Chemistry Naming Compounds and Writing Formulas
Page 1: Chemical Names and Formulas Overview
Overview of essential concepts in chemical nomenclature.
Metals and Non-Metals: Distinction between these categories.
Ions and Ionic Charges: Importance of understanding ion characteristics.
Types of Compounds: Differentiating between ionic and molecular compounds.
Systematic Names: Guidelines for writing names and formulas of compounds.
Page 2: Ions
Ions: Charged atoms that form through electron loss or gain.
Cations: Positively charged ions (e.g., Na+).
Anions: Negatively charged ions (e.g., Cl-).
Page 3: Ionic Charges (Groups 1-3)
Ionic Charges: Charge patterns in groups of the periodic table.
Group 1: +1 charge
Group 2: +2 charge
Group 13: +3 charge
Page 4: Ionic Charges (Groups 14-17)
Continued Ionic Charges:
Group 14: +4 or -4 charge
Group 15: -3 charge
Group 16: -2 charge
Group 17: -1 charge
Page 5: Chemical Formulas
Definition of Chemical Formula: Representation showing the kind and number of atoms in the smallest unit of a substance (e.g., NaCl).
Page 6: Ionic Compounds
Formula Units: The lowest whole number ratio of ions in an ionic compound.
Example: Na2Cl2 simplifies to NaCl.
Important note: There is no distinct molecule of NaCl due to its ionic nature.
Page 7: Writing Ionic Formulas
Balancing Charges: For ionic compounds:
If charges cancel: Write symbols directly (e.g., Na+ Cl- = NaCl).
If charges do not cancel, use criss-cross method for subscripts (e.g., Ca+2 Cl- = CaCl2).
Avoid moving the charge; only the number is transferred, omit writing the 1.
Page 8: Naming Compounds
Compound Classification: Understanding whether compounds are ionic or molecular is key to naming and writing formulas.
Page 9: Binary Ionic Compounds
Definition of Binary: Involves 2 elements.
Definition of Ionic: Involves a metal (cation) and a non-metal (anion).
Writing Formulas: Ensure charges balance for a neutral compound.
Page 10: Writing Formulas from Names
Name Structure:
1st word = Cation (metal).
2nd word = Anion (non-metal) with an "ide" ending.
Page 11: Examples of Binary Ionic Compounds
NaBr: Sodium Bromide
MgF2: Magnesium Fluoride
Page 12: More Example Binary Ionic Compounds
KCl: Potassium Chloride
Al2O3: Aluminum Oxide
Note: Anionic compound names end with "ide!"
Page 13: Naming with Transition Metals
Cation and Anion Structure:
Recognize the charge from the Roman numeral.
Silver (Ag): Notable exception with a +1 charge.
Page 14: Naming Transition Metals
Copper Example:
Copper (I) as Cu+ and forms compounds with Oxides.
Example: Cu2O.
Page 15: Writing Formulas with Transition Metals
Examples:
FeCl3: Iron (III) Chloride (Fe+3 Cl- 1).
FeCl2: Iron (II) Chloride (Fe+2 Cl- 1).
Emphasizes the necessity of utilizing the back crisscross method with Roman numerals for charge identification.
Page 16: Polyatomic Ions
Definition: Charged entities composed of tightly bound atoms that behave as a unit.
Examples: SO3^2-, NO2^-, ClO2^-
Page 17: Ternary Ionic Compounds
Definition: Comprised of three different elements, often containing polyatomic ions.
Characteristics: Retains cation and anion structure.
Page 18: Ternary Ionic Formulas
Example:
CaCO3: Combines Ca2+ with CO3^2-.
When charges cancel, symbols are written directly.
Page 19: Ternary Ionic Compounds: Naming
Calcium Nitrate:
For Ca(NO3)2, recognize that charges crisscross since they don’t cancel out directly.
Page 20: Types of Compounds
Molecular Compounds:
Comprised of molecules sharing electrons, usually made of two nonmetals.
Characteristics of bonding and attachment.
Page 21: Molecular Formula
Definition: Shows the number and types of atoms in a molecule of a compound.
Example: CO (Carbon Monoxide).
Page 22: Molecular Compounds Examples
Example Compounds: CS2, SiO2, BF3
Focus on composition of two nonmetals.
Page 23: Binary Molecular Compounds
Definition:
Consists of two elements (non-metals), emphasizing the absence of ionic charges.
Page 24: Naming Binary Molecular Compounds
Prefixes Usage: Indicates the number of atoms in each molecule.
Page 25: Covalent Prefixes
List of Covalent Prefixes:
Mono (1), Di (2), Tri (3), Tetra (4), Penta (5), Hexa (6), Hepta (7), Octa (8), Nona (9), Deca (10).
Page 26: Writing Binary Molecular Compounds
Example Calculation: CO2 - Carbon Dioxide;
Note that "mono" prefix is not used for the first element.
Page 27: Naming Binary Molecular Compounds
Methods:
Use prefix + element name (e.g., N2O = Dinitrogen Monoxide).
Page 28: Further Naming Methodology
Ending with Ide:
Utilize prefix + element root + ide for naming (e.g., PCl3 = Phosphorus Trichloride).
Reminder: All binary compounds conclude with "ide"!