Atomic Structure and the Periodic Table
Atomic structure
- Atoms are made up of sub-atomic – protons, neutrons and electrons
- protons have a positive charge, neutrons has neutral charge (same mass as protons) and electrons are negatively charged (same as no. of protons
| Particle | Relative charge | Mass (atomic mass) |
| Proton | +1 | 1 |
| Neutron | 0 | 1 |
| Electron | -1 | 1/18371 |
- Proton number: number of protons in an atom [atomic number]
- Nucleon number: total number of protons and neutrons in the nucleus of an atom [mass number]
Definition of terms
- Atom is the unit particle of an element
- Element is a substance that consists of atoms all with the same proton number.
- Proton no. is number of protons in an atom (and no. of electrons in an atom). in the periodic table, proton number increases with group number
- Nucleon no. is number of protons + neutrons in an atom
- Isotopes are atoms of same element with different number of neutrons eg chlorine 35 and 37
Electronic Configuration
- Electrons are arranged in electron shells.
- Electron shell structure: 2, 8, 18.
- Atoms want to have full outer shells (full set of valency electrons), this is why they react.
- Noble gases have full outer shells so they have no need to react.
Structure of the Periodic Table
- The number of protons in each element increases by 1 across each row
- Period number is the number of occupied shells in an element
Group number is the number of electrons in the outermost shell
Isotopes
- E.g. Carbon 12 and Carbon 14.
- Two types: Non-radioactive isotopes and radioactive-isotopes (unstable atoms that break down and produce radiation)
- Medical use: cancer treatment (radiotherapy) – rays kill cancer cells using cobalt-6
- Industrial use: to check for leaks – radioisotopes (tracers) added to oil/gas. At leaks radiation is detected using a Geiger counter.
Bonding
Terms to be familiar with
- Element: Pure substance consisting of one type of atom
- Mixture: two or more elements mixed together but not chemically combined
- Compound: substance in which two or more different elements are chemically combined
- Alloy: Mixture of two or more elements in which at least one is a metal, eg. brass (copper and zinc)
Elements, Compounds and Mixtures
An element is a substance that cannot be broken down into simpler substances through any chemical or physical means. Elements can exist as atoms or molecules. Each molecule of an element can consist of two or more atoms that are chemically combined.
A compound is a substance that contains two or more elements which are chemically combined in a fixed ratio. It can consist of either molecules or ions. The properties of a compound differ from its constituent elements.
A mixture consists of two or more substances that are mixed together. These substances can be elements or compounds. The ratio of these substances in a mixture is not fixed. The components in a mixture can easily be separated through physical methods.
| Metals | Non-metals |
| Good conductors of heat & electricity | Poor conductors of heat & electricity (except graphite) |
| High m.p. and b.p. | Lower m.p. and b.p. than metals |
| High density | Low density |
| Forms basic oxides | Forms acidic oxides |
| Forms cations in reactions | Forms anions in reactions |
| Malleable and ductile | Not malleable or ductile |
Ions and Ionic Bonds
Ionic bonding: Electrostatic force of attraction between a lattice of alternating positive and negative ions
- Chemical bonds are formed by transfer of electrons from one atom to another
- Metals lose electrons to form cations; non-metals gain electrons to form anions
- Positive cations & negative anions attract to each other
- Strong electrostatic force of attraction between positive cations and negative anions is called ionic bonding
Ionic bonding between Group I metal and Group VII non-metal
| Property | Reason |
| Form giant lattice | Cations and anions attract |
| High m.p. and b.p. | Strong bonds between ions |
| Don’t conduct electricity when solid | Ions can’t move |
| Conduct electricity when molten/aqueous | Ions can move |
| Usually soluble in water | Not required |
Molecules and Covalent Bonds
Covalent bonding: When atoms share electrons to obtain a full outer shell electron configuration; only between non-metals.
| Single Bond | Double Bond | Triple Bond |
| 2ē shared(1 from each atom) | 4ēs shared(2 from each atom) | 6ēs shared(3 from each atom) |
Examples:
 |
 |
|
| HCl | CO2 | N2 |
| Covalent bonding | Ionic bonding |
| Mostly volatile | Mostly non-volatile |
| Insoluble in water | Soluble in water |
| Poor electrical conductors | Good electrical conductors |
Covalent bonds, due to the sharing of electrons between atoms, have weaker attractive forces than ionic bonds. Thus they have lower melting and boiling points.
Macromolecules
| Diamond | Graphite | Silicon Dioxide |
 |
 |
 |
| 1 carbon atom bonded to 4 carbon atoms [tetrahedral structure] | 1 carbon atom bonded to 3 carbon atoms [hexagonal layers] | Each silicon is bonded to 4 oxygen atoms, and each oxygen is bonded to 2 silicon atoms [tetrahedral structure] |
| High m.p. and b.p | High m.p. and b.p | High m.p. and b.p |
| no free electrons | Conducts electricity (free electrons) | no free electrons |
| Used for cutting as it is strongest known substance | Used in pencil lead and as a lubricant | Used in production of glass |
Metallic Bonding
Metallic bonding: An electrostatic force of attraction between a lattice of positive metal ions and a sea of mobile electrons
