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Z University > BMAT Chemistry > Flashcards

BMAT Chemistry Flashcards

1
Q

Describe the structure of the atom

A

A central nucleus (containing protons and neutrons) surrounded by electrons moving in shells/energy levels/orbits

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2
Q

What are the relative masses and charges of protons, neutrons and electrons?

A
  • Proton: 1
  • Neutron: 1
  • Electron: 1/2000
  • Most of the mass of an atom is in the nucleus
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3
Q

What is atomic number?

A

number of protons

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4
Q

What is mass number?

A

number of protons + number of neutrons

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5
Q

Why does an atom have no overall charge?

A

In an atom the number of protons = number of electrons so that atoms have no overall charge

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6
Q

What are isotopes?

A

Atoms of an element with the same number of protons but different numbers of neutrons (so having different mass numbers)

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7
Q

How can chemical composition be identified?

A

From a spectra

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8
Q

What is the role of a mass spectrometer?

A

identifying isotopes and the structure of molecules

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9
Q

What are groups and periods?

A
  • Periods are horizontal rows

- Groups are vertical columns

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10
Q

What are the use of displacement reactions?

A

In establishing the order of reactivity

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11
Q

Explain how the uses of metals are related to their physical and chemical proprieties

A
  • Al: lightweight, soft and malleable: foils, aeroplane parts
  • Fe: rust easily, used to manufacture steel, cast iron for pumps
  • Cu: conducts heat and electricity well, so wires and can be drawn into wires
  • Ag: jewellery, silver tableware, used to make mirrors as best reflector of visible light known
  • Au: jewellery, soft an does not tarnish or corrode and filling cavities in teeth
  • Ti: low density high strength resent to corrosion in sea water, alloying agent, aircraft, missiles, bicycles
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12
Q

What are metal ores and what does the extraction fo metals always involve?

A
  • Metal ores are the oxides of the metal

- The extraction of metals always involves reduction processes

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13
Q

How are elements arranged in the periodic table?

A

In the order of increasing atomic number

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14
Q

What do elements in the same group have in common?

A

Elements in the same groups have similar chemical properties and that down. metal group, reactivity increases and down a non-metal group reactivity decreases

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15
Q

What are the physical and chemical properties of alkali metals (group 1)?

A
  • Low densities and low bp and mp compared to other metals (melting point decreases but density increases, down the group)
  • Very soft and become softer down the group
  • More reactive down group
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16
Q

What are the physical and chemical properties of halogens (group 7)?

A
  • Low mp and bp
  • Darker as you go down group
  • Less reactive down group
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17
Q

What are the physical and chemical properties of the noble gases (group 8)?

A
  • Odourless
  • colourless
  • Monatomic gases
  • Inert
  • Low density (density increases)
  • Low mp and bp (Increase down the group)
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18
Q

What are the common properties of transition metals?

A
  • Form coloured compounds (coloured ions)
  • Multiple stable ions
  • Used as catalysts
  • Good conductors of heat and electricity
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19
Q

Why might elements have a relative atomic masses that are not whole numbers? (e.g. CL)

A

Isotopes are responsible for this fact

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20
Q

What happens in a chemical reaction?

A
  • New substances are formed by the rearrangement of atoms but no atoms are destroyed or created; energy may be absorbed or release by the reaction
  • A chemical reaction can be described using a word equation
  • A one headed row is used to show a reaction where all the reactant can be converted into products (when the correct reacting amounts are used)
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21
Q

What are formula for a compound?

A
  1. Names of many covalent compounds SO3 sulfur trioxide

2. Recall of the names of common compounds e.g. H2SO4 as sulphuric acid

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22
Q

What are the ionic charges for ionically bonded compounds?

A
  1. Cations (positive ions) for metal elements can be found from their Group number in the Periodic Table, as can the Anions (negative ions) of non-metals
  2. The charges of polyatomic anions need to be learned e.g. CO3 2- and OH -
  3. Where a cation can have more than one charge e.g, Cu, Fe then Roman numerals are used, eg.. iron (III) chloride as FeCl3
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23
Q

What are the factors that can affect the position of the equilibrium and the rate at which the equilibrium is achieved?

