2.1 Study Guide Flashcards
What are isotopes?
The copy of an element but with different nucleon numbers due to a different amount of neutrons in the original element and the similar element.
Describe the position, charge, mass, and function of protons.
Position: In the nucleus.
Charge: +1.
Mass: Heavy.
Function: Identifies an element.
Describe the position, charge, mass, and function of neutrons.
Position: In the nucleus.
Charge: 0.
Mass: Heavy.
Function: Holds the nucleus together.
Determine the atomic mass of an element. Explain.
HG/Mercury’s atomic mass is 80. It’s the amount of protons. It’s also the number above the symbol of the element.
Describe the position, charge, mass, and function of electrons.
Position: Outside the nucleus.
Charge: -1.
Mass: Virtually 0.
Function: Reactivity/chemical reactions.
Determine elements.
Over 100 substances that cannot be chemically interconverted or broken down into simpler substances and are primary constituents of matter.
Determine ion charges.
The charge of an element. Protons - electrons.
If there are 8 protons, 8 neutrons, and 8 electrons, what are the element, the ion charge, and atomic mass?
- The atomic mass = the number of protons, so 8.
- The ion charge = protons - electrons, so 0.
- The element is oxygen because the atomic mass is 8, and oxygen has an atomic number of 8.
The element Zinc has an atomic mass of 30 and an ion charge of +2. What is the number of protons, neutrons, and electrons?
- Protons: 30, because the atomic mass + the protons, and the atomic mass is 30.
- Neutrons: 35 because the mass is 65 and 65-30=35, and because protons + neutrons = mass.
- Electrons: 30.
Explain why isotopes can be useful in scientific research.
Less common isotopes can be used as tracers because they react in the same way during chemical reactions, but can be detected from the most common isotopes.
What is a common isotope?
Radioactive - Can measure and find location/amount of radioactivity.
What is the last common isotope?
Isotope that can measure differences in mass.
