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General Chemistry MCAT > Periodic Trends > Flashcards

Periodic Trends Flashcards

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1
Q

Periodic Law

A

Chemical and physical properties of the elements are dependent, a perioid way upon their atomic numbers

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2
Q

Elements in a group share the same ______________

A

electron configuration in their valence shell and share similar similar chemical properties

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3
Q

How do you tell how many valence electrons are there for an atom?

A

the Roman Numeral

for A elements: whatever the element is = your valence electrons (they are called representative elements) their valence electrons are in the s or p subshell)

for B elements: unexpected configurations

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4
Q

Another names for groups (columns)

A

Families

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5
Q

Period

A

Rows

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6
Q

Groups

A

Columns

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7
Q

A elements

A

Representative elements, groups IA through VIIIA

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8
Q

Group B elements

A

Non representative elements and include both transition elements, lanthanide and actinide, have 2 or more oxidation states (charges when forming bonds with other atoms)

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9
Q

Metal

A

lustrous shiny solids except mercury, generally high melting points and densities except lithium (other exceptions), deformed without breaking

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10
Q

at the atomic level, a metal is defined by a

A

low effective nuclear charge, low electronegativity (high electropositivity), large atomic radius, small ionic radius, low ionization energy, and low electron affinity

all of these qualities are manifestations of the ability of metals to easily give up electrons

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11
Q

Describe Ductility.

A

metals ability to be pulled or drawn into wires

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12
Q

Describe malleability.

A

Metals ability to be hammered into shapes

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13
Q

Groupe B transition metals have

A

Two or more oxidation states (charges when forming bonds with other atoms)

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14
Q

Metals are good conductors because

A

the valence electrons of all metals are only loosely held to their atoms, therefore they are free to move making metals good conductors of heat and electricity

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15
Q

Valence electrons of active metals are found in the

A

s subshell

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16
Q

Valence electrons of transition metals are found in the

A

s and d subshells

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17
Q

valence electrons of lanthanide and actinide series metals are found

A

s and f subshells

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18
Q

copper, nickel, silver, gold, palladium, and platinum

A

transition metals that are relatively nonreactive that makes them ideal for coins and jewelry

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19
Q

Transition metals conductibility

A

good conductors

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20
Q

Metals electron transfer abilities

A

Easily give up electrons

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21
Q

Nonmetals

A

Upper right of periodic table, brittle in solid state, little or no metallic luster, high IE, EA, and EN, small atomic radii and large ionic radii

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22
Q

Nonmetals electron transfer abilities

A

DO NOT easily give up electrons

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23
Q

conductibility of nonmetals.

A

they are poor conductors

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24
Q

Metalloids

A

stair-step group of elements, semimetals because they share some characteristics with both metals and nonmetals, physical properties vary widely and can be combinations of characteristics

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25
Q

As you move from left to right the amount of protons in a nucleus increases, this causes what

A

the electron cloud to bind together tighter and closer to teh nucleus because the electrons feel a great electrostatic pull

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26
Q

Effective Nuclear Charge

A

electrostatic attraction between he valence shell electrons and the nucleus

a measure of the net positive charge experienced by the outermost electrons

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27
Q

The pull of the positivity of the nucleus is mitigated by

A

the nonvalence electrons that reside closer to the nucleus

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28
Q

effective nuclear charge _____ from left to right (for elements in the same period) (figure 2.4 page 47)

A

INCREASES

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29
Q

as you move down on the periodic table: ___ happens

A

the principal quantum number increased by one each time – so the valence electrons are separated from the nucleus by a greater number of filled principal energy levels (aka inner shells) more and more each time

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30
Q

what does increased separation of the valence electrons and nucleus result in?

A

reduction in the electrostatic attraction between the positively charged nucleus and valence electrons, so the outermost electrons are held less tightly by the nucleus

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31
Q

z-eff is constant in a group, why?

A

as you go down a group the increased shielding (caused by the inner shells) cancels out the positivity of the nucleus

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32
Q

as you move down the periodic table _____________ because of increased separation between ____________

A

valence electrons are held less tightly to the nucleus

valence electrons and the nucleus

33
Q

elements can either gain or lose electrons in order to achieve

A

a stable octet formation (like the noble gases) this rule is often broken but for the most part, especially for elements with biological roles, elements are the most stable with eight electrons in their valence shell

34
Q

atomic radius

A

1/2 the distance between the centers of the two atoms (you need two atoms because in order to measure the radius of one atom, its impossible because of how much atoms move around)

35
Q

the z-eff ______ as you move left to right across a period, and as a result, atomic radius ____ from left to right on a period

A

increases because electrons are added to the outermost shell and the inner shells remain constant

decreases because the outer electrons are held more tightly to the nucleus

36
Q

the z-eff ______ as you move left to right across a period, and as a result, atomic radius ____ from left to right on a period

A

decreases because the outer electrons are held more tightly to the nucleus

37
Q

atomic radius ___ down a group because

A

increases: there is more inner shells shielding the outermost electrons from the nucleus, therefore they are held less tightly to the nucleus

38
Q

within each period the largest atom is:
within each group the largest atom is:

A

Group 1
at the bottom

39
Q

in order to understand ionic radii, must make two generalizations

A

metals lose electrons and become positive, while nonmetals gain electrons and become negative

metalloids can go in either direction, but tend to follow the trend based on which side of the stairs they fall on

40
Q

nonmetals close to the metalloid line posses a

A

larger ionic radius than their counterparts closer to noble gases because they can gain electrons while their nucleus maintains the same charge

41
Q

metals close to the metalloid line posses a

A

smaller ionic radius, opposite to nonmetals close to the line, because they have more electrons to lose

42
Q

why do group IA elements experience a less dramatic reduction in radius during ionization?

