Isotopes

Question 1

Define isotopes and give examples to explain

Answer 1

Are atoms of the same atomic number (same element) that have different numbers of neutrons. Ex. Hydrogen has three isotopes, H1, H2, and H3

Question 2

Can describe how electrons occupy orbitals in energy levels around the nucleus (ground state configuration)

Answer 2

Use:
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule

Question 3

Pauli exclusion Principle

Answer 3

Describes the restrictions on the placement of electrons into the same orbital. “ if two electrons occupy the same orbital, they must have opposite spins”

Question 4

Hund’s Rule

Answer 4

Electrons will pair up in an orbital only when all orbitals in the same sublevel have one electron. When single electrons occupy different orbitals of the same sublevel, they all have the same spin

Question 5

Aufbau Principle

Answer 5

Must fill up lower sublevels first before higher ones.

Question 6

If an isotope has more neutrons what will it have?

Answer 6

more mass

Question 7

Percent abundance

Answer 7

percent of an isotope found naturally occurring in a sample of an element

Question 8

Find the average atomic mass of an isotope:

Answer 8

multiply the mass of each isotope by its percent abundance, then add together to get the total average atomic mass of the element

Question 9

Ground state

Answer 9

Lowest potential energy arrangement of electrons in an atom: 1s

Question 10

Percent abundance

Answer 10

percentage of an isotope found naturally occurring in a sample of an element

Question 11

Mass spectrometry

Answer 11

Used to analyze and measure the exact atomic mass of a sample.

Ionizes molecules and then separates them based on their mass

Generated by a graph displaying the relative abundance of each isotope