| The type of chemical bonding that occurs between atoms of metal elements, characterized by the sharing of delocalized electrons. | Metallic Bonding |
| What joins the atoms of metal elements together? | Metallic bonding. |
| A three-dimensional arrangement of atoms or ions that extends throughout a material. | Giant Structure |
| How are the atoms arranged in metals? | Metals have giant structures of atoms arranged in a regular pattern. |
| Electrons that are not associated with any specific atom and are free to move throughout the structure of a material. | Delocalised Electrons |
| What characterizes the electrons in the outer shells of metal atoms? | They are delocalised. |
| Atoms of metal elements that have lost electrons and therefore carry a positive charge. | Positive Metal Ions |
| What happens to the metal atoms' outer electrons in metallic bonding? | They become delocalised, leading to the formation of positive metal ions. |
| Forces of attraction or repulsion between electrically charged particles. | Electrostatic Forces |
| What is responsible for the strong bonding in metallic bonds? | The strong electrostatic forces of attraction between the positive metal ions and the delocalised electrons. |
| The robustness and durability of the bonding between metal atoms in a metallic structure. | Strength of Metallic Bonds |
| How would you describe the strength of metallic bonds? | Metallic bonds are very strong due to the electrostatic forces between metal ions and delocalised electrons. |
| A structure in which metal atoms are arranged in a giant lattice with strong metallic bonding between them. | Metallic Structure |
| What type of structure do metals typically have? | Metals have giant structures of atoms with strong metallic bonding. |
| The temperatures at which substances change from solid to liquid (melting) and from liquid to gas (boiling) are relatively high. | High Melting and Boiling Points |
| How do metallic bonds affect the melting and boiling points of metals? | Metallic bonding contributes to high melting and boiling points in metals. |
| The ability of a material to conduct an electric current. | Electrical Conductivity |
| Why are metals good conductors of electricity? | Metals are good conductors of electricity because the delocalised electrons in their structure can move to carry an electric charge. |
| The ability of a material to transfer heat energy. | Thermal Conductivity |
| How do the delocalised electrons in metals affect their thermal conductivity? | The delocalised electrons in metals can transfer thermal energy, making metals good conductors of heat. |
| The property of a material that allows it to be easily shaped or formed by hammering, rolling, or pressing. | Malleability |
| Why are metals malleable? | Metals are malleable because their atoms are arranged in layers that can slide over each other fairly easily. |
| A metal that contains only one type of metal atom. | Pure Metal |
| What is a pure metal? | A pure metal contains only 1 type of metal atom. |
| The organization of metal atoms in a structure where they are stacked in planes or layers. | Layered Arrangement |
| How are metal atoms arranged in a pure metal? | Metal atoms in a pure metal are arranged in layers. |
| The ability of layers of metal atoms to move or slide past each other. | Sliding Layers |
| Why can metals be shaped easily? | Metals can be shaped easily because their layers can slide over each other, allowing them to be bent, hammered, rolled into sheets, or stretched into wires. |
| Elements characterized by properties such as shininess, high melting points, high densities, and good electrical conductivity. | Metals |
| What are some common properties of metals? | Metals tend to be shiny solids with high melting points and high densities, and they are good conductors of electricity. |
| Elements characterized by properties such as low boiling points and poor electrical conductivity. | Non-metals |
| What are some common properties of non-metals? | Non-metals tend to have low boiling points and to be poor conductors of electricity. |
| Broad guidelines or principles that describe typical characteristics or behaviors. | General Rules |
| What do general rules tell us about the properties of metals and non-metals? | They provide guidelines indicating that metals have specific characteristics, while non-metals exhibit different properties. |
| Cases or instances that deviate from the norm or general rule. | Exceptions |
| Can you provide examples of exceptions to the properties of metals and non-metals? | Mercury is a metal that's a liquid at room temperature, and graphite, a form of carbon, is a non-metal but is a good conductor of electricity. |
| The ability of a material to allow the flow of electric current. | Electrical Conductivity |
| How do the properties of graphite challenge the typical characteristics of non-metals? | Graphite, despite being a non-metal, exhibits good electrical conductivity, which is uncommon among non-metals. |
