Download Phy. Sci Mid-term review

Physical Science Mid-term Review
Name _____________________
Review for Chemistry Final
1.
Explain the steps in the scientific method.
2. Scientists use the metric system for measurement. What are the basic metric units for the following?
Length –
Volume Time Mass 3. List the values for 6 different prefixes.
4. All matter has both physical and chemical properties. Give 3 examples of physical properties.
5. What is a chemical property? Give an example.
6. Explain how to find the density of an object or a liquid.
7. A piece of wood has a mass of 2.0 grams and a volume of 6 cm3. What is the density of the wood?
Will the wood float on top of water or sink?
8. Define the 4 phases of matter
a) Draw a molecular interpretation of a solid changing to a liquid and then to a gas.
b) How much heat energy is needed to boil a 10.0 g piece of ice that has a temperature of – 30.0°C
9. Matter can undergo physical and chemical changes. Give 3 examples of physical changes.
10. Give 3 examples of chemical changes.
11. Describe the 3 classes that matter can be divided into and give 3 examples of each.
12. The law of conservation of mass states that matter cannot be made or destroyed by ordinary
chemical means. Explain what is meant by this statement.
13. Who is Democritus and what did he believe? How about the early Greeks?
14. John Dalton created an atomic theory in the early 1800’s. It has been slightly revised. Write down
the 5 parts of the modern atomic theory. Include the names and models of 5 scientist.
15. Describe the 3 basic particles found in the atom?
16. Draw a picture of the modern day atom.
17. Describe an isotope and give two examples.
18. Describe an ion and give two examples.
19. Fill in the following table. Use a periodic table
Remember: (atomic number = number of protons),
(number of electrons = number of protons), (mass number = number of protons + number of neutrons.)
Element
Symbol
Sodium
Atomic #
Mass #
11
23
Ar
Aluminum
13
Ion
Charge
+1
# of protons
# of neutrons
0
18
22
14
+3
27
32
127
Br
80
-1
# of electrons
25
53
36
20. Draw the Bohr diagrams for three of the elements in the above table. Change the third one into an
anion or cation that would be most appropriate for that element.
21.
Chemical bonds are forces that hold two or more atoms together. There are two types of
chemical bonds: ionic bonds and covalent bonds. Explain the difference between the two bonds.
22. Name the groups on the Periodic Table and describe how to predict valence e- # & Oxidation #
23. Using e-dot diagrams show the bonding structure for the following compounds and molecules
a.
Aluminum and Chlorine
b.
Hydrogen and Oxygen
c.
Calcium and Phosphorus
24. Choose three metals and 2 non-metal element and 1 negative poly-atomic ion. Using those 6 ions
create 9 different compounds list formulas and names.
25. Name the following formulas
a. Ni(NO3)3
b. BaS
c. NaC2H3O2
d. (NH4)3(PO4)
e. FeP
Study your notes know the major concepts and understand the connections between them.
Physical Science Mid-term ANSWERS
Name ______FSK____
Review for Chemistry Final
1.
Explain the steps in the scientific method.
1) Define the Problem 2) Hypothesis 3) Experiment 4) Draw Conclusions (Theory/Law) 5) Publish
(Report Results)
2. Scientists use the metric system for measurement. What are the basic metric units for the following?
Length – Meter
Volume - Liter
Time - Second
Mass - Kilogram
3. List the values for 6 different prefixes.
Micro = 1/1,000,000;
Deka – 10 ;
milli- 1/1000;
kilo 1000;
centi 1/100;
Mega – 1,000,000
4. All matter has both physical and chemical properties. Give 3 examples of physical properties.
Color, Mass, Density, Temperature, volume, texture ….
5. What is a chemical property? Give an example. A chemical property is a description of how a
substance reacts or relates to other substances. Ex: Flammable, reacts with acids, decomposes …
6. Explain how to find the density of an object or a liquid. D = mass/volume
7. A piece of wood has a mass of 2.0 grams and a volume of 6 cm3. What is the density of the wood?
Will the wood float on top of water or sink? D = m/v = (2.0 g)/6cm3 = 0.33 g/cc it will
float because its density is less then water’s 1.0 g/ml.
8. Define the 4 phases of matter Solid  liquid  gas  plasma increased motion and energy
a) Draw a molecular interpretation of a solid changing to a liquid and then to a gas.