A
  • Products
  • Reactants
  • Catalysts
  • Temperature
  • Pressure
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24
Q

What is the amount of a substance?

A

Number of moles of a substance

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25
Q

What does saturated mean and how do you calculate solubility?

A
  • The degree or extent to which something is dissolved or absorbed compared with the maximum possible, usually expressed as a percentage
  • Ksp = Solubility of one x solubility of two (moldm-3)
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26
Q

What are some logical reasons why, in practical solutions the percentage yield is rarely 100%?

A
  • Some of the reactants may remain unreacted when the reaction is complete.
  • Some of the product may be lost when liquids or solids are transferred from one container to another.
  • Some of the reactants may form other products.
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27
Q

What is oxidation?

A
  • Gain of oxygen
  • Removal of hydrogen
  • Loss of electrons
28
Q

What is reduction?

A
  • Removal of oxygen
  • Gain of hydrogen
  • Gain of electrons
29
Q

What are the four possibilities for any reaction?

A

-Identify any reaction as being oxidation only, reduction only, redox (both oxidation and reduction taking place) or no change in oxidation/reduction

30
Q

What is the definition for an element and a compound and what is the distinction between them?

A
  • Element: made up of one type of atom only

- Compound: when two or more different elements are chemically boned together

31
Q

Why to atoms react to form compounds?

A
  • To attain the electronic configuration of a nobel gas (the most stable configuration in the Periodic Table)
  • Understand the type of bonding taking place depends on the atoms involved in the reaction
32
Q

What are the characteristics of ionic bonding?

A
  • NaCl, MgO
  • High mp
  • Conduct electricity when molten but not in ionic lattice
33
Q

What are the characteristics of covalent (simple and giant)?

A
  • Small molecules, which contain a fixed number of atoms joined by covalent bonds
  • Giant covalent substances, which contain many atoms joined by covalent bonds
  • Giant: silicon dioxide, high mp and bp and can’t conduct electricity (except graphite), usually insoluble
  • Simple: very low mp and bp and non conductive, hydrogen and ammonia and water
34
Q

What are the characteristics of metallic bonding?

A
  • Metals consist of giant structures of atoms arranged in a regular pattern.
  • The electrons from the outer shells of the metal atoms are delocalised, and are free to move through the whole structure. This sharing of delocalised electrons results in strong metallic bonding
  • Electric conductors
  • Good conductors of thermal energy
  • High mp and bp
35
Q

What is group chemistry for group 1?

A
  1. Group 1 metals are highly reactive, and are defined as electron donor producing cations
  2. Physical properties: soft, and having for metals relatively low melting and boiling points
  3. They need to be stored under oil to prevent a reaction with air
  4. Reactivity increases down Group 1
  5. React with water: very reactive ones: vigorously
36
Q

What are the properties of transition metals?

A
  • Form stable ions in different conditions
  • Form coloured compounds
  • Used as catalysts (as ions or atoms)
37
Q

What chemical procedures are capable of separating?

A
  1. Compounds (by chemical reactions e.g. by displacement or electrolysis)
  2. Mixtures (defined as substances that my be mixed together but not chemically bonded
38
Q

What are miscible liquids (mixture)?

A

Liquids which can be separated by fractional distillation (because of differences in boiling points), or for non-volatile liquids, paper chromatography

39
Q

How do you calculate Rf value?

A

distance travelled by solute / distance travelled by solvent

40
Q

What are immiscible liquids (mixture)?

A

They can be separated using a separating funnel (the layers can be removed one at a time)

41
Q

How are soluble solids mixed with insoluble solids separated?

A

Using dissolving, filtering, evaporation or distillation and crystallisation

42
Q

What is a strong acid?

A

One which is virtually 100% ionised in solution

43
Q

What is a weak acid?

A

One which does not fully ionise when it is dissolved in water

44
Q

What is a base?

A

A proton (hydrogen ion) acceptor

45
Q

What is mono-, di-, try-, poly- protic/basic?

A
  1. Mono: contain one hydrogen ion
  2. Poly: contain multiple hydrogen ion
  3. Monoprotic acid: an acid that can only Donte one proton
  4. Polypootic acid can donate more than one proton
  5. Mono-portic base can accept one proton
  6. Polyportoic base can accept more than one proton
46
Q

What are catalysts?

