Module 3: Periodic Table and Qualitative Analysis V2 Flashcards
Define the term first ionisation energy
The first ionisation energy is the energy needed to remove 1 mole of electrons ✓
from 1 mole of gaseous atoms ✓
to form 1 mole of gaseous 1+ ions ✓
Write an equation, with state symbols, to represent the first ionisation energy of Magnesium
Don’t forget that they are gaseous
Write an equation, with state symbols, to represent the fourth ionisation energy of sodium
Don’t forget that they are gaseous
Define what is meant by the “second ionisation energy”
The second ionisation is the energy needed to remove 1 electron from each ion ✓
in 1 mole of gaseous 1+ ions ✓
to form 1 mole of gaseous 2+ ions ✓
Explain why the first ionisation energy, is an endothermic process
Energy is required to overcome electrostatic attraction between positive nucleus and negative electron ✓
Describe and explain the trend in first ionisation energy going down the group
First ionisation energy decreases ✓
Number of shells increases, so shielding increases ✓
Atomic radius increases down the group ✓
Nuclear charge increases down the group, but is outweighed by increase in atomic radius and shielding ✓
Nuclear attraction for outer electron decreases, so electron more easily lost ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron
Describe and explain the trend in first ionisation energy going across the period.
First ionisation energy increases ✓
Nuclear charge increases ✓
Shielding is similar, outermost electron is being removed from the same shell ✓
Atomic radius decreases. ✓
Greater nuclear attraction for outer electron ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron
Explain why first ionisation energy decreases between groups 2 to 3 (Mg to Al)
Mg has outer electron in 3s sub-shell and Al has outer electron in 3p sub-shell ✓
3p sub-shell has higher energy than 3s sub-shell. ✓
There is a slight increase in shielding which outweighs the increase in nuclear charge. ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Explain why first ionisation energy decreases between groups 5 to 6 (P to S)
Shielding is identical in phosphorous and sulfur atoms and electron is being removed from 3p-subshell. ✓
In sulfur, the electron is easier to remove – lower ionisation energy. ✓
Orbital has 2 electrons – repulsion between the two electrons. ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Sketch a graph to show how ionisation energy changes across period 3.
Predict where you would expect lithium to be by adding an additional cross above Sodium.
Li would be much higher compared to the rest, as it has one less shell. Li is much greater in ionisation energy due to having less shielding and being closer to the nucleus.
Describe and explain the trend in successive ionisation energies
Increases as more electrons are removed. ✓
Electrons are removed from a more positive ion ✓
Attraction between remaining electrons and nucleus increases. Radius also decreases. ✓
more energy is needed to remove the next electron. ✓
Same number of protons, same nuclear charge attracting fewer electrons. ✓
The successive ionisation energies of element X is shown below. State and explain what group element X belongs to.
Group 5
Big jumps are caused when a new shell is broken into ✓
Electron removed from a shell closer to the nucleus ✓
Describe and explain the trend in reactivity going down the group for group 1 and 2 metals.
Increases down the group ✓
Number of shells increases, so shielding increases ✓
Atomic radius increases down the group ✓
Nuclear charge increases down the group, but is outweighed by increase in atomic radius and shielding ✓
Nuclear attraction for outer electron decreases, so less is energy is required to remove electrons✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Write a balanced equation for the reaction of calcium with water and state what observations you would observe.
Fizzing ✓
Solid dissolves ✓
Write an equation for the reaction of Calcium with oxygen.
Write an equation to show how the product above can react with water to produce calcium hydroxide.
State and explain a use of calcium hydroxide
Used in agriculture ✓
to neutralise acidic soils ✓
State and explain a use of magnesium hydroxide and calcium carbonate
Antacids ✓
Neutralises excess stomach acid ✓
State and explain a use of barium sulfate
Barium meals ✓
barium sulfate is insoluble ✓
Describe and explain the trend in atomic radius going across the period.
