Salters Chemistry, Elements From The Sea F332

Front 1

An advantage of fluorine

Back 1

Advantages
- used to make plastics such as PTFE
- used to make HCFCs
- added to toothpaste

Front 2

A disadvantage of fluorine

Back 2

Highly reactive
Handing must be kept to a minimum

Front 3

An advantage of chlorine

Back 3

Water treatment, to make pesticides, medicines and bleach

Front 4

A disadvantage of chlorine

Back 4

Pesticides can accumulate in the environment
CFCs destroy stratospheric ozone

Front 5

An advantage of bromine

Back 5

used in the manufacture of flame retardants, agricultural fumigants and in photography

Front 6

A disadvantage of bromine

Back 6

Organic bromine compounds can destroy ozone in the stratosphere

Front 7

An advantage of iodine

Back 7

Used in antiseptics, germicides and dyes
Iodine-131 used to diagnose thyroid diseases

Front 8

What structure is the lattice of sodium chloride

Back 8

Simple cubic

Front 9

Water hydrating a negative ion

Back 9

Front 10

How do you obtain an ionic equation for a reaction?

Back 10

Cross out all of the spectator ions(those which are the same on the left and right of the arrow)

Front 11

What is the ionic equation for all acid/alkali neutralisation reactions?

Back 11

H+ (aq) + OH- (aq) ---> H2O (l)

Front 12

How do you convert cm3 to dm3?

Back 12

÷1000

Front 13

What are the equations involving c, v and n

Back 13

c=n÷v n=c×v v=n÷v

Front 14

Define the first ionisation enthalpy in words

Back 14

The first ionisation enthalpy is the energy needed to remove one electron from each of one mole of isolated gaseous atoms if an element

Front 15

What is the equation for the first four ionisation enthalpies

Back 15

X(g) ---> X+(g) + e-
X +(g) ---> X 2+(g) + e-
X 2+(g) ---> X 3+(g) + e-
X 3+(g) ---> X 4+(g) + e-

Front 16

How does the first ionisation enthalpy vary down a group and why?

Back 16

-Decreases
-The outermost electron is further from the nucleus
-Electron shielding

Front 17

What is a redox reaction?

Back 17

When an oxidation reaction and reduction reaction occur simultaneously

Front 18

What is oxidation?

Back 18

The loss of electrons

Front 19

What is reduction?

Back 19

The gain of electrons

Front 20

The oxidation state of F, O, H and Cl rarely change, what are they?

Back 20

F = -1
O = -2
H = +1
Cl = -1

Front 21

Why do some compounds contain Roman numerals in brackets?

Back 21

some compounds contain elements that can exist in more than one oxidation state, when this occurs the systematic name for the compound includes the oxidation state, for example FeO is iron(II) oxide

Front 22

2Na + Cl2 ---> 2NaCl
What is the reduction half equation?

Back 22

Cl2 + 2e- ---> 2Cl-

Front 23

2Na + Cl2 ---> 2NaCl
What is the oxidation half equation?

Back 23

2Na ---> 2Na+ + 2e-

Front 24

When does a displacement reaction occur?

Back 24

When a more reactive halogen like Cl2 is passed into a solution of less reactive halide ions such as Kl

Front 25

Appearance and state of Fluorine at room temperature and it's solubility in water

Back 25

-Pale yellow gas
-soluble in water

Front 26

Volatility and solubility in organic solvents for Fluorine

Back 26

-Gas
-Soluble in organic solvents

Front 27

Appearance and state of Chlorine at room temperature and it's solubility in water

Back 27

-Green gas
-Slightly soluble to give pale green solution

Front 28

Volatility and solubility in organic solvents for Chlorine

Back 28

-Gas
-soluble to give a pale green solution in organic solvents

Front 29

Appearance and state of Bromine at room temperature and it's solubility in water

Back 29

-Dark red liquid
-Slightly soluble to give a red-brown solution

Front 30

Volatility and solubility in organic solvents for Bromine

Back 30

-Liquid quickly forms a brown gas on warming
-Soluble to give a red solution

Front 31

Appearance and state of Iodine at room temperature and it's solubility in water

Back 31

-Shiny black solid
-Barely soluble, gives a brown solution

Front 32

Volatility and solubility in organic solvents for Iodine

Back 32

-Sublimes on warming to give a purple vapour
-Soluble to give a violet solution

Front 33

Does reactivity increase or decreases down a group?

