Periodic Table Flashcards

1
Q

modern periodic law

A

physical and chemical properties of elements are periodic functions of their atomic numbers

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2
Q

modern periodic table correlates position of element with

A

electronic configuration

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3
Q

define bridge elements

A

show similarities in properties diagonally with the period of the next group

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4
Q

what happens to electronegative character across period

A

increases

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5
Q

what happens to electropositive character across period

A

decreases

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6
Q

metasilisic acid formula

A

H2SiO3, weak acid

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7
Q

perchloric acid formula

A

HClO4, strong acid

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8
Q

chlorine heptoxide formula

A

Cl2O7, strongly acidic

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9
Q

phosphine formula

A

PH3, weaker base

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10
Q

metaphosphoric acid formula

A

HPO3, weak acid

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11
Q

orthophosphoric acid

A

H3PO4, weak acid

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12
Q

transition elements have how many valence electrons

A

2

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13
Q

metallic character down a group

A

increases

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14
Q

periodicity in properties of elements mean

A

occurrence of characteristic properties of elements at regular intervals in the modern periodic table, when elements are arranged in increasing order of their atomic numbers.

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15
Q

define ionisation potential

A

the amount of energy required to remove an electron from the outermost shell of an isolated, gaseous atom.

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16
Q

define electron affinity

A

the amount of energy released when an atom in the gaseous state accepts an electron to form an anion

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17
Q

define electronegativity

A

tendency of an atom to attract electrons to itself when combined in a compound

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18
Q

what happens to atomic radius when nuclear charge increases

A

atomic size decreases, because electrons of outermost shell are attracted with more force.

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19
Q

define nuclear charge

A

positive charge on the nucleus of an atom. it is equal to its atomic number

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20
Q

atomic radius across the period

21
Q

why do noble gases have larger atomic radius in a period

A

the outermost shell is filled, so there is repulsion. nuclear pull over valence electrons is not seen, so radius is maximum

22
Q

atomic radius down a group

A

increases (nuclear charge increase down a group, but increase in number of shell dominates increase in nuclear charge)

23
Q

what happens to IP when radius increases

A

decreases (nuclear attraction on outermost shell decreases, so less energy needed)

24
Q

what happens to IP when nuclear charge increases

25
why do metals have lower IP than non metals
because they lose electrons
26
IP across a period
increasesI
27
IP down a group
decreases
28
what happens to EA when radius increases
decreases, because smaller the atom, the more readily it takes up electrons, so more energy released.
29
which elements have highest EA
halogens
30
which elements have 0 EA
noble gases
31
greater the value of EA...
more electronegative/ more oxidising is the element
32
EA across a period
increases
33
EA down a group
decreases
34
electronegativity (EN) indicates what?
net result of the tendency of elements to attract the bond forming electron pair
35
most EN element
fluorine
36
least EN element
caesium
37
EN across a period
increases
38
EN down a group
decreases
39
what happens to metallic and non metallic character when ionisation potential decreases
increases, decreases
40
metallic character across period
decreases
41
non metallic character across period
increases
42
most metallic elements
at bottom of the group, because they have largest AR, lowest IP
43
metallic character down a group
increases
44
non metallic character down a group
decreases
45
density across a period
increase gradually (slight decrease thereafter)
46
density down a group
increases (so m.p and b.p decrease)
47
define light metals
elements arranged in periodic table having n/p ratio around 1 (stable elements)
48
define heavy metals
elements having n/p ratio more than 1.5 (unstable elements)