Notes Name: Atomic Structure
ATOM
ELEMENT
An ________________
is the smallest, complete part of an ________________that
retains all of the properties
and characteristics of the element (like ionization energy, reactivity, and electronegativity.) At atom is
NUCLEUS
neutral, meaning it has no charge. There are two parts of an atom, the _______________________ and the
ELECTRON CLOUD All of the mass of the atom is in the ____________________
NUCLEUS
____________________.
while all of the space of
ELECTRON CLOUD
the atom is in the _________________________.
The atom is made up of 3 things:



Finding # of protons, neutrons, and electrons
Protons: ____charge,
+
mass =____,
1 are in
To find the:
the nucleus. Protons = Atomic #
# protons:
Look at the atomic number
1
Neutrons: NO
____ charge, mass =____, in the
# neutrons:
Subtract the two numbers from
nucleus. Neutrons are the peacekeepers of
periodic table
the nucleus.
# electrons:
Electrons: ____charge, mass =____,
0 are in
same as # protons.
For a neutral element it is the
the electron cloud.
Atomic Mass Unit (AMU): is the definition for what the mass of an atom is. AMU gives meaning to what 1
means in the periodic table. 1 AMU is the mass of Carbon-12 divided by 12
Ex: complete the table for the elements below:
Atom
Mass #
Atomic #
Protons +
Look in the
How do you
periodic table
calculate/find Neutrons
this?
59
27
Cobalt-59
Sulfur-32
32
Date: _________________________
16
# Protons
Same as atomic
#
# Neutrons
Mass – protons
# Electrons
Same as protons
in neutral atom
27
32
27
16
16
16
Page # ______
Notes Name: Ionic Structure
CHARGED ATOM
An ion is a __________________________.
Atoms will give up or loose electrons in order to have a stable
electron configuration like the noble gases.
CATIONS
+ charged atoms are called ________________
ANIONS
- charged atoms are called _____________
To find the number of electrons for a +
CATIONS
element (________________)
you
To find the number of electrons for a –
ANIONS
element (________________)
you ADD
SUBTRACT the charge from # protons.
the charge to the # protons
ex: Ca+1 = 20 -1 = 19 electrons
Ex: F-1 = 9+1 = 10 electrons
Notes Name: Atomic History
___________________:
all matter is made up of atoms
DEMOCRITUS
DALTON
___________________:
tiny solid ball theory, 3 Laws:
The Law of Conservation of Mass _______________________________________________________
THOMSON
___________________:
used cathode rays to discover the electron, Plum Pudding Model
___________________:
discovered the nucleus & protons, Planetary Model
RUTHERFORD
Rutherford’s Gold Foil Experiment: The atom has a small nucleus that has all the mass and a large
empty electron cloud around it.
BOHR
___________________: Energy Level Model
ELECTRON CLOUD current model, electrons orbit the nucleus is set pathways called orbitals.
___________________:
THEORY
Notes Name: Periodic Table Basics
The periodic table is made of groups (columns) and periods (rows). Elements in the same group have the
same: # valence e-, have same # of dots on a Lewis dot structure, have similar chemical properties
ATOMIC NUMBER
The periodic table is organized by increasing ___________________________.
Types of atoms:

DUCTILE
Metals: Groups 1-3 including the transition metals and lanthanides/ actinides. Are ________________,
malleable, will always give up an electron for a + charge

Non-Metals: Groups 4-7, exist as gases at room temperature, always ________________
an electron to
TAKE
get a – charge