Decreases across a period ✓
Number of protons / nuclear charge increases ✓
Outer electrons are in the same shell and have similar shielding ✓
Stronger nuclear attraction and electrons are drawn in more ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Describe and explain the trend in atomic radius going down the group
Increases down the group ✓
Number of shells increases ✓
Describe and explain the trend in melting and boiling points going down group 7
Increases down group 8 ✓
Number of electrons and atomic radius increases ✓
Strength of induced dipole-dipole interactions between atoms increases ✓
which require more energy to overcome ✓
Could use “London forces”
Sketch a graph to show how boiling points change across period 3
Explain why the melting points increases from sodium to aluminum.
Number of delocalised electrons increases ✓
Charge on positive ion increases ✓
Metallic bonding, electrostatic attraction between the positive metal ion and delocalised electrons, gets stronger ✓
Explain why the conductivity increases in period 3, from Na to Al.
Number of delocalised electrons increases ✓
Explain why boron has a higher melting and boiling point compared to nitrogen
Boron has a giant covalent lattice with lots of strong covalent bonds ✓
N2 has simple covalent lattice and induced dipole-dipole interactions between molecules ✓
Covalent bonds require more energy to overcome ✓
Explain why phosphorous has a higher melting and boiling point compared to argon
Phosphorous has a simple covalent lattice and induced dipole-dipole interactions between molecules ✓
Argon has induced dipole-dipole interactions between atoms ✓
Phosphorous more atoms and electrons ✓
hence stronger induced dipole-dipole interactions between molecules which requires more energy to overcome ✓
Explain why a nitrogen atom is larger than an oxygen atom.
Nitrogen has less protons than oxygen and has a weaker nuclear charge ✓
Both have similar shielding ✓
Weaker nuclear attraction in nitrogen and shell is drawn in less by nuclear charge ✓
Explain why phosphorous has a lower boiling point than sulfur.
Sulfer has more atoms and more electrons ✓
Stronger induced dipole-dipole interactions between molecules ✓
… which require more energy to overcome ✓
Describe and explain the trend in boiling and melting points going down group 7.
Increases down group 7 ✓
Number of electrons and atomic radius increases ✓
Strength of induced dipole-dipole interactions between molecules increases ✓
which require more energy to overcome ✓
Describe and explain the trend in volatility going down group 7.
Decreases down group 7 ✓
Number of electrons and atomic radius increases ✓
Strength of induced dipole-dipole interactions between molecules increases ✓
Which require more energy to overcome ✓
Describe and explain the trend in reactivity going down group 7.
Halogens are less reactive and less oxidising down the group ✓
Atomic radius increases ✓
Outer electrons are further away from the nucleus and are more shielded from the nucleus ✓
Less nuclear attraction, so more difficult for larger atoms to attract electrons needed to form an ion ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Explain how you could investigate the reactivity of the halogens.
Oxidising strengths seen in displacement reactions with halide ions ✓
More reactive halogens will oxidise and displace halide ions of less reactive halogens ✓
Write an ionic equation for the reaction between chlorine and potassium bromide.
If needed, include observations in your answer, in aqueous conditions and when using an organic solvent i.e. cyclohexane.
Write an ionic equation for the reaction between chlorine and magnesium iodide.
If needed, include observations in your answer, in aqueous conditions and when using an organic solvent i.e. cyclohexane.
Write an ionic equation for the reaction between bromine and lithium iodide.
If needed, include observations in your answer, in aqueous conditions and when using an organic solvent i.e. cyclohexane.
State the colour change from the following mixtures, if any and write an ionic equation for the reaction between the following:
a) Magnesium iodide added to a test tube containing chlorine.
b) Sodium iodide added to a test tube containing bromine.
c) Potassium bromide added to a test tube containing chlorine.
d) magnesium chlorine added to a test tube containing bromine.
State symbols needed for an ionic equation - always
For the following reactions, write half equations for both the oxidation and reduction process.
You are provided with 3 solids, which could contain either sodium chloride, magnesium bromide or lithium iodide.
Plan an investigation to deduce the identity of the solids.
Dissolve unknown halide in water with nitric acid ✓
Add aqueous solution of silver nitrate ✓
Silver ions from the silver nitrate reacts with the halide ions forming a silver halide precipitate ✓
Silver halide precipitates are coloured with the colour intensity increasing from Cl- to I-. Colour tells you which halide ion is present. ✓
If it is too difficult to decide on a colour, first add dilute ammonia solution, then check with concentrated ammonia solution ✓
as the halide ions have different solubilities in ammonia. ✓
Silver nitrate solution is added to a beaker of solution containing NaCl, NaBr and NaI. Concentrated ammonia solution is then added, and the resulting mixture is filtered.
What compound(s) are contained within the residue on the filter paper?
AgI ✓
Silver nitrate solution is added to a beaker of solution containing NaCl, NaBr and NaI. Dilute ammonia solution is then added, and the resulting mixture is filtered.
What compound(s) are contained within the residue on the filter paper?
AgBr and AgI ✓
Explain how you can test for chloride ions.
Write an ionic equation to support your answer.
State the name of the product formed and observations seen.
Add nitric acid followed by silver nitrate solution to sample ✓
White precipitate formed ✓
Silver chloride ✓
## Footnote
State symbols needed for an ionic equation - always
Explain how you can test for bromide ions.
Write an ionic equation to support your answer.
State the name of the product formed and observations seen.
Add nitric acid followed by silver nitrate solution to sample ✓
Cream precipitate formed ✓
Silver bromide ✓
## Footnote
State symbols needed for an ionic equation - always
Explain how you can test for iodide ions.
Write an ionic equation to support your answer.
State the name of the product formed and observations seen.
Add nitric acid followed by silver nitrate solution to sample ✓
Yellow precipitate formed ✓
Silver iodide ✓
## Footnote
State symbols needed for an ionic equation - always
Define what is meant by a “precipitation reaction”
where aqueous ions react together to form a solid precipitate ✓
A student tests conducts a test for halide ions, but the precipitate appears to be cream-yellow.
State what they could do next to confirm the presence of bromide or iodide ions.
Add concentrated ammonia solution ✓
Precipitate dissolves if bromide ions present ✓
No visible change if iodide ions present ✓
A student tests conducts a test for halide ions, but the precipitate appears to be white-cream.
State what they could do next to confirm the presence of chloride or bromide ions.
Add dilute ammonia solution ✓
Precipitate dissolves if chloride ions present ✓
No visible change if bromide ions present ✓
State why dilute nitric acid is added to a solution before the silver nitrate test.
Include an ionic equation in your answer.
To remove any carbonates ✓
Which would produce a white solid, silver carbonate ✓
Which gives a false positive ✓
State why nitric acid is added instead of hydrochloric acid before the addition silver nitrate test when testing for halide ions.
Include an ionic equation in your answer.
Silver ions react with chloride ions ✓
Which would produce a white solid, silver chloride ✓
Which gives a false positive ✓
State why nitric acid is added instead of sulfuric acid before the addition silver nitrate test when testing for halide ions.
Include an ionic equation in your answer.
Silver ions react with sulfate ions ✓v
Which would produce a white solid, silver sulfate ✓
False positive ✓
Define what is meant by a “disproportionation reaction”
The simultaneous oxidation and reduction of the same element ✓
State the condition required for halogens to undergo disproportionation reaction
cold ✓ dilute NaOH or KOH ✓
Write an equation for the formation of bleach and give the conditions required for the reaction.
cold ✓ dilute aqueous NaOH ✓
Give two uses of bleach
Water treatment ✓
bleaching paper and textiles ✓
Using oxidation states, explain how the following reaction is defined as being a disproportionation reaction
The simultaneous oxidation and reduction of the same element ✓
O in H2O2 is -1… O in H2O is -2… and O in O2 is 0 ✓
O is oxidised from -1 to 0 oxidation state AND ✓
O is reduced from -1 to -2 oxidation state ✓
State two advantages and two disadvantages to treating water with chlorine.
Advantages:
kill bacteria ✓
Prevents growth of algae ✓
Disadvantages:
Chlorine is toxic ✓
Chlorine can react with organic matter to form carcinogenic chlorinated hydrocarbons ✓
State two alternatives to chlorine
Ozone ✓
UV light ✓
A student is provided with a set of solutions including sodium chloride, sodium carbonate and sodium sulfate.
To identify the ions, he conducts qualitiative analysis.
In which order should he conduct these tests in? Explain why
Carbonates → Sulfates → Halides ✓
To avoid false positives ✓
A student is provided with a set of solutions including sodium chloride, sodium carbonate and sodium sulfate.
How would he identify the presence of carbonate ions? include an ionic equation and observations in your answer.
Add dilute nitric acid ✓
Observation: Fizzing ✓
A student is provided with a set of solutions including sodium chloride, sodium carbonate, ammonium nitrate and sodium sulfate.
How would he identify the presence of sulfate ions? include an ionic equation and observations in your answer.
Add barium nitrate solution ✓
Observation: White precipitate ✓
A student is provided with a set of solutions including sodium chloride, sodium carbonate, ammonium nitrate and sodium sulfate
How would he identify the presence of ammonium ions? include an ionic equation and observations in your answer.
Heat with sodium hydroxide solution ✓
Litmus paper turns blue due to ammonia gas being produced ✓
Which element has the highest melting point?
A silicon
B phosphorus
C sulfur
D chlorine
A silicon ✓
Silicon - Giant covalent lattice
Phosphorous - Simple molecular (4 atoms)
Sulfur - Simple molecular (8 atoms)
Chlorine - Simple molecular (2 atoms)
What is the best explanation for the trend in boiling points down the halogens group?
A The covalent bonds become stronger.
B The hydrogen bonds become stronger.
C The permanent dipole–dipole interactions become stronger.
D The induced dipole–dipole interactions (London forces) increase.
D The induced dipole–dipole interactions (London forces) increase. ✓
Which silver compound is insoluble in concentrated NH3(aq)?
A AgNO3
B AgCl
C AgBr
D AgI
D AgI ✓
Which statement best explains why nitrogen has a larger first ionisation energy than oxygen?
A N atoms have less repulsion between p-orbital electrons than O atoms.
B N atoms have a smaller nuclear charge than O atoms.
C N atoms lose an electron from the 2s subshell, while O atoms lose an electron from the 2p subshell.
D N atoms have an odd number of electrons, while O atoms have an even number.
A N atoms have less repulsion between p-orbital electrons than O atoms. ✓
Which statement about ammonium carbonate is not correct?
A It reacts with Ba(NO3)2(aq) to form a white precipitate.
B It effervesces with dilute nitric acid.
C It release an alkaline gas with warm NaOH(aq).
D It has the formula NH4CO3.
D It has the formula NH4CO3. ✓
What determines the order of elements in the Periodic Table?
number of protons in the nucleus ✓
The first five successive ionisation energies of an element Y are shown below.
What is the formula of a chloride of Y?
YCl ✓
Which element has induced dipole–dipole interactions (London forces) in its solid lattice?
A boron
B magnesium
C silicon
D sulfur
D sulfur ✓
Which statement about the reactions of halogens with halide ions is correct?
A I2(aq) can oxidise Br–(aq).
B Cl 2(aq) can reduce Br–(aq).
C Br–(aq) can reduce Cl 2(aq).
D Cl –(aq) can oxidise I2(aq).
C Br–(aq) can reduce Cl2(aq) ✓
Reduce in this case, is “give electrons to”. Bromine is less reactive than chlorine. Chlorine can oxidise Br-.
Which set of elements in the solid state contain a simple molecular lattice, a giant covalent lattice and a giant metallic lattice?
A S, Si, Al
B P, Si, C
C S, P, Si
D Mg, P, S
A S, Si, Al ✓
Which statement is not correct for Group 2 hydroxides?
