The Periodic Table Flashcards

1
Q

What are the three types of elements

A

Metals metaloids non metals

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2
Q

where are metals located on the periodic table

A

left side of staircase

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3
Q

where are non metals located

A

right side of staircase

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4
Q

where are metalloids

A

either side of the staircase ex aluminum

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5
Q

horizontal rows

A

periods

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6
Q

how many periods are there

A

7

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7
Q

vertical columns

A

groups or families

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8
Q

group A

A

representative elements

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9
Q

group B

A

Transition elements

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10
Q

Cations

A

Metals that lose electrons to become positive charged ions

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11
Q

Anions

A

Non metals that gain electrons to become negativity charged ions

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12
Q

Periodic law

A

elements arranged in order of increasing atomic
number with similar
chemical properties appear periodically

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13
Q

Periodic Trends

A

chemical reactivity
Atomic Radius
Ionic Radius
Ionization Energy
electronegavativity

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14
Q

Chemical Reactivity

A

similar # of valance electron = similar chemical properties

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15
Q

Atomic Radius

A

length from center of nucleus to outermost electron

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16
Q

What happens to the atomic radius when you go down a group

A

Atomic radius increases because there are more electron shells = more shielding electrons which block the attraction between the nucleus and the outer most electron, electrons repel spreading out

17
Q

what happens to atomic radius when you move across periods

A

when you go left to right across and period the atomic radius decreases because there are more protons without an additional electron shell = higher effective nuclear charge ( attraction) to pull in the electrons

18
Q

Ionic radius

A

Cations become smaller
Anions become larger

19
Q

Cations become smaller why? (ionic radius)

A

lost of an electron which increases effective nuclear charge ( more attraction between nucleus and electron bring the electrons closer) which makes the atom smaller

20
Q

( Ionic radius ) Anions become bigger Why?

A

Gain of electrons decreases effective nuclear charge causing the electrons to repel and spread out ( atom gets bigger)

21
Q

Ionization Energy

A

the energy required to remove the outer most electrons

22
Q

what happens to the ionization energy when the atom is smaller ( across a period )

A

it increases because the attraction to the nucleus is greater ( effective nuclear charge) needed more energy to remove the outer electrons

23
Q

what happens to the ionization energy when the atom is big ( down a period)

A

it decreases because the attraction between the electrons and the nucleus is lower due to shielding electrons

24
Q

Why are atomic mass and ionization energy trends the opposite?

A

When atomic radius decreases ionization energy increases
when atomic radius decreases ionization increases

25
successive ionization energies
when trying to remove a core electron the ionization energy is very high because the electrons are held closer to the nucleus due to the effective nuclear charge is very high
26
electronegativity
tendency for a bonded atom to attract electrons decreases going down groups increases moving left to right in periods
27
why do smaller atoms have high electronegativity
smaller atoms have a greater effective nuclear charge causing the electrons to be closer to the nucleus so the smaller atom will hold the shared election closer to its self then the larger bonded atom
28
when do the protons stay in the nucleus
the protons are attracted to the neutrons
29
what is nuclear force
the attraction between the protons and neutrons that is holding the nucleus together
30
what groups are the periodic table broken up into
alkali metals alkali earth metals transition metals non metals metalloids halogens noble gases lanthanoids actinoids
31
what metal is not a solid
mercury
32
what non metals are not gase
bromine (liquid) and iodine( solid)
33
characteristics of metals
often grey and shinny solid conductors of heat and electricity Cations
34
characteristics of non metals
mostly gases anions non conductors
35
characteristics metalloids
elements along staircase both metallic and non metallic proprieties partail conductor Malleable
36
what are sheliding electrons
electrons that block the atrraction from the outer moste elctrons to the nucleus making them repel and spread out increased protons is not enough to over come sheliding electrons