Periodicity

Front 1

_____ and ____ of atoms provide the theoretical foundation for the periodic classification

Back 1

Aufbau principle, electronic configuration

Front 2

The elements in ____ exhibit similar ____ behaviour.

Back 2

Group, chemical

Front 3

The similarity arises because the elements have the ______ and ______ of electrons in their outermost orbitals

Back 3

Same number, same distribution

Front 4

Helium belongs to ______ block but is positioned in the ______ .

Back 4

S, p

Front 5

On what basis hydrogen is similar to alkali metals

Back 5

Has only one s electron

Front 6

On what basis hydrogen is similar to group 17 family

Back 6

To achieve noble gas arrangement can gain an electron

Front 7

Give the atomic number of rubidium

Back 7

37

Front 8

Give the atomic number of caesium

Back 8

55

Front 9

Give the atomic number of francium

Back 9

87

Front 10

S block elements are all ____ with _____ ionization enthalpy

Back 10

Reactive metals, low

Front 11

The reactivity _____ as we go down the group

Back 11

Increases

Front 12

S block elements are never found in ____ owing to their _____ .

Back 12

Pure state, high reactivity

Front 13

S and p block elements together constitute _____ elements or _____ elements

Back 13

Representative , main group

Front 14

In p block the non metallic character ____ as we move from left to right across a period

Back 14

Increases

Front 15

The D Block Elements have general electronic configuration of _____

Back 15

Front 16

All D block elements are _____

Back 16

Metals

Front 17

The lanthanoids starts from _____(____) to ___ ( ____)

Back 17

Ce(Z=58), Lu(Z= 71)

Front 18

The actinoids start from _____ ( ___) to ____(___) .

Back 18

Th(Z=90), Lr( Z= 103)

Front 19

The electronic configuration of f block elements are

Back 19

(n-2) f1-14(n-1) d0-1 ns2

Front 20

The last electron in F block elements added to each element is filled in

Back 20

F orbital

Front 21

F block elements are all

Back 21

Metals

Front 22

The chemistry of _____ is more complicated than the corresponding lanthanoids, due to the large number of oxidation States possible

Back 22

Early actinoids

Front 23

Many of the actinoid elements have been made only in _____ quantities or even less by nuclear reactions and their chemistry is _____ fully studied

Back 23

Nanogram, not

Front 24

Elements after uranium are called

Back 24

Trans uranium elements

Front 25

The electronic configuration of Z =117

Back 25

(Rn) 5f14 6d10 7s2 7p5

Front 26

Electronic configuration of Z = 120

Back 26

(Uuo) 8s2

Front 27

Metals comprise more than ____ of all known elements and appear on the ____ side of periodic table

Back 27

78%, left

Front 28

______ And ____ also have very low melting points

Back 28

Gallium, caesium

Front 29

By ____ property metals can be flattened into thin sheets by hammering

Back 29

Malleable

Front 30

By _____ property metals can be drawn into wires

Back 30

Ductile

Front 31

Non metals are usually solids or gases at room temperature with ____ melting and boiling points

Back 31

Low

Front 32

Non metals are _____conductors of heat and electricity

Back 32

Poor

Front 33

Most non metallic solids are ___ and are neither malleable nor ductile

Back 33

Brittle

Front 34

The change from metallic to non metallic character is not ____

Back 34

Abrupt

Front 35

Give example of semi metals

Back 35

Silicon , Germanium , arsenic, antimony , tellurium

Front 36

Si, Be, Mg, Na, P : Order of metallic character is

Back 36

Na>Mg>Be>Si>P

Front 37

In non metals the reactivity ____ down the group

Back 37

Decreases

Front 38

The measurement of the distance between two atoms when they are bound Together by a _____ bond in _____ molecule forms the covalent radius.

Back 38

Single, covalent

Front 39

______ Is taken as half the inter nuclear distance separating the cores

Back 39

Metallic radius

Front 40

Noble gases are ____ .

Back 40

Monoatomic

Front 41

Noble gases have ____ radii.

Back 41

Van der waal

Front 42

Noble gases have _____ radii

Back 42

Non bonded

Front 43

The ionic radii can be estimated by measuring the distance between cations and anions. T/F.

Back 43

T

Front 44

The Ionic radius of fluoride ion is ____ where as the atomic radius of fluorine is only _____ .

