Structure of the Atom quiz

The electron was discovered by:

The neutron was discovered by:

In Rutherford's experiment, most alpha particles:

The maximum number of electrons in the M shell is:

The atomic number of an element is the number of:

Isotopes of an element have the same:

The valency of magnesium (atomic number 12) is:

Calcium-40 and argon-40 are:

The isotope used in the treatment of goitre is an isotope of:

Thomson's model of the atom is compared to a:

What are valence electrons? How many does chlorine have? (2 marks)

Why are noble gases chemically inactive? (2 marks)

Write the electronic configuration of argon and state its valency. (2 marks)

An atom has 13 protons and 14 neutrons. Find its atomic number and mass number. Identify the element. (2 marks)

Why did Rutherford use a very thin gold foil? (2 marks)

What was the drawback of Thomson's model? (2 marks)

Name the three isotopes of hydrogen and their mass numbers. (2 marks)

What is the relation between mass number, atomic number and the number of neutrons? (2 marks)

Why is an atom electrically neutral? (2 marks)

Which isotope is used as fuel in nuclear reactors? Which is used in treating cancer? (2 marks)

An atom has electronic configuration 2, 8, 7. Find its atomic number and valency. Identify the element. (3 marks)

The mass number of an atom is 31 and it has 16 neutrons. Find the number of protons and electrons and write the electronic configuration. (3 marks)

Carbon has isotopes carbon-12 and carbon-14. Find the number of protons, neutrons and electrons in each. (3 marks)

Element Z has two isotopes of mass 10 u and 11 u present in the ratio 1 : 4. Find its average atomic mass. (3 marks)

Find the number of neutrons in the nuclei of sodium-23, uranium-235 and cobalt-60, given their atomic numbers 11, 92 and 27. (3 marks)

Read the passage and answer the questions. In 1911, Rutherford's team bombarded a gold foil about 1000 atoms thick with fast-moving alpha particles. Most passed through, some were deflected by small angles, and about one in 12,000 bounced back. (i) What did the passage of most particles show? (ii) What did the bouncing back of a few particles show? (iii) What did Rutherford conclude about the size of the nucleus? (5 marks)

Read the passage and answer the questions. Doctors use cobalt-60 to treat cancer and iodine-131 to treat goitre. Scientists use carbon-14 to find the age of fossils. (i) What are these substances called? (ii) Why are they radioactive? (iii) Name one isotope used as fuel in nuclear power plants. (5 marks)

Read the passage and answer the questions. An element has 2 electrons in its K shell, 8 in its L shell and 2 in its M shell. (i) Find its atomic number. (ii) Identify the element and its valency. (iii) Will it lose or gain electrons to form an ion? Write the ion. (5 marks)

Read the passage and answer the questions. Thomson proposed that an atom is a sphere of positive charge with electrons embedded in it like seeds in a watermelon. Rutherford's experiment later disproved this. (i) Why is the atom neutral according to Thomson? (ii) Which observation of Rutherford's experiment could Thomson's model not explain? (iii) Name the model that replaced Thomson's model. (5 marks)

Read the passage and answer the questions. Neon has atomic number 10 and mass number 20. Sodium has atomic number 11 and mass number 23. (i) Write their electronic configurations. (ii) Why is neon unreactive while sodium is very reactive? (iii) Find the number of neutrons in each. (5 marks)

Draw a labelled diagram of Rutherford's model of the atom. Explain its features and why it was not stable. (6 marks)

Draw Bohr's model of the atom showing the K, L, M and N shells. State the rules for filling electrons in these shells. (6 marks)

Draw the atomic structures of the first 10 elements showing electrons in shells. Find the valency of each. (6 marks)

Draw a labelled diagram of the discharge tube experiment that led to the discovery of canal rays. Explain how it showed the presence of positive particles. (6 marks)

Draw a chart comparing isotopes and isobars with examples. Explain the applications of isotopes. (6 marks)