Ionic bonding is typing of chemical bonding occurs when electrons are transferred from one atom to another. This typically happens between a metal and no metal gains those electrons to from an electricity negatively charged ion. These oppositely charged ions attract each other to from a strong bond.
Ionic bonds form when a metal atom transfers on eor more of its outer electrons to a non- metal atom. The strong becomes a positively charged ion, while the no metal becomes a negatively charged ion. The strong electrostatic force of attraction between these opposite changes holds the ions tougher, creating the ions bond.
Ionic compounds generally have high melting and boiling points because of the strong icon bonds, between their ions. They are usually hard and brittle solids at room temperature. In their solid state, they do not conduct electricity, but when melted or dissolved or dissolved in water, they become good conductors because the ions are free to move.
Ions compound soluble in water because water molecules are polar, meaning they have positive side. The positive end of water molecular attracts the negative ions, and the negative and attract the positive ions. This interactions breaks the ions bonds in the compounds, causing the ions to disperse in the water.
Sodium chloride commonly known as table salt is an example of an ionic compounds sodium (Na) is a metal that loses one electrons to become a negatively charged ion. These oppositely charged ion attract and from a strong ionic bond.
Covalent bonding is a type of chemical bond formed when two non- metal atoms share electrons. This sharing allows both atoms to achieve a full outer electrons shell making them more stable.
Covalent bonds from when share one or more pairs of electrons. Each shared created a bond. For example, in a water molecules oxygen electrons with one two hydrogen atoms forms covalent bonds.
Covalent compounds usually have low melting and boiling points , are poor conductors of electricity and may exists as solids, liquids or gasses at room temperature , depending on their molecular structure.
A single bonds involves shared pair of electrons a double bond involves two shared pairs, and a tripe bond involves three shared pairs , For instance, forms a double bond , while nitrogen forms a triple bonds.
Methane an example of a covalent compound. Carbon shares its four outer electrons with four hydrogen atoms, forming four covalent bonds that hold the molecules tougher.
Coordinates covalent bonding occurs when both electrons in a shared pair come from the same atom. It is similar to covalent bonding but involves one atom donating a lone pair to from the bond atom. It is similar to covalent bonding but involves one donating a lone pair to form the bond.
A coordinate covalent bonds forms one atom with a lone pair of electrons, donates them to another r atom or ion that lacks electrons Foe example in the ammonium ion nitrogen donates a lone pair to bond with a hydrogen ion.
In covalent bonds , each atom contributes one electron to the shares pair .In electrons covalent bonds on atom donates both electrons to the shared pair, though the resulting bond behaves like a regular covalent bond?
Examples includes the ammonium ion, where nitrogen donates alone pair hydrogen, and carbon monoxide, where one oxygen atom dominates a lone pair to carbon.
Coordinate bond covalent are typically indistinguishable from regular covalent bonds once formed. They are surrounded by a sea of free moving delocalized electrons. This gives metals their unique properties.
Metallic bonding is the type of bonding is metals, where positively charged metal ions are surrounded by sea of free moving delocalized electrons. This gives metals their unique properties.
Metallic bonding occur when metals atoms release their electrons, which become delocalized and move freely throughout the metal lattice. The positive metal ions are helps tougher by the attraction to these free electrons.
Metallic bonding gives metals properties like high electrons and thermal conducting malleability ductility, and a shiny appearance. These properties Aries from the movement of delocalized electrons.
Metals are good conductors because the delocalized electrons in the metals bond can more freely allowing electric current to follow easily through the metal.
An example of metallic bonding id found aluminum .In aluminum, the positively changed ions are surrounded by a sea of delocalized, creating strong bonds that give aluminum it’s strange and conductivity.
Intermolecular forces are the attractive forces between molecules that hold them tougher to solids, liquid and gasses, .While weaker than chemical bonds, they play a critical role in determining the physically properties of substances such as melting points, boiling points ,and solubility points.
There are three main types of intermolecular forces :
1. Lodan dispersion forces: weak forces present in all molecules, caused by temporary with permanent dipoles.
2. Dipole –dipole forces: stronger forces that occur between polar moleclues with permanent dipole.
3. Hydrogen bonding: The strongest intermolecular forces, occurring when hydrogen is bonded to electro negatively atom like oxygen nitrogen or fluorine.
Intermolecular forces arise from the attraction between molecules, while chemical bonds involve the actual sharing or transfer of electrons between atoms, because on electrons are directly shared or transferred in intermolecular forces , they are much weaker than covalent or ion bonds.
The strength of inter molecular forces of depends bonding of molecules. Polar molecules have stronger forces like dipole interactions or hydrogen while large molecules with more electrons have strong London desperation forces. What are the consequences of strong intermolecular forces?
Substance with strong intermolecular forces have high boiling and melting point because more energy is required to overcome these attractions. They also have higher viscosity and surface tension, as seen in water due to hydrogen bonding.
Dipole forces are attraction between the positive en doff on polar molecular and the negative end of the. These forces occur because polar molecules have an uneven distribution of electrons creating a permanent dipole. For example in hydrogen chloride the hydrogen end of the slightly positive, and the chlorine end is slightly negative, resulting in dipole- dipole attraction.
Dipole – dipole forces occur when molecules are polar, meaning have a partial positive charge on one end and a partial negative charge on the other. This happens in molecules where there is a significant difference in electro negatively between bonded atoms, such as in sulfur dioxide in hydrogen fluoride
Molecules with dipole – dipole forces typically boiling points compared to nonpolar molecules of similar size. The stronger attraction between polar molecules requires more energy to separate them resulting in higher boiling and melting points, For example, hydrogen fluoride has a much higher boiling point than fluorine which only exhibits Lodan dispersion forces.
Hydrogen bonding is a special type of dipole – dipole interaction that occur when hydrogen atom is bonded to highly electronegative elements like oxygen, nitrogen or fluorine. The hydrogen atom becomes highly positive due to the electro negatively its bonding partner, allowing it to form strong attraction with a lone pair of electrons on another electronegativeley atom in a neighboring molecules.
Hydrogen bonding in water is responsible properties, such as its boiling point, surface tension and ability to dissolve many substances. For instances water molecules form a network of hydrogen bonds, making it harder to separate them, which is why water has a much higher boiling point compared to other similar –sized moleclues like hydrogen sulfide.
A classic example of hydrogen bonding is in water. Each water molecules can form up to four hydrogen bonds: two through its lone pairs on oxygen and two through hydrogen atoms. These bonds result in water liquids state at room temperature and its high heat capacity.
Hydrogen bonds play a crucial in the structure of DNA. They hold two strands of the DNA bonds, helix tougher by forming specific base pairs: adenine pairs with thymine via two hydrogen bonds, while cytosine pairs with guanine via three hydrogen bonds. These ensures stability and specificity in the genetic code.
Hydrogen bonding is strongest than regular dipole forces because it involves a high polar bond and a very small hydrogen atom. The small size of hydrogen allows for closer proximity to the electrogative have similar sizes. This is because hydrogen bonds in water require more to break.
Hydrogen bonding significantly increase the boiling points substance. For example, water has a much higher boiling points than hydrogen Due it hydrogen bonding thought both molecules have similar sizes. This is because the hydrogen bonds in water require more energy to break.
The boiling point of HF is less than H2o because water can from up to four hydrogen bonds per molecules, while HF can only form two water extensive hydrogen network requires bonds energy to break, resulting in higher boiling point.
