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AP Chemistry
Review:
Big Idea #1 MRS. BRAYFIELD
Review before we start…
Significant figures:
Nonzero integers count as significant
Leading zeros precede all nonzero digits and are not
significant
Zeros between nonzero digits are significant
Trailing zeros ARE NOT significant
Apparently some college rules are different…..
Exact numbers never limit the number of significant
figures in a calculation
Significant figures in calculations
For multiplication and division, the number of sig figs is
the same as the measurement with the least number of
sig figs
For addition and subtraction, the number of decimal
places is the same as the measurement with the fewest
number of decimal places
Big Idea #1
The chemical elements are fundamental building
materials of matter, and all matter can be
understood in terms of arrangements of atoms.
These atoms retain their identity in chemical
reactions.
Chapters in Book
Refer to chapters 1, 2, 3, 4, 7, 8
Atomic Structure
John Dalton
His model had 4 parts:
Each element is made of atoms
Atoms of a given element are identical
Atoms can combine to form compounds
These compounds have the same relative number and type of
atoms
Chemical reactions involve rearrangement of bonded atoms – do not change atoms
Dalton’s Laws
Law of Definite Proportion
A given compound always contains exactly the same
proportions of elements by mass
Law of Multiple Proportions
When two elements form a series of compounds, the
ratio of masses of the second element that can
combine with 1 gram of the first element can be
reduced to the smallest whole number
How we calculate empirical formulas
Atomic Structure
Dalton’s model of hard spheres was challenged
because of isotopes
Isotopes – atoms of the same element with different
numbers of neutrons (different masses)
Average atomic mass calculations
Take the percent abundance and multiply by the
weight
Mass Spectrometry
This is a technique to
determine the mass
spectrum of an element.
In this technique, a sample
is ionized and the fragments
are passed through a
sensor
Atomic Structure
Niels Bohr used line spectrums to develop his atomic
theory
Looks like a solar system
You have a nucleus that is orbited by electrons
Electromagnetic Radiation
From shortest to longest:
Gamma rays, x-rays, ultraviolet, visible, infrared, microwave, and radio
Electromagnetic radiation can acts as particles and
waves
Electromagnetic Radiation
𝑣 = 𝑐/𝜆
v = frequency; c = speed of light; λ = wavelength
We can quantize light:
Δ𝐸 = 𝑛ℎ𝑣
Where E is energy, n is integer (quantum number), h is Planck’s constant, and v is frequency
𝐸𝑝ℎ𝑜𝑡𝑜𝑛 = ℎ𝑐/𝜆
Atomic spectrum – it shows us the absorption lines
for an element
Quantum Mechanical Model
The quantum mechanical
(QM) model shows us the
three dimensions of the
wave functions
This is the mathematical
probability of finding
electrons in the electron
cloud
Structure of Atom
Subatomic particles (proton, neutron, electrons)
Coulomb’s Law:
𝐹 = 𝑘𝑞1𝑞2
𝑟
Where F is force, k is a constant, q is charge, r is
distance
Coulomb’s Law shows us the force that holds the atom
together
Photoelectron Spectroscopy
Photoelectron spectroscopy (PES)
is a technique that can be used
for electron shells in an atom
Light is shined on an atom and the
minimum frequency needed to
remove an electron is determined
From this data, you can find the
ionization energy
Electrons further away from the
nucleus need less energy than
ones close to the nucleus due to
shielding
PES
To read the graph of PES, it shows the relative
number of electrons that come off at different
energies
BASICALLY, it is a pictorial diagram/graph of the
electron configuration and how ionization energies
relate
http://www.chem.arizona.edu/chemt/Flash/photoe
lectron.html for simulation
http://www.adriandingleschemistrypages.com/ap/s
ummary-of-additions-to-new-ap-chemistry-
curriculum-part-1-pes/ for questions
Quantum Numbers
There are four quantum numbers:
n: principle quantum number; related to size and
energy of the orbital
l: angular momentum quantum number; related to
shape of the orbital
ml: magnetic quantum number; related to the position
of the orbital in space
ms: electron spin quantum number; related to the spin
of the electron (only two values)
Quantum Numbers
Quantum number n
Values of 1, 2, 3, 4, etc.
Refers to the row number
Quantum number l
Values of s, p, d, f
Electron Configurations
Aufbau principle:
Fill lower orbitals first
For example
Config. for Oxygen:
To find # of valence
electrons, it’s the # of
electrons in highest level
6 for Oxygen
Periodic Trends
Atomic Radii
Decrease going across
Increases going down
Ionization Energy
Increases going across
Decreases going down
Electron Affinity
Increases going across
Decreases going down
Periodic Trends
Ionic Radii
Cations are smaller than parent
Anions are larger than parent
Matter on Macro Scale
Molar mass
The weight (in grams) of one mole of a substance
Percent composition
𝑀𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑖𝑛 1 𝑚𝑜𝑙 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
𝑀𝑎𝑠𝑠 𝑜𝑓 1 𝑚𝑜𝑙 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑× 100%
Mixtures
Pure substances (element and compound)
Mixtures (homogeneous and heterogeneous)
How to separate mixtures (distillation, filtration,
chromatography)
Conservation
Atoms and therefore mass must ALWAYS be
conserved in any chemical reaction
Identifying Matter
Infrared spectroscopy
This measures the radiation absorbed by molecules
This is from different bonds absorbing different frequencies
Each molecule produces a unique spectra
Identifying Matter
UV-Vis spectroscopy
This measures the radiation
that double bonds absorb
Gravimetric Analysis and
Titration
Titrations with acids and
bases to reach an endpoint
Homework
http://www.cengagebrain.com/shop/isbn/97805471
25329
Go towards bottom of page and click “Free Materials”
Click “Access Now” to go to companion site
From the pull down menu select the chapter you wish
to view
Take the “Tutorial Quiz”
When finished, make sure to print out results or email them to me: [email protected]
Do chapters 1, 2, and 7