Back 44

136 pm, 64 pm

Front 45

In the ionic form the radius of the metals or nonmetals generally decreases or increases by a factor of

Back 45

2

Front 46

In isoelectronic Species the radii would be ____

Back 46

Different

Front 47

The energy required to remove an electron from an isolated gaseous atom in its ground state is

Back 47

Ionization enthalpy

Front 48

Energy is always required to ____ electrons from an atom and hence ionization enthalpy are always _____ .

Back 48

Remove, positive

Front 49

In the graph of ionization enthalpy ____ occupy the maxima and _____ occupy the minima

Back 49

Noble gases, alkali metals

Front 50

Why alkali metals occupy the minimum position in the ionization enthalpy graph

Back 50

Due to their low ionization enthalpy

Front 51

Shielding is effective when the orbitals in the inner shells are ____ .

Back 51

Completely Filled

Front 52

Down the group increase in ____ outweighs the increasing _____ so removal of outermost electron requires ______ energy down the group

Back 52

Shielding, nuclear charge, less

Front 53

The penetration of ____ electron to the nucleus is more than that of ____ electron.

Back 53

2s, 2p

Front 54

In oxygen atom ____:of the four ____ electrons must occupy the same ____ orbital resulting in an increased ___ repulsion

Back 54

2, 2p, 2p, electron - electron

Front 55

Due to ______ it is ___ to remove the fourth 2p electron from oxygen in comparison to nitrogen

Back 55

Electron electron repulsion, easier

Front 56

Back 56

Front 57

Ionization enthalpy _____ across the period

Back 57

Increases

Front 58

Electron gain enthalpy provides a measure of the ease with which an atom ____ an electron to form _____ .

Back 58

Adds, anion

Front 59

For many elements energy is _____ when an electron is added to the atom and the electron gain enthalpy is ______ .

Back 59

Released, negative

Front 60

Halogens have ______ electron gain enthalpy because they can attain stable electronic configuration by _____ electron.

Back 60

High negative, adding one

Front 61

Noble gases have _____ electron gain enthalpy because the electron has to enter the next higher _____ level leading to very unstable electronic configuration

Back 61

Large positive, principle Quantum,

Front 62

The electron gain enthalpies have ________ values toward the upper right of the periodic table preceding the noble gases

Back 62

Large negative,

Front 63

As a general rule electron gain enthalpy becomes _____ with increase in atomic number across a period

Back 63

More negative

Front 64

Cl has -349 ∆Hege . What does negative sign means

Back 64

When an electron is added to the atom enthalpy is negative

Front 65

Cl has -349 ∆Hege. What does the magnitude represent

Back 65

The high magnitude represents the tendency to gain electron

Front 66

What is the general rule which can be applied for electron gain enthalpy

Back 66

Enthalpy is negative when an electron is added

Front 67

When does an atom has positive electron gain enthalpy

Back 67

When it does not want to add electron , eg: noble gas

Front 68

The positive and electron gain enthalpy indicates

Back 68

The tendency with which an electron is repelled

Front 69

The high value of electron gain enthalpy indicates

Back 69

Height of Desire

Front 70

The effective nuclear charge ____ from left to right across a period

Back 70

Increases

Front 71

Due to increased effective nuclear charge it will be ____ to add an electron to _____ atom because the added electron on an average would be closer to the positively charged _____

Back 71

Easier, smaller, nucleus

Front 72

Electron gain enthalpy becomes _____ as we go down a group

Back 72

Less negative

Front 73

The electron gain enthalpy of oxygen or fluorine is ______ than that of the succeeding element because of significant ____ .

Back 73

Less negative, repulsion

Front 74

The negative of electron gain enthalpy is defined as

Back 74

Electron affinity

Front 75

Electron affinity is defined as

Back 75

Absolute zero

Front 76

Give the relation between electron gain enthalpy and electron affinity

Back 76

Front 77

Back 77

Front 78

Electronegativity is a _____ measure

Back 78

Qualitative

Front 79

Electronegativity is a measurable quantity. T/F

Back 79

F.

Electronegativity is not a measurable quantity

Front 80

Mulliken-Jaffe scale is applicable to _____

Back 80

Electronegativity

Front 81

Allred - Rochow scale is related to

Back 81

Electronegativity

Front 82

Why does the magnitude of electron gain enthalpy decreases down the group

Back 82

Because down the group the size of the atom increase and the added electrons would be farther from the nucleus

Front 83

The magnitude of electron gain enthalpy ______ down the group

Back 83

Decreases

Front 84

The electronegativity of any given element is _____ .

