Ch.8 - Periodic Properties of the ElementsWorksheetSee 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: How many orbitals are there in the third shell ( n=3)? Express your answer numerically as an integer. Show the orbital-filling diagram for N (nitrogen). Stack the subshells in order of energy, with th

Solution: How many orbitals are there in the third shell ( n=3)? Express your answer numerically as an integer. Show the orbital-filling diagram for N (nitrogen). Stack the subshells in order of energy, with th

Problem

How many orbitals are there in the third shell ( n=3)? Express your answer numerically as an integer.

 

Show the orbital-filling diagram for N (nitrogen). Stack the subshells in order of energy, with the lowest-energy subshell at the bottom and the highest-energy subshell at the top.

 

 

 

 

Show the orbital-filling diagram for S (sulfur). Stack the subshells in order of energy, with the lowest-energy subshell at the bottom and the highest-energy subshell at the top.

 

 

 

 

Show the orbital-filling diagram for Br (bromine). Stack the subshells in order of energy, with the lowest-energy subshell at the bottom and the highest-energy subshell at the top.

Solution

• At n =3 

3s, 3p, 3d (f doesn't start until n=4)
• 3s = orbital

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