Which block contains metals, non-metals, and metalloids?

📚 Chapter: Classification of Elements and Periodicity in Properties

📘 Detailed Solution

🔵 Step 1: Identify the Blocks

The modern periodic table is divided into four blocks based on the subshell into which the differentiating electron enters:

Block	Groups	General Character
s-block	1–2	Mostly metals
p-block	13–18	Metals, non-metals & metalloids
d-block	3–12	Mostly metals
f-block	Lanthanoids & Actinoids	Metals

🟢 Step 2: The Correct Block

The p-block contains elements showing all three major categories:

⚙️
Metals 🌿
Non-metals 🔶
Metalloids

p-block → Metals + Non-metals + Metalloids

🟣 Examples from the p-Block

Category	Examples
Metals	Al, Ga, In, Sn, Pb, Bi
Non-metals	C, N, O, F, P, S, Cl
Metalloids	B, Si, Ge, As, Sb, Te

Thus, the p-block is unique because it includes elements with a wide range of metallic and non-metallic properties.

🎬 p-Block Property Zone

p-Block (Groups 13–18)

Al
Metal Si
Metalloid P
Non-metal Cl
Non-metal

↓

🎯 All three categories are found in the p-block.

🟠 Important Concept

The p-block extends from Group 13 to Group 18. It contains metals on the left side, metalloids near the zig-zag line, and non-metals mainly towards the right side.

Group 13–18 → p-block

✅ Final Answer

The p-block contains metals, non-metals, and metalloids.

Answer: p-block (Groups 13–18)

📝 20 MCQs with Answers

1. Which block contains metals, non-metals and metalloids?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

B) p-block

---

2. The p-block consists of which groups?

A) 1–2

B) 3–12

C) 13–18

D) 1–18

✅ Answer

C) 13–18

---

3. Which of the following is a p-block metal?

A) Na

B) Al

C) Fe

D) Ca

✅ Answer

B) Al

---

4. Which of the following is a p-block non-metal?

A) O

B) Fe

C) Na

D) Ca

✅ Answer

A) O

---

5. Which of the following is a p-block metalloid?

A) Si

B) Na

C) Fe

D) Mg

✅ Answer

A) Si

---

6. Which block contains Groups 3–12?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

C) d-block

---

7. Which block contains Groups 1 and 2?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

A) s-block

---

8. The lanthanoids belong to the:

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

D) f-block

---

9. Which block mainly contains transition metals?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

C) d-block

---

10. Boron is classified as a:

A) Metal

B) Non-metal

C) Metalloid

D) Noble gas

✅ Answer

C) Metalloid

---

11. Silicon belongs to which block?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

B) p-block

---

12. Which p-block group contains halogens?

A) Group 15

B) Group 16

C) Group 17

D) Group 18

✅ Answer

C) Group 17

---

13. Which p-block group contains noble gases?

A) Group 15

B) Group 16

C) Group 17

D) Group 18

✅ Answer

D) Group 18

---

14. Carbon is a:

A) Metal

B) Non-metal

C) Metalloid

D) Transition metal

✅ Answer

B) Non-metal

---

15. Which of the following is a p-block metal?

A) Pb

B) Fe

C) Zn

D) Na

✅ Answer

A) Pb

---

16. Which block is located mainly on the right side of the periodic table?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

B) p-block

---

17. The position of an element in a block is determined by:

A) Atomic mass

B) Differentiating electron

C) Number of neutrons

D) Density

✅ Answer

B) Differentiating electron

---

18. Which block contains the greatest variety of element types?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

B) p-block

---

19. Metalloids are mainly located near the:

A) Left edge

B) Centre only

C) Zig-zag line

D) Bottom only

✅ Answer

C) Zig-zag line

---

20. Which statement is correct?

A) p-block contains only metals

B) p-block contains only non-metals

C) p-block contains metals, non-metals and metalloids

D) p-block contains only noble gases

✅ Answer

C) p-block contains metals, non-metals and metalloids

Q1. Which block contains metals, non-metals and metalloids?