Back 84

Not constant

Front 85

Electronegativity depends on the ____ to which it is bound

Back 85

Element

Front 86

Elements have constant electronegativity

Back 86

False

Front 87

Electronegativity is a measurable quantity

Back 87

False

Front 88

Electronegativity is not a _____ quantity

Back 88

Measurable

Front 89

_____ provides a mean of predicting the nature of force that holds a pair of atoms together

Back 89

Electronegativity

Front 90

The electronegativity of any given element is

Back 90

Variable

Front 91

Electronegativity generally increases across a period from

Back 91

Left to right

Front 92

Electronegativity value _____ with the increase in atomic radii down a group.

Back 92

Decreases

Front 93

The trend of electronegativity is similar to

Back 93

Ionization enthalpy

Front 94

Electronegativity is directly related to _____ property of the element

Back 94

Non metallic

Front 95

Electronegativity is ______ related to the metallic properties of elements

Back 95

Inversely

Front 96

Increase in electronegativities across a period is accompanied by _______ in non metallic properties

Back 96

Increase

Front 97

Decrease in electronegativities down a group is accompanied by

Back 97

Increase in metallic properties

Front 98

Give the electronegativity of

Back 98

Front 99

Give the electronegativity of

Back 99

Front 100

Give electronegativity of

Back 100

Front 101

Give electronegativity of

Back 101

Front 102

The _____ is the most characteristic property of the element

Back 102

Valence

Front 103

In OF2 molecule oxygen ____ two electrons with fluorine atoms

Back 103

Shares

Front 104

Oxidation state is defined as the charge acquired by its atom on the basis of _____ consideration from other atoms in the molecule

Back 104

Electronegative

Front 105

Back 105

Front 106

Give the number of valence electron

Back 106

Front 107

Give the valence of

Back 107

Front 108

There are many elements which exhibit variable valence. This is particularly characteristic of _____ elements and _____ .

Back 108

Transition, actinoides

Front 109

Lithium shows diagonal relationship with

Back 109

Magnesium

Front 110

Beryllium shows diagonal relationship with

Back 110

Aluminium

Front 111

The maximum covalency of the first member of each group is

Back 111

4

Front 112

The first member of p block elements displays greater ability to form _______ multiple bonds to itself and to the other ___ period elements.

Back 112

Pπ-pπ, second

Front 113

Give the order of metallic radius of Lithium and magnesium

Back 113

Mg>Li

Front 114

Give the order of Ionic radius of Lithium and magnesium ion

Back 114

Li+>Mg+

Front 115

Back 115

Front 116

The chemical reactivity at the two _____ is highest and the lowest in the _____ .

Back 116

Extremes, centre

Front 117

The metallic character ___ while the non metallic characters ____ while moving from left to right across the period

Back 117

Decreases, increases

Front 118

Oxides of elements in the centre are ____ or ____

Back 118

Amphoteric , neutral

Front 119

As2O3 is _____ in nature

Back 119

Amphoteric

Front 120

Give example of neutral oxides

Back 120

CO

NO

N2O

Front 121

Give the nature of N2O

Back 121

Neutral

Front 122

Back 122

Front 123

Transition metals are _____ electropositive than first and second group metals

Back 123

Less,

Front 124

Who was the first to consider the idea of trends among properties of elements

Back 124

Johann dobereiner

Front 125

Give the group one triad of Dobereiner's triad

Back 125

Li Na K

Front 126

Give the group two triad of Dobereiner's triad

Back 126

Ca Sr Ba

Front 127

Give the group 17 triad of Dobereiner's triad

Back 127

Cl Br I

Front 128

What comment did the dobereiner passed on the triads

Back 128

Properties of the middle element was in between those of the other two members

Front 129

Who arranged the then known elements in order of increasing atomic weights

Back 129

Chancourtois

Front 130

Who made a cylindrical table of elements to display the periodic reference of properties

Back 130

Chancourtois

Front 131

Law of triods was given in

Back 131

Early 1800s(1829)

Front 132

Law of octaves was given in

Back 132

1865

Front 133

Who gave law of octaves

Back 133

Newland

Front 134

Law of octaves seemed to be true only for elements up to

Back 134

Calcium

Front 135

Who was awarded the davy medal in 1887

Back 135

Newland

Front 136

Dimitri mendeleev

Back 136

1834 to 1907

Front 137

Lothar Meyer

Back 137

1830- 1895

Front 138

Who is generally credited with the development of modern periodic table

Back 138

Dimitri mendeleev

Front 139

Who plotted various physical properties against atomic weight to obtain a periodically repeated pattern

Back 139

Meyer