Download Unit 4 Notepack

Unit 4 Atomic Structure, Periodic
Table, Matter, and Chemical Equations
I.
Name:_________________________________
Period:___
Atomic Structure:
A. ___________Atomic Theory.
a. All matter is made of ____________
b. Atoms are ________________and cannot be divided into ___________________
c. Atoms of one element are __________________, but they are _______________
from atoms of other ________________
B. Subatomic Particles: Actually means ______________ atom.
1. Electrons: This is what makes elements____________________________.
a. Located __________________________________________.
b. Charge is ____________________________.
c. Electrons __________________so they can___________________________.
d. Have no ________________________
e. Exist at different______________. The number of ______________can be
found by looking at ____________________________the element
f. The only electrons that can bond with other atoms are the _________________
______________. Called ____________________________.
2. Protons: Protons make elements _______________________ because their positive
charge controls the _______ attractions of an atom, thus controlling it’s ______________
a. Located in the ______________.
b. Charge is ______________.
c. Found on periodic table by looking at the ___________________of an element.
d. Has a mass of __________________________________________
Carbon
12.01
Example: Potassium has how many protons? ___________
Potassium (K) has how many electrons? ______________
Potassium has how many energy levels? _____________
Diagram here:
K has how many outer electrons for bonding? _____________
3. Neutrons: This is what adds to the ______________of an atom.
a. Located in the ______________
b. Charge is ______________
d. Total mass of an atom from the _______________ and the ________________
4. Isotopes: All atoms of an element have same number of______________ . But, in
nature, some atoms of the same element have different numbers of______________,
they are called different______________. This causes their masses to be different.
Diagram of Neon-20 and Neon 22
b. When reading the periodic table _________, round to the nearest ___________
number to find the most ______________________________ for that element.
Q: How many protons, neutrons, electrons are in the most common isotope of potassium?
How many protons, neutrons, electrons are in the most common isotope of aluminum?
Obj. 1: Fill in the grid below for each subatomic particle.
Location in atom
Protons
Neutrons
Electrons
Symbol
Charge
Mass
Obj. 2: Directions: Complete the table for the following isotopes of each element:
Element Symbo Number of Number of Number of Atomic
Mass
l
Protons
Electrons Neutrons
Number
Number
Sodium
13
47
97
4
Valence
Electrons
X
5
F
19
II. Obj. 3: Bohr Models: Uses ______________to show the energy levels. The number of
rings should match the ______________of that element. This model
is________________________.
1. ______________mass of all the isotopes found in nature = _______________.
2. The protons in the nucleus are found by looking at the______________.
3. The neutrons plus the protons must add up to______________.
4. The electrons fill the shells from ______________until they match the number of
______________. They fill in the following order ______________
a. You can check you outer electrons to make sure they match the _____________
b. This model can only be used for the first 20 atoms. After that it ____________
i.e. Calcium 44
i.e. lithium 7
Obj. 3: Draw Bohr Models for the following Isotopes. Include…

# of Electrons in correct rings, # of Protons in nucleus # of Neutrons in nucleus
Sulfur 34
Boron 10
Helium 3
Sulfur 32
Boron 14
Helium 4
III. Obj. 4: Classifying matter
A. Matter: Anything that has _______and ______________.
B. Pure Substances: Matter that has fixed _______ _______ and definite _______ _______. Cannot be
broken down by _______ _______ means.
a. Element: a substance that cannot be __________________________________________
by chemical means.
i.e.
b. Compound: a substance made of __________________________________________
that are chemically combined.
1. Every compound is _____________ _ from the__________ ____ that it contains.
i.e. Water: H2O
Physical Properties:
Chemical Properties:
Hydrogen: H2
Oxygen: O2
Physical Properties:
Physical Properties:
Chemical Properties:
Chemical Properties:
2. Chemical formula: Shows the _______ _______ _______ in a compound. It also shows
_______ _______ _______ _______ _______ _______ are in the compound.
try 4 Ca(ClO3)2
c. Mixtures: Matter that has compositions that are not_______or _____________________.
