Studied by 0 people
Looks like no one added any tags here yet for you.
Subatomic particles
Particles that make up an atom: protons, neutrons, and electrons.
Relative atomic mass
Mass of subatomic particles compared to each other.
Proton
A subatomic particle with a relative charge of +1 and a relative mass of 1.
Neutron
A subatomic particle with a relative charge of 0 and a relative mass of 1.
Electron
A subatomic particle with a relative charge of -1 and a negligible mass.
Nucleus
The positively charged center of an atom containing protons and neutrons.
Electrostatic attraction
The force that holds electrons in orbit around the nucleus.
Atomic number (Z)
The number of protons in the nucleus of an atom.
Mass number (A)
The total number of protons and neutrons in the nucleus of an atom.
Isotopes
Atoms of the same element with the same number of protons but different numbers of neutrons.
Atomic structure
The arrangement of subatomic particles within an atom.
Neutral atom
An atom with an equal number of protons and electrons.
Ion
A charged particle that has gained or lost electrons.
Relative charge of a proton
+1.
Relative charge of a neutron
Relative charge of an electron
-1.
Number of neutrons
Calculated by mass number - atomic number.
Chemical symbol of an element
A notation consisting of one or two letters representing an element.
Balanced charge in a neutral atom
Number of protons equals the number of electrons.
Percentage abundance
The relative amount of an isotope in a sample.
Relative atomic mass (Ar) definition
The average mass of one atom of an element compared to one twelfth of the mass of an atom of carbon-12.
Atomic model
A visual representation showing the nucleus and electron arrangement.
Mg2+ ion
A magnesium ion with a charge of +2, meaning it has lost two electrons.
Carbon atom
An atom with an atomic number of 6, containing 6 protons and 6 electrons.
Mass of a proton
Assigned a relative mass of 1.
Mass of an electron
Considered negligible compared to protons and neutrons.
Formation of a positive ion
Occurs when an atom loses one or more electrons.
Formation of a negative ion
Occurs when an atom gains one or more electrons.
Relative atomic mass calculation
Total mass of isotopes divided by total number of isotopes.
Copper
Element X with 29 protons and mass number 63.
Carbon-12
An isotope of carbon containing 6 protons and 6 neutrons.
Carbon-14
An isotope of carbon containing 6 protons and 8 neutrons.
Mass of oxygen isotopes example
Calculating the relative atomic mass using percentage abundances.
Formula for calculating neutrons
Number of neutrons = mass number (A) - number of protons (Z).
What does it mean to be an isotope?
Same element with the same number of protons but different number of neutrons.
Note 
Flashcard (80)