A

they have fewer electrons to lose

43
Q

ionization energy/potential

A

energy required to remove an electron from a gaseous species

44
Q

emoving an electron from a gas

A

requires an input of heat, makes it an endothermic process

45
Q

the greater the Z-eff, or the closer the valence electrons are to the nucleus, the more tightly bound they are making them harder to remove therefore ______ the ionization energy

A

increasing, therefore the ionization energy increases from left to right across a period and bottom to top in a group

46
Q

removal of a second or third electron requires

A

increasing amounts of energy because the removal of more than one electron means that the electrons are being removed from an increasingly cationic (positive) species

47
Q

because groups 1 and 2 have such low ionization energies they are called

A

Active Metals

48
Q

active metals are never found in ____ forms they are found in _____ because _____

A

neutral, ionic compounds minerals or ores
losing one electron in Group I and two electrons in Group II resulting

49
Q

halogens do not give up their electrons normally, in fact they reside in their ____ form

A

ionic form (anion)

50
Q

the second ionization energies are disproportionally larger for Group IA monovalent cations but not for Group 2 or subsequent monovalent cations because

A

removing one electron from a Group IA metal results in a noble gas-like electron configuration

51
Q

noble gases have the ___ ionization energies, why?

A

highest, because they are the least likely to give up electrons, they have a stable configuration and do not want to disrupt that stability by giving up an electron

52
Q

halogens are the most _____ drop of elements when it comes to electrons

A

greedy, because one additional electron and they achieve a noble gas configuration

53
Q

when a halogen is able to complete its octet this is a ______

A

exothermic process which expels energy in the form of heat

54
Q

electron affinity

A

energy dissipated by a gases species when it gains an electron (opposite of ionization energy

55
Q

exothermic process what is the sign on delta H reaction

A

negative sign which means they give off heat so the electron affinity is positive

56
Q

electron affinity of group 18

A

0

57
Q

Electronegativity

A

Measure of the attractive force that an atom will exert on an electron in a chemical bond

58
Q

the greater the EN

A

the more it attracts electrons within a bond

59
Q

the lower the ionization energy

A

the lower the electronegativity

60
Q

exceptions to electronegativity

A

first three noble gases, despite their high ionization energies, these elements have negligible EN because they do not often form bonds

61
Q

Pauling electronegativity scale

A

Ranges for Cs the lowest electronegativity of .7 (most electropositive) to F of most electronegativity of 4

62
Q

EN trend

A

increases across a period from left to right and decreases in a group from top to bottom (so bottom left to top right)

63
Q

Periodic table metal classification

A
64
Q

alkali metals

A

Group 1, densities lower than those of other metals, one loosely bound electron in outermost shell, Zeff low, large AR, low IE, low EA, low EN, readily react with nonmetals, easily lose electron

65
Q

alkaline earth metals

A

Group IIA, share most characteristics with alkali metals, slightly higher Zeff, easily lose two electrons to be divalent cation form

66
Q

chalcogens

A

group VIA, nonmetals and metalloids, 6 e- in outer shell, proximity to metalloids means small AR and large IR, some elements generally toxic and primarily metallic

67
Q

halogens

A

group 7A, Contains nonmetals, 7 valence electrons in it’s outermost energy level. Very reactive, not naturally found in normal state, rather as ions called halides or diatomic molecules

68
Q

noble gases

A

group VIIIA, inert gases because minimal reactivity, extremely low boiling points and exist as gases at room temperature

69
Q

transition metals

A

group B, considered to be metals, very hard, high melting and boiling points, malleable and good conductors due to loose electrons in d-orbitals

unique- many have different possible charged forms or oxidation states because capable of losing different numbers of electrons

often vibrant colors in solutions

70
Q

transition metals tend to associate in solution either with

A

molecules of water (hydration complexes) or with nonmetals

71
Q

formation of complexes causes

A

d-orbitals to split into two energy sub levels

72
Q

subtraction frequencies

A

Frequencies not absorbed; give complexes their characteristic colors

73
Q

the complementary color of the frequency that was absorbed

A

if an object absorbs a given color of light and reflects all others, our brain mixes these subtraction frequencies and we perceive

74
Q

high reactivity to water

A

groups 1 and 2

75
Q

six valence electrons

A

Group 6 and 16

76
Q

contains at least one metal

A

groups 1 through 15

77
Q

multiple oxidation states

A

all groups, most notably transition metals

78
Q

negative oxidation states

A

almost all, most notably 14-17

79
Q

full octet in neutral state

A

group 18

General Chemistry MCAT (7 decks)

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