Chemistry AQA GCSE Triple Higher Paper 1 - Statistics

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Answer Stats

Hint	Answer	% Correct
Elements are made up of ___ type of atom	One	85%
Separation of insoluble solids from liquids is done by ___	Filtration	49%
Compounds are formed when different elements are ___ ___ in fixed proportions	Chemically bonded	40%
Pour mixture into funnel. Insoluble solids remain in the ___ ___ and liquids pass through into flask	Filter paper	34%
Avogadro's constant = ___ x 10^23	6.02	32%
Mol = ___ / Mr	Mass	29%
Separation of a solid dissolved in water is done by ___	Crystallisation	26%
Atoms of the same element that have different numbers of neutrons	Isotopes	18%
___ were the first subatomic particles discovered	Electrons	16%
Number of protons in one atom of an element (same as number of electrons as atoms have no overall charge)	Atomic number	15%
Put paper into a chromatography tank with solvent ___ the line	Below	15%
To separate a mixture of more than two liquids	Fractional distillation	15%
Draw a ___ ___ near the bottom of the paper, add spots of colouring	Pencil line	15%
Nowadays, the periodic table is sorted by ___ ___	Atomic number	13%
Going ___ the group, reactivity increases	Down	13%
Titrations RP: Wear eye protection. Rise a ___ and fill with NaOH solution.	Burette	12%
This meant that similar elements lined up in ___	Groups	12%
Electrons in elements occupy the ___ possible energy level.	Lowest	12%
Dmitri Mendeleev's periodic table improved early versions because it left gaps for ___ ___	Undiscovered elements	12%
pH scale is measured from 0 to ___	14	10%
___'s model showed electrons orbiting the nucleus at a specific distance, and the discovery of protons supported this.	Bohr	10%
They are much ___ reactive with water, oxygen and halogens	Less	10%
Total number of protons and neutrons in an atom	Mass number	10%
___ model showed small positively charged sphere with a nucleus and empty space.	Nuclear	10%
The ___ ___ model illustrated a positively charged "pudding" studded with electrons. JJ Thomson	Plum pudding	10%
Dyes carried up by paper at different ___ and you can calculate their Rf value to identify them	Rates	10%
Going ___ the group, reactivity increases	Up	10%
Concentration = Amount (in mol or g) / ___	Volume	10%
pH___ is neutral	7	9%
Pure metals are too soft to use for many purposes, so other metals are mixed in to make ___ that are harder.	Alloys	9%
Negative ions move to the positive one (___)	Anode	9%
As electrolysis occurs, positive ions move to the negative electrode (___)	Cathode	9%
Bonds formed when non-metal atoms bond to other non-metal atoms	Covalent	9%
Form of carbon with giant covalent structure.	Diamond	9%
A ___ pH means the substance is more acidic.	Lower	9%
All of these except ___ are solids at room temperature. All conduct electricity.	Mercury	9%
Have few electrons in outer shell, lose electrons to form positive ions in ionic compounds	Metals	9%
Are few electrons short of full outer shell. Gain electrons to form negative ions in ionic compounds or share electrons in covalent compounds.	Non metals	9%
React with ___ to form solid, white ionic oxides	Oxygen	9%
To see what kind of different substances are in a mixture, eg. ink, you use ___ ___	Paper chromatography	9%
Rinse a ___ and then use it to add 25.0cm^3 dilute HCl to a conical flask.	Pipette	9%
___ metals, compared to the alkali metals, are higher density, stronger, harder, have higher melting/boiling points	Transition	9%
React with metals to form ionic compounds, forming halide ions with a charge of ___	-1	7%
A more reactive halogen can ___ a less reactive halogen from an aqueous solution of its salt.	Displace	7%
Stronger forces between particles = ___ melting/boiling points	Higher	7%
As a solution becomes more acidic, ___ ion concentration increases	Hydrogen	7%
As it becomes more alkaline, ___ concentration increases	Hydroxide	7%
Loss of electrons.	Oxidation	7%
React with ___ to form hydroxides and hydrogen.	Water	7%
