Chapter 5 Flashcards
electron shells can be regarded as..
energy levels
electrons possess certain quanta of energy so
can only exist at certain quantised energy levels
energy levels get— at higher energy
closer together
principle quantum represented with the letter
n
how do electrons move between energy levels
they abosorb or emit energy
atomic orbital
region of space around the nucleus that can hold up to two electrons with opposite spin
types of orbitals
s orbital
p orbital
d orbital
f orbital
s orbitals
spherical shape
each shell from energy level 1 contains 1 orbital and 2 electrons
p orbitals
dumbbell shape
from n=2, each has 3 separate orbitals at right angles to eachother
d orbitals
comes in sets of 5 from n=3
f orbitals
Seven f orbitals from n=4
ionic bonding
electrostatic attraction between positive ions and negative ions
common cations
metals
potassium, calcium, mg, al, nh4
common anions
chlorine, oxygen, sulfur
so42-, co32-
structure of ionic compounds
each ions attracts oppositely charged ions in all directions in solid state
forms giants ionic lattice
properties of ionic compounds
solids at RT
high mp and bp- depends on ionic charges + sizes of ions
soluble in polar solvents
electrically conductive in molten
when charge on ion increases, strength of bond
increases
strength of ionic bond increases when size on ion
decreases
covalent bonding
strong electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms
elements
where does covalent bonding occur
non metallic elements
compounds of non metallic elements
polyatomic ions(holds the ion as an ion)
covalent bonding in terms of orbitals
overlap of atomic orbitals, each with one electron, giving a shared pair
covalent bonding is localised
happens solely between a shared pair of electrons
dative covalent bond
shared pair of electrons has been supplied by one of the bonding atoms only, originally a lone pair
average bond enthalpy
measurement of covalent bond strength, how much energy is needed to break
