When Atoms Change…. What we KNOW… Atoms on the periodic table are neutral. Atoms are neutral...
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![Page 1: When Atoms Change…. What we KNOW… Atoms on the periodic table are neutral. Atoms are neutral because they have the same number of protons as electrons.](https://reader035.fdocuments.net/reader035/viewer/2022062407/56649e165503460f94b00396/html5/thumbnails/1.jpg)
When Atoms
Change…
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What we KNOW…
• Atoms on the periodic table are neutral.
• Atoms are neutral because they have the same number of protons as electrons.
• protons have a positive charge.
• neutrons have no charge.• electrons have a negative charge.
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What we Also need to KNOW…
• The identity of an atom is determined ONLY by the number of protons.
• For example… If I tell you there is an atom with 3 protons… you know it’s a Lithium atom.
• What about 8 protons, 13 protons, 79 protons???
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What happens if the number of neutrons
change???If an atom gains Neutrons…1. The mass increases by 1 for every neutron added. 2. The charge remains neutral. (Neutrons don’t have
a charge.) 3. The number of protons and electrons stay the
same.
If an atom loses Neutrons…1. The mass decreases by 1 for every neutron taken
away. 2. The charge remains neutral. (Neutrons don’t
have a charge.)3. The number of protons and electrons stay the
same.
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What happens if the number of neutrons
change???If an atom gains Neutrons…1. The mass increases by 1 for every neutron
added. 2. The charge remains neutral. (Neutrons don’t have
a charge.) 3. The number of protons and electrons stay the
same.
If an atom loses Neutrons…1. The mass decreases by 1 for every neutron
taken away. 2. The charge remains neutral. (Neutrons don’t
have a charge.)3. The number of protons and electrons stay the
same.
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The atom is now called an ISOTOPE!
When atoms gain or lose neutrons!
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ISOTOPE EXAMPLE
Hydrogen AtomHas a mass of 1 and an atomic number of 1
Hydrogen Isotope
Has a mass of 2 and an atomic number of 1
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ISOTOPE NOTATION
We communicate that we have an isotope by using the Atomic Symbol of the isotope followed by the “NEW” mass number.
ISOTOPE NOTATION Li-7Ex: An Isotope of Lithium is:
Li - 6
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Isotope INVENTORY
Completing a particle inventory for an Isotope is almost the same as the neutral atom EXCEPT we USE THE “NEW” MASS NUMBER to calculate neutrons.
Ex: Li-63p+ (since it’s Lithium!!!)3e- (since they are still equal to p+)3n
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Isotope Practice• Ca atom has a mass of 40.• The isotopes for Ca are: • Ca-42, Ca-43,Ca-44, Ca-46, & Ca-
48.• 1.) How many neutrons are in a Ca
atom and each of its isotopes?
2.) What are the differences and similarities between the Ca atom and its isotopes?
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Isotope PracticeCa atom has a mass of 40. (atomic # =20)The isotopes for Ca have masses of 42,43,44,46, & 48.
1.) How many neutrons are in a Ca atom and each of its isotopes?
(Ca ATOM: 40 – 20 = 20n)(ISOTOPES: 42-20=22n, 43-20=23n, 44-20=24n, 46-20=26n, 48-20=28n)2.) What are the differences and similarities between
the Ca atom and its isotopes? Similarities Differences
(All have 20 p+ all have 20 e- all neutral
all are Calcium)
(The # of neutrons is different, masses are all different.)
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• Everyone gets 7 blue, 7 red, 7 yellow• Red = Protons• Blue = Neutrons• Yellow = Electrons• Play 1-5 marbles per turn.
Number of neutrons and protons
Number of protons and electrons
Subtract the two to find the number of neutrons
The Atom Building Game
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Everyday Uses of IsotopesSmoke Detectors and Americium-241
What most consumers don't know is that many of these units contain a small amount of americium-241. By utilizing the radioactive properties of this material, smoke from a fire can be detected at a very early stage. This early warning capability has saved many lives. In fact, studies have shown that 80% of fire injuries and 80% of fire fatalities occur in homes without smoke detectors.
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Carbon-14 DatingRecalling that all biologic organisms contain a given
concentration of carbon-14, we can use this information to help solve questions about when
the organism died. When an organism dies it has a specific ratio by mass of carbon-14 to carbon-12
incorporated in the cells of it's body. At the moment of death, no new carbon-14 containing molecules are metabolized, therefore the ratio is
at a maximum. After death, the carbon-14 to carbon-12 ratio begins to decrease because carbon-14 is decaying away at a constant and predictable rate. Remembering that the half-life of carbon-14 is 5700 years, then after 5700 years half as much carbon-14 remains within the organism.
