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Inorganic Chemistry Flashcards

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1
Q

State three characteristics of
the Alkali Metals

A

All have one electron in their outer shell; have low density; are stored
under oil (to prevent reactions with oxygen or water); are soft (can be cut
with knife).

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2
Q

How do Group 1 elements react with non-metals? Why are these reactions similar for the different Group 1 elements?

A

They form ionic compounds which are soluble white solids which form
colourless solutions – they all have one electron in their outer shell.

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3
Q

How do Group 1 elements
react with water?

A

They release hydrogen gas and form hydroxides which dissolve to form alkaline solutions; react vigorously with water fizzing and moving around on the surface of the water.

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4
Q

How does the reactivity change moving down Group 1? Why?

A

It increases as the atoms get larger and the distance between the nucleus and the outer electrons increases and thus attraction from the nucleus decreases, allowing them to more easily lose electrons.

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5
Q

State five characteristics of Group 7

A
  • 7 electrons in outer shell
  • Coloured vapours
  • Diatomic molecules
  • Form ionic salts with metals
  • Form molecular compounds with non-metals
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6
Q

State Group 7 elements and their states of matter.

A
  • Fluorine, F. F2 is a pale yellow gas.
  • Chlorine, Cl. Cl2 is a pale green gas.
  • Bromine, Br. Br2 is dark brown liquid (gives off orange vapour at room temperature).
  • Iodine, I. I2 is a grey solid (gives off purple vapour when heated).
  • Astatine, At. At2 solid at room temperature.
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7
Q

State three changes that occur in Group 7 as one moves down the group

A
  • Higher relative molecular mass
  • Higher melting and boiling point
  • Less reactive – electrons less easily gained
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8
Q

A more reactive halogen displaces a less reactive
one from an aqueous solution of its salt; write the
equations and state the colour change seen when
chlorine reacts with sodium bromide and when
chlorine/bromine reacts with sodium iodide.

A

more reactive halogen displaces a less reactive one from an
aqueous solution of its salt; write the equations and state the colour
change seen when chlorine reacts with sodium bromide and when
chlorine/bromine reacts with sodium iodide.

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9
Q

A more reactive halogen displaces a less reactive
one from an aqueous solution of its salt; explain the
trend in reactivity of halogens in these reactions

A

A more reactive halogen displaces a less reactive one from an aqueous solution of its salt; explain the trend in reactivity of halogens in these reactions
Reactivity decreases down the group. As we go down the group, the atoms get larger, so an incoming electron will be less tightly held by the attractive forces from the nucleus. That’s why Cl2 displaces Br– and I–
.

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10
Q

What are the “rules” for solubility of salts?

A
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11
Q

What is rusting?

A

It is a process of forming hydrated iron (III) oxide.
When iron is exposed to water and air, it forms hydrates of Fe2O3
.
This leaves a brown deposit on the surface of a material.

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12
Q

Outline how you would prepare a sample of PbSO4

A
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13
Q

Outline how you would prepare a sample of NaCl from NaOH and HCl

A

In this case, we don’t know when to stop adding one of the reagents - there is no indication of the completion of our reaction.
You can use an indicator in this case, just like in acid/base titration. Adding one of the reagents by a burette will help with accuracy.
Then boil the mixture to remove some solvent and leave to crystallise. Filter and dry the product.

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14
Q

You have a sample of a pure liquid. How could you check its identity?

A

Measure the boiling point.
Say we have water - it boils at 100 Celsius degrees

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15
Q

How can you show that a liquid contains pure water?

A
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16
Q

What is an oxidising agent?
What is a reducing agent?

A

An oxidising agent is a species that gets reduced in a redox reaction (gains electrons; causes the oxidation of another substance).
A reducing agent is a species that gets oxidised in a redox reaction (loses electrons; causes the reduction of another substance).

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17
Q
A
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18
Q

State the colours of flames observed when lithium, sodium, and potassium burn in oxygen

A

Crimson-red, Li
Yellow-orange, Na
Lilac, K

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19
Q

How to conduct a titration?

A
  1. Rinse the pipette with a solution of unknown concentration. Use the pipette to measure out the known volume of this solution.
  2. Add an indicator (a substance that changes colour at the end of titration)
  3. Rinse the burette with a solution of known concentration. Discard the liquid. Use a burette to gradually add the solution of a known concentration.
  4. When indicator changes colour (at the end point), the volume added is recorded.
  5. It is important to get concordant volume results - they have to lie close to each other.
  6. Suitable calculations are performed to find the concentration.
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20
Q

What is oxidation/reduction?

A

Oxidation is the addition of oxygen to a substance. Reduction is the loss of oxygen from a substance

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21
Q

What is the reactivity series of metals? What are the trends in reactivities of metals in reactions with acids/water?

A
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22
Q

What is a displacement
reaction?

A

A reaction where a more reactive metal displaces a less reactive metal in a compound.

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23
Q

What is the general equation for a reaction between metals and acids? What type of reaction is this?

A

Metal + acid → salt + hydrogen
Redox reaction, also a displacement reaction.

24
Q

What is the general equation for a
neutralisation reaction?

