Unit - 1 Flashcards
What factors affect rate of reaction
Temperature Concentration Particle Size Pressure The presence of a catalyst
How does temperature affect reaction rate
Increased temp = increased rate
Decreased Temp = Decreased Rate
How does concentration affect reaction rate
Increased Concentration = Increased Rate
Decreased Concentration = Decreases Rate
How does particle size affect reaction rate
Decreased Particle Size = Increased Rate
Increased Particle Size = Decreased Rate
How does Pressure affect reaction rate
Increased Pressure = Increased Rate
Decreased Pressure = Decreased Rate
What is the statement for Particle Collision
For particles to collide they need enough kinetic energy and the correct orientation
What are Catalysts
- They lower activation energy of a reaction
- They remain unchanged/ they are reusable
- Can become denatured
An example are enzymes
Why are the two types of catalyst
Homogeneous- catalyst is in the same state as the reactants
Heterogeneous- catalyst is in a different state as the reactants
Where is the atomic number, mass number and symbol in nucleotide notation
Mass
Symbol
Atomic
How does the covalent radius change as you down a group and across a period
It gets smaller as you across a period due to their being more electrons and a them being pulled in closer towards to nucleus of the atom
It gets larger as you go down a group as there are more shells and the outer shells are being pulled in less as they are being shielded from the electronegative pull of the atom
What is the ionisation energy
The energy required to remove one mole of electrons from one mole of gaseous atoms
What does the strength of attraction between the electron and nucleus depend on
- The size of the nucleus charge
- the distance between the nucleus and the electrons
- the number of other electrons between the electrons and the nucleus
What does electronegativity mean
It is the attraction an atom has for a shared pair of electrons in a bond
What electronegativities mean what type of bonding
0-.4 pure covalent bonding
.5-1.9 polar covalent bonding
2.0- ionic bonding
What properties do covalent networks possess
High melting and boiling point
Insoluble in water
Mostly don’t conduct electricity
All atoms joined by strong inter-molecular forces
What are some examples of covalent networks
Silicon Carbide
Silicon Dioxide
Polymorphism (allotropes) of carbon
Graphite ( conducts electricity)
What are the properties of Discrete Covalent Molecular Bonding
Low melting and boiling points
Joined by weak inter-molecule bonds
Don’t conduct electricity
No charged particles or free electrons
What are some example of covalent molecular bonding
Nitrogen Oxygen Halogens Sulfur (S8) Phosphorus (P4) Fullerene (C60)
What are the properties of ionic bonding
Crystal Lattice Structure
Very strong bonds between positive and negative atoms
Conduct when Molten or in Solution
High Melting and Boiling Points
What are the properties of Metallic Bonding
High Melting and Boiling Points
Conducts electricity as it contains delocalised electrons
Lots of inter-molecular forces
What is the name for all of the intermolecular forces
Van Der Waavls
What are the three Van Der Waavl Forces
London Dispersion Forces
Permanent Dipole -Permanent Dipole
Hydrogen Bonding
How do London Dispersion Forces work
Atoms wobble
Electrons move between the poles of the atom
Causes a temporary dipole
How do permanent dipole interaction work
When a bond forms between a slightly negative atom in one molecular and a slightly positive atom in another
How does hydrogen bonding work
A very strong bond forms between a hydrogen atom on molecular and a Nitrogen, Fluorine or Oxygen atom in another molecule
