Bond polarity Flashcards

1
Q

What is electronegativity ?

A

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

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2
Q

What is the scale of electronegativity ?

A

0.7 to 4

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3
Q

What happens to electronegativity as you go across a period ?

A

Increases across a period

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4
Q

What happens to electronegativity as you go up a a group ?

A

Increases as you go up a group

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5
Q

What group of atoms are electronegative and why ?

A

Group 7 are electron negative atoms because they have high electromagnetivity and can therefore attract electrons towards themselves.

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6
Q

What are atoms with low electronegativity called ?

A

Electropositive atoms.

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7
Q

What factors affect electronegativity ?

A

Shielding
Nuclear charge
Atomic radius

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8
Q

How does shielding affect electronegativity ?

A

The more orbitals the less electronegative charge as there is less attraction between the nuclear charge and the valence electrons

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9
Q

How does nuclear charge affect electronegativity ?

A

The greater the nuclear charge , the more electronegative charge because there is more attraction between the nuclear charge and electrons.

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10
Q

How does atomic radius contribute to electronegativity ?

A

The greater the nuclear charge, the smaller the atomic radius because the nuclear charge pulls some of the electrons in slightly.

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11
Q

Which is the most electropositive atom ?

A

Caesium

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12
Q

Which is the most electronegative atom ?

A

Fluorine

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13
Q

Draw a diagram showing the bond polarity between H-O

A

Notes

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14
Q

What is a polar covalent atom - definition ?

A

The electron distribution between elements with different electronegative charges will be unsymmetrical.

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15
Q

When do non-polar covalent bonds occur ?

A

If the electronegativity of both atoms in a covalent bonds is the same or very similar there will be no partial charge and therefore the bond will be non-polar.

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16
Q

Give examples of non-polar Covalent bonds and show their arrangement.

A

O2

H2

17
Q

What type is bonding has no difference between electronegativity?

A

Non- polar covalent

18
Q

What type of bonding will have a small difference in electronegativity

A

Polar covalent bonds

19
Q

What type of bonds will have a large difference in electronegativity ?

A

Ionic

20
Q

What atoms are always electropositive.

A

Metals

21
Q

What causes metallic structure ?

A

Both atoms are electropositive. This means neither of the atoms have the ability to attract the electrons therefore the electrons delocalised and become free to move