NEW
Font size
Worksheets3.1.1 Atomic structure
Total questions: 40
Worksheet time: 20mins
In the early twentieth century the apparatus shown in the diagram was used to investigate atomic structure. When He2+ particles were fired at a thin sheet of gold, most of the particles were detected at point P. What conclusion can be drawn from the detection of He2+ particles at point P?
Gold atoms contain electrons.
Gold atoms contain protons.
Gold atoms contain neutrons.
Gold atoms are mainly empty space.
When He2+ particles were fired at a thin sheet of gold, about 1 in 8000 of the particles were detected at point Q. What conclusion can be drawn from the detection of He2+ particles at point Q?
Gold atoms have a small, positive nucleus.
Gold atoms have electrons in orbitals.
Gold consists of ions in a sea of delocalised electrons.
Gold atoms have more protons than He2+ particles.
Which of these correctly shows the numbers of sub-atomic particles in a 41K+ ion?
Number of electrons: 19, Number of protons: 19, Number of neutrons: 20
Number of electrons: 18, Number of protons: 20, Number of neutrons: 21
Number of electrons: 18, Number of protons: 19, Number of neutrons: 22
Number of electrons: 19, Number of protons: 18, Number of neutrons: 23
Which of these correctly shows the numbers of sub-atomic particles in a 21Na+ ion?
Number of electrons: 11, Number of protons: 11, Number of neutrons: 10
Number of electrons: 10, Number of protons: 12, Number of neutrons: 9
Number of electrons: 10, Number of protons: 11, Number of neutrons: 10
Number of electrons: 11, Number of protons: 10, Number of neutrons: 11
Which of these correctly shows the numbers of sub-atomic particles in a 42Ca2+ ion?
Number of electrons: 20, Number of protons: 20, Number of neutrons: 22
Number of electrons: 18, Number of protons: 21, Number of neutrons: 21
Number of electrons: 18, Number of protons: 20, Number of neutrons: 22
Number of electrons: 20, Number of protons: 19, Number of neutrons: 23
Which species has the same number of electrons as the radical •CH3?
CH2
CH3+
CH3−
CH4+
What are the numbers of neutrons and electrons in the 57Fe2+ ion?
Neutrons: 31, Electrons: 24
Neutrons: 57, Electrons: 24
Neutrons: 31, Electrons: 26
Neutrons: 57, Electrons: 28
Which of these atoms has the largest atomic radius?
Ar
Cl
Mg
Na
Which of these atoms has the smallest atomic radius?
Ar
Cl
Mg
Na
Which of these atoms has the smallest atomic radius?
F
O
B
Be
Which of these atoms has the largest atomic radius?
K
Ca
Br
Kr
Which of these atoms has the largest atomic radius?
He
Ne
Ar
Kr
Which of these atoms has the smallest atomic radius?
He
Ne
Ar
Kr
An atom in which the number of protons is greater than the number of neutrons is:
234U
6Li
3He
2H
A student has a 10 cm3 sample of 1.00 × 10–2 mol dm–3 methanoic acid solution. The student is asked to dilute the methanoic acid solution to a concentration of 2.00 × 10–4 mol dm–3 by adding distilled water.
Which volume of water should be added?
200 cm3
490 cm3
500 cm3
510 cm3
Which statement about time of flight mass spectrometry is correct?
The current in the detector is proportional to the ion abundance
Sample particles gain electrons to form positive ions
Particles are detected in the order of their kinetic energies
Ions are accelerated by a magnetic field
Chlorine exists as two isotopes 35Cl and 37Cl in the ratio 3:1
Which statement about peaks in the mass spectrum of Cl2 is correct?
Peaks at m/z = 70 and 74 in the ratio 3:1
Peaks at m/z = 70, 72 and 74 in the ratio 9:6:1
Peaks at m/z = 70, 72 and 74 in the ratio 9:3:1
Peaks at m/z = 70 and 72 in the ratio 3:1
Bromine exists as two isotopes 79Br and 81Br, which are found in almost equal abundance.
Which of the statements is correct?
The first ionisation energy of 79Br is less than the first ionisation energy of 81Br
The atomic radius of 79Br is less than the atomic radius of 81Br
The mass spectrum of C3H7Br has two molecular ion peaks at 122 and 124
79Br is more reactive than 81Br
Which of these atoms has the smallest number of neutrons?
3H
4He
5He
4Li
Ions of two isotopes of iron are
53Fe2+ 56Fe2+
Which statement is correct?
The ions of both the isotopes have the electronic configuration 1s22s22p63s23p64s23d6
The ions of both the isotopes contains 26 neutrons
53Fe2+ has fewer protons than 56Fe2+
After acceleration to the same kinetic energy 56Fe2+ will move more slowly than 53Fe2+
The successive ionisation energies for element X are shown in the graph. Which element is X?
