Download Unit 3 Study Guide

Unit 3 Atomic Structure and the Periodic Table
Vocabulary to know
proton
neutron
electron
nucleus
atom
atomic mass
mass number
atomic number
isotope
ion
charge
element
period
group
alkali metal
alkaline earth metal
transition metal
representative metal
nonmetal
halogen
noble gas
atomic radii
ionic radii
isoelectronic series
ionization energy
electronegativity
s orbital
p orbital
d orbital
f orbital
s block
p block
d block
f block
quantum numbers
principle quantum number
angular momentum quantum number
magnetic quantum number
spin quantum number
orbital energy
Aufbau Principle
Hund’s rule
Pauli Exclusion Principle
Electron configuration
People:
Democritis Boyle
Lavoisier Dalton
Thomson Millikan Rutherford Bohr
-
Chadwick Schrӧdinger Heisenberg deBroglie Mendeleev -
first person to propose the existence of atoms
Started scientific revolution with his Skeptical Chemist publication
Demonstrated Law of Conservation of Mass, Discovered Oxygen
First atomic theory based on experimental evidence, 5 parts, atoms are spheres.
Discovered electron using the Cathode Ray Tube; Plum Pudding model of atom,
measured charge to mass ratio of electron
Oil drop experiment allowed accurate measure of electron mass and charge
Used gold foil experiment to discover nucleus of the atom; Discovered protons; Nuclear
model of atom
Explained optical spectra using the planetary Bohr Model of atom; First quantized model
Uses orbits.
Discovered neutrons
Provided mathematical description of quantum mechanical orbitals
Proposed the Uncertainty principle – the electron is only probably located in orbital
Proposed electrons and other particles have wavelengths
Developed the first periodic table; Predicted the discovery of Gallium
Atomic models
Atomic theory - Know 4 parts
Plum Pudding model - Be able to describe parts of atom including what parts are +/Nuclear atom first model that is still relevant; we use the nuclear model; know 3 parts; know features of
subatomic particles, know where subatomic particles are located, their charges, relative
masses, and symbols
Bohr model Basically the nuclear model + electrons organized into quantized circular orbits
Quantum mechanics Currently accepted atomic theory; Basically the nuclear model + electrons
organized into quantized regions of space where you are likely to find an electron
called orbitals, HIGHLY confirmed theory. 100 yrs old, and still best
Experiments:
Cathode Ray Tube -
Millikan Oil Drop-
Gold Foil Experiment Optical Spectra -
Vacuum tube with an electrical charge creates a stream of negatively
charged particles that respond to an applied magnetic field. – used by
Thomson to discover electron, first subatomic particle and measure its
charge/mass ratio, led to Plum pudding model – used in CRT televisions
Tiny oil drop exposed to radiation to give it a charge. Size of charge measured by
balancing oil drop in an electric field. Determines charge on an electron, and
therefore mass of electron.
Radioactive source of heavy positively charged alpha particles shot at very thin
gold foil. Most go through, but some are highly deflected.
When neon light is passed through a prism, you get lines. Explained by electrons
being excited from one orbit to a higher orbit by absorbing a photon of a certain
wavelength, and then emitting that same wavelength when the electron drops back
down. Explained by quantized orbits of the Bohr model.
Memory items
Particle
Symbol
Location
Charge
Relative Mass
1
Actual Mass
(amu)
Electron
e
Outside
nucleus
-1
Proton
p
nucleus
+1
1
1.0073
Neutron
n
nucleus
0
1
1.0087
Common labels
1840
~0
0.00055
Quantum
Number
Name
Allowed
Values
Determines
Specifies
n
Principle
1, 2, 3, 4…..
Size and
Energy
Shell
1, 2, 3,…
(Period #)
Angular
Momentum
0, 1, 2… (only
up to n-1)
Shape
Subshell
s, p, d, f
ml
Magnetic
  ml 
Orientation
Orbital
subscripts: x, y,
z, xz, yz, z2…
ms
Spin
+½ or -½
Spin
Electron
Up ↑, Down ↓
States of the elements ( 2 liquid, 11 gas, all others solid)
Molecular elements (9, including 7 diatomic elements)
Filling order of atomic subshells and the maximum number of electrons for each subshell
Skills
Calculate using percent composition: % = part/whole x 100
Calculate using conservation of mass
Determine average atomic mass from natural isotopic abundances and masses
Determine group #, period #, group name for an element
Rank elements based on atomic size, ionic size, ionization energy or electronegativity
State orbitals described by a given set of quantum numbers
Count electrons within shells, subshells or orbital
Write an electron configuration
Other Review Resources
Class powerpoints (posted online)
Homework worksheets
Personal Class notes
Review worksheet (Hint: The test will look VERY much like the Review worksheet)
After school and/or lunch meeting with teacher
20 pt Vocab quiz on Friday.
Test on Monday
Unit 3 Test Description:
20 x 1 pts
10 x 2 pts
9 pts
10 x 1 pt
6 x 2 pts
3 x 4 pts
1 x 5 pts
1 x 5 pts
1 x 7 pts
People, Experiments, Theories, Vocabulary (like quiz)
Quantum numbers, shell, shapes, electron counting, etc…
Subatomic particle memory items
Element designations from periodic table
Periodic trend decision with justification
Electron configurations
Percent composition calculation
Conservation of Mass problem
Atomic mass calculation
There will be two parallel versions of the test. You will not be allowed to sit next to someone with the same
version. Testing folder crosses will be positioned around the center of each table to block view of same
version on opposite side of table. BEWARE: YOU WILL NOT BE ALLOWED TO USE YOUR PHONE
AS A CALCULATOR AND THERE ARE LIMITED CALCULATORS AVAILABLE TO BORROW.
BRING YOUR OWN CALCULATOR. You will be asked to place your phone in your backpack at your
feet or in a box on the front bench. There shall be nothing on the tables beside the test, your calculator, the
vocabulary word bank, a periodic table, and a writing implement.