Formula of binary hydride for the second period elements from L i to F have to be written. The change from ionic character to covalent character of these compounds has to be discussed given that beryllium behaves differently from the rest of the group 2A metals. Concept Introduction: Ionic bond is the electrostatic force of attraction that binds ions of opposite charges into a stable molecule. Compounds formed of ions and bound by ionic bond are called ionic compounds. Covalent bond refers to the bond formed between two atoms by mutual sharing of electrons – that each atom shares equal number of electrons between them and the charge distribution (electron) between the two atoms held by covalent bond is symmetrical. Such compounds are called covalent compounds . Polar covalent bond refers to the covalent bond which has polarity caused by unsymmetrical distribution of bonding electrons between the two atoms. When atoms of moderately different electronegativity bonded by mutual sharing of electrons, the atom having more electronegativity tend to pull the electron cloud towards it. This leads to unsymmetrical distribution of electrons between the bonded atoms that one end of the molecule develops slight positive charge and another end of the molecule develops slight negative charge. This is called polarity and such bond is called polar covalent bond. Electronegativity difference between the atoms must be 1.7 or nearer to 1.7 to form polar covalent bond between these atoms.
Formula of binary hydride for the second period elements from L i to F have to be written. The change from ionic character to covalent character of these compounds has to be discussed given that beryllium behaves differently from the rest of the group 2A metals. Concept Introduction: Ionic bond is the electrostatic force of attraction that binds ions of opposite charges into a stable molecule. Compounds formed of ions and bound by ionic bond are called ionic compounds. Covalent bond refers to the bond formed between two atoms by mutual sharing of electrons – that each atom shares equal number of electrons between them and the charge distribution (electron) between the two atoms held by covalent bond is symmetrical. Such compounds are called covalent compounds . Polar covalent bond refers to the covalent bond which has polarity caused by unsymmetrical distribution of bonding electrons between the two atoms. When atoms of moderately different electronegativity bonded by mutual sharing of electrons, the atom having more electronegativity tend to pull the electron cloud towards it. This leads to unsymmetrical distribution of electrons between the bonded atoms that one end of the molecule develops slight positive charge and another end of the molecule develops slight negative charge. This is called polarity and such bond is called polar covalent bond. Electronegativity difference between the atoms must be 1.7 or nearer to 1.7 to form polar covalent bond between these atoms.
Solution Summary: The author explains the formula of binary hydride for the second period elements from Li to F and the change from ionic character to covalent character of these compounds.
Formula of binary hydride for the second period elements from Li to F have to be written. The change from ionic character to covalent character of these compounds has to be discussed given that beryllium behaves differently from the rest of the group 2A metals.
Concept Introduction:
Ionic bond is the electrostatic force of attraction that binds ions of opposite charges into a stable molecule. Compounds formed of ions and bound by ionic bond are called ionic compounds.
Covalent bond refers to the bond formed between two atoms by mutual sharing of electrons – that each atom shares equal number of electrons between them and the charge distribution (electron) between the two atoms held by covalent bond is symmetrical. Such compounds are called covalent compounds.
Polar covalent bond refers to the covalent bond which has polarity caused by unsymmetrical distribution of bonding electrons between the two atoms. When atoms of moderately different electronegativity bonded by mutual sharing of electrons, the atom having more electronegativity tend to pull the electron cloud towards it. This leads to unsymmetrical distribution of electrons between the bonded atoms that one end of the molecule develops slight positive charge and another end of the molecule develops slight negative charge. This is called polarity and such bond is called polar covalent bond.
Electronegativity difference between the atoms must be 1.7 or nearer to 1.7 to form polar covalent bond between these atoms.
An ionic compound of formula XY2 (X = cation with two positive charges, Y = anion with one negative charge) has the following mass composition: Mg 10.9%, Cl 31.8%, O57.3%. (a) What is the chemical formula and name of the compound? (b) Give the most probable Lewis structure for the ions contained in the compound.
Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X.
The enthalpy of formation of MX2 is ΔHf∘=−975 kJ/mol.
The enthalpy of sublimation of MM is ΔHsub=133 kJ/mol.
The first and second ionization energies of MM are IE1=751 and IE2=1412
The electron affinity of X is Δ?EA=−323Kj/mol
The bond energy of X2 is BE=203 kJ/mol.
Determine the lattice energy of MX2.
Suppose a chemist discovers a new metallic element and names it "Xercisium" (Xr). Xr exhibits chemical behaviour similar to an alkaline earth.
Xr(s) + Cl2(g) → XrCl2(s)
Lattice energy for XrCl2
-2020. kJ/mol
First Ionization energy of Xr
500. kJ/mol
Second Ionization energy of Xr
950. kJ/mol
Electron affinity of Cl
-348.7 kJ/mol
Bond energy of Cl2
239 kJ/mol
Enthalpy of sublimation (atomization) of Xr
200. kJ/mol
Use the above data to calculate ΔH°f for Xercisium chloride.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell