Atomic Structure and Bonding

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What is the reason behind metals being able to be squashed and stretched without breaking?

Delocalised electrons, which allows the atoms to roll over one another.

How do delocalised electrons contribute to metals being good electrical conductors?

Delocalised electrons act as mobile charge carriers.

What is the primary difference between network covalent bonds and molecular covalent bonds?

Network covalent bonds have high melting/boiling points due to the arrangement of atoms in a 3D lattice structure.

Why are network covalent bonds typically hard and brittle?

The arrangement of atoms in a 3D lattice structure results in strong electrostatic forces between atoms, making it difficult to break the bonds. Signup and view all the answers

What is the reason behind molecular covalent bonds having low melting/boiling points?

Weak intermolecular forces between atoms require minimal energy to overcome and break the bonds. Signup and view all the answers

Why do network covalent bonds not conduct electricity?

There are no free moving electrons in network covalent bonds, making them unable to conduct electricity. Signup and view all the answers

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

The strong electrostatic forces between cations and anions in a 3D lattice structure, which require a lot of energy to overcome. Signup and view all the answers

Why do metals tend to lose their valence electrons to form positive ions?

Because metals have low ionization energy and low electronegativity, making it easier for them to lose electrons. Signup and view all the answers

What is the role of electrostatic forces in the formation of ionic bonds?

Electrostatic forces of attraction between cations and anions result in the formation of ionic bonds. Signup and view all the answers

Why do ionic compounds typically form a 3D crystalline lattice structure?

Because of the strong electrostatic forces between cations and anions, which arrange them in a repeating pattern. Signup and view all the answers

What is the key difference between the properties of metals and non-metals that leads to the formation of ionic bonds?

Metals have low ionization energy and low electronegativity, while non-metals have high ionization energy and high electronegativity. Signup and view all the answers

Why do ionic compounds not conduct electricity?

Because they do not have delocalized electrons to conduct electricity and act as mobile charge carriers. Signup and view all the answers

What is the primary reason for the high melting and boiling points of metals, according to the electrostatic attraction model of metallic bonding?

The high melting and boiling points of metals are due to the closely packed arrangement of cations in a lattice, requiring high amounts of energy to overcome and break the bonds. Signup and view all the answers

How do the low ionisation energy and low electronegativity of metals contribute to their physical properties?

The low ionisation energy and low electronegativity of metals allow them to easily lose electrons and form cations, resulting in a 'sea of electrons' that enables their high melting and boiling points, as well as their malleability and ductility. Signup and view all the answers

What is the main difference between ionic and covalent bonds in terms of the type of attraction involved?

Ionic bonds involve the electrostatic attraction between oppositely charged ions, whereas covalent bonds involve the sharing of electrons between atoms. Signup and view all the answers

How do metallic bonds differ from ionic and covalent bonds in terms of the arrangement of electrons?

Metallic bonds involve a 'sea of electrons' surrounding the positive ions, whereas ionic bonds involve the transfer of electrons and covalent bonds involve the sharing of electrons. Signup and view all the answers

What is the significance of the lattice structure in determining the physical properties of metals?

The lattice structure of metals, with closely packed cations surrounded by delocalised electrons, is responsible for their high melting and boiling points, as well as their malleability and ductility. Signup and view all the answers

How do the delocalised electrons in metallic bonds contribute to the physical properties of metals?

The delocalised electrons in metallic bonds allow for the easy flow of electrons, enabling the malleability and ductility of metals, as well as their high melting and boiling points. Signup and view all the answers