All about radius of atoms: determination

The radius of an atom can be estimated by taking half the distance between the nucleus of two of the same atoms.
Going across the periodic table, the atomic radius decrease: This is due to the fact that the principle energy level (principle quantum number) remains the same, but the number of electrons increase. The increase in the number of electrons cause an increase in the electrostatics attraction which cause the radius to decrease.
Going down the periodic table, the atomic radius increase: The principle energy level increases and hence the atomic radius increases.

All about Electronegativity: its determination and application

The relative attraction of an atom for an electron in a covalent bond.
Fluorine has highest electronegativity (4.0)
The grater the difference in the electronegativities the more ionic in nature is the bound.
The smaller the difference in the electronegativities the more covalent is the bond.http://positions.dolpages.com

All about Ionization Energy: determination and application

The minimum amount of energy needed to remove an electron from a gasous atom or ion, and expressed in electron volts (eV).

All about Quantum numbers

Describe the placement of an electron in atom, divide into four.
The principle quantum number (n): determine the energy of an orbital and has a value of n = 1,2,3,4…..
The angular momentum quantum number (l): determine the shape of an orbital and has a value of 0 to (n–1).
The magnetic quantum number (m): determine the orientation of the orbital and has a value of – m to + m.
The spin quantum number (ms): determine the magnetic field generated by the electron and has a value of – ½ and + ½.

All about Relative atomic mass

The average weight of the isotopes relative to 1/12 the mass of a 6C12 isotope

Example:
The atomic mass of neon (Ne-19, amu 19.99245, natural abundance of 90.92%, Ne-20, amu 20.99396, natural abundance of 0.260%, Ne-21, amu of 21.99139. natural abundance of 8.82%)

All about Isotopes: facts and figure

Atoms that having same atomic number (equal no of proton) but having different atomic mass (unequal number of neutrons) i.e. isotopes of carbon 6C12, 6C13

All about Atomic number (Z)

Atomic number (Z): The number of proton within the nucleus of an atom. In a neutral atom, the number of proton and electrons are equal and atomic number also indicates the number of electron.

All about Atomic structure and its constituents

An atom of any element consists the electron, proton and neutron.
An atom is the smallest possible particle of any chemical element, which will retain its chemical properties.
An atom consists of 3 subatomic particles - electrons, protons and neutrons. Electrons have a negative charge, protons have a positive charge and neutrons have no charge.
An atom of any element consists the electron, proton and neutron.
Electron: 9.108 × 10-31 Kg, –1.602 × 10-19 Coulomb
Proton 1.672 × 10-27 Kg, +1.602 × 10-19 Coulomb
Neutron 1.675 × 10-27 Kg, 0 Coulomb
Electron: Revolving around the nucleus and determined the volume of atom.
Proton and Neutron: contribute to the majority of mass of atom
The nucleus is very small compared to the atom, about 10000 times smaller. The diameter of an atom is in the order of 10-10 m, whereas the diameter of the nucleus in the order of 10-15 m.
The atom is a very dynamic entity. The diagram shows a stylised representation; the reality is that there is absolute bedlam at the atomic level.
The neutron has a very slightly higher mass than the proton.

All about scope of Coordination Chemistry

Highlights:
1. Tuning of variable valency via ligand control of reductions potentials;

2. Tuning of spin states;

3. Isomer preference of oxidation states and valence/geometry recognition;

4. Water oxidation by a ruthenium shuttle;

5. Oxygen atom transfer from water, per-acids, and oxo-metal reagents;

6. Correlating excited state properties of metal complexes with electronic and molecular structure;

7. Photo-induced electron and energy transfer in metal complex-based molecular assemblies;

8. Thioether coordination and activation of homolog-specific transformations;

9. Recognition of the importance of metal nitrosyl complexes in the ‘‘biology’’ and ‘‘physiology’’ of NO;

10. Spontaneous polynucleation via oximato and phenolato bridging ligands;

11. Characterization of vanadate esters of carbohydrates;

12. Unraveling of modes of actions of some metaloenzymes;

13. Development of metal acycles and the insertion of unsaturates into metalacycles;

14. recognition of ‘‘non-innocence’’ as a significant factor in systems where ligands and metals are both redox active;

15. isolation and characterization of radical anion ligand complexes, and recognition of their role in biology;

16. custom design of cluster oxo-anions and rationalization of their structural parameters, and creation of super-large cluster ions modeling pieces of oxide surfaces;

17. increased understanding of structure–function relationships through structural solutions of metallo-enzymes and other bio-molecules;

18. application of density functional theory to the elucidation of electronic and molecular structure;

19. providing an understanding of the localized-to-delocalized transition in mixed-valence chemistry.

20. bio-transformations, particularly hydrogen evolution, conversion of nitrogen into ammonia,

21. multi-electron transfer processes, and methane oxidation – all under ambient conditions; and water oxidation;~

22. all aspects of materials chemistry where the unique properties of transition metals can be exploited;

23. metal complexes in supramolecular assemblies for use in catalysis and in optical and magnetic devices;~

24. use of metal complexes in aqueous solutions (avoidance of organic solvents in synthesis and catalysis, particularly with respect to industrial processes); it is no exaggeration to say that a large part of life processes are basically pH-controlled in aqueous solution;

25. metal complexes in biology – either for (i) medical purposes such as chemotherapy or (ii) the identification of metal complex cores in biological functions such as their role as ‘‘acids’’ in aqueous media;

26. development of ligand design to facilitate supramolecular systems and designed self-assembly;

27. use of coordination compounds as optical triggers and probes, particularly with respect to long-distance electron tunneling in proteins;

28. metal binding by carbohydrates.

All about 30 % Hydrogen Peroxide (H2O2): Morality

Highlights:
1. 30g H2O2/100 g solution
2. The density of the solution is 1.11 g/cm3
3. Morality is measured in moles per liter
M = (w/mwt)x V (lit)
w = weight in grams
mt = Molecular weight
V = Volume in Liters
(D = w/V)
M = (D/Mt)x % of solution x 1000
Mt = 34.01,    % of solution = 30,  Density = 1.1 g/cm3. 
4. Hence Morality of 30 % H2O2 is 9.79 M