Flashcard: Fundamentals of Chemical Bonding and Reactions — 24 carte

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.