OZ6 Electronegativity Flashcards

1
Q

What is electronegativity?

A

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

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2
Q

What attracts negativity charged outer electrons to an atom?

A

It’s positivity charged nucleus.

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3
Q

What is the most electronegativity element?

A

Fluorine.

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4
Q

Why is fluorine the most electronegative?

A

It is best at attracting electrons.

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5
Q

What factors affects electronegativity?

A

Nuclear charge, atomic radius, and shielding.

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6
Q

What happens to electronegativity as nuclear charge increases?

A

It increases.

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7
Q

Why does an increase in nuclear charge lead to an increase in electronegativity?

A

An increase in protons in the nucleus result to more attraction with outer shell electrons.

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8
Q

What happens to electronegativity as atomic radius increases?

A

It decreases.

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9
Q

Why does an increase in atomic radius lead to a decrease in electronegativity?

A

Electrons further from the nucleus have a weaker attraction.

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10
Q

What happens to electronegativity as the number of shells increases?

A

It decreases.

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11
Q

Why does an increase in the number of shells lead to a decrease in electronegativity?

A

Filled energy levels shield the nucleus leading to less attraction.

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12
Q

What happens to the electron distribution in a covalent bond between elements with different electronegativities?

A

It will be unevenly distributed as the more electronegative side will have more electrons.

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13
Q

What happens to electronegativity across a period?

A

It increases.

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14
Q

What happens to electronegativity down a group?

A

It decreases.

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15
Q

Why does electronegativity increase across a period?

A

The nuclear charge increases and the shielding doesn’t change, causing the atomic radius to decrease and result in stronger attraction.

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16
Q

Why does electronegativity decreased down a group?

A

The nuclear charge, shielding, and atomic radius increase leading to a decrease in attraction.