1) What charge do electrons have? a) -1 b) +1 c) 0 d) +2 2) What charge will an ion of lithium take? a) +1 b) -1 c) +2 d) 0 3) What charge will an ion of beryllium take? a) +2 b) +1 c) -1 d) 0 4) What charge will an ion of barium take? a) +2 b) +1 c) -1 d) 0 5) What charge will an ion of fluorine take? a) 1+ b) 2+ c) 1- d) 1-  6) If something has gained electrons, what charge will it have? a) Positive (because they have lost a negative!) b) Negative c) Neutral d) Variable 7) If something has lost electrons, what charge will it have? a) Positive b) Negative (because they have lost a positive!) c) Neutral d) Variable 8) What charge will an ion of oxygen take? a) 2+ b) 1+ c) 1- d) 2-  9) What charge will an ion of Selenium take? a) 2+ b) 1+ c) 1- d) 2-  10) Explain in terms of electrons what occurs when lithium bonds with chlorine  a) One electron transferred from lithium to chlorine b) One electron transferred from chlorine to lithium c) One electron shared between lithium and chlorine d) No electrons are transferred or shared 11) Why do atoms transfer electrons in ionic bonding? a) So that they can have full outer shells b) To increase their atomic radius c) To decrease their atomic number d) To form covalent bonds 12) Explain in terms of electrons what occurs when lithium bonds with fluorine  a) One electron transferred from lithium to fluorine b) One electron transferred from fluorine to lithium c) One electron shared between lithium and fluorine d) No electrons are transferred or shared 13) Explain in terms of electrons what occurs when magnesium bonds with oxygen a) Two electrons transferred from magnesium to oxygen b) Two electrons transferred from oxygen to magnesium c) Two electrons shared between magnesium and oxygen d) No electrons are transferred or shared 14) Explain in terms of electrons what occurs when beryllium bonds with oxygen (3 marks) a) Two electrons transferred from beryllium to oxygen  b) Two electrons transferred from oxygen to beryllium c) Two electrons shared between beryllium and oxygen d) No electrons are transferred or shared 15) Explain in terms of electrons what occurs when magnesium bonds with chlorine a) One electron transferred from magnesium to two different chlorine atoms b) One electron transferred from chlorine to magnesium c) One electron shared between magnesium and two chlorine atoms d) No electrons are transferred or shared 16) Explain in terms of electrons what occurs when sodium bonds with oxygen  a) Two electrons transferred to an oxygen atom from two different sodium atoms b) Two electrons transferred from oxygen to sodium c) Two electrons shared between sodium and oxygen d) No electrons are transferred or shared 17) Why do sodium ions and chlorine ions form an ionic bond?  a) They have similar electronegativity values b) They both need to gain electrons c) They both need to lose electrons d) There is an electrostatic force of attraction between oppositely charged ions 18) Why don't sulphur ions and oxygen ions form ionic bonds with each other? a) Both have positive charges so would repel b) They have similar electronegativity values c) Both have negative charges so would repel d) They do not need to gain or lose electrons 19) What is the name for a substance made of billions of oppositely charged ions joined together? a) Giant ionic lattice b) Ionic superstructure c) Strong ionic lattice d) Huge 3D network of ions 20) Define giant ionic lattice a) Strong ionic arrangement b) A huge 3D network of ions c) Stable ionic structure d) Massive ionic framework 21) State the melting points of ionic substances a) Moderate b) High c) Variable d) Low 22) Explain why ionic substances have high melting points. a) Weak bonds between ions are hard to break b) Electrostatic forces repel ions at high temperatures c) Strong bonds between oppositely charged ions are hard to break d) Ions have low kinetic energy at high temperatures 23) Will NaCl(s) conduct electricity? a) Yes b) No c) Only at high temperatures d) Depends on the crystal structure 24) Will NaCl (aq) conduct electricity? a) No b) Yes c) Only in the solid state d) Depends on the concentration of the solution 25) Will NaCl (l) conduct electricity? a) Yes b) No c) Only at low temperatures d) It only conducts heat 26) What does molten mean? a) Solidified b) Melted c) Dissolved in water d) Highly reactive 27) Explain why ionic compounds do not conduct electricity when solid  a) Ions are highly reactive in the solid state b) Ions lose mobility at low temperatures c) The crystal lattice structure prevents ion movement d) Because the ions are not free to move 28) Explain why ionic compounds conduct electricity in solution  a) Ions gain kinetic energy in solution b) Water acts as a conductor for ions