Structure S 1.2—The nuclear atom

What are the main components of an atom?

• Protons, neutrons, and electrons

• Protons, neutrons, and positrons

• Protons, electrons, and quarks

• Neutrons, electrons, and photons

How do protons and neutrons differ in terms of charge?

• Protons are neutral, neutrons are negatively charged.

• Protons are negatively charged, neutrons are positively charged.

• Both protons and neutrons are positively charged.

• Protons are positively charged, neutrons are neutral.

What is the charge of an electron?

• 0 coulombs

• -1.0 coulombs

• +1.602 x 10^-19 coulombs

• -1.602 x 10^-19 coulombs

Define the term 'nuclear symbol' in relation to atoms.

• A diagram showing the bonding between atoms.

• A representation of an atom's electron configuration.

• A symbol indicating the temperature of an atom.

• A notation that shows the chemical element, atomic number, and mass number of an atom.

How can you determine the number of neutrons in an atom using its nuclear symbol?

• Number of neutrons = Mass number x Atomic number

• Number of neutrons = Atomic number + Mass number

• Number of neutrons = Mass number - Atomic number

• Number of neutrons = Atomic number - Mass number

What is the significance of the atomic number in the periodic table?

• The atomic number is significant because it defines the element and its properties.

• The atomic number determines the color of the element.

• The atomic number indicates the mass of the element.

• The atomic number is irrelevant to chemical reactions.

Explain what isotopes are and give an example.

• Isotopes are always radioactive and cannot be stable.

• An example of isotopes is Oxygen-16 and Oxygen-18, which have different atomic numbers.

• An example of isotopes is Carbon-12 and Carbon-14, where both have 6 protons but Carbon-12 has 6 neutrons and Carbon-14 has 8 neutrons.

• Isotopes are atoms with different numbers of protons.

How do isotopes of the same element differ from each other?

• Isotopes differ in the number of neutrons and atomic mass.

• Isotopes are identical in mass but differ in their electron configuration.

• Isotopes differ in the number of protons and chemical properties.

• Isotopes have the same number of neutrons but different atomic numbers.

What is the relative mass of a proton compared to a neutron?

• The relative mass of a proton is twice that of a neutron.

• The relative mass of a proton is half that of a neutron.

• The relative mass of a proton compared to a neutron is approximately 1:1.

• The relative mass of a proton compared to a neutron is 2:1.

Why is the mass of an electron considered negligible?

• Electrons have more mass than protons.

• The mass of an electron is significant in atomic structure.

• Electrons are heavier than neutrons.

• The mass of an electron is negligible compared to protons and neutrons.