Structure & Bonding (Triple) quiz Loading... 1. Why do ionic substance have high melting and boiling points?There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcomeThere is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcomeThere are weak intermolecular forces, in a simple molecular structure, which require little energy to overcomeThere is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcomeQuestion 1 of 20 Loading... 2. A student has drawn a diagram to show the structure of a metallic solid, but forgotten to label the parts. Which of the following correctly lists those parts?Positive metal ions. Delocalised electrons. Weak intermolecular forces.Positive metal ions. Delocalised negative ions. Giant Structure.Positive metal ions. Delocalised electrons. Giant Structure.Oppositely charged ions in a sea of delocalised electrons. Giant structure.Question 2 of 20 Loading... 3. Explain why nitrogen gas, N₂, is a gas at room temperatureNitrogen has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcomeNitrogen has a giant covalent structure with many weak covalent bonds which require little energy to overcomeNitrogen has a simple molecular structure with weak intermolecular forces that require little energy to overcomeNitrogen has a giant covalent structure with many strong covalent bonds which require a lot of energy to overcomeQuestion 3 of 20 Loading... 4. Describe the formation of a covalent bondThe electrostatic attraction between positive metal ions and a sea of delocalised electronsThe sharing of a single electron between two nucleiThe transfer of electrons from one atom to anotherThe sharing of a pair of electrons between two nucleiQuestion 4 of 20 Loading... 5. Typically, do covalent substances conduct electricity?Depends on conditions (e.g. pressure, temperature etc.)Depends on the substanceNoYesQuestion 5 of 20 Loading... 6. Why are alloys harder than pure metals?Alloys contain different sized positive ions, so there are no layers of ions to slide over each otherAlloys are more magnetic than pure metals so when they are formed the ions are packed closer togetherAlloys have higher melting points because they are mixtures so are harderAlloys often contain carbon which is a very hard elementQuestion 6 of 20 Loading... 7. Describe the structure of metalsA giant random structure of positive metal ions surrounded by a sea of delocalised electronsA simple random structure of positive metal ions surrounded by a sea of delocalised electronsA simple regular structure of positive metal ions surrounded by a sea of delocalised electronsA giant regular structure of positive metal ions surrounded by a sea of delocalised electronsQuestion 7 of 20 Loading... 8. What holds ions together?Ions are held together by a strong electrostatic attraction between the similarly charged ionsIons are held together by a strong electrostatic attraction between the oppositely charged ionsIons are held together by a strong magnetic attraction between the oppositely charged ionsIons are held together by a strong electrostatic attraction between the shared pair of electrons and their nucleiQuestion 8 of 20 Loading... 9. What is needed to complete this diagram to show the ionic bonding in potassium oxide, K₂O ?1) eight electrons around the potassium (any combination of dots and one crosses) 2) A charge of +2 on the oxide and -1 on the potassium 3) A second potassium ion the same as the first1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second potassium ion the same as the first1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second oxide ion the same as the first1) eight electrons around the oxide (six dots and two cross) 2) A charge of +2 on the potassium and -1 on the oxide 3) A second potassium ion the same as the firstQuestion 9 of 20 Loading... 10. Do ionic substances conduct electricity?Only when moltenNot when solid, but they do when either molten or in solutionNo, ionic substances never conduct electricityYes, ionic substances always conduct electricityQuestion 10 of 20 Loading... 11. Do larger molecules have higher or lower boiling points than smaller molecules?It depends on which atoms are presentHigherSize doesn\'t affect boiling pointLowerQuestion 11 of 20 Loading... 12. Give the definition of a covalent bondStrong electrostatic attraction between a shared pair of electrons and a nucleusStrong electrostatic attraction between a shared pair of electrons and two nucleiStrong electrostatic attraction between a postive ion and a sea of delocalised positive ionsStrong electrostatic attraction between oppositely charged ionsQuestion 12 of 20 Loading... 13. Explain, in terms of its structure, why graphite can conduct electricity.Graphite has layers which can easily slide over each otherGraphite has delocalised protons which can moveGraphite has positive ions which can moveGraphite has delocalised electrons which can moveQuestion 13 of 20 Loading... 14. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethane (C₂H₆), how many electrons should be shown in areas 1, 2, 3, 4, 5, 6 and 7?There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also two more on the outside of each hydrogen atomThere should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7There should be two electrons in each of areas 1, 3, 4, 5, 6 and 7, but none in area 2There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also seven more on the outside of each hydrogen atomQuestion 14 of 20 Loading... 15. Why do covalent compounds (e.g H₂O) not conduct electricity?There are no charged particles that are free to moveThere are weak intermolecular forces that require little energy to breakThere are charged particles that are free to moveThere is a sea of delocalised electrons that are free to moveQuestion 15 of 20 Loading... 16. State two properties of aluminium that make it suitable for use in food cansLight and reactiveDuctile and malleableMalleable and low density Light and resists corrosionQuestion 16 of 20 Loading... 17. Suggest why buckminsterfullerene, C₆₀, has a low melting point.Buckminsterfullerene has a giant covalent structure with many strong covalent bonds that need a lot of energy to breakBuckminsterfullerene has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcomeBuckminsterfullerene has a giant metallic structure with weak forces of attraction between layersBuckminsterfullerene has a simple molecular structure with weak intermolecular forces that require little energy to overcomeQuestion 17 of 20 Loading... 18. What does the word malleable mean?Able to carry currentWill break or crack under pressureAble to be drawn into a wireAble to be hammered or pressed into shape without breaking or crackingQuestion 18 of 20 Loading... 19. What is an alloy?An alloy is a mixture of a non-metal and one or more elements, usually other metals or hydrogenAn alloy is a mixture of a metal and one or more elements, usually other metals or hydrogenAn alloy is a mixture of a non-metal and one or more elements, usually other metals or carbonAn alloy is a mixture of a metal and one or more elements, usually other metals or carbonQuestion 19 of 20 Loading... 20. Explain whether solid ionic compounds conduct electricitySolid ionic compounds can conduct electricity because the ions are free to moveSolid ionic compounds sometimes conduct electricity, only when the ions are free to moveSolid ionic compounds cannot conduct electricity because the ions are not free to moveSolid ionic compounds can conduct electricity because there is a sea of delocalised electrons that can moveQuestion 20 of 20 Loading... Related Posts:The entire quiz question bank!The entire quiz question bank (Double only)!Key Calculations quizEquilibria (triple) quizCondensation Polymers quizElectrolysis quiz Hydr0Gen2020-02-16T12:32:52+00:00Categories: Uncategorized|Tags: Quiz, Topic: Structure & Bonding| Share This Story, Choose Your Platform! FacebookTwitterRedditLinkedInTumblrPinterestVkEmail