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Chemistry Basics

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Atom name symbol electron configuration
1) Copper Cu 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1 Chromium Cr 1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1 Chlorine Cl 1s2, 2s2, 2p6, 3s2, 3p5 Neon Ne 1s2, 2s2, 2p6 Potassium k 1s2, 2s2, 2p6, 3s2, 3p6, 4s1 Magnesium Mg 1s22, 2s2, 2p6, 3s2
2) Electronegativity Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.
The Pauling scale is the most commonly used. Fluorine (the most electronegative element) is assigned a value of 4.0, and values range down to ceasium and francium which are the least electronegative at 0.7. As you go down a group, electronegativity decreases. (If it increases up to fluorine, it must decrease as you go down.) As you go across a period the electronegativity increases.

4) TYPES OF BONDS Primary;
Ionic bonding
Covalent bonding
Metallic bonding Ionic bonding
Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion.

Secondary bonds (also known as interparticle, intermolecular, or Van der Waals attractions) are the relatively weaker attractions between nearby atoms or molecules that are important in most liquids (especially liquid mixtures) and some solids. Three types of inter molecular forces are Hydrogen bonds, Dipole-Dipole…...

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