Click on image to enlarge

Bonding I - Wins Single User Shipped in 7 days Cat.# MSC-24 $240.00 BUY

After completing these activites, students should:

• Explain that metal and non-metal atoms combine with a complete transfer of electrons.

• Explain that valence electrons are transferred from metal atoms to non-metal atoms to form ions.
• State that atoms lose or gain electrons until a full octet of electrons is formed.
• Predict what happens when a wide range of metals and non-metals combine.
• Explain that covalent bonding involves the sharing of pairs of electrons, with each atom supplying one electron to be shared.
• Explain that co-ordinate bonding (dative covalency) is a type of covalent bonding where both electrons are supplied by one atom.
• Explain that in a metal the ions are closely packed together, and that they are held together by a sea of delocalized electrons.
• Describe how electricity is conducted through the metal by moving electrons. The electrons move from the negative terminal to the positive terminal.
• Define electronegativity as the power of an atom to withdraw electron density from a covalent bond.
• Explain that the electron distribution in a covalent bond may not be symmetrical.
• Explain that covalent bonds between different elements will be polar to different extents.
• State that anions can be polarized by cations of high charge density.
• Describe the behavior of gases, liquid and solids in terms of the particles, their motion and the forces acting between them.
• Explain the energy changes associated with changes of state.
• Explain how molecules may qualitatively interact by permanent dipole-dipole, induced dipole-dipole (van der Waals) forces and hydrogen bonding.
• Recognize the four main types of crystalline solid (metallic, ionic, molecular, and giant covalent or macromolecular) in terms of the particles present and the bonding forces between them.
• Describe the structures of iron, sodium chloride, iodine, diamond and graphite.
• Relate the physical properties of substances such as iron, sodium chloride, iodine, diamond and graphite to the appropriate types of structure and bonding.

Lesson: Ionic Bonding
These activities provide opportunities to view and manipulate images of atoms and electrons to enable students to grasp the processes involved in ionic bonding. This includes electron transfer and the formation of ions in reactions between metal and non-metal elements. Students can also explore relationships between the number of electrons in an atom and the position of the element in the Periodic Table. Two video clips show real reactions taking place – one in which sodium chloride is formed and the other in which magnesium oxide is produced.

Lesson: Covalent Bonding
These activities investigate atoms sharing electrons. Single, double and triple covalent bonds are examined in a range of molecules. You are then able to practise correctly placing electrons in molecules. These exercises range from simple examples such as hydrogen chloride to more complicated examples such as carbon monoxide. In doing this you can see that some electrons are bonding electrons and others are non-bonding electrons. Co-ordinate bonding is also examined.

Lesson: Metallic Bonding
Aluminium is used as an example of a metal that displays typical metallic properties. This activity uses an animation to show the structure of a piece of aluminium, demonstrating that in a metal the atoms are packed closely together. The image shows that the valency electrons of the aluminium atoms are delocalized, so electrons can move throughout the metal carrying the charge.

Lesson: Polarization
Aluminium is used as an example of a metal that displays typical metallic properties. This activity uses an animation to show the structure of a piece of aluminium, demonstrating that in a metal the atoms are packed closely together. The image shows that the valency electrons of the aluminium atoms are delocalized, so electrons can move throughout the metal carrying the charge.

Lesson: Forces Between Molecules
These activities review the relationship between temperature and states of matter, explore dipoles and investigate hydrogen bonding. The behaviour of particles is examined as different substances are heated or cooled and the attraction between permanent and induced dipoles in a range of substances is presented. Factors that affect the strength of van der Waals forces are investigated and the special case of hydrogen bonding is introduced. The polarity in covalent bonds between hydrogen and other elements is explored, and examples of hydrogen bonding are presented, including that of ice and proteins.

Lesson: Types of Structures
The first activity consists of a one, two or four pane display which can be used to show pictures, structures, animations and video clips of the four main types of crystalline solid (metallic, ionic, molecular and giant covalent) and their properties. The examples used are iron, sodium chloride, iodine, diamond and graphite. The properties examined are melting point, hardness and electrical conductivity. In most cases both a video clip of the property being tested and an animation to explain the behaviour in terms of structure and bonding is included. The lattice structure of solid argon and a close-up view of zinc crystals are also available.

The last activity consists of an interactive revision exercise on the properties of the above five solids. The solubility of each substance in water and in non-polar solvents is included in this summary. This section concludes with an interactive exercise in which the user has to identify unknown types of solid by gradually revealing their properties.

Click on image to enlarge

Bonding II - Wins Single User Shipped in 7 days Cat.# MSC-25 $240.00 BUY

After completing these activites, students should:

• Describe bonding and lone pairs of electrons as charge clouds occupying orbitals.

• Predict the shapes of, and bond angles in, simple molecules and ions, limited to 2, 3, 4, 5 and 6 co-ordination.