Solution: The p-block contains metals, non-metals and metalloids. It consists of Groups 13–18.

Q2. Give one example each of a metal, non-metal and metalloid from the p-block.

Solution: Metal – Al; Non-metal – O; Metalloid – Si.

Q1. Explain why the p-block contains different types of elements.

Solution:

1. The p-block contains Groups 13–18.
2. It includes metals, non-metals and metalloids.
3. Metallic character generally decreases from left to right across a period.

p-block → Metals + Metalloids + Non-metals

Q1. Compare the four blocks of the periodic table.

Block	Groups	Main Elements
s-block	1–2	Mostly metals
p-block	13–18	Metals, non-metals & metalloids
d-block	3–12	Transition metals
f-block	Lanthanoids & Actinoids	Inner transition metals

Q1. Describe the position and characteristics of the p-block elements.

Solution:

• The p-block is located on the right side of the periodic table.
• It includes Groups 13–18.
• The differentiating electron enters a p-subshell.
• It contains metals, non-metals and metalloids.
• It includes important families such as halogens and noble gases.

Therefore, the p-block shows the greatest variety of metallic and non-metallic character.

Q1. Explain the classification of elements into s-, p-, d- and f-blocks and identify the block containing metals, non-metals and metalloids.

Solution:

Elements are divided into four blocks according to the subshell into which the differentiating electron enters.

Block	Groups/Series	Characteristic
s-block	1–2	Mostly metals
p-block	13–18	Metals, non-metals & metalloids
d-block	3–12	Transition metals
f-block	Lanthanoids & Actinoids	Inner transition metals

Among these blocks, the p-block has the widest range of properties. Its elements include metals such as Al and Pb, metalloids such as B and Si, and non-metals such as C, N, O and Cl.

🎯 Final Answer:

The p-block (Groups 13–18) contains metals, non-metals and metalloids.

🎯 Quick Revision

Answer → p-block
Groups → 13–18
Contains → Metals + Non-metals + Metalloids
Example Metal → Al
Example Metalloid → Si
Example Non-metal → O

Identify the group of an element with the outer configuration ns 2 np 4 .

📚 Chapter: Classification of Elements and Periodicity in Properties

📘 Detailed Solution

🔵 Step 1: Identify the Outer Configuration

The given outer electronic configuration is:

ns²np⁴

Here, the valence shell contains:

ns² + np⁴

Therefore, the total number of valence electrons is:

2 + 4 = 6 valence electrons

🟢 Step 2: Determine the Group

For p-block elements, the general outer electronic configuration is:

ns²np¹ → Group 13
ns²np² → Group 14
ns²np³ → Group 15
ns²np⁴ → Group 16
ns²np⁵ → Group 17
ns²np⁶ → Group 18

Since the given configuration is ns²np⁴, the element belongs to Group 16.

🎬 Valence Electron Calculation

ns² + np⁴

↑↓ ↑↓ ↑ ↑

↓

2 + 4 = 6 Valence Electrons

⚡

6 Valence Electrons → Group 16

🟣 Step 3: Examples

Elements having outer configuration ns²np⁴ belong to Group 16.

Element	Outer Configuration	Group
Oxygen (O)	2s²2p⁴	16
Sulphur (S)	3s²3p⁴	16
Selenium (Se)	4s²4p⁴	16
Tellurium (Te)	5s²5p⁴	16

🟠 Important Rule

For p-block elements, if the outer configuration is ns²npˣ, the group number is:

Group Number = 10 + Total Valence Electrons

For ns²np⁴:

10 + (2 + 4) = 10 + 6 = 16

✅ Final Answer

An element with the outer electronic configuration ns²np⁴ belongs to Group 16 of the modern periodic table.