Nitrogen
Phosphorus
Aluminium
Boron
Chlorine has two isotopes, 35Cl and 37Cl. The number of molecular ion peaks in the mass spectrum of a sample of Cl2 is
2
3
4
5
Assuming that chlorine exists as two isotopes, and that hydrogen and carbon exist as one isotope each, how many molecular ion peaks will be shown in the mass spectrum of C4H6Cl4?
2
3
4
5
Which of these has the highest first ionisation energy?
Na
Al
Si
Cl
Element Q forms a sulfate with formula QSO4
Which of these could represent the electronic configuration of an atom of Q?
[Ne]3s1
[Ne]3s2
[Ne]3s23p1
[Ne]3s13p2
Bromine exists as two isotopes 79Br and 81Br, which are found in almost equal abundance.
Which of the statements is correct?
The first ionisation energy of 79Br is less than the first ionisation energy of 81Br
The atomic radius of 79Br is less than the atomic radius of 81Br
The mass spectrum of C3H7Br has two molecular ion peaks at 122 and 124
79Br is more reactive than 81Br
What is the electron configuration of Cu2+?
[Ar]3d94s2
[Ar]3d104s1
[Ar]3d9
[Ar]3d10
Which change requires the largest amount of energy?
He+(g) --> He2+(g) + e–
Li(g) --> Li+(g) + e–
Mg+(g) --> Mg2+(g) + e–
N(g) --> N+(g) + e–
Ions of two isotopes of iron are
53Fe2+ 56Fe2+
Which statement is correct?
The ions of both the isotopes have the electronic configuration 1s22s22p63s23p64s23d6
The ions of both the isotopes contains 26 neutrons
53Fe2+ has fewer protons than 56Fe2+
After acceleration to the same kinetic energy 56Fe2+ will move more slowly than 53Fe2+
Photochromic glass contains silver ions and copper ions. A simplified version of a redox equilibrium is shown below. In bright sunlight the high energy u.v. light causes silver atoms to form and the glass darkens. When the intensity of the light is reduced the reaction is reversed and the glass lightens.
Cu+(s) + Ag+(s) ⇌ Cu2+(s) + Ag(s)
clear glass dark glass
Which one of the following is a correct electron arrangement?
Cu+ is [Ar]3d94s1
Cu is [Ar]3d104s2
Cu2+ is [Ar]3d84s1
Cu+ is [Ar]3d10
Which one of the following statements is not correct?
The first ionisation energy of iron is greater than its second ionisation energy.
The magnitude of the lattice enthalpy of magnesium oxide is greater than that of barium oxide.
The oxidation state of iron in [Fe(CN)6]3− is greater than the oxidation state of copper in [CuCl2]−
The boiling point of C3H8 is lower than that of CH3CH2OH
Which one of the following is the electronic configuration of the strongest reducing agent?
1s2 2s2 2p5
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6 4s2
Which one of the following atoms has only two unpaired electrons in its ground (lowest energy) state?
helium
beryllium
nitrogen
oxygen
Which one of the following does not have a pair of s electrons in its highest filled electron energy sub-level?
H−
Mg
P3+
Ar
Which one of the following explains why boron has a lower first ionisation energy than beryllium?
A boron atom is smaller than a beryllium atom.
In beryllium all the electrons are paired in full sub-shells.
A beryllium atom has fewer protons than a boron atom.
In boron the 2p electron occupies a higher energy level than a 2s electron.
Which one of the following ionisations requires less energy than the first ionisation energy of oxygen?
S(g) → S+(g) + e−
O+(g) → O2+(g) + e−
N(g) → N+(g) + e−
F(g) → F+(g) + e−
Which atom has an incomplete sub-shell?
Be
Ca
Ge
Zn
In which one of the following pairs is the first ionisation energy of element Y greater than that of element X?
X: 1s1 Y: ls2
X: 1s2 2s2 Y: ls22s2 2p1
X: 1s2 2s22p3 Y: ls22s22p4
X: 1s2 2s22p6 Y: ls22s22p6 3s1
Which one of the following lists the first ionisation energies (in kJ mol−1) of the elements Mg, Al, Si, P and S in this order?
577 786 1060 1000 1260
736 577 786 1060 1000
786 1060 1000 1260 1520
1060 1000 1260 1520 418
Which one of the following is the electronic configuration of an element with a maximum oxidation state of +5?
1s2 2s2 2p5
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p6 3s2 3p3
1s2 2s2 2p6 3s2 3p6 3d7 4s2