• Explain that lone pair/lone pair repulsion is greater than lone pair/bonding pair repulsion, which is greater than bonding pair/bonding pair repulsion; and understand the resulting effect on bond angles.

Lesson: Shapes of Simple Molecules
The concept of valency shell electron repulsion is introduced using simple molecules. Diagrams showing electron shells are used to establish the presence of bonding and non-bonding electrons. Interactive models show the number, shape and orientation of bonding orbitals and are used to explore ideas of molecular shape and bond angles. These concepts are further developed to encompass more complex molecules and molecular ions. Finally a summary quiz tests the knowledge gained during the lesson.

Click on image to enlarge

Atomic Structure - Wins Single User Shipped in 7 days Cat.# MSC-22 $240.00 BUY

After completing these activites, students should:

• State the relative masses and charges of the three main atomic particles and describe where these particles are located in the atom.

• Explain the meaning of the terms 'atomic (proton) number' (Z) and 'mass number' (A), and be able to represent the atoms of elements in symbolic form.
• Explain the existence of isotopes and the similarities and differences, in terms of particles, between isotopes of an element.
• Identify atoms or ions of different elements given information about the number of protons, electrons or neutrons in them, and vice versa.
• Explain the meaning of 'relative atomic mass' (Ar), 'isotopic mass', 'molecular mass' (Mr) and 'formula mass', based on the carbon-12 scale.
• Calculate the relative atomic mass of an element consisting of more than one naturally occurring isotope when given the relative amounts of each isotope.
• Describe the principles of operation of a simple low-resolution mass spectrometer limited to ionization, acceleration, deflection and detection.
• Explain what a mass spectrum represents for elements and for molecules.
• Interpret simple mass spectra of elements and calculate relative atomic mass from isotopic abundance.
• Describe how mass spectrometry can be used to determine relative molecular mass.
• Write the simple electron arrangement of the first 36 elements.
• Describe the shapes of s and p orbitals.
• Demonstrate a knowledge of the relative energies of orbitals in shells 1 to 4. Work out the electron arrangements of the first 36 elements in terms of orbitals.

Lesson: Atomic Structure
These activities provide a variety of animations and diagrams to illustrate the concepts and definitions used to describe and identify atoms of different elements.  The effect of an electric or magnetic field on the movement of the three most important subatomic particles (protons, electrons and neutrons) is observed and a brief summary illustrating the historical development of our model for the atom is included.

The meaning of ‘atomic number', ‘mass number' and the existence of isotopes is explained using animated atoms that can be separated into heaps of their constituent subatomic particles. Symbolic notation for isotopes is introduced. A ‘particle counter' provides opportunities to practice working out the numbers of each type of subatomic particle present in a range of atoms. Alternatively, the numbers of these particles in an atom can be used to find the atomic and mass numbers for that atom. This exercise extends to the common ions formed from atoms of some elements. The relative atomic mass scale is introduced and explored further using two atomic balances.

Lesson: Mass Spectrometer
The activities use an animation of a simple magnetic-sector mass spectrometer in which the ionization, acceleration, deflection and detection of the particle beam from various samples can be followed at the same time as the mass spectrum is recorded.

Lesson: Electron Arrangement
These activities examine the arrangement of electrons in various atoms. The first 36 elements are investigated and the simple electron arrangement for each of these elements is displayed, e.g. 2.8.1 (for sodium). The shapes of s and p orbitals are compared and the electron arrangements of s, p, and d orbitals are investigated. This time the electron arrangement in terms of orbitals is displayed, e.g. 1s22s22p63s1 (for sodium).

Wins   Mac Contact us for pricing on 20 or 30 User Network Licences

Electronic Structure Single User Shipped in 7 days Cat.# CYC-5 $140.00   BUY 5 User Lab Pack Shipped in 7 days Cat.# CYC-5LP $250.00 Wins BUY     Mac BUY Site Licence Shipped in 7 days Cat.# CYC-5SL $410.00 Wins BUY     Mac BUY

Electronic Structure delves into the intricacies of electrons – their properties, configurations, and orbital patterns. Animations and 3-D diagrams clearly depict and explain quantum mechanical levels, sublevels, and orbitals. This program will greatly aid the student in understanding electronic structure. For example, this comprehensive program uses a periodic table that is created, atom by atom, using the Aufbau Principle, dynamic 2D and 3D atom representations, and carefully constructed relative energy diagrams.

Topics covered in this program:
Chemical Properties, The Role of Electrons, Arranging the Elements, Atomic Structure, Electron Energy Levels, Energy Diagrams, Quantum Theory, Quantum Mechanics, Electron Orbitals, Building Electron Shells, The Pauli Principle, The Aufbau Principle, Hund's Rule, The Closed Shell Concept, and Building the Periodic Table