Download Standard A

STANDARD A
• MOST OF THE SLIDES FROM THIS POWER POINT PRESENTATION COMES FROM HOLT
CHEMISTRY. PLEASE DISREGARD THE CHAPTER NUMBERS.
• STANDARD A ASSESSEMENT WILL BE ON CHAPTER 2 OF THE IB CHEMISTRY BOOK
STANDARD A
LG (a) SUBATOMIC PARTICLES
Describe the proton,
neutron and electron in terms of location in atom,
relative mass and charge and number of each in atoms
and ions as described by atomic number and atomic
mass.
Standard A
LG (b) EARLY HISTORY OF ATOMIC MODEL: Know the
contributions made by Dalton, Thomson, Millikan,
Rutherford and Chadwick as well as the experiments
the lead to the discovery of the atom and its
subatomic particles.
Thomson’s experiment involved
a cathode ray tube with a gas at low
pressure. The gas flowed from the
negative end to the positive end of the
tube. Because the gas consisted of
electrons, it
was repelled by the negative end of the
magnet and attracted by the positive end
of the magnet showing that an electron is
negatively charged
THOMSON’S MODEL IS
CALLED THE PLUM
PUDDING MODEL
Thomson explained that
the model was like plums
representing the
electrons in pudding
represented as protons
Rutherford’s Gold Foil
experiment involved shooting
positively charged alpha
particles through a thin piece of
gold foil. He expected the alpha
particles to pass straight through
or get struck in the positive part.
Instead most alpha particles
passed straight through but a
few were deflected or bounced
straight back. This lead to the
conclusion that an atom is
mostly empty space but has a
very small positively charged
center (nucleus)
James Chadwick discovered the neutron.
The neutron was the last subatomic particle to be discovered
because the neutron is neutrally charged. However because it
has a mass almost equal to the proton, it became obvious that
there had to be something else in the nucleus besides the
proton
STANDARD A
LG (c) ISOTOPES: Describe an isotope, compare the
properties of the isotope of an element and deduce the
symbol of an isotope given its mass number and atomic
number.
LG (d) RELATIVE MASS (AVERAGE ATOMIC MASS):
Calculate the non integer relative mass and abundance
of isotopes from given data.
LG (e) Discuss the use of radioisotopes
LG (f) MASS SPECTROMETER: Describe how the mass spectrometer is
used to determine relative atomic masses
LG (g) ELECTROMAGNETIC SPECTRUM/ELECTRON CONFIGURATIONS: Describe the
electromagnetic spectrum, explain how the lines in the emission spectrum of
hydrogen are related to energy levels and distinguish between continuous and line
spectrum.
LG (h) ELECTRON ARRANGEMENT: Deduce the electron arrangement for atoms
and ions up to Z=20.