3.1 test Flashcards

1
Q

Deduce which of the following ions has the smallest ionic radius: Mg2+, F-, Na+, O2- (and why)

A

Mg2+
Why: all have the same electron configuration, so we must look at atomic number. Magnesium has the highest atomic number (12) so the valence electrons are mostly strongly attracted to the nucleus (so smallest radius)

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2
Q

define atomic radius

A

total distance from the nucleus of an atom to the outermost orbital of its electrons

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3
Q

define ionic radius

A

the distance between the nucleus of an ion and its outermost shell.

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4
Q

atomic radius trend

A

increases down a group, decrease left to right across a period (highest in bottom left corner)

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5
Q

define ionisation energy

A

amount of energy required to remove an electron from an atom/molecule

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6
Q

ionization energy trend

A

decreases down a group, increases left to right across a period (highest in top right corner)

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6
Q

electron affinity trend

A

decreases down a group, increases left to right across a period, highest in top right corner (same as ionization energy)

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6
Q

define electron affinity

A

energy change that results when an electron is ADDED to a gaseous atom (opposite of ionisation energy)

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7
Q

define metallic character

A

tendency of an element to lose electrons and form cations

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8
Q

metallic character trend

A

increases down a group, decreases left to right across a period (highest in bottom left corner)

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9
Q

define non-metallic character

A

the tendency of an element to accept electrons and form negative ions or anions

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10
Q

non-metallic character trend

A

decreases down a group, increases from left to right across a period (highest in upper right corner, opposite of metallic character)

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11
Q

electronegativity definition

A

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons

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12
Q

electronegativity trend

A

decreases down a group, increases from left to right across a period (highest in top right corner)

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13
Q
A
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