Chemistry paper one

what is the charge of a proton?
+1
1 of 81
true or false ? elements contain more than one type of atom
false they only contain atoms with the same atomic number
2 of 81
give the formula for carbon dioxide
CO2
3 of 81
give the formula for sodium carbonate
Na2CO3
4 of 81
balance this equation Mg+O2 = MgO
2Mg+O2= 2MgO
5 of 81
What is the difference between a compound and a mixture?
mixtures are not chemically bonded like compounds
6 of 81
what is the name of the pattern formed from carrying out paper chromatography?
chromatogram
7 of 81
Which method of serration is useful to separate an insoluble solid from a liquid?
Filtration
8 of 81
Give the name of a method to separate a soluble solid from a liquid
Evaporation
9 of 81
which method of distillation would you use to separate liquids with similar boiling points?
fractional distillation
10 of 81
who discovered that the plum pudding model was wrong?
Ernest rutherford
11 of 81
who first devised an experiment that proved the existence of the neutron?
James chadwick
12 of 81
What is the electronic structure of sodium?
2,8,1
13 of 81
why did mendeleev leave the gaps in his table of elements?
to make sure elements with similar properties stayed in the same groups
14 of 81
How are the group number and the number of electrons in the outer shell of an element related?
the group number is the amount of electrons that are on the outer shell
15 of 81
what kind of ions do metals form?
positive ions
16 of 81
Where are the non metals on the periodic table?
to the right of the periodic table
17 of 81
Give three properties which are specific to transition metals
they can have more than one ion, often coloured , make good catalysts
18 of 81
State three trends as you go down group 1
increasing reactivity , lower melting and boiling points, higher relative atomic mass
19 of 81
State the products of the reaction of sodium and water
sodium hydroxide , hydrogen
20 of 81
state the differences between group 1 and the transition metals for the following properties hardness , reactivity , melting points
group one are more reactive then the transition metals also they are less hard then the transition metals and have much lower melting points
21 of 81
How do the boiling points of halogens change as you go down the group from fluorine to astatine?
as you go down the elements have higher boiling points
22 of 81
what is the charge of the ions that halogens form when they react with metals?
1-
23 of 81
predict whether iodine is displaced by chlorine in a solution of potassium iodide
chlorine will displace it as its more reactive
24 of 81
what is the trend in boiling point as you go down group 0?
as you go down the boiling point increases due to an increase in the number of electrons
25 of 81
what type of ion do elements from each of the following groups form A) group 1 B) group 7
A)positive ions B)negative ions
26 of 81
describe how an ionic bond forms
a metal and non metal react together the metal atom loses electrons to form a positively charged ion and the non metal gains these electrons making it a negatively charged ion
27 of 81
describe the structure of a crystal of sodium chloride
it has a giant ionic lattice the Na+ and Cl- are held together in a regular lattice
28 of 81
list the main properties of ionic compounds
high melting and boiling points, dissolve easily once they melt the have ions that are free to move
29 of 81
describe how covalent bonds form
when non metal atoms bond together they share pairs of electrons
30 of 81
Explain why simple molecular compounds typically have low melting and boiling points
weak force of attraction between between the molecules
31 of 81
describe the structure of a polymer
lots of small units linked together to form a long molecule
32 of 81
give three examples of giant covalent substances
diamond, graphite , silicon dioxide
33 of 81
explain why graphite can conduct electricity
because each carbon atom has a free electron that can move
34 of 81
explain how fullerenes could be used to deliver drugs into the body
because the structure from around another atom or molecule which is then trapped inside
35 of 81
what is metallic bonding?
the strong attraction between closely packed positive metal ions and delocalised electrons
36 of 81
explain why alloys are harder than pure metals
the layers of metal atoms make it more difficult for them to slide over each other this makes them harder
37 of 81
name the three states of matter
solid , liquid , gas
38 of 81
what is the state symbol of an aqueous substance?
aq
39 of 81
what is the name of the temperature at which a liquid becomes a gas?
boiling point
40 of 81
what is nano science ?
investigating the uses and properties of nanoparticles
41 of 81
give three uses of nanoparticles
make catalysts , cosmetics, surgical masks
42 of 81
How do you calculate the relative formula mass (Mr) of a substance ?
