Write the condensed electron configuration for manganese (Mn, atomic number 25) and determine if it is paramagnetic.
The Nelson Chemistry 12 solutions manual provides step-by-step derivations. It doesn't just say "$\lambda = 450\text nm$." It shows the conversion factor $1\text m = 1 \times 10^9\text nm$ explicitly. This attention to detail in the solutions helps students practice "dimensional analysis," a skill that is non-negotiable for the rest of the course.
This is a typical "Chapter 1 Review" question from Nelson Chemistry 12.
| Concept | Definition | Example | |--------|------------|---------| | | Ability of an atom to attract electrons. Difference (ΔEN) predicts bond type: <0.5 non-polar covalent, 0.5-1.7 polar covalent, >1.7 ionic (approx.) | H₂O: ΔEN = 1.4 (polar covalent) | | Polar Molecule | Molecule with a net dipole moment (asymmetric charge distribution). Must have polar bonds AND asymmetric shape. | H₂O (bent), NH₃ (trigonal pyramidal) | | Non-polar Molecule | No net dipole; either no polar bonds or symmetric shape. | CO₂ (linear), CCl₄ (tetrahedral) | | Hydrogen Bonding | Strongest IMF; H covalently bonded to F, O, or N attracts lone pair on another F, O, or N. | Between H₂O molecules | | London Dispersion Force | Temporary, instantaneous dipole; strength increases with # electrons & surface area. | Between noble gases, I₂, all molecules | | Network Covalent | Giant 3D lattice of covalent bonds; very high m.p., hard, insoluble, non-conductive (except graphite). | Diamond (C), silicon dioxide (SiO₂) | nelson chemistry 12 solutions chapter 1
The final section of the chapter transitions from structure to transformation. Solutions involve classifying and predicting the outcomes of several major reaction types: Addition Reactions:
Remember the "like dissolves like" rule. Polar functional groups increase solubility in water, while long carbon chains decrease it. Why Organic Chemistry Matters
This is a detailed study and solution guide for of the Nelson Chemistry 12 textbook (commonly used in Ontario, Canada). This guide focuses on the key concepts, provides step-by-step solutions to representative problems, and offers tips for mastering the material. This attention to detail in the solutions helps
Remember the rules:
Calculating the energy of an electron in a hydrogen atom using the Bohr model.
The central theme of Chapter 1 is the unique versatility of the carbon atom. Because carbon can form four stable covalent bonds, it creates a nearly infinite variety of structures, including long chains, rings, and complex branched networks. Solutions in this chapter heavily emphasize the IUPAC nomenclature system Difference (ΔEN) predicts bond type: <0
| Mistake | Correction | |---------|-------------| | Assuming all polar bonds = polar molecule | Check molecular symmetry (e.g., CCl₄ has polar bonds but is non-polar). | | Forgetting LDF exists in all molecules | When comparing molecules with similar dipole/H-bonding, compare LDF (molar mass/size). | | Thinking H-bonding = bond within a molecule | It is an force, not a bond inside one molecule. | | Equating melting point with bond strength only | For molecular compounds, melting point depends on IMF, not covalent bond strength. |
In previous grades, you learned that atomic radius decreases as you move right across a period. In Grade 12 Nelson Chemistry, you