Chapter 5 Electrons and Bonding Flashcards
what properties do electrons have
electrons have the properties of both a particle and a wave
what are the four sub shells represent the principle quantum shells
s sub shells
p sub shells
d sub shells
f sub shells
what happens to electrons closer to the nucleus
they are lower in energy because the charges of the electron and proton cancel
what are the ‘s’ sub shells shape
spheres
what are the ‘p’,’d’,’f’ sub shells shape
dumbells in the x,y and z axis
why do electrons go around in pairs
electrons go round in pairs because they spin either clockwise or anticlockwise and pair up to cancel out spins
what is the first electron configuration rule
> orbitals fill with electrons in a specific order to produce the lowest energy state possible
what is the second electron configuration rule
> orbitals fill in order of increasing energy
what is the third electron configuration rule
> where there is more than one orbital with the same energy they fill simply at first and electrons have parallel spins
what is the fourth electron configuration rule
when every orbital of the same energy is singly occupied the electrons then start to pair up with opposite spins
what does the large number for electron configuration represent
the principle quantum shell
what does the letter for electron configuration represent
the sub shell
what does the number in the super script for electron configuration represent
number of electrons in the sub shell
what is the max number of electrons in the ‘s’ sub shell
2
what is the max number of electrons in the ‘p’ sub shell
6
what is the max number of electrons in the ‘d’ sub shell
10
what is the max number of electrons in the ‘f’ sub shell
14
what is the max number of electrons per orbital
2
how do you write the short hand electron configuration
[Previous Noble Gas] outer shell orbitals
what does the position of the element in the periodic table correspond to
the highest energy sub shell being filled
what is the transitional metal ion electron configuration rule
when shells are filling 4s fills before 3d because it is lower in energy. 4s empties first because it is further away from the nucleus
what is an orbital
region around the nucleus that can hold a maximum of 2 electrons
what is ionic bonding
bonding between a metal and a non-metal caused by electrostatic attraction between oppositely charged ions which arises when electrons are transferred
what 2 things happen to metals in ionic bonding
they lose outer shell electrons
form positively charged cations
what 2 things happen to non metals in ionic bonding
they gain outer shell electrons
form negatively charged anions
how is a giant ionic lattice formed
when each ion attracts many others of the opposite charge
what does the giant ionic lattice structure cause the ion to be
strong and crystalline
why ionic compounds have high melting and boiling points
the electrostatic forces are very strong so need lots of energy to be broken
why are most ionic compounds soluble in water
water is a polar molecule which breaks the ionic bond and forms an aqueous ion
why can ions in solution or molten conduct electricity
the ions are no longer in the giant lattice structure and are free to move
what is BIN MIX
BIN > Breaking Is eNdothermic
MIX > Making Is eXothermic
what three things does the solubility of the ionic compound depend on
> relative strength of ionic attraction
water - water bond attraction
attraction between ions and water
what is covalent bonding
involves sharing electrons as orbitals overlap between non-metals
do covalent bonds need a full outer shell of electrons
no
what is expansion of octect
principle quantum shells of 3 and above can have more than 8 electrons in their outer shell because they have an empty d sub shell
what are bonding pairs
electron pairs that form bonds
what are lone pairs
pairs of electrons not involved in bonding
what is dative covalent bonding
a covalent bond where at least one pair of electrons come from the same atom
what do more bonds mean
the bond gets shorter and stronger
what is average bond enthalpy
the amount of energy needed to break or make a bond
