Upload
gabriel-gibson
View
212
Download
0
Embed Size (px)
Citation preview
Note Guide 1-1 Science and Studying Atoms
•What is science?
--Science begins as curiosity and tries to end with discovery.
--system of knowledge and the methods used to find that knowledge.
--scientists use models to help bring things into perspective and to make it easier to understand.
--scientists use a systematic method (scientific method) to try and discover the answers to their curiosity.
--steps include observations, forming hypothesis, testing the hypothesis, analyzing and drawing conclusions.
keep in mind, one test does not make a theory AND parts, predictions and ideas of the experiment can be revised
--scientists also communicate in the same language (SI).
this is a system of measurement similar to metrics.
EX: We use things like inches and they use things like centimeters….BUT WE ALL IN SCIENCE USE THE SAME (centimeters, for example)
Atoms--get origin from greek scientist Democritis, who says they are indivisible.
•Dalton = Early Scientist = matter is made up of individual particles called atoms (too small to study to observe)
--these atoms have no electrical charge neutral
•Next, Thomson through experiments, provides first evidence that atoms are made of smaller particles
--thomson’s experiment (see pg. 103) showed the presence of negatively charged particles
•Next, Rutherford = gold foil experiment (see pg 104)
--aims a narrow beam of alpha particles at a thin piece of gold foil.
--using a screen around the gold, rutherford was hoping to be able to follow the path an alpha particle takes after it passes through the gold.
--Particles did not behave like he thought: some went straight through, some bounced off at weird angles, while some came straight back.
RESULT: rutherford suggests the nucleus, where positive charges hang out.
•Atoms made of 3 main parts*
Parts Symbol AMU Charge
Electron e- About 0 -Proton* p+ 1 +
Neutron* n0 1 0
**mass of an atom mostly in the nucleus
Note Guide 1-2 The structure of an atom
•Atomic number = # of p+ in an element. Atoms of any given element has same # of p+
i.e. Hydrogen (H) has 1 proton = Atomic number is 1
•Mass number = tells how many p+ and n0 there are in an atom
i.e. Al = Aluminum
p+ = (13) n0 = (14) = mass number is (27)
--Protons + neutrons = mass number
•Isotopes – atoms of the same element that have different #’s of neutrons, thus different mass numbers.
--isotopes do have the same atomic #--Why? # of protons stay the same
--mass # different because # of neutrons different.
EX: Oxygen (O) – 8 protons (never changes!)
--some oxygens have 9 neutrons, giving a mass # of 17.--naming isotopes = using the element name and mass number (Oxygen – 17)
--when an element has a number after it, we are talking about an isotope.