Reacts to form ions with ___ charge.	+1	6%
In reactions with gases, calculate the number of moles and then multiply by ___ to find gas volume	24	6%
About 20 years after the nucleus was accepted, ___ discovered neutrons.	Chadwick	6%
The decomposition of an ionic compound when melted or dissolved, using electricity	Electrolysis	6%
Strong acids are ___ ionised into hydrogen. Include hydrochloric, nitric, sulfuric.	Fully	6%
Form of carbon where carbon atoms form layers with weak intermolecular forces between them	Graphite	6%
The bonds are strong but the ___ ___ are not	Intermolecular forces	6%
Bonds formed when metals react with non-metals. Atoms of metal transfer outer electrons to non-metal atoms. Oppositely charged ions with full outer shells. Strong bond between ions.	Ionic	6%
When they have sufficient energy to overcome the forces between them, the substance ___	Melts	6%
Electrons in the same group have similar properties and the same number of ___ ___	Outer electrons	6%
Weak acids are ___ ionised. Include carbonic, ethanoic.	Partially	6%
Gain of electrons.	Reduction	6%
Acid + base -> ___ + water	Salt	6%
Equal numbers of moles of any gas have the same volume at the same ___ and pressure	Temperature	6%
One mole of any substance contains ___ ___ number of particles.	The same	6%
This group is the alkali metals. Low density - first three are less dense than water.	1	4%
Many also form coloured compounds, are useful ___ and form more than one type of ion	Catalysts	4%
A ___ is used to condense the gases into liquids when they have evaporated (has two tubes, one inside other, and cooling water runs through space in between.)	Condenser	4%
A molten mixture is made of aluminium oxide and ___ to lower the melting point	Cryolite	4%
Leave in a warm place until ___ have formed	Crystals	4%
A more reactive metal will ___ a less reactive metal from its compound.	Displace	4%
Particle Theory: When solid substance is ___, particles gain energy.	Heated	4%
Many metals react with oxygen from the air to form ___ ___	Metal oxides	4%
If the metal in the substance being electrolysed is ___ reactive than hydrogen, hydrogen is produced at the cathode. If not, the metal is.	More	4%
Unreactive metals are found as their ___	Ore	4%
If the electrolysed substance contains halide ions, the halogen is produced at the anode. If not, ___ is produced.	Oxygen	4%
To separate a mixture of two liquids or a solution of a solid in water	Simple distillation	4%
Forces between molecules are relatively strong compared with other covalent molecules so they are ___ at room temperature.	Solid	4%
These, and atoms, have properties different to the same material in bulk due to a high ___ ___ compared to volume	Surface area	4%
Maximum yield that can be obtained from a chemical reaction	Theoretical yield	4%
In a solution of a solid in water, the ___ is collected	Water	4%
Amount of product obtained in a chemical reaction	Yield	4%
This group is the halogens. Non-metals consisting of molecules with pairs of atoms.	7	3%
Rutherford's ___ ___ ___ experiment showed most positive particles fired at an atom went straight through, suggesting that most of an atom is empty space.	Alpha particle scattering	3%
Include ___, C60, which is spherical.	Buckminsterfullerene	3%
They do not conduct electricity, except some forms of ___	Carbon	3%
___ can replace metals less reactive than itself from their compounds.	Carbon	3%
This produces ___ ___ when reacting with the electrode	Carbon dioxide	3%
When melted/dissolved in water, the ions are released and can move and carry ___, therefore are conductors	Current	3%
Electrolysis is ___ because of the energy required to melt compounds and produce currents	Expensive	3%
___ ___ is packed with glass beads	Fractionating column	3%
Molecules of carbon atoms with spherical or otherwise hollow structures	Fullerene	3%
Some have ___ structures and are solids at room temperature with a high melting point.	Giant	3%
In a compound, strong electrostatic attraction between oppositely charged ions forms a ___ ___ structure.	Giant lattice	3%