Example: Oxygen (2s²2p⁴)

📝 20 MCQs with Answers

1. The outer configuration ns²np⁴ belongs to which group?

A) Group 14

B) Group 15

C) Group 16

D) Group 17

✅ Answer

C) Group 16

---

2. How many valence electrons are present in ns²np⁴?

A) 4

B) 5

C) 6

D) 7

✅ Answer

C) 6

---

3. ns²np⁴ represents a:

A) s-block configuration

B) p-block configuration

C) d-block configuration

D) f-block configuration

✅ Answer

B) p-block configuration

---

4. Which element has the configuration 2s²2p⁴?

A) Carbon

B) Nitrogen

C) Oxygen

D) Fluorine

✅ Answer

C) Oxygen

---

5. Oxygen belongs to:

A) Group 14

B) Group 15

C) Group 16

D) Group 17

✅ Answer

C) Group 16

---

6. Sulphur has the outer configuration:

A) 3s²3p²

B) 3s²3p³

C) 3s²3p⁴

D) 3s²3p⁵

✅ Answer

C) 3s²3p⁴

---

7. Group 16 elements have how many valence electrons?

A) 4

B) 5

C) 6

D) 7

✅ Answer

C) 6

---

8. The p-block groups are:

A) 1–2

B) 3–12

C) 13–18

D) 1–18

✅ Answer

C) 13–18

---

9. The group number for ns²np¹ is:

A) 13

B) 14

C) 15

D) 16

✅ Answer

A) 13

---

10. The group number for ns²np² is:

A) 13

B) 14

C) 15

D) 16

✅ Answer

B) 14

---

11. The group number for ns²np³ is:

A) 14

B) 15

C) 16

D) 17

✅ Answer

B) 15

---

12. The group number for ns²np⁵ is:

A) 15

B) 16

C) 17

D) 18

✅ Answer

C) 17

---

13. The group number for ns²np⁶ is:

A) 16

B) 17

C) 18

D) 2

✅ Answer

C) 18

---

14. Which of the following belongs to Group 16?

A) N

B) O

C) F

D) Ne

✅ Answer

B) O

---

15. Group 16 is also known as:

A) Halogens

B) Chalcogens

C) Noble gases

D) Alkali metals

✅ Answer

B) Chalcogens

---

16. An element with 6 valence electrons in the p-block belongs to:

A) Group 14

B) Group 15

C) Group 16

D) Group 17

✅ Answer

C) Group 16

---

17. Which configuration represents a Group 16 element?

A) ns²np²

B) ns²np³

C) ns²np⁴

D) ns²np⁵

✅ Answer

C) ns²np⁴

---

18. Selenium belongs to:

A) Group 15

B) Group 16

C) Group 17

D) Group 18

✅ Answer

B) Group 16

---

19. The general valence configuration of Group 16 is:

A) ns²np²

B) ns²np³

C) ns²np⁴

D) ns²np⁵

✅ Answer

C) ns²np⁴

---

20. For p-block elements, the group number of ns²np⁴ can be found by:

A) 10 + 4

B) 10 + 6

C) 10 + 8

D) 18 + 6

✅ Answer

B) 10 + 6 = 16

Q1. Identify the group of an element having outer configuration ns²np⁴.

Solution: It has 6 valence electrons. Therefore, it belongs to Group 16.

Q2. Give one example of an element having the configuration ns²np⁴.

Solution: Oxygen has the configuration 2s²2p⁴ and belongs to Group 16.

Q1. Determine the group of an element with outer configuration ns²np⁴.

Solution:

1. Number of s electrons = 2.
2. Number of p electrons = 4.
3. Total valence electrons = 2 + 4 = 6.

Group = 10 + 6 = 16

Hence, the element belongs to Group 16.

Q1. Explain how the group of a p-block element is determined from its outer electronic configuration.

Solution:

Outer Configuration	Valence Electrons	Group
ns²np¹	3	13
ns²np²	4	14
ns²np³	5	15
ns²np⁴	6	16
ns²np⁵	7	17
ns²np⁶	8	18

Therefore, ns²np⁴ → Group 16.

