Chapter 5 Electrons & Bonding Flashcards
What are shells?
Energy levels
What are atomic orbitals?
A region around the nucleus that can hold up to two electrons with opposite spins
What are the 3 main orbitals, and how many electrons can they hold
- s, 2 electrons
- p, 6 electrons
- d, 10 electrons
In what order do electrons fill up orbitals?
In order of increasing energy?
What is the exception to filling up orbitals and why?
The 4s sub-shell fills before the 3d sub-shell because the 3d sub-shell is at a higher energy level than 4s
In an orbital, Why can negative electrons pair up without repelling away?
Two electrons in an orbital have opposite spins which helps to counteract the repulsion between the negative charges of the two electrons
What is ionic bonding?
The electrostatic attraction between positive and negative ions
How do giant ionic lattices form?
When each ion attracts oppositely charged ions in all directions
Describe the melting and boiling point of ionic compounds
Ionic compounds have very high melting and boiling points this is because a lot of energy is required to overcome the strong electrostatic forces of attraction between the oppositely charged ions
Describe the solubility of ionic compounds
Most ionic compounds dissolve in polar solvents like water, Polar water molecules break down the lattice and surround each ion in solution
What two main processes are required for an ionic compound to be soluble in water?
- The ionic lattice must be broken down
- Water molecules must attract and surround the ions
Describe the electrical conductivity of ionic compounds when solid
In the sold state, an ionic compound does not conduct electricity because the ions are fixed in positions so there are no mobile charge carriers
Describe the electrical conductivity of ionic compounds when dissolved or melted
Once melted or dissolved in water the ionic compounds do conduct electricity as the ions are free to move as mobile charge carriers
What is covalent bonding?
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atom
What are lone pairs?
Paired electrons that are not shared in a covalent bond
