Quiz about PERIODIC-TABLE IN GENERAL AWARENESS

Question 1

Among fluorine and chlorine the electron affinity of the latter is high. This is due toA. high electronegativity of fluorineB. low dissociation energy of fluorineC. due to small size repulsion between valence electrons and added electronD. small size of chlorine atom

Accepted Answer

NA

Question 2

`EA_(1)` values of the following elements has positive value (I) Be (II) Br (III) Mg (IV) Cl The correct answer isA. I and IIIB. II and IVC. I II and IIID. I II and IV

Accepted Answer

NA

Question 3

Which of the following is not the reason for the higher `EA_(1)` of halogens (I) high nuclear charge (II) larger atomic size (III) easy to get octet configuration `ns^(2)np^(6)` (IV) half filled p-orbitals The correct answer isA. I and IVB. I II and IIIC. II and IVD. II and III

Accepted Answer

NA

Question 4

Electronegativity is the property of an atom in a bonded molecule.

Accepted Answer

NA

Question 5

Which of the following will have almost positive `EA_(1)`A. ChlorineB. OxygenC. MagnesiumD. Sulphur

Accepted Answer

NA

Question 6

If electro negativity of x be 3.2 and that of y be 2.2 the percentage ionic character of xy isA. 19.5B. 18.5C. 9.5D. 29.5

Accepted Answer

NA

Question 7

The atomic radii of transition elements from Cr to Cu are almost equal becauseA. Increased effective nuclear charge is balanced by decreased screening effect of (n-1)d or bitals.B. Increased effective nuclear charge is balanced by increased screening effect of (n-1)d or bitalsC. Decreased effective nuclear charge is balanced by increased screening effect of (n-1)d orbitalsD. Decreased effective nuclear charge is balanced by decreased screening effect of (n-1)d orbitals

Accepted Answer

NA

Question 8

Nature of bond can be predicted on the basis of electronativity of bonded atoms greater difference in electronegativity (X) more will be the polarity of bond and polar bond are easily broken in polar solvent like water. For hydroxy acids `X_(0) - X_(A)` difference predict the nature of oxide formed by the element A. `|X_(0) - X_(A)| gt |X_(0) - X_(H)|` then `A-O-H` show basic nature `(NaOH)` `|X_(0) - X_(A)| lt |X_(0) - X_(H)|` then `A-O-H` show acidic nature `(H-O-CI)` With the help of EN values `[EN_(A) = 1.8 EN_(B) = 2.6 EN_(C) = 1.6 EN_(D) = 2.8]` answer the following questions for the compounds `HAO HBO HCO HDO`. Percentage ionic character of compound AB isA. `42.42%`B. `24.24%`C. `15.04%`D. None of these

Accepted Answer

NA

Question 9

Nature of bond can be predicted on the basis of electronativity of bonded atoms greater difference in electronegativity (X) more will be the polarity of bond and polar bond are easily broken in polar solvent like water. For hydroxy acids `X_(0) - X_(A)` difference predict the nature of oxide formed by the element A. `|X_(0) - X_(A)| gt |X_(0) - X_(H)|` then `A-O-H` show basic nature `(NaOH)` `|X_(0) - X_(A)| lt |X_(0) - X_(H)|` then `A-O-H` show acidic nature `(H-O-CI)` With the help of EN values `[EN_(A) = 1.8 EN_(B) = 2.6 EN_(C) = 1.6 EN_(D) = 2.8]` answer the following questions for the compounds `HAO HBO HCO HDO`. Compounds whose aqueous solution is basic and order of their basic strengthA. `AOH COH AOH lt COH`B. `HDO HBO HDO gt HBO`C. `AOH COH AOH gt COH`D. `HDO HBO HDO lt HBO`