c) Ions become more reactive in solution d) Because the ions are free to move 29) Explain why ionic compounds conduct electricity when molten  a) Ions gain energy when heated b) The molten state enhances ion mobility c) Ions form stronger bonds in the molten state d) Because the ions are free to move 30) What does soluble mean? a) Evaporates quickly b) Reacts with oxygen c) Dissolves in water d) Forms a solid precipitate 31) What does insoluble mean? a) Evaporates slowly b) Reacts with acids c) Dissolves in water d) Does not dissolve in water 32) Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity? a) Dissolve it in water b) Heat it to a high temperature c) Melt it d) Mix it with an acid 33) Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is  a) Heat it to a high temperature b) Dissolve it in water because this does not require high temperatures  c) Convert it to a gas d) Add a catalyst to the solid state 34) Explain why chlorine and fluorine form covalent bonds a) They both have a positive charge b) They are both metals c) They are both non-metals d) They have opposite charges 35) Complete the sentence: In covalent bonds, electrons are _______________________ a) Transferred b) Lost c) Gained d) Shared 36) In ionic bonds, electrons are ___________________ a) Transferred b) Shared c) Lost d) Gained 37) What is the name given to the structure of diamond, graphite and silicon dioxide? a) Giant ionic b) Metallic c) Simple molecular d) Giant covalent 38) How many bonds does each carbon have in diamond? a) 1 b) 2 c) 3 d) 4 39) Explain why diamond has a high melting point  a) It has weak intermolecular forces b) It is a simple molecular substance c) It has a giant structure, and strong covalent bonds between the atoms that require a lot of energy to break d) It conducts electricity 40) Explain why most giant covalent substances do not conduct electricity (3 marks) a) They have free-moving ions b) They have a low density c) There are no electrons/ions/charged particles that are free to move d) The atoms are not held together by strong forces 41) Explain why graphite conducts electricity  a) It has a high melting point b) It has free-moving protons c) It has delocalized electrons between the layers that can move through the graphite d) It has a low density 42) Making full reference to structure and bonding in graphite, explain how it conducts electricity a) Each carbon has 1 bond, and 2 electrons are delocalized, free to carry charge through the graphite b) Each carbon has 2 bonds, and 1 electron is delocalized, free to carry charge through the graphite c) Each carbon has 3 bonds, and 1 electron is delocalized, free to carry charge through the graphite  d) Each carbon has 4 bonds, and 2 electrons are delocalized, free to carry charge through the graphite 43) Explain why graphite can act as a lubricant a) It has a high density b) It has strong intermolecular forces c) It has weak forces between layers that are free to slide over each other d) It has a high melting point 44) What is graphene? a) A three-dimensional network of carbon atoms b) One layer of graphite c) A metal oxide d) A giant ionic structure 45) What is a fullerene? a) A substance made of metal atoms arranged in a cage b) A substance made of carbon and hydrogen atoms c) A substance made of carbon atoms arranged in a cage d) A type of ionic crystal 46) What type of substance are methane and water? a) Simple molecular (or simple molecules) b) Metallic c) Ionic d) Giant covalent 47) What is a molecule? a) A group of atoms with a net positive charge b) A group of atoms chemically bonded together c) A group of atoms with a net negative charge d) A group of atoms with no charge 48) Describe the structure of simple covalent molecules a) Weak covalent bonds between atoms b) Strong forces holding the molecules together c) Strong ionic bonds between atoms d) Strong covalent bonds between atoms, weak forces holding the molecules together  49) What are intermolecular forces? a) Strong forces between ions within a crystal b) Weak forces between protons within a nucleus c) Strong forces between atoms within a molecule d) Weak forces between molecules that hold them together 50) Explain why methane has a low melting point a) It is a simple molecular substance with weak forces between the molecules (which are easy to break) b) It has strong intermolecular forces c) It is a giant covalent substance d) It has a high density 51) What is a polymer? a) A substance made of metal atoms b) A type of ionic crystal c) A substance made of carbon and hydrogen atoms d) Millions of small molecules joined together in a chain to form a large molecule

3/4 Structure and Bonding Quiz (IONIC AND COVALENT)

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