chapter 5 Flashcards
what are electrons contained in generally?
energy shells
what happens when the number of energy shells increases?
energy increases
energy levels get closer together due to increased energy
what is the order that electrons fill the sub shells in?
1S, 2S, 2P, 3S, 3P, 4S, 3D, 4P, 4D, 4F
what are atomic orbitals?
region of space around nucleus that can hold up to two electrons with opposite spins
which ways do electrons spin in orbitals?
up and down
what is the shape of s-orbitals?
sphere
how many electrons can fit in one orbital?
2 electrons
how many electrons fit in an S subshell?
2 electrons
what is the shape of p-orbitals?
dumb-bell shape
how many variations of p-orbitals are there?
3
how many electrons can fit in a P subshell?
6
how many electrons can fit in a D subshell?
10
how many electrons can fit in a F subshell?
14
what is ionic bonding?
bonding between a metal and non-metal due to electron transfer
what happens in ionic bonding?
metals lose electrons to form positive cations
non-metals gain electrons to form negative anions
what happens in ionic bonding (attractions between ions)?
cations and anions are oppositely charged so form an ELECTROSTATIC ATTRACTION
forms an ionic compound
why do ionic compounds have high melting points?
strong electrostatic attraction
requires lots of energy to overcome
what shape do ions form when they bond ionically?
lattice structure
what is covalent bonding?
bonding where two non-metals have a strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms
how many electrons is boron happy with?
6
what is a dative covalent bond?
when elements bond by a lone pair of electrons from one element
what is meant by the term covalent bond?
the sharing of electrons between two nuclei (atoms)