STAIRS
Metalloids/Semi-Metals: Elements on the ________________.
Have properties of both metals and
non-metals
Date: _________________________
Page # ______
Notes Name: Valence Electrons & Noble Gas Configurations
Periodic law states:
ELEMENTS ARE ARRANGED
ACCORDING TO INCREASING
_________________________________
ATOMIC NUMBER
A valence electron is:
THE OUTERMOST S AND P
ELECTRONS. YOU CAN HAVE A
MAXIMUM OF 8 VALENCE
a. Germanium:_1s22s22p63s23p64s23d104p2____________________________________________
ELECTRONS
What are the configurations for:
b. Chlorine: __1s22s22p63s23p 5__(shown above in bubble diagram)
Group
Group 1:
Group 2:
Group 3:
Group 4:
Group 5:
Group 6:
Group 7:
Group 8:
Name
Alkali Metals
Alkaline Earth Metal
Boron Group
Carbon Group
Nitrogen Group
Oxygen Group,
Halogens
Noble gases
Date: _________________________
Charge
+1
+2
+3
+4 or -4
-3
-2
-1
no charge
e config
s1
s2
2 1
sp
s2 p 2
s2 p 3
s2 p 4
s2 p 5
s2 p 6
Valence e-/ dots
1
2
3
4
5
6
7
8
# e- available to bond
1
2
3
4
3
2
1
0
Page # ______
Notes Name: Periodic Trends
Ionization Energy:
FLOURINE has the highest
KEEP
The ability to ________________
electrons. ________________
FRANCIUM
ionization energy and therefore will not give away any electrons. ________________
has the lowest
ionization energy and will therefore give up an electron to any element.
DOWN
LEFT
a. Ionization Energy decreases as you travel ________________ and to the ______________
IF THEY LOSE 1 ELECTRON THEY HAVE
b. Why are the alkali metals so reactive? ________________________________________________
NOBLE GAS CONFIGURATION
Electronegativity:
TAKE
FLOURINE
The ability to ________________ electrons. ________________ has the highest
electronegativity and will therefore take electrons from any element (other than noble gases).
________________
FRANCIUM
has the lowest electronegativity and therefore cannot take an electron from any
element.
DOWN
LEFT
a. Electronegativity decreases as you travel ________________ and to the ______________
b. Why are the halogens so reactive?
Atomic Size/Radii:
IF THEY TAKE 1 ELECTRON THEY HAVE
________________________________________________
NOBLE GAS CONFIGURATION
FRANCIUM
How big the atom is. ________________
has the largest atomic size and radius. As you
AS YOU ADD MORE ELECTRONS
travel towards the noble gases, atomic radii gets smaller because_______________________________.
THEY GET PULLED CLOSER TO
THE ATTRACTIVE NUCLEUS
UP
RIGHT
a. Atomic size/radii decreases as you travel ________________
and to the ______________
Notes Name: Spectra
When you put metals in a flame, the flame will glow a specific color, depending on the metal.
Excited valence electrons will jump out of their orbital and into a higher energy orbital. When they calm down
PHOTON
and go back to where they belong, they release a ________________
which is a ray of light.
If you look at the emission spectra of an element, it will show you the photons of light the atoms give off. The
EMISSION SPECTRA
__________________________ is like a fingerprint of the element.
Date: _________________________
Page # ______
Standard 11 Nuclear Chemistry Notes



Date
Chemical Reactions vs. Nuclear Reactions
Chemical reactions:
Nuclear reaction:
happen because of changes in _number of
 happen because of changes in the nucleus
electrons
(either the protons or neutrons)
Stable atoms go through chemical reactions
 __Unstable___________ atoms go through
Small amounts of energy released (think of the
nuclear reactions until they becomes stable
heater in the classroom)

99% of chemistry involves chemical reactions

Follow the Law of Conservation of Mass
and Energy, which states you must have the
again



same number of the same atoms on BOTH
sides of the equation

2KClO3 → 2KCl + 3O2
K, Cl, and O on BOTH sides

LARGE amounts of energy released (think of
the sun or a nuclear bomb)
The 1% exception to the rule
Partially follows the Law of Conservation of
Mass and Energy, you must make sure that
the mass on both sides of the reaction are the
same. Violates the energy part!
40
40
0
19
20
1
K
 Ca 
Isotopes
Isotopes are the same element, but they have a different number of ___neutrons__________. Isotopes will
always have the _____same________ number of protons.
Ex: All isotopes of Carbon will have the same number of:
a. neutrons
b. electrons
c. protons
Stability Graphs
Not all isotopes of an element are radioactive. To be radioactive, the isotope must be unstable. To be
radioactive, the atom must have either too many neutrons or not enough neutrons. There are 2 ways to
determine if an isotope is unstable:
1. Use a stability curve:
a.
This is the most _____accurate________way to
determine if an isotope if radioactive. For your
element, plot the # neutrons against the # of protons.
b.
If element is ___on__________ the curved band of
stability, then it is stable.
c.
If the element is ___above__________ or
___below__________ the band, then it is unstable
and radioactive.
Ex: is the isotope Cobalt-111 stable?
____no_______
2. Calculate the # neutrons : # protons ratio. You should
do this __calculation___________ if you are not
provided with a stability graph. (Study tip: Neutrons
come before Protons because N is before P)
a. For elements #1-20: If the #neutrons :
#protons is 1:1 the isotope is stable.
b. For elements #21-82: If the #neutrons : # protons is 1:1½ , then the isotope is stable.
c. For elements # 83 and above: the isotope is always unstable and radioactive.
Date: _________________________
Page # ______
Radiation & Nuclear Reactions
__Radiation___________ is the matter and energy emitted from the
nucleus of an unstable isotope. (Think of it as the crazy cat lady
throwing her cats out!)
There are 3 types of nuclear reactions:
Type
Alpha
Symbol
4
2 He
Beta
0
1
gamma
 or
0
0
0
1
Blocked By
Paper
e
Aluminum foil
Heavy lead, concrete
Isotopes will continue to go through nuclear decay until they reach a
_____________ isotope.
For each reaction below, determine if is an alpha, beta, or gamma reaction.
a.
b.
14
14
0
233
229
6
7
1
93
91
Np* Pa 24He  00
C N  B
c.
210
84
4
Po206
Pb

