11 mark
Which element has the most exothermic electron affinity?
Mg
Br
Na
K
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Periodic Trends (College Board AP® Chemistry)
Exam Questions
9 mins9 questions21 mark
Which element has the smallest atomic radius?
Na
S
Mg
Cl
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31 mark
Various trends can be observed down groups and across periods in the Periodic Table. Which statement about these trends is true?
Ionization energy increases going down a group.
Atomic radius generally decreases across a period.
Electronegativity decreases across a period.
Electron affinity generally increases down a group.
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41 mark
Electrons removed | 1st | 2nd | 3rd | 4th | 5th |
Ionization energy / kJ mol-1 | 736 | 1450 | 7740 | 10500 | 13600 |
Successive ionization energies for an element, X, are shown in the table above.
What is the most likely formula for the ion of X?
X+
X2+
X3+
X4+
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51 mark
C (g) + e- → C- (g) EA = -121 kJ/mol
N (g) + e- → N- (g) EA = > 0 kJ/mol
The equations for the electron affinities of carbon and nitrogen are shown above.
Why is the electron affinity for C more favourable (more negative) than the electron affinity for N?
The electron added to carbon experiences less repulsion that the electron added to nitrogen
The electron added to carbon experiences a lesser effective nuclear charge than the electron added to nitrogen
The electron added to carbon goes into a lower electron shell than the electron added to carbon goes into
The electron added to carbon goes into a lower orbital than the electron added to carbon goes into
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61 mark
Which of the following identifies the most probable value for the fourth ionization energy of boron and provides the best justification?
4860 kJ/mol because the electron removed during the fourth ionization is a core electron.
4860 kJ/mol because the electron removed during the fourth ionization is a valence electron.
25025 kJ/mol because the electron removed during the fourth ionization is a core electron.
25025 kJ/mol because the electron removed during the fourth ionization is a valence electron.
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11 mark
Which of the following electron configurations represents the element with the highest electronegativity?
1s22s22p3
1s22s22p4
1s22s22p63s2
1s22s22p63s23p1
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21 mark
Consider the following ions:
S2−,Cl-, K+, Ca2+
Which of the following arranges the ions in order of increasing ionic radius?
Ca2+ < K+ < Cl-, < S2−
S2− < Cl-, < K+ < Ca2+
K+ < Ca2+ < Cl- < S2−
Cl- < S2− < Ca2+ < K+
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31 mark
Element X | Element Y | |
|---|---|---|
First | 1313 | 1086 |
Second | 3373 | 2353 |
Third | 6050 | 4620 |
Fourth | 8400 | 6223 |
Fifth | 22800 | 37831 |
Sixth | 32600 | 47277 |
The first six ionization energies for elements X and Y are shown in the table above. The units are in kJ/mol.
Based on the data in the table, which of the following correctly identifies elements X and Y, respectively?
Be and Mg
Mg and Be
C and Si
Si and C
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