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Group 1 (GCSE Chemistry)
The following is a GCSE Chemistry test covering 'Group 1' from the broader topic Atomic Structure And The Periodic Table. The test is geared towards the AQA exam board style syllabus.Incorrect: 0
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Question 1
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Which of the following is a correct safety reason for not storing alkali metals in open water?
Which property makes potassium hydroxide solution (from potassium + water) change the colour of universal indicator to purple/magenta?
Which statement about the trend in density of Group 1 metals going down the group is generally correct?
Which observation would best show that rubidium is more reactive than potassium when each is added to water?
What is the electron configuration of a potassium ion (K+)?
Which explanation correctly explains why potassium is more reactive than lithium?
What is the main reason Group 1 metals form ionic compounds rather than covalent compounds with non-metals?
Which trend describes melting points of Group 1 metals going down the group?
Which sentence best explains why Group 1 elements have similar chemical properties?
Which flame colour is commonly produced by a sodium compound in a flame test?
Which of these is the best explanation for why the outer electron is lost more easily from cesium than from lithium?
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