Term
| Negative element in ionic bonding |
|
Definition
| Known as the anion, normally non-metal |
|
|
Term
| Positive element in ionic bonding |
|
Definition
| Known as the cation, normally a metal |
|
|
Term
|
Definition
|
|
Term
|
Definition
| Is the attraction of oppositely charged ions. |
|
|
Term
|
Definition
|
|
Term
| When do ionic bonds conduct electricity? |
|
Definition
| Only when aqueous or molten form. They do NOT conduct electricity in a solid form and are there have quite strong bonds. |
|
|
Term
|
Definition
| The sharing of valence electrons to complete a full outer shell. Non metals only. |
|
|
Term
| Covalent bonding occurs with both non metals and metals. True or False? |
|
Definition
False:
Covalent bonding occurs with non metals only. |
|
|
Term
How strong is a covalent bond?
Do it conduct electricity? |
|
Definition
| Extremely strong (more than ionic bond) and therefore does not conduct electricity as a solid or liquid as the strength of the bond is too great. |
|
|
Term
| What happens to charged in covalent bonds? |
|
Definition
| When valence electrons are shared some elements with the molecule might become slightly positive or negative enabling the covalent bond (the molecule) to form another bond with another substance. |
|
|
Term
| Why don't covalent bonds conduct electricty? |
|
Definition
| Because the negative part of the bond needs to travel to a positively charged object whilst the positive part of the bond needs to travel to a negatively charged object. When this happens a flow of electrons (electricity) occurs. Covalent bonds are so great that the atoms inside them cannot separate and move off to attract something so electricity just cannot occur. Same applies to ionic solid bonds. |
|
|
Term
| What do we mean when we say a bond is very strong? |
|
Definition
| We are not talking about it being physical hard which is a result of how tightly bonding each molecule is and is known as inter-molecular bonding. Intra-molecular bonding is strictly the bonds of one molecule where the atoms are held in place. So when we talk about a strong bond it is about how strong or tightly held the atoms are in one molecule and if they are strong they won't separate as easily. |
|
|
Term
|
Definition
| The bonds that are formed by atoms in molecule being held together or the molecule in a substance being held together. They are quite weak and the bonds can loosen or contract and this is when solids, liquids or gases are formed. |
|
|
Term
|
Definition
| Only talking about the atom or molecule itself. A molecular will have atoms of different elements bonded together and this bond is intra-molecular bonding and very strong. When these bonds seperate chemical changes occur. |
|
|
Term
| What are the difference in intra-molecular bonds and inter-molecular bonds effect changes in substances. |
|
Definition
| When inter-molecular bonds change by maybe spreading out or constricting, then physical changes occur. This is like changing from a solid to a liquid to a gas. When intra-molecular changes occur the whole chemical structure is altered and therefore chemical changes will happen,this involves conduction of electricity, further bonding with other substance, burning, changes of colour etc. |
|
|
Term
|
Definition
| A very strong solid bond as atoms are tightly bound. Rectangular prism like. |
|
|
Term
| The _____ the bond, the ______ conductive to electricity it is. |
|
Definition
| The weaker the bond, the more conductive to electricity it is. |
|
|
Term
|
Definition
| Is the attraction of delocalised (free to move) electrons in metal atoms. Obviously only occurs in metals. Due to the atoms being able to move wherever they want, inter-molecular bonding is very flexible and therefore you can even bend thin metal without it breaking because the electrons can move and change the structure of the object to form a new shape. Electricity (flow of electrons) will obviously flow very easily as electrons are free to move and can travel all across the substance / object. This is why metals are conductors. |
|
|
Term
| When do metallic bonds conduct electricity |
|
Definition
| As solids and liquids. Metallic bonds are often NOT of gas form. |
|
|
Term
| If a chemical has 'ate' on the end... |
|
Definition
| Then it has bonded with oxygen |
|
|
Term
| Why do ionic compounds have high melting points? |
|
Definition
Because the charges of the ions are greater than the charger of ions in covalent bonds (slight charged, remember?)
This means the attraction is stronger (intermolecularly not intramolecularly (that's covalent))
More energy is required via heat to loosen the bonds and melt |
|
|
Term
|
Definition
| 3 dimensional structure consisting of bonded and bounded molecular or atoms. Drawn as a cubic with dots in it representing atoms or molecules. |
|
|
Term
| Do three - five balancing chemical compounds questions |
|
Definition
|
|
Term
| When do equations have prefixes and suffixes. |
|
Definition
| When they are covalent bonds, you can identify this by referring to the charged table and seeing if the bond is ionic. If it isn't then add the prefixes. |
|
|
Term
| What prefixes are used on covalent compound names. |
|
Definition
1 - mono
2 - di
3 - tri
4 - tetra
5 - penta |
|
|
Term
|
Definition
|
|
