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Chemistry > General knowledge - including all definitions > Flashcards

General knowledge - including all definitions Flashcards

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1
Q

Proton Number

A

The

number of protons in the nucleus of an atom

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2
Q

Nucleon Number

A

The
total number of protons and neutrons in the
nucleus of an atom

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3
Q

Isotopes

A

The same element
which have the same proton number but a
different nucleon number

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4
Q

Relative Atomic Mass

A

The average
mass of naturally occurring atoms of an element
on a scale where the 12C atom has a mass of
exactly 12 units

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5
Q

Relative Molecular mass

A

The sum

of the relative atomic masses in a molecule

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6
Q

Mole

A

1 mol is the amount of substance that contains the same number of particles as there are atoms in 12.0 g of carbon-12

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7
Q

Avogadro constant

A

Number of units in one mole of any substance, equal to 6.02214076 × 10^23

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8
Q

Electrolysis

A

The breakdown of an ionic
compound, molten or in aqueous solution, by the
passage of electricity

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9
Q

Redox

A

It is a reaction in which an element is both oxidized and reduced

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10
Q

Oxidizing agent

A

A substance which
oxidizes another substance during a redox
reaction.

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11
Q

Reducing agent

A

A substance
which reduces another substance during a redox
reaction.

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12
Q

Polymers

A

Large molecules built up from small units

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13
Q

Acids

A

Proton donors

When acids dissolve in water to form an aqueous solution, they produce hydrogen ions (H+). These H+ ions make the aqueous solution acidic.

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14
Q

Bases

A

Proton acceptor

A base is a substance that can neutralize the acid by reacting with hydrogen ions.

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15
Q

Alkali

A

Any base that dissolves in water is called an alkali

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16
Q

Atom

A

A particle which can no longer be broken down by chemical means

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17
Q

Ions

A

A charged particle which is charged because of an imbalance of protons and electrons

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18
Q

Molecules

A

Two or more atoms chemically combined

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19
Q

Mixture

A

Two or more substances mixed together but not chemically combined

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20
Q

Solute

A

What is being dissolved

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21
Q

Solvent

A

What are we dissolving in

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22
Q

Solution

A

Solute + solvent = Solution

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23
Q

Saturated solution

A

No more solute can dissolve at a given volume and temp of solvent

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24
Q

Volatile liquid

A

A liquid which evaporates quickly

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25
Q

A pure substance

A

A substance with no particles of any other substance mixed into it

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26
Q

Impurity

A

An unwanted substance mixed in with the desired substance

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27
Q

Methods of separation

A

Filtration

Crystallization

Evaporation

Simple distillation

Fractional distillation

Paper chromatography

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28
Q

Residue and Filtrate

A

Filtering Chalk and water through filter paper, the chalk would be trapped as residue and the water would go through as a filtrate

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29
Q

Rf value

A

Distance moved by solutes/ Distance moved by solvent

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30
Q

Element

A

An element contains only one type of atom

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31
Q

Radioactive

A

Unstable-nucleus

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32
Q

Properties of metals

A 
Conduct heat and electricity 
Sonorous
High bp and mp
Shiny when polished
Hard and strong
Malleable and Ductile

(chemical)
React with oxygen to form basic oxides
Form positive ions

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33
Q

Properties of non metals

A

Do not conduct
Low mp and bp
dull
britlle

(chemical)
React with oxygen to form acidic bases
Form negative ions

34
Q

A compound

A

Two or more elements chemically combined

35
Q

Signs of chemical change

A

One or more new substance is formed

Energy is taken in or given out

It is difficult to reverse

36
Q

Allotropes

A

Two forms of the same element, Diamond and graphite

37
Q

Valency

A

The number of electrons an atom, gains/loses or shares to form a compound

38
Q

Purity formula

A

(Mass of pure substance/total substance)x100%

39
Q

Electrolyte

A

A liquid that contains ions and therefore conducts electricity

40
Q

Uses of chlorine

A

(yellow-green poisonous)

