Paper 1

Question 1

What is an Ion?

Answer 1

-An atom that either loses/gain electrons
-To from a charged particle

Question 2

Give the Relative Mass & Relative charge of Subatomic Particles

Answer 2

PROTONS
RM - 1
RC - +1
NEUTRON
RM - 1
RC - 0
ELECTRON
RM - 0.0005
RC - -1

Question 3

What is the Atomic Radius of an Atom?

Answer 3

10(-10)m

Question 4

1.What is the Mass No.
2. What is the Atomic No.
3.How do you find the No. of neutrons

Answer 4

1. No. Of Protons + Neutrons
2. Proton No. (=Electrons No.)
3. Mass No. - Atomic No.

Question 5

Give the History of the Atom

Answer 5

-Dalton - Solid spheres, couldn’t be broken down, different for different elements
-Thompson - discovered the charge & mass prove smaller particles, (-) electrons. (PPM)
-Rutherford - gold foil exp. (alpha particles), PPM, some where deflected backwards (not fully positive atom). Nuclear Model, (+) nucleus, electrons surround nucleus. Nucleus deflected alpha particles
-Bohr - ‘cloud’ electrons would attract nucleus and collapse atom. Electrons contained in shells.

Question 6

What is an Isotope?

Answer 6

Different forms of the same element, which have the same number of protons but a different number of neutrons.

Question 7

Isotopes have the same (1)________ _____ but a different (2) ________ _____.

Answer 7

1. Atomic Number
2. Mass Number

Question 8

What is Electrolysis?

Answer 8

The process of using electricity to separate the elements in insoluble ionic compounds.

Question 9

What is an Electolyte?

Answer 9

A liquid/solution that contains an ionic compound (ions are free to move)

Question 10

What are Electrodes?

Answer 10

Electrical conductors in Electrolysis

Question 11

Why must electrolytes be molten/liquid?

Answer 11

So the ions are free to move

Question 12

If a metal oxide is less reactive than carbon, then they are split by the Reduction of Carbon. Why do industries prefer this?

Answer 12

Because it’s cheaper than electrolysis.

Question 13

The Anode is (1)_________ and (2)_____________ ions.
The Cathode is (3)_________ and (4)___________ ions.

Answer 13

1. Positive
2. Oxidises
3. Negative
4. Reduces

Question 14

The Negative Cathode attracts the (1)_________ ion from the compound, and the positive anode attracts the (2)_________ ions.

Answer 14

1. Metal
   2.Negative

Question 15

What ions would you find in the water of an electrolyte?

Answer 15

Hydrogen and Hydroxide ions

Question 16

What is a Covalent Bond?

Answer 16

Strong bonds that are formed when a pair of electrons are shared between atoms.

Question 17

1. Give the three examples of Simple Molecular Substances?
2. What do they all have in common?

Answer 17

1. Any from: Hydrogen, Hydrogen Chloride, Water, Methane, Oxygen, Carbon Dioxide.
2. All made by Covalent Bonds

Question 18

Substances containing covalent bonds normally have what?

Answer 18

Simple Molecular Structures (e.g. H2O and CO2)

Question 19

Covalent Bonds are very (1)________, however they have weak (2) _____________ _______.

Answer 19

1. Strong
2. Intermolecular Forces

Question 20

Properties of Covalent Bonds

Answer 20

• Melting/Boiling Points are low (breaking the intermolecular force, not bond)
• (most) substances are gases/liquids at room temp.
• Bigger Molecules have bigger M.p/B.P because the strength of intermolecular forces increases.
• Don’t conduct electricity (not charged, no free electrons/ions).

Question 21

What is Metallic Bonding, and what does it involve?

Answer 21

Bonding between Metals only.

It involves the electrons on the outer shell being delocalised, there are strong forces of electrostatic attraction between the +ions and -ions. These forces hold the atoms in a regular structure.

Question 22

What are the Properties of Metals/Metallic Bonding?

