Structure & Bonding (Triple) quiz Loading... 1. Explain the term ionic bondAn ionic bond is the strong electrostatic attraction between a shared pair of electrons and two nucleiAn ionic bond is the strong electrostatic attraction between similarly charged ionsAn ionic bond is the strong electrostatic attraction between oppositely charged ionsAn ionic bond is the strong magnetic attraction between oppositely charged ionsQuestion 1 of 20 Loading... 2. Why do ionic compounds conduct electricity only when molten or in solution?When solid the ions are arranged regularly. When molten or in solution the ions are arranged irregularlyWhen solid the electrons are held in place. When molten or in solution the electrons are free to moveWhen solid the ions are free to move. When molten or in solution the ions are held in placeWhen solid the ions are held in place. When molten or in solution the ions are free to moveQuestion 2 of 20 Loading... 3. Describe the formation of a covalent bondThe transfer of electrons from one atom to anotherThe electrostatic attraction between positive metal ions and a sea of delocalised electronsThe sharing of a pair of electrons between two nucleiThe sharing of a single electron between two nucleiQuestion 3 of 20 Loading... 4. Describe the bonding in a metalThe strong electrostatic attraction between a regular structure of positive ions and a sea of delocalised electronsThe strong electrostatic attraction between a shared pair of electrons and two nucleiThe strong electrostatic attraction between protons and neutronsThe strong electrostatic attraction between oppositely charged ionsQuestion 4 of 20 Loading... 5. Give the definition of a covalent bondStrong electrostatic attraction between a shared pair of electrons and a nucleusStrong electrostatic attraction between oppositely charged ionsStrong electrostatic attraction between a shared pair of electrons and two nucleiStrong electrostatic attraction between a postive ion and a sea of delocalised positive ionsQuestion 5 of 20 Loading... 6. Explain why metals are malleableMetals have strong covalent bonds which require a lot of energy to breakMetals have delocalised electrons which are free to moveMetals have layers of ions that can slide over each otherMetals have delocalised protons which can moveQuestion 6 of 20 Loading... 7. Alloys contain different sized positive ions. What properties does this give alloys compared to pure metals?Alloys are more ductile than pure metalsAlloys are harder and less malleable than pure metalsAlloys are more magnetic than pure metalsAlloys are harder and more magnetic than pure metalsQuestion 7 of 20 Loading... 8. Explain, in terms of structure and bonding, why sodium chloride has a very high melting pointNaCl has a simple molecular structure with weak intermolecular forces that require little energy to breakNaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to breakNaCl has a simple molecular structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to breakNaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to breakQuestion 8 of 20 Loading... 9. Why do covalent compounds (e.g H₂O) not conduct electricity?There are weak intermolecular forces that require little energy to breakThere are charged particles that are free to moveThere are no charged particles that are free to moveThere is a sea of delocalised electrons that are free to moveQuestion 9 of 20 Loading... 10. Explain why Silica, SiO₂ is a solid with a high melting pointSilica has a giant metallic structure with weak forces of attraction between layersSilica has a giant covalent structure with many strong covalent bonds that need a lot of energy to breakSilica has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcomeSilica has a simple molecular structure with weak intermolecular forces that require little energy to overcomeQuestion 10 of 20 Loading... 11. Explain, in terms of its structure, why graphite can conduct electricity.Graphite has positive ions which can moveGraphite has delocalised electrons which can moveGraphite has delocalised protons which can moveGraphite has layers which can easily slide over each otherQuestion 11 of 20 Loading... 12. Explain why carbon dioxide gas, CO₂, is a gas at room temperatureCarbon dioxide has a giant covalent structure with many weak covalent bonds which require little energy to overcomeCarbon dioxide has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcomeCarbon dioxide has a simple molecular structure with weak intermolecular forces that require little energy to overcomeCarbon dioxide has a giant covalent structure with many strong covalent bonds which require a lot of energy to overcomeQuestion 12 of 20 Loading... 13. State the fomula for the two ions in vanadium (V) oxideV⁵⁺ and O²⁻V²⁺ and O²⁻V⁺ and O⁻There are no ions because it is covalentQuestion 13 of 20 Loading... 14. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of chlorine (Cl₂), how many electrons should be shown in areas 1, 2 and 3?There should be four electrons in each of areas 1, 2 and 3There should be four electrons in area 2 and three in each of areas 1 and 3There should be two electrons in area 2 and six in each of areas 1 and 3There should be two electrons in area 2 and seven in each of areas 1 and 3Question 14 of 20 Loading... 15. State 3 properties that makes aluminium suitable for power cablesDuctile (can be drawn into a wire), bad conductor and low densityDuctile (can be drawn into a wire), good conductor and low densityDuctile (can be drawn into a wire), good conductor and lightDuctile (can be drawn into a wire), bad conductor and lightQuestion 15 of 20 Loading... 16. What is an alloy?An 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 carbonAn 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 hydrogenQuestion 16 of 20 Loading... 17. When can ionic substances conduct electricity?In any stateWhen molten or dissolvedNeverOnly when moltenQuestion 17 of 20 Loading... 18. 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 18 of 20 Loading... 19. Do larger molecules have higher or lower boiling points than smaller molecules?LowerIt depends on which atoms are presentSize doesn\'t affect boiling pointHigherQuestion 19 of 20 Loading... 20. Typically, do covalent substances conduct electricity?Depends on conditions (e.g. pressure, temperature etc.)Depends on the substanceNoYesQuestion 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