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Periodic Table Flashcards

(98 cards)

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1
Q

How did early chemists arrange elements ? why was this discarded?

A
  1. Basis of valency , metallic and non metallic character

2. elements showed variable valency and dual character

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2
Q

Groups of three elements as grouped by Dobereiner are called ______

A

Triads

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3
Q

What was the specialty in Dobereiner’s triads?

A

The avg of first and last element’s atomic weight = atomic weight of middle term

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4
Q

Why was Dobereiner’s method discarded?

A

it did not hold true for all elements

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5
Q

Newland arranged elements in series of _____

A

8

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6
Q

what was Newland’s Law of Octaves?

A

Properties of every 8th element is a repetition of the first

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7
Q

Why was Newland’s method discarded?

A

It did not leave spaces for undiscovered elements

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8
Q

In what form did Mendeleev arrange the elements and what did he call it?

A

In the form of a table called Mendeleev’s periodic table

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9
Q

What law did Mendeleev state?

A

Properties of elements are periodic functions of their atomic weights

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10
Q

Why was Mendeleev’s method discarded?

A

did not justify position of certain elements, rare earths and isotopes

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11
Q

Who came closest to achieving the periodic table which we use today?

A

Mendeleev

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12
Q

Who was the only one to arrange on the basis of atomic number and not weight?

A

Robert moseley

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13
Q

Who founded today’s modern periodic table ?

A

Robert Moseley

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14
Q

State the modern periodic law

A

Physical and chemical properties of elements are periodic functions of their atomic.no

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15
Q

What is the fundamental property of an element

A

Atomic number

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16
Q

Group 18 in Modern periodic table is known as _____ and consists of _______

A

Zero group , Inert/Noble gases

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17
Q

Group 1,2,13 to 17 in the Modern periodic table are called ___ elements

A

Normal

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18
Q

Group 3 to 12 in the Modern periodic table are called ______ elements

A

Transition elements

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19
Q

How many periods are there in the Modern periodic table ?

A

7

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20
Q

How many groups are there in the Modern periodic table ?

