# Chemical Periodicity Test 3

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:The element with quantum numbers $$n = 2,l = 1,m = 1,s = - 1/2$$ has the following position in the periodic table

Group VII-A, period II

Group 0, period II

Group VII-A, period III

Group 0, period III

## Questions 2 of 50

Question:Who developed the long form of periodic table

Lothar Meyer

Niels Bohr

Mendeleef

Moseley

## Questions 3 of 50

Question:Elements of atomic number 6 is placed in

IV group

IV period

VI group

III group

## Questions 4 of 50

Question:Which of the following elements is a lanthanide (Rare–earth element)

Californium

Cerium

Cesium

## Questions 5 of 50

Question:Which of the following dinegative anion is quite common

$${S^{2 - }}$$

$$S{e^{2 - }}$$

$$T{e^{2 - }}$$

$${O^{2 - }}$$

## Questions 6 of 50

Question:An element has electronic configuration $$1{s^2}2{s^2}2{p^6}3{s^2}3{p^4}$$. Predict their period, group and block

Period = 3rd, block = p, group = 16

Period = 5th, block = s, group = 1

Period = 3rd, block = p, group = 10

Period = 4th, block = d, group = 12

## Questions 7 of 50

Question:Mosley's name is most closely associated with the discovery of

Positron

Deutrons

Atomic number

Atomic weight

## Questions 8 of 50

Question:In the periodic table going down in fluorine group

Reactivity will increase

Electronegativity will increase

Ionization potential will increase

## Questions 9 of 50

Question:Alkali metals in each period have

Smallest size

Lowest ionization potential

Highest ionization potential

Highest electronegativity

## Questions 10 of 50

Question:The elements on the right side of the periodic table are

Metals

Metalloids

Non-metals

Transition elements

## Questions 11 of 50

Question:Who is called the father of chemistry

Priestley

Rutherford

Lavosier

## Questions 12 of 50

Question:The total number of rare–earth elements is

8

32

14

10

## Questions 13 of 50

Question:To which block is related an element having electronic configuration $$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^{10}}4{s^1}$$ in the periodic table

s – block

p – block

d – block

f – block

## Questions 14 of 50

Question:$$Ce - 58$$ is a member of

s-block elements

p-block elements

d-block elements

f-block elements

## Questions 15 of 50

Question:The nitride ion in lithium nitride is composed of

$$7P + 7e$$

$$10P + 7e$$

$$7P + 10e$$

$$10P + 10e$$

## Questions 16 of 50

Question:Which set has the same number of unpaired electrons in their ground state

$$C{l^ - },F{e^{3 + }},C{r^{3 + }}$$

$$N{a^ + }$$, $$M{g^{2 + }}$$, $$Al$$

$$Na,\,P,\,\,Cl$$

$$N,\,P,V$$

## Questions 17 of 50

Question:Of the following, the one with largest size is

$$C{l^ - }$$

$$Ar$$

$${K^ + }$$

$$C{a^{2 + }}$$

## Questions 18 of 50

$${K^ + }$$

$$N{a^ + }$$

$$L{i^ + }$$

$$B{e^{2 + }}$$

## Questions 19 of 50

Question:In $${K^ + }{F^ - }$$ ionic radius of $${F^ - }$$ is more while atomic radius of $${K^ + }$$ is

Less than $${F^ - }$$

More than $${F^ - }$$

Equal of $${F^ - }$$

None of these

## Questions 20 of 50

Question:Which one of the following species possesses maximum size

$$N{a^ + }$$

$${F^ - }$$

$$Ne$$

$${O^{2 - }}$$

## Questions 21 of 50

Question:Which statement is correct

## Questions 22 of 50

Question:Which of the following ion is the smallest ion

$$O_2^ +$$

$$O_2^ -$$

$${O_2}$$

$$O_2^{ - 2}$$

## Questions 23 of 50

Question:An atom of an element has electronic configuration 2, 8, 1. Which of the following statement is correct

The element's valency is 7

The element exists as a diatomic molecule

The element is of non-metallic nature

The element forms a basic oxide

## Questions 24 of 50

Question:Which of the following ions has the smallest radius

$$B{e^{2 + }}$$

$$L{i^ + }$$

$${O^{2 - }}$$

$${F^ - }$$

Point out the wrong statement :

## Questions 25 of 50

Directly proportional to effective nuclear charge

Directly proportional to square of effective nuclear charge

Inversely proportional to effective nuclear charge

Inversely proportional to square of effective nuclear charge.

