Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Which statement for NH3 and NF3 is false? Electronegativities: N = 3.0, H = 2.1, F = 4.0.a. The NF3 molecule is more polar than the NH 3 molecule. b. The bond angles in NF3 are smaller than those in N

Problem

Which statement for NH3 and NF3 is false? Electronegativities: N = 3.0, H = 2.1, F = 4.0.

a. The NF3 molecule is more polar than the NH 3 molecule. 

b. The bond angles in NF3 are smaller than those in NH3.

c. The bond dipoles in NF3 are directed toward the more electronegative fluorine atoms.

d. Both molecules have one unshared pair of electrons in the outer shell of nitrogen.

e. Both are sp3 hybridized at nitrogen. 

f. The bond dipoles in NF3 oppose the effect of the unshared pair of electrons. 

g. The nitrogen atom can be described as utilizing sp3 hybrid orbitals in the nitrogen trifluoride molecule. 

h. The bond dipoles of NF3 are directed toward fluorine, whereas those in NH 3 are directed toward nitrogen.

Solution

We are being asked to determine the false statements for NH3 and NF3.


In order to answer each statement, we need to determine first the Lewis structures of both structures, and their geometries.


We determine the Lewis structures with the following steps:

Step 1: Determine the central atom in the structure.

Step 2: Calculate the total number of valence electrons present.

Step 3: Draw the Lewis structure for the molecule.


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