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Helium Neon Argon Chlorine Naphthalene (C10H8) Iodine Bromine Solid paraffin (C28H58) KCl Solid wax (C20H42) RbBr CsI Brass Quartz Diamond ------- Argon Solid Was (C20H42) Iodine KCI Brass
Bromine is a molecular compound Br2 and the intermolecular forces are london dispersion forces. Potassium chloride is an ionic compound forming a lattice with strong electrostatic forces holding the lattice together. Less thermal energy is required to shake solid Br2 apart than that required for KCl
MgCl2 because although K has a higher mass than Mg, the Mg compound with Cl has two atoms of Cl not one.
KCl
why kcl has less meting point than the nacl
Melting points: KCl: 770oC HCl: -114.22oC
KF has small size than KCl. So the packing of atoms / ions in KF is more than that in KCl. So a larger energy is needed to separate the atoms from solid state to liquid state and hence KF has higher melting point than KCl.
There is no reaction (decomposition) when KCl is heated, other than the melting of KCl, above its melting point.
To decrease melting point of NaCl
KCl is an ionic compound and glucose is a molecular compound. Ionic compounds have higher boiling points than molecular compounds.
KCl is an ionic substance (strong intermolecular forces) and CO2 is a non-polar covalent substance (weak intermolecular forces)
No, because neither of them sublimate at 760 torr (1 atm). They melt. You could separate them by melting point, as NaCl has a melting point of 801ºC, but KCl has a melting point of 770ºC.
1. Argon 2. Solid Wax (C20H42) 3. Iodine 4. KCl 5. Brass
If you melt the HCl, and it melts at the proper melting point for HCl, then it is a pure substance. If not, it has been mixed with something else, which has altered the purity of the HCl.
Helium Neon Argon Chlorine Naphthalene (C10H8) Iodine Bromine Solid paraffin (C28H58) KCl Solid wax (C20H42) RbBr CsI Brass Quartz Diamond ------- Argon Solid Was (C20H42) Iodine KCI Brass
kcl...more reactive
This can be rationalised by looking at the lattice energy. Using Madelungs method the smaller Na+ ion causes a stronger coulombic attraction making it harder to beak up the lattice and increasing the mp.