Atomic Theory & Structure

Multiple Choice

Which Greek philosopher was among the first to suggest the existence of atoms?

• Democritus

• Aristotle

• Plato

• Socrates

Open Ended

Why do you think understanding atomic structure is important for studying chemistry and the periodic table?

Multiple Choice

Which statement is NOT part of Dalton's Atomic Theory?

• Atoms of the same element are identical.

• Atoms can be divided into smaller particles.

• Atoms combine in whole-number ratios to form compounds.

• Atoms are never changed into atoms of another element in a chemical reaction.

Open Ended

Explain how the use of scanning tunneling microscopes has changed our understanding of atoms.

Multiple Select

Which of the following are examples of subatomic particles?

• Electrons

• Protons

• Neutrons

• Molecules

Multiple Choice

What is a modern application of cathode ray tubes?

• Smartphones

• Television sets

• LED bulbs

• Solar panels

Multiple Choice

Who determined the mass of the electron using the oil drop experiment?

• John Dalton

• J.J. Thomson

• Robert Millikan

• Ernest Rutherford

Multiple Choice

Based on the conclusions from the study of the electron, why must atoms contain positive particles?

• To provide energy for chemical reactions

• To balance the negative charge of electrons

• To increase the mass of the atom

• To allow atoms to bond with each other

Multiple Choice

Which subatomic particle was discovered by Eugene Goldstein and what is its charge?

• Neutron, no charge

• Electron, negative charge

• Proton, positive charge

• Proton, negative charge

Multiple Select

Which of the following statements about subatomic particles is/are correct?

• Electrons are found in the nucleus.

• Protons have a positive charge and are found in the nucleus.

• Neutrons have no charge and are found in the nucleus.

• Electrons have a much smaller mass than protons and neutrons.

Open Ended

Compare the mass and charge of protons, neutrons, and electrons as shown in the table. How do these differences affect the structure of the atom?

Multiple Choice

Which of the following conclusions did Rutherford draw from his gold foil experiment?

• The nucleus is small, dense, and positively charged.

• The atom is made only of electrons.

• Atoms are indivisible.

• Electrons are found inside the nucleus.

Open Ended

Explain how the results of Rutherford's gold foil experiment led to a new model of the atom.

Multiple Select

Based on the Rutherford atomic model, which of the following statements are correct?

• The atom is mostly empty space.

• The nucleus contains protons and neutrons.

• Electrons are found inside the nucleus.

• The electrons occupy most of the atom's volume.

Multiple Choice

According to Niels Bohr's model, how do electrons move around the nucleus?

• In circular paths of fixed energy levels.

• Randomly throughout the atom.

• In straight lines.

• Only inside the nucleus.

Multiple Choice

When electrons jump from one energy level to another, what do they absorb or emit?

• Light energy

• Sound energy

• Heat energy

• Mechanical energy

Multiple Choice

What does the equation E=hv represent in the context of atomic physics?

• The relationship between energy and frequency of light

• The number of protons in an atom

• The difference in energy between two states

• The atomic number of an element

Open Ended

Explain how the energy of an emitted photon is related to the energy levels of an atom.

Multiple Select

Which of the following statements are correct regarding atomic number and protons?

• Atomic number is equal to the number of protons in the nucleus.

• Elements are different because they have different numbers of protons.

• The number of protons in an atom is always equal to the number of electrons.

• Atomic number is equal to the number of neutrons in the nucleus.

Open Ended

Given the table of elements, if an atom has 15 protons, what is its atomic number and which element is it?

Multiple Choice

Which elements do you think will have a low ionization energy and lose electrons more readily?

• elements that form anions (negative charge)

• Elements that form cations (positive charge)

• Transition metals

Multiple Choice

Which of these elements has the highest ionization energy?

• Lithium (Li)
• Potassium (K)
• Francium (Fr)
• Sodium (Na)

Multiple Choice

What is ionization energy?

• The energy required to make an ion.

• The energy required to add an electron to an atom.

• The energy required to remove an electron form an atom.

• The energy required to power up a warp drive.

Multiple Choice

What elements do you expect to have a high electron affinity?

• Elements that form cations

• Elements that form anions

• Transition metals

Multiple Choice

What family has almost zero or very little electron affinity?

• Halogens
• Noble gases
• Alkali gases
• Chalcogens

Multiple Choice

What elements have the highest Electronegativity?

• Halogens (group 17)

• Alkali Metals (Group 1)

• Alkaline-earth Metals (group 2)

• Noble gases (group 18)

Multiple Choice

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)
• Neon (Ne)
• Antimony (Sb)
• Germanium (Ge)

Multiple Choice

Atoms that have a high electronegativity, _______________.

• give up their electrons more easily.
• hold on to their electrons more tightly.
• have more electron shells.

Open Ended

What questions do you still have about atomic structure or the history of atomic theory?