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chemistry > chp 5 test > Flashcards

chp 5 test Flashcards

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1
Q

alkali metals properties (group 1)

A

highly reactive

not found isolated in nature

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2
Q

alkaline-earth elements properties (group 2)

A

metals

highly reactive

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3
Q

transition elements properties (groups 3-12)

A

metals
good conductors
reactivity varies

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4
Q

metals properties (groups 3-16)

A

reactive

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5
Q

metalloids properties (groups 3-16)

A

some properties of metals/ some properties of nonmetals

semiconductors

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6
Q

nonmetals properties (groups 3-16)

A

C, N, O, P, S

primary components of living things

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7
Q

halogens properties (group 17)

A

most reactive nonmetals

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8
Q

noble gases properties (group 18)

A

nonreactive

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9
Q

lanthanides properties (top bottom row)

A

metals

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10
Q

actinides properties (bottom bottom row)

A

tend to be radioactive

some actinides are man made

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11
Q

ionization energy

A

the energy required to remove one electron from an atom

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12
Q

IE equation

A

A + energy —> e- + A+

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13
Q

highest and lowest IE

why?

A

highest: group 18
because it has a full octet and is already stable so more energy is required to break up the octet

lowest: group 1
because the elements become more stable by losing an electron

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14
Q

IE trend down a group

why?

A

as you move down a group, IE decreases

because the electron being removed is further from the positive nucleus

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15
Q

second ionization energy

A

the energy required to remove the second electron from an atom

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16
Q

second IE equation

A

A+ + energy —> e- + A2+

17
Q

highest and lowest second IE

why?

A

highest: group 1
because they have an octet of electrons after leaving 1e-

lowest: group 2
because they obtain an octet by losing 2e-

18
Q

third ionization energy

A

the energy required to remove the third electron from an atom

19
Q

third IE equation

A

A2+ + energy —> e- + A3+

20
Q

highest and lowest third IE

why?

A

highest: group 2
because they have an octet after losing 2e-

lowest: group 3
because they achieve an octet by losing 3e-

21
Q

electron affinity

A

the energy charge that occurs when an atom gains an electron

22
Q

positive EA

A

energy is required for an atom to gain the electron

23
Q

negative EA

A

energy is released as the atom gains the electron

24
Q

positive EA equation

A

A + e- + energy—> A-

25
Q

negative EA equation

A

A + e- —> A- + energy

26
Q

highest positive EA

why?

A

group 18

because they have an octet of electrons

27
Q

highest negative EA

why?

A

group 17

because they become more stable by gaining 1e-

28
Q

electronegativity

A

a measure of the ability of an atom in a chemical compound to attract electrons

29
Q

highest and lowest EN

why?

A

highest: group 17
because they become more stable by gaining electrons

lowest: group 1
because they become more stable by losing electrons

30
Q

noble gases (group 18) EN

A

do not have EN values because they do not form compounds

31
Q

atomic radius trend down a group

why?

A

as you move down a group, the atomic radius increases

because new energy levels of electrons are added

32
Q

atomic radius trend across a group

why?

A

as you move across a group, the atomic radius decreases
because no new energy levels are added, the nuclear charge increases, and electrons are being pulled closer to the nucleus

33
Q

cation

A

positive ion

34
Q

anion

A

negative ion

35
Q

cation size compared to neutral atom

why?

A

always smaller than their neutral atoms

because the same nuclear charge is exerted on fewer electrons

36
Q

anion size compared to neutral atom

why?

A

always larger than their neutral atoms

because the same nuclear charge is exerted on more electrons

chemistry (16 decks)

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