Gr 10 Physical Sciences Ch 4: Metallic Bonding
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Questions and Answers

What is the main component of the 'sea' in metallic bonding?

  • Neutrons
  • Valence electrons
  • Positive ions
  • Delocalized electrons (correct)

What is the purpose of the colored balls in the model-building activity?

  • To represent delocalized electrons
  • To represent the electrostatic forces
  • To represent positive metal ions (correct)
  • To represent the crystal lattice

What is the arrangement of atoms in a Body-Centered Cubic (BCC) crystal lattice?

  • Atoms are at the corners of a cube with atoms at the centers of each face of the cube
  • Atoms are at the corners of a cube with one atom at the center of the cube (correct)
  • Atoms are packed closely together in a hexagonal arrangement
  • Atoms are arranged in a random pattern

What is the name of the crystal lattice structure where atoms are packed closely together in a hexagonal arrangement?

<p>Hexagonal Close-Packed (HCP) (D)</p> Signup and view all the answers

What is the role of the sticks in the model-building activity?

<p>To represent the delocalized electrons (C)</p> Signup and view all the answers

What is the purpose of the model-building activity?

<p>To gain a deeper understanding of metallic bonding (C)</p> Signup and view all the answers

What type of electrons are lost by metal atoms to form positive ions?

<p>Valence electrons (D)</p> Signup and view all the answers

What is the arrangement of atoms in a Face-Centered Cubic (FCC) crystal lattice?

<p>Atoms are at the corners of a cube with atoms at the centers of each face of the cube (C)</p> Signup and view all the answers

What is the main characteristic of metallic bonds?

<p>Electrons are delocalized and free to move throughout the structure (B)</p> Signup and view all the answers

What is the definition of a metallic bond?

<p>The electrostatic attraction between positively charged atomic nuclei and the delocalized electrons in the metal (D)</p> Signup and view all the answers

What is the reason behind the high melting and boiling points of metals?

<p>The strong electrostatic attraction between the positive nuclei and the sea of electrons (A)</p> Signup and view all the answers

Why are metals good conductors of electricity?

<p>Because the electrons are free to move throughout the structure (A)</p> Signup and view all the answers

What is the reason behind the shininess of metals?

<p>The absorption and re-emission of light by the delocalized electrons (D)</p> Signup and view all the answers

Why are metals malleable and ductile?

<p>Because the atoms can slide past each other without breaking the metallic bond (B)</p> Signup and view all the answers

What is a characteristic of metals due to the densely packed positive nuclei?

<p>High thermal conductivity (D)</p> Signup and view all the answers

What is the term for the delocalized electrons in a metal?

<p>Sea of electrons (B)</p> Signup and view all the answers

What is the primary force that holds the metal ions together in a metallic bond?

<p>Electrostatic forces (D)</p> Signup and view all the answers

What is the purpose of the model-building activity in understanding metallic bonding?

<p>To visualize the arrangement of delocalized electrons (C)</p> Signup and view all the answers

What is a common feature of the different crystal lattice structures found in metals?

<p>They all have a repeating pattern of atoms (C)</p> Signup and view all the answers

What is a result of the delocalized electrons in a metal?

<p>The metal becomes more flexible and able to be shaped (A)</p> Signup and view all the answers

What is a characteristic of the 'sea' of delocalized electrons in a metal?

<p>It is free to move throughout the entire structure (A)</p> Signup and view all the answers

What is the advantage of exploring different crystal lattice structures in metals?

<p>It provides insight into the behavior of metals under various conditions (D)</p> Signup and view all the answers

What is the arrangement of metal ions in a metal?

<p>Regular and repeating (A)</p> Signup and view all the answers

What is a consequence of the electrostatic forces between the metal ions and delocalized electrons?

<p>The metal maintains its structure while being flexible (A)</p> Signup and view all the answers

What is the primary reason for the electrical conductivity of metals?

<p>The delocalized electrons that can carry electric current (D)</p> Signup and view all the answers

What is the main characteristic of the metallic bond that gives metals their distinctive properties?

<p>The strong electrostatic attraction between the nuclei and electrons (D)</p> Signup and view all the answers

What is the reason behind the high thermal conductivity of metals?