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Food Irradiation
Food irradiated by exposing it to the gamma rays of a radioisotope -- one that is widely used is cobalt-60. The gamma rays pass through the food to destroy many disease-causing bacteria as well as those that cause food to spoil. It’s not strong enough to change the quality, flavor or texture of the food. The food never comes in contact with the radioisotope and is never at risk of becoming radioactive!
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Reviewing IsotopesWhat are isotopes gaining or losing?
Here is an Atom of Oxygen (how many neutrons?)
Atomic Mass=16 These are isotopes of Oxygen
O-17 O-18
So…How many neutrons does each isotope of Oxygen NOW have?
8 neutrons
Neutrons!
10N9N
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Isotope Practice
1.)How many neutrons are in each of Zinc’s isotopes? Zn-65
Zn-64____ Zn-67_____ Zn-70____
2.) What are the differences and similarities between the Zn atom and its isotopes? Set-up a “T” Chart
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Isotope Practice
1.)How many neutrons are in each of Zinc’s isotopes? Zn-65
Zn-64____ Zn-67_____ Zn-70____
2.) What are the differences and similarities between the Zn atom and its isotopes?
34 4037
Similarities Differences
• All have 30 p+ all have 30 e-
• all neutral • all are Zinc
• # of neutrons is different• masses are all different
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Isotope Warm up
1.)How many neutrons are in each of Strontium’s isotopes?
Sr-84____ Sr-86_____ Sr-87____
Answers:Sr-84 46Sr-86 48Sr-87 49
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Quiz QuickIsotopes gain or lose…
A. electronsB. protonsC. neutronsD. nuclei
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When an atom gains neutrons, its charge
changes.A. TrueB. False
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When an atom gains neutrons, the number of protons and electrons do
not change.A. TrueB. False
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The only subatomic particles that never change
are…A. Valance
electronsB. ProtonsC. ElectronsD. Neutrons
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What happens if the number of electrons
change???If an atom gains electrons…1. The charge becomes negative. (There are more
negative e- than positive p+ now!)2. The mass stays the same (electron’s mass = 0). 3. The number of protons and neutrons stays the
same.
If an atom loses electrons…1. The charge becomes positive. (There are less
negative e- than positive p+ now!)2. The mass stays the same (electron’s mass =0).3. The number of protons and neutrons stays the
same.
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What happens if the number of electrons
change???If an atom gains electrons…1. The charge becomes negative. (There are
more negative e- than positive p+ now!)2. The mass stays the same (electron’s mass = 0). 3. The number of protons and neutrons stays the
same.
If an atom loses electrons…1. The charge becomes positive. (There are
less negative e- than positive p+ now!)2. The mass stays the same (electron’s mass =0).3. The number of protons and neutrons stays the
same.
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The atom is now called an ION!!!
When atoms gain or lose electrons!
*Ions are charged particles!Ions form so that unstable atoms can bond with other unstable elements to become a stable
substance!
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Charged Ions
Anion (-) Negatively charged ion.
Cation (+) Positively charged ion
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Quick QuizIf an atom loses electrons,
its mass changes?A. TrueB. False
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Ions gain or lose…
A. isotopesB. protonsC. neutronsD. electrons
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Gaining electrons causes atoms to…
A. Gain more mass
B. Have a chargeC. Stay neutralD. Lose mass
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ION EXAMPLE
H+ is a positive
hydrogen ION
H: Is the neutral
hydrogen atom
H- : is a negative hydrogen
ION
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Ion PracticeNaBeI
CaSbSPC
Na+1
Be+2
I-1 Ca+2
Sb-3
S-2
P-3
C+/-4
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Ion Worksheet AnswersLi +1
Br -1
Mg +2
B+3
F -1
N -3
Cl -1
K +1
Ba +2
Te -2
Sn -4
As -3
Si +/-4
O -2
Al+3
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Ion Worksheet ColoringLi +1
Br -1
Mg +2
B+3
F -1
N -3
Cl -1
K +1
Ba +2
Te -2
Sn -4
As -3
Si +/-4
O -2
Al+3
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What patterns did you notice from coloring your ions on the periodic
table? *hint* there is more than one!
• The families where the same color.• The families had the same ionic
charge.• Metals have a positive charge.• Non-metals have a negative charge.• Metals lose electrons.• Non-metals gain electrons.
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PracticeDraw the Bohr models for the following elements and find the ionic charges for each.
