Periodic Properties of Elements Test

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Periodic Properties of Elements Test - 4

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Weekly Quiz Competition

Question 1
1 / -0

Which element has the highest 1^st ionisation energy?

A
Na

B
O

C
Be

D
N

Solution

Nitrogen atom has stable electronic configuration due to half filled p subshell. So it will have very high value of the first electronic configuration.
Question 2
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The process requiring absorption of energy is

A
F → F^-

B
F → F⁺

C
Cl → Cl^-

D
O → O^-

Solution

Energy is required to release an electron from an atom. So F → F⁺ will require the absorption of energy.
Question 3
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Which of the following elements has the greatest tendency to lose electrons?

A
F

B
S

C
Fr

D
C

Solution

The tendency to lose electrons increases as we go down a group in the case of alkali metals. So, Fr has the highest tendency to lose electrons.
Question 4
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To which group of the periodic table does the element with electronic configuration 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 4d¹⁰, 5s², 5p³ belong?

A
13

B
12

C
15

D
17

Solution

Since this element contains five valence electrons, it belongs to group 15 of the periodic table.
Question 5
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Modern periodic table is based on the atomic numbers of elements. Which of the following experiments proved the significance of the atomic number?

A
Millikan\'s drop experiment

B
Moseley\'s work on X-ray spectra

C
Bragg\'s work on X-ray diffraction

D
Discovery of X-ray roentgen

Solution

Moseley was able to show that the frequencies of certain characteristic X-rays emitted from chemical elements are proportional to the square of a number which is close to the element\'s atomic number; a finding which supported van den Broek and Bohr\'s model of the atom in which the atomic number is the same as the number of positive charges in the nucleus of the atom.
Question 6
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Choose the correct increasing order of electronegativities of the corresponding elements.

A
C < N < Si < P

B
N < Si < C < P

C
Si < P < C < N

D
P < Si < N < C

Solution

Electronegativity increases on moving from left to right across a period and decreases on moving from top to bottom in a group in the periodic table. Hence, the correct order is Si < P < C < N.
Question 7
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Diagonal relationship in the periodic table is shown by the elements of

A
first and second periods

B
second and third periods

C
third and fourth periods

D
None of these

Solution

A diagonal relationship is said to exist between certain pairs of diagonally adjacent elements in the second and third periods of the periodic table.
Question 8
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Which of the following pairs contains an example of metalloid elements in the periodic table?

A
Sodium and potassium

B
Fluorine and chlorine

C
Calcium and magnesium

D
Boron and silicon

Solution

Boron and silicon are metalloid elements in the periodic table.
Question 9
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Iron triad of elements also contains

A
cobalt and nickel

B
manganese and chromium

C
palladium and platinum

D
platinum and iridium

Solution

Iron, nickel and cobalt make up the iron triad. They are called so because all the three have similar properties even though they are distinct elements.
Question 10
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Which of the following statements is correct?

A
The ionic radius of a metal is same as its atomic radius.

B
The ionic radius of a metal is greater than its atomic radius.

C
The ionic radius of non-metal is less than its atomic radius.

D
The ionic radius of a metal is less than atomic radius of parent atom.

Solution

The ionic radius of a metal is less than its atomic radius because metal forms positive ions due to low ionisation energy. Since positive ions are formed by loss of electrons from valence shells, but nuclear charge remains same, thus, the ionic radius of metal is smaller in size as compared to their source atom.
Question 11
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The decreasing order of the first ionisation energies of the following elements is

A
Li > Be > B > Cl

B
C > B > Be > Li

C
C > Be > B > Li

D
Be > B > Li > C

Solution

First ionisation energy decreases as the stability of the configuration after the loss of first electron increases. So, the correct decreasing order of first ionisation energies is C > Be > B > Li.
Question 12
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The following question has four choices out of which ONLY ONE is correct.

Which of the following orders of elements is correct in terms of decreasing ionization enthalpies?

A
Na > Li > H

B
H > Li > Na

C
Li > H > Na

D
Na > H > Li

Solution

Ionization energy decreases on moving down a group in the periodic table. This is due to increase in the size of the atoms on moving down the group.

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Periodic Properties of Elements Test - 4

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Periodic Properties of Elements Test - 4

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Question 1

Na

O

Be

N

Solution

Question 2

F → F-

F → F+

Cl → Cl-

O → O-

Solution

Question 3

F

S

Fr

C

Solution

Question 4

13

12

15

17

Solution

Question 5

Millikan\'s drop experiment

Moseley\'s work on X-ray spectra

Bragg\'s work on X-ray diffraction

Discovery of X-ray roentgen

Solution

Question 6

C < N < Si < P

N < Si < C < P

Si < P < C < N

P < Si < N < C

Solution

Question 7

first and second periods

second and third periods

third and fourth periods

None of these

Solution

Question 8

Sodium and potassium

Fluorine and chlorine

Calcium and magnesium

Boron and silicon

Solution

Question 9

cobalt and nickel

manganese and chromium

palladium and platinum

platinum and iridium

Solution

Question 10

The ionic radius of a metal is same as its atomic radius.

The ionic radius of a metal is greater than its atomic radius.

The ionic radius of non-metal is less than its atomic radius.

The ionic radius of a metal is less than atomic radius of parent atom.

Solution

Question 11

Li > Be > B > Cl

C > B > Be > Li

C > Be > B > Li

Be > B > Li > C

Solution

Question 12

Na > Li > H

H > Li > Na

Li > H > Na

Na > H > Li

Solution

F → F^-

F → F⁺

Cl → Cl^-

O → O^-