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Higher Chemistry > Unit One > Flashcards

Unit One Flashcards

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1
Q

How do you find relative rate

A

1/time

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2
Q

What changed the rate of reaction (ppctA)

A

Pressure
Particle size
Concentration
Temperature
Add a catalyst

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3
Q

How can activation energy be changed

A

Activation energy cannot be changed unless with a catalyst

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4
Q

What is temperature the measure of

A

Average kinetic energy

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5
Q

What happens to the number of particles with energy equal to or greater than the activation energy when the temperature is increased

A

Particles increase

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6
Q

Why does increasing temperature increase the reaction rate

A

Speed of particles has increased leading to more collisions
Collide with higher energy so higher chance of successful collisions

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7
Q

Describe Haber process

A

Reactants= nitrogen and hydrogen
Products = ammonia
Catalyst = iron

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8
Q

Describe Ostwald process

A

Reactants = ammonia and oxygen
Products = nitric acid
Catalyst = platinum

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9
Q

What is meant by the term activation energy

A

The lowest energy required for a reaction to occur

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10
Q

Adsorption (action of a catalyst)

A

One of the reactant molecules is adsorbed onto the surface of the catalyst it is held in place by weak bonds with the active sites on the catalyst. This weakens the reactant

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11
Q

Reaction (action of catalyst)

A

With the reactant held at the correct geometry and the chemical finds weakened, successful collisions can occur. The activation energy is lowered because I’d the reactant being adsorbed

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12
Q

Desorption (action of a catalyst)

A

The product molecules leave the active sites of the catalyst to be reused in further chemical reactions

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13
Q

Give an example of a catalytic converter

A

Reactants= carbon monoxide nitrogen oxide
Products= co2 and nitrogen
Catalyst= platinum

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14
Q

What is meant but the term activated complex

A

Unstable intermediate arrangement of atoms formed as old bonds are breaking and new bonds forming

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15
Q

What is meant by the term enthalpy

A

The potential energy involved in reactants becoming products

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16
Q

What must occur for a chemical reaction to take place

A

Particles must collide
Collisions must have sufficient energy
Reacting particles must have correct orientation

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17
Q

Give an example of catalyst poisoning

A

Iron catalyst used in Haber process will rust so it needs to be replaced or scrubbed

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18
Q

What are the names of the groups

A

Group one- alkali metals
Group two- alkali earth metals
Group seven- halogens
Group eight- Nobel gasses

19
Q

What happens to the covalent radius when going across a period

A

From left to right electrons are being added to the same energy level and protons are being added to the nucleus. The electrons in the outer energy level are therefore attracted more strongly to the nucleus making the radius smaller

20
Q

What happens to the covalent radius as you move down a group

A

The number of occupied electron energy levels increases. The shells are being increased so is the shielding because there are many shells. There are no values for the covalent radii of monoatomic asses as they do not form covalent bonds easily.

21
Q

What is the covalent radius a measure of

A

Half of the distance between atoms

22
Q

What is the meaning of the first ionisation energy

A

The amount of energy required to remove one mole of electrons from one mole of atoms In the gaseous state

23
Q

What is the meaning of the second ionisation energy

A

The amount of energy required to remove one mole of electrons from one mole of 1+ ions in the gaseous state

24
Q

Why is the second ionisation energy always higher than the first

A

On the second not much energy more positive 2nd and 3rd very stable, require a lot because it wants to stay stable

25
Q

What happens to the ionisation energy across a period

A

More protons are being added through the period. So the electrostatic attraction will be increased Arabs the outer electrons more strongly so there will need to be more energy

26
Q

What happens to the ionisation energy in a trend going down a group

A

It decreases base there is more outer shells so they will be further away from the nucleus so there is less force of attraction therefore it will be easier to remove the electron. With less energy.

27
Q

What happens to the electronegativity across the period

A

It increases because of the increased nuclear charge

28
Q

How can you increase rate of reaction

A

Particle size decrease increase surface area so more a collisions will occur
Concentration increase so more reactant more chance of collision
Temperature increase more energy, increased speed more chance of collision
Adding a catalyst faster reaction help geometry to collide

29
Q

What is a pure covalent bond

A

When atoms involved in the bond have an equal share of bonding electrons

30
Q

What is a polar covalent bond

A

When atoms with different electronegativity values join together

31
Q

What type of molecules have permanent dipole permanent dipole interaction

A

Molecules that are polar

32
Q

What is a highly electronegative element

A

Nitrogen,oxygen or fluorine

33
Q

What happens as the relative atomic mass in the halogen increases

A

Boiling point increases

34
Q

What is the definition of electronegativity

A

A measure of the attraction of an element for bonding electrons

35
Q

Why is the third ionisation energy higher than the second

A

Successive ionisation energies increase as the atoms become more positive

36
Q

Where does the melting and boiling point values peak

A

At carbon and silicon

37
Q

What happens as you go down group 7

A

Increase in mp so
An increase in the force of attraction

38
Q

What do melting and boiling points show

A

Periodic properties
This means that they vary in a regular way or pattern depending on their position in the periodic table

39
Q

What do the melting points and boiling points depend on

A

The strength of forces which exist between the particles which make up a substance

40
Q

What is the definition of density

A

The mass per unit volume

41
Q

Where does density values peak

A

at boron(a group three element)in group two and aluminium a group three element in period three

42
Q

What happens to density going down a group

A

It increases

43
Q

What is the definition of London dispersion force

A

They are formed as a result of electrostatic attraction between temporary dipoles and induced dipoles Inducrd by movement of electrons in atoms and molecules

Higher Chemistry (3 decks)

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