MYP 10 Chemistry 2013-14
Atomic Structure Worksheet
(SL/HL)
Name: _________________________________ ( )
Class: _________ Date: _____________
_________________________________________________________________________________
2.1 The atom
2.1.1 State the position of protons, neutrons and electrons in the atom.
2.1.2 State the relative masses and relative charges of protons, neutrons and electrons.
2.1.3 Define the terms, mass number (A), atomic number (Z) and isotopes of an element.
2.1.4 Deduce the symbol for an isotope given its mass number and atomic number.
2.1.5 Calculate the number of protons, neutrons and electrons in atoms and ions from the mass number,atomic number and charge.
2.1.6 Compare the properties of the isotopes of an element.
2.1.7 Discuss the uses of radioisotopes.
2.2 The mass spectrometer
2.2.1 Describe and explain the operation of a mass spectrometer.
2.2.2 Describe how the mass spectrometer may be used to determine relative atomic mass using the 12C scale.
2.2.3 Calculate non-integer relative atomic masses and abundance of isotopes from given data.
2.3 Electron arrangement
2.3.1 Describe the electromagnetic spectrum.
2.3.2.Distinguish between a continuous spectrum and a line spectrum.
2.3.3 Explain how the lines in the emission spectrum of hydrogen are related to electron energy levels.
2.3.4 Deduce the electron arrangement for atoms and ions up to Z= 20.
12.1 Electron configuration (HL)
12.1.1 Explain how evidence from first ionization energies across periods accounts for the existence of main energy levels and sublevels in atoms.
12.1.2 Explain how successive ionization energy data is related to the electron configuration of an atom.
12.1.3 State the relative energies of s,p,d and f orbitals in a single energy level.
12.1.4 State the maximum number of orbitals in a given energy level.
12.1.5 Draw the shape of an a orbital and the shapes of p x, py and pz. orbitals.
12.1.6 Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and
ions up to Z=54.
1. Carbon dioxide gas is
A.
B.
C.
D.
a mixture of carbon and oxygen atoms.
made up a diatomic molecules.
a diatomic gas made up of two molecules of oxygen.
a triatomic gas with each molecule made up of 1 atom of carbon and 2 atoms of oxygen.
2. An element X forms a negative ion with the electronic configuration of (2.8.8).
What is the proton number(atomic number) of X?
A. 10
B. 16
C. 18
D. 20
3. An element X has two isotopes, which may be represented as
How does
A.
B.
C.
D.
238
X differ from
235
X?
It has 3 more protons and 3 more electrons.
It has 3 more protons, but same number of electrons.
It has 3 more neutrons and 3 more electrons.
It has 3 more neutrons, but same number of electrons.
238
X
and
235
X.
4. Which of the following could be an ion of an isotope of the following atom, X?
A.
7
3
X
B.
7
3
X
C.
10
3
X
D.
10
3
X
5. Give the number of protons, neutrons and electrons in the following atoms or ions:
protons
neutrons
electrons
50
23
V
102
44
Ru 
Ca 2
40
20
Z
91
40
31
15
P 3
127 
53
I
6. The element bromine exists as the isotopes 79Br and 81Br, and has a relative atomic mass of 79.90.
(a) Complete the following table to show the numbers of sub-atomic particles in the species shown.
An atom of 79Br
An atom of 81Br
Protons
Neutrons
Electrons
(b) State and explain which of the two isotopes
79
Br and 81Br is more common in the element bromine.
[SL paper 2, Nov 05]
7. Indium has two naturally occurring isotopes: indium-113 and indium-115.
The relative atomic mass of indium is 114.82. Calculate the natural abundance of each isotope.
8(a) In a mass spectrometer, particles are deflected according to their ________________ ratio.
_____________ ions and particles are deflected more. The __________ the ion is charged, the more it
gets deflected.
(b) Arrange the following ions in terms of how much they will be deflected in a mass spectrometer
(the one that will be deflected most first):
84
23
Kr 2
81
35
Br 
120
50
Sn 2
23
11
Na 
9. A sample of iridium is analysed in a mass spectrometer. The first and last processes in mass
spectrometry are vaporization and detection.
(a)(i) State the names of the second and third processes in the order in which they occur in a mass
spectrometer.
(ii) Outline what occurs during the second process.
(iii) State and explain which one of the following ions undergo the greatest deflection (under the same
conditions in a mass spectrometer):
191 +
Ir or 193Ir+
(b) The sample of iridium is found to have the following composition of stable isotopes:
Isotope
Relative abundance / %
(i) Define the term relative atomic mass.
Ir – 191 Ir –
193
37.1
62.9
(ii) Calculate the relative atomic mass of this sample of iridium, giving your answer to decimal places.
(c) Iridium – 192 is a short-lived radioisotope used to treat cancer. Define the term radioisotope and name
another radioisotope used in nuclear medicine.
[(b)(ii) 192.26]
10. Using the periodic table, give the symbol(s) of:
(a) an ion with a double positive charge (2+) with an electronic configuration of [Ar]3d5.
(b) two elements with a ground state configuration of ns2np3.
[HL paper 2, May 01]
11(a) State the full electron configuration for a bromide ion.
(b) Write the symbol for the ion with a 2+ charge which has the electron configuration of 1s22s22p6.
(c) Write the symbols for three other species, which also have the electron configuration of 1s22s22p6
[HL paper 2, May 06]
12. Explain the difference in the two values of ionisation energy for each of the following pairs:
(a) The 1st ionization energy of berylium is 900kJ mol-1 whereas the 2nd ionization energy of berylium is
1757 kJmol-1.
(b) The 1st ionization energy of aluminium is 577 kJ mol-1 whereas the ionization energy of magnesium is
735 kJ mol-1.
(c) The successive ionization energies of germanium are show in the following table:
1st
760
2nd
1540
3rd
3300
4th
4390
5th
8950
Ionization energy
/ kJmol-1
(i) Identify the sub-level from which the electron is removed when the first ionization energy of germanium
is measured.
(ii) Write an equation, including state symbols, for the process occurring when measuring the second
ionization energy of germanium.
(iii) Explain why the difference between the 4th and 5th ionization energies is much greater than the
difference between any two other successive values.
[HL paper 2, Nov 05]