Isotopes and Atoms

^atomic number: number of protons

-atomic mass - atomic number = number of neutrons
 (p+n)           -    (p)                =  (n)

Example:
Isotopes    Mass   Atomic #    #of protons   # of neutrons
C                 14        6                     6                    8
K                 39       19                  19                   20
Na                23       11                 11                    12

Mass spectrometers: is used to determine the abundance and mass of the isotopes of elements

mass spectrom for boron:

Nicole H

Quantum Mechanics

-The difference between the bohr theory and quantum theory
Bohr Theory: the electron is a particle theat must be in orbital in the atom
Quantum Theory: the electron is a cloud of negative charge or a wave function



S orbital - each orbital holds 2 electrons
P orbital - 3 suborbitals: contain 2 electrons each
D orbital - 5 suborbitals: contain 2 electrons each
F orbital - 7 suborbitals: contain 2 electrons each


Nicole H

How to Draw Bohr Diagrams

Follow this link to learn how to draw Bohr Diagrams:
http://www.slideshare.net/profpaul/bohr-diagrams

Remember:

Electrons occupy shells which are divided into orbitals, the first shell holds 2 electrons, the second one holds 8, and the third one 8, and the fourth one 16.





Janine R

October 12 class (Bohr Notes)

Bohr (1920's)

-Rutherfords first tried to make a model before Bohr, his model was very unstable

-Bohr based his model on the energy (light) emitted by different elements

-Bohr believed each atom has a specific spectra of light 

Bohr's Theory

-electrons exist in orbitals

-when they absorb energy they move to a higher orbital

-as they fall from a higher orbital to a lower one they release energy as a photon light

Sofia N

THE TEST

This class we did the test :(

A Review of what was on it :
1. Lab safety
     -Do not run in the lab
     -Wear safety equipment
     -Tie your hair back

2. Balancing Equations
     -Refer to link below on a review of how to balance equations
                 http://www.youtube.com/watch?v=8KH3laR2iR4

3. Dimensional Analysis
     -How many miles are equal to 120km?
                1.6km =1 mi
            120km  x  1mi       =75 mi
                           1.6km
4. Scientific Notation

Nicole H

(September 22 Class) Units

In class we learned all about the different SI units, which include;

SI BASE UNITS 


Base Quantity                          Base Unit                                     Symbol
Length-----------------------------meter------------------------------m
Mass------------------------------kilogram---------------------------kg
Time------------------------------second-----------------------------s
Temperature----------------------kelvin------------------------------K
Amount of a substance------------mole------------------------------mol
Electric Current-------------------ampere----------------------------A
Luminous intensity----------------candela-----------------------------cd

COMMON METRIC PREFIXES 

Prefix	Abbreviation	Meaning
Mega-	M	106 or 1000000
Kilo-	k	103 or 1000
Deci-	d	10-1 or 0.1
Centi-	c	10-2 or 0.01
Milli-	m	10-3 or 0.001
Micro-	µ	10-6 or 0.000001
Nano-	n	10-9 or 0.000000001
Pico-	p	10-12 or 0.000000000001

IF YOU HAVE ANY OTHER QUESTIONS ABOUT UNITS PLEASE REFER TO THE LINK BELOW THANKS!
http://en.wikipedia.org/wiki/SI_derived_unit


SOFIA NGUYEN

Atomic Theories

Democritus 

-called these particles atoms
-in 300 BC said atoms were indivisible particles






















John Dalton 

-each element is composed of extremely small particles called atoms
-identical, but differ from other elements
-neither created or destroyed in any chemical reactions
-always same relative numbers












Lavoisier

-law of conversation of mass














Proust

-if a compound is broken down into its constituents, the producers exist in the same ratio as in the compound
















JJ Thompson

-raisin bun model 
-said, positive, spheres with negative particles embedded in them
-1st atomic theory to have positive (protons) and negative (electrons) changes












Rutherford

-showed that atoms have a positive, dense centre with electrons outside it














Janine R