Q1. Explain the relationship between the outer electronic configuration and group number for p-block elements.

Solution:

The general outer electronic configuration of p-block elements is ns²np¹–⁶. The number of valence electrons determines the group number.

Group Number = 10 + Number of Valence Electrons

For ns²np⁴:

10 + (2 + 4) = 16

Thus, an element having the outer configuration ns²np⁴ belongs to Group 16.

Q1. Explain in detail how the group of an element with outer configuration ns²np⁴ is determined.

Solution:

The given outer electronic configuration is:

ns²np⁴

The element is a p-block element because the last electron enters a p-subshell.

The number of electrons in the outer shell is:

2 + 4 = 6 valence electrons

For p-block elements, the group number is obtained by adding 10 to the number of valence electrons:

Group Number = 10 + 6 = 16

Therefore, the element belongs to Group 16. Examples include oxygen, sulphur, selenium and tellurium.

🎯 Final Answer:

ns²np⁴ → 6 valence electrons → p-block → Group 16.

🎯 Quick Revision

Outer Configuration = ns²np⁴
Valence Electrons = 2 + 4 = 6
Block = p-block
Group = 10 + 6 = 16
Example = Oxygen (2s²2p⁴)

How many elements are present in the 6th period of the periodic table?

📚 Chapter: Classification of Elements and Periodicity in Properties

📘 Detailed Solution

🔵 Step 1: Identify the 6th Period

The 6th period is the sixth horizontal row of the modern periodic table.

6th Period → Cs to Rn

🟢 Step 2: Count the Elements

The 6th period contains elements from atomic number 55 to 86.

86 − 55 + 1 = 32 elements

Therefore, the 6th period contains 32 elements.

🎬 6th Period – Element Count

Atomic Number 55 → 86

55
Cs 56
Ba 57
La 58
Ce 59
Pr 60
Nd

⋯

71
Lu 72
Hf 73
Ta 74
W 75
Re 76
Os

⋯

81
Tl 82
Pb 83
Bi 84
Po 85
At 86
Rn

🎯 Total = 32 Elements

🟣 Why does the 6th period contain 32 elements?

The 6th period involves the filling of the 6s, 4f, 5d and 6p subshells.

Subshell	Maximum Electrons
6s	2
4f	14
5d	10
6p	6
Total	32

2 + 14 + 10 + 6 = 32

🟠 Important Point

The Lanthanoids are associated with the 6th period. They are shown separately at the bottom of the periodic table to keep the main table compact.

6th Period → 32 Elements
Lanthanoids → 14 Elements

✅ Final Answer

The 6th period contains 32 elements.

It starts with Cesium (Cs, Z = 55) and ends with Radon (Rn, Z = 86).

