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Very Short Question and Answers - How Do Metals and Non-Metals React

Q 1.
What is the main type of chemical bond formed when a metal reacts with a non-metal?

Ans:

An ionic bond (also called an electrovalent bond) is formed.

Q 2.
What happens to a metal atom during its reaction with a non-metal?

Ans:

The metal atom loses electrons to form a positively charged ion (cation).

Q 3.
What is the tendency of non-metals during reaction with metals?

Ans:

Non-metals tend to gain electrons to form negatively charged ions (anions).

Q 4.
Define cation with an example.

Ans:

A cation is a positively charged ion, e.g., Na⁺ formed when sodium loses one electron.

Q 5.
Define anion with an example.

Ans:

An anion is a negatively charged ion, e.g., Cl⁻ formed when chlorine gains one electron.

Q 6.
Write the reaction showing sodium atom forming a sodium ion.

Ans:

Na → Na⁺ + e⁻

Q 7.
How many electrons does Magnesium lose to achieve a stable configuration?

Ans:

Magnesium loses two electrons.

Q 8.
Show the reaction when Magnesium forms a magnesium ion.

Ans:

Mg → Mg²⁺ + 2e⁻

Q 9.
How does Chlorine become a chloride ion? Write the equation.

Ans:

Chlorine gains one electron: Cl + e⁻ → Cl⁻

Q 10.
What are the charges present in the ions formed by the reaction of metals and non-metals?

Ans:

Metals form positive ions (cations) and non-metals form negative ions (anions).

Q 11.
How do cations and anions combine to form ionic compounds?

Ans:

They are held together by electrostatic forces of attraction resulting in a neutral compound.

Q 12.
Write the chemical reaction for the formation of sodium chloride from sodium and chlorine.

Ans:

2Na + Cl₂ → 2NaCl

Q 13.
Name the products formed when magnesium reacts with oxygen.

Ans:

Magnesium oxide (MgO) is formed.

Q 14.
What is the formula of the ionic compound formed between calcium and chlorine?

Ans:

The formula is CaCl₂ (calcium chloride).

Q 15.
State one physical property of ionic compounds related to melting point.

Ans:

Ionic compounds have high melting and boiling points.

Q 16.
Why do ionic compounds conduct electricity in molten or dissolved form but not in solid state?

Ans:

Because ions are free to move in molten or dissolved state, but not in solid state.

Q 17.
How are the ions arranged in the structure of an ionic compound?

Ans:

They are arranged in a regular three-dimensional lattice pattern.

Q 18.
Give the electron configuration of sodium before and after it forms a Na⁺ ion.

Ans:

Before: 2,8,1; After losing one electron (Na⁺): 2,8

Q 19.
Explain with a chemical equation how potassium reacts with bromine.

Ans:

2K + Br₂ → 2KBr

Q 20.
What are the key steps when a metal and non-metal react to form an ionic compound?

Ans:

Step 1: Metal loses electrons (forms cation); Step 2: Non-metal gains electrons (forms anion); Step 3: Oppositely charged ions attract to form an ionic compound.

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