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Chemistry > The Periodic Table > Flashcards

The Periodic Table Flashcards

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1
Q

Periodic Law

A

chemical/physical properties of elements are dependent in a periodic fashion based off of atomic numbers

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2
Q

The seven periods represent

A

seven rows based on quantum numbers n=1-7 for s and p blocked elements

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3
Q

Groups/Families

A

columns

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4
Q

Elements with the same electronic config in valence shell share…

A

similar chemical properties

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5
Q

Why valence electrons form chemical bonds…

A

because they are less tightly held by nucleus and hold high potential energy

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6
Q

A elements

A

representative elements

IA - VIIA

orbitals in s or p shells

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7
Q

B Elements

A

non representative elements

transition elements, lanthanide and actinide series

s & d, s & f subshells

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8
Q

Metals are found in the _

A

left and middle side of the periodic table

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9
Q

Metals contain the following:

A

active metals , transition metals , lanthanide and actinide

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10
Q

Metal Properties

A 
Lustrous
High mp and density
Maleable
Ductile 
Good Conductor
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11
Q

Atomic Metal Properties

A 
Low effective nuclear charge
low electronegativity 
large atomic radius 
small ionic radius 
low ionization energy
low electron affinity

all together make metals easy to give up electrons!!!!

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12
Q

Oxidation States

A

charges formed when forming bonds with other atoms

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13
Q

Metals are good conductors because..

A

they have free moving electrons

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14
Q

Active Metal Subshell

A

s

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15
Q

Transition Metal Subshells

A

s and d

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16
Q

Lanthanide and Actinide Subshells

A

s and f

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17
Q

Nonmetals are found predominantly on the

A

upper right side of periodic table

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18
Q

Nonmetal Properties

A

Brittle as solids
Little to no metallic luster
Poor Conductors

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19
Q

Nonmetal Atomic Properties

A

small atomic radii (opposite of metals)
large ionic radii (opposite of metals)

Hard to give up electrons!!!

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20
Q

Metalloid Properties

A

electronegativity/ionization between that of metals (loq) and nonmetals (high)

others (density, mp, etc) vary widely

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21
Q

Lanthanides and Actinides are located…

A

separated bottom 2 rows respectively

22
Q

All the Nonmetals:

A

Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, Astatine

23
Q

Moving left to right on periodic table…

A

electrons and protons are added one at a time

effective nuclear charge (Zeff) increases

atomic radii decreases

24
Q

As the POSITIVITY of the nucleus increases…

A

the electrons around the nucleus experience a STRONGER ELECTROSTATIC PULL toward center of atom

electron cloud moves closer ot binds more tightly to nuclues

25
Q

Effective Nuclear Charge (Zeff)

A

electrostatic attraction

net positive charge experienced by outermost electron

increases left to right!!!

constant up and down!

26
Q

Electrons inbetween nucleus and outermost electron…

A

can cancel some nuclear charge

27
Q

Moving down on the periodic table….

A

principle quantum number increases by 1 each time (number of shells increases)

reduction in electrostatic attraction

reduced positivity of nucleus

valence electrons held less tightly

28
Q

Going down the table, increased shielding caused by inner shell electrons causes…

A

cancellation of increased positivity of nucleus

hence Zeff of a group is constant!!!

29
Q

Atomic radius

A

1/2 the distance between the centers of two atoms briefly in contact with one another

decreases left to right as electrons are pulled more inward

increases going down the periodic table

30
Q

2 things to generalize

A

1) metals lose electrons and become more positive and non metals gain electrons to become more negtive
2) metalloids act either way with a tendency to act more like one dependent on what side of the line they fall on

31
Q

Nonmetals close to the metalloid possess…

A

larger ionic radii than their counterparts in VIIIA

32
Q

Metals close to the metalloids possess…

A

smaller radii than other metals

33
Q

Ionization Energy (IE)

A

energy required to remove electron from a gas

endothermic process;

increases from left to right, bottom to top

34
Q

Why are some metals ‘active’?

A

they contain low ionization energies that they are not found in neutral state

35
Q

First/Second Ionization Energies

A

Energy required to remove the first and second electrons respectively

36
Q

Electron Affinity

A

opposite of IE

energy dissipated (exothermic) when a gas gains an electron

increases left to right, bottom to top and is the opposite sign of IE

37
Q

Electronegativity

A

measure of attractive force an atom will exert on an electron in chemical bond

38
Q

Electronegativity is ___ related to ionization energy

A

directly! lower , lower or higher, higher

39
Q

Pauling Electronegativity Scale

A

0.7 - 4.0 (least electronegative to most electronegative)

40
Q

Left to Right Trends Periodic Table

A 
ionization energy increases
electron affinity increases
electronegtavity increases
effective nuclear charge (Zeff) increases 
atomic radii decreases
41
Q

Bottom Up Trends

A 
ionization energy Increases
electron affinity Increases
electronegtativity increases
effective nuclear charge (Zeff) constant 
atomic radii decreases
42
Q

Chemistry Groups

A 
Alkali Metals
Alkaline Earth Metals
Chalcogens
Halogens
Noble Gases
Transition Metals
43
Q

Alkali metals (Group 1)

A

lower densities than other metals

one valence electron

lowest Zeff , electron affinity/negativity and ionization energy

highest atomic radius

active metals

44
Q

Alkaline Earth Metals (Group 2)

A

like all metals but higher Zeff and smaller atomic radii

active metals

45
Q

Chalcogens (Group 16)

A

nonmetals and metalloids

six valence electrons

small atomic radii and large ionic radii since close to metalloids

biological importance

46
Q

Halogens (17)

A

highly reactive nonmetals

7 valence electrons

physical properties variable

high electron affinity/negativity

reactive towards alkali and alkaline earth metals

47
Q

Noble Gases (18)

A

inert with no chemical reactivity

high ionization energies, but no tendency to lose or gain electrons and no electronegativity

low boiling points and gases

48
Q

Transition Metals (Groups 3-12)

A

low electron affinities, ionization energies and electronegativities

hard, high melting and boiling points, malleable, conductos

loose electrons in d orbitals

different possible charged forms/oxidation states to form many ionic compounds

49
Q

Color is seen because…

A

it is reflected

50
Q

Complementary color

A

the color that is complementary to the color of the wavelength absorbed; this is what is seen

ex: blue gets absorbed so we see yellow

Chemistry (9 decks)

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