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Atomic Structure

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Rachel Esquibel

on 29 September 2016

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Transcript of Atomic Structure

mass number
: Protons + Neutrons
Atomic Mass expressed as a whole #
# Neutrons = Mass # - Atomic #

Atoms By Number
Electromagnetic Force:
Like charges repel, opposite charges attract.
Strong Force:
Opposes the electromagnetic force between protons in the nucleus.
The strongest of the four forces, but only acts over short distances.
Weak Force:
The force responsible for radioactive decay.
The force of attraction between all objects in the universe.
The weakest of the four forces.
Forces in Atoms
Positively charged, densely packed, Protons + Neutrons
positive charged, mass = 1
neutrally charged, mass = 1
electron cloud
: negatively charged, mostly empty space, location of electrons
negatively charged, mass = 1 / 1840 (0)
Basic Parts of the Atom
9. 09/10/15 Atomic Structure 17
Date Lecture/Lab/Activity Pg#
Table of Contents
Today I will distinguish between atomic number, mass of an atom and average atomic mass So that I can describe the structure of an atom and draw a simple atomic model using information extracted from the periodic table.
I know I've got it when I can construct a model using the information on the periodic table.

Atoms by Number - Explore
Structure of the Atom – Lecture

What is the most recognizable atomic model that you remember. Draw a picture of a model of lithium and the distinctive parts of the model.

Nuclear Symbol for elements
Parts of the Atom
1. Here is a simple atomic model of the beryllium atom. Draw and label the electrons, protons, and neutrons.
2. The total charge on each atom is zero. Explain why.
3. Why do you think the mass of the carbon atom shown is 12 atomic mass units (amu)
Using Atom #'s
1. Compare the two models. List three similarities and three differences.
2. Based on the models, why do you think helium is number 2 and beryllium number 4 on the periodic table.
Element Symbol Atomic# #Proton #electron #neutrons Mass#
Beryllium 5 9
Fluorine 10
6 12
Chlorine 18
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