Exploring the fundamentals of chemical bonding, this overview delves into ionic, covalent, and metallic bonds. Ionic bonds involve electron transfer to form stable ions, as seen in sodium chloride. Covalent bonds, including polar and nonpolar, arise from electron sharing, exemplified by the molecules of hydrogen and oxygen. Metallic bonds feature a sea of delocalized electrons, giving metals their characteristic properties. Bond strength, energy, and reaction enthalpy are also discussed, highlighting the importance of these concepts in chemistry.
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Chemical bonds are the forces that link atoms together to form molecules and compounds
Electronegativity
Electronegativity is the tendency of an atom to attract electrons and determines the type of bond formed
Pauling Scale
The Pauling scale is used to measure electronegativity and determine if a bond is ionic, covalent, or metallic
There are three primary types of chemical bonds: ionic, covalent, and metallic
Ionic bonds form through the transfer of electrons between a metal and a non-metal with a large electronegativity difference
Ionic Compounds
Ionic compounds are typically crystalline solids with high melting points and electrical conductivity in solution
Electrostatic Forces
The strong electrostatic forces in the crystal lattice of ionic compounds contribute to their stability
Sodium chloride (NaCl) and magnesium oxide (MgO) are examples of ionic compounds formed through the transfer of electrons
Covalent bonds form through the sharing of electrons between two non-metal atoms
Nonpolar Covalent Bonds
Nonpolar covalent bonds form when the electronegativity difference is less than 0.5
Polar Covalent Bonds
Polar covalent bonds form when the electronegativity difference is between 0.5 and 1.7
Hydrogen molecule (H2) and oxygen molecule (O2) are examples of covalent compounds formed through the sharing of electrons
Metallic bonds are unique to metals and involve a lattice of cations immersed in a sea of delocalized electrons
Conductivity
The delocalization of electrons in metallic bonds allows for excellent thermal and electrical conductivity
Malleability
The metallic bond's ability to move and shift allows for metals to be malleable and ductile
Metals such as iron, copper, and gold exhibit metallic bonding
00
Atoms are linked by ______ ______, which are crucial for creating molecules and compounds around us.
chemical
bonds
01
The ______ scale measures an atom's tendency to attract electrons, known as ______.
Pauling
electronegativity
02
Ionic bond formation process
Electron transfer from one atom to another, typically metal to non-metal.
