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Chem > Periodic Table > Flashcards

Periodic Table Flashcards

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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
Q

Name two non metals which are in the gaseous state at room temperature

A

Fluorine, Chlorine

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26
Q

Transition metals are placed in the ___

A

Middle

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27
Q

Transition from metallic to non metallic character is seen __________( across a period or down a group)

A

Across a period

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28
Q

Transition metals are _____( heavy or light) metals

A

Heavy

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29
Q

Valence electrons _____ as we move across a period

A

increase one by one

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30
Q

non metallic character _____( increases/decreases) along a period

A

Increases

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31
Q

What are bridge elements ?

A

Elements which show similarity in properties diagonally with period of next group
Period 2 elements are said to be bridge elements

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32
Q

Which period consists of typical elements

A

3

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33
Q

Why r period 3 elements called typical elements?

A

The elements of period 3 summarises the properties of their respective groups hence they r called typical elements

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34
Q

state the bridge and typical elements which are similar in properties

A

Li - Mg
Be - Al
B - Si

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35
Q

Periodicity in properties occur after a difference of ___.___.____._____ in atomic numbers due to recurrence of ____________

A

2,8,18 or 32

similar valence shell configuration

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36
Q

What does group number signify ?

A

no. of valence electrons in an element

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37
Q

Lanthanides are ____

A

rare earths

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38
Q

Actinides are ____

A

radioactive

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39
Q

Metallic character _____ down a group

A

increases

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40
Q

No. of electron shells ______ down a group

A

increases one by one

41
Q

Chemical properties _____ (differ/remain similar ) down a group

A

remain similar

42
Q

Alkali metals( group I elements )

A

Lithium(Li) - Sodium(Na)- Potassium(K)- Rubidium(Rb)- Caesium(Cs)- Francium(Fr)

43
Q

Alkaline earth metals ( group 2 elements)

A

Beryllium(Be) - Magnesium(Mg) - Calcium(Ca)- Strontium(Sr) - Barium(Ba) - Radium(Ra)

44
Q

Halogens( Group 17 elements)

A 
Fluorine(F)
Chlorine(Cl)
Bromine(Br)
Iodine(I)
Astatine (At)
45
Q

Noble gases ( group 18 elements)

A 
Helium(He)
Neon(Ne)
Argon(Ar)
Krypton(Kr)
Xenon(Xe)
Radon(Rn)
46
Q

First transition elements

A 
Sc- scandium
Ti-titanium
V- vanadium
Cr- chromium
Mn- manganese
Fe- iron
Co- cobalt 
Ni- nickel 
Cu- copper
Zn- zinc
47
Q

Group I elements are ___valent and group 17 elements are ____valent

A

uni, uni

48
Q

Halogens are strong ______ agents and are electro_____

A

oxidising,negative

49
Q

Alkali metal with hydrogen -

Alkali metal with non metal -

A

Ionic hydrides

Ionic compounds

50
Q

Non metal with hydrogen - ____

Non metal with non metal - _____

A

Covalent hydrides

Covalent compounds

51
Q

Metals are soft or hard

A

Soft

52
Q

Alkali metals are strong _____agents and are electro_____

A

reducing, positive

53
Q

What are periodic properties?

A

properties which appear at regular intervals in the periodic table

54
Q

Reason for periodicity?

A

After definitie intervals of 2,8,18 or 32… there is a similar valence shell configuration so the properties are periodic

55
Q

What is atomic size or radius? it is measured in _____

A
  1. the distance between the centre of nucleus of an atom and its outermost shell
  2. Angstron(A^0)
56
Q

when no. of shells increase … atomic size ______.

A

increases

57
Q

when nuclear charge increases …. atomic size ______

A

decreases

58
Q

Atomic size determines ___ length

A

Bond

59
Q

Why Noble gases have higher atomic size when they r supposed to have the lowest?

A

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
Q

Atomic size _______ across a period

A

decreases

61
Q

Atomic size _____ down a group

A

increases

62
Q

What is Ionisation potential ?

A

The amount of energy required to remove a loosely bound electron from the outermost shell of an isolated gaseous atom

63
Q

When atomic size increases …. Ionisation energy _____

A

decreases

64
Q

When nuclear charge increases … Ionisation potential _____

A

increases

65
Q

Energy required to remove second electron is ____(more/less) than the energy required to remove first electron

A

More

66
Q

Ionisation potential _____ across a period and _____ down a group

A

increases, decreases

67
Q

____ has the lowest I.P and __ has the highest I.P

A

Caesium , Helium

68
Q

What is Electron affinity ?

A

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

69
Q

When atomic size increases…. electron affinity/electronegativity _____

A

decreases

70
Q

When nuclear charge increases …. electron affinity/electronegativity ____

A

increases

71
Q

electron affinity/electronegativity ______across a period

A

increases

72
Q

electron affinity/electronegativity ______ down a group

A

decreases

73
Q

E.A/E.N is highest for _____ and lowest for _____

A

halogens, alkali metals

74
Q

What is electronegativity ?

A

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

75
Q

which is the most electronegative element and which is the least electronegative element?

A

Fluorine,Caesium

76
Q

What is metallic character and non metallic character?

A

an atom is a metal if it loses electrons and non metal if it gains electrons

77
Q

When atomic radii increases … metallic character ___ and non metallic character ____

A

increases, decreases

78
Q

When I.P increases …. metallic character ____ and non metallic character _____

A

decreases , increases

79
Q

Across a period, metallic character ____ and non metallic character ____

A

decreases,increases

80
Q

Down a group,metallic character ____ and non metallic character ____

A

increase,decrease

81
Q

across a period … density of elements _______ and m.p and b.p of elements _________

A

increase , increase

82
Q

Down a group .. density of elements _____ and m.p and b.p of elements ______

A

increases , decreases

83
Q

across a period … Oxides varies from _____ to ______

A

Strongly basic to Strongly acidic

84
Q

Down a group …Oxides varies from _____ to ______

A

Acidic to Basic

85
Q

Across a period …. Hydroxides vary from _____ to ______

A

Strongly basic to amphoteric

86
Q

Down a group ,Hydroxides vary from _____ to ______

A

Less basic to strong basic

87
Q

Across a period…. Oxy acids vary from ____ to ____

A

weak oxy acids to strong oxy acids

88
Q

Down a group…Oxy acids vary from ____ to ____

A

Strong oxy-acids to weak oxy-acids

89
Q

Across a period.. Hydrides vary from _____ to ______

A

Strongly basic to strongly acidic

90
Q

Down a group… Hydrides vary from ______ to _______

A

Less acidic to more acidic

91
Q

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

A

Bromine

92
Q

Alkali and alkaline earth metals are ______(light/heavy) metals

A

Light

93
Q

Very short period

A

First period

94
Q

Short periods

A

2nd and 3rd periods

95
Q

Long periods

A

4th and 5th periods

96
Q

Very long periods

A

6th and 7th periods

97
Q

Element having highest electron affinity

A

Chlorine

98
Q

Just above room temp, bromine is in ___ state

A

Liquid

Chem (5 decks)

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