Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
36 Cards in this Set
- Front
- Back
- 3rd side (hint)
|
Cu (s) - type of solid |
Metallic |
|
|
|
Cu (s) type of particle |
Atom in a sea of electrons |
|
|
|
Cu (s) attractive forces between particles |
Metallic bond attraction between the positive metal nucleus and negative electrons |
|
|
|
PCL3 type of solid |
Molecular |
|
|
|
PCL3 type of particle |
Molecule |
|
|
|
PCl3 attractive forces between particles |
Intermolecular forces |
|
|
|
Silicon dioxide- type of solid |
Covalent network |
|
|
|
Silicon dioxide- type of particle |
Atoms |
|
|
|
Silicon dioxide- attractive forces between particles |
Strong covalent bond |
|
|
|
KCl type of solid |
Ionic |
|
|
|
KCl type of particle |
Ions |
|
|
|
KCl attractive forces between particles |
Ionic bond |
|
|
|
Bond angle Linear |
180 |
|
|
|
Bond angle trigonal pyramid |
109 |
|
|
|
Bond angle angular |
120 or 109 |
|
|
|
The name of the molecular shape with 120 as a bond angle and 3 regions of negative charge |
Trigonal planer |
|
|
|
Bond angle tetrahedral |
109 |
|
|
|
Most electronegative elements |
F O N/Cl S C H.... |
|
|
|
Contain polar bonds AND lack of molecule symmetry |
Polar molecules |
Dipoles do not cancel out |
|
|
Contain polar bonds BUT molecule is symmetrical |
Non polar molecules |
Dipoles cancel out due to symmetry |
|
|
Energy absorbed from surroundings |
Endothermic |
|
|
|
Bond breaking |
Endothermic |
|
|
|
Energy released to surroundings |
Exothermic |
|
|
|
Bond making |
Exothermic |
|
|
|
Type of solid Between metal and non metal |
Ionic |
|
|
|
Type of solid Between non metal and non metal |
Covalent |
|
|
|
Type of solid- bonding between metal atoms |
Metallic |
|
|
|
What is Diamond, graphite or silicon dioxide |
Covalent network |
|
|
|
Electrical conductivity- metals (solid or molten) |
DELOCALISED ELECTRONS are free to move |
|
|
|
Electrical conductivity- ionic substances (molten/dissolved in water (aq)) |
IONS are free to move |
|
|
|
Electrical conductivity- graphite |
DELOCALISED ELECTRONS are free to move |
|
|
|
Non polar substances dissolve in non polar solvents because... |
They have similar weak intermolecular forces |
|
|
|
Polar substances dissolve in polar solvents because... |
They have similar weak intermolecular forces |
|
|
|
Ionic solids dissolve in polar solvents because... |
Of the attraction between positive and negative charged ions AND polar solvent. Ions are partially surrounded, the ionic bond is weakened. Ions are removed from the crystal. (DO NOT call ionic solids "polar" THEY ARE NOT!) |
|
|
|
MEMORISE!!! THE WORDING IS IMPORTANT |
In each _ molecule, there are _ regions of negative charge around the central _atom. These repel to be at maximum separation in a _ shape resulting in a bond angle of _. The molecule has _ bonding electrons and _ lone pair electrons, so the overall shape of the molecule is _. |
|
|
|
Why does Cu not dissolve |
The metallic bond is too strong so the water molecules are unable to break it and form new bonds between water AND Cu atoms |
|