Accepted Answer

NA

Question 10

Nature of bond can be predicted on the basis of electronativity of bonded atoms greater difference in electronegativity (X) more will be the polarity of bond and polar bond are easily broken in polar solvent like water. For hydroxy acids `X_(0) - X_(A)` difference predict the nature of oxide formed by the element A. `|X_(0) - X_(A)| gt |X_(0) - X_(H)|` then `A-O-H` show basic nature `(NaOH)` `|X_(0) - X_(A)| lt |X_(0) - X_(H)|` then `A-O-H` show acidic nature `(H-O-CI)` With the help of EN values `[EN_(A) = 1.8 EN_(B) = 2.6 EN_(C) = 1.6 EN_(D) = 2.8]` answer the following questions for the compounds `HAO HBO HCO HDO`. Compounds whose aqueous solution is acidic and order of their acidic strengthA. `AOH COH AOH lt COH`B. `HDO HBO HDO gt HBO`C. `AOH COH AOH gt COH`D. `HDO HBO HDO lt HBO`

Accepted Answer

NA

Question 11

The main group elements complete their elctron configuration using s and p electrons in the periodic table. These elements range from the most metallic to the most non-metallic with intermiediate properties of semi-metals in between . The elements which occur at the two extremes of the periodic table are highly reactive and therefore these highly reactive elements do not occur in free state they usually occur in the combined forms. A compound (i.e and oxide of metal) has an element in its lowest oxidation state. Then it will be A. highly acidicB. highly basicC. neutralD. half acidic half basic

Accepted Answer

NA

Question 12

The main group elements complete their elctron configuration using s and p electrons in the periodic table. These elements range from the most metallic to the most non-metallic with intermiediate properties of semi-metals in between . The elements which occur at the two extremes of the periodic table are highly reactive and therefore these highly reactive elements do not occur in free state they usually occur in the combined forms. Which of the following properties show opposite trend on moving along a period from left to right and from top to bottom in a group ?A. Atomic radius and electron gain enthalpy (negative value)B. Nuclear charge and ionisation enthalpyC. ionisation enthalpy and electron gain enthalpy (negative value)D. None of the above

Accepted Answer

NA

Question 13

The main group elements complete their elctron configuration using s and p electrons in the periodic table. These elements range from the most metallic to the most non-metallic with intermiediate properties of semi-metals in between . The elements which occur at the two extremes of the periodic table are highly reactive and therefore these highly reactive elements do not occur in free state they usually occur in the combined forms. Select the correct statement.A. Chemical reactively of the elements is generally less in the centre of a period.B. Most of the elements forming amphoteric oxides are placed in the centre of a period.C. Metallic character increases with increasing atomic number in a group where as decrease form left to right in a period.D. All of these

Accepted Answer

NA

Question 14

The periodicity is related to the electronic configuration. That is all chemical and phyical properties are a manifestation of the electronic configurfation of the elements. The atomic and ionic radii generally decrease in a preiod from left or right. As a consequence the ionisation enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words the ionisation enthalpy of the extreme left element in a period is the least and the electron left element on the extreme right is the highest negative. This results into high chemical reactivity at two extgremes and the lowest in the centre. Similarly down the group the increase in atomic and ionic radii result in gradual decrease (with excetption in some third period elements) in electron gain enthalpies in the case of main group elements . These properties can be related with the (i) reducing and oxidising behacviour of the elements (ii) metallic and no-metallic charcter of element (iii) acidic basic amphoteric and neutral character of the oxides of the elements. Among `Al_(2)O_(3) SiO_(2)P_(2)O_(3)` and `SO_(2)` the correct order of acid strenght is A. `B gt Al gt Mg gt K`B. `Al gt Mg gt B gt K`C. `Mg gt Al gt K gt B`D. `K gt Mg gt Al gt B`

Accepted Answer

NA

Question 15

If electro negativity of x be 3.2 and that of y be 2.2 the percentage ionic character of xy isA. `19.5`B. `18.5`C. `9.5`D. `29.5`

Accepted Answer

NA

Question 16

Sizes of the second and third row transition elements are almost the same because ofA. d- and f-orbitals do not shield the nuclear charge very effectivelyB. Lanthanide contractionC. Both are trueD. None

Accepted Answer

NA

Question 17

A correct variation in the electronegativity value of atoms isA. `F gt N lt O gt C`B. `F gt O gt N gt C`C. `F lt N lt O lt C`D. `F gt N gt O lt C`

