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Molarity
Preparing a solution
Dilution
Solubility rules
Complete & Net Ionic Equations
Colligative properties
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Heat Flow
Energy diagrams
Thermochemical equations
Heating/ Cooling curves
Specific Heat Capacity
Calorimetry
Hess's Law
Enthalpies of formation
Bond enthalpies
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Collision Theory
Rate Comparisons
Integrated Rate Law
Differential Rate Law
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Equilibrium
Equilibrium Expression
ICE Tables
Calculating K
K vs Q
Le Chatelier's Principle
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Definitions
Conjugate Acids & Base Pairs
Autoionization of water
pH Scale
Strong Acids/ Bases
Ka and Kb
Buffer
Titrations
Indicators
pH salts
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Entropy
Gibb's Free Energy
G and Temperature
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Oxidation numbers
Half Reactions
Balancing Redox reactions
Voltaic cells
Cell potential (standard conditions)
Cell potential (non-standard)
Electrolysis
Quantitative Electrochemistry
Covalent & Molecular Compound
Related Examples and Practice Problems
Additional Worked Out Examples/ Practice
Identifying classification types: Differentiation between elements, compounds or mixtures and homogeneous and heterogenous mixtures
Separation techniques: Selected and explaining limitation of appropriate separation
Relating Properties to Composition: Predicting classification based on descriptive properties
and more …
Topic Summary & Highlights
and Help Videos
Core Concept
Covalent compounds are substances formed by the sharing of electrons between nonmetals. Unlike ionic compounds, which involve the transfer of electrons, covalent compounds consist of molecules held together by strong covalent bonds.
Naming Covalent Compounds
Use prefixes to indicate the number of atoms for each element.
The first element keeps its full elemental name.
The second element takes its root name and ends with "-ide."
Omit "mono-" for the first element if there’s only one atom.
Examples:
CO: Carbon monoxide (not monocarbon monoxide)
CO₂: Carbon dioxide
PCl₅: Phosphorus pentachloride
N₂O₄: Dinitrogen tetroxide
Write Formula of Covalent Compounds
Identify the elements in the compound.
Use prefixes to determine the number of atoms for each element.
Write the formula by listing the elements and using subscripts to show the number of atoms for each element (based on the prefixes).
Example:
Dinitrogen trioxide: The prefix "di-" indicates two nitrogen atoms (N₂), and "tri-" indicates three oxygen atoms (O₃), so the formula is N₂O₃.
It is important to note that when writing the formula, the prefixes are not included for the first element if there is only one atom of that element. However, if there is more than one atom of the first element, the prefix "mono-" is used. The prefixes are always included for the second element.
Practice Tips
Memorize the Prefixes: Knowing the prefixes makes it easy to determine the number of atoms.
Check for Mono- Prefix: Only use “mono-” for the second element if there's only one atom of that element.
Remember -ide Ending: The second element should always end with “-ide.”
