The p-Block Elements Test

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The p-Block Elements Test - 59

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Question 1
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In the modern periodic table, elements are arranged in order of increasing atomic number which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz s, p, d and f. The modern periodic table consists of 7 periods and 18 groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle filling of a new energy shell. In accordance with the Aufbau principle, the seven period (1 to 7) have 2,8,8,18,18,32 and 32 elements respectively. The seventh period is still incomplete. To avoid the periodic table being too long, the two series of f - block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.
The elements with atomic number $$35,53$$ and $$85$$ are all ________.

A
Noble gases

B
Halogens

C
Heavy metals

D
Light metals

Solution
Question 2
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The table shows some information about elements in Group VII of the Periodic Table.
Name State at room temperature Colour
Chlorine Gas yellow-green
Bromine liquid brown
Iodine ? ?
Astaine solid black
Which information about iodine completes the table?

A
State - liquid, colour - black

B
State - liquid, colour - green

C
State - solid, colour - grey

D
State - solid, colour - yellow

Solution

$$\text{D) State-solid,Colour-yellow}$$
$$\text{Iodine is solid at room temperature and appears yellow in low concentrat}$$
Question 3
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Which oxide is insoluble in aqueous sodium hydroxide?

A
MgO

B
$$Al_2O_3$$

C
$$P_4O_{10}$$

D
$$SO_2$$

Solution

$$\text{MgO is insoluble in aqueous sodium hydroxide.}$$
Question 4
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Which of the following inert gas participate in chemical reaction?

A
$$Xe$$

B
$$He$$

C
$$Ne$$

D
None

Solution

Xenon participate in chemical reactions because ionising power of $$Xe$$ and oxygen are almost same and atomic size $$Xe$$ is large.
Question 5
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Nitrogen and phosphorus are both in Group 15 of the Periodic Table. Phosphorus forms a chloride with the formula $$P{Cl}_{5}$$ but nitrogen does not form $$N{Cl}_{5}$$.
Which statements help to explain this?
1. Nitrogen's outer shell cannot contain more than eight electrons.
2. Nitrogen cannot have an oxidation state of $$+5$$
3. Nitrogen is less electronegative than phosphorus.

A
1, 2 and 3 are correct

B
1 and 2 only are correct

C
2 and 3 only are correct

D
1 only is correct

Solution

Only highly electrnegative elements can make nitrogen exhibit +5 oxidation state

We know that, on going from top to bottom in a group, non- metalllic character decreases. The non- metallic character of any element is characterized by its tendency to lose electron i.e electronegativity.
Hence, electronegativity decreases on going from top to bottom in a group.
Therefore, Nitrogen is more electronegative than Phosphorus.

Also, Nitrogen is smaller in size as compared to Phosphorus. Due to its small size, the net electron charge increases. Hence, its nucleus exerts greater force on the electrons.
Thetefore, its tendency to gain electron is more as compared to that of Phosphorus.
That is the reason why, Nitrogen is more electronegative element than Phosphorus.
Question 6
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Which of the following order of acidic strength is correct?

A
$$HClO > HClO_{2} > HClO_{3} > HClO_{4}$$

B
$$HClO_{4} > HClO_{2} > HClO_{3} > HClO$$

C
$$HClO_{2} > HClO > HClO_{4} > HClO_{3}$$

D
$$HClO_{4} > HClO_{3} > HClO_{2} > HClO$$

Solution

Acidic strength will increase with an increase in the oxidation state of $$Cl$$ in its oxyacid.
Since the oxidation state of $$Cl$$ in $$HClO_4$$ is maximum followed by $$HClO_3,HClO_2,$$ and $$HClO$$.
THus option $$D$$ is correct.
Question 7
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The elements with atomic numbers 10, 18, 36, 54 and 86 are all:

A
light metals

B
inert gases

C
halogens

D
rare-earths

Solution

The atomic number given are 2, 10, 18, 36, 54, 86 which shows that these elements have completely filled orbitals and are noble gases or zero group members.

Option B is correct.
Question 8
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A radioactive halogen is:

A
polonium

B
radon

C
astatine

D
iodine

Solution

All elements with atomic numbers greater than 83 have unstable nuclei and are radioactive.

Astatine is a radioactive chemical element with the symbol At and atomic number 85.

Polonium and Radon are radioactive but they are not halogens and Iodine are not radioactive because its atomic number 53.

Hence, option C is correct.
Question 9
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Which of the block of elements does belong to inert gases?

A
s-block

B
p-block

C
d-block

D
f-block

Solution

Inert gases belong to 18th group of the periodic table which is in the p-block

Option B is correct.
Question 10
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How many electrons are present in the outermost orbit of halogens?

A
1

B
3

C
5

D
7

Solution

The general electronic configuration of halogens is $$ns^2np^5$$. Therefore, halogens have seven electrons in their outermost shell.

Therefore, option (D) is correct.

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Name	State at room temperature	Colour
Chlorine	Gas	yellow-green
Bromine	liquid	brown
Iodine	?	?
Astaine	solid	black

The p-Block Elements Test - 59

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The p-Block Elements Test - 59

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Question 1

Noble gases

Halogens

Heavy metals

Light metals

Solution

Question 2

State - liquid, colour - black

State - liquid, colour - green

State - solid, colour - grey

State - solid, colour - yellow

Solution

Question 3

MgO

$$Al_2O_3$$

$$P_4O_{10}$$

$$SO_2$$

Solution

Question 4

$$Xe$$

$$He$$

$$Ne$$

None

Solution

Question 5

1, 2 and 3 are correct

1 and 2 only are correct

2 and 3 only are correct

1 only is correct

Solution

Question 6

$$HClO > HClO_{2} > HClO_{3} > HClO_{4}$$

$$HClO_{4} > HClO_{2} > HClO_{3} > HClO$$

$$HClO_{2} > HClO > HClO_{4} > HClO_{3}$$

$$HClO_{4} > HClO_{3} > HClO_{2} > HClO$$

Solution

Question 7

light metals

inert gases

halogens

rare-earths

Solution

Question 8

polonium

radon

astatine

iodine

Solution

Question 9

s-block

p-block

d-block

f-block

Solution

Question 10

1

3

5

7

Solution

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