Download Chem 101 Lesson 4 Reading Guide Modern Atomic Theory

Chem 101 Lesson 4 Reading Guide
Modern Atomic Theory: Chapter 11.1  11.11 pages 302-331
Directions: Fill in the answer or select the correct answer from the choices given in parentheses.
If a number in parentheses follows the question (like (F11.4)) it means you should look at Figure
11.4 in the text for the answer.
This is a longer Chapter than normal, so occasionally, Section numbers will be given to let you know
that the following questions will come from the new referenced section and following sections.
1. ______________________ is the distance a light wave travels to complete one cycle, the distance
between two peaks on a wave. (F11.3)
2. _____________________ refers to the number of wave cycles completed in 1 second or the number of
peaks that pass a given point in one second.
3. The wavelength of red light is _________(longer, shorter) than the wavelength of blue light. (F11.6)
4. Light with a longer wavelength has ___________(more, less) energy than light with a shorter
wavelength. This means that red light has __________(more, less) energy than blue light. (F11.6)
5. The visible spectrum refers to energy that has wavelengths between _______ and ______ nm. (F11.4)
6. Ultraviolet light has a wavelength (less than, greater than) visible light, while infrared light has a
wavelength (less than, greater than) visible light. (F11.4)
7. The wavelength and frequency of light are inversely related, which means as wavelength increases,
the frequency decreases and vice versa. Refer to Figure 11.4 to answer this question.
Comparing X-rays and microwaves, which has the larger
a) frequency? _________________ b) wavelength? _______________ c) energy? ____________
8. Energy from an excited atom is released as a _______________, which is a form of light.
Section 11.4-11.5
9. Spectral lines seen for hydrogen were caused by excited electrons dropping from
__________________ energy levels in the atom to __________________ energy levels in the atom.
The red colored line corresponded to the electron transition with the _____________ amount of
energy, while the violet colored line corresponded to the electron transition with the ____________
amount of energy. (F11.11)
10. Experimental evidence for Bohr’s model of the atom came from the ______________atom.
11. Observing that each element has its own unique set of spectral lines leads us to believe that the
differences between energy levels in atoms of different elements must be _______________( the
same, different).
Section 11.7
12. The lowest energy state for hydrogen electrons is the ______orbital or ground state.
13. It has been determined that the energy levels of electrons in hydrogen atoms contain sublevels with
different shapes. They have been designated as ____, _____, ______, and _______.
14. The number of sublevels in each main energy level corresponds to the number of the main energy level.
For example, energy level 1 contains only ________ sublevel, while energy level 2 contains
______ sublevels.
15. Indicate the maximum number of electrons that can exist in each of the following sublevels.
s ____
p ____
d _____
f _____
16. Electrons that have higher energies exist _____________ (closer to , farther from) the nucleus.
Section 11.8
17. What is the Pauli Exclusion Principle?
Section 11.9
18. Write the electron configuration and orbital diagram for the 1st 18 elements on the periodic table. Use
the back of this page or your own paper.
Section 11.10
19. Within a given energy level, the order in which the sublevels are filled is ___, ____, ____, then ____.
20. The d orbitals of an energy level are always filled after the ___ orbitals of the next higher energy
level have been filled.
21. Which sublevel gains electrons after each of the following sublevels is filled?
a) 2p _______
b) 3p ______
c) 3d _______
d) 5s _____
21. In the following representation of part of an electron configuration, indicate what each number and
letter represent. (choose from principle energy level, sublevel or shape, and number of electrons in the
sublevel)
3p4
22. Write the electron configuration for the element nitrogen, whose atomic number is 7.
23. The shapes of the orbitals are described as follows: s _________________
p ______________
24. Group IA elements are called _____________ ___________.
25. Group IIA elements are called ______________________ ______________ _______________.
26. Group VIIA elements are called _____________________.
27. Group VIIIA elements are called _____________ or __________ gases.
28. The periodic table can be divided into four major blocks based on the type of orbitals that are being
filled. Referring to section 6.6 in your text, complete the following. (F11.31, F11.34)
s- block elements = elements in Groups _____ and _____
p-block elements = elements in Groups ___ through _______
The s- and p- block elements together are referred to as the ______- _________ or
_________________________________ elements.
d-block elements = the ____________________________ metals or elements
f-block elements = the _______ - ____________________________ elements
The atomic radius is the distance from the nucleus to the outermost electrons. The atomic radius is half of
the atomic size and the trends shown in Figure 11.36 for atomic size also apply to the atomic radius.
29. The atomic radius __________________( decreases, increases) as you move up a group of elements
due to the elements at the top of the table having _______________ (fewer, more) energy levels
occupied by electrons.
30. The atomic radius __________________ (decreases, increases) as you move from left to right in a
period due to the increase in the number of _______________ in the nucleus which
_______________ the nuclear charge leading to a greater attraction for the electrons in the atom.
31. Metals tend to _________ (gain, lose) their outermost electrons when they react.
32. Metallic character is a measure of how easily an element loses its outermost
electrons. It is observed that as you move down a group of elements, the metallic character of the
elements _____________(decreases, increases), and as you move from right to left across a period,
the metallic character of the elements ________________ (decreases, increases).
33. What can you conclude about the relationship between the metallic character of an element and its
atomic radius? In other words, if you have an element with a large amount of metallic character, would
you expect it to have a large or small atomic radius? ______________________________________
34. Elements in the same group or family react in _________________ (different, similar) ways.
35. The outermost electrons of an atom are the electrons involved in chemical
reactions. These electrons are called __________________ electrons and are equal to the total
number of _____ and _____ electrons in the outermost energy level. Because of this, the maximum
number of these electrons in an atom is ______________.
36. We can predict the number of valence electrons by noting the ____________ number of the family
they are in, if they are a representative element.
37. Indicate the number of valence electrons in the following elements.
B ____
Ca ____
K _____
P ______
Cl _____
38. Any atom bearing a charge has had electrons removed or added and is called an _______.
39. The amount of energy needed to remove an electron from a neutral atom in the gaseous state is called
the __________________________ energy.
40. The ionization energy (I.E.) __________________ (decreases, increases) up a group of elements,
while it _____________________ (decreases, increases) from left to right across a period.
41. Ionization energy ____________________ (decreases, increases) as the atomic radius increases.
42. Which of the following elements has the larger I.E. ?
Ba or Ca _______
Al or Cl _____
43. In general, when metals and nonmetals react, the metal atom becomes a ion with a ________________
(negative, positive) charge, while the nonmetal ___________( gains, loses) electrons and becomes an ion
with a _______________(negative, positive) charge.