(a) Interpretation: The term valence electrons should be defined. Concept introduction: Valence electrons are electrons which are most like to involve in a chemical reaction .
(a) Interpretation: The term valence electrons should be defined. Concept introduction: Valence electrons are electrons which are most like to involve in a chemical reaction .
Solution Summary: The author explains the meaning of valence electrons, which are located at outermost shell of an atom.
Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.
Chapter 10, Problem 131SAE
Interpretation Introduction
(a)
Interpretation:
The term valence electrons should be defined.
Concept introduction:
Valence electrons are electrons which are most like to involve in a chemical reaction.
Interpretation Introduction
(b)
Interpretation:
The term electronegativity should be defined.
Concept introduction:
Electronegativity of an atom is affected by both its atomic number and the size of the atom.
Interpretation Introduction
(c)
Interpretation:
The term bond dissociation energy should be defined.
Concept introduction:
Bond dissociation energy is the measure of the strength of a chemical bond.
Interpretation Introduction
(d)
Interpretation:
The term double covalent bond should be defined.
Concept introduction:
Covalent bonding is the sharing of electrons between two atoms. There are three types of covalent bonds such as single, double and triple bonds.
Interpretation Introduction
(e)
Interpretation:
The term coordinate covalent bond should be defined.
Concept introduction:
A coordinate covalent bond is a kind of 2-center, 2-electrons covalent bond.
3)
The molecule diphosphorus tetraoxide (P,O,) has two central atoms and four different resonance
structures that do not violate the octet rule. Draw two of these resonance structures below.
4)
The compound acetone is a common solvent. It has a chemical formula of CH,COCH, Acetone has
three central atoms.
(a) Draw the Lewis Dot structure for acetone.
(b) Give the Ideal Bond Angle for all three central atoms.
5)
Four covalent molecules are drawn below.
:o:
H.
H-CH
H
H
(1)
(2)
(3)
(4)
a)
Define each of these molecules as polar or non-polar.
(1)
(2)
(3)
b)
Describe the type of intermolecular force that each molecule would use:
(1)
(2)
(3)
(4)
Write Lewis structures for the following: (c) C2F6 (contains a C¬C bond), (d) AsO3 3 -, (e) H2SO3 (H is bonded to O), (f) NH2Cl..
Arrange the bonds in each of the following sets in order of increasing polarity: (a) C¬F, O¬F, Be¬F; (b) O¬Cl, S¬Br, C¬P; (c) C¬S, B¬F, N¬O.
What is the Lewis symbol for each of the following atoms or ions? (a) K, (b) As, (c) Sn2 + , (d) N3
Write electron configurations for the following ions and determine which have noble-gas configurations: (a) Cd2+, (b) P3-, (c) Zr4+
Although I3- is a known ion, F3- is not. (a) Draw the Lewis structure for I3- (it is linear, not a triangle). (b) One of your classmates says that F3 - does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says F3- does not exist because it would violate the octet rule.Is this classmate possibly correct? (d) Yet another classmatesays F3- does not exist because F is too small to make bonds tomore than one atom. Is this classmate possibly correct?
Chapter 10 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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