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3.2 Periodic trends

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Core » Topic 3: Periodicity » 3.2 Periodic trends

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16N.1.sl.TZ0.7:
Which equation represents the first electron affinity of chlorine?

A. Cl(g)+e^-→ Cl^-(g)
B. $\frac{1}{2}$ Cl₂(g) + e^- → Cl^-(g)
C. Cl⁺(g) + e^- → Cl(g)
D. Cl(g) → Cl⁺(g) + e^-
16N.1.hl.TZ0.7: Which property increases down group 17, the halogens? A. Electron affinity B. Boiling point C....
16N.1.sl.TZ0.8:
Which solution forms when phosphorus(V) oxide, P₄O₁₀, reacts with water?
16N.1.hl.TZ0.8: Which correctly describes the reaction between potassium and excess water? A. The reaction is...
16N.2.sl.TZ0.4d: Describe the trend in acid-base properties of the oxides of period 3, sodium to chlorine.
16N.2.sl.TZ0.4e:
In addition to magnesium oxide, magnesium forms another compound when burned in air. Suggest the formula of this compound
17M.2.sl.TZ1.2d.ii:
Explain why an aluminium-titanium alloy is harder than pure aluminium.
17M.2.hl.TZ1.2d.ii:
Suggest why the melting point of vanadium is higher than that of titanium.
17M.1.sl.TZ1.8: Which oxide, when added to water, produces the solution with the highest pH? A. Na2O B. ...
17M.1.hl.TZ1.6: What is the order of decreasing ionic radius? A. S2− > Cl− > Al3+ > Mg2+ B. ...
17M.2.sl.TZ2.1c.i:
Some oxides of period 3, such as Na₂O and P₄O₁₀, react with water. A spatula measure of each oxide was added to a separate 100 cm³ flask containing distilled water and a few drops of bromothymol blue indicator.

The indicator is listed in section 22 of the data booklet.

Deduce the colour of the resulting solution and the chemical formula of the product formed after reaction with water for each oxide.
17M.1.hl.TZ2.5: X, Y and Z represent the successive elements, Ne, Na and Mg, but not necessarily in that...
17M.1.sl.TZ2.12: Which metal has the strongest metallic bond? A. Li B. Na C. K D. Rb
20N.1.sl.TZ0.8:
Which oxide will dissolve in water to give the solution with the lowest pH?

A.   $P_{4} O_{10}$

B.   ${SiO}_{2}$

C.   ${Al}_{2} O_{3}$

D.   $MgO$
20N.1.sl.TZ0.7:
Which of the following shows a general increase across period 3 from $Na$ to $Cl$ ?

A. Ionic radius

B. Atomic radius

C. Ionization energy

D. Melting point
20N.1.hl.TZ0.6: What is the correct trend going down groups 1 and 17? A. Melting points increase B. Boiling...
20N.2.sl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
20N.2.sl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(iii):
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
20N.2.hl.TZ0.1a(ii):
State, giving a reason, whether the chlorine atom or the chloride ion has a larger radius.
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
17N.1.sl.TZ0.8: Which oxide dissolves in water to give a solution with a pH below 7? A. MgO B. Li2O C. CaO D....
17N.1.sl.TZ0.7:
Which trends are correct across period 3 (from Na to Cl)?

I. Atomic radius decreases
II. Melting point increases
III. First ionization energy increases

A. I and II only

B. I and III only

C. II and III only

D. I, II and III
17N.2.sl.TZ0.2a: Explain the general increasing trend in the first ionization energies of the period 3 elements,...
17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
17N.2.sl.TZ0.2c:
State an equation for the reaction of phosphorus (V) oxide, P₄O₁₀ (s), with water.
21M.1.sl.TZ1.8: Which trend is correct, going down group 1? A. Melting point increases B. Reactivity...
21M.1.sl.TZ2.7: Which property increases down group 1? A. atomic radius B. electronegativity C. first...
21M.2.sl.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.hl.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
21M.2.sl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
21M.2.hl.TZ2.2a(i): Explain why Si has a smaller atomic radius than Al.
18M.2.hl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.2.hl.TZ1.2f:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ1.8: Which statement is correct? A. Atomic radius decreases down group 17. B. First...
18M.2.sl.TZ1.2e:
Calcium carbide reacts with water to form ethyne and calcium hydroxide.

CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)

Estimate the pH of the resultant solution.
18M.1.sl.TZ1.7: Which describes the oxide of sodium, Na2O?
18M.2.sl.TZ1.2d.i:
Suggest two reasons why solid calcium has a greater density than solid potassium.
18M.1.sl.TZ2.7: Which increase across a period from left to right?
18M.2.sl.TZ2.3b.ii:
Outline why the ionic radius of K⁺ is smaller than that of Cl⁻.
18M.2.sl.TZ2.3b.i:
Outline why atomic radius decreases across period 3, sodium to chlorine.
21N.1.sl.TZ0.7: Which element has the highest metallic character in Group 14? A. C B. Si C. Ge D. Sn
21N.1.sl.TZ0.8: Which combination describes the acid–base nature of aluminium and phosphorus oxides?
21N.1.hl.TZ0.6: Which ion has the largest radius? A. Na+ B. Mg2+ C. P3− D. S2−
21N.2.sl.TZ0.2: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
21N.2.hl.TZ0.2a: Explain the general increase in trend in the first ionization energies of the period 3 elements,...
22M.1.sl.TZ1.7: Which gases are acidic? I. nitrogen dioxideII. carbon dioxideIII. sulfur dioxide A. I and...
22M.1.sl.TZ1.8:
Which of the following is the electron configuration of a metallic element?

A. [Ne] 3s² 3p²

B. [Ne] 3s² 3p⁴

C. [Ne] 3s² 3p⁶ 3d³ 4s²

D. [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵
18N.2.sl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.2.hl.TZ0.4a: Explain the decrease in atomic radius from Na to Cl.
18N.1.sl.TZ0.8: Which species will require the least energy for the removal of one electron? A. Na+ B. ...
18N.2.hl.TZ0.4b: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
18N.1.sl.TZ0.7: Which oxides produce an acidic solution when added to water? I. Al2O3 and SiO2 II. P4O6...
18N.2.sl.TZ0.4b.i: Explain why the radius of the sodium ion, Na+, is smaller than the radius of the oxide ion, O2−.
22M.1.sl.TZ2.7: Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of...
22M.1.hl.TZ2.5: What is the correct order for increasing first ionization energy? A. Na < Mg < Al B. Na...
22M.1.hl.TZ2.6: Which are the most reactive elements of the alkali metals and halogens? A. Lithium and...
22M.2.sl.TZ1.1a(iii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.1a(ii): Identify a metal, in the same period as magnesium, that does not form a basic oxide.
22M.2.sl.TZ1.3f(iii): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.hl.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
22M.2.hl.TZ1.5d(iv): The polarity of the carbon–halogen bond, C–X, facilitates attack by HO–. Outline, giving a...
22M.2.sl.TZ2.2a:
Explain why the first ionization energy of calcium is greater than that of potassium.
22M.2.sl.TZ2.1d: Describe two observations that indicate the reaction of lithium with water is exothermic.
19M.2.hl.TZ1.3b:
Outline why the alkali metals (group 1) have similar chemical properties.
19M.2.hl.TZ1.3e:
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.hl.TZ2.3b(iii):
Predict, giving two reasons, how the first ionization energy of ¹⁵N compares with that of ¹⁴N.
19M.2.hl.TZ2.4e(i):
Suggest why the existence of salts containing an ion with this formula could be predicted. Refer to section 6 of the data booklet.
19M.3.hl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.hl.TZ1.7: Which series represents atoms in order of decreasing atomic radius? A. N > C > Be >...
19M.2.sl.TZ1.3a(ii):
Write equations for the separate reactions of solid sodium oxide and solid phosphorus(V) oxide with excess water and differentiate between the solutions formed.

Sodium oxide, Na₂O:

Phosphorus(V) oxide, P₄O₁₀:

Differentiation:
19M.2.sl.TZ2.3c:
Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.
19M.2.sl.TZ2.4a:
Before its isolation, scientists predicted the existence of rhenium and some of its properties.

Suggest the basis of these predictions.
19M.3.sl.TZ1.1b(iv):
Sketch how the first ionization energies of elements vary with their atomic radius.
19M.1.sl.TZ2.8: How do the following properties change down Group 17 of the periodic table?
19M.1.sl.TZ1.8: What are typical characteristics of metals?
19N.2.sl.TZ0.6b:
Another airbag reactant produces nitrogen gas and sodium.

Suggest, including an equation, why the products of this reactant present a safety hazard.
19N.1.sl.TZ0.7: Which property shows a general increase from left to right across period 2, Li to F? A. Melting...

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