Master this deck with 62 terms through effective study methods.
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Increasing ionic radii as there are more shells of electrons
decreasing ionic radii because the nuclear charge increases as we go across a period the outer electrons are more strongly attracted to nucleus so smaller ion
There is increased effective nuclear charge because the ions have lost an electron so the attraction between outer e and nucleus is stronger. Sometimes positive ions lose an entire outer shell making them much smaller
The ion has gained an electrons so there is more electron-electron repulsion and the electron cloud is larger
The nuclear charge increases because there are more protons meaning the attraction between the nucleus and the electron cloud increases so their ionic radius decreases
the energy change when one mole of an ionic solid is formed from its gaseous ions. More energy released means stronger ionic bonding
High. Strong electrostatic attraction between the delocalised electrons and the cations. Takes a lot of energy to overcome
When metals are solids and molten they can conduct electricity. They have delocalised electrons can move through the structure carrying charge
Good. Delocalised electrons can move through the structure carrying a flow of charge
the electrostatic attraction between two nuclei and the shared pair of electrons between them
it is a simple molecular structure and intermolecular bonds between the molecules is weak and takes little energy to overcome
lone pair of electrons is a pair of electrons in the outer shell of one of the atoms in a molecule or ion which isn't involved in bonding
a dative covalent bond is a bond in which two atoms share electrons, both the electrons being donated by one atom
the electrostatic attraction between the positively charged nucleus and the shared bonding pairs of electrons whose orbitals have overlapped
Pi bonds and sigma bonds
a double bond is more electron dense because it involves the sharing of 4 electrons which makes the bond shorter as the bond is stronger
because F atoms are smaller so the lone pair of electrons are closer together and this causes more repulsion
low because only the intermolecular forces have to be broken
they are more soluble in non-polar solvents such as hexane than water because many simple covalent substances don't form covalent bonds with water
they have no overall charge and have no delocalised electrons which can move or carry charge
A highly ordered arrangement of atoms , ions or molecules extending in all directions
covalent
If you shift the layers of ions over there are forces of repulsion as there are like charges opposite each other
no as they have no mobile charged particles
simple molecular structure
Valence shell electron pair repulsion theory
Trigonal pyramidal
The ability of an atom to attract the bonding electrons in a covalent bond
104.5
107
109.5
Electrons distributer evenely
2 distinct regions of electron density
Distribution if electrons is not even and a dipole is formed
Size of the atom Shielding Proton number
Electro negativity decreases
Electro negativity increases
0.5
Due to the mobile nature of electrons the electron density randomly fluctuates around the molecule causing dipoles
Induced dipole
Number of electrons
The greater the difference in negativity
Oxygen, Nitrogen and fluorine
90 and 180
Born harber cycle
Covalent, polar covalent and ionic
Giant covalent. Each carbon is bonded to 3 others in flat hexagonal sheets so there is 1 delocalised electron per carbon. There are weak intermolecular forces between the layers.
Each carbon atom covalently bonded to 4 others and forms a rigid tetrahedral structure
Increases the attraction between cation and sea of delocalised electrons because more electrons are released into the sea
The layers of positive ions are able to slide over each other and are held by the sea of delocalised electrons
Each carbon bonded to 3 other carbons. They can conduct electricity. In each carbon layer is arranged in hexagonal rings
Octahedral
linear
Trigonal planer
The intermolecular forces between layers of graphite are weak and the layers can slide over each other so it can be used as a lubricant. It can conduct electricity because of the delocalised electrons
Graphene is a single 2D sheet of graphite that are just 1 atom thick. Sheets are formed from hexagonal carbon rings
The hexagonal rings makes it a very strong, rigid material which is lightweight. The delocalised electrons means it can conduct electricity.
Trigonal bipyramidal
90 and 120
V-Shaped
T-Shaped
Giant covalent