A
  • A substance which alters the rate of reaction without being used up by the reaction
  • Positive catalysts increase the rate fo reaction. by providing na alternate route/reaction mechanism that has a lower activation energy
  • Catalysts are chemically unchanged at the end of a reaction and are not used up in the reaction (although there may be some physical changes, e.g. lumps to powder)
47
Q

What is an electrode?

A

A solid conductor of electricity, which is used to make electrical contact with an electrolyte

48
Q

What is a cathode?

A

Negative electrode

49
Q

What is an anode?

A

Positive electrode

50
Q

What happens in electrolysis at the cathode?

A

-The cations receive electrons (reduction) to change into atoms or molecules

51
Q

What happens in electrolysis at the anode?

A

-The anions lose electrons to from atoms or molecules (oxidation)

52
Q

Outline the electrolysis of brine

A
  1. Cl- goes to the anode and is oxidised (bleaches damp litmus paper)
    - Two chloride ions lose they electrons and become one chloride molecule
  2. H+ goes to the cathode and is reduced (litmus paper is blue)
    - Two hydrogen ions accept two electrons to become one hydrogen molecule
    - Hydrogen gas is given off
  3. NaOH is left in solution
53
Q

Why are alkanes unreactive and alkenes are?

A
  • Alkanes are chemically unreactive because of the stability of the C-C bond
  • Increased reactivity of alkenes is due to the C=C bond opening up (to form a single bond) to enable other atoms to be added on, i.e. addition reactions
54
Q

What addition reactions take place with alkenes?

A
  • Hydrogen (form alkanes)
  • Halogens (form haloalkanes)
  • Hydrogen halides (forms haloalknes)
  • Steam (forms alcohols)
55
Q

What are polymers?

A

Giant molecules made up of monomers

56
Q

What does biodegradable and non-biodegradable mean?

A
  • Able to b broken down by bacteria or other organisms)
  • Takes a long time for addition polymers to biodegrade as they are inert due to the saturated bonds which ar every strong
57
Q

What are the pollution problems of polymers?

A
  • Burning plastics can release toxic gases
  • Stay in landfill for ages
  • Best thing is to reuse and recycle
58
Q

What are the pollution problems of polymers?

A
  • Burning plastics can release toxic gases (and carbon dioxide)
  • Stay in landfill for ages
  • Best thing is to reuse and recycle, but different polymers must be separated from each other first and this can be difficult and expensive to do
59
Q

What is the general formula of alcohols?

A

RCOH

60
Q

What is the general formula of carboxylic acids?

A

RCOOH

61
Q

What are the chemical properties of alcohols?

A
  1. Polar
  2. undergo complete combustion
  3. Soluble but solubility decreases as length of alcohol molecule increases
  4. Can be oxidised to form carboxylic acids using an oxidising agent
62
Q

What are the chemical properties of carboxylic acids?

A
  1. Dissolve in water to form acidic solution
  2. React with metals to form a salt and hydrogen
  3. React with carbonates to form a salt, water and carbon dioxide
  4. React with bases to form salt and water
  5. React with alcohols to form esters
  6. Weak acid, very few of the molecules are ionised
63
Q

What are the common uses of alcohols?

A
  1. Methanol sued as chemical feedstock and is toxic
  2. Ethanol present in alcoholic drinks and is sued as a fuel and a solvent
  3. Proponal and butanol are used as solvents and fuels
64
Q

What are the common uses of carboxylic acids?

A
  1. Vinegar is a dilute solution of ethanoic acid
  2. Manufacture of soap
  3. Manufacture of many drugs e.g. aspirin
65
Q

What happens when lithium reacts with water?

A
  • Moves slowly around the surface
  • Fizzes
  • Then disappears
66
Q

What happens when sodium reacts with water?

A
  • Moves rapidly on the surface
  • Fizzes rapidly
  • May ignite
67
Q

What happens when potassium reacts with water?

A
  • React vigorously
  • Burns with a lilac flame
  • Sometimes explodes

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