Chapter 5 - Electrons and Bonding Flashcards
What is an atomic orbital?
An atomic orbital is a region surrounding the nucleus that can hold up to two electrons with opposite spins
What is the shape of an S orbital?
A sphere
What is the shape of a P orbital?
A dumb-bell shape
What is the order of filling of subshells?
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, …
What is each block of the periodic table called?
What is the definition for ionic bonding?
Ionic bonding is the electrostatic force of attraction between a positive ions and negative ions.
What is the structure of ionic compounds?
A giant ionic lattice
What are the properties of ionic compounds and why?
-High melting and boiling points - lots of energy is needed to overcome the strong electrostatic force of attraction between the oppositely charged ions.
-Soluble in polar solvents (e.g. water)- polar water molecules break down the lattice and surround each ion in solution.
-Do not conduct electricity when solid but do when molten or dissolved- when solid the ions are fixed in position, but when liquid the solid ionic lattice breaks down and the ions are free to move and carry charge.
What is the definition for covalent bonding?
Covalent bonding is the electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms. (two non metals)
What is a molecule?
A molecule is the smallest part of a covalent compound that can exist whilst keeping the chemical properties of that compound.
What is a dative (coordinate) covalent bond?
A covalent bond in which the shared pair of electrons has been supplied by one of the bond atoms only. The shared pair of electrons was originally a lone pair of electrons.
What is average bond enthalpy?
A measurement of covalent bond strength, the larger the bond enthalpy, the stronger the covalent bond.
