EL 7 - Blood, sweat, and seas

Question 1

What reactants produce magnesium sulfate?

Answer 1

sulfuric acid + magnesium

Question 2

What reactants produce lithium chloride?

Answer 2

hydrochloric acid + lithium oxide

Question 3

What reactants produce barium sulfate?

Answer 3

barium chloride + magnesium sulfate

Question 4

What reactants produce sodium ethanoate?

Answer 4

ethanoic acid + sodium carbonate

Question 5

What reactants produce ammonium nitrate?

Answer 5

nitric acid + ammonium hydroxide

Question 6

Give an example of a use of magnesium sulfate

Answer 6

bath salts

Question 7

Give an example of a use of lithium chloride

Answer 7

lithium batteries

Question 8

Give an example of a use of barium sulfate

Answer 8

‘barium meal’ shows up soft tissue on x-ray

Question 9

Give an example of a use of sodium ethanoate

Answer 9

hand warmers

Question 10

Give an example of a use of ammonium nitrate

Answer 10

fertiliser

Question 11

Name all of the period 3 elements (in order)

Answer 11

Na, Mg, Al, Si, P, S, Cl and Ar

Question 12

What do Na and Mg oxides (basic oxides) produce when they are added to water?

Answer 12

An alkali

Question 13

How can aluminium oxide be described (what type of oxide)?

Answer 13

An amphoteric oxide - can react with acids/alkalis

Question 14

What do Al and Si oxides produce when added to water?

Answer 14

The products are the same as the reactants as both Al and Si oxides don’t dissolve in water

Question 15

What type of oxides are Na and Mg oxide?

Answer 15

basic oxides

Question 16

What types of oxides are Si, P, S and Cl oxide?

Answer 16

acid oxides

Question 17

What do Si, P, S and Cl oxides produce when they are added to water?

Answer 17

An acid

Question 18

Define electronegativity

Answer 18

The tendency of an element to attract electrons in a covalent bond

Question 19

How would you describe the difference in the electronegativity of ionic bonds?

Answer 19

Big difference in electronegativity

Question 20

How would you describe the difference in the electronegativity of polar covalent bonds?

Answer 20

Medium

Question 21

How would you describe the difference in the electronegativity of covalent bonds?

Answer 21

Small

Question 22

What does an oxyanion consist of?

Answer 22

XOy^z-
X: another element
y: no. of oxygen atoms
z-: negative ion

Question 23

What is the difference between a cation and an anion?

Answer 23

Cation: positive ion
Anion: negative ion

Question 24

What products are made from acid + alkali?

Answer 24

salt + water

Question 25

What products are made from acid + base?

Answer 25

salt + water

Question 26

What products are made from acid + carbonate?

Answer 26

salt + water + carbon dioxide

Question 27

What products are made from acid + metal?

Answer 27

salt + hydrogen

Question 28

Many ionic substances dissolve in water but which ones don't?

Answer 28

- barium, calcium, lead and silver sulfates - silver + lead halides - all metal carbonates - metal hydroxides (except group 1 and ammonium hydroxides)

Question 29

What happens when ionic substances dissolve and what does this allow them to do?

Answer 29

The ions become surrounded by water molecules and spread out through the solution. Once separated, behave independently of each other. This presence of hydrated ions in solution explains why aqueous solutions of salts can conduct electricity.

Question 30

What are spectator ions?

Answer 30

The ions that are non involved in the reaction (+ not part of the ionic equation)

Question 31

What is ionic precipitation?

Answer 31

A suspension of solid particles is produced by a chemical reaction in solution

Question 32

Name the solution that is added to Cu2+, the name of the precipitate formed and what colour it is

Answer 32

Solution added: sodium hydroxide Precipitate formed: copper hydroxide Colour of precipitate: blue

Question 33

Name the solution that is added to Fe2+, the name of the precipitate formed and what colour it is

Answer 33

Solution added: sodium hydroxide Precipitate formed: iron (II) hydroxide Colour of precipitate: (dirty) green

Question 34

Name the solution that is added to Fe^3+, the name of the precipitate formed and what colour it is

Answer 34

Solution added: sodium hydroxide Precipitate formed: iron(III) hydroxide Colour of precipitate: orange/brown

Question 35

Name the solution that is added to Pb^2+, the name of the precipitate formed and what colour it is

Answer 35

Solution added: potassium iodide Precipitate formed: lead iodide Colour of precipitate: bright yellow

Question 36

Name the solution that is added to Cl^-, the name of the precipitate formed and what colour it is

Answer 36

Solution added: silver nitrate Precipitate formed: silver chloride Colour of precipitate: white

Question 37

Name the solution that is added to Br^-, the name of the precipitate formed and what colour it is

Answer 37

Solution added: silver nitrate Precipitate formed: silver bromide Colour of precipitate: cream