Back 33

Decreases

Front 34

Chlorine, Bromine, and Iodines precipitate colours

Back 34

-Chlorine, white precipitate of silver chloride
-Bromine, cream precipitate of silver bromide
-Iodine, yellow precipitate of silver iodine

Front 35

Shells are divided into sub shells called...

Back 35

s, p, d and f

Front 36

How many electrons can sub shell s hold?

Back 36

2

Front 37

How many electrons can sub shell p hold?

Back 37

6

Front 38

How many electrons can sub shell d hold?

Back 38

10

Front 39

How are the orbitals filled?

Back 39

The orbitals are filled in order of increasing energy

Front 40

If there are more than one orbital at the same energy level what happens?

Back 40

The orbitals are first occupied by one electron

Front 41

When does a dipole occur?

Back 41

when a molecule(or part of a molecule) has a positive end and negative end

Front 42

What makes an instantaneous dipole?

Back 42

If the electron density is unevenly distributed at any one time, because the distribution is always changing the polarity will change

Front 43

What makes a permanent dipole?

Back 43

When there is a big enough difference in electronegativity, the slightly positive end attracts the slightly negative end

Front 44

What is electronegativity?

Back 44

The degree to which an atom of an element attracts electrons

Front 45

Generally where are the more electronegative elements?

Back 45

Towards the top right of the Periodic Table

Front 46

Do C-Hal bond strength increase or decrease down a group and why?

Back 46

-Decreases down the group
-As the atom size increases

Front 47

Does the reactivity increase or decrease down a group?

Back 47

-Increases down the group
-As the bonds become easier to break

Front 48

What are the conditions for homolytic fission?

Back 48

Gas phase with high temperatures or the presence of UV radiation

Front 49

What are the conditions for heterolytic fission?

Back 49

Dissolved in a polar solvent such as an ethanol/water mixture

Front 50

What is a nucleophile?

Back 50

They have one or more lone pairs of electrons that they can donate to form new bonds

Front 51

What are two example of a nucleophile?

Back 51

Just three examples
- hydroxide ion
-water
-ammonia

Front 52

what are the conditions needed to react ammonia with a halogenoalkane?

Back 52

Halogenoalkane is heated with concentrated ammonia solution in a sealed tube

Front 53

What are the five main stages in the purification of 1-bromobutane after it's production from butan-1-ol?

Back 53

Halogens are immiscible in water:
1)separate the organic layer and aqueous layer using a separating funnel
2)shake the product with sodium hydrocarbonate to remove any acid impurities
3)separate the product from the immiscible aqueous layer using a separating funnel
4)dry the product with anhydrous sodium sulfate
5)purify by simple distillation

Front 54

Advantages of batch process's

Back 54

-Cost effective for small quantities
-Low capital cost for plants
-Different products made using the same vessel

Front 55

Disadvantages of batch process's

Back 55

-Filling cleaning and emptying reaction vessel is time consuming
-may require larger workforce
-contamination possible if making different products

Front 56

Advantages of continuous process's

Back 56

-Suited to high tonnage products
-Can operate for months at a time without a shut down
-More easily automated,so workforce can be smaller

Front 57

Disadvantages of continuous process's

Back 57

-Less flexible- usually designed. to make one product
-Much higher capital cost in building the plant
-Not cost effective if run below full capacity

Front 58

What is the equation to work out percentage yield?

Back 58

% yield = actual mass of product÷ relative formula mass of the product used × 100

Front 59

What is the equation to work out atom economy?

Back 59

% atom economy = relative formula mass of useful product ÷ relative formula mass of reactants used × 100

Front 60

What are the differences between a by-product and a co-product?

Back 60

-By-products are made through an unwanted side reaction
-Co-products are made through the desired chemical reaction, but it isn't the target product

Front 61

Suggests why locating a new chemical plant on an existing site of a chemical manufacture can lower costs

Back 61

-The infrastructural such as a road network is already in place
-A skilled workforce is available

Front 62

Why might a company manufacturing bleach want to site it's self near a chlor-alkali plant?

Back 62

Two of the products in the plant (sodium hydroxide and chlorine) are feedstocks in the production of bleach

Front 63

What is a feedstock?

Back 63

The reactant that go into a production process