all the relative atomic masses of all the atoms in the substance added together
43 of 81
state the value of the avogadro constant
6.02 times 10 to the power of 23
44 of 81
what is the formula that relates the number of moles of a substrate to its mass and Mr?
number of moles = mass / relative formula mass
45 of 81
what does the conservation of mass mean?
during a chemical reaction no atoms are destroyed or created this means no mass is lost or gained
46 of 81
suggest why the mass of a reaction vessel might decrease during a reaction
because one of the products is a gas
47 of 81
explain what is meant by the term limiting reactant
if one reactant is completely used up before the rest then the reaction will stop that reactant is called limiting
48 of 81
what is concentration ?
how crowded things are
49 of 81
give the equation for working out the concentration of a solution in g/dm3
mass of solute / volume of solvent
50 of 81
give the equation for calculating the atom economy of a reaction
relative formula mass of desired products , relative formula mass of all reactants times the answer by 100
51 of 81
whats the atom economy of a reaction that only produces one product?
100%
52 of 81
give the equation for calculating the percentage yield
mass of product actually made / maximum theoretical mass of product then times your answer by 100
53 of 81
give three reasons why percentage yield is always less than 100%
not all reactants react to make a product , there might be side reactions, you loses some product when you separate it from the reaction mixture
54 of 81
state whether the following pH values are acidic , alkaline or neutral A) 9 B)2 C)7 D)6
A) alkali B) acid C) neutral D) acid
55 of 81
give the general word equation for the reaction between an acid and a base
acid + base = salt+ water
56 of 81
whys shouldn't you use universal indicator as an indicator in a titration?
because you need to see a sudden colour change
57 of 81
Name two suitable indicators for a titration and state their colours when in acidic or alkaline solution
litmus - blue in alkalis red in a acids , methyl - yellow in alkalis red in acids
58 of 81
what is a strong acid?
acids that completely ionise in water and all acid particles dissociate to release H+ ions
59 of 81
is zinc more or less reactive than iron?
more reactive
60 of 81
what is the general equation for the reaction of a metal with an acid?
acid + metal = salt + hydrogen
61 of 81
will copper react with water ?
no because it not very reactive
62 of 81
what product forms in the oxidation of magnesium by oxygen?
magnesium oxide
63 of 81
in terms of electrons give the definition of oxidation
oxidation is the loss of electrons
64 of 81
during electrolysis which electrode are the positive ions attracted to ?
the anode
65 of 81
why can ionic solids not undergo electrolysis ?
because the ions are in fixed positions and won't move
66 of 81
do ions get reduced or oxidised at the anode
oxidised
67 of 81
if halide ions are present in an aqueous solution of an ionic solid will oxygen gas be released?
no molecules of chlorine bromine or iodine will be formed
68 of 81
in an exothermic reaction is heat transferred to or from the surroundings?
transfers energy to its surroundings
69 of 81
name two different types of reaction which are exothermic
burning fuels (combustion), neutralisation reactions
70 of 81
define what is meant by the term endothermic reaction
a reaction that takes in energy from the surroundings
71 of 81
write down the equation for the thermal decomposition of calcium carbonate
CaCO3 + heat = CO2 + CaO
72 of 81
what is the activation energy of a reaction ?
minimum amount of energy required for the start of reaction
73 of 81
is a bond breaking an exothermic process?
no its endothermic
74 of 81
is bond forming an exothermic process ?
yes
75 of 81
what is an electrolyte in an electrochemical cell?
a liquid that contains ions which react with the electrodes
76 of 81
give two factors that affect the voltage produced by an electrochemical cell
type of electrodes , difference in reactivity
77 of 81
what is a battery?
two or more cells together in series
78 of 81
explain why non rechargeable batteries eventually lose their charge
because the reactants get used up
79 of 81
what is a fuel cell ?
an electrical cell thats supplied with fuel and oxygen
80 of 81
name an electrolyte commonly used in hydrogen oxygen fuel cells
potassium hydroxide
81 of 81

Other cards in this set

Card 2

Front

true or false ? elements contain more than one type of atom

Back

false they only contain atoms with the same atomic number

Card 3

Front

give the formula for carbon dioxide

Back

Preview of the front of card 3

Card 4

Front

give the formula for sodium carbonate

Back

Preview of the front of card 4

Card 5

Front

balance this equation Mg+O2 = MgO

Back

Preview of the front of card 5
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