Download Matter and Atomic Structure Lesson 8

Ch 3 Matter and Atomic Structure
Lesson 1
Atoms
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes: Your teacher will give you notes on atoms.
Directed Reading:
1.
Skip to the Directed Reading.
Read pp. 53-57. Answer the following questions.
What is an element? _______________________________________________
_______________________________________________________________
2. How many elements occur naturally on Earth and in the stars? ________________
3. What is an atom? _________________________________________________
_______________________________________________________________
4. Where is the nucleus of an atom? _____________________________________
5. The Parts of an Atom: Fill in the Chart …
Subatomic
Particle
1. Proton
2. Neutron
3. Electron
Where in the atom is
it?
What type of charge
does it have?
Does it have mass?
6. Define: atomic number. _____________________________________________
7. Define: atomic mass. ______________________________________________
8. FITB: Atomic number = the number of _____________ = the number of electrons
9. What are valence electrons? _________________________________________
10. A Hydrogen Atom: Look at Figure 3-1 on page 56. Draw and label Part A and copy
its caption below.
Picture of Hydrogen
Caption
11. An Oxygen Atom: Look at Figure 3-1 on page 56. Draw and label Part B and copy its
caption below.
Picture of Oxygen
Caption
12. An Aluminum Atom: Look at Figure 3-1 on page 56. Draw and label Part C and copy
its caption below.
Picture of Aluminum
Caption
Practice:
For each element … Fill in the information and draw it.
1. Helium
a. Atomic number - ______
b. Number of protons - ______
c. Number of electrons - _____
d. Atomic mass - ______
e. Number of neutrons – ______
2. Lithium
a.
b.
c.
d.
e.
Atomic number - ______
Number of protons - ______
Number of electrons - _____
Atomic mass - ______
Number of neutrons – ______
( ______
Atomic mass
( ______
Atomic mass
-
minus
-
______ )
atomic number
______ )
minus
atomic number
-
______ )
3. Nitrogen
a.
b.
c.
d.
e.
Atomic number - ______
Number of protons - ______
Number of electrons - _____
Atomic mass - ______
Number of neutrons – _____
( ______
Atomic mass
minus
atomic number
Ch 3 Matter and Atomic Structure
Lesson 2
Elements and the Periodic Table
Name: ____________________________ Date: _____________ Period: _____
Focus Question: __________________________________________________
______________________________________________________________
Notes:
Directed Reading:
1.
2.
3.
4.
5.
Read pp. 58-59. Answer the following questions.
What is an isotope?
__________________________________________________
Give an example of isotopes.
_______________________________________________________________
What is atomic mass?
_______________________________________________________________
What is radioactivity?
_______________________________________________________________
Draw and label Figure 3-3. Write the caption.
The Periodic Table
Draw Figure 3-4. You do not need to write the caption.
Abundance of Elements
Review:
1.
What are the two most common elements of the universe? (List percentages.)
_______________________________________________________________
2. What are the two most common elements of the Earth’s crust? (List percentages.)
_______________________________________________________________
3. List the other 6 elements that are prevalent in Earth’s crust.
a. ___________________
b. ___________________
c. ___________________
d. ___________________
e. ___________________
f. ___________________
4. Look at p. 917. Pick three elements that prevalent in Earth’s crust and draw their
information inside the “boxes” below.
Ch 3 Matter and Atomic Structure
Lesson 3
Covalent Bonds
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes:
Directed Reading:
Read pages 60-62. Answer the following questions.
1. What is a compound? _________________________________________
_________________________________________________________
2. What is a chemical bond? _____________________________________
_________________________________________________________
3. What is a covalent bond? ______________________________________
_________________________________________________________
4. What is a molecule? __________________________________________
_________________________________________________________
5. FITB: Polar Bonds p. 62 - When atoms in a covalent bond do not share
electrons equally, they form _______________________ bonds. A polar
bond has a ________________ and a ________________ end.
6. The Formation of a Water Molecule. Draw Figure 3-6 below (NEATLY,
please!). Label the two hydrogen atoms, the oxygen atom, and the water
molecule.
The Formation of a Water Molecule
7. A Polar Molecule. Draw and label Figure 3-7 below. Write the caption in
the box next to your picture.
A Polar Molecule
Practice:
Caption
Show the covalent bonding of one hydrogen atom to another hydrogen
atom to make a hydrogen molecule (which is how hydrogen gas exists in nature).
Remember: Hydrogen has an atomic number of 1. Draw protons and electrons only.
Ch 3 Matter and Atomic Structure
Lesson 4
Ionic Bonds
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes:
Directed Reading:
Read pages 62-63. Answer the following questions.
