Chemistry equations

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103 Terms

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Concentration
Concentration gdm3 \= mass / volume (dm3)
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Convert cm3 to dm3
Divide by 1000
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Number of moles in a substance
Number of moles \= mass (g) / R.F.M
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empirical formula
a chemical formula showing the ratio of elements in a compound rather than the total number of atoms
-find number of moles and divide by smallest number
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molecular formula
actual number of atoms
-find empirical mass and divide rfm by it
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Avogadro constant
in 1 mole of a substance, there are 6.02 x 10^23 particles of the substance
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Percentage yield
Actual yield/ theoretical yield x 100
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theoretical yield
Add the R.F.M
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Atom economy
R.F.M useful products / R.F.M of reactants x 100
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Concentration in mol dm3
Number of moles in solute / volume of solute dm3
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Concentration in mol dm3
Concentration gmd3 / r.f.m solute
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Rf
distance substance travels from origin/ distance solvent travels from origin
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Amount of gas mol
Vol of gas / molar vol (24dm3)
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metal + water →
metal hydroxide + hydrogen
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Metal + Acid
Salt + Hydrogen
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ionic bond
Formed when one or more electrons are transferred from one atom to another, metal + non metal
Do not conduct as solid but as liquid or dissolved conduct
High melting point: strong electrostatic bonds between ions
Soluble in water: water molecules slight electrical charge, attracting ions away from the lattice
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covalent bond
a bond formed when atoms share one or more pairs of electrons, non metal + non metal
Molecular solids: low melting ans boiling points however larger solid stronger molecular forces
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Graphite
Only three out of four electrons in carbon involved so can conduct electricity and soft and slippery, lube, malleable
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Diamond
Massive covalent
High melting + boiling
Can't conduct electricity
V hard
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metallic bonding
a bond formed by the attraction between positively charged metal ions and the electrons around them, giant lattice w delocalised electrons\=conduct
Malléable: sea of electrons slide over each other
High melting point: string bonds
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Smart alloy
Metal that changes shape depending on temperature
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Allotrope
Different structural forms of the same element
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What is pH?
the measure of the hydrogen ion concentration in a solution. If you decrease the concentration of H+ ions by a factor of 10 the ph increase by 1
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Strong acids
Fully dissociate into H+ ions
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Acid + Base
Salt + Water
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Acid + Carbonate
Salt + Water + Carbon Dioxide
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concentrated solution
a solution containing a large amount of solute dissolved in small amount of solvent
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Bases
Bases neutralise acids. They are hydrogen ion acceptors. When they react, they accept H+ions.
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Acids
Acids are hydrogen ion donors. When they react, they release H+ ion(s).
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soluble in water
sodium, potassium, and ammonium compounds, nitrates, MOST chlorides, MOST sulfates
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insoluble in water
Silver lead carbonates, lead barium calcium sulfate, MOST carbonates, MOST hydroxides
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Reactivity series
Potassium
sodium
calcium
magnesium
aluminium
Carbon
zinc
iron
lead
Hydrogen
copper
silver
gold
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Anodes
Electrodes where oxidation occurs, anions (negative ions) go, positive, non metals, oxygen forms
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Cathode
Reduction, negative, cations (positive ions) go, metals, hydrogen forms
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Ore
a rock that contains a large enough concentration of a mineral making it profitable to mine
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METHODS OF EXTRACTION
Higher than carbon: electrolysis
Lower than carbon: displacement reaction with carbon
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Bioleaching
Process of extraction of metals from ores using microorganisms. Bacteria produce solution called a leachate where copper extracted via displacement and purified by electrolysis
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Phytoextraction
The process by with plants exact metals from soil or water and store them above ground. Burnt to get the element
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Equilibrium
Increase of temperature exothermic direction (to the right)
Increases of pressure favours reaction which produces less moles (to the right)
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Haber process
450 dégrées, 200 atmosphères, iron catalyst
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Properties of transition metals
-malleable
-good conductors of electricity
-high melting points
- high densities
- typically show catalytic activity
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Fermentation Advantages
-made from renewable carbohydrates
-lower temperature
-low pressure
HOWEVER ITS SLOW AND PRODUCT IS IMPURE
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Properties of alkali metals
-malleable
-conduct electricity
-low melting points
-very reactive
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Properties of halogens
-non metallic
-poor conductors of heat and electricity
-toxic and corrosive
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Properties of noble gasses
-colourless
-low melting and boiling points
-poor conductors of heat and electricity
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Metal properties
Shiny, malleable, ductile, conductive, and sometimes magnetism
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Non metal properties
Low melting points
Not shiny
Brittle
Low density
Poor conductors of electricity
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Insoluble in water
-silver, lead chloride
-lead, barium, calcium sulfates
-most carbonates
-most hydroxides
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Water for drinking treatment
-sedimentation tank
-filtration tower including sand and gravel
-chlorination which kills micro organisms
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Calculate r.a.m from abundances
Total mass of the atoms / number of atoms
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R.A.M
The mean mass of an atom of an element compared with carbon-12
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Mendeleev's periodic table
Organized by 3 criteria: 1- atomic mass 2- reactivity and 3- formula
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-ide ending
In two element compounds the non-metal ends in ide
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polyatomic ion
an ion made of two or more atoms
If it contains oxygen it ends in -ate or -ite
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Neutralisation reaction
Acid + base \= salt + water
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Polymer
A long molecule consisting of many similar or identical monomers linked together.
