Bonding Flashcards
Define metallic bonding (1)
- Strong electrostatic attraction between positive ions and delocalised electrons
Define covalent bonding (1)
- A covalent bond is a shared pair of electrons between two atoms
Name 3 macromolecular structures (3)
- Silicon
- Carbon
- Silicon dioxide
Define ionic bonding (1)
- An ionic bond is the strong electrostatic attraction between oppositely charged ions
Define a co-ordinate bond (1)
- Shared pair of electrons where both electrons come from the same atom
Define the term electronegativity (2)
- The power of an atom to attract a pair of electrons
- In a covalent bond
When does hydrogen bonding occur? (1)
Between hydrogen covalently bonded to nitrogen/oxygen/fluorine and lone pair on nitrogen/oxygen/fluorine
Explain why a fluoride ion is larger than a sodium ion. (2)
- Fluoride ion has fewer protons
- Weaker attraction between nucleus and (outer) electrons
Explain, in terms of structure and bonding, why the melting point of sodium fluoride is high. (2)
- (Electrostatic) forces of attraction between
oppositely charged ions/Na+ and F– - Lots of energy required to overcome forces
How does hydrogen bonding arise? (2)
- Large difference in electronegativity between hydrogen and N/O/F which creates a dipole in the H-N/O/F bond
- partially positive H on one molecule is attracted to lone pair of N/O/F on another molecule
When do permanent dipole dipole forces arise? (1)
- Between polar molecules
How do permanent dipole dipole forces arise? (3)
- Differences in electronegativity lead to polar bonds
- In non-symmetrical molecules, the individual bonds don’t cancel out
- Partially positive H on one molecule attracts partially negative on another molecule
When do induced dipole dipole forces occur? (1)
- Between all molecules and atoms
How do induced dipole dipole forces (Van der Waals) arise? (5)
- Random movement of electrons, leading to
- Uneven distribution of electrons, creating a
- Temporary dipole in one molecule
- Induces a dipole in another molecule
- Dipoles attract