Download Unit 2 Exam Review: Matter and its Properties This review does not

Unit 2 Exam Review: Matter and its Properties
This review does not cover everything that will be on Thursday’s exam. In order to perform at your highest level, I suggest completing the following:
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Unit 2 Exam Review Guide
Review quizzes and correct mistakes
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Review Notes
Make flashcards as you study
The review is divided into sections, one for each TEK covered on the exam.
CHEM 6A understand the experimental design and conclusions used in the development of modern atomic theory, including
Dalton’s Postulates, Thomson’s discovery of electron properties, Rutherford’s nuclear atom, and Bohr’s nuclear atom
1.
Using the picture above, explain Rutherford’s gold foil experiment. What was Rutherford’s hypothesis? Did it hold true?
What model did Rutherford disprove? What did the gold foil experiment tell us about the structure of the atom?
2.
Describe one conclusion made by each of the following scientists that led to the development of the modern atomic theory.
a. J.J. Thomson
b. John Dalton
3.
Draw the Bohr model for the following elements:
Beryllium
Chlorine
4.
Highlight the valence electrons in your models above. What is the definition of ‘valence electron?’
5.
Write down Dalton’s postulate that is no longer believed to be true. Explain why it is false and what it should say in order to be
true.
6.
Compare and contrast the three types of subatomic particles in terms of location in the atom, mass, and relative charge.
7.
In the space below, make a timeline for the modern atomic theory. Your timeline should include the following individuals:
Dalton, Thomson, Rutherford, and Bohr. For each individual, you should write key points relating to their discovery AND how
they pictured the atom (draw the individual’s representation of the atom).
CHEM 6D use isotopic composition to calculate an average atomic mass of an element
8.
Complete the following table using your knowledge of isotopes
Symbol
Atomic
Number
Mass Number
Number of
Protons
22
109
Number of
Electrons
Number of
Neutrons
11
12
20
9
10
37
17
17
Ag+1
9. How are the atomic number and the number of protons related to each other?
10. How do the number of protons, number of neutrons, and the mass number relate to each other?
11. What is the one thing that determines the identity of an atom (that is, whether it is an oxygen atom or a carbon atom,
etc.)?
12. How many protons are in the isotope 54Cr?
13. How many neutrons are in the isotope 42Ca?
14. How many electrons are in the isotope 23Na?
15. What is the mass number of a Magnesium isotope that consists of 12 protons, 12 electrons, and 13 neutrons?
16. Calculate the average atomic mass of iridium using the following data for two iridium isotopes.
Isotope
mass (amu)
relative abundance
Ir-191
191.0
37.58%
Ir-193
193.0
62.42%
17. Lithium has two naturally occurring isotopes: lithium-6 and lithium-7. If the average atomic mass of lithium is 6.941 amu, which
isotope is the most abundant? How do you know?
CHEM 5A explain the use of chemical and physical properties in the historical development of the Periodic Table
18. Compare
and contrast Mendeleev’s periodic table to the modern periodic table used today.
19. Why do elements in the same group/family have the same chemical properties?
20. Which elements are most likely to undergo the same kinds of reactions, those in a group or those in a period? Explain your
answer.
CHEM 5B use the Periodic Table to identify and explain the properties of chemical families, including alkali
metals, alkaline earth metals, halogens, noble gases, and transition metals
21. Which elements are designated as noble gases? What is the most significant property of these elements?
22. This group of the periodic table is highly reactive and elements are soft enough to cut with a knife…
23. This group of the periodic table contains metals that exist in elemental form…;
24. This group of the periodic table contains highly reactive nonmetals…
25. Without using your notes, attempt to fill in the blank periodic table below. Label the alkali metals, alkaline earth metals,
halogens, noble gases, and transition metals. Write in the group numbers and the number of valence electrons for the main
groups. Draw in the staircase and write in where the metals, metalloids, and nonmetals are on the PT.
Complete the following table using your knowledge of the Periodic table families:
PT Family
Physical Properties
Chemical Properties
MOST IMPORTANT FACT
Alkali Metals
Alkaline Earth
Metals
Transition
Metals
Halogens
Noble Gases
CHEM 5C use the Periodic Table to identify and explain periodic trends, including atomic and ionic radii, electronegativity,
and ionization energy
26. What type of ion will lithium form? What will the ion’s charge be and why? Will the lithium ion be larger or smaller than the
parent lithium atom? Explain.
27. Rank the following elements by increasing atomic radius…Cl, Ar, Mg, Al. How do you know this is the order?
28. Rank the following elements by increasing electronegativity: cesium, oxygen, neon, barium. How do you know this is the order?
29. What trend in atomic radius do you see as you go down a group/family on the periodic table? Why?
30. What trend in atomic radius do you see as you go across a period/row on the periodic table? Why?
31. What trend in electronegativity do you see as you go down a group/family on the periodic table? Why?
32. What trend in electronegativity do you see as you go across a period/row on the periodic table? Why?
33. Why does fluorine have a higher ionization energy than iodine?
34. What trend in ionization energy do you see as you go down a group/family on the periodic table? Why?
35. What trend in ionization energy do you see as you go across a period/row on the periodic table? Why?
36. Which of the following is a correct explanation for why Magnesium is more electronegative than Calcium?
a. Ca has a larger radius and larger number of protons
b. electrons in Mg are not very attracted to the nucleus
c. Mg has less electrons
d. Mg has fewer electrons shells between the valence electrons and the nucleus
Chem.6E express the arrangement of electrons in atoms through electron configurations and Lewis
valence electron dot structures.
37. Which two orbitals satisfy the octet rule?
38. Complete the following table:
Atomic Subshell
Number of Orbitals
Number of total electrons in SUBSHELL
s
3
14
39. How many electrons are required to fill the 2 nd energy level? (*Hint – which subshells are in the 2nd energy level?)
a. 2
b. 4
c. 8
d. 10
40. How many electrons are required to fill the 3 rd energy level? (*Hint – which subshells are in the 2nd energy level?)
a. 6
b. 10
c. 18
d. 32
41. Describe the shape of each subshell (s, p, d and f)
42. Match the following rules with their definitions
_____Hund’s Rule
_____Aufbau’s Principle
_____Pauli Exclusion Principle
a. each electron occupies the lowest energy orbital available
b. a max of 2 e- can inhabit one orbital if they have opposite spins
c. single electrons with the same spin must occupy each equal-energy orbital before
additional electrons with opposite spins can occupy the same orbital
43. Write the electron configurations for Na, Sr, Ti, Se
44. Write the electron configurations in Noble Gas Notation for Li, Cr, Ag
45. Draw the Lewis Dot Diagram for helium.
46. Draw the Lewis Dot Diagram for aluminum.