A Mg(OH)2 can be used to treat indigestion.
B Ca(OH)2 is used in agriculture to neutralise alkaline soils.
C The anion in Sr(OH)2 contains 10 electrons.
D Ba(OH)2 is a product from the reaction of barium and water.
B Ca(OH)2 is used in agriculture to neutralise alkaline soils. ✓
used to neutralise acidic soils
Some Group 2 compounds can be used to neutralise acid soils and to treat acid indigestion.
Which Group 2 compound would not be suitable for either use?
A BaSO4
B CaCO2
C Ca(OH)2
D Mg(OH)2
A BaSO4 ✓
Which sequence has elements in order of increasing first ionisation energy?
A Na < Mg < Al
B Mg < Al < Si
C Al < Si < P
D Si < P < S
C Al < Si < P ✓
Think NANCARS using your periodic table
Which row shows elements in order of increasing first ionisation energy?
A Ca < Si < P < N
B N < P < Si < Ca
C Ca < N < P < Si
D C < Si < P < Ca
A Ca < Si < P < N ✓
Which statement(s) explain(s) the trend in boiling points down the halogens group?
1: The induced dipole–dipole interactions (London forces) become stronger.
2: The covalent bonds become stronger.
3: The permanent dipole–dipole interactions become stronger.
1: The induced dipole–dipole interactions (London forces) become stronger. ✓
An aqueous solution contains a mixture of chloride, bromide and iodide ions.
AgNO3(aq) is added to this mixture, followed by an excess of dilute NH3(aq).
The resulting mixture is then filtered.
Which compound(s) is/are present in the residue on the filter paper?
AgBr and AgI ✓
Which substance has a giant covalent lattice structure in its solid state?
A potassium
B silicon
C sodium chloride
D water
B silicon ✓
The first four ionisation energies of a Period 3 element X are shown in the table.
Element X is reacted with chlorine.
What is the formula of the chloride formed?
XCl2
Which block in the periodic table does nickel belong to
d-block ✓
Explain why Na has a lower first ionisation energy than to Li
Na has more shells increases, so more shielding ORA ✓
Na has a larger atomic radius ✓
Na has a larger nuclear charge but is outweighed by increase in atomic radius and shielding ✓
Nuclear attraction for Na outer electron is less, so electron more easily lost ✓
A comparative NAN-CARS Question. You have to be specific in terms of “which element”
Explain why Cl is more reactive than Br
Halogens are less reactive and less oxidising down the group ✓
Br has a greater atomic radius ✓
Outer electrons are further away from the nucleus and are more shielded from the nucleus in Br ✓
Br has less nuclear attraction, so more difficult for larger atoms to attract electrons needed to form an ion ✓
A comparative NAN-CARS Question. You have to be specific in terms of “which element”
Which halogen most readily forms 1– ions
fluorine ✓
Which statement is not correct for Group 2 metals?
A. An unpaired electron is present in an s-orbital.
B. Chemical reactivity increases with increasing atomic number.
C. The first ionisation energy decreases with increasing atomic number.
D. Atomic radius increases with increasing atomic number.
A. An unpaired electron is present in an s-orbital. ✓
In actual fact, a pair of electrons are present in the s-orbital
HBr(aq), forms two ions in solution.
State the observations with the following reacting with HBr.
A. sodium carbonate solution.
B. silver nitrate solution.
A. Fizzing ✓
B. Cream precipitate ✓
Three qualitative tests are carried out on a solution of an unknown compound.
Test 1: On heating with NaOH(aq), a pungent smelling gas evolves which turns red litmus paper blue.
Test 2: On addition of AgNO3(aq), a white precipitate forms which is soluble in dilute NH3(aq).
Test 3: On addition of Na2CO3(aq), there is no visible reaction.
State the name of the uknown compound.
Ammonium chloride. ✓
This question is about halogens.
Chlorine is used to kill bacteria in drinking water.