RP Salt Preparation: Measure 50cm^3 dilute acid into a beaker, and gently ___.	Heat	3%
Different liquids leave the top of the column in order of ___ boiling point	Increasing	3%
Cylindrical fullerenes which are very ___ compared to their diameter.	Long	3%
The mixture is put into a tank. At the carbon anode, ___ is formed	Oxygen	3%
Actual yield is less than this. Some product lost while separating from reaction mixture, reactants may produce by-___, reaction may be reversible so not go to completion.	Products	3%
At the cathode, aluminium ions are ___, producing pure alumium	Reduced	3%
Using a ___, add metal oxide and stir with glass rod.	Spatula	3%
Electrostatic attraction between metal ions and electrons makes a ___ metallic bond.	Strong	3%
Outer shell of this group is full. Stable arrangement means atoms do not easily form molecules and are inert.	0	1%
Minimum energy needed for a reaction to occur when reactant particles collide	Activation energy	1%
Bases include ___ (soluble metal hydroxides), insoluble metal hydroxides, and insoluble metal oxides.	Alkali	1%
Mass of moles of desired product/mass of moles of all reactants = ___	Atom economy	1%
Two or more of these can be connected to form a ___ of higher voltage	Battery	1%
If further heated, the substance ___ when particles have sufficient energy to overcome forces between them again	Boils	1%
Energy needed to break a bond	Bond energy	1%
Contain chemicals that react together to produce electricity	Cell	1%
Heat in evaporating dish to ___ the solution. Leave in warm place to allow remaining water to evaporate.	Concentrate	1%
In a solid, ions are held firmly in a lattice so solid ionic compounds don't ___ ___	Conduct electricity	1%
At the cathode, either hydrogen will produce a colourless gas, or ___ will produce a red-brown solid.	Copper	1%
In a mixture of two liquids, the one with the lower boiling point is collected as the ___	Distillate	1%
Those more reactive than carbon require ___	Electrolysis	1%
RP: Set up two carbon electrodes in a beaker, with a soluble substance dissolved in water for the ___.	Electrolyte	1%
Chemical cells are where 2 metals are connected in contact with an ___	Electrolyte	1%
Transfer to an ___ ___ and heat until half the water has evaporated to concentrate the solution.	Evaporating dish	1%
Wait until all has reacted, then add a further sample. Repeat till there's an ___ of oxide.	Excess	1%
Energy required to break bonds is less than energy given out when making bonds	Exothermic	1%
Portable and can be rechargeable (reaction is reversed by applying an ___ ___)	External current	1%
___ into another beaker.	Filter	1%
Single layer of ^^^ one atom thick.	Graphene	1%
React with ___ to form solid, white ionic chlorides	Halogens	1%
Very ___ and does not conduct electricity. High melting point.	Hard	1%
Metals above ___ in the reactivity series will displace it from acids.	Hydrogen	1%
This leaves a ___ of metal ions	Lattice	1%
Energy of products is ___ than the energy of the reactants.	Less	1%
Acid + ___ ___ -> salt + water + carbon dioxide	Metal carbonate	1%
Metal + acid -> ___ ___ + hydrogen	Metal salt	1%
Energy of products is ___ than the energy of reactants	More	1%
___ relates to structures with a few hundred atoms - nanoparticles.	Nanoscience	1%
Add a few drops of ___ and swirl.	Phenolphthalein	1%
Some compounds with atoms that are joined up by covalent bonds form very large molecules, made of repeating units - ___	Polymers	1%
Set up a beaker in a ___ cup with a thermometer.	Polystyrene	1%
Repeat until you have 3 values that are within 0.10 cm^3 of each other - ___ results. Do this by adding the alkali in drops when close to the end point.	Precise	1%
The ___ ___ ___ of a substance in grams is known as one mole of that substance.	Relative formula mass	1%
Rf = distance moved by ___/distance moved by ___ (answer as __, __)	Substance, solvent	1%
Mixtures are two or more elements and/or compounds not chemically bonded. Chemical properties of each element are ___.	Unchanged	1%
