2.12 periodic trends in atomic properties Flashcards

0
Q

which e- is removed first?

A

the one bound least tightly aka, the highest E e-

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1
Q

define ionization energy

A

the E required to remove an e- from a gaseous atom or ion:

X(g) —->X+(g) + e-

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2
Q

I1, the first ionization E is the E required to remove the ________ e- of an atom

A

highest E

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3
Q

why are the values of subsequent ionization energies (after the first) so much bigger

A

the first e- is removed from a neutral atom, however, subsequent e-‘s are removed from atoms with increasingly higher (+) charge thus requiring more E to separate from the nucleus

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4
Q

which ionization energy value is the highest and why?

A

the ionization E required to remove a core e- is the highest because core e- are bound much more tightly than valence e-‘s

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5
Q

first ionization energy (I1) increases moving across a period from:

A

left to right

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6
Q

going down a group on the PTE, the I1

A

decreases

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7
Q

as (n) increases, the size of the orbital increases and the e- is _______ to remove

A

easier

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8
Q

X(g) + e- —–> X-(g)

A

electron affinity

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9
Q

the addition of an e- can result in either a _______ E or a _______ E

A

lower or higher E

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10
Q

if the addition of an e- results in a lower E state, the value for e- affinity will be

A

negative

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11
Q

if the addition of an e- results in a _______ E state, the e- affinity value will be positive

A

higher

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12
Q

covalent atomic radii

A

the atomic radii determined by measuring the distance between the nuclei in a diatomic molecule (then dividing by 2)

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13
Q

metallic radii

A

the radii for metal atoms determined by by measuring the distance between the radii in solid metal crystals

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14
Q

atomic radii for nonmetallic atoms that don’t form diatomic molecules

A

estimated from various covalent compounds

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15
Q

why do atomic radii decrease going from left to right?

A

there is decreased shielding going from left to right–the valence e- are drawn closer to the nucleus, decreasing the size of the atom

16
Q

because of increases in orbital sizes in successive principle quantum levels, atomic radii increase going

A

down a group