Plastic PVC

Medical drugs

Bleaches

Hydrochloric acid

Herb/Pesticides

41
Q

Uses of Sodium hydroxide

A

(corrosive)

Soaps

Detergents

Paper

Medical drugs

42
Q

Uses of hydrogen

A

Nylon

Hydrogen peroxide

Harden vegetable oils to make margarine

Fuel for hydrogen fuel cells

43
Q

Tests for water

A

Water will turn

White anhydrous copper (II) sulfate blue

Blue cobalt chloride paper pink

44
Q

Dynamic equilibrium

A

In a closed system the rate of forward and back reaction of a reversible reaction are equal, meaning no overall change is happening

45
Q

Rate

A

A measure of change that happens in a single unit of time

46
Q

Noble gases and their uses

A

Helium-Fills balloons and airships

Argon-Inert atmosphere for lightbulbs, Welding

Neon- Glowing signs

Krypton- Lasers and car headlamps

Xenon- Car headlamps, Hospital lights, light house lights

47
Q

Reactivity series

A 
Potassium, K
Sodium, Na
Calcium, Ca
Magnesium, Mg
Aluminum, Al
Carbon, C
Zinc, Zn
Iron, Fe
Lead, Pb
Hydrogen, H
Copper, Cu
Silver, Ag
Gold/Platinum, Au/Pt
48
Q

Precious metals

A

Metals which are rare and scarce such as gold, silver, platinum or palladium.

49
Q

Aluminum Oxide

A

Bauxite

50
Q

Iron (III) oxide ore

A

Hematite

51
Q

Zinc sulfide

A

Zinc Blend

52
Q

Zinc extraction and uses

A

Zinc blend is roasted in air (to react with Oxygen)

The Zinc oxide formed is the reacted with Carbon monoxide to obtain pure zinc.

Zinc is used in

  • Galvanizing
  • Sacrificial protection
  • Alloys, such as brass and bronze
  • Batteries
53
Q

Iron extraction

A

Coke burns giving out heat and carbon dioxide

Unreacted carbon reacts with carbon dioxide to form carbon monoxide.

Hematite (Iron (III) oxide) is reduced by the Carbon monoxide

Limestone is added, which decomposes into lime and reacts with the impurity sand to form Calcium silicate (slag) that runs off

54
Q

Aluminum extraction and uses

A

Electrolysis

Bauxite dissolved in molten cryolite to lower mp

Aluminum forms at cathode and runs off

Oxygen formed reacts with carbon anodes to form carbon dioxide. Because of this the carbon anodes must be replaced periodically

Used in

  • Aircrafts
  • Food/drink containers
  • Overhead power cables
  • Cooking foil
55
Q

Alloys

A 
Brass (copper and zinc)
Mild steel (Iron and carbon[buildings, cars and ships])
Stainless steel (nickel, chromium and steel[cutlery, medical and chemical equipment])
56
Q

Fractional distillation of air

A

Air is first filtered to remove dust, carbon dioxide and water

Compressed and cooled till liquified (condensed)

Nitrogen -196 (top fraction)

Argon -186

Oxygen -183

Krypton -153

Xenon -108 (bottom fraction)

57
Q

Uses of Oxygen

A

Oxygen masks

Oxygen tents

Reserve for pilots and astronauts

Purifying iron in steel production

58
Q

Uses of Nitrogen

A

Liquid nitrogen to quick freeze food

Unreactive so used to replace oxygen in food packaging

59
Q

Pollutants

A

Carbon monoxide

Sulfur dioxide

Nitrogen oxides

Lead

60
Q

Effects of Carbon monoxide and its source

A

(from incomplete combustion eg in car engines)

Effect: Binds to hemoglobin in irreversible reaction, leading to death by oxygen starvation

61
Q

Effects of Sulfur dioxide and its source

A

(fossil fuels)
Effect: Causes respiratory problems and dissolves in rain to from acid rain which eats away at building, statues and can kill plants and fish by lowering the pH of their land or lake/river.

