Polarity / Electronegativity + Intermolecular Forces + Hydrogen Bonding Flashcards

1
Q

Define Electronegativity

A

The ability of an atom to attract the bonding pair of electrons in a covalent bond

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2
Q

How does London Dispersion Forces Arise

A

-Constant random movement of electrons
-Uneven distribution of electrons
-Creates an Instantenous Dipoles
-Which causes a induced dipole in neighbouring molecules

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3
Q

Why does Br-Br have a higher melting point / boiling point Cl-Cl

A

The higher number of electrons
The stronger London dispersion forces
Which require more energy to overcome

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4
Q

Name 2 Anomalous Properties of Water

A

Ice is less dense than Water
-In a solid state H2O Molecules are held apart by hydrogen bonds
-Ice has an open lattice

Water has a relatively high MP and BP
-More energy is required to overcome the bonds

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5
Q

What is the description of a Polar Molecule

A

-X is more electronegative ( delta negative ) than x ( delta positive )
- X is not symmetrical
-The dipoles in the don’t cancel
-

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6
Q

What is the description of a Non-Polar Molecule

A

-X is more electronegative ( delta negative ) than x ( delta positive
- X is symmetrical
-The dipoles in the molecule cancel

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7
Q
A
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