Answer 22

At least 3 from:

• High M.p/B.p (strong electrostatic forces between ions & delocalised electrons are strong, so more energy is needed).
• Shiny Solids (at room temp).
• Not soluble in Water
• More dense than non-metals (ions closely packed)
• Malleable
• Good Conductors of Electricity
• Ductile

Question 23

What are Fullerenes and what is their bonding?

Answer 23

Fullerenes are molecules made up of carbon atoms, arranged into rings and structured like a tube or hollow sphere.
They are made from Covalent bonding.

Question 24

1. Why are fullerenes used to deliver drugs around the body?
2. Why are Fullerenes good industrial catalysts?

Answer 24

1. The fullerene structure is hollow so it can ‘cage’ other molecules (the drug). This then allows it to deliver a drug directly to the cell.
2. They have a huge surface area, which allow other individual catalysts to be attached to them.

Question 25

Give the two main Fullerenes.

Answer 25

Nanotubes and Buckminsterfullerene

Question 26

Explain what a carbon Nanotube is and its properties

Answer 26

A carbon nanotube is a type of fullerene, structured like a hollow tube and is made of cylinders of graphene (causes it to conduct electricity) PROPERTIES • conducts electricity • high tensile strength (don’t break when stretched) - used to strengthen materials without adding weight (e.g sports equipment).

Question 27

Explain what Buckminsterfullerene is and give its molecular formula

Answer 27

Buckminsterfullerene is a hollow sphere made up of carbon hexagons/rings; it’s a stable molecule that forms soft brown/black crystals and has a molecular formula of C60.

Question 28

What is a Polymer and how is it formed?

Answer 28

Polymers are molecules of long chains, made of covalently bonded carbon atoms. They are formed when smaller molecules called monomers join together.

Question 29

Give a famous example of a Polymer

Answer 29

Poly(ethene)

Question 30

Why doesn’t the mass in a closed system change?

Answer 30

Because there is no way the products can evaporate/escape, therefore the mass will remain the same. (Also because no atoms are created or destroyed).

Question 31

What does it mean is the mass increasing during a chemical reaction?

Answer 31

Because one of the reactants will (probably) be a gas. The gas is in the air, but not in the reaction vessel (can’t measure its mass). During the reactions, the gas reactants with the reactants to form the product, so the mass of the reaction vessel increases

Question 32

What does it mean if the mass decreases during a chemical reaction?

Answer 32

Before the reaction, all the reactants are in the reaction vessel. If the vessel isn’t enclosed then the gas can escape (evaporation), therefore the total mass inside the reaction vessel decreases.

Question 33

Explain the process in Ionic bonding

Answer 33

Ionic bonding is when a metal and a non-metal transfer a pair of elections • The metal will lose elections to form a positively charged ion, a cation. • The non-metal will gain the electrons that the metal lost to form a negatively charged ion, an anion.

Question 34

What is the force called between the ions in an ionic bond

Answer 34

Electrostatic Force

Question 35

What does the group number of an element tell you about it?

Answer 35

How many electrons the an atom will either lose or gain

Question 36

What is an Ionic Compound?

Answer 36

Any compound that only contains ionic bonds

Question 37

Give the properties of ionic compounds

Answer 37

• High m.p/b.p (lots of strong bonds between the ions - a lot of energy is needed) • can’t conduct electricity when solid but can when molten • Some ionic compounds dissolve in water, because the ions separate and are free to move in the solution (so they carry an electric charge).

Question 38

Explain why ionic compounds can’t conduct electricity when solid but can when their molten

Answer 38

When an ionic compound is solid, the ions are closely packed together (in a regluar lattice structure) and held by very strong electrostatic forces. The ions are held in place, therefore there are no delocalised electrons to hold an electric current. However, when molten, the energy overcomes the forces, making the ions free to move and therefore able to carry and electric charge

Question 39

Give two reasons why percentage yield might be less than 100%

Answer 39

• Incomplete Reactions • Side Reactions

Question 40

Give two other indicators other than Universal Indicators

Answer 40

• Litmus Paper • Methyl Orange

Question 41

What are the two types of reactions in Reversible Reactions?