A

Acid + Base → Salt + Water

25
Q

What is the general equation for the reaction between metal carbonate and acid?

A

Metal Carbonate + Acid → Salt + Water + Carbon Dioxide

26
Q

What is the general equation for the reaction between metal oxide and acid?

A

Metal Oxide + Acid → Salt + Water

27
Q

What is a redox reaction?

A

A reaction where both oxidation and reduction occurs

28
Q

How is a soluble salt formed?

A
  1. Add an insoluble base (e.g. metal oxide) to warm acid to form a soluble salt and water until no more base will dissolve (the acid has been completely neutralised).
  2. Filter off the leftovers (excess solid base).
  3. Heat the solution to evaporate the water then leave the salt to crystallise.
29
Q

What do acids and alkalis produce in aqueous solutions?

A

Acids produce hydrogen ions, alkalis produce hydroxide ions.

30
Q

What are bases, acids and alkalis?

A
  • Bases are compounds that neutralise acids to produce a salt.
  • Acids are substances that produce hydrogen ions in aqueous solutions.
  • Alkalis are soluble bases that produce hydroxide ions in aqueous solutions.
31
Q

What is the pH scale and what does a pH of 7 show?

A

The measure of acidity/alkalinity of a solution; neutral solution.

32
Q

State the general equation for a neutralisation reaction in a short, ionic form.

A
33
Q

What is a concentrated acid and what is a dilute acid? Is this the same as a strong and weak acid?

A
  • Concentrated has more moles of acid per unit volume of water than dilute (dilute refers to solutions of low concentrations).
  • Not the same - concentration is not the same thing as strength of an acid.
  • Strength refers to whether the acid is completely ionised in water (strong) or only partially (weak).
34
Q
A

Lithium nitrate
Potassium carbonate
Magnesium bromide
Barium sulfate

35
Q

Describe the tests for hydrogen, oxygen, carbon dioxide and chlorine

A
36
Q

Describe the flame test results

A

Lithium compounds - crimson red flame.
Sodium compounds - yellow flame.
Potassium compounds - lilac flame.
Calcium compounds - orange-red flame.
Copper compounds - blue-green flame.

37
Q

Describe the sodium hydroxide test results and write the equations

A
38
Q

Describe the test for carbonate anions

A
39
Q

Describe the test for sulfate anions

A
40
Q

Describe the proportions of gases in the modern atmosphere

A
41
Q

What is the greenhouse effect? What are greenhouse gases? Give examples

A

Greenhouse gases in the atmosphere maintain temperatures on Earth high enough to support life.
They allow short wavelength radiation from the sun to pass through the atmosphere to the Earth’s surface, but absorb and reflect back the outgoing long wavelength radiation from the Earth causing an increase in temperature.

Water vapour, carbon dioxide, and methane.

42
Q

How have human activities led to an increase in greenhouse gases?

A

Carbon dioxide – combustion of fossil fuels and deforestation.
Methane – increased farming and decomposition in landfills.

43
Q

What are the potential effects of global climate change?

A
  • Sea level rise, which may cause flooding and increased coastal erosion.
  • Melting of glaciers and polar ice caps.
  • More frequent and severe storms.
  • Changes in the amount, timing and distribution of rainfall.
  • Temperature and water stress for humans and wildlife.
  • Changes in the food-producing capacity of some regions.
  • Changes to the distribution of wildlife species.
44
Q

What are the issues regarding sulfur dioxide and oxides of nitrogen?

A

Sulfur dioxide and oxides of nitrogen cause respiratory problems in humans and cause acid rain. Acid rain kills animals (by making the lakes in which they live in acidic) and damages plants and buildings

45
Q

Compare Group 1 metals and transition metals

A

Group 1 metals and transition metals are heat and electricity conductors. They are shiny when polished and form ionic compounds with non metals.
Transition metals have higher densities and higher melting points than Group 1 metals. They are less reactive and harder than Group 1 metals.

46
Q

State three common characteristics of transition metals

A
  • Form ions with different charges
  • Coloured compounds
  • Catalytic properties
47
Q

How are unreactive metals found in Earth?

A

In their natural state, that being the metal alone rather than in a compound (well, they are unreactive…).

48
Q

How can metals less reactive than carbon be extracted?

A

Reduction with carbon. Carbon displaces the metal in a metal oxide - gets oxidised to carbon oxides. Metal from the metal oxide gets reduced to the pure metal.

49
Q

How are metals more reactive than carbon extracted?

A

By electrolysis.

50
Q

How are oxidation and reduction defined in terms of electron transfer?

A

Oxidation – loss of electrons.
Reduction – gain of electrons

51
Q

Which metals in the reactivity series will react with acid?

A

Those above hydrogen.

52
Q

Explain in terms of gain or loss of electrons which species has been oxidised and which species has been reduced when magnesium reacts with hydrochloric acid

A
53
Q

What is a strong acid?
What is a weak acid?

A

Strong acid is completely ionised in aqueous solution; weak acid is only partially ionised in aqueous solution.

54
Q

What happens to pH as concentration of H+ increases?

A

It decreases.

55
Q

As the pH is decreased by one unit, what change is seen in the hydrogen ion concentration?

A

Increases by a factor of 10

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