03.01 Atomic Theory Guided Notes Objectives:
In the lesson you will:
explain how Dalton's atomic theory was modified, but not discarded
describe the structure of an atom
describe the electrical charges and forces that exist between protons, neutrons, and electrons
state the atomic masses of protons, neutrons, and electrons
Big Ideas:
Key Questions and Terms
Notes
What new scientific evidence led to changes in Dalton’s atomic theory?

What did J. J. Thomson discover about electrons?

What was Rutherford’s contribution to the structure of an atom?

Explain the process of how James Chadwick found the neutron.

Explain what can happen to scientific theories over time.

What is the structure of an atom?

What is a proton?

What is a neutron?

What is an electron?

What are the forces that exist inside an atom?

Explain how a neutral atom can become positively or negatively charged.

What are the atomic masses of protons, neutrons, and electrons?

How is the atomic mass of an atom determined and why are electrons not used in the calculation?

What is an amu?

Which describes interactions between substances and stomata during photosynthesis? check all that apply. oxygen enters stomata. oxygen is released through stomata. carbon dioxide enters stomata. carbon dioxide is released through stomata. hydrogen enters stomata. hydrogen is released through stomata.

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap

Tell me the iupac names of the following alcohols: