Physical - Electronegativity Flashcards

1
Q

Electronegativity

A

= the power of an atom to attract a pair of electrons in a covalent bond

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2
Q

Two elements that have similar electronegativity

A

will form a covalent
bond

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3
Q

Two elements that have very different electronegativity

A

will form an ionic bond.

One atom attracts the pair of electrons so much that they gain the
electrons to form a negative ion.
* The other atom has lost electrons and forms a positive ion

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4
Q

Are metals or non metals more electronegative

A

non
metals are more
electronegative
than metals

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5
Q

There are three factors affecting electronegativity:

A

-Nuclear charge
* Shielding
* Atomic radius

Shielding outweighs all

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6
Q

Nuclear charge

A

The more protons the element has, the greater the nuclear charge, the
stronger the attraction between the nucleus and the bonding pair of
electrons.

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7
Q

Shielding

A

The nucleus attracts the electrons however electrons repel each other.

This means full electron shells shield the
bonding pair of electrons from the attraction of nucleus.

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8
Q

The more electron shells,

A

the greater the
shielding effect. This means there is a weaker
attraction between the nucleus and the pair of
electrons in the covalent bond i.e. less
electronegative

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9
Q

Atomic radius

A

The further away the shared pair of electrons are from the nucleus the more weakly they are attracted
to the nucleus and therefore less electronegative

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10
Q

What factors might affect atomic radius?
*

A

Nuclear charge – the higher the nuclear charge the stronger the attraction between
nucleus and outer shell electrons therefore they are held closer
* Shielding – the more shielding there is the weaker the attraction between the nucleus
and outer shell electrons therefore they are held further away

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11
Q

Explain why atomic radius decreases across a period

A
  • Outer electrons are in same
    shell
  • There is the same amount of
    shielding
  • More protons in nucleus
  • So stronger attraction
    between nucleus and outer
    shell electrons
  • So outer shell electrons pulled
    closer to nucleus
  • Atomic radius decreases
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12
Q

The atomic radius increases down a group.

A
  • Outer electrons are in a shell
    further away from the nucleus
  • More shielding
  • So weaker attraction between
    nucleus and outer shell
    electrons
  • The outershell electrons move
    further away from the nucleus
  • Atomic radius increase
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13
Q

Electronegativity increases
across a period

A
  • Atomic radius decreases
  • Nuclear charge increases
  • Same shielding
  • ∴ Greater attraction between
    nucleus and bonding pair of
    electro
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14
Q

Electronegativity decreases
down the group
*

A

Atomic radius increases
* Nuclear charge increase
* More shielding
* ∴ Less attraction between nucleus
and bonding pair of electrons

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