What different types of bonding exist, and how are they different?

There is 3 types of chemical bonds: ionic, covalent or metallic. All are due to electrostatic attractions between positive charge and negative particles. Ionic bonding happens between opposite charge ions. Covalent bond involves electron pairs being shared between atoms. Metallic bonding consist of a lattice of positive ions surrounded by delocalised electrons.

HI Laura. There's Ionic bonding (loss of electrons by a metal, the same electrons being absorbed by a non metal) to form ions. The bonding is purely electrostatic as if the ions were just charged spheres. Then you have covalent bonding (between non-metal atoms), which is the overlap of electron shells. Each atom appears then to have a full outer electron shell which provides stability. The bonding is maintained by the pull of the two nuclei for the bonding electron pair. Metallic bonding is the bonding within metals, characterised as an array of positive ions in a "sea" of delocalised electrons. That's all you need for GCSE. At A level the covalent model is modified by the idea of polarisation- the more electronegative atom attracts the electrons within the bond at the expense of the less electronegative atom. That is why water is so polar. At A level you also meet "dative" or "co-ordinate" covalent bonding. It is still a covalent bond but BOTH electrons are said to come from one atom in the bond (the ligand). They are often depicted as arrows, though they don't look much different from normal covalent bonds. In reality ionic and covalent bonding are extremes in a continuum but most school courses steer clear of this! I wouldn't count "hydrogen bonding" as real bonding. Rather it is an unusually strong form of intermolecular force, due to the heavy polarisation of the N-H, O-H and H-F bonds. Hope this helps! Colin

1. Ionic Bonding: Firstly its between metals and non metals. Ions are transfered from metals to non metals. Metals loose the electrons and non metals gain the electrons. E.g Sodium looses on electron and that one electron lost from Sodium is gained by chlorine. 2. Covelant bonding: It happens between non metals only. Its when non metal atoms share their electrons. 3. Metallic bondiong: its between metals only. This happens when metals ions have electrostatic forces of attraction between them and sea of delocalised electrons Most importantly biggest tip please remember for ionic and covelant bonding; the primary reason for any of these two bonding is to have a complete outer shell.

There are 3 different types of bonding 1) Ionic bonding 2) Metallic bonding 3) covalent bonding 4) These are different on the basis of their loss & gain of electrons .

Well, always bonding between two different compounds exists which could be commonly either ionic or covalent bonds for example. In more depth, we can still discuss about coordinate covalent bonds exists etc.

If you are in GCSE level (A levels are kinda similar as well): - ionic bonding Atoms "lose or gain electrons to form ions" and create positive or negative charge. This allows to form "electrostatic force between oppositely charged ions" (like a magnetic) to form molecules. Atoms included in this bonding should contain both non metallic and metallic. Forms giant lattice. - covalent bonding Atoms "share outershell electrons" to fill in each other's shell (e.g. If you got 7 outershell electrons in one molecule, other should have 1 outershell electrons to get 8 <-- full). This forms "electrostatic force between non-metallic atoms". Also, they have form of "giant covalent bonding", which is for specific molecules such as diamond, or graphite. The bonding there is very strong which "needs strong energy to overcome the intermolecular force" when you want to melt. (Diamond has 4 covalent bond on each carbon. Graphite has hexagon shape on each layer, and between those layers, it has weak bonding which allows electric current goes through.) - metallic bonding Forms giant lattice between metallic atoms. Electrons are delocalised (moving around) on the outershell, and interacts with positively charged nucleus to create electrostatic forces.

There are 3 types of bonding exist: covalent (sharing of electrons), ionic (transfer of electrons) and metallic (free electrons). Covalent bonding exist between non metals, ionic bonding exist between metal and non metals and metallic bonding exists between metals.

Basically in simple terms there are three types of bonding. 1. Ionic Bonding -Between Metals (Losing electrons) and Non-Metals (gaining Electrons). 2. Covalent bonding (Normally happens between Non metals and involves sharing of electrons e.g Hydrogen bond) 3. Metallic which is basically the bonding in a metallic lattice (Positive particals attracted to the negative particals within the metal).

Hi LauraThere are three main types of bonding. Firstly, there is metallic bonding, which, as the term suggests, involves bonding between metal atoms. Next we have Covalent bonding, which is bonding between 'non-metal' atoms and finally we have Ionic bonding, which is bonding between a metal and non-metal atoms e.g sodium chloride. So in a nutshell those are the three main types of bonding. If you want to learn more about these and other types of bonding such as intermolecular forces etc then. I hope you find this information useful, give me a like and thank you for reading.

There are three different types of bonding at GCSE chemistry. Firstly you have covalent bonds which are between a non metal and another non metal. Then you have metallic bonding which is between two metals . And lastly you have ionic bonds which are between a metal and a non metal.

Let's start with a few basic ones: Covalent bond- a type of bond where atoms "share" their electrons (the orbitals combine to make "hybrid" orbitals). Depending on whether there is a separation of electric charge, they can be polar (like in water) or non-polar (like the ones in oil) Ionic bond- these are the bonds typically found in compounds containing metals and non-metals, like salts. There is no sharing of electrons- the metal is positively charged, while the non-metallic component is negatively charged, which causes them to attract each other. Hydrogen bonds- these usually exist in larger molecules (polymers) and are bonds between Hydrogen atoms and one of the 3 most electronegative atoms : Fluorine, Oxygen and Nitrogen. They are what keeps the DNA molecule stable! Metallic bonds- an electrostatic force develops between the delocalized electrons of the first and second atom. It's an attractive force which causes the atoms to stick together

Ionic and covalent Ionic bond involves transfer of electrons from onee atom to another atom Covalent bond involves sharing of pair of electrons between atoms

Hello Laura. There are three kinds of bonds that I'm aware of. At GCSE level, you'll be expected to learn ionic, covalent, and in some cases metallic bonding. Ionic bonds are quite simple to understand, involving one metal and one or more non-metal substances to create an ionic compound, such as magnesium chloride, lithium oxide, or sodium hydroxide. The ionic part of this comes from the fact that atoms are ionised when metals and non-metals react in this way, an easy way I was given to remember this being to think that the non-metal borrows electrons from the metal. As the metal becomes a positive ion (loses electrons) and the non-metals become negative ions (gain electrons), the pair are drawn together to create an ionic compound through electrostatic force, which creates an ionic bond. TL;DR: Ionic bonds involve metals and non-metals losing or gaining electrons respectively to form a magnetic bond to each other. Covalent bonds are about as common as ionic bonds, but aren't quite as simple to understand as ionic bonds. They involve exclusively non-metals, and form when the non-metal pair share a set of electrons to complete their outer shell. Examples of this include dihydrogen monoxide (water) or hydrogen chloride, where in both the smaller hydrogen atoms are sharing their singular electron with the larger oxygen or chlorine atoms to finish all of their outer shells in one go. These kinds of atomic bonds take a lot of effort to break the atoms apart, but have weak intermolecular forces between molecules, requiring less energy to separate. TL;DR: Covalent bonds use exclusively non-metals sharing electrons to complete their outer shells and form molecules that way. The force between atoms requires a lot of energy to break, but less energy between molecules. Metallic bonds are the least common kind of bonds and also the most complex, so it's unlikely to be seen much but is still handy to know. Metallic bonds aren't bonds in the traditional sense that ionic and covalent bonds are, but rather they represent a force of attraction between a metal's delocalised (free-moving) electrons and positive metallic ions, which is what makes most metals so tough, but also makes them good conductors of electricity and heat as the delocalised electrons are able to move through the metal. Let me know personally if you have any questions.