Download Fundamentals Fall Final Review

FUNDAMENTALS
Name: ____________________________ Period: ______
Fall Final Exam Review
UNIT 1: NATURE OF SCIENCE (SCIENTIFIC METHOD)
1. List and describe the steps of the scientific method.
2. Know the following terms and be able to identify them in a scenario: hypothesis, control, independent
variable, and dependent variable.
Read the following passage and answer the questions that follow (#3-6):
After reading cooking instructions that said to add salt to water before boiling it, Jade guessed that adding salt
must make the water boil at a higher temperature. She decided to test her idea by performing the following
experiment.
Jade measured out 1 quart of water and added 2 tablespoons of salt. She then brought the water to a boil
and measured its maximum temperature. Jade ran two more trials using 2 tablespoons of salt. She then ran 3
trials each with 4 tablespoons of salt and 6 tablespoon of salt. For each trial, Jade used 1 quart of distilled
water and the same pot and stove. The average temperature for 2 tablespoons of salt was 102.7°C. The
average temperature for 4 tablespoons of salt was 105.4°C. The average temperature for 6 tablespoons of salt
was 107.1°C. Since Jade knew that the boiling point of water is 100°C, she concluded that adding salt to water
does cause it to boil at a higher temperature.
3. What was Jade’s hypothesis?
4. What was Jade’s conclusion?
5. What were the independent and dependent variables in the experiment?
6. Construct a table that shows amount of salt and the corresponding average temperature.
MEASUREMENTS AND METRICS
SOLVE THE FOLLOWING DENSITY PROBLEMS:
7. Limestone has a density of 2.72 g/cm3. What is the mass of 24.9 cm3 of limestone?
8. What is the volume of a tank that holds 595 g of methanol if the density of methanol is 0.788 g/cm3?
PERFORM THE FOLLOWING SI PREFIX CONVERSIONS:
9.
84 g = _
mg
10. 177 mL = ____ L
11. 56 m =
_____ cm
12. 0.093 kg = ____
mg
13. What is the metric unit (SI Unit) and what instrument would you use to measure each of the following:
Length, Volume, Mass.
UNIT 2: INTRODUCTION TO MATTER
1. What is chemistry?
2. What are the seven indicators of a chemical reaction?
3. What are physical properties? Give two examples of physical properties.
4. What are chemical properties? Give two examples of chemical properties.
5. What are physical changes? What are chemical changes?
6. Compare and contrast homogeneous and heterogeneous mixtures.
SAMPLE PROBLEMS:
7. Identify which of the following are chemical changes (C) and which are physical changes (P)?
a. melting ice ___
c. burning hydrogen ___
b. cutting vegetables ___
d. baking a cake ___
8. Identify each of the following as being elements (E), compounds (C), homogeneous mixtures/solutions (S) or
heterogeneous mixtures (H).
a. Iron (Fe) _______________
d. ocean water _______________
b. dirt _______________
e. sugar (C6H12O6) _______________
c. carbon (C) _______________
f. Dissolved Kool-Aid _______________
9. Identify each of the following as either chemical properties (C) or physical properties (P).
a. burning in air _______________
d. rusting _______________
b. boiling point _______________
g. density _______________
c. cooking/baking _______________
h. shape _______________
10. How are the three main states of matter different (complete table below)?
State of Matter
Solid
Liquid
Shape
Gas
Volume
particle motion
PRACTICE PROBLEMS:
For each of the statements, identify whether it describes a solid (S), liquid (L), or gas (G).
11. Has definite volume and shape
14. When water boils it becomes this
12. Has a definite volume but no shape
15. Particles are tightly packed and neatly
13. Particles move freely is this type of matter
arranged
Conservation of mass problem:
16. In a flask, 50.3 grams of aluminum reacted with bromine to form 263.0 grams of aluminum bromide. How
many grams of bromine were reacted? Aluminum + bromine  aluminum bromide
Percent by mass problems:
17. A 156 gram sample of an unknown compound contains 25 grams of hydrogen. What is the percent by
mass of hydrogen in the compound?
18. If 5.11 g of hydrogen reacts completely with 46.5 g of oxygen to form hydrogen peroxide, what is the
percent by mass of hydrogen in hydrogen peroxide? Hydrogen + Oxygen  Hydrogen peroxide
THE ATOM AND PERIODIC TABLE
19. Fill in the table below about the three types of particles in an atom
Subatomic Particle
Proton
Location
Charge
Mass
Neutron
Electron
20. Isotopes of a given element have the same number of __________, but different number of ____________.
21. Know how to calculate the number of protons, neutrons and electrons in an atom when given its isotope
mass and atomic number. As an example: Iron (Fe) has an atomic number of 26. An isotope of iron has a
mass of 57 amu. Calculate the number of protons, neutrons and electrons in an atom of this isotope. How
would you write the isotope symbol for this isotope of iron?
22. When given the isotope symbol for an element be able to give its number of protons, electrons and
neutrons.
As an example: Give the number of each of these particles for !"
!"𝐾
23. Know the contributions of the following individuals according to the models we talked about in class.
A.
