Paper 1

Question 1

What is ionic bonding?

Answer 1

Ionic bonds form between metal ions and non-metal ions. A transfer of electrons.

Question 2

What is covalent bonding?

Answer 2

Covalent bonding form between non-metals and non-metals. Forms when atoms share electrons.

Question 3

Do metals gain or lose electrons?

Answer 3

Metals lose electrons to become positive ions.

Question 4

Do non-metals gain or lose electrons?

Answer 4

Non-metals gain electrons to form negative ions.

Question 5

What are isotopes?

Answer 5

Atoms of the same element, that have the same number of protons, but a different number of neutrons.

Question 6

What did Mendeleev’s periodic table feature?

Answer 6

He placed them in the order of their atomic weights. He then arranged them so that a periodic pattern in their properties could be seen. He left gaps for elements that hadn’t been discovered, using the table to predict what their properties would be.

Question 7

Why are the noble gases mainly unreactive?

Answer 7

The atoms have eight electrons in their outermost shell. This very stable electron arrangement makes them less reactive.

Question 8

Why are the alkali metals so reactive?

Answer 8

They only have one electron in their outermost shell. They only need to lose one electron to get the stable electronic structure of a noble gas, meaning they’re very reactive.

Reactivity increases down the group.

Question 9

What is produced when alkali metals react with water?

Answer 9

Hydrogen and an alkaline solution containing the metal hydroxide.

Question 10

How does reactivity change in Group 7?

Answer 10

The reactivity of the halogens decreases going down the group. They all have 7 electrons in their outermost shell, so they only need to gain one to be stable.

Question 11

What are the transition metals?

Answer 11

Metals between Group 3 and Group 3.

• Conductive
• Strong, hard, and dense (due to metallic bonding)

Question 12

How can graphite conduct electricity?

Answer 12

The delocalised electrons can move along its layers. Electrons will drift from the negative terminal in a battery towards a positive terminal in a circuit.

Question 13

What is metallic bonding?

Answer 13

The outer electrons from a metal can move through the structure, and form a sea of free moving electrons surrounding the positively charged metal ions. Strong electrostatic attraction between the negatively charged electrons and the positive ions bond the metal ions to each other.

Question 14

What are nano particles? What are some of their properties and uses?

Answer 14

Nanoparticles are small objects that are between 1 and 100 nanometers in size.
Properties) They have a very high surface area to volume ratio, meaning their properties can be very extreme
Uses) Sun cream, anti-microbial, carbon nano fibre coat foam.

Question 15

What is the Avogadro constant?

Answer 15

6.02 x 10(23)

Question 16

How would you calculate moles from mass?

Answer 16

Moles= Mass divided by rfm

Question 17

How do you calculate mass from moles?

Answer 17

Mass= number of moles x rfm

Question 18

When is titration is used?

Answer 18

To measure accurately what volumes of acid and alkali react together completely.

Question 19

What is the reactivity series?

Answer 19

1) Potassium
2) Sodium
3) Lithium
4) Calcium
5) Magnesium
6) Aluminium
7) Carbon
8) Zinc
9) Iron
10) Hydrogen
11) Copper
12) Silver
13) Gold

Question 20

What is oxidation?

Answer 20

The loss of electrons, and the gain of oxygen.

Question 21

What is reduction?

Answer 21

The gain of electrons, and the loss of oxygen.

Question 22

How can metal be extracted by carbon?

Answer 22

Carbon can displace a less reactive metal from their oxides. By heating the metal oxide with carbon, it releases carbon dioxide and the metal.

Metals more reactive than carbon can’t be extracted in this way, they’re extracted by electrolysis.

Question 23

How are salts made?

Answer 23

1) acid + alkali —> salt + water
2) acid + metal —–> salt + hydrogen
3) acid + metal carbonate —–> salt + water + carbon dioxide

Question 24

What are bases?

Answer 24

Substances that neutralise an acid. This includes alkali-soluble bases, like hydroxides.

Question 25

What is the ionic equation for neutralisation?

Answer 25

H+(aq) + OH–(aq) → H2O(l)

Alkalis are OH-
Acids are H+

Question 26

What are weak acids?

Answer 26

Acids with a low concentration of H+ ions, a lower pH.

- Organic acids, like carboxylic acids

Question 27

What are strong acids?

Answer 27

Acids with a higher concentration of H+ ions. Lower pHs.
-Mineral acids, like HCL, HNO3

The higher the concentration of H+ ions, the lower the pH

Question 28

What is the negative electrode, and what type of ion goes to it?

Answer 28

The Cathode

-Positively charged electrons

Question 29

What is the positive electrode, and what type of ion goes to it?

Answer 29

The Anode

-Negatively charged electrons

Question 30

What are the rules considering the changes at the electrodes?

Answer 30

1)The least reactive is changed at the electrodes
2) If the aqueous solution contains a high concentration of halide ions, then the halide is given off at the anode, not oxygen
A redox reaction is any reaction where you have both oxidisation and reduction.

Question 31

What’s the difference between exothermic and endothermic energy changes?

Answer 31

Exothermic is transferred to the surroundings

Endothermic is transferred from the surroundings

Question 32

What is battery made up of?

Answer 32

Two or more chemical cells joined together. Electrons flow from the more reactive metal to the less reactive.