Ionic Bonding — definition?
Transfer of electrons between metal and non-metal.
Covalent Bonding — electrons?
Sharing of electrons between non-metal atoms.
Metallic Bonding — electrons?
Delocalized 'sea' of electrons in metals.
Naming ionic compounds — rule?
Metal + non-metal with '-ide'; Roman numerals for transition metals; polyatomic ions as units.
Criss-cross rule — purpose?
Balance charges to determine formula subscripts.
Polyatomic ions — examples?
Nitrate, sulfate, hydroxide, carbonate.
Reaction type — neutralization?
Acid reacts with base to produce salt and water.
Neutralization — main products?
Salt and water.
Acid-metal reaction — produces?
Salt and hydrogen gas.
Acid-carbonate reaction — products?
Salt, water, and CO₂ gas.
Precipitation reaction — forms?
Insoluble salt as a solid precipitate.
Solubility rules — key?
Nitrates, Group 1 metals, ammonium always soluble.
Ionic bonding — high?
Melting and boiling points.
Covalent compounds — conduct?
No, they do not conduct electricity.
Metallic bonding — explains?
Properties like conductivity, malleability.
Naming transition metals — need?
Roman numerals for oxidation state.
Criss-cross — used for?
Writing formulas of ionic compounds.
Polyatomic ions — notation?
Parentheses for multiple ions in formulas.
Reaction involving CO₂?
Acid-carbonate reaction.
Reaction involving H₂ gas?
Acid-metal reaction.
Precipitate — symbol?
(s) in equations.
Solubility of nitrates?
Always soluble in water.
Solubility of carbonates?
Generally insoluble unless with Group 1 or ammonium.
Ionic bond — key force?
Electrostatic attraction.
Test your knowledge with 12 questions on Fundamentals of Chemical Bonding and Reactions.
1. What is ionic bonding primarily characterized by?
2. What is a characteristic property of covalent compounds?
Review the complete course in the revision sheet for Fundamentals of Chemical Bonding and Reactions.
See revision sheet →Import your course and AI generates flashcards in 30 seconds.
Flashcard generator