Chemistry Study Guide for Chapters 5 and 6.
CHAPTER 5:
1. Who inherited the planetary model of the atom? Describe this model.
2. According to Bohr, electrons can only reside in & not between _________ _________.
In Bohr’s model, each orbit or energy level has a _________ amount of energy. The ____________the electron is
from the nucleus, the more / less (circle one) energy that electron has.
3. When an electron jumps to a higher level, the electron _____________ a quantum of energy.
Know that quantum means “specific quantity”.
4. What is an excited state? _________________________________________________
5. What happens when an electron falls back to a lower energy level? ____________________________________
The farther apart the energy levels are, the greater / lesser (circle one) the amount of energy of the light emitted.
6. What is an atomic emission spectra? What does it look like? Know that atomic emission spectra is a characteristic and
identifiable physical property for each pure element.
7. What is a ground state?
8. Red light has _______ wavelength and _____ frequency; Blue light has ________ wavelength and _______ frequency.
9. Define: wavelength, amplitude and hertz.
10. How does an electron have a dual nature?
11. To explain the wave and particle natures of electrons, what model of the atom was developed? By whom? Describe this
model.
12. What’s another word for electron cloud? _________What is the probability of finding up to two electrons in it?
13. KNOW the Heisenberg Uncertainty Principle
14. Electron configuration means where the electrons are_____________What does electron configuration predict?
15. Know what each of the 4 sets of quantum numbers describe ____________________
16. The principle quantum number describes what ______________the electrons are in.
The seven energy levels corresponds to ________________ ___________in the periodic table?
17. The farther from the nucleus, or the higher the n value, the _______ the energy of the electron in that energy level.
18. Electrons tend to fill in the _______ energy levels and _______ sublevels first. (This is the Aufbau Principle.KNOW.)
19. There’s a max of _____electrons per energy level. There are “ “ number of sublevels per energy levels.
20. Per principle E-level, how many s orbitals can there be? ___ How many p orbitals? ___ d orbitals? ___f orbitals___
What are the shapes of the s, p, & d orbitals? ________________________________
What is the maximum number of electrons that can occupy the s, p, d, & f sublevels?
21. Know what the Pauli Exclusion Principle says:
22. After argon, what accounts for any deviations noted in electron configuration?
Ex: The 4s sublevel has __________energy than the 3d sublevel.
23. Be able to give the electron configuration for any element. Ex:
21Sc
24. What are some orbitals of equal energy?_________________________________________________________
Be able to apply Hund’s Rule when distributing electrons in orbitals of equal energy.
25. What is unique about the outermost s and p sublevels of the noble gases?
What chemical property does this confer upon them?
CHAPTER 6:
1. What is the Periodic Law?
2. Elements are arranged in the modern Periodic Table according to increasing ________ __________.
3. Properties are a periodic function of an element’s atomic number because elements in the same group have…
4. Another name for the Group A elements are the ________________________elements.
5. The Group B elements are known as the _________ _________ or the “________” block.
The d sublevels lag behind in filling by _______ energy level, compared to the s and p sublevels.
6. The Lanthanides and Actinides are known as the _______ ________________ metals or the “_______” block.
The f sublevels lag behind in filling by ______ energy levels, compared to the s and p sublevels..
7. What are the three regions of elements in the Periodic Table and where are they located?
8. What are the characteristic properties of metals?
9. Define:
ductile
malleable
lustrous
10. What are the characteristic properties of nonmetals?
11. Metalloids have properties that are __________those of metals & nonmetals. They are important as…..
12. Be able to locate the alkali metals, alkaline earth metals, halogens and noble gases on a Periodic Table.
13. Horizontal rows are called ___________ and vertical columns or chemical families are called ____________.
14. Define:
Atomic radius
Shielding
Ionization energy
Electron affinity
Electronegativity
Ionic radius
15. Know the periodic trends for each of these and be able to compare the relative values of these for any two or more
elements, as demonstrated in the homework problems or quiz.
16. For Group II A elements, what is the trend for first ionization energy, second ionization energy and third ionization
energy? What does ionization energy mean in terms of difficulty in removing an outer electron?
MISCELLANEOUS INFORMATION
1. For Group A elements, elements in the same group have the ______ of electrons in the ____________ energy level. If
given an A element, be able to give the # of electrons found in the outermost level.
2. What is an ion?
3. What is the charge (oxidation number) of an ion formed from elements in Group
1A_______ 2A________ 3A________ 5A________ 6A________ 7A________
Applications:
1. What is the Octet Rule?
2. The most reactive group of metals in the Periodic Table are the ______________ Why?
3. Describe the physical appearance of the alkali metals.
4. The reactivity of metals increases / decreases (circle one) as we go down any group. The most reactive metal is…
5. Any alkali metal will react with oxygen to form metal __________.
6. Any alkali metal will react with H2O to form _________ solutions containing ______ (the hydroxide ion), which turns red
litmus paper blue. In addition, what gas will form? _______
7. Alkali metals are _________________ conductors and are/are not found free in nature because they’re….
8. What physical properties do all metals share in common?
9. Why are the alkaline earth metals reactive, but not as reactive as the alkali metals?
10. The alkaline earth metals react with halogens to form __________. They also react with H 2O to form alkaline solutions
of _________ ______________and __________ gas. Alkaline earth metals also react with oxygen to form __________
11. What outer electron configuration does group 13 or 3A have? These atoms lose or gain (circle one) ____electrons to
form what charge ions_______.
12. What outer electron configuration does Group 14 or 4A have?
Will carbon and silicon tend to form ions? ________ What will they want to do with their electrons?_________
But tin and lead are in the same group and will form positively charged ions, why?
13. Describe the outer electron configuration of Group 15 (5A) and Group 16 (6A) elements._______ and ______ What
charge will their ions have? _____ and ______The names of these ions are changed to end in __________.
14. Because sharing electrons make them more stable, the halogens generally exist as ________________ molecules.
15. F2 & Cl2 are __________, Br2 is a reddish-brown ___________, & I2 is a _________.
16. What feature involving electron configuration accounts for the halogens being the most reactive nonmetals?
17. Reactivity of the halogens increases/decreases going UP the group. The most reactive nonmetal is_______.Which is
the least reactive nonmetal of the following: F, Cl, Br, I
18. When halogen atoms gain one electron, the resulting ion has a ___charge and the name is changed to end in____.
Ex: the fluorine molecule = ___________ but the fluoride ion = _______________
19. The reaction between an alkali metal and a halogen produces a ______________. Ex: Na (s) + Cl2 →
20. What is a salt?
21. Which element forms its own chemical family or group?
22. This element occurs in nature as _______, which is explosive, or with other elements, such as _________.
23. What is the chemical symbol & name of the H-atom after it loses an electron, like the alkali metals?___________
24. What is the chemical symbol & name of the H-atom after it gains an electron, like the Group 17(7A) ions?______
25. How does the group number of the B Groups correspond to their electron configuration?
26. What is the reactivity and physical properties of the B elements compared to Groups 1 (1A) & 2 (2A)?
27. What’s another word for outer electrons: _____________ electrons.
28. What is the oxidation number of an ion? ______________________________