<p>The densely packed positive nuclei that can transfer kinetic energy (B)</p> Signup and view all the answers

What is the reason behind the malleability and ductility of metals?

<p>The ability of atoms to slide past each other without breaking the metallic bond (D)</p> Signup and view all the answers

What is the characteristic of metals that is responsible for their shininess?

<p>The ability of electrons to absorb and re-emit light (B)</p> Signup and view all the answers

What is the primary reason for the high density of metals?

<p>The densely packed positive nuclei (B)</p> Signup and view all the answers

What is the result of the strong electrostatic attraction between the positively charged nuclei and the negatively charged delocalized electrons in metals?

<p>The high melting and boiling points of metals (D)</p> Signup and view all the answers

What is the characteristic of metallic bonding that distinguishes it from covalent and ionic bonds?

<p>The delocalization of valence electrons (B)</p> Signup and view all the answers

What is the primary reason for the flexibility of metals?

<p>The ability of delocalized electrons to move freely throughout the entire structure (C)</p> Signup and view all the answers

Which of the following is a characteristic of the crystal lattice structure of metals?

<p>The arrangement of positive ions in a regular, repeating pattern (A)</p> Signup and view all the answers

What is the primary reason for the ability of metals to maintain their structure?

<p>The electrostatic forces between the metal ions and delocalized electrons (C)</p> Signup and view all the answers

What is the result of the delocalized electrons in a metal undergoing a physical change?

<p>The metal's crystal lattice structure changes (C)</p> Signup and view all the answers

What is the primary advantage of exploring different crystal lattice structures in metals?

<p>To gain further insight into the properties and behaviors of metals under various conditions (A)</p> Signup and view all the answers

What is the primary characteristic of the 'sea' of delocalized electrons in a metal?

<p>It is a dynamic structure that allows for free movement (C)</p> Signup and view all the answers

What is the primary reason for the high melting and boiling points of metals?

<p>The strong electrostatic attraction between the positively charged nuclei and the negatively charged delocalized electrons (B)</p> Signup and view all the answers

What is the primary characteristic of metallic bonds that gives metals their distinctive properties?

<p>The electrostatic forces between the metal ions and delocalized electrons (C)</p> Signup and view all the answers

What is the primary reason for the high melting and boiling points of metals?

<p>The strong electrostatic attraction between the positively charged nuclei and the negatively charged delocalized electrons (B)</p> Signup and view all the answers

What is the characteristic of metals that allows them to be drawn into wires?

<p>Malleability and ductility (D)</p> Signup and view all the answers

What is the result of the delocalization of valence electrons in metals?

<p>The creation of a 'sea of electrons' (C)</p> Signup and view all the answers

What is the primary force that holds the metal ions together in a metallic bond?

<p>Electrostatic attraction (B)</p> Signup and view all the answers

What is the characteristic of metals that is responsible for their ability to conduct electricity?

<p>The delocalization of valence electrons (D)</p> Signup and view all the answers

What is the characteristic of metals that allows them to absorb and re-emit light?

<p>The delocalization of valence electrons (D)</p> Signup and view all the answers

What is the result of the densely packed positive nuclei in metals?

<p>The increase in thermal conductivity of metals (B)</p> Signup and view all the answers

What is the primary characteristic of metallic bonds that distinguishes them from covalent and ionic bonds?

<p>The delocalization of valence electrons (D)</p> Signup and view all the answers

What is the primary function of the delocalized electrons in a metal?

<p>To act as a glue that holds the positively charged ions together (D)</p> Signup and view all the answers

What is the main advantage of exploring different crystal lattice structures in metals?

<p>To gain a deeper understanding of the unique properties of metals (A)</p> Signup and view all the answers

What is the result of the electrostatic forces between the metal ions and delocalized electrons in a metal?

<p>The metal ions are held together, allowing the metal to maintain its structure (D)</p> Signup and view all the answers

What is the characteristic of metals that arises from the delocalized electrons?

<p>Flexibility and ability to be shaped (B)</p> Signup and view all the answers

What is the benefit of using a model-building activity to understand metallic bonding?

<p>It provides a visual representation of the metallic bond, aiding understanding (C)</p> Signup and view all the answers

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