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Chemistry > L-1 Periodic Table > Flashcards

L-1 Periodic Table Flashcards

(85 cards)

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1
Q

Examples of Dobereiner’s triads

A

Cl, Br, I and Ca, Sr, Ba

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2
Q

Modern Periodic Law? Coined by?

A

Physical and chemical properties of elements are a periodic function of their atomic number.
Henry Moseley

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3
Q

Elements known at time of Mendeleev’s periodic table

A

63

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4
Q

Drawbacks of Dobereiner’s triads and Newland’s Octaves

A

1- Not fitted well for all elements known at the time
2- Applicable only upto Ca

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5
Q

Achievements of Mendeleev’s periodic table

A

Atomic mass of Be was corrected
Predicted undiscovered elements (Eka- Aluminium- Gallium, Eka-Silicon- Germanium)

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6
Q

Drawbacks of Mendeleev’s periodic table

A

Hydrogen- no fixed position
No regular trend in increasing order of atomic masses
Isotopes failed to comply
Newly discovered elements did not fit well

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7
Q

Group-1 elements (Name, valence electrons)

A

Alkali metals
1 valence electron
H,Li,Na,K,Rb,Cs,Fr

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8
Q

Why are G1 elements also called Alkali metals?

A

Because they form basic hydroxides on reaction with water

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9
Q

G-2 elements (Name, valence electrons)

A

Alkaline earth metals
2 valence electrons
Be,Mg,Ca,Sr,Ba,Ra

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10
Q

Why are G-2 elements called Alkaline earth metals?

A

Form bases with water, found in earth’s crust

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11
Q

G-3-12

A

Transition elements
2 Valence shells incomplete

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12
Q

Elements with one valence shell incomplete

A

Representative elements

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13
Q

G-13

A

Boron family
B,Al,Ga,In,Th

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14
Q

G-14

A

Carbon family
C,Si,Ge,Sn,Pb

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15
Q

G-15

A

Nitrogen family (Pnictogens)
N,P,As,Sb,Bi

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16
Q

why are G-15 elements called Pnictogens

A

They are suffocating in nature

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17
Q

G-16

A

Oxygen family (Chalcogen)
O,S,Se,Te,Po

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18
Q

Why are G-16 elements called Chalcogens?

A

Ore formers

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19
Q

G-17

A

Halogens
F,Cl,Br,I,At

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20
Q

Why are G-17 elements called Halogens?

A

Salt formers

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21
Q

G-18

A

Noble gases
Do not react
Stable
He,Ne,Ar,Kr,Xe,Rn

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22
Q

Why are Lanthanides and Actinides shown at the bottom?

A

Because they are large in number and would distort the shape of the periodic table.

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23
Q

Typical Elements

A

3rd period elements summarise the properties of their respective groups

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24
Q

Periodicity

A

Phenomenon in which properties are repeated at regular intervals or in which their is gradual variation at regular intervals

