6.2 Electronegativity and polarity Flashcards

1
Q

When elements are the same, the bonded electron pair is shared evenly, this changes when the elements are different:

A

The nuclear charges are different
The atoms may be different sizes
The shared pair of electrons may be closer to one nucleus than the other

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2
Q

What is electronegativity

A

The attraction of a bonded atom for the pair of electrons in a covalent bond

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3
Q

What is the Pauling scale used for

A

Comparing the electronegativity of the atoms of different elements

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4
Q

How do the Pauling electronegativity values depend on their positions in the periodic table

A

Across the table, the nuclear charge increases and the atomic radius decreases
Electronegativity increases up the periodic table

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5
Q

What does a large Pauling value indicate

A

That atoms of the element are very electronegative

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6
Q

Which part of the periodic table have the most electronegative atoms

A

The non-metals nitrogen, oxygen, fluorine and chlorine

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7
Q

Which part of the periodic table have the least electronegative atoms

A

The group 1 metals including lithium, sodium and potassium

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8
Q

If the electronegativity difference in large, what happens to the attraction between atoms

A

The bonded atom will have a much greater attraction for the shared pair than the other bonded atom
The more electronegative atom will have gained control of the electrons and the bond will now be ionic rather than covalent

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9
Q

Electronegativity difference of covalent bonds

A

0

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10
Q

Electronegativity difference of polar covalent bonds

A

0 to 1.8

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11
Q

Electronegativity difference of ionic bonds

A

Greater than 1.8

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12
Q

A bond will be non-polar when

A

The bonded electron pair is shared equally between the bonded atoms
The bonded atoms are the same
or
The bonded atoms have the same or similar electronegativity

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13
Q

What is a pure covalent bond

A

When the molecule comes from bonded atoms of the same element

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14
Q

What happens in a polar bond

A

The bonded electron pair is shared unequally between the bonded atoms.

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15
Q

When will a bond be polar

A

When the bonded atoms are different and have different electronegativity values, resulting in a polar covalent bond

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16
Q

Example of a polar bond - hydrogen chloride

A

HCl has atoms of different elements
H has electronegativity 2.1
Cl has electronegativity 3.0
The chlorine atom is MORE electronegative than the hydrogen atom
The chlorine atom has a greater attraction for the bonded pair of electrons than the hydrogen atom, resulting in a polar covalent bond
The H-Cl bond is polarised with a small partial + charge on the H and a small - on the Cl

17
Q

What does 𝛿 mean

A

Lower case delta meaning small

18
Q

What are the partial charges

A

𝛿+
𝛿-

These are much smaller than the full + and - charges

19
Q

What is a permanent dipole

A

A dipole in a polar covalent bond does not change and is called a permanent dipole to distinguish it from an induced dipole

20
Q

Depending on the _____ of a molecule, the dipoles may _____ one another to produce a larger dipole over the whole molecule, or _____ ___ if the dipoles act in opposite directions

A

Shape
Reinforce
Cancel out

21
Q

What charge does the atom with the larger electronegativity value have

A

𝛿-

22
Q

What charge does the atom with the smaller electronegativity value have

A

𝛿+

23
Q

Example of a polar molecule - water

A

The two O-H bonds each have a permanent dipole
The two dipoles act in different directions but do not exactly oppose one another
Overall the oxygen end of the molecule has a 𝛿- charge and the hydrogen end has a 𝛿+ charge

24
Q

Example of a non-polar molecule - carbon dioxide

A

The two C=O bonds each have a permanent dipole
The two dipoles act in opposite directions and exactly oppose one another
Over the whole molecule, the dipoles cancel and the overall dipole is zero

25
Q

What is a dipole

A

A separation in electrical charge so that one atom of a polar covalent bond or one end of a polar molecule has a small positive charge 𝛿+ and the other has a small negative charge 𝛿-

26
Q

What is a dipole-dipole force

A

An attractive force between permanent dipoles in neighbouring polar molecules