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.
Teste tes connaissances avec un QCM de 12 questions sur Fundamentals of Chemical Bonding and Reactions.
1. What is ionic bonding primarily characterized by?
2. What is a characteristic property of covalent compounds?
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