Unit 3 – Atoms

Warm up – CRASH COURSE – THE NUCLEUS Atomic Structure Notes What is an atom? How do we know they exist? Agenda: Warm up – CRASH COURSE – THE NUCLEUS Atomic Structure Notes Brain break – POWERS OF TEN Atomic structure practice Exit ticket Homework: Complete practice examples Objective: Objectives: Students will be able to.... 1. Describe the three types of subatomic particles, their charge, and location in an atom. 2. Use an isotope symbol to find the number of protons, neutrons, and electrons in an atom of that element.

Warm up: 1. What are the three subatomic particles and their locations in the atoms? Agenda: Warm up Check / Review HW – atomic symbols Building an atom pHet prelab / lab Atomic History Video (10 min) ? Exit ticket 2! Homework: Atomic structure POGIL Objective: Be able to identify the type and number of subatomic particles in an atom of a given element and write the appropriate isotope symbol.

Warm up: 1. Use the information from the right to determine the number of protons, neutrons, and electrons in an atom of astatine 2. Is the mass of 1.01 amu on the periodic table the exact mass of a Hydrogen atom? Agenda: Check and review homework Isotopes notes and average atomic mass notes Homework: isotopes and average atomic weight practice EXIT TICKET Objective: Be able to identify the type and number of subatomic particles in an atom of a given element and write the appropriate isotope symbol. Be able to calculate the average atomic weight for an element based on the relative abundance of its ions.

Average Atomic Weight Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. The exact mass and relative abundance of each of these isotopes can be found in the table below. Calculate the average Atomic weight for carbon. mass number exact weight percent abundance 12 12.000000 98.90 13 13.003355 1.10

Average Atomic Weight Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. The exact mass and relative abundance of each of these isotopes can be found in the table below. Calculate the average Atomic weight for carbon. mass number exact weight percent abundance 12 12.000000 98.90 13 13.003355 1.10 To calculate the average atomic weight: Convert the percent abundance to a decimal. Multiply the exact weight of each isotope by its relative abundance. Add the results together and round off to an appropriate number of decimals This is the solution for carbon: (12.000000) (0.9890) + (13.003355) (0.0110) = 12.011 amu

Warm up: 1. Write the isotope symbol for an atom with 53 protons, 74 neutrons and 54 electrons. 2. Nitrogen-14 is 99.63% abundant and nitrogen-15 is 0.37% abundant. Calculate the average atomic weight. Agenda: Check and Review homework Notes III Drawing Bohr Models and lewis dot diagrams Exit ticket Homework: Review ws study for quiz next class REVIEW UNIT 3 CONCEPTSOBJECTIVES Students will be able to determine the number of protons, neutrons, and electrons in an atom by using the periodic table or isotope symbols. When given a model of an atom, students will be able to identify it on the periodic table or write an isotope symbol. Students will understand how the structure or identity of an atom changes when the number of subatomic particles changes. (atoms vs. isotope vs ion)

SUMMARIZER What is the difference between the isotopes Hydrogen-1 and hydrogen-3? Write their isotope symbols. What changes to cause a neutral atom to form an ion? Draw and write the symbol for an atom with 7 protons, 7 neutrons, and 10 electrons.

Check study guide – questions Test on atomic structure Homework: Warm up: 1. Review your study guide! Test in a few minutes. Agenda: Check study guide – questions Test on atomic structure Homework: READ AND HIGHLIGHT LAB Answer prelab questions Illustrate procedure part A & B in margin