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Fullerene
A molecule in which each carbon atom is covalently bonded to three other carbon atoms, forming tubes or spheres
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functional group
Group of Atoms that is responsible fir te molecules chemical reactions and properties
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fuel cell
A device that converts chemical energy to electrical energy.
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Homologous series
same general formula and similar chemical properties but different number of carbon atoms
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Halide ion
Negatively charged ion formed from one of the group 7 elements
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Nanoparticle
Tiny pieces of a substance with a diameter between 1 nanometre and 100 nanometres
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Alkaline tests
Litmus: blue
Methyl orange: yellow
Phenolphthalein: pink
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Acid tests
Litmus: red
Methyl Orange: red
Phenolphthalein: colourless
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Fractions of crude oil
Gases
Petrol
Kerosene: fuel for aircraft
Diesel
Fuel
Bitumen: surfacing roads
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Properties of fractions of crude oil
Top: small carbons, low boiling point, easy to ignite, flows easy
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Alkanes
Alkanes
CnH2n+2
React with oxygen to form carbon dioxide + water
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Complete combustion
Only oxygen and water are given out and energy is produced
If not carbon monoxide is produced
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Hydrocarbon pollutants
Car engines 'internal combustion' and oxides of nitrogen are produced
Contain impurities such as carbon
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Saturated
Carbon atoms are joined only be C-C
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Cracking
Large alkane molecules split into alkane and alkane
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Alkenes
CnH2n
Unsaturated
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Isomers
Molecules with the same molecular formula but different arrangements of atoms
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Bromine water test
Alkanes do not cause de-colourisation
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Alcohols
CnH2n+1
Have the functional group OH
Produce oxygen and water on complete combustion
Can be oxidised to form carbolyxic acids
React with sodium
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carboxlyic acid
CnH2n+1 COOH
FORM ACIDIC solutions
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carboxlyic acid + metal
\= salt + hydrogen
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carboxlyic acid + base
\= salt + water
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carboxlyic acid + carbonates
\= salt + water + carbon dioxide
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Poly (ethene)
Flexible, cheap
Plastic bags
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Poly (propène)
Flexible, does not shatter
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Poly (chloroethene) PVC
tough, hard
Window frames
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PTFE (teflon)
Tough, slippery
Non stick pans
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condensation polymerization
2 monomers react to form a larger unit while a small molecule, water is the by product
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Flame tests
Wire loop dipped in HCL before testing each sample
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Lithium
Red
Li+
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Sodium
Yellow
N'a+
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Potassium
Lilac
K+
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Calcium
Orange-red
Ca2+
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Copper
Blue/green
CU2+
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Sodium Hydroxide tests
Test for metal precipitation reaction
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Iron
Fe2+ \= green
Fe3+ \= Brown
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Copper
Cu2+ \= blue
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Calcium, aluminium
Ca2+, Al3+ \= white
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Ammonium test
Damp red litmus paper blue
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Carbonate ions test
Add HCL to substance and see if lime water goes cloudy
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Sulfate ions test
Add HCL to remove carbon ions and than add barium chloride to give white precipitate
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Halide ion test
Add nitric acid to remove carbon atoms and add silver nitrate to see precipitate (white Cl-, cream Br-, yellow I-)
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composite material
A material with two or more materials combined to produce a material with improved properties
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matrix material
In a composite material, the substance that binds the reinforcement material together