Mixtures can be separated by _____________________into the _____________________that are
mixed w/in them.
1. Homogeneous Mixture: (homo = ______)The composition is the_____throughout.
a. Homogeneous Mixture Examples. Something must be ________________________ in order
to be truly ____________________.
b. If something is dissolved in water, we call it _____________________ and label it ______.
_______, ____________, & ____________ are always aqueous.
1) Solid  Solid:
2) Liquid  Liquid:
3) Gas  Gas:
4) Solid (dissolves)  Liquid:
5) Gas (dissolves)  Liquid:
2. Heterogeneous Mixture: (Hetero = ______________) The composition is ______________ .
a. Anytime more than one ______________exists in a mixture, it is considered
heterogeneous b/c “___________” states of matter are of __________ composition.
Question: Which three types of matter will always “look” homogeneous? Why.
 Practice Problems
Hetero or Homo Mixture
1. Dish Soap:________________
Why?
2. A Rock: ________________
3. Stainless Steel:________________
4. Saltwater: ______________
5. Pen ink: _______________
6. An Egg: ________________
7. Dust Free Air: ________________
8. Rusty Nail: _________________
IV. Obj. 5: Reading trends in the Periodic Table (Ch 3.2)
A. ______________Go down, ______________pass across.
1. Tall groups tell you the number of ______________ electrons in that group.
2. Some common names for special groups
a. Group 1A: __________________________________________
b. Goup 2A: __________________________________________
c. Group 7A: ______________________________________________
d. Group 8A: ______________________________________________
3. Size (pgs. 256-257): Atoms get _____________ as you go down a Group, but
___________as you go to the right b/c more ______________________ in outer energy level.
4. The ___________identifies ___________to the left, ___________ to the right, and
___________ touch the ladder
a. Short groups are ___________metals, charges may change (are in transition)
b. To remember where metals and non-metals are, just______________________.
5. The ___________will tell you the number of______________________.
V. Obj. 6: Properties and Changes in Matter
A. Physical Change: Affects one or more ______________ properties of a substance w/o
____________________________. Chemical properties are ________________________.
i.e.
1. More on Dissolving. Two different substances visually become ___________________
2. Phase changes=
B. Chemical Changes: Occur when one or more substances are changed into ___________
____________________________ that have ____________________________.
i.e.
Chemical or Physical Property?
Chemical or Physical Change?
1. Tarnishes in Rain:_______________________
1. Lighting a firework: _____________________
2. Bends easily: _______________________
2. Boiling Pasta:_______________________
3. Decomposes: _______________________
3. Chewing gum: _______________________
4. Reusable/Recyclable: _______________________
4. Running your car: ______________________
5. Shiny______________________________
5. Rolling your bike: _______________________
6. Not Flammable: _______________________
6. Melting a crayon: _______________________
7. Perishable Food: _______________________
7. Rusting a nail: _______________________
8. Freezable Food: _______________________
8. Opening a can of pop: ____________________
Chemical equation: Describes the original beginning substances (called
chemical formulas. Then an arrow points to the newly created substances (called
(s) =
+=
(l) =
=
(g) =
∆=
(aq) =
H2 (subscripts) =
____
)
using
).
2 H2 = (Coefficients) =
Example:
VI. Obj. 7: Balancing Equations: The law of conservation of mass states that matter cannot be
________________ or _________________. So, the number of atoms reacting must equal the number of
atoms produces. However, a chemical change rearranges these atoms into new __________________.
To balance equations, follow these steps.
1. Count atoms on each side of_________. They should be _________. If not, you need to
_________them.
2. Balance both sides by using ____________. Remember, they multiply through everything inside of
that compound. NEVER change _________.
3. Double check work.
Try These
____ KClO3  ____ KCl + ____ O2
____AlBr3 + ____ K2SO4  ____ KBr + ____ Al2(SO4)3
____ C3H8 + ____ O2  ____ CO2 + ____ H2O
Examples from class demos and life examples. Balance as well.
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