C2

• What is a similarity between graphite and diamond?

  Both have a high melting point due to strong covalent bonds.
• Why do graphite and diamond have high melting points?

  They have strong covalent bonds that require a lot of energy to break.
• What are graphite and diamond made of?

  They are made of carbon or allotropes of carbon.
• What type of structure do graphite and diamond have?

  They have a giant covalent structure.
• How many bonds does graphite form?

  Graphite forms 3 bonds.
• What are two common uses of graphite?

  Graphite is used for pencils and lubricants.
• What is the structure of graphite like?

  Graphite has a layered structure.
• Why is graphite considered soft and slippery?

  Because it has weak intermolecular forces that allow layers to slide over each other.
• How does graphite conduct electricity?

  Graphite conducts electricity due to delocalised electrons that carry charge through the structure.
• How many covalent bonds does diamond form?

  Diamond forms 4 covalent bonds.
• What is the physical property of diamond?

  Diamond is hard and rigid due to its giant covalent structure.
• Why doesn't diamond conduct electricity?

  Diamond does not conduct electricity because there are no delocalised electrons to carry charge.
• What is the structure of diamond?

  Diamond has a tetrahedron structure due to the 4 formed bonds.
• Why is diamond used for cutting tools?


  Because its rigid network of carbon atoms makes it very hard and it has a high melting point and not a conductor
• What is an example of a tool that uses diamond for cutting?

  Diamond-tipped glass cutting tools.
• Why is graphite used as a lubricant?

  Because the layers of carbon atoms can slide over each other due to weak intermolecular forces.
• What is a key difference in the electrical conductivity between graphite and diamond?

  Graphite conducts electricity while diamond does not.
• How do the bonding structures of graphite and diamond affect their properties?

  Graphite's 3 bonds allow for layered structure and conductivity, while diamond's 4 bonds create hardness and rigidity.
• What are the three strong chemical bonds that students need to know about?

  Ionic, covalent, and metallic bonds
• What type of atoms does ionic bonding occur between?

  Metal and non-metal atoms
• What happens to electrons during ionic bonding?

  Electrons are transferred from metal atoms to non-metal atoms
• What causes ionic bonding?

  It is caused by oppositely charged ions
• What type of bonding occurs between non-metal and non-metal atoms?

  Covalent bonding
• What is the result of covalent bonding?

  Atoms share pairs of electrons
• What is metallic bonding characterized by?

  Sharing delocalized electrons among metal atoms
• What happens to sodium atoms during ionic bonding?

  Sodium atoms lose electrons and become positively charged ions
• What is the electron configuration of sodium?

  2, 8, 1
• How many protons and electrons does a sodium atom have?

  11 protons and 11 electrons
• What is the electron configuration of chlorine?

  2, 8, 7
• How many protons and electrons does a chlorine atom have?

  17 protons and 17 electrons
• What occurs during a chemical reaction between sodium and chlorine?

  An electron is transferred from sodium to chlorine
• Why do sodium and chlorine atoms transfer electrons?

  To achieve a stable arrangement of electrons
• What is the electron configuration of the sodium ion?

  2, 8
• What is the charge of a sodium ion?

  +1
• What is the electron configuration of the chloride ion?

  2, 8, 8
• What is the charge of a chloride ion?


  • 1
• What type of force attracts sodium and chloride ions?

  Electrostatic force of attraction
• What is the structure of ionic compounds like sodium chloride?

  They are giant lattice structures
• What holds ionic compounds together?

  Strong electrostatic forces of attraction between oppositely charged ions
• What are the properties of ionic compounds regarding melting and boiling points?

  Ionic compounds have high melting and boiling points