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10.9Chapter 10: Structure, Bonding, and Properties

Chapter 10 Review: Structure, Bonding, and Properties — Alhussan Chemistry - Stage 9 Revision Notes & Topical Questions

5 min read 7 parts Lesson 9 of 9 1 quiz

📚 Alhussan Chemistry - Stage 9 Hub / Topical Revision
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Lesson summary

10.9 Chapter 10 Review: Structure, Bonding, and Properties — Alhussan International Academy — Chemistry (Stages 7–9) notes: Revise atomic structure, ions, covalent molecules, giant structures and how structure determines properties.Proton number — it is the number of protons in a…

  • Period and group
  • Same group
  • Ion formation
  • Drawing ions
  • Covalent bond
  • Simple molecules

Section 1 of 7Atoms, shells and the periodic table

Atoms, shells and the periodic table
Proton number
  • Proton number it is the number of protons in an atom and fixes the position of the element in the periodic table.
Electrons
  • Electrons a neutral atom has as many electrons as protons, arranged in shells.
  • Aluminium has proton number 13, so 13 electrons arranged 2,8,3.
Period and group
  • Period and group the period number equals the number of shells and the group number equals the outer electrons.
  • Aluminium is in period 3 and group 3, and boron also has three outer electrons.
Same group
  • Same group elements in the same group have the same number of outer electrons and similar properties.

Section 2 of 7Ions and ionic compounds

Ion formation
  • Ion formation metals lose outer electrons to form positive ions and non-metals gain electrons to form negative ions, giving each a full outer shell.
Formulae
  • Formulae magnesium forms Mg2+ and iodine forms I-, so magnesium iodide is MgI2 with two iodide ions for each magnesium ion.
Properties
  • Properties ionic compounds form giant lattices with high melting points and are brittle.
  • They conduct only when molten or dissolved, because the ions are then free to move.
Drawing ions
  • Drawing ions show outer shells only, put the charge with the number first and the sign second, and use brackets around ions.

Section 3 of 7Covalent substances

Covalent substances
Covalent bond
  • Covalent bond non-metal atoms share pairs of electrons.
Simple molecules
  • Simple molecules water, methane and carbon dioxide have weak forces between molecules, so melting points are low and they do not conduct.
Giant covalent structures
  • Giant covalent structures diamond, graphite and silicon dioxide have many strong bonds and very high melting points.
Graphite
  • Graphite it conducts because each carbon atom has a delocalised electron,
    • and it is a lubricant because its layers are held by weak forces and slide easily.

Section 4 of 7Comparing structure types

TypeMelting pointConducts?
IonicHighMolten or dissolved
Simple molecularLowNo
Giant covalentVery highNo (graphite yes)
MetallicHighYes
Comparing structure types
Water and salt solution
  • Water and salt solution pure water has no ions or free electrons, whereas dissolved sodium chloride releases free Na+ and Cl- ions that carry charge.
Explaining a property
  • Explaining a property identify the structure, name the particles, state the force that must be overcome and link it to the property.
  • Sodium chloride has a high melting point because a giant lattice of ions has strong electrostatic forces that need much energy to overcome.

Section 5 of 7Particle numbers and ions

Particle numbers and ions
Atoms
  • Atoms the numbers of protons and electrons equal the proton number, and the neutrons equal the mass number minus the proton number.
  • 27Al has 13 protons, 13 electrons and 14 neutrons.
Oxide ion
  • Oxide ion it has eight protons and ten electrons arranged 2,8, so its charge is 2-.
Potassium sulfide
  • K+ and S2- give K2S.

Section 6 of 7Key terms

TermMeaning
Proton numberthe number of protons in an atom.
Ionic bondthe attraction between oppositely charged ions.
Covalent bonda shared pair of electrons.
Giant latticea regular structure of many particles.
Delocalised electronan electron free to move in a structure.

Section 7 of 7Exam technique

1
Writing the sign before the number or leaving out the superscript layout — write the number first then the sign, as in Mg2+.
2
Saying molecules break when a simple covalent substance melts — only the weak forces between molecules are overcome.
3
Forgetting that ionic solids do not conduct — ions are fixed in the solid.
4
Using the group number as the number of shells — the period gives the shells.

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