Electronegativity Flashcards
Electronegativity
The ability of an atom to attract a pair of electrons in a covalent bond
Explain trend shown in electronegativity across period 3
Nuclear charge ⬆️
Shielding stays the same
Atomic radius ⬇️
Nuclear attraction ⬆️
Electronegativity ⬆️
What elements in period 3 are giant metallic
Na, Mg, Al
What elements are giant covalent in period 3
Si
What elements are simple molecular structures across period 3
P, S, Cl, Ar
Explain melting & boiling point in first 3 elements across period 3
More delocalised electrons
More charge on cations
Stronger electrostatic attraction between them
Needs more energy to overcome them
Why is the melting point of element 4 so high
It has lots of covalent bonds which require more energy to break
What forces determine the melting point of molecular elements
Intermolecular forces = London forces
Molecular formulae for P4, S8, Cl2, Ar
And explain the pattern
60e-
128e-
34e-
18e-
The more electrons you have, the stronger London forces so more dipoles will occur