Accepted Answer

NA

Question 18

The main group elements complete their elctron configuration using s and p electrons in the periodic table. These elements range from the most metallic to the most non-metallic with intermiediate properties of semi-metals in between . The elements which occur at the two extremes of the periodic table are highly reactive and therefore these highly reactive elements do not occur in free state they usually occur in the combined forms. Which of the following properties show opposite trend on moving along a period from left to right and from top to bottom in a group ?a)Atomic radius and electron gain enthalpy (negative value)b)Nuclear charge and ionisation enthalpyc)ionisation enthalpy and electron gain enthalpy (negative value)d)None of the aboveA. Atomic radius and electron gain enthalpy (negative value)B. Nuclear charge and ionisation enthalpyC. ionisation enthalpy and electron gain enthalpy (negative value)D. None of the above

Accepted Answer

NA

Question 19

The periodicity is related to the electronic configuration. That is all chemical and phyical properties are a manifestation of the electronic configurfation of the elements. The atomic and ionic radii generally decrease in a preiod from left or right. As a consequence the ionisation enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words the ionisation enthalpy of the extreme left element in a period is the least and the electron left element on the extreme right is the highest negative. This results into high chemical reactivity at two extgremes and the lowest in the centre. Similarly down the group the increase in atomic and ionic radii result in gradual decrease (with excetption in some third period elements) in electron gain enthalpies in the case of main group elements . These properties can be related with the (i) reducing and oxidising behacviour of the elements (ii) metallic and no-metallic charcter of element (iii) acidic basic amphoteric and neutral character of the oxides of the elements. Which of the following statement is incorrect?A. In general metallic character increases down the group and decrease across a period.B. In general reducing property decreases down the group and increases across a period.C. In general the oxide formed by the element on extreme right of the periodic table is the most acidic.D. Chemical reactivity of non-metals in terms of oxidisong power increases from nitrogen to fluroine across the period.

Accepted Answer

NA

Question 20

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. The correct order of the metallic character isA. `AI gt Mg gt Na gt Si`B. `Na gt Mg lt AI gt Si`C. `Na gt Mg gt AI gt Si`D. `AI gt Mg gt Si gt Na`

Accepted Answer

NA

Question 21

The correct order of variation in the sizes of atoms isA. `Be gt C gt F gt Ne`B. `Be lt C lt F lt Ne`C. `Be gt C gt F gt Ne`D. `F gt Ne gt Be gt C`

Accepted Answer

NA

Question 22

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary down the group the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. The correct order of the non-metallic character isA. `B gt Al gt Mg gt K`B. `Al gt Mg gt B gt K`C. `Mg gt Al gt K gt B`D. `K gt Mg gt Al gt B`

Accepted Answer

NA

Question 23

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. Considering the elements `B C N F` and `Si` the correct order of their non-metallic character isA. `B gt C gt Si gt N gt F`B. `Si gt C gt B gt N gt F`C. `F gt N gt C gt B gt Si`D. `F gt N gt C gt Si gt B`

Accepted Answer

NA

Question 24

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. Which of the following statements is correct?A. ionisation enthalpies of elements decrease along a period and increase along a group in Modern periodic table.B. In the `3^(rd)` period of Modern periodic table the two most reactive elements are sodium and fluorine.C. Fluorine has the least negative electron gain enthalpy among all halogens.D. Ionisation enthalpy of `Pb` is greater than that of `Sn`.

Accepted Answer

NA

Question 25

The term periodicity in the properties of element are arranged in the increasing order of their atomic numbers similar elementsA. Reoccur after a fixed intervalB. Reoccur after certain regular intervalC. Form vertical groupsD. Form horizontal rows

Accepted Answer

NA

Question 26

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary down the group the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. Which of the following statements is incorrect?A. Oxide of aluminium `(AI_(2)O_(3))` and arsenic `(As_(2)O_(3))` are amphotericB. Oxide of chlorine `(CI_(2)O_(7))` is less acidic than oxide of nitrogen `(N_(2)O_(5))`C. Oxide of carbon `(CO_(2))` is more acidic than oxide of silica `(SiO_(2))`.D. The correct increasing order of basic character of various oxides is `H_(2)O lt CuO lt MgO lt CaO`

Accepted Answer

NA

Question 27

The periodicity is related to the electronic configuration. That is all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary down the group the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour and also with metallic and non-metallic character respectively of the elements. The correct order of the non-metallic character isA. `B gt C gt Si gt N gt F`B. `Si gt Cgt B gt N gt F`C. `F gt N gt C gt B gt Si`D. `F gt N gt C gt Si gt B`

