paper 1

Question 1

give 3 features of a transition metal.

Answer 1

malleable
strong
high m.p

Question 2

how does a metal conduct electricity?

Answer 2

metals have delocalized electrons that are free to move through the lattice structure.

Question 3

what is an ionic bond?

Answer 3

bond between metal and non-metal

Question 4

in an ionic bond, describe the transfer of electrons

Answer 4

metal to non-metal

Question 5

in an ionic bond, what forces hold it together?

Answer 5

electrostatic forces.

Question 6

what form do ions have to be in order to conduct electricity?

Answer 6

molten or dissolved

Question 7

why don’t ions conduct electricity while solid?

Answer 7

the ions are fixed (cannot move)

Question 8

describe the covalent bonding

Answer 8

2+ non-metals sharing electrons.

Question 9

What forces hold together a covalent bond?

Answer 9

electrostatic between electrons and nuclei.

Question 10

what is the bonding of a diamond?

Answer 10

covalent

Question 11

what is the structure of a diamond?

Answer 11

giant covalent structure
no free electrons
each carbon atom forms 4 bonds

Question 12

why do giant covalent structures have a very high m.p?

Answer 12

due to strong covalent bonds that require a lot of energy to break.

Question 13

why can the fullerene be used in medicine?

Answer 13

the ball structure means it can act as a cage to carry the drug

Question 14

what is the formula for moles?

Answer 14

mass / rfm

Question 15

what metals are most reactive?

Answer 15

lithium, sodium and potassium

Question 16

what forces hold the graphite layers together?

Answer 16

intermolecular forces

Question 17

what forces hold a metallic bond together?

Answer 17

electrostatic forces between delocalized electrons and positive metal ions

Question 18

why are metals more reactive than each other?

Answer 18

the outer shell of the more reactive one is further from the nucleus. Weak electrostatic forces so electrons can be lost easily.

Question 19

what is a noble gas?

Answer 19

completely unreactive gases

Question 20

name a strong acid

Answer 20

Hydrochloric acid (HCl)

Question 21

name a weak acid

Answer 21

citric acid

Question 22

give 3 differences between transition metals and group 1 elements.

Answer 22

high density (tm)
malleable (TM)
hard (tm)

Question 23

Name one other compound that the student could add to hydrochloric acid to produce
zinc chloride

Answer 23

zinc hydroxide OR zinc carbonate

Question 24

why is rubidium more reactive than potassium?

Answer 24

as the outer electrons are further away from the nucleus, meaning there is less electrostatic attraction. This means the electrons are easier to lose.

Question 25

why is there a mesh to separate the products during electrolysis?

Answer 25

to ensure the products don't react.

Question 26

what particle may pass through the net during electrolysis?

Answer 26

an ion

Question 27

what element is produced at the anode?

Answer 27

oxygen unless halogens are present.

Question 28

what element is produced at the cathode?

Answer 28

hydrogen is produced unless the metal is less reactive than it.

Question 29

what are nanoparticles used for? | why?

Answer 29

catalysts as they react fast, increasing the r.o.r

Question 30

name 3 common acids | name their formula?

Answer 30

hydrochloric (HCL) Sulfuric (H2SO4) Nitric (HNO3)

Question 31

# usually hydroxides or carbonates name 2 common bases | can you name their formula?

Answer 31

sodium hydroxide (NaOH) calcium carbonate (CaC03)

Question 32

what 2 ways can ph be measured?

Answer 32

chemical indicator Ph probe

Question 33

uinversal indicator becomes more what in acidic solutions? and what in alkaline?

Answer 33

red bluey purple

Question 34

# Litmus is an indicator for titrations Name the colour Litmus is in both alkali and acidic solutions

Answer 34

Red in acidic blue in alkali

Question 35

# Methyl orange is a titration indicator Name the colour of methyl orange in both alkali and acidic solutions

Answer 35

red in acidic yellow in alkali

Question 36

# think when you add them to water what makes an acid strong or weak?

Answer 36

How much they ionise in water (split apart)

Question 37

define the term base

Answer 37

a substance that has a ph level of over 7

Question 38

what is an insoluble base?

Answer 38

a base which does not dissolve in water

Question 39

# thinks positive and negative ions in neutralisation reactions, how do you work out the formula of the salt?

Answer 39

take the positive ion from the base, such as sodium from sodium oxide (**Na**2O), and the negative ion from the acid, such as chloride from hydrochloric acid (H**Cl**), and combine them together. NaCl

Question 40

when metal reacts with water what does it form?

Answer 40

metal hydroxides + hydrogen