Term
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Definition
| Atoms of the same element with a different number of neutrons (and the same number of protons) |
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Term
| Why do elements in the same group have similar chemical properties? |
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Definition
| Because they have the same number of electrons in the outer shell |
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Term
| How does the boiling point of Group 0 elements change down the group? |
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Definition
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Term
| Explain why group 1 elements get more reactive down the group |
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Definition
| More electrons, more shielding, weaker electrostatic attraction from the nucleus to the outer shell, easier to lose an electron |
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Term
| What type of elements will form ionic bonds? |
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Definition
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Term
| What happens to the electrons in an ionic bond? |
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Definition
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Term
| If an atom has lost electrons, what charge will it have as an ion? |
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Definition
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Term
| Explain why ionic compounds do not conduct electricity when solid, but do conduct when molten or in solution |
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Definition
| The ions are not free to move and carry charge in a solid, but are free to move and carry charge in solution or when molten |
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Term
| What type of elements will form covalent bonds? |
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Definition
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Term
| What happens to the electrons in a covalent bond? |
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Definition
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Term
| Explain why most covalent substances do not conduct electricity |
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Definition
| There are no electrons or ion that are free to move and carry charge |
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Term
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Definition
| Millions of small molecules joined (bonded) together in a chain to form a large molecule |
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Term
| What happens to the electrons in a metallic bond? |
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Definition
| The outer shell electrons delocalise and form a “sea” of electrons that surrounds the positively charged metal ions |
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Term
| How can metals be placed in order of their reactivity? |
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Definition
| Add the metals to water or acid and see which ones react more vigorously, or try a displacement reaction with another metal. |
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Term
| What is a displacement reaction? |
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Definition
| A reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or solutions. |
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Term
| State the three common acids and give their formulae. |
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Definition
| Hydrochloric acid HCl(aq), sulfuric acid H2SO4(aq) and nitric acid HNO3(aq) |
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Term
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Definition
| A metal (or ammonium) oxide, hydroxide or carbonate that will react with and neutralise an acid |
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Term
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Definition
| An alkali is a soluble base |
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Term
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Definition
| A compound formed when some or all of the hydrogen from an acid is replaced by a metal (or ammonium) e.g. calcium sulfate |
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Term
| What salts are formed by hydrochloric acid? |
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Definition
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Term
| What salts are formed by sulfuric acid? |
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Definition
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Term
| What salts are formed by nitric acid? |
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Definition
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Term
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Definition
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Term
| metal hydroxide + acid GIVES... |
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Definition
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Term
| metal carbonate + acid GIVES... |
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Definition
| salt + carbon dioxide + water |
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Term
| What 5 factors can affect the rate of a reaction? |
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Definition
temperature,
surface area of a solid,
concentration of reactants in solution,
pressure of gases,
catalyst |
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Term
| How do you calculate rate of reaction from a graph of amount of product against time? |
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Definition
| Draw a tangent to the curve and find the gradient |
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Term
| What are the units for rate of reaction? |
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Definition
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Term
| Why does increasing concentration of reactants in solution, increase rate of reaction? |
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Definition
| More particles, therefore more frequent collisions between reactant particles |
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Term
| How do catalysts speed up reactions? |
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Definition
| They provide another route for the reaction to take place which has a lower activation energy |
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Term
| What is a reversible reaction? |
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Definition
| A reaction which can go from reactants to products but also from products to reactants |
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Term
| What is dynamic equilibrium? |
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Definition
| The point in a reversible reaction when the forward and reverse reactions are occurring at the same rate |
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Term
| What is the general formulae for alkanes? |
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Definition
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Term
| How does viscosity change with the length of an alkane? |
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Definition
| The longer the alkane, the more viscous (the thicker) it is |
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Term
| Why is cracking important and what are the products? |
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Definition
| Because smaller hydrocarbons are more useful than longer ones. Short alkanes and alkenes |
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Term
| How do you test for an alkene and what colour change would you see? |
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Definition
| React with bromine water which turns from orange to colourless |
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