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22 Cards in this Set
- Front
- Back
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Non-Metals
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Upper right side of the Periodic table
Have low melting and boiling points Do not conduct electricity Are soft and brittle in solid form Decrease in reactivity going down the group because the atomic radii gets bigger and the attraction between the + and the - become weaker so the want to gain electrons is less. |
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Covalent Bonding
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When a pair of valence electrons are shared between non-metals.
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Molecule
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Covalently bonded atoms
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Allotrope
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Different physical structures in which an element can exist.
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Nitrogen
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Atomic no. 7
Mass no. 14 Clear gas Odourless Soluble E.A: 2, 5 Ion charge: -3 Makes 78% of atmosphere |
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Ammonia
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NH3
Used in fertiliser N2 + 3H2 --> 2NH3 Ion is called 'ammonium' - NH4 (-1) |
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Haber Process
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Making of Ammonia
Nitrogen + Hydrogen --> (Iron catalyst + 450c + 200 atmospheres) --> Ammonia gas + coolant --> Liquid ammonia |
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Oxygen
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Atomic no. 8
Mass no. 16 Clear gas Odourless Soluble E.A: 2, 6 Ion charge: -2 Makes 21% of atmosphere Used in: steel industry and welding tools to increase combustion temperature (also bonds with unwanted C that leaves as gasses); hospitals to assist with respiratory system. |
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Ozone
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Allotrope of oxygen
Pale blue gas Pungent smell Less stable than O2 Central O atom double bonded to another O, and single bonded to another O. Formed by UV light or an electrical discharge being run through O2. O2 + O --> O3 |
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Chlorine
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Atomic no. 17
Mass no. 35.5 Pale green gas Pungent smell Soluble E.A: 2, 8, 7 Ion charge: -1 Toxic Used in: water purification, bleach |
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Carbon
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Atomic no. 6
Mass no. 12 Solid Insoluble Allotropes are diamond, graphite and buckyballs. E.A: 2, 4 Does not form ion. |
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Organic Chemistry
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The study of carbon
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Diamond
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Allotrope of carbon
Covalently bonded to 4 other C atoms Strongest natural substance (forms tetrahedral lattice) Insoluble in anything Colourless Does not conduct electricity Giant molecular structure Used in jewellery, cutting tools, abrasives |
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Graphite
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Allotrope of carbon
Covalently bonded to 3 C atoms; 1 valence electron holds the 2D layers together. Insoluble Dark silver Relatively soft Conducts electricity Giant molecular structure Used as dry lubricant, pencil 'lead', batteries, fishing rods, bike frames |
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Buckyballs/Buckminsterfullerene
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Allotrope of carbon
Covalently bonded to 2 C atoms (singular bond) and 1 double bond to form a hexagonal shape - looks like a football Soluble in petrol Electrical conductor Used as catalyst, cages to put material in |
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Sulfur
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Atomic no. 16
Mass no. 32 Brittle, yellow solid Odourless (NB: it's sulfur dioxide that smells not sulfur itself) Insoluble E.A: 2, 8, 7 Ion charge: -1 Found near volcanic activity |
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Sulfuric Acid
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H2SO4
Made using the Contact Process Used in: fertilisers, lead acid battery, cleaning |
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Contact Process
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S combusted with O2 --> SO2
SO2 + O (+ Vanadium pentoxide)--> SO3 (exothermic - produces 400 - 600c heat which may be used) SO3 + Conc. H2SO4 showered down --> Oleum (H2S2O7) (Waste SO2 gas is neutralised by filters - CaCO3) H2S2O7 + H2O --> 2H2SO4 |
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Oleum
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H2S2O7
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Bromine
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Atomic no. 35
Mass no. 80 Reddish brown liquid (only non-metal liquid) Strong smell Toxic |
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Why are most non-metals gasses at room temperature?
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The intermolecular bonds are weak so are easy to break apart.
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Why don't most non-metals conduct electricity?
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They do not have free electrons to carry the charge.
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