not Definite Shape
Molecules Are Much Closer Than Gases
Intermolecular Forces In Between Solids And Gases
properties of liquids
Evaporation
Process Of Changing A Liquid Into A Gas Phase
For example, liquid water conversion into vapor form
Cooling Process
Solids are characterized by their definite shape and also their considerable mechanical strength and rigidity. The particles that compose a solid material(with few exceptions), whether ionic, molecular, covalent or metallic, are held in place by strong attractive forces between them.
Definite Volume
Not Definite Shape
Molecules Are Much Closer Than Gases
Intermolecular Forces In Between Solids And Gases
properties of liquids
Evaporation
Process Of Changing A Liquid Into A Gas Phase
For example, liquid water conversion into vapor form
Cooling Process
factors effecting ionization energy,first,second third ionization energy complete article must follow link-
googlegalaxychemistry.com /search ionization energy trend
The ionization energy trend changes when move across period and group. It is quite evident that ionization enthalpy of elements are linked with their electronic configurations .in each period ionization energy maximum are found at noble gases while minimum energy to remove electron notice at the alkali metals
Kinetic theory of Gases provides the much-needed interlink between the macroscopic and the microscopic. It depicts the behavior of gases under different physical conditions.
Surface and Interface • When phases exist together, the boundary between two of them is known as an interface. • The properties of the molecules forming the interface are often sufficiently different from those in the bulk of each phase. • The term surface is used when referring to either a gas–solid or a gas–liquid interface.
This slides will give us a brief idea about the surface tension of a liquid. it will also describe about the importance and effect in our day to day life. determine the theory on surface tension and solve various problems on it.
This presentation covers concepts such as surface tension, surface energy, liquid drops and bubbles, wetting, capillarity at the elementary school level. Comment down in a box for improvement.
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
factors effecting ionization energy,first,second third ionization energy complete article must follow link-
googlegalaxychemistry.com /search ionization energy trend
The ionization energy trend changes when move across period and group. It is quite evident that ionization enthalpy of elements are linked with their electronic configurations .in each period ionization energy maximum are found at noble gases while minimum energy to remove electron notice at the alkali metals
Kinetic theory of Gases provides the much-needed interlink between the macroscopic and the microscopic. It depicts the behavior of gases under different physical conditions.
Surface and Interface • When phases exist together, the boundary between two of them is known as an interface. • The properties of the molecules forming the interface are often sufficiently different from those in the bulk of each phase. • The term surface is used when referring to either a gas–solid or a gas–liquid interface.
This slides will give us a brief idea about the surface tension of a liquid. it will also describe about the importance and effect in our day to day life. determine the theory on surface tension and solve various problems on it.
This presentation covers concepts such as surface tension, surface energy, liquid drops and bubbles, wetting, capillarity at the elementary school level. Comment down in a box for improvement.
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
Suitable for: 1. Technical Personnel and Decision-Makers are encouraged to participate in this training. 2. DECISION MAKERS: Technical Directors, Managers, Purchasers. 3. TECHNICAL PERSONNEL: Lecturers, Technical Sales, Marketing, Failure Analysis, Research & Development, Quality Control and Assurance, Production Engineers or Technicians. The characteristic of surface and near-surface regions of materials can be characterised by various surface analysis techniques. Applications of many engineering materials are determined by the surface and near-surface structures. Therefore, the well being of this region is essential in order to obtain a pre-required condition for those materials to be applied for a specific application. Typically, failure of engineering products may be traced back to surface/near-surface contamination or surface reconstruction. In order to obtain more information related to the failure, in-sight of these regions need to be exposed. This course is outlined to introduce basic principles of surface science, which serve as an essential foundation to explain the operation concepts and applications of several important surface analysis techniques. Know-how of interpreting the analysis data is also explained in this “easy-to-follow” and “easy-to-understand” training course. With these and the support of brief but sufficient fundamental theories, skill of selecting a relevant technique with respect to its practical engineering usage will be covered. Ultimate goal for this course is to increase level of knowledge in making a correct technical decision to solve surface related issues and transform knowledge into applications.
There are two types of atomic bonds - ionic bonds and covalent bonds.pdfaswrd
There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their
structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and
bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 -
200 kcal/mol). Whether two atoms can form a covalent bond depends upon their
electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two
atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the
atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and
negatively charged ion (anion). The bond between these two ions is called an ionic bond.
Covalent BondsIonic Bonds
Polarity:LowHigh
Formation:A covalent bond is formed between two non-metals that have similar
electronegativities. Neither atom is \"strong\" enough to attract electrons from the other. For
stabilization, they share their electrons from outer molecular orbit with othersAn ionic bond is
formed between a metal and a non-metal. Non-metals(-ve ion) are \"stronger\" than the
metal(+ve ion) and can get electrons very easily from the metal. These two opposite ions attract
each other and form the ionic bond.
Shape:Definite shapeNo definite shape
What is it?:Covalent bonding is a form of chemical bonding between two non metallic atoms
which is characterized by the sharing of pairs of electrons between atoms and other covalent
bonds.Ionic bond, also known as electrovalent bond is a type of bond formed from the
electrostatic attraction between oppositely charged ions in a chemical compound. These kinds of
bonds occur mainly between a metallic and a non metallic atom.
Melting point:lowHigh
Examples:Methane (CH4), Hydro Chloric acid (HCl)Sodium chloride (NaCl), Sulphuric Acid
(H2SO4 )
Occurs between:Two non-metalsOne metal and one non-metal
Boiling point:LowHigh
State at room temperature:Liquid or gaseousSolid
Ability to conduct electricity in molten/aqueous state:
Yes
Ability to conduct electricity in solid state:
Solution
There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their
structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and
bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 -
200 kcal/mol). Whether two atoms can form a covalent bond depends upon their
electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two
atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the
atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and
negatively charged ion (anion). The bond between these two ions is called an ionic bond.
Covalent BondsIonic Bonds
Polarity:LowHigh
Formation:A covalent bond is formed between two non-metals that have similar
electronegativities. .
Metallic bond was defined as a type of chemical bond formed between the positively charged ions (+) and the free-floating electrons (e) in a lattice structure.
It was also mentioned that the structure of a metallic bonds is very different from that of ionic and covalent compounds. In metallic bond the valence electrons of the interacting metal atoms are delocalized
Similar to Classification of crystalline solids (20)
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2. Ionic solids
Lattice points are occupied by positive and negative ions.
Hard and brittle solids.
High m.p due to very strong electrostatic forces of attraction.
Poor conductors of electricity in solid state but good in
molten state.
Packing of spheres depends upon:
a) presence of charged species present.
b) difference in the size of anions and cations.
Two types:
AB types.
AB2 types.
3. Covalent solids
Lattice points are occupied by neutral atoms.
Atoms are held together by covalent bonds
Hard solids.
High m.p.
Poor conductors of electricity.
Two common examples: diamond & graphite.
4. Molecular solids
Lattice points are occupied by neutral molecules.
The molecules are held together by Vander Waal’s forces.
Very soft solids.
Low m.p.
Poor conductors of electricity.
5. Metallic solids
Lattice points are occupied by positive metal ions
surrounded by a sea of mobile e-.
Soft to very hard.
Metals have high tensile strength.
Good conductors of electricity.
Malleable and ductile.
Bonding electrons in metals remain delocalized over
the entire crystal.
High density.
