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IB Chemistry SL > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

what is periodicity

A

the regular reputation of properties of elements arising from patterns in their electron arrangement

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2
Q

how are elements arranged in the periodic table

A

according to their increasing atomic number and the number of protons

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3
Q

what are the 4 blocks

A

s p d f

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4
Q

why is Zn not a transition metal

A

because it does not form complete ions with incomplete d sub levels

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5
Q

what is atomic radii

A

the distance from the nucleus the the outermost electrons

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6
Q

how is atomic radii defined

A

as half the distance between the nuclei of two bonded atoms of the same element

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7
Q

atomic radii trend

A

Helium has the smallest atomic radii

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8
Q

why does atomic radii increase down a group

A

because the electron becomes further away from the nucleus

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9
Q

why does atomic radii decrease across a period

A

due to the increasing number of protons that pull the electrons in more tightly

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10
Q

what is ionic radius

A

the radius of an atom ion obtained by adding the distance between two ions and adding the ionic radius of the cation and anion

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11
Q

what is a cation

A

the positive ion

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12
Q

what is an anion

A

the negative ion

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13
Q

cations + ionic radius

A

positive ions radii are smaller than that of their parent atoms

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14
Q

anions + ionic radius

A

negative ions radii are bigger than that of their parent atoms

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15
Q

way of remembering size order of cation anion and atom

A

cation

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16
Q

ionic radius trend down a group

A

cation + anion INCREASE as outer level gets further away from nucleus

17
Q

ionic radius trend across a period

A

CATIONS: ionic radii decrease due to the increasing number of protons

ANIONS: decrease of atomic radii, but the electrons remain the same for the anions

18
Q

what is the first ionization energy

A

the energy required to remove one mole of electrons from one mole of gaseous atoms

19
Q

ionization energy trend down a group

A

DECREASES due to the increased distance between the nucleus + outer energy level that reduces the force of attraction between the nucleus and outer electrons

20
Q

ionization energy trend across a period

A

INCREASES due to the the increase in effective nuclear charge that causes electrons to be held more tightly

21
Q

what is electron affinity

A

the energy change when one mole of electrons is added to one mole of gaseous atoms to form on mole of gaseous ions

x + e- = x-

22
Q

electron affinity ACROSS PERIOD:

A

increases due to the increase in nucleus charge

23
Q

electron affinity trend

A

F has the highest electron affinity

24
Q

what is electronegativity

A

its the measure of attraction of a nucleus to bonding electrons

25
Q

electronegativity trend

A

F has the highest electronegativity

26
Q

electronegativity trend across a period

A

INCREASE from left to right due to the increase in nuclear charge

27
Q

electronegativity trend down a group

A

decrease as electrons move further away from the nucleus

28
Q

melting point trend down group 1

A

decreases

29
Q

melting point trend down group 17

A

increases

30
Q

period 3 oxide trend

A

oxides change from basic to amphoteric to acidic across a period

31
Q

acidic oxides reaction

A

react with water to produce acidic solutions

32
Q

basic oxide

A

react with water to form salt and water

33
Q

bonding trend

A

left to right: ionic to covalent

34
Q

group 17 trend

A

reactivity decreases down the group

35
Q

group 1

A

reactivity increases down a group

36
Q

boilin gpoint trend

A
  1. increase due to intermolecular forces
  2. increase due to number of carbons attached
  3. DECREASE due to branching

IB Chemistry SL (7 decks)

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