Question

4 니 (c) 3 (6) Ar (c) Kr (2) Ne 4. Number of electrons lost by atoms of group IIIA equals: (a) (b) 2. (d) 4 5. Atom which loses two electrons from its outer shell to form ion is called (a) oxygen (b) potassium (c) magnesium (d) carbon 6. In NaCl crystal lattice each Na ion is surrounded by: (a) 6 CI ions (b) 6 Na ions (c) 8 Cl ions (d) 12 Clions 7. At room temperature most of ionic compounds are: (a) amorphous solids (b) crystalline solids​

Answer 1

Answer:

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Answer 2

Answer:

4. Number of electrons lost by atoms of group IIIA equals: (c) 3

5. Atom which loses two electrons from its outer shell to form an ion is called (c) magnesium

6. In NaCl crystal lattice each Na ion is surrounded by:  (a) 6 CI ions

7. At room temperature most of ionic compounds are: (b) crystalline solids​

Explanation:

The number of electrons lost by atoms of group IIIA equals 3

• Group 3A is the boron group.
• The group 3A elements are also referred as earth metals.
• These elements have 3 valence electrons.
• So, to attain stability, IIIA elements lose 3 electrons.

The atom which loses two electrons from its outer shell to form an ion is magnesium.

• From the given elements, oxygen has 6 valence electrons, carbon has 4 valence electrons, magnesium has 2 valence electrons, and potassium has 3 valence electrons.
• To attain stability, oxygen takes 2 electrons, carbon either takes or loses 4 electrons, and potassium loses 3 three electrons.
• Magnesium having 2 valence electrons, loses both these electrons to form an ion.

In a NaCl crystal lattice, each Na ion is surrounded by 6 Cl ions.

• Sodium atom has 1 valence electron. It loses this electron to attain a stable electronic configuration and forms a sodium cation $Na^{+}$.
• Chlorine atom has 7 valence electrons. It captures one electron to attain a stable electronic configuration and forms a chlorine anion $Cl^{-}$.
• In the crystal structure, the anion $Cl^{-}$ and the cation $Na^{+}$ form a regular pattern alternating back and forth even in 3D.
• Because of this, each sodium ion is surrounded by six chloride ions.

At room temperature, most of the ionic compounds are crystalline solids.

• Since the electrostatic force of attraction between the elements is strong, ionic compounds are hard in nature.
• This gives such solids a definite shape and sharp melting point.
• Therefore, they are crystalline solids.

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