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25
Cause of periodicity
Recurrence of similar electronic configuration
26
Atomic size
The distance between nucleus of an atom and outermost shell
27
Unit of atomic size
Angstrom and Picometre
28
Nuclear charge (Z effective)
Positive charge present in the nucleus, equal to the number of protons
29
Z effective
Attraction of nucleus on outermost shell
30
Across a period, Nuclear charge: Down the group:
Increases decreases
31
Atomic size decreases across a period, why
Because of increase in Nuclear charge
32
Atomic size increases down the group
Because increase in no of shells overpowers the increased Nuclear charge
33
Why are noble gases bigger than halogens?
Their outermost shells are complete. they have maximum no of electrons in Valence shells, so electronic repulsions are maximum. The effect of nuclear pull over valence electrons is not seen
34
Cation
Cation: deficiency of electrons, so nuclear pull is increased Anion: excess of electrons, which repel each other and reduce overall attraction between nucleus and electrons
35
isoelectric ions
ions having same number of electrons Size depends upon the nuclear charge (no of protons). Greater nuclear charge, smaller size
36
Metallic character
Tendency to lose electrons and form cations
37
Why is hydrogen's cation also called proton?
It has only one electron and proton, on removing e, it's cation has only a proton (no neutrons)
38
Metallic character, down group and across period
Down group: increases (no of shells) Across period: decreases (increase in Nuclear charge)
39
Greatest metallic character
Caesium
40
Non metallic character
Tendency to gain electrons to form anions
41
Non metallic char, down group and across period
Down the group: decreases Across period: increases
42
Oxides of elements across a period
Decreasing basic nature and increasing acidic nature
43
Chemical reactivity
Across period: first decreases then increases Down group: Increases for metals and decreases for non metals
44
Most non metallic element
Fluorine
45
Melting and boiling points for metals
Down the group decreases
46
Meltint and boiling point for non metals
Increases
47
Melting and boiling points across a period
increase upto g-14 then decrease
48
Density across a period
Increases gradually to maximum, then slight decrease may be noticed
49
Density down a group
increases gradually
50
Ionisation energy/potential/enthalpy
Energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion
51
equation of IE
M(g)+IE----M*+(g)+e
52
IE is ______
Endothermic (absorption of energy)
53
IE is measured in
electron volts per atom (eV/atom)
54
SI unit of IE
kilojoules per mole (kJ/mol)
55
Trends in IE
Across period: Increases Down group: decreases
56
Highest IE
Helium (2372 KJ/mol)
57
Lowest IE
Caesium (375 KJ/mol)
58
Electron Affinity
Amount of energy released while converting a neutral isolated gaseous atom into a negatively charged gaseous ion by addition of electrons
59
equation of EA
X(g)+e------>X-(g)+EA
60
EA is represented by _____ sign
negative
61
EA trends (down group and across period)
Down group: decreases Across period: Increases
62
Exceptions in IE Across a period
2nd Period: Be, N 3rd Period: Mg, P
63
Exception in EA in G-17,16
Fluorine has lower EA than Cl, and O has less than S Because Atomic size of O and F is very small, so strong inter electronic repulsions and thus incoming electron does not feel much attraction
64
Electronegativity
Tendency of an atom in a molecule to attract the shared pair of electrons towards itself (covalent bond)
65
EA in inert gases
Zero values due to their stable Elec Config so they find it difficult to accept electrons
66
EN is a dimension less property
Because it is only a tendency. Indicates the net result of tendencies if different elements to attract the bond forming electron pair
67
Scale used for EN devised by
Linus Pauling
68
highest value of EN and lowest
F- 4.0 and Cs- 0.7
69
Trends in EN
Down group: decreases Across period: Increases
70
EN for inert gases
No tendency to attract electrons because of stable config
71
Why do elements of second period differ in properties from their respective groups?
Because of small size of atoms and high EN
72
Bridge elements/ Diagonal relationship
Properties which have increasing trend in periods have decreasing trends in groups. So elements of 2nd period show resemblance in properties to elements of the next group of 3rd period, present at right diagonals
73
Eg of Bridge elements
Li- Mg, Be-Al, B-Si
74
Atomic number
No of protons in nucleus
75
Mass number
Sum of protons and neutrons
76
Elements with n/p ratio around 1 are
stable eg light metals like sodium, Potassium, calcium etc
77
Elements with n/p ratio 1.5 and above are
radioactive, they emit radiations. Unstable elements, eg- Uranium (heavy metals)
78
Hardest Alkali metal
Lithium
79
Alkalis are _____ conductors of electricity
good
80
Halogens are _____ conductors of electricity
non, bad
81
Why is Chlorine's EA greater than Fluorine?
F's size is smaller than Cl and it cannot accommodate more electrons
82
Smallest Value of IE of an element
Cs
83
Highest value of IE
Cl
84
Highest EN
F
85
Lowest EN
Cs

Chemistry (3 decks)

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