📝 20 MCQs with Answers

1. How many elements are present in the 6th period?

A) 8

B) 18

C) 32

D) 36

✅ Answer

C) 32

---

2. The 6th period starts with:

A) Rb

B) Cs

C) Ba

D) Fr

✅ Answer

B) Cs

---

3. The 6th period ends with:

A) At

B) Xe

C) Rn

D) Og

✅ Answer

C) Rn

---

4. The atomic number of Cs is:

A) 54

B) 55

C) 56

D) 57

✅ Answer

B) 55

---

5. The atomic number of Rn is:

A) 84

B) 85

C) 86

D) 87

✅ Answer

C) 86

---

6. The 6th period belongs to which row?

A) 6th horizontal row

B) 6th vertical column

C) 5th horizontal row

D) 7th horizontal row

✅ Answer

A) 6th horizontal row

---

7. Which series is associated with the 6th period?

A) Actinoids

B) Lanthanoids

C) Halogens

D) Noble gases only

✅ Answer

B) Lanthanoids

---

8. The 6th period includes the filling of which subshell?

A) 4f

B) 3d

C) 5f

D) 4d only

✅ Answer

A) 4f

---

9. Maximum electrons in the 4f subshell are:

A) 2

B) 6

C) 10

D) 14

✅ Answer

D) 14

---

10. Which block contributes 14 elements to the 6th period?

A) s-block

B) p-block

C) d-block

D) f-block

✅ Answer

D) f-block

---

11. How many s-block elements are present in the 6th period?

A) 2

B) 6

C) 10

D) 14

✅ Answer

A) 2

---

12. How many d-block elements are present in the 6th period?

A) 2

B) 10

C) 14

D) 18

✅ Answer

B) 10

---

13. How many p-block elements are present in the 6th period?

A) 2

B) 6

C) 10

D) 14

✅ Answer

B) 6

---

14. The total number of elements in the 6th period can be calculated as:

A) 2 + 10 + 6

B) 2 + 14 + 10 + 6

C) 14 + 6

D) 2 + 14

✅ Answer

B) 2 + 14 + 10 + 6

---

15. Which element has atomic number 57?

A) La

B) Ce

C) Ba

D) Hf

✅ Answer

A) La

---

16. Which element has atomic number 72?

A) Ta

B) Hf

C) W

D) Lu

✅ Answer

B) Hf

---

17. Which noble gas is present at the end of the 6th period?

A) Xe

B) Rn

C) Kr

D) Og

✅ Answer

B) Rn

---

18. The 6th period is called a:

A) Short period

B) Long period

C) Very short period

D) Incomplete period

✅ Answer

B) Long period

---

19. The 6th period contains:

A) Only main-group elements

B) s, d, f and p-block elements

C) Only f-block elements

D) Only d-block elements

✅ Answer

B) s, d, f and p-block elements

---

20. The correct answer for the number of elements in the 6th period is:

A) 18

B) 24

C) 32

D) 36

✅ Answer

C) 32

Q1. How many elements are present in the 6th period?

Solution: The 6th period contains 32 elements, from Cs (Z = 55) to Rn (Z = 86).

Q2. Why does the 6th period contain 32 elements?

Solution: The 6th period involves the filling of 6s, 4f, 5d and 6p subshells. Their capacities are 2, 14, 10 and 6 respectively.

2 + 14 + 10 + 6 = 32

Q1. Explain the distribution of elements in the 6th period among different blocks.

Block	Number of Elements
s-block	2
f-block	14
d-block	10
p-block	6
Total	32

Q1. Explain why the 6th period is called a long period.

Solution:

1. The 6th period contains 32 elements.
2. It starts with Cs (Z = 55) and ends with Rn (Z = 86).
3. It includes the filling of the 4f subshell.
4. Therefore, it contains more elements than the short periods and is called a long period.

Q1. Describe the 6th period of the modern periodic table.

Solution:

The 6th period starts with Cesium (Cs, Z = 55) and ends with Radon (Rn, Z = 86). It contains a total of 32 elements.

Block	Subshell	Elements
s	6s	2
f	4f	14
d	5d	10
p	6p	6

2 + 14 + 10 + 6 = 32 elements

Q1. Explain in detail why the 6th period contains 32 elements.

Solution:

The number of elements in a period depends upon the number of electrons that can be accommodated in the subshells being filled during that period.

1️⃣ s-block

The 6s subshell can accommodate 2 electrons.

2️⃣ f-block

The 4f subshell can accommodate 14 electrons.

3️⃣ d-block

The 5d subshell can accommodate 10 electrons.

4️⃣ p-block

The 6p subshell can accommodate 6 electrons.

2 + 14 + 10 + 6 = 32 elements

Hence, the 6th period contains 32 elements.

Final Answer: The 6th period has 32 elements, from Cs (Z = 55) to Rn (Z = 86).

🎯 Quick Revision

6th Period = 32 Elements
Starts: Cs (Z = 55)
Ends: Rn (Z = 86)
6s = 2 | 4f = 14 | 5d = 10 | 6p = 6
Total = 2 + 14 + 10 + 6 = 32