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Higher Chemistry > Unit - 1 > Flashcards

Unit - 1 Flashcards

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1
Q

What factors affect rate of reaction

A 
Temperature 
Concentration 
Particle Size
Pressure
The presence of a catalyst
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2
Q

How does temperature affect reaction rate

A

Increased temp = increased rate

Decreased Temp = Decreased Rate

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3
Q

How does concentration affect reaction rate

A

Increased Concentration = Increased Rate

Decreased Concentration = Decreases Rate

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4
Q

How does particle size affect reaction rate

A

Decreased Particle Size = Increased Rate

Increased Particle Size = Decreased Rate

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5
Q

How does Pressure affect reaction rate

A

Increased Pressure = Increased Rate

Decreased Pressure = Decreased Rate

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6
Q

What is the statement for Particle Collision

A

For particles to collide they need enough kinetic energy and the correct orientation

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7
Q

What are Catalysts

A
  • They lower activation energy of a reaction
  • They remain unchanged/ they are reusable
  • Can become denatured

An example are enzymes

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8
Q

Why are the two types of catalyst

A

Homogeneous- catalyst is in the same state as the reactants

Heterogeneous- catalyst is in a different state as the reactants

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9
Q

Where is the atomic number, mass number and symbol in nucleotide notation

A

Mass
Symbol
Atomic

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10
Q

How does the covalent radius change as you down a group and across a period

A

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

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11
Q

What is the ionisation energy

A

The energy required to remove one mole of electrons from one mole of gaseous atoms

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12
Q

What does the strength of attraction between the electron and nucleus depend on

A
  • 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
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13
Q

What does electronegativity mean

A

It is the attraction an atom has for a shared pair of electrons in a bond

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14
Q

What electronegativities mean what type of bonding

A

0-.4 pure covalent bonding
.5-1.9 polar covalent bonding
2.0- ionic bonding

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15
Q

What properties do covalent networks possess

A

High melting and boiling point
Insoluble in water
Mostly don’t conduct electricity
All atoms joined by strong inter-molecular forces

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16
Q

What are some examples of covalent networks

A

Silicon Carbide
Silicon Dioxide
Polymorphism (allotropes) of carbon
Graphite ( conducts electricity)

17
Q

What are the properties of Discrete Covalent Molecular Bonding

A

Low melting and boiling points
Joined by weak inter-molecule bonds
Don’t conduct electricity
No charged particles or free electrons

18
Q

What are some example of covalent molecular bonding

A 
Nitrogen
Oxygen
Halogens
Sulfur (S8)
Phosphorus (P4)
Fullerene (C60)
19
Q

What are the properties of ionic bonding

A

Crystal Lattice Structure
Very strong bonds between positive and negative atoms
Conduct when Molten or in Solution
High Melting and Boiling Points

20
Q

What are the properties of Metallic Bonding

A

High Melting and Boiling Points
Conducts electricity as it contains delocalised electrons
Lots of inter-molecular forces

21
Q

What is the name for all of the intermolecular forces

A

Van Der Waavls

22
Q

What are the three Van Der Waavl Forces

A

London Dispersion Forces
Permanent Dipole -Permanent Dipole
Hydrogen Bonding

23
Q

How do London Dispersion Forces work

A

Atoms wobble
Electrons move between the poles of the atom
Causes a temporary dipole

24
Q

How do permanent dipole interaction work

A

When a bond forms between a slightly negative atom in one molecular and a slightly positive atom in another

25
Q

How does hydrogen bonding work

A

A very strong bond forms between a hydrogen atom on molecular and a Nitrogen, Fluorine or Oxygen atom in another molecule

Higher Chemistry (3 decks)

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