1. What is an ion? _____________________________________________
2. FITB: Ions- p. 62.
a. An atom in which the outermost energy level is less than half-full
tends to _____________ its valence electrons to become a
_____________________ ion.
An example of this is a sodium ion. Write the symbol for a sodium
ion: ________. Then draw it in the box below.
Positive Sodium Ion
b. An atom in which the outermost energy level is more than half-full
tends to fill its outermost energy level by _________________ one
or more needed electrons to become a _____________________
ion.
An example of this is a chlorine ion. Write the symbol for a chlorine
ion: ________. Then draw it in the box below.
Negative Chlorine Ion
c. An atom in which the outermost energy level is exactly half full may
form either a ______________ or _________________ ion.
An example of this is a silicate ion. Write the symbol for a silicate
ion: _______________
3. What is an ionic bond?
_________________________________________________________
Practice:
Draw the NaCl only of Figure 3-8.
NaCl
Ch 3 Matter and Atomic Structure
Lesson 5
Metallic Bonds
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes:
Directed Reading:
Read pages 64. Fill in the Blanks …
1. Most compounds on Earth are held together by _____________ or
_____________ bonds.
2. In METALS, the _______________ electrons are shared by all the atoms.
3. You could think of a METAL as a group of positive __________ floating in a
sea of ________________ electrons.
4. The positive ions of the METAL are held together by the
________________ ________________ between them.
5. A METALLIC bond allows METALS to conduct ____________________
because the ________________ can move freely throughout the entire
solid metal.
Ch 3 Matter and Atomic Structure
Lesson 6
Chemical Reactions
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes:
Directed Reading:
1.
Read page 64.
Remember that atoms gain, lose, or share electrons to become more
_______________________.
2. What is a chemical reaction?
_________________________________________________________
3. FITB: Chemical reactions are described by chemical _________________.
4. FITB: You must balance an equation by showing an ___________________ number
of atoms for each element on each side of an equation.
This is because
the same amount of matter is present both before and ___________________
the reaction.
Practice:
Practice writing the following equations. Be sure to balance them!
A. Iron (Fe) combines with oxygen (O2) to yield rust (FE2O2).
B. Hydrogen (H2) combines with oxygen (O2) to yield water (H2O).
C. Carbon (C ) combines with oxygen (O2) to yield carbon dioxide (CO2).
Ch 3 Matter and Atomic Structure
Lesson 7
Mixtures and Solutions
Name: _________________________ Date: ________________ Period: ___________
Focus Question: ________________________________________________________
____________________________________________________________________
Notes:
Directed Reading:
Read page 65.
1.
What is a mixture?
_________________________________________________________
2.
FITB: When a mixture’s components are easily recognizable, it is called a
__________________________ mixture.
3. Why is soil a heterogeneous mixture? (That is, what does it consist of?)
_______________________________________________________________
___________________________________________________
4. FITB: In a _______________________ mixture, the component particles cannot
be distinguished.
5. A homogeneous mixture is also called a _________________________.
6. Examples of solutions …
Type of Solution
Example
Solid
Liquid
Gas
Matter and Atomic Structure
Lesson 8
States of Matter
Name: ______________________________ Date: ___________ Period: _____
Notes:
Read and Draw:
Read page 67-69.
A. FITB: Solids …
1.
A solid is a substance with densely _________________ particles.
2. Most solids have a _________________________ structure.
3. Crystals form symmetrical solid objects with ____________________faces
and ___________________ edges between faces.
4. A glass is a solid that consists of densely packed atoms arranged at
_______________________. Glasses form when molten material is chilled so
rapidly that atoms cannot arrange themselves into a regular
___________________.
5. Draw the (solid) crystals of Figure 3-12 and write the caption.
Table Salt Crystals
Vanadium Crystals
Caption
B. FITB: Liquids …
1.
When the particles of a substance can slide past each other, the substance
becomes _______________________.
2. Liquids do not have their own ________________ but take the shape of the
container they are placed in.
3. Liquids do have a definite _______________________.
C . FITB: Gases …
1.
In gases, the particles are separated by relatively _______________
distances and move about at extremely ________________ speeds.
2. Gases have no definite ________________ and no definite
____________________.
D. Changes of State…
1.
What is melting?
_________________________________________________________
2.
E. What is evaporation?
_________________________________________________________
F. What is sublimation?
_________________________________________________________
G. What is condensation?
_________________________________________________________
5. FITB: Plasma …
Plasma occurs when temperatures exceed _________ degrees C. The
collisions between particles are so violent that ______________ are
knocked away from atoms. Three examples of plasma include:
______________, ______________, and ___________________.