Answer 41

• Forward Reactions • Backward Reactions

Question 42

Explain what Rates the Reversible Reactions happen at and at what point do they reach equilibrium?

Answer 42

(Usually), the forward reactions quickly happens first, then the slower backward reaction happens after. However, they do eventually acth up to the same speed - and by this point the concentrations of reactants and products won’t change anymore. The reaction is now at Equilibrium.

Question 43

What happens when a reversible reaction reaches Equilibrium?

Answer 43

• The forward & backward reaction are still happening (but at the same speed), therefore they cancel each other out

Question 44

True or Flase: At a reversible reaction the reactants and products are constant, so that means they are the same amount as each other.

Answer 44

False In a Reversible Reaction, the reactants and products are constant, but that does not mean they have the same amount. E.g, just because there’s a big amount of the reactant, doesn’t mean that the products will also have high masses

Question 45

Reversible Reactions at Equilibrium are constant, but the reactants & products don’t always have the same mass. Explain How this affects the position of the Equililbrium. (Hint: you need three main points to answer this question)

Answer 45

• If there is a larger amount of products than reactants, the position of equilibrium lies to the Right. • If there is larger amount of reactants than products, the position of equilibrium will lie to the left. • However, the position of equilibrium can changed depending on the conditions. For example, if you add heat to a reversible reaction, the amount of product will grow larger and therefore the equilibrium will move to the right. Whereas, if you cooled the conditions of the reaction, the amount of reactants will grow larger than the products and therefore the equilibrium will move back to the left.

Question 46

What type of Reaction vessel must a reaction have to take place in if you want it to reach equilibrium?

Answer 46

A closed system, so no reactants or products can escape (incomplete reaction)

Question 47

How do you know which reaction in a reversible reaction is Endothermic & exothermic.

Answer 47

If you increase the temperature, the equilibrium would shift to the left, and therefore the reaction would be exothermic, vice versa.

Question 48

What is Le Chatelier’s Principle?

Answer 48

If there’s a change in concentration, pressure or temperature in a reversible reaction. The equilibrium position will move to counteract that change.

Question 49

What three things can impact the position of equilibrium?

Answer 49

• Temperature • Pressure • Concentrations

Question 50

Free Card on Le Chateliers principle

Answer 50

If the Temperature, pressure and concentration in a reversible reaction, the equilibrium position Will always move to counteract that change.

Question 51

1. What is the Haber Process 2. Give the equation for the Haver process

Answer 51

1. The industrial production of forming Ammonia from Nitrogen & Hydrogen 2. N2 + 3H2 ⇌ 2NH3

Question 52

Explain the Characteristics of the Haber Process Reaction

Answer 52

• 450 degrees Celsius • 200 atmospheres • Iron Catalyst • Produces Heat (Exothermic) • Reversible Reaction

Question 53

Explain how the Haber Process Works

Answer 53

1. Gaseous Nitrogen & Hydrogen are fed into the reaction vessel (containing an iron catalyst). The conditions are kept at 450C and at 200 atm. 2. Some of the Nitrogen &. Hydrogen react together to form Ammonia (however, because it’s a reversible reaction, there will still be a lot of hydrogen & ammonia. 3. Ammonia is fed into a condenser, ammonia had a low b.p. Ammonia condenses to liquid Ammonia. 4. Nitrogen & Hydrogen have higher b.p so they remain gaseous in the condenser. Therefore they are recycled and put back into the reaction vessel.

Question 54

For the Haber Process to work, we need a temperature of 450 degrees Celsius and a pressure of 200 atmospheres. Explain why (in terms in % yield, rate of reaction & costs)

Answer 54

450 DEGREES CELSIUS • % Yeild - need a low temp to favour the forward reaction • Rate of Reaction - high temp, so particles have lots of kinetic energy in order to react. • Cost - generating too much heat is expensive 200 ATMOSPHERES • % Yield - High pressure so particles collide more frequently. • Rate of Reaction - high because of % Yield. • Cost - expensive but also for safety reasons (high pressure can be dangerous)