Periodic table — structure?
Organized by atomic number in periods and groups.
Period — definition?
Horizontal row with increasing atomic number.
Group — definition?
Vertical column with similar properties.
Atomic number — role?
Number of protons, identifies element.
Electron shells pattern — rule?
Fill 2, 8, 8… electrons per shell.
Valence electrons — location?
In the outermost shell.
Metals — properties?
Shiny, malleable, good conductors.
Non-metals — properties?
Dull, brittle, poor conductors.
Reactivity trend — alkali metals?
More reactive down the group.
Reactivity trend — halogens?
More reactive up the group.
Ion — definition?
Charged atom or molecule.
Cation — charge?
Positive ion.
Anion — charge?
Negative ion.
Ion formation — metals?
Lose electrons, form cations.
Ionic compound — formed by?
Ions held by electrostatic attraction.
Covalent bond — mechanism?
Atoms share electrons.
Molecule — definition?
Atoms bonded together by covalent bonds.
Diatomic elements — examples?
H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂.
Types of reactions — main?
Synthesis, decomposition, displacement, combustion.
Balancing equations — purpose?
Ensure same atoms on both sides.
Precipitate — formation?
Insoluble solid from solution.
pH scale — measures?
Acidity or alkalinity of solutions.
Indicator — role?
Changes colour with pH.
Litmus paper — colour in acids?
Red.
Answer 12 questions on Periodic Table and Bonding Fundamentals.
1. What does the structure of the periodic table primarily represent?
2. What is the pattern of filling electron shells in an atom according to the Bohr model?
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