Q. \( \text{NaCl} \) is what type of bond?

Q: What type of bond is \mathrm{NaCl} ?

\mathrm{NaCl} has an ionic bond. Electrons transfer from \mathrm{Na} to \mathrm{Cl} , forming \mathrm{Na^+} and \mathrm{Cl^-} electrostatic attraction.

Q: Why is \mathrm{NaCl} considered ionic instead of covalent?

\mathrm{Na} is a metal with low ionization energy, and \mathrm{Cl} is a nonmetal with high electron affinity. The large electronegativity difference favors electron transfer.

Q: What ions form when \mathrm{NaCl} dissolves or melts?

In aqueous solutions, \mathrm{NaCl} separates into \mathrm{Na^+} and \mathrm{Cl^-} . In molten \mathrm{NaCl} , ions can also move and conduct.

Q: What are the charges of the ions in \mathrm{NaCl} ?

\mathrm{Na} forms \mathrm{Na^+} and \mathrm{Cl} forms \mathrm{Cl^-} . The charges balance to give a neutral ionic compound.

Q: How does the electron configuration lead to bond formation in \mathrm{NaCl} ?

\mathrm{Na} is [\mathrm{Ne}]3s^1 and tends to form [\mathrm{Ne}] by losing one electron. \mathrm{Cl} is [\mathrm{Ne}]3s^2 3p^5 and gains one electron to become [\mathrm{Ar}] .

Answer

NaCl (nacl) is held together by an ionic bond. Sodium (Na) transfers an electron to chlorine (Cl), forming opposite charges \( \text{Na}^+ \) and \( \text{Cl}^- \), which attract electrostatically.

Detailed Explanation

\( \mathrm{NaCl} \) is held together by an ionic bond.

Here is how to tell:

Identify the ions formed.

Sodium loses one electron to become \( \mathrm{Na^+} \):

\( \mathrm{Na} \rightarrow \mathrm{Na^+} + \mathrm{e^-} \)

Chlorine gains one electron to become \( \mathrm{Cl^-} \):

\( \mathrm{Cl} + \mathrm{e^-} \rightarrow \mathrm{Cl^-} \)
Notice the attraction between opposite charges.

\( \mathrm{Na^+} \) and \( \mathrm{Cl^-} \) attract each other through electrostatic (Coulombic) forces.
Conclude the bond type.

This electron transfer and resulting attraction between ions defines an ionic bond.

Answer: \( \mathrm{NaCl} \) has an ionic bond.

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General Chemistry FAQs

What type of bond is \( \mathrm{NaCl} \)?

\( \mathrm{NaCl} \) has an ionic bond. Electrons transfer from \( \mathrm{Na} \) to \( \mathrm{Cl} \), forming \( \mathrm{Na^+} \) and \( \mathrm{Cl^-} \) electrostatic attraction.

Why is \( \mathrm{NaCl} \) considered ionic instead of covalent?

\( \mathrm{Na} \) is a metal with low ionization energy, and \( \mathrm{Cl} \) is a nonmetal with high electron affinity. The large electronegativity difference favors electron transfer.

What ions form when \( \mathrm{NaCl} \) dissolves or melts?

In aqueous solutions, \( \mathrm{NaCl} \) separates into \( \mathrm{Na^+} \) and \( \mathrm{Cl^-} \). In molten \( \mathrm{NaCl} \), ions can also move and conduct.

What are the charges of the ions in \( \mathrm{NaCl} \)?

\( \mathrm{Na} \) forms \( \mathrm{Na^+} \) and \( \mathrm{Cl} \) forms \( \mathrm{Cl^-} \). The charges balance to give a neutral ionic compound.

How does the electron configuration lead to bond formation in \( \mathrm{NaCl} \)?

\( \mathrm{Na} \) is \( [\mathrm{Ne}]3s^1 \) and tends to form \( [\mathrm{Ne}] \) by losing one electron. \( \mathrm{Cl} \) is \( [\mathrm{Ne}]3s^2 3p^5 \) and gains one electron to become \( [\mathrm{Ar}] \).

Is \( \mathrm{NaCl} \) ever considered covalent?

Mostly no. It is classified as ionic. However, real ionic solids can have slight polarization, but bonding is still primarily ionic.

What physical properties indicate \( \mathrm{NaCl} \) is ionic?

High melting point, solubility in water, and electrical conductivity when molten or dissolved indicate ionic bonding due to mobile ions.

NACL is an ionic compound.
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