82
2 He
For each reaction below, determine what the missing isotope is:
a.
40
19
K  Ca 
40
20
264
c.
84
Po
0
β
-1
b.
U  Ca   
238
92
40
20
0
0
198
72
Hf
4
260
Ca

82
2 He
Date: _________________________
Page # ______
Balancing Reactions Notes
According to the Law of Conservation of Mass and Energy, matter and energy cannot be created or
destroyed. We must account for this fact when we are writing equations.
# Atoms of Each element & Energy → # Atoms of Each element & Energy
To balance chemical reactions:
1.
Calculate the number of each atom on both sides of the reaction by multiplying the
coefficient by the subscript for each element.
a. If the same polyatomic appears in both the reactants and the products, you may balance
the polyatomic as one item. If the polyatomic breaks up, you have to balance each
element separately.
2.
You may use coefficients to balance the reactions. Coefficients go in front of the formula and
multiply each atom in the formula. You cannot change any subscripts. You cannot
change, add, or subtract anything from the reactions to balance them.
Ex: 4 KNO3 How many K? ____4_______ N?_____4_______ O?________12_______
3.
When you think that you have balanced the reaction, look at the coefficients. If all of the
coefficients can be reduced, then do so.
Helpful hint: If something does not balance, odd numbers will never work. Try multiplying
the odd number by 2 to make it even!
Examples:
___2__NH4OH(s) + _____LiS(s) → _____Li(OH)2 (s) + _____ (NH4)2S (s)
___2__ZnS + __3___O2 →___2__ ZnO +___2__ SO2
Molecular Mass Notes
In the beginning of the year, we used the periodic table to determine the atomic mass. To review,
find the atomic masses for the following:
a. H ____1.01_______ b. Cu ___63.55________
c. F _____19______ d. Cl ___35.45_____
Molecular mass is the mass of a molecule. To find the molecular mass, you add up the atomic masses
for every atom in a molecule. In our class, we will only use whole numbers (no decimals!!)
1. Write the formula.
2. Substitute the atomic mass for the atomic symbol. When you move from symbol to
symbol, ADD the masses.
3. Use the order of operations to solve. (PEMDAS)
Ex1: What is the molecular mass of NaCN? 49.01g/mol Ex2: What is the molecular mass of
F2O? 35g/mol
Ex3: What is the molar mass of Sr(OH)2? 121.64g/mol Ex4: What is the molar mass of
Ga2(CO3)2 189.7 g/mol
Mole Maps
Date: _________________________
Page # ______
For a chemist, the mole is the universal translator, meaning that we can translate from one unit to another, if we
first use moles. When a mole problem does not have moles in it, you must first convert to moles, then convert
to what the problem tells you to.
Conversion factors:
1 mole = 6.02 x 1023 atoms/molecules
1 mole = 22.4 L
1 mole = molecular mass grams
FOR THE REMAINDER OF STOICHIOMETRY,
PLEASE REVIEW THE PRACTICE PROBLEMS I
HAVE ATTACHED. FOR MORE STOICHIOMETRY
PRACTICE, PLEASE REFER TO THE EXAM 5 TAB
ON MY TEACHER SITE.
Page # 8