Your cell phone should be away during all times today.

Learning Intentions

• You can use shorthand notation for an element to determine element identity, number of protons, neutrons and electrons.

• You can describe and  determine average atomic mass for an element using given data about abundance and mass of each isotope of the element.

• You can create a data table to collect data for an lab.

Content Standards being covered:

Student understands the structure of matter at the atomic level and the history that lead to our current understanding.
51. Atoms of elements are the smallest discrete forms of matter in the universe
52. Each element has a nucleus, made of protons and neutrons, which surrounded by a cloud of randomly moving electrons.
53. Protons are positively charged, neutrons are neutral, and electrons are negatively charged.
54. Protons and neutrons have a general mass of 1 atomic mass unit (amu), while an electron has a relative mass of 0.0005 amu. Protons and neutrons therefore contribute to an atom's mass and can be added together to determine atomic mass. The electron’s mass is not significant in comparison.
55. An isotope is the same element with different amounts of neutrons and therefore affects the mass of the atom
56. Average atomic mass is a relative atomic mass number that is based on the masses of all known isotopes and their relative abundance in the universe

Habits of Mind/Life skills being covered:

Striving for Accuracy

Journal Entry:

How do you think average atomic mass is determined for an element?