Which one is more covalent among NaCl and KCl and why?

Smaller the cation, greater is its polarizing power and hence larger is the covalent character. The covalent character decreases as the size of cation increases LiCl > NaCl > KCl > RbCl. Thus LiCl is more covalent than KCl and hence KCl is more soluble in water because of decreased covalent character.

Which bond is more ionic NaCl or KCl?

KCl is more ionic because the ionic character increases as down the group while decreases along the period in the periodic table. Also, the bonding in KCl is more ionic than in NaCl.

Is KCl more covalent?

Fajan’s rule states “Larger the cation size lesser is the covalent character.” $ A{g^ + } $ cation is generally bigger and larger than $ {K^ + } $ atoms. Hence $ KCl $ is more covalent than $ AgCl $ . Note: In covalent bonds, atoms share electrons, whereas in ionic bonds atoms transfer electrons.

Is NaCl most covalent?

For example, sodium (Na), a metal, and chloride (Cl), a nonmetal, form an ionic bond to make NaCl. In a covalent bond, the atoms bond by sharing electrons. Covalent bonds usually occur between nonmetals….Table 2.11.

Why melting point of NaCl is more than KCl?

Answer: NaCl has higher lattice enthalpy than KCl thus its melting point also becomes higher.

Which is more covalent NaBr or KCl?

Larger cation-smaller anion interaction gives more ionic character whereas smaller cation-larger anion interaction gives more covalent character. Thus the order of increasing ionic character is LiI < NaBr < KCl < CsF. Q3.

Is KCl stronger than NaCl?

Charge on the ions: Greater the charge on the ions greater will be lattice energy. Between NaCl and KCl ,NaCl is stronger than KCl .

Why is KCl more conductive than NaCl?

Explanation: which has higher molar conductivity hcl or nacl and why? H+ ion is smaller than Na+ ion due to which it moves faster. Hence, molar conductivity of HCl is higher than NaCl.

Which is more covalent KCl or AgCl?

Larger the cation size lesser the covalent character. Ag+ is larger than K+ so AgCl has less covalent character than KCl.

Does NaCl have covalent character?

Table salt, NaCl, is a good example of this type of compound. Ionic bonds differ from covalent bonds. All ionic bonds have some covalent character, but the larger the difference in electronegativity between the two atoms, the greater the ionic character of the interaction.

Is KCl more covalent than NaBr?

According to the statement above, in sodium chloride and sodium bromide, the cations are same, but the anions are different, as the size of the bromide ion is bigger than the size of the chloride ion, so it’s polarisability will be higher than the chloride ion and thus sodium bromide is more covalent than sodium …

Why NaCl has higher lattice energy than KCl?

(ii) K+ is larger than Na+ so NaCl has a higher lattice energy and a higher melting point than KCl. The Ag+ ion is intermediate in size between Na+ and K+.

Why does NaCl have a higher ionic character than KCl?

Nacl is much smaller then kcl and hence it’s more electronegative and electronegativity difference between Na and Cl is greater then K and Cl that leads to greater ionic character to nacl.. The hack this influencer used to break the private jet industry.

Why is KCl more soluble in water than LiCl?

Thus LiCl is more covalent than KCl and hence KCl is more soluble in water because of decreased covalent character. Please log in or register to add a comment.

Which is more covalent Na+ or nanacl?

Nacl is more covalent as per fajan rule. Fajan rule states that polarising power of cation is directly proportional to charge and inversely to volume. Here anion is same so we have to compare cation and Na+ is more covalent.

What is the covalency Order of LiCl NaCl KCl?

So, covalency order – LiCl>NaCl>KCL. For AgCl, Electronic configuration of Ag+ is – 4d 10 . It has d block which is poorly screaning power than s,p-block which cannot effectively screaning the outermost electrons and they feel stronger attractive force towards nucleous and make it smaller in size than Li+,Na+,k+.