1.8 Metals and non-metals

• In metallic bonding, the valence electrons are delocalized
• Metallic bonding is different from covalent or ionic
• Non-metals have a dull appearance because they do not reflect light.


  True
• The lustrous appearance of metals is a result of light being reflected by their delocalized electrons
• Delocalized electrons in metals allow for high electrical and thermal conductivity.


  True
• What is a unique property of metallic bonds that allows them to be easily distorted without breaking?

  Delocalized electrons
• Which property of metals allows them to be hammered into thin sheets without breaking?

  Malleability
• Why are metals good conductors of heat and electricity?

  Delocalized electrons
• Arrange the properties of metals and non-metals based on their increasing value:

  1️⃣ Low electrical conductivity

  2️⃣ High electrical conductivity

  3️⃣ Brittle ||| Malleable

  4️⃣ Dull appearance ||| Lustrous appearance
• Non-metals are primarily located on the right side of the periodic table.
• What type of bonding is unique to metals and involves delocalized valence electrons?

  Metallic bonding
• What gives metals their lustrous appearance?

  Delocalized electrons
• Non-metals are brittle because their bonds cannot be easily distorted
• The lustrous appearance of metals is due to the reflection of light by delocalized electrons
• Metallic bonding is found in metals, where valence electrons are delocalized
• What causes the lustrous appearance of metals?

  Delocalized electrons
• Match the property with the correct type of material:

  Malleable ↔️ Metals

  Brittle ↔️ Non-metals
• What type of bonding is found in non-metals?

  Covalent or ionic
• The reactivity of metals increases as you move down a group in the periodic table.


  True
• Match the element with its type:

  Sodium ↔️ Metal

  Oxygen ↔️ Non-metal
• Non-metals tend to be reduced in chemical reactions.


  True
• The lustrous appearance of metals is due to delocalized electrons reflecting light.

  True
• Non-metals are brittle and lack malleability or ductility
• Malleability allows metals to be shaped into wires without breaking.

  False
• Metals are malleable, whereas non-metals are brittle
• The high electrical conductivity of metals is due to the movement of delocalized electrons.


  True
• Metals are generally good conductors of electricity and heat.

  True
• Match the property of metals with its explanation:

  High electrical conductivity ↔️ Delocalized electrons

  Malleability ↔️ Distortion without breaking

  Lustrous appearance ↔️ Reflection of light
• The lustrous appearance of metals is due to the reflection of light by delocalized electrons
• What are the three categories of elements on the periodic table based on their properties?

  Metals, non-metals, metalloids
• Arrange the groups on the periodic table from left to right based on their increasing non-metallic properties:

  1️⃣ Metals

  2️⃣ Metalloids

  3️⃣ Non-metals
• Delocalized electrons in metals allow for the easy movement of charge and heat.


  True
• Why do non-metals have low electrical conductivity?

  Lack of delocalized electrons
• What allows metals to have high thermal conductivity?

  Delocalized electrons
• What is a property that non-metals have but metals do not?

  Brittleness
• Metals are malleable because their metallic bonds can be distorted without breaking.

  True
• Arrange the following properties of metals in order from most to least characteristic:

  1️⃣ High electrical conductivity

  2️⃣ High thermal conductivity

  3️⃣ Malleability

  4️⃣ Ductility

  5️⃣ Lustrous appearance
• Non-metals have a dull appearance.


  True
• Why are metals more reactive than non-metals?

  Lose valence electrons
• What is the tendency of metals in terms of valence electrons?

  Lose valence electrons