## Questions 26 of 50

Question:Correct energy value order is

$$ns\;np\;nd(n - 1)f$$

$$ns\;np(n - 1)d\;(n - 2)f$$

$$ns\;np(n - 1)d\;(n - 1)f$$

$$ns(n - 1)d\;n(n - 1)f$$

## Questions 27 of 50

Question:Which of the following element has maximum, first ionisation potential

V

Ti

Cr

Mn

## Questions 28 of 50

Question:Highest energy will be absorbed to eject out the electron in the configuration

$$1{s^2}2{s^2}2{p^1}$$

$$1{s^2}2{s^2}2{p^3}$$

$$1{s^2}2{s^2}2{p^2}$$

$$1{s^2}2{s^2}2{p^4}$$

## Questions 29 of 50

Question:Which of the following elements has the lowest ionistion potential

N

O

F

Ne

## Questions 30 of 50

Question:Which of the following has lowest first ionisation potential

B

C

N

O

## Questions 31 of 50

Question:Which of the following order is wrong

$$N{H_3} < P{H_3} < As{H_3}$$-acidic nature

$$L{i^ + } < N{a^ + } < {K^ + } < C{s^ + }$$-ionic radius

$$A{l_2}{O_3} < MgO < N{a_2}O < {K_2}O$$-basic

$$Li < Be < B < C$$-1st ionisation potential

## Questions 32 of 50

Question:Which of the following has the least ionization potential

Lithium (Li)

Helium (He)

Nitrogen (N)

Zinc (Zn)

## Questions 33 of 50

Question:Which of the following species has lowest ionization potential

$$O$$

$${O_2}$$

$$O_2^ +$$

$$O_2^ -$$

## Questions 34 of 50

Question:Which of the following has minimum ionization energy

Ge

Se

As

Br

## Questions 35 of 50

Question:If the IP of $$Na$$ is 5.48 eV, the ionisation potential of $$K$$ will be

Same as that of $$Na$$

5.68 eV

4.34 eV

10.88 eV

## Questions 36 of 50

Question:Mg and Li are similar in their properties due to

Same e/m ratio

Same electron affinity

Same group

Same ionic potential

## Questions 37 of 50

Question:The electron affinity for the inert gases is

Zero

High

Negative

Positive

## Questions 38 of 50

Question:The electron affinities of halogens are $$F = 322$$, $$Cl = 349$$, $$Br = 324$$, $$I = 295kJ\,mo{l^{ - 1}}$$. The higher value for $$Cl$$ as compared to that of $$F$$ is due to

Weaker electron-electron repulsion in $$Cl$$

Higher atomic radius of $$F$$

Smaller electronegativity of $$F$$

More vacant P - subshell in $$Cl$$

## Questions 39 of 50

Question:Electron affinity is the lowest for

Nitrogen

Carbon

Oxygen

Sulphur

## Questions 40 of 50

Question:Which one of the elements has the maximum electron affinity

F

Cl

Br

I

## Questions 41 of 50

Question:Keeping in view the periodic law and the periodic table suggest which of the following elements should have the maximum electronegative character

P

As

Bi

Sb

## Questions 42 of 50

Question:The outermost electronic configuration of the most electronegative element is

$$n{s^2}n{p^3}$$

$$n{s^2}n{p^4}$$

$$n{s^2}n{p^5}$$

$$n{s^2}n{p^6}$$

## Questions 43 of 50

Question:The attraction that an atom exerts on a pair of electrons that are being shared between that atom and another atom to which it is bonded by a covalent bond is referred to as its

Electron affinity

Electronegativity

Ionisation energy

Valence

## Questions 44 of 50

Question:The electronegativity of the following elements increases in the order

C, N, Si, P

N, Si, C, P

Si, P, C, N

P, Si, N, C

## Questions 45 of 50

Question:The order in which the following oxides are arranged according to decreasing basic nature is

$$N{a_2}O,\,MgO,\,A{l_2}{O_3},\,CuO$$

$$MgO,\,A{l_2}{O_3},\,CuO,\,N{a_2}O$$

$$A{l_2}{O_3},\,MgO,\,CuO,\,N{a_2}O$$

$$CuO,\,N{a_2}O,\,MgO,\,A{l_2}{O_3}$$

## Questions 46 of 50

Question:Strongest reducing agent is

$$C{l_2}$$

$$C{l^ - }$$

$$B{r^ - }$$

$${I^ - }$$

## Questions 47 of 50

Question:The correct order of reactivity of halogen is

Flourine > bromine > chlorine > iodine

Flourine > chlorine > bromine > iodine

Iodine > bromine > chlorine > fluorine

Bromine > chlorine > flourine > iodine

## Questions 48 of 50

Question:Elements A and B with their respective electronic configurations $$3{d^{10}}\,4{s^1}$$ and $$4{d^{10}}\,5{s^1}$$ in their outermost shell are

Both non-metals

Both coinage metals

A is a non-metal and B is coinage metal

A is a coinage metal and B is non-metal

## Questions 49 of 50

Question:Which of the following electronic configurations in the outermost shell is characteristic of alkali metals

$$(n - 1)\,{s^2}{p^6},\,n{s^2}{p^1}$$

$$(n - 1)\,{s^2}{p^6}{d^{10}},\,n{s^1}$$

$$(n - 1)\,{s^2}{p^6},\,n{s^1}$$

$$n{s^2}{p^6}{d^1}$$

## Questions 50 of 50

Question:On moving down the group gradually increase