What determines the order of elements in the Periodic Table?
First ionisation energy
Number of electrons in the outer shell
Number of protons in the nucleus
Relative atomic mass
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What determines the order of elements in the Periodic Table?
First ionisation energy
Number of electrons in the outer shell
Number of protons in the nucleus
Relative atomic mass
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Which element has the highest melting point?
Silicon
Phosphorus
Sulfur
Chlorine
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Electron configurations for atoms of different elements are shown below.
Which electron configuration represents the element with the largest first ionisation energy?
1s22s2
1s22s22p4
1s22s22p6
1s22s22p63s2
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Sodium sulfide, Na2S, is a reactive yellow solid, produced when sodium and sulfur react together.
Which of the following statements is correct?
A |
The ions have the same ionic radii |
B |
The atoms have the same atomic radii |
C |
Sodium < sulfur |
D |
Sodium > sulfur |
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The trends in three physical properties of the elements of Period 3 are shown in the graphs below.
Which physical property is not illustrated?
First ionisation energy
Atomic radius
Melting point
Electrical conductivity
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What is the correct classification for the element zirconium, Zr?
s block
d block
f block
p block
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What is the correct equation for the second ionisation energy of rubidium, Rb?
Rb+ (g) → Rb2+ (g) + e-
Rb (g) → Rb+ (g) + e-
Rb2+ (g) → Rb3+ (g) + e-
Rb2+ (g) + e- → Rb+ (g)
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Why is the first ionisation energy of magnesium lower than the second ionisation energy?
Less shielding
Ionic radius increases
Nuclear charge increases
Greater attraction between positive nucleus and outer electron
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The trend in melting points of some Period 3 elements can be represented as:
S8 > P4 > Cl2
What intermolecular force explains this trend in melting point?
Permanent dipole- dipole
Covalent bonding
Hydrogen bonding
Induced dipole-dipole interactions
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In the Periodic Table, element X is in Group 3 and element Y is in Group 16 (6).
What is the likely formula of an ionic compound of X and Y?
X3Y6
X3Y2
X2Y3
X6Y3
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What determines the order of elements in the Periodic Table?
First ionisation energy
Number of electrons in the outer shell
Number of protons in the nucleus
Relative atomic mass
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Which element has the highest melting point?
Silicon
Phosphorus
Sulfur
Chlorine
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Which trend in the periodic table is correct?
Melting point decreases from lithium to carbon
Boiling point decreases from fluorine to iodine
First ionisation energy decreases from lithium to caesium
First ionisation energy increases from nitrogen to oxygen
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Which statement best explains why phosphorus has a larger first ionisation energy than sulfur?
P atoms have less repulsion between p-orbital electrons than S atoms
P atoms have a smaller nuclear charge than S atoms
P atoms lose an electron from the 3s subshell, while S atoms lose an electron from the 3p subshell
P atoms have an odd number of electrons, while S atoms have an even number
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The first five successive ionisation energies of an element Z are shown below.
1st | 2nd | 3rd | 4th | 5th |
495 | 4563 | 6914 | 9543 | 13351 |
What is the formula of a hydroxide of Z?
ZOH
Z(OH)2
Z(OH)3
Z(OH)4
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Which p-block element contains atoms with one unpaired electron?
B
C
N
O
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Which statement below shows the correct information about diamond and graphite?
Diamond and graphite both conduct electricity due to delocalised electrons in their structure
The bond angles in the two structures are not the same
Diamond is macromolecular and graphite is simple molecular
All the valence electrons are covalently bonded in both graphite and diamond
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Consecutive elements X, Y and Z, are in the third period of the periodic table. Element Y has the highest first ionisation energy and the lowest melting point of these three elements.
What could be the identities of X, Y and Z?
Silicon, phosphorus, sulfur
Sodium, magnesium, aluminium
Aluminium, silicon, phosphorus
Magnesium, aluminium, silicon
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Which of the following metals would have the highest melting point?
Na
Mg
K
Al
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Which statement best explains why nitrogen has a larger first ionisation energy than oxygen?
N atoms have less repulsion between p-orbital electrons than O atoms.
N atoms have a smaller nuclear charge than O atoms.
N atoms lose an electron from the 2s subshell, while O atoms lose an electron from the 2p subshell.
N atoms have an odd number of electrons, while O atoms have an even number.
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Successive ionisation energies of four elements in Period 3 are shown below.
Which letter could represent magnesium?
1st (kJ mol-1) | 2nd (kJ mol-1) | 3rd (kJ mol-1) | 4th (kJ mol-1) | 5th (kJ mol-1) | |
A | 1251 | 2298 | 3822 | 5159 | 6542 |
B | 738 | 1451 | 7733 | 10543 | 13630 |
C | 496 | 4563 | 6913 | 9544 | 13352 |
D | 578 | 1817 | 2745 | 11577 | 14842 |
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Which statement about trends in first ionisation energies is correct?
The first ionisation energy generally increases across a period due to increased nuclear charge and shielding.
First ionisation energy drops between magnesium and aluminium because the outer electron is in the 3p subshell which is higher in energy than the 3s orbital.
First ionisation energy drops between nitrogen and oxygen because the spin-pair repulsion of the 2p electron means that this electron is higher energy.
First ionisation energy down a group increases due to increased nuclear charge.
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The successive ionisation energies of elements X and Y are shown below.
Element X |
||||||||
IE |
1st |
2nd |
3rd |
4th |
5th |
6th |
7th |
8th |
IE (kJ mol-1) |
590 |
1145 |
4912 |
6491 |
8153 |
10496 |
12270 |
14206 |
Element Y |
||||||||
IE |
1st |
2nd |
3rd |
4th |
5th |
6th |
7th |
8th |
IE (kJ mol-1) |
1012 |
1907 |
2914 |
4964 |
6274 |
21267 |
25431 |
29872 |
X and Y form ions with the same electron configuration as argon.
What are the identities of elements X and Y respectively?
Calcium and phosphorus
Sodium and oxygen
Magnesium and nitrogen
Phosphorus and potassium
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In which row is the first ionisation energy of atom Y greater than that of atom X?
|
Element X |
Element Y |
A |
1s22s22p63s2 |
1s22s22p63s23p1 |
B |
1s22s22p63s23p3 |
1s22s22p63s23p4 |
C |
1s22s22p63s23p5 |
1s22s22p63s23p6 |
D |
1s22s22p63s23p6 |
1s22s22p63s23p64s1 |
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Which row is correct?
Property |
Increasing order |
Atomic radius |
Nitrogen, oxygen, fluorine |
First ionisation energy |
Lithium, beryllium, boron |
Electronegativity |
Nitrogen, carbon, boron |
Melting Point |
Neon, fluorine, oxygen |
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