Electrovalent Bonding Of Metals Test


15 Questions MCQ Test Science Class 10 | Electrovalent Bonding Of Metals Test


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This mock test of Electrovalent Bonding Of Metals Test for Class 10 helps you for every Class 10 entrance exam. This contains 15 Multiple Choice Questions for Class 10 Electrovalent Bonding Of Metals Test (mcq) to study with solutions a complete question bank. The solved questions answers in this Electrovalent Bonding Of Metals Test quiz give you a good mix of easy questions and tough questions. Class 10 students definitely take this Electrovalent Bonding Of Metals Test exercise for a better result in the exam. You can find other Electrovalent Bonding Of Metals Test extra questions, long questions & short questions for Class 10 on EduRev as well by searching above.
QUESTION: 1

Among the following, ionic compound is formed between:

Solution:
QUESTION: 2

The electrovalent compounds are formed by the transfer of electrons from:

Solution:

An electrovalent bond is formed when a metal atom transfers one or more electrons to a non metal atom and these compounds are called ionic compounds.

QUESTION: 3

Which of the following element has a tendency to gain electrons?

Solution: It has 7 electrons in their outer most shell so, to complete its octane it gain one electron.
QUESTION: 4

What are the ions present in NaCl?

Solution:

The ions present in NaCl is one ion of Na and one ion of Cl. So, option ( c) is the correct one.

QUESTION: 5

The electronic configuration of Phosphorus (atomic number 15) will be:

Solution:

We know phosphorus has atomic no. 15. Therefore it's electronic configuration is :- 2,8,5 , which means 2 electrons  in k- shell, 8 electrons in L-shell and 5 electrons in M - shell.

QUESTION: 6

Due to the presence of strong electrostatic forces of attraction between ions, ionic compounds:

Solution:

Ionic compounds have high boiling and melting points as they're very strong and require a lot of energy to break. 

QUESTION: 7

The valency of magnesium and chlorine in magnesium chloride is:

Solution:

Magnesium has electronic configuration 2,8,2 . It loses 2 electrons to complete octet configuration in its valence shell. Chlorine has electronic configuration 2,8,7 . It gains 1 electron to complete octet configuration in its valence shell. 

QUESTION: 8

Ionic bond involves:

Solution:
QUESTION: 9

The compounds formed when metals react with non-metals are:

Solution:
QUESTION: 10

The correct electronic configuration for sodium ion is:

Solution:

Atomic number of sodium is 11 so its electronic configuration will be 2, 8, 1. But sodium ion is formed by the loss of an electron so its electronic configuration is 2, 8.

QUESTION: 11

Ionic compounds are soluble in water but insoluble in kerosene because:

Solution:

Water is a polar covalent compound. It decreases the electrostatic forces of attraction,resulting in free ions in aqueous solution. Hence ionic compounds disslove in water. Kerosene is a non polar organic solvent and dissolves non polar covalent compounds.

QUESTION: 12

Valency of aluminium is:

Solution: Its atomic number is 13 hence its electronic configuration is 2,8,3. To complete the rule of octane it loses 3 electrons. Hence its valence is three.
QUESTION: 13

A solution of ionic compound conducts electricity due to the presence of:

Solution: A solution of ionic compound conducts electricity due to the presence of ions because they conatain charged particles . But ionic compound can only conduct electricity in its Aqueous Solution not in solid state. It conducts electricity when ions are free to move.
QUESTION: 14

Potassium chloride conducts electricity in _______ state.

Solution:

Potassium Chloride is an excellent water soluble crystalline Potassium source for uses compatible with chlorides.. Chloride compounds can conduct electricity when fused or dissolved in water. Chloride materials can be decomposed by electrolysis to chlorine gas and the metal.

QUESTION: 15

Which of the following will not conduct electricity?

Solution:

Solid NaCl does not conduct electricity due to absence of free ions.