Continue to break more and more intermolecular bonds till there are none in a gas.
b) How much heat energy is needed to boil a 10.0 g piece of ice that has a temperature of – 30.0°C
1) q = mCp∆T = (10.0 g)(4.184 J/g/C°)(30C) = J
2) q = mHf = (10.0g)(334J/g) = ___J
3) q = mCp∆T = (10.0 g)(4.184 J/g/C°)(100C) = J
4) q = mHv = (10.0g)(2260J/g) = ___J
9. Matter can undergo physical and chemical changes. Give 3 examples of physical changes.
Folding paper, squeezing water out of a sponge, freezing gasoline in the tank.
10. Give 3 examples of chemical changes.
Burning paper, pouring water on Sodium(explode), Eating a freezer pop.
11. Describe the 3 classes that matter can be divided into and give 3 examples of each.
Element  Lead,
Compound  Alcohol,
Solution  pen ink.,
Colloid  Mayo,
Suspension  house Paint, Solid mixture  Wood
12. The law of conservation of mass states that matter cannot be made or destroyed by ordinary
chemical means. Explain what is meant by this statement.
The mass you start with must be the same mass you finish with regardless of
the type of change the matter endures.
13. Who is Democritus and what did he believe? How about the early Greeks?
Coin the term “ATMOS” 1st to believe the concept of the atom.
14. John Dalton created an atomic theory in the early 1800’s. It has been slightly revised. Write down
the 5 parts of the modern atomic theory. Include the names and models of 5 scientist.
1) All matter is made of atoms that are in constant motion.
Dalton  Billiard Ball
2) Atoms are indivisible
Thompson  Plum Pudding
3) Atoms from different elements are different.
Rutherford  Nuclear Model
4) Atoms from the same elements are the same
Bohr  Planetary Model
5) Law of Multiple Proportions.
Heisenberg and Schrödinger  Modern Day Model
15. Describe the 3 basic particles found in the atom?
Proton  Positive charge mass of 1 amu
Electron  Negative charge mass of 0 amu
Neutron  No charge mass of 1 amu
16. Draw a picture of the modern day atom.
Should include, p.n.e, orbitals , energy levels, and nucleus
17. Describe an isotope and give two examples.
Element with different # of N Carbon-14 and Deuterium (H-2)
18. Describe an ion and give two examples.
Charged atom (different # e then P) Na+ Cation or Cl- anion
19. Fill in the following table. Use a periodic table Remember: (atomic number = number of protons),
(number of electrons = number of protons), (mass number = number of protons + number of neutrons.)
Element
Ion
Charge
+1
# of
protons
# of
neutrons
# of
electrons
11
12
0
18
22
+3
13
27
14
11
18
13
32
27
53
74
45
53
Symbol
Atomic #
Mass #
Na
11
23
Argon
Ar
18
Aluminum
Al
Co
I
13
40
27
59
127
-1
Sodium
Cobalt
Iodine
Bromine
27
53
35
Br
80
35
35
20. Draw the Bohr diagrams for three of the elements in the above table. Change the third one into an
anion or cation that would be most appropriate for that element. Al  +3 Draw
21.
Chemical bonds are forces that hold two or more atoms together. There are two types of
chemical bonds: ionic bonds and covalent bonds. Explain the difference between the two bonds.
Ionic bonds transfer e- from cation to anion :::
Covalent bonds is a sharing of electrons between two atoms
Ionic is metal to non-metal bonds
:::
Covalent bond are between to non-metals
22. Name the groups on the Periodic Table and describe how to predict valence e- # & Oxidation #
Outline of table with charges & e- listed.
23. Using e-dot diagrams show the bonding structure for the following compounds and molecules
d.
Aluminum and Chlorine
 AlCl3
e.
Hydrogen and Oxygen
 H2O
f.
Calcium and Phosphorus
 Ca3P2
24. Choose three metals and 2 non-metal element and 1 negative poly-atomic ion. Using those 6 ions
create 9 different compounds list formulas and names. Multiple Answers possible.
25.
a. Ni(NO3)3 Nickle(III) Nitrate
b. BaS
Barium Sulfide
c. NaC2H3O2 Sodium Acetate
d. (NH4)3(PO4)
e. FeP
Ammonium Phosphate
Iron(III) Phosphide