62
Q

Effects of Nitrogen oxides and its source

A

(heat from car engines causes Nitrogen in air to react with Oxygen in air)[and lightning strikes]
Effect: Causes respiratory problems and causes acidic rain

63
Q

Effects of lead and its source

A

(petrol)

Effect- Brain damage for children, Kidney and nervous system issues for adults

64
Q

Rust

A

Fe2O3.2H2O (rusting is sped up in salt water)

65
Q

Water treatment

A

Screening traps large particles

Coagulant clumps small particles together

Flotation tanks cause coagulated particles to float and be skimmed off

Sand bed filtration

Charcoal to remove bad tastes and smells

Chlorine to kill microbes

Fluorine added to fight tooth decay

Pumped to reservoir (storage)

66
Q

Haber process

A

Gasses mixed and scrubbed

Compressed

Passed over Iron catalyst at 450 degrees and 200atm

Cooled ammonia (liquid stored) un reacted gas is recycled

67
Q

Sources of hydrogen

A

Electrolysis of water

Cracking hydrocarbons

Methane and steam

68
Q

Fertilizers

A

NPK (nitrogen, phosphorus and potassium)

Ammonium sulfate/Nitrate/phosphate

Potassium sulfate

69
Q

Lead sulfide

A

Galena

70
Q

Sulfur is found where and in what state?

A

Found as the element in Mexico, Poland and USA

71
Q

Properties of sulfur

A

Brittle and yellow

Two allotropes (rhombic and monoclinic)

Low mp

Insoluble in water

reacts with metals to form sulfides

72
Q

Uses of sulfur

A

Produce sulfuric acid

Vulcanizing (toughening rubber)

Drugs, paper, and pesticides

Cosmetics, shampoo, and lotion

Sulfur concrete which doesn’t react with acid (used in acid production factories)

73
Q

Sulfur dioxide properties and uses

A

Colourless gas heavier than air with a strong chocking smell

Disolves in water to form sulfurous acid (H2SO3)

Acts as bleach when damp or in solution (turns litmus white)

Kills bacteria

Uses:

Production of sulfuric acid

Bleaching wool/ silk/wood pulp for paper

Sterilizing agent used in making soft drinks/ jams/ dried fruit

74
Q

Contact process

A

Sulfur burned in air to get Sulfur dioxide

Passed over Vanadium (V) oxide at 450 degrees and 2 atm to form Sulfur trioxide(SO3)

Dissolved in conc H2SO4 to form oleum

Mixed carefully with water to form H2SO4

75
Q

Uses of sulfuric acid

A

(corrosive)

Plastics and fibers

Soaps and detergents

Fertilizers such as ammonium sulfate

Paints and pigments

76
Q

Water to acid or acid to water?

A

Acid to water always, as water to acid is highly exothermic and could burn you if splashed

77
Q

Concentrated Sulfuric acid

A

Dehydrating agent which removes all Hydrogen and oxygen form sugar molecules leaving only black carbon

Mixed with water, highly exothermic

78
Q

Limestone uses

A 
[CaCO3]
(Crushed) 
Extracting iron from hematite
Road building
Chips for concrete

(powdered)
Neutralize acidity in soil
Desulfurization

(heated with clay)
Cement

79
Q

Lime

A

[CaO (by thermoly decomposing limestone)]
Making steel from iron
Neutralize acidic soil
Drying agent

80
Q

Slaked lime

A

[Ca(OH)2] Lime + water
Neutralize acidic soil and lakes
Desulfurization

81
Q

Limestone in a kiln

A

Limestone is heated in a rotary kiln with a fan blowing through the kiln to blow away carbon dioxide which would otherwise react with the Calcium Oxide to form Limestone again

82
Q

Flue gas desulferization

A

SO2 coming out of the chimney (flue) at power stations reacts with Calcium Hydroxide to form calcium sulfate that is then turned into gypsum (hydrated calcium sulfate) by reacting with oxygen and water

SO2 + Ca(OH)2 —> CaSO3 +H2O

2CaSO3 + H2O + 4O2 —> 2CaSO4.2H2O

Chemistry (3 decks)

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