The mean value of atomic masses of these is the relative atomic mass and is calculated proportionally to the ___ of these (above).	Abundance	0%
We need aluminium as it's low density and strong when ___	Alloyed	0%
With acid, vigorous fizzing down to ___.	Aluminium	0%
Includes thermal decomposition, and the reaction of ___ ___ with sodium hydrogen carbonate	Citric acid	0%
RP Energy Changes: Different ___ of acid give different temperature rises.	Concentrations	0%
Constant voltage and do not run down as fuel is supplied ___	Continuously	0%
React with other non-metals to form simple molecular ___ ___	Covalent compounds	0%
Turn on ___ supply.	dc	0%
Metallic bonding: In metal elements and alloys, outer electrons of atoms are ___	Delocalised	0%
___ originally thought atoms were tiny spheres that could not be made smaller	Democritus	0%
Energy required to break bonds is more than energy given out when making bonds	Endothermic	0%
From potassium to aluminium, a ___, decreasing in speed, is seen when reacting with water.	Fizzing	0%
Can be used in medicine to deliver drugs, as synthetic skin, in electronics, cosmetics, suncreams, in deoderants, and as catalysts in ___ ___ (due to large SA)	Fuel cells	0%
Metals less reactive than carbon can be extracted from their oxides by ___ with carbon	Heating	0%
Based off ___ of carbon, may also have five-carbon and seven-carbon rings.	Hexagons	0%
Fuel cells are continuously supplied with ___ which is oxidised to provide a potential difference.	Hydrogen	0%
These distort the ___ ___ ___, so layers cannot slide as easily as in a pure metal.	Layers of ions	0%
Used in medicines to contain and deliver drugs, as a ___, or as a surface for a catalyst.	Lubricant	0%
Stir with thermometer until temperature stops increasing. Record the ___ temperature.	Maximum	0%
They form a ___ ___ and hydrogen gas.	Metal hydroxide	0%
React with acids to form a ___ ___ and hydrogen.	Metal salt	0%
Used in electronics, ____, or reinforcing materials (such as the frame of a tennis racket.)	Nanotechnology	0%
Includes combustion, oxidation, and ___.	Neutralisation	0%
However, difficult to dispose of, and, when one of the reactants in a ___ ___ cell runs out, chemical reactions stop.	Non rechargeable	0%
At the anode, oxygen will produce a colourless gas, bromine an ___ ___, or chlorine a pale green gas.	Orange solution	0%
Scrape onto filter paper and ___ ___	Pat dry	0%
Mnemonic for this order (type in with no commas)	Please stop calling me a careless zebra instead try learning how copper saves gold	0%
Reactivity series order (type in with no commas)	Potassium sodium calcium magnesium aluminium carbon zinc iron tin lead hydrogen copper silver gold	0%
Add alkali slowly, swirling the flask. Take a ___ titration when the indicator changes colour	Rough	0%
It's a ___conductor so is useful in electronics.	Semi	0%
Some are ___ ___ and are gases, liquids or solids at room temperature with a low melting point.	Simple molecules	0%
It's soft and ___, conducts electricity and has a high melting point.	Slippery	0%
___ ___ have a low melting and boiling point due to weak (above)	Small molecules	0%
Limitations of the model: particles in real substances aren't often ___ and the model does not show forces between particles.	Spheres	0%
When an acid reacts with a metal, metal carbonate or alkali, the energy change of the reaction causes change in the ___ of the mixture.	Temperature	0%
High ___ ___. Good conductors.	Tensile strength	0%
Each atom bonds to 4 others to form a lattice with a ___ structure.	Tetrahedral	0%
Repeat the experiment with acid and ___ mixtures	Water	0%
Only waste product is ___. However, they're not portable	Water	0%
From ___ down, no observable reaction.	Zinc	0%
___ and iron see slow fizzing. There's no observable reaction in copper, silver or gold.	Zinc	0%
Measure 50cm^3 of dilute HCl and record the initial temperature. Add ___ powder in excess.	Zinc	0%

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