Question 38

Name the solution that is added to I^-, the name of the precipitate formed and what colour it is

Answer 38

Solution added: silver nitrate Precipitate formed: silver iodide Colour of precipitate: pale yellow

Question 39

Name the solution that is added to SO4^2-, the name of the precipitate formed and what colour it is

Answer 39

Solution added: barium chloride Precipitate formed: barium sulfate Colour of precipitate: white

Question 40

Give the ionic equation of Cu and sodium hydroxide

Answer 40

Cu^2+(aq) + 2OH^-(aq) -> Cu(OH)v2(s)

Question 41

Give the ionic equation of sulfate and barium chloride

Answer 41

Ba^2+(aq) + SOv4^2- -> BaSOv4(s)

Question 42

Give the ionic equation of iodine and silver nitrate

Answer 42

Ag^+(aq) + I^-(aq) -> AgI(s)

Question 43

What shape do ionic compounds often form?

Answer 43

lattice + regularly shaped crystals

Question 44

What substances have an ionic structure?

Answer 44

Compounds of metals with non-metals

Question 45

What substances have a covalent network structure?

Answer 45

Some elements in group 4 and some of their compounds

Question 46

What substances have a metallic structure?

Answer 46

Metals

Question 47

What substances have a simple molecular structure?

Answer 47

Some non-metal elements and some non-metal/non-metal compounds

Question 48

What substances have a macromolecular structure?

Answer 48

Polymers

Question 49

Give an example of a compound that has an ionic structure

Answer 49

NaCl and CaO

Question 50

Give an example of a compound that has a covalent structure

Answer 50

Diamond, graphite and silica

Question 51

Give an example of a compound that has a metallic structure

Answer 51

Na, Cu and Fe

Question 52

Give an example of a compound that has a simple molecular structure

Answer 52

COv2, Clv2 and Hv2O

Question 53

Give an example of a compound that has a macromolecular structure

Answer 53

poly(ethene), nylon, proteins and DNA

Question 54

What type of particles does an ionic structure contain?

Answer 54

ions

Question 55

What type of particles does a covalent network contain?

Answer 55

atoms

Question 56

What type of particles does a metallic structure contain?

Answer 56

positive ions surrounded by delocalised electrons

Question 57

What type of particles does a simple molecular structure contain?

Answer 57

small molecules

Question 58

What type of particles does a macromolecular structure contain?

Answer 58

long-chain molecules

Question 59

How are the particles bonded in an ionic structure?

Answer 59

Strong ionic bonds - attraction between oppositely charged ions

Question 60

How are the particles bonded in a covalent structure?

Answer 60

Strong covalent bonds - attraction of atom's nuclei for shared electrons

Question 61

How are the particles bonded in a metallic structure?

Answer 61

Strong metallic bonds - attraction of atom's nuclei for delocalised electrons

Question 62

How are the particles bonded in simple molecular structure?

Answer 62

Weak intermolecular bonds between molecules - strong covalent bonds between the atoms within molecules

Question 63

How are the particles bonded in a macromolecular structure?

Answer 63

Weak intermolecular bonds between the atoms within molecules - strong covalent bonds between the atoms within the molecules

Question 64

What are the typical properties/boiling or melting points of ionic, covalent (network), metallic, simple molecular and macromolecular structures?

Answer 64

Ionic: high Covalent (network): very high Metallic: generally high (except mercury) Simple molecular: low Macromolecular: moderate - often decompose on heating

Question 65

What is the hardness of an ionic, covalent (network), metallic, simple molecular and macromolecular structure?

Answer 65

Ionic: hard but brittle Covalent (network): very hard (if three-dimensional) Metallic: hard but malleable (except mercury) Simple molecular: soft Macromolecular: variable - many are soft but often flexible

Question 66

What is the electrical conductivity of ionic, covalent (network), metallic, simple molecular and macromolecular structures?

Answer 66

Ionic: electrolytes conduct when molten or dissolved in water Covalent (network): do not normally conduct (except graphite) Metallic: conduct when solid or liquid Simple molecular: do not conduct Macromolecular: do not normally conduct

Question 67

What is the solubility of an ionic, covalent (network), metallic, simple molecular and macromolecular structure like in water?

Answer 67

``` Ionic: often soluble Covalent (network): insoluble Metallic: insoluble (but some react) Simple molecular: usually insoluble, unless molecules contain groups which can hydrogen bond with water Macromolecular: usually insoluble ```

Question 68

What is the solubility of an ionic, covalent (network), metallic, simple molecular and macromolecular structure like in non-polar solvents (e.g hexane)?

Answer 68

``` Ionic: insoluble Covalent (network): insoluble Metallic: insoluble Simple molecular: usually soluble Macromolecular: sometimes soluble ```