State twos risks in using chlorine in drinking water.
Toxic. ✓
Forms chlorinated hydrocarbon compounds which are toxic and carcinogenic ✓
Nickel and gallium are in period 4 of the periodic table.
Which block in the periodic table does nickel belong to?
d-block. ✓
Suggest the type of lattice structure in solid silicon dioxide and in solid carbon dioxide and explain the difference in melting points in terms of the types of force within each lattice structure.
Carbon dioxide: simple covalent lattice. ✓
Silicon dioxide: Giant covalent lattice. ✓
Silicon dioxide has lots of strong covalent bonds, which is the shared pair of electrons, between atoms. ✓
Carbon dioxide has weak induced dipole-dipole interactions between molecules. ✓
Covalent bonding is stronger and requires more energy to overcome. ✓
Compound A has the following percentage composition by mass: Ca, 81.10%; N, 18.90%.
A student reacts compound A with water to form alkaline gas B and alkali C.
Identify A, B and C and write the equation for the reaction of compound A with water.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element that forms a 1− ion with the same electron configuration as helium.
Hydrogen/H ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element with the highest first ionisation energy.
Helium/He ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element in Period 3 which has the successive ionisation energies shown below.
Magnesium/Mg ✓
Large increase from 2nd and 3rd showing 3rd electron is taken from a shell closer to the nucleus.
Therefore 2 electrons in its outer shell, so must be in group 2.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which forms a compound with fluorine that has octahedral molecules.
Sulfur/S ✓
Remember, S and Se can expand the octet and have 12 electrons in their outer shell.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
An element which reacts with water to form an acidic solution.
Chlorine/Cl. ✓
fluorine/F. ✓
Either two, but you probably put chlorine.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element X, which forms a compound with hydrogen, XH3, with a molar mass of 34.0 g mol−1.
Phosphorus/P ✓
34-3=31. P has a molar mass of 31.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
An element which forms a compound with hydrogen in which the element has an oxidation number of −4.
Carbon/C ✓
More specifically in methane
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
A molecule, which has a density of 1.33 × 10−3 g cm−3 at room temperature and pressure.
Oxygen/O ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which forms trigonal planar molecules with 3 chlorine atoms.
Boron/B ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element with the lowest first ionisation energy.
Sodium/ K ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element that exists as a simple molecular lattice structure and is also a solid at room temperature and pressure.
Sulfer/ S ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element that exists as a simple molecular lattice structure and is also a liquid at room temperature and pressure.
Bromine/ Br ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element with an average atomic mass of 6.63 x 10^-23
Argon/ Ar ✓
The average atomic mass is the mass of 1 atom, in g.
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which forms molecules with 8 atoms arranged in a ring.
Sulfur/ S ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which forms molecules with 4 atoms arranged in a ring.
Phosphorous/ P ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element in the p block which has the smallest atomic radius
Neon/ Ne ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which has the smallest fourth ionisation energy.
Silicon/ Si ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which forms the strongest metallic bonds.
Aluminium/ Al ✓
This question refers to the elements in the first three periods (H → Ar) of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.
The element which contains 3 unpaired electrons in period 2.
Nitrogen/ N ✓
Add crosses to the graph below to show the first 11 ionisation energies of Magnesium. You do not have to join the crosses.
Make sure there is a big jump between 2-3 and 10-11 as remove electrons from a shell closer to the nucleus.
Describe what is meant by the term “periodicity”
Repeating pattern in chemical and physical properties. ✓
Describe how elements are arranged in the periodic table.
Atoms are arranged in increasing atomic number. ✓
Write the equation, including state symbols for the reaction between
a) Barium and oxygen. Include a name for this reaction.
b) Barium oxide and water.
c) Barium hydroxide and hydrochloric acid. Include a name for this reaction.
d) Barium and hydrochloric acid. Include a name for this reaction.
e) Barium and water. Include a name for this reaction.
Complete the following sketch, to show the ionisation energies across period 3.
