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Chemistry
| Question | Answer |
|---|---|
| Define an ion | An atom or molecule with a net electric charge due to the loss or gain of one or more electrons. |
| Define an atom | The smallest particle of a chemical element that can exist. |
| Define an isotope | Each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties; in particular, a radioactive form of an element |
| Explain why atoms form ions | |
| Identify the group on the periodic table where the two atoms are found | |
| Explain how atoms become charged on loosing or gaining electrons in chemical reactions. | |
| Give examples eg explain why both magnesium and calcium ions have a charge of +2. | |
| Complete all work set in class | |
| Tabulate first 20 elements, atomic number, electron number, proton number, electron shell diagram, charge on ion formed | |
| Compare the charges on the individual ions found in compounds eg sodium hydroxide and beryllium hydroxide | |
| Explain why the ions combine in the ratios the way they do to form compounds using charge balance eg NaOH and Be(OH)2. | |
| State the sub atomic particles in isotopes eg Lithium-6 (Li) and Lithium-7 (Li). | |
| Consider the atomic structure of each given atom eg Lithium-6 (Li) and Lithium-7 (Li). | |
| Consider the meaning of the numbers ‘6’ and ‘7’ in terms of the atomic structures | |
| Explain how the particles within an atom contribute to its overall mass. Drawings are a clever method of communicating | |
| Define an indicator | |
| Describe the colours and meanings of the colours of universal indicator solution. | |
| Define an ion | |
| Define an atom | |
| Define an isotope | |
| Explain why atoms form ions | |
| Identify the group on the periodic table where the two atoms are found | |
| Explain how atoms become charged on loosing or gaining electrons in chemical reactions. | |
| Give examples eg explain why both magnesium and calcium ions have a charge of +2. | |
| Complete all work set in class | |
| Tabulate first 20 elements, atomic number, electron number, proton number, electron shell diagram, charge on ion formed | |
| Compare the charges on the individual ions found in compounds eg sodium hydroxide and beryllium hydroxide | |
| Explain why the ions combine in the ratios the way they do to form compounds using charge balance eg NaOH and Be(OH)2. | |
| State the sub atomic particles in isotopes eg Lithium-6 (Li) and Lithium-7 (Li). | |
| Consider the atomic structure of each given atom eg Lithium-6 (Li) and Lithium-7 (Li). | |
| Consider the meaning of the numbers ‘6’ and ‘7’ in terms of the atomic structures | |
| Explain how the particles within an atom contribute to its overall mass. Drawings are a clever method of communicating | |
| Define an indicator | |
| Describe the colours and meanings of the colours of universal indicator solution. | |
| Describe the colour of universal indicator solution in different common acids and bases eg hydrochloric acid, sodium hydroxide, nitric acid solution and sodium carbonate solution. | |
| Describe the colour of universal indicator solution in different an equal mixture of two common acids and bases eg hydrochloric acid, sodium hydroxide. | |
| Predict your observation if the acid and base was mixed dropwise. |
Created by:
tianawilliamson00
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