Atoms, their properties and how they are bonded together
|
|
How are electrons arranged in an atom?
What are the trends in the periodic table? What are the different types of bonds between atoms? |
How are trends in the periodic table explained using the idea of attraction and repulsion of electrons and nucleus?
How are intermolecular forces related the the physical properties of the substances? |
How are orbital diagrams correctly filled to represent the electrons distribution in an atom?
How is the electron domain and molecular domain geometry of covalent compounds identified? |
Can all trends in the periodic table be explained with the idea of attraction and repulsion of electrons and nucleus?
Can the geometry of covalent compounds be determined by looking at the attraction and repulsion of electrons and nucleuses' of the atoms in the compound? |
|
Vocabulary sheet
| ||
Introduction to the topics in this unit - Essential ideas
|
2.1 The mass of an atom is concentrated in its minute, positively charged nucleus
2.2 The electron configuration of an atom can be deduced from its atomic number. 12.1 The quantized nature of energy transitions is related to the energy states of electrons in atoms and molecules. |
3.1 The arrangement of elements in the Periodic Table helps to predicttheir electron configuration.
3.2 Elements show trends in their physical and chemical properties across periods and down groups. 13.1 The transition elements have characteristic properties; these properties are related to their all having incomplete d sub-levels. 13.2 d orbitals have the same energy in an isolated atom, but split into two sub-levels in a complex ion. The electric fi eld of ligands cause the d orbitals in complex ions to split so that the energy of an electron transition between them corresponds to a photon of visible light. |