A

18

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21
Q

What does period number signify

A

No. of electron shells in an element

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22
Q

Non metals are placed in the ______ corner of the periodic table

A

Upper right

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23
Q

Name a non metal which is solid at room temp

A

Iodine

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24
Q

Name a non metal which is in liquid state at room temp

A

Bromine

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25
Name two non metals which are in the gaseous state at room temperature
Fluorine, Chlorine
26
Transition metals are placed in the ___
Middle
27
Transition from metallic to non metallic character is seen __________( across a period or down a group)
Across a period
28
Transition metals are _____( heavy or light) metals
Heavy
29
Valence electrons _____ as we move across a period
increase one by one
30
non metallic character _____( increases/decreases) along a period
Increases
31
What are bridge elements ?
Elements which show similarity in properties diagonally with period of next group Period 2 elements are said to be bridge elements
32
Which period consists of typical elements
3
33
Why r period 3 elements called typical elements?
The elements of period 3 summarises the properties of their respective groups hence they r called typical elements
34
state the bridge and typical elements which are similar in properties
Li - Mg Be - Al B - Si
35
Periodicity in properties occur after a difference of ___.___.____._____ in atomic numbers due to recurrence of ____________
2,8,18 or 32 | similar valence shell configuration
36
What does group number signify ?
no. of valence electrons in an element
37
Lanthanides are ____
rare earths
38
Actinides are ____
radioactive
39
Metallic character _____ down a group
increases
40
No. of electron shells ______ down a group
increases one by one
41
Chemical properties _____ (differ/remain similar ) down a group
remain similar
42
Alkali metals( group I elements )
Lithium(Li) - Sodium(Na)- Potassium(K)- Rubidium(Rb)- Caesium(Cs)- Francium(Fr)
43
Alkaline earth metals ( group 2 elements)
Beryllium(Be) - Magnesium(Mg) - Calcium(Ca)- Strontium(Sr) - Barium(Ba) - Radium(Ra)
44
Halogens( Group 17 elements)
``` Fluorine(F) Chlorine(Cl) Bromine(Br) Iodine(I) Astatine (At) ```
45
Noble gases ( group 18 elements)
``` Helium(He) Neon(Ne) Argon(Ar) Krypton(Kr) Xenon(Xe) Radon(Rn) ```
46
First transition elements
``` Sc- scandium Ti-titanium V- vanadium Cr- chromium Mn- manganese Fe- iron Co- cobalt Ni- nickel Cu- copper Zn- zinc ```
47
Group I elements are ___valent and group 17 elements are ____valent
uni, uni
48
Halogens are strong ______ agents and are electro_____
oxidising,negative
49
Alkali metal with hydrogen - | Alkali metal with non metal -
Ionic hydrides | Ionic compounds
50
Non metal with hydrogen - ____ | Non metal with non metal - _____
Covalent hydrides | Covalent compounds
51
Metals are soft or hard
Soft
52
Alkali metals are strong _____agents and are electro_____
reducing, positive
53
What are periodic properties?
properties which appear at regular intervals in the periodic table
54
Reason for periodicity?
After definitie intervals of 2,8,18 or 32... there is a similar valence shell configuration so the properties are periodic
55
What is atomic size or radius? it is measured in _____
1. the distance between the centre of nucleus of an atom and its outermost shell 2. Angstron(A^0)
56
when no. of shells increase ... atomic size ______.
increases
57
when nuclear charge increases .... atomic size ______
decreases
58
Atomic size determines ___ length
Bond
59
Why Noble gases have higher atomic size when they r supposed to have the lowest?
Bcoz their shell is completely filled, it results in a force of repulsion which balances the effect of nuclear pull over the valence electrons
60
Atomic size _______ across a period
decreases
61
Atomic size _____ down a group
increases
62
What is Ionisation potential ?
The amount of energy required to remove a loosely bound electron from the outermost shell of an isolated gaseous atom
63
When atomic size increases .... Ionisation energy _____
decreases
64
When nuclear charge increases ... Ionisation potential _____
increases
65
Energy required to remove second electron is ____(more/less) than the energy required to remove first electron
More
66
Ionisation potential _____ across a period and _____ down a group
increases, decreases
67
____ has the lowest I.P and __ has the highest I.P
Caesium , Helium
68
What is Electron affinity ?
The amount of energy released when an atom in the gaseous state accepts an electron to form an anion
69
When atomic size increases.... electron affinity/electronegativity _____
decreases
70
When nuclear charge increases .... electron affinity/electronegativity ____
increases
71
electron affinity/electronegativity ______across a period
increases
72
electron affinity/electronegativity ______ down a group
decreases
73
E.A/E.N is highest for _____ and lowest for _____
halogens, alkali metals
74
What is electronegativity ?
The tendency of an atom to attract atoms to itself when combined in a compound
75
which is the most electronegative element and which is the least electronegative element?
Fluorine,Caesium
76
What is metallic character and non metallic character?
an atom is a metal if it loses electrons and non metal if it gains electrons
77
When atomic radii increases ... metallic character ___ and non metallic character ____
increases, decreases
78
When I.P increases .... metallic character ____ and non metallic character _____
decreases , increases
79
Across a period, metallic character ____ and non metallic character ____
decreases,increases
80
Down a group,metallic character ____ and non metallic character ____
increase,decrease
81
across a period ... density of elements _______ and m.p and b.p of elements _________
increase , increase
82
Down a group .. density of elements _____ and m.p and b.p of elements ______
increases , decreases
83
across a period ... Oxides varies from _____ to ______
Strongly basic to Strongly acidic
84
Down a group ...Oxides varies from _____ to ______
Acidic to Basic
85
Across a period .... Hydroxides vary from _____ to ______
Strongly basic to amphoteric
86
Down a group ,Hydroxides vary from _____ to ______
Less basic to strong basic
87
Across a period.... Oxy acids vary from ____ to ____
weak oxy acids to strong oxy acids
88
Down a group...Oxy acids vary from ____ to ____
Strong oxy-acids to weak oxy-acids
89
Across a period.. Hydrides vary from _____ to ______
Strongly basic to strongly acidic
90
Down a group... Hydrides vary from ______ to _______
Less acidic to more acidic
91
Name a non metal which is in liquid state at room temp
Bromine
92
Alkali and alkaline earth metals are ______(light/heavy) metals
Light
93
Very short period
First period
94
Short periods
2nd and 3rd periods
95
Long periods
4th and 5th periods
96
Very long periods
6th and 7th periods
97
Element having highest electron affinity
Chlorine
98
Just above room temp, bromine is in ___ state
Liquid

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