electronegativity Flashcards

1
Q

define electronegativity

A

a measure of the tendency of an atom to attract a bonding pair of electrons in a covalent bond

GREATER ELECTRONEGATIVITY = MORE IT ATTRACT ELECTRONS TO IT

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2
Q

what are the 3 factors that affect how electronegative an atom is

A
  • atomic charge
  • atomic radius (distance from nucleus)
  • electron shielding
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3
Q

if there is a bond between identical atoms what does this mean in terms of electrons

A

bonds between identical atoms = electrons are shared equally

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4
Q

if there is a bond between different atoms what does this mean in terms of electrons?

A

the more electronegative atom will have a greater share of the electrons

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5
Q

what type of molecule are symmetrical molecules even if they have polar bonds

A

non polar

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6
Q

if the difference in electronegativity is greater what does this do to the strength of the permanent dipole

A

the difference in electronegativity is greater = greater the strength of the permanent dipolr

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7
Q

what is the most electronegative atom

A

fluorine

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8
Q

what is the least electronegative atom

A

francium

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9
Q

why does electronegativity increase across a period

A
  • the same amount of shielding
  • atomic radius is increasing
  • more protons
    = higher electronegativity
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10
Q

why does electronegativity decrease down a group

A

shielding is increasing
atomic radius is decreasing
more protons
lower electronegativity

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11
Q

if there is no difference in electronegativity name the bond and give an example

A

non polar covalent bond
Cl-Cl
(electronically symmetrical)

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12
Q

if there is a small difference in electronegativity name the bond and give an example

A

polar covalent bond
H-Cl

(partial charges represented by delta)

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13
Q

if there is a large difference in electronegativity name the bond and give an example

A

ionic bond
Cl-Na

(full charges)

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14
Q

why does atomic radius decrease when going to the right of the periodic table

A

This is because new electrons get added to the same shell while going from left to right in a period, which increases the attraction between electrons and protons, thus pulling electrons closer to protons and decreasing the atomic radius.

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