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Bonding

Molecules are formed when atoms bond together. Chemical bonding is hugely important in chemistry and, unsurprisingly, it forms a large part of the GCSE Chemistry syllabus. This is the first of four quizzes on bonding and it looks at some of the types of bonding – covalent, ionic and metallic - which occur between different elements.

A chemical bond is an attraction between atoms. Everything in nature wants to be stable. For atoms, this means having a full outer shell of electrons. To do this, atoms need to have the electron structure of one of the unreactive noble gases. These are the elements in the group at the extreme right hand end of the most commonly used periodic table. There are different ways of numbering the groups of the periodic table. Most UK exam boards still follow the convention that the number of electrons in the outer shell = the number of the group. If you study chemistry to higher levels, you will find that this is no longer the case other than for groups 1 and 2, so most schools teach that the noble gases are in group 8, but a few call it group 0 or group 18.

To achieve this, atoms give away electrons to other atoms; some will take electrons from other atoms and some will share their outer electrons with other atoms. How atoms achieve states of stability determines which types of bonding they undertake; whether it be covalent or ionic. There are other types of bonding too but you will only need to learn about covalent, ionic and metallic bonding for your GCSE exams.

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The type of bonding also determines the structure of a material. Covalently bonded compounds usually form individual molecules but there are some covalent substances, like diamond and graphite, which have giant structures. Ionic compounds are never found as molecules, they are always giant lattices that sometimes form very beautiful crystals. In the right circumstances, crystals can be enormous - there are people who make a living from finding and selling these.

Bonding also gives rise to the properties of substances like hardness, solubility in water, melting point and boiling point but it is not always clear-cut - there are some molecules that behave partly like ionic compounds and vice versa. Understanding bonding can help you to understand the behaviour of chemicals as well as helping you to predict and explain the behaviour of unknown substances.

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  1. What type of bonding has 'free' electrons?
    In metals positive metal ions are surrounded by a 'sea' of negative electrons that are free to move. These free electrons are the reason why metals are good conductors of heat and electricity
  2. What type of bonding occurs when electrons are shared between the atoms in a molecule?
    One example of this occurs between hydrogen and oxygen atoms in water molecules
  3. What type of structure does the carbon in diamond form?
    A diamond owes its hardness to the arrangement of its atoms in this structure
  4. In an ammonia molecule hydrogen and nitrogen atoms share electrons. What kind of bonding is this?
    Ammonia is an important manufacturing chemical that we make using the Haber process
  5. The type of bonding that holds the atoms together in salt is...
    The sodium atoms donate an electron to the chlorine atom; they become ions - Na+Cl- - and their opposite charges hold them together
  6. What type of bonding occurs when electrons are transferred from the outer shell of one atom to the outer shell of another?
    One example of this occurs between lithium and fluorine atoms in lithium fluoride
  7. The type of bonding that holds the atoms together in water is...
    Hydrogen and oxygen are both non-metals and so share electrons to form covalent bonds
  8. What type of bonding is present in gold?
    A metal consists of positively charged metal ions surrounded by a 'sea' of electrons
  9. Glucose molecules are formed from atoms of carbon, hydrogen and oxygen. What type of bonding is present in a glucose molecule?
    Covalent bonds are made between the non-metal atoms in glucose
  10. Graphite is a substance made of carbon atoms only, as is diamond. However, the two substances are very different. Why?
    The atoms in graphite are in layers. The bonding between the layers is weak and because of this they can slide over each other, making the substance very soft and slippery - it is a good lubricant e.g. for things like zip fasteners

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