Download Oct 14th ,2015

Welcome to Chemistry! Oct 14, 2015 Wednesday
Do now: if you clearly have a Agenda:
–Finish Work on st4
hetrogenous mixture what are
classwork #2 Look at st 3
some ways you can separate
assessment
it?
(Pick up periodic table up
front)
Objectives:
St 4: Matter: Understand the structure of an
atom in terms of its subatomic particles;
isotopes and ions; differentiate between the
classification and separation of matter
(mixtures, pure substances…)
IONS: LEARN EM!
Atomic Structure
introduction
Assignments:
Mass volume lab final report
due Thursday
St 4 cw 1 and 2 check off
thursday
The Week:
Thursday Atomic practice
Periodic table
• This is your copy to use for any assessement
(except the ion assessment)
• You make make any handwritten notes on it
you want. ( I will give some hints on that
through out the year)
• Find a safe and easily accessible place for it.
– If you don’t have a pocket you can make one out
of the provided cardstock later today in your
notebook.
Right hand side!!!!!
If you have mystery substance
consider putting the substance
through these steps
*
Can it physically
be separated?
See 1 and 2
2. If your sample
looks uniform, and
you get a result for
Distillation and
Chromotography
Then yes for
homo.mixture
I. If you get a result
(solids) with Filtration
, Decanting and
Centrifuging then you
have a hetro.mixture
3. Electrolysis
Also here here
Standard 3 check in
•
•
•
•
•
Retake will be next week
St 3 classwork is due Friday if not done?
DPSE solving method
Sample problem?
If you know that gold has a density of 19.6
g/mL and you have 354ML of Gold ( a pop
can!) then how many grams is that? How
much money is that worth 37 dollar/gram
Right hand side!!!!!
10/14/15 EQ: What is the landscape of an
atom?
Matter
Matter: Anything that has
mass and takes up space.
Atoms
Building blocks of matter.
Contains subatomic particles:
abbreviations
Electrons
E
Neutrons
N
Protons
P
Subatomic Particles
Protons and electrons are the only particles
that have a charge.
Protons and neutrons have essentially the
same mass.
The mass of an electron is so small we ignore
it.
Symbols of
Elements
Mass number (number of
protons plus neutrons)
Atomic number (number
of protons)
C
12
6
Resulting
Charge
Symbol of the
Element
Elements are symbolized by one
or two letters.
Atomic Number
Mass number (number of
protons plus neutrons)
Atomic number (number
of protons)
C
12
6
Resulting
Charge
Symbol of the
Element
All atoms of the same element
have the same number of
protons
Atomic Mass
Mass number (number of
protons plus neutrons)
Atomic number (number
of protons)
C
12
6
Resulting
Charge
Symbol of the
Element
The mass of an atom in atomic
mass units (amu) is the total
number of protons and neutrons in
the atom.
Determining Electrons
Mass number (number of
protons plus neutrons)
Atomic number (number
of protons)
Resulting Charge
C
12
6
Symbol of the
Element
In elements the # of protons = the # of electrons,
so the element is electrically neutral and no
charge is shown.
However atoms can gain or lose electrons to
become ions and the resulting charge is shown.
Isotopes
•Atoms of the same element with
different masses.
•Isotopes have different numbers of
neutrons. Carbon actually has 15
different isotopes!
11
C
6
12
C
6
13
C
6
14
C
6
• Protons = electrons in Atoms
• Protons ≠ electrons in Isotopes
Isotopes
•Your periodic tables show an AVERAGE atomic
mass.
•Round this to the nearest whole #.
•On our tables, atomic mass of carbon is 12.01
•IRL:
•98.9 % is Carbon-12
It averages to 12.01
•1.1% is Carbon-13
•.0001% is Carbon-14
11
C
6
12
C
6
13
C
6
14
C
6