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Chemistry - Unit A1
Fundamentals in Chemistry
| Question | Answer |
|---|---|
| What is an Atom? | The smallest part of an Element. |
| What is an Element? | Made from only one type of Atom. |
| What is a Compound? | Made from two or more elements which have been chemically bonded. They cannot be separated. |
| What is a Mixture? | Made from two or more substances which are not chemically bonded. Can be separated. |
| What method of separation would you use to separate a mixture of sand and water? | Filtration |
| What equipment is needed for Filtration? | Filter paper, Funnel, Conical Flask |
| What method of separation would you use to separate a mixture of Copper Sulphate crystals in water? | Crystallisation |
| What method of separation would you use to separate a mixture of water from ink? | Distillisation |
| What method of separation would you use to separate the different colours in pen ink? | Chromotography |
| What is the Plum Pudding model of the atom? | A sphere of positive charge with negatively charged electrons embedded |
| What was the Alpha scattering experiment? | Alpha particles were discovered. These particles had a positive charge. These were fired at a thin sheet of gold foil. |
| What conclusions were drawn from the Alpha scattering experiment? | The nucleus is very small and positively charged - because they repel α particles which are also positive and because most α particles pass straight through. Most of the mass of the atom is found in the nucleus. Most of the atom is empty space |
| What happened during the Alpha scattering experiment? | The alpha particles would either go straight through or reflect/deflect off. |
| What is the Nuclear model of the atom? (Current model) | Atoms have a very small, positive nucleus. The Electrons orbit the nucleus at specific distances (in Shells). |
| What are the three sub-atomic particles? | Protons, Neutrons and Electrons |
| Which sub atomic particles can be found in the Nucleus of an atom? | Protons and Neutrons |
| Where is all of the mass of an atom concentrated? | In the Nucleus |
| What is the relative atomic mass of a Proton? | 1 |
| What is the relative atomic mass of a Neutron? | 1 |
| What is the relative atomic mass of an Electron? | 1/2000 |
| What is the relative charge of a Proton? | +1 (Positive proton) |
| What is the relative charge of a Neutron? | 0 (Neutral Neutron) |
| What is the relative charge of an Electron? | -1 (Negative Electron) |
| Electrons orbit the Nucleus in _________. | shells |
| What is between the Nucleus of an atom and the Electron shells? | The atom is mainly empty space. |
| What does the Atomic number of an Element tell you? | The number of Protons = The number of Electrons |
| What does the Mass number of an Element tell you? | The number of protons + the number of neutrons |
| How can you determine the number of Neutrons in an atom? | Mass number - Atomic number = Number of Neutrons |
| Elements have no overall charge. What does this mean for the number of Protons and Electrons? | Elements have no charge because there are the same number of protons and electrons. |
| What is an Isotope? | Isotopes are the same element (same number of protons) but have different numbers of neutrons. |
| How did John Dalton arrange the Elements? | John Dalton arranged the elements by putting them in order of their atomic mass. |
| How did Newland's arrange the Elements? | Elements were arranged by atomic mass/weight. Every 8th element had similar properties. |
| What were the downfalls with Newland's Periodic table? | Elements were grouped that had different properties. He didn’t leave gaps for undiscovered elements. Some elements were grouped together in the same space. Newland was not a respected Scientist. |
| How did Mendeleev overcome the problems with Newlands Periodic table? | He left gaps where elements didn’t match up with similar chemical properties as he assumed these elements hadn’t been discovered. He switched elements so that their properties matched the group. This is explained by the discovery of isotopes. |
| How many electrons are on the outer shell of a Group 1 element? | 1 |
| How many electrons are on the outer shell of a Group 7 element? | 7 |
| How does a Group 1 element become stable? | Loses one electron |
| How does a Group 7 element become stable? | Gains one electron |
| If a Sodium atom loses on Electron to become stable, what happens to it's overall charge? | Sodium becomes a positively charged ion. |
| How does reactivity change as you go down the Group 1 elements? | Reactivity increases |
| How does reactivity change as you go down the Group 7 elements? | Reactivity decreases |
| How does reactivity change as you go down the Group 0 elements? | These elements are unreactive (Noble gases) |
| What is formed what Group 1 metals react with non metals? | They form salts (these are always white). |
| How do Group 1 elements become stable? | They lose one electron to leave a full outer shell, becoming +1 ions. |
| What happens when you dissolve the group 1 metal salts in water? | All group 1/alkali metal salts dissolve to form colourless solutions. |
| Which gas is produced when Group 1 alkali metals react with water? | Hydrogen (H) |
| What Group are the 'Alkali metals'? | Group 1 elements |
| What happens to the Group 1 alkali metals when they react with Oxygen in the air? | They turn from a shiny metal to a dull grey colour. Metal + Oxygen = Metal oxide |
| What is the chemical equation for when Group 1 alkali metals react with water? | Alkali metal + water = Metal hydroxide + hydrogen |
| Why do Group 1 alkali metals react more violently as you go down the group? | They react more violently as you go down the group because the outer electron gets further from the nucleus. This means that outer electron is less strongly attracted to the nucleus and is more easily donated during the reactions. |
| What group are 'The Halogens'? | Group 7 elements |
| What properties change as you go down the Group 7 Halogens? | The melting points increase. The boiling points increase. They become darker in colour. The relative molecule masses increase. |
| What is a displacement reaction? | When a more reactive element replaces a less reactive element in a compound. |
| Complete this displacement reaction: Chlorine + potassium bromide --> | --> potassium chloride + bromine |
| Complete this displacement reaction: Chlorine + potassium iodide --> | --> potassium chloride + iodine |
| Complete this displacement reaction: Bromine + potassium iodide --> | --> potassium bromide+ iodine |
| How does a Group 7 element become stable? | Gaining one electron, therefore becoming a -1 ion. |
| Why do Group 7 Halogens become less reactive as you go down the group? | As you go down the group the outer shell of electrons get further from the nucleus. Therefore electrons are less strongly attracted by the positive nucleus as you go down the group. |
| Why are the Noble gases unreactive? | They all have full outer shells. They are stable. |
| As you go down the Group 0 elements, what changes? | As you go down the group the boiling point increases As you go down the group the atomic mass increases |
| What properties do the Transition metals have? | Hard Strong High melting points High boiling points High density Less reactive in air than Alkali metals Transition elements react very slowly or not at all with water |
| What does a catalyst do? | A catalyst lowers the activation energy meaning that a reaction can occur |
Created by:
nashl
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