Bohr
B. J.J. Thomson
C. Millikan
D. Rutherford
E. Dalton
24. What is the name for the current model of the atom that we use today? Briefly describe this model.
25. For the element sodium (Na), determine the following:
(a) # electrons (b) # protons
(c) # neutrons
(d)# energy levels (e) # valence electrons
(f) Lewis Diagram
(g) Bohr Diagram
26. Use the diagram below to answer the following questions:
(A) Protons __________
(B) Neutrons _________
(C) Electrons _________
(D) Mass Number ________
(E) The element is _________
(F) Atomic Number is ________
UNIT 3: RADIOACTIVITY, HALF LIVES, EM SPECTRUM
1. What are the three types of radiation particles? What symbols correspond to each of these? Which is the
most dangerous of these? What protects you from each type?
2. Know how to balance a nuclear reaction selecting the correct particle.
As an example: What particles would you use to balance the following nuclear reactions?
!"
A. !"
(a) !!𝐻𝑒 (b) !!!𝑒 (c) !!!𝑒 (d) !!𝑛 (e) gamma ray
!"𝑀𝑔 → !"𝐴𝑙 + _______
B.
!"#
!"𝑃𝑏 → !"#
!"𝐵𝑖 + _______
(a) !!𝐻𝑒
(b)
!
!!𝑒
(c) !!!𝑒
(d) !!𝑛
(e) gamma ray
3. What is half-life and what can you use it for?
4. An isotope of cesium (cesium-137) has a half-life of 30 years. If 1.0 g of cesium-137 breaks down over a period
of 90 years, how many grams of cesium-137 would remain?
0 year
30 yrs
60 yrs 90 yrs
1.0 g
0.5 g
??
??
5. According the Electromagnetic (EM) Spectrum, which color light has the shortest wavelength?
6. According to the EM Spectrum, which color light has the lowest energy?
ELECTRON CONFIGURATION, ORBITAL DIAGRAMS (BOARDING HOUSE MODEL)
7. Define the following Aufbau Principle, Pauli Exclusion Principle and Hund’s Rule.
8. Which is the correct orbital diagram? Which rule supports your answer?
[
9. Using arrows, show how the following orbitals will fill with electrons.
Electron Configuration
K
1s22s22p63s23p44s1
Ne
1s22s22p6
S
1s22s22p63s23p4
Al
1s22s22p63s23p1
1s
2s
2p
3s
3p
4s
10. Write the Manager’s Code (electron configuration) for nitrogen.
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PERIODIC TABLE
11. Who organized the Periodic Table of Elements?
12. The original Periodic Table was arranged by increasing _____________, but now is arranged by increasing
_____________.
13. Vertical columns on the Periodic Table are called _________________________.
14. Horizontal rows on the Periodic Table are called ____________________.
15. Name the following groups:
#1or 1A______
#2 or 2A _____
#17 or 7A____
#18 or 8A ____
16. How many valence electrons do each of the following groups contain? #1 ______, #2 _______, #13______,
#14 ______, #15 ______, #16 ______, #17______, #18 ______
17. What are elements in the groups 3-12 called? ___________________________________
18. Know what happens to the size of atoms as you move across a period or down a group. Know which
member of the following pairs of particles is larger: Pd, Rb; Mg, Ba; Cs, Lu; Se, O.
19. Which of the following atoms would we expect to have the largest radius? Li, B, O, or F
20. Know which is larger, metal atoms or their ions. Also, know which is larger nonmetal atoms or their ions.
Which member of the following pairs of particles is larger? Br, Br-; Na, Na+; F, F-; Al3+, Al
Determine if the statement refers to a metal (M), nonmetal (NM) or metalloid (ML).
21. Also known as semiconductors.
22. Have high melting points.
23. Are brittle and dull.
24. Touching the staircase on Periodic Table.
25. Good conductors, malleable and ductile
CHEMICAL BONDING
1. Why do most elements need to bond?
2. Which group of elements do NOT need to bond because they already have eight valence electrons?
3. What is a chemical bond?
4. What is an ion? Give two examples of ions.
5. Atoms with less than 4 valence electrons will (give / take) electrons to fulfill the octet rule.
6. Atoms with more than 4 valence electrons will (give / take) electrons to fulfill the octet rule.
7. Give an example of an ionic compound. Draw a picture of the bond forming.
8. Give an example of a covalent compound. Draw a picture of the shared electrons.
9. Write the formula for a compound with two hydrogen and two oxygen atoms.
PRACTICE PROBLEMS:
10. Are these compounds ionic or covalent? (A) SO3
(B) FeCl3
(C) NaCl (D) CO2
11. Identify these properties as ionic (I), covalent (C) or metallic (M).
(A) Form individual molecules.
(D) Involve the sharing of electrons.
(B) Involve the transfer of electrons.
(E) Conduct electricity in solution.
(C) Form a crystal structure of charged particles.
(F) Electron sea model
12. Name these COVALENT compounds: (A) PCl3
(B) SO2
(C) N2O5.
13. Name these IONIC compounds:
(A) LiBr
(B) MgO
(C) NaOH (D) FeS
14. What type of bond forms between a metal and a nonmetal?
15. What type of bond forms between two metals?
16. What type of bond forms between two nonmetals?
17. Give an example of a polar molecule and explain why it is polar.
18. Write covalent formulas for: (A) carbon tetrachloride (B) sulfur hexafluoride (C) dinitrogen monoxide.
19. Write ionic formulas for: (A) calcium chloride, Ca+2 and Cl-1
(B) aluminum oxide, Al+3 and O-2
20. Draw Lewis Structures for H2O, CH4, CCl4, SF2 (TYPO ON REVIEW HANDED OUT IN CLASS)
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