Accepted Answer

NA

Question 28

The following is the reason for the periodicity in the properties of elementsA. Similarity in atomic massB. Similarity in atomic numbersC. Similarity in outer electronic configurationD. Similarity in atomic radius

Accepted Answer

NA

Question 29

Which of these does not reflect the periodicity of the elements.A. Bonding behaviourB. Electro negativityC. Noble gasD. An alkali metal

Accepted Answer

NA

Question 30

The Lanthanide contraction is responsible for the fact thatA. Zr and Hf have same radiusB. Zr and Zn have the same oxidation stateC. Zr and Y have same radiusD. Zr and Nb have similar oxidation state

Accepted Answer

NA

Question 31

The Lanthanide contraction is responsible for the fact thatA. `Zr` and Y have almost the same radiusB. Zr and Nb have similar oxidation stateC. Zr and Hf have almost the same radiusD. Zr and Zn have the same oxidation state

Accepted Answer

NA

Question 32

CONSEQUENE OF LANTHANIDE CONTRACTIONA. Contraction of atom of lanthanum element due to poor shielding d-subshell electronB. Contraction of atom of lanthanum element due to high shielding of d-subshell electronC. Contraction of atom of elements after lanthanum due to poor shielding of f-subshell electronD. Contraction of atom of elements before lanthanum due to poor shielding of f-subshell electron.

Accepted Answer

NA

Question 33

The species having smallest ionic radius isA. `AI^(3+)`B. `Ba^(2+)`C. `K^(+)`D. `Mg^(2+)`

Accepted Answer

NA

Question 34

In the crystals of which of the following ionic compounds would you expect maximum distance between the centres of the cations and anion?A. `CsF`B. `CsI`C. `LiI`D. `LiF`

Accepted Answer

NA

Question 35

Electrons which have the highest penetrating power through lower orbits areA. p-electronsB. s-electronsC. d-electronsD. f-electrons

Accepted Answer

NA

Question 36

Atomic radii of fluorine atom and neon atom in angstrom units are respectively given byA)0.762 1.60B)1.60 1.60C)0.72 0.72D)1.600.762A. 0.762 1.60B. 1.60 1.60C. 0.72 0.72D. 1.600.762

Accepted Answer

NA

Question 37

Which one of the following statements is incorrect in relation to ionization enthalpy ?A. Ionization enthalpy increases for each successive electrons.B. The greatest increses in ionization enthalpy is experiencedd on removal of electron from core noble gas configurationC. End of valence electrons is marked by a big jump in ionization enthalpy .D. Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value.

Accepted Answer

NA

Question 38

Identify the incorrect order of first ionization energy.A. `Li gt Na gt K`B. `F gt CI gt I`C. `Be lt B lt C`D. `O lt N lt F`

Accepted Answer

NA

Question 39

The ionisation potential and electron affinity of an element X are 275 and 86 kcalmole. Then the electronegativity of X according to Mulliken scale isA. 4B. 3.5C. 2.8D. zero

Accepted Answer

NA

Question 40

In a compound XY the electronegativity difference between X and Y is greater than 1.7 then compound XY soluble inA. BenzeneB. `C Cl_(4)`C. `H_(2)O`D. `CS_(2)`

Accepted Answer

NA

Question 41

The stable oxide state of Thallium a III A group element isA. `+1`B. `+ 3`C. `- 3`D. `+ 5`

Accepted Answer

NA

Question 42

Nuclear charge actually experienced by an electron is termed as effective nuclear charge The effective nuclear `Z^(**)` actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is .`s gt p gt d gt f` (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with nucleus . It is thus evident that more is the shielding effect lesser is the effective nuclear charge and lesser is the ionizatio energy. Which of the following is not concerned to effective nuclear charge?A. Higher ionization potential of carbon than boronB. Higher ionization potential of magnesium than aluminiumC. Higher values of successive ionization energyD. Higher electronegativity of higher oxidation state

Accepted Answer

NA

Question 43

Nuclear charge actually experienced by an electron is termed as effective nuclear charge The effective nuclear `Z^(**)` actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is .`s gt p gt d gt f` (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with nucleus . It is thus evident that more is the shielding effect lesser is the effective nuclear charge and lesser is the ionizatio energy. In which of the following valence electron experience maximum effective nuclear charge?A. KB. GaC. SrD. N

