Unit 1: Topic 1 Bonding Flashcards
Q: How does electron arrangement determine bonding?
A: Atoms bond to achieve stable valence shells.
Q: How many ions can transition metals form?
A: More than one (e.g., Fe²⁺, Fe³⁺).
Q: What are ions?
an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
Q: What causes chemical bonds?
A: Electrostatic attractions from electron sharing or transfer.
Q: What is valency?
A: The number of bonds an atom can form based on its electron configuration.
Q: Differentiate empirical, molecular, and formula unit.
Empirical formula: Simplest ratio of atoms.
Molecular formula: Actual number of atoms.
Formula unit: Ratio of ions in an ionic compound.
Q: How do you determine Lewis structures?
A: Show valence electrons, bonding, and lone pairs.
Q: How do you determine the formula of ionic compounds?
identify the cation and anion, write their symbols and charges, and then combine them in a ratio that balances the charges, ensuring the overall compound is neutral.
SWAP AND DROP
Q: How do you determine the formula of covalent compounds?
A: Use the prefix system for naming non-metals (e.g., CO₂ = Carbon dioxide).
empirical formula,
the empirical formula of a chemical compound is the simplest whole number ratio of atoms present in a compound
molecular formula
indicate the simple numbers of each type of atom in a molecule, with no information on structure
formula unit.
is the smallest unit of a non-molecular substance, like an ionic compound, representing the lowest whole-number ratio of ions