RbSrBi
Rb
Sr
Bi-3
+2
+1
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How is the neutral(no charge) atom Se and it’s isotope Se-78
similar and different?(Set up a “T” chart)
SimilarSame element
Same # of protonsSame # of electrons
Same charges
DifferentDifferent masses
Different # of neutrons
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How are isotopes and ions similar and different? (setup a T chart)
(hint* think about particles, masses and charges) Similarities
Same number ofprotons only!
DifferencesDiff Masses
Diff Number ofneutrons
Diff ChargesDiff Number of
electrons
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PracticeDraw the Bohr models for the following elements and find the ionic charges for each.
GaSrPb
Ga
Sr
Pb-4
+2
-5
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Patterns on the
Periodic Table
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+1
+2
+3
+/-4 -3 -1-2
0
Ionic Charg
es
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Valence Electron
s
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1 Shell
3 Shells
4 Shells
5 Shells
6 Shells
7 Shells
2 Shells
Period 1
Period 2
Period 4
Period 3
Period 5
Period 6
Period 7
Energy Shells of Atoms
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Families/Groups have a lot in common…
• We now know that elements in a group all have the same # of valence e-.
• We also now know they all form ions with the same charge.
• But…there are a lot of other properties that elements in a family also share!
• Such as…Atomic Width, Ionization Energy, Electronegativity and reactivity.
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Atomic Radius (Width)• Atomic radius is simply the radius (width) of the
atom, an indication of the atom's volume. • Periods - atomic radius decreases as you go
from left to right across a period. • Why?• Stronger attractive forces in atoms (as you go
from left to right) between the opposite charges in the nucleus and electron cloud cause the atom to be 'sucked' together a little tighter.
• Largest atomic species are those found in the SW corner of the periodic table.
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Atomic Radius (Width)• Groups - atomic radius increases as you
go down a group. • Why? • There is a significant jump in the size of
the nucleus (protons + neutrons) each time you move from period to period down a group. Additionally, new energy levels of elections clouds are added to the atom as you move from period to period down a group, making the each atom significantly more massive, both is mass and volume.
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Ionization Energy
• Ionization energy is the amount of energy required to remove the outmost electron. It is closely related to electronegativity.
• Group - ionization energy decreases as you go down a group.
• Why? • The shielding affect makes it easier to
remove the outer most electrons from those atoms that have many electrons (those near the bottom of the chart).
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Electronegativity• Electronegativity is an atom's 'desire' to grab
another atom's electrons. • Period - electronegativity increases as you go
from left to right across a period. • Why? • Elements on the left of the period table have 1
-2 valence electrons and would rather give those few valence electrons away, as a result, they have low electronegativity.
• Elements on the right side of the period table only need a few electrons, so they have strong desire to grab another atom's electrons.
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Electronegativity
• Electronegativity is an atom's 'desire' to grab another atom's electrons.
• Group - electronegativity decreases as you go down a group.
• Why? • Elements near the top of the period table
have few electrons to begin with; every electron is a big deal. They have a stronger desire to acquire more electrons. Elements near the bottom of the chart have so many electrons that loosing or acquiring an electron is not as big a deal.
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Reactivity• Elements become more reactive as
you go down a group on the left side • And more reactive as you go up a group
on the right side!
• Reactivity refers to how likely or vigorously an atom is to react with other substances.
• Based on this, where are the most reactive elements found on the periodic table?
Bottom left corner (Fr) and top right corner (F)
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What are (7) things you can now predict about the element Iodine (I),
based on where it is located on the Periodic Table?
1. It has 7 valence electrons2. It has 5 energy rings/shells3. It is a non-metal4. It’s gaining 1 electron5. It’s ionic charge is -16. Less reactive than Br and Cl7. But it’s more massive than Br
and Cl
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Properties of Non-metals
• No luster• Brittle• Not ductile • Not malleable
(dull)
(breaks easily)
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What can you now tell me about the element Nitrogen (N) and
Potassium (K), based on where they are located on the Periodic Table?
(think about shells, valence e’s, charges, metal/non-metal, gaining/losing e’s)
Potassium
• 1 valence electron• It has 4 energy rings• It is a metal• It’s losing 1 electron• It’s ionic charge is +1
Nitrogen•5 valence electrons
•It has 2 energy rings
•It is a non-metal•It’s gaining 2
electrons•It’s ionic charge is -
3
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You are the bus driver. At your first stop, you pick up 29 people. On your second stop, 18 of those 29 people get off, and at the same time 10 new passengers arrive. At your next stop, 3 of those 10 passengers get off, and 13 new passengers come on. On your fourth stop 4 of the remaining 10 passengers get off, 6 of those new 13 passengers get off as well, then 17 new passengers get on. What is the color of the bus driver's eyes?