Accepted Answer

NA

Question 44

Nuclear charge actually experienced by an electron is termed as effective nuclear charge The effective nuclear `Z^(**)` actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is .`s gt p gt d gt f` (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with nucleus . It is thus evident that more is the shielding effect lesser is the effective nuclear charge and lesser is the ionizatio energy. Ionization energy is not influenced by A. size of atomB. Effective nuclear chargeC. Electron present in inner shellD. Change in entropy

Accepted Answer

NA

Question 45

Which one of the following statements related to the modern periodic table is incorrect?A. The p-block has 6 columns because a maximum of 6 electrons can occupy all the orbitals in a p-subshell.B. The d-block has 8 colums because a maximum of 6 electrons can occupt all the orbitals in a p-subshell.C. Each block contains a number of columns equal to the number of electrons that can occupy that subshell.D. The block indicates value of Azimuthal quantum number `(l)` for the last subshell that received electrons in building up the electronic configuration.

Accepted Answer

NA

Question 46

Which of the following statement is incorrect ?A. Oxide of aluminium `(Al_(2)O_(3))` and arsenic `(As_(2)O_(3))` are amphoteric.B. Oxide of chlorine `(Cl_(2)O_(7))` is less acidic than oxide of nitrogen `(N_(2)O_(5))`.C. Oxide of carbon `(CO_(2))` is more acidic than oxide of silica `(SiO_(2))`.D. The correct increasing order of basic character of various oxides is `H_(2)O lt CuO lt MgO lt CaO`.

Accepted Answer

NA

Question 47

Which of the following statements is INCORRECT ?A. Generally the radius trend and the ionization energy trend across a period are opposites.B. metallic and covalent radii of potassium are `2.3A` and `2.03A` respectively.C. Amongst `Li^(-)Be^(-)` and `C^(-)Li^(-)` is least stable ion.D. Atomic and ionic radii of Niobium and Tantalum are almost same

Accepted Answer

NA

Question 48

The stable oxidation sate (+8) is exhibited byA. `Co` & `Ni`B. `Ru` & `Os`C. `Cl` & `I`D. `Te` & `I`

Accepted Answer

NA

Question 49

Xenon has an octet configuration in the valence shell but it shows variable valency with the highly electronegative elements like oxygen and fluorine. Comment.

Accepted Answer

NA

Question 50

Which of the following statement is incorrect?A. The tendency to attract bonded pair of electron in case of hybrid orbitals follow the order `sp gt sp^(2) gt sp^(3)`B. Alkali metals generally have negative value of electron gain enthalpy.C. `Cs^(+)(g)` release more energy upon gain of en electron than `CI(g)`.D. The electronegativity values for `2p`-series elements is less than that for `3p`-series elements on account of small size and high inter electronic repulsions.

Accepted Answer

NA

Explore topic-wise InterviewSolutions in .

Among fluorine and chlorine, the electron affinity of the latter is high. This is due toA. high electronegativity of fluorineB. low dissociation energy of fluorineC. due to small size repulsion between valence electrons and added electronD. small size of chlorine atom

`EA_(1)` values of the following elements has positive value (I) Be (II) Br (III) Mg (IV) Cl The correct answer isA. I, and IIIB. II and IVC. I, II and IIID. I, II and IV

Which of the following is not the reason for the higher `EA_(1)` of halogens (I) high nuclear charge (II) larger atomic size (III) easy to get octet configuration, `ns^(2)np^(6)` (IV) half filled p-orbitals The correct answer isA. I and IVB. I, II and IIIC. II and IVD. II and III

Electronegativity is the property of an atom in a bonded molecule.

Which of the following will have almost positive `EA_(1)`A. ChlorineB. OxygenC. MagnesiumD. Sulphur

If electro negativity of x be 3.2 and that of y be 2.2 , the percentage ionic character of xy isA. 19.5B. 18.5C. 9.5D. 29.5

If electro negativity of x be 3.2 and that of y be 2.2 , the percentage ionic character of xy isA. `19.5`B. `18.5`C. `9.5`D. `29.5`