What is the rule regarding orbitals with the same energy?
Key Terms
How can electron configuration be shortened?
1s2 can be expressed as [He].
1s2 2s2 2p6 can be expressed as [Ne].
1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar].
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| Term | Definition |
|---|---|
What is the rule regarding orbitals with the same energy? | Within a sub shell, the orbitals have the same energy. One electron occupies each orbital before pairing begins. |
How can electron configuration be shortened? | 1s2 can be expressed as [He]. |
What happens in terms of energy sub-shells when forming ions? | The highest energy sub-shells lose or gain electrons. |
What is ionic bonding? | The electrostatic attraction between positive and negative ions. |
What is the result of ions attracting oppositely charged ions in all directions? | Giant ionic lattice |
What happens to the melting points for giant ionic lattices, when ionic charge increases? | Melting point increases as there is a stronger attraction between ions. |
Are ionic compounds soluble? | They dissolve in polar solvents such as water. |
What does solubility require? | The ionic lattice must be broken down. Water molecules must attract and surround the ions. |
What does solubility (of ionic compounds) depend on? | The relative strengths of the attractions within the giant ionic lattice and the attractions between ions and water molecules. |
When can ionic compounds conduct electricity? | Not in the solid state. | When molten or dissolved in water. |
Why can't ionic compounds conduct electricity when solid? | The ions are in a fixed position. | There are no mobile charge carriers. |
Why can ionic compounds conduct electricity when molten or dissolved in water? | The solid ionic lattice breaks down. | The ions are now free to move as mobile charge carriers. |
Summarise the properties of most ionic compounds | High melting and boiling points. |
What is covalent bonding? | The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms. |
What is a covalent bond? | The overlap of atomic orbitals, each containing one electron, to give a shared pair of electrons. |
How does covalent bonding differ to ionic bonding? | The attraction is localised, acting only on the shared pair of electrons and the two nuclei of the bonded atoms. |
How can covalent bonding be displayed? | With dot and cross diagrams. |
What is a multiple covalent bond? | Two atoms share more than one pair of electrons. |
What is a double bond? | The electrostatic attraction is between two shared pairs of electrons, and the nuclei of the bonding atoms. |
What is a triple bond? | The electrostatic attraction is between three shared pairs of electrons, and the nuclei of the bonding atoms. |
What is a dative covalent bond? | The shared pair of electrons has been supplied by one of the bonding atoms only. |
Give an example of a dative covalent bond | An ammonia molecule donates its lone pair of electrons to an H+ ion. Forming an ammonium ion. |
What is average bond enthalpy? | A measurement of covalent bond strength. Larger value = stronger bond. |