Bonding Flashcards

1
Q

Define metallic bonding (1)

A
  1. Strong electrostatic attraction between positive ions and delocalised electrons
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2
Q

Define covalent bonding (1)

A
  1. A covalent bond is a shared pair of electrons between two atoms
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3
Q

Name 3 macromolecular structures (3)

A
  1. Silicon
  2. Carbon
  3. Silicon dioxide
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4
Q

Define ionic bonding (1)

A
  1. An ionic bond is the strong electrostatic attraction between oppositely charged ions
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5
Q

Define a co-ordinate bond (1)

A
  1. Shared pair of electrons where both electrons come from the same atom
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6
Q

Define the term electronegativity (2)

A
  1. The power of an atom to attract a pair of electrons
  2. In a covalent bond
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7
Q

When does hydrogen bonding occur? (1)

A

Between hydrogen covalently bonded to nitrogen/oxygen/fluorine and lone pair on nitrogen/oxygen/fluorine

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8
Q

Explain why a fluoride ion is larger than a sodium ion. (2)

A
  1. Fluoride ion has fewer protons
  2. Weaker attraction between nucleus and (outer) electrons
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9
Q

Explain, in terms of structure and bonding, why the melting point of sodium fluoride is high. (2)

A
  1. (Electrostatic) forces of attraction between
    oppositely charged ions/Na+ and F–
  2. Lots of energy required to overcome forces
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10
Q

How does hydrogen bonding arise? (2)

A
  1. Large difference in electronegativity between hydrogen and N/O/F which creates a dipole in the H-N/O/F bond
  2. partially positive H on one molecule is attracted to lone pair of N/O/F on another molecule
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11
Q

When do permanent dipole dipole forces arise? (1)

A
  1. Between polar molecules
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12
Q

How do permanent dipole dipole forces arise? (3)

A
  1. Differences in electronegativity lead to polar bonds
  2. In non-symmetrical molecules, the individual bonds don’t cancel out
  3. Partially positive H on one molecule attracts partially negative on another molecule
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13
Q

When do induced dipole dipole forces occur? (1)

A
  1. Between all molecules and atoms
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14
Q

How do induced dipole dipole forces (Van der Waals) arise? (5)

A
  1. Random movement of electrons, leading to
  2. Uneven distribution of electrons, creating a
  3. Temporary dipole in one molecule
  4. Induces a dipole in another molecule
  5. Dipoles attract
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