Chemistry A, Unit 3 (Chapters 5 & 6) Study Guide: Electrons in Atoms and the PTOE
Answer on a separate sheet of paper.
On a separate sheet of paper, Answer.
The answers are due at the start of the period when the Unit 3 Exam is given.
Chemistry content standards addressed in this unit: Students know how to - 1A, relate the position of an element in the
PTOE to its atomic number and mass; 1B, use the PTOE to identify metals, nonmetals, semimetals and halogens; 1C.
use the PTOE to identify alkali metals, alkaline earth metals and transition metals, trends in ionization energy,
electronegativity, and the relative sizes of ions and atoms; 1D, use the PTOE to determine the number of electrons
available for bonding; 1G, relate the position of an element in the PTOE to its quantum electron configuration and to its
reactivity with other elements in the table; 1H, know the experimental basis for the development of the quantum theory of
electron structure and the historical importance of the Bohr model of the atom; I.F. distinguish between hypothesis and
theory as scientific terms; I.G. recognize the usefulness and limitations of models and theories as scientific
representations of reality
Vocabulary: Given the definitions below, come up with the term that best fits that definition.
1) arrangement of electrons around atomic nucleus
2) spectrum caused by separate and distinct electron transitions
3) 3.00 x 108 m/s
4) energy needed to move an electron from one energy level to another (the formula)
5) tendency of electrons to enter orbitals of lowest energy first
6) height of a wave from origin to crest
7) discrete bundle of electromagnetic energy
8) distance between wave crests
9) each orbital has at most two electrons
10) number of wave cycles passing a point per second
11) region of high probability of finding an electron
12) lowest energy level
13) vertical column on the Periodic Table
14) horizontal row on the Periodic Table
15) electrons in the outermost energy level, usually in s & p orbitals
16) elements characterized by having 1 valence electron
17) elements characterized by having 2 valence electrons
18) elements characterized by having 7 valence electrons
19) elements characterized by having 8 valence electrons
20) elements characterized by having the “last” electrons in d-orbitals (two answers here)
21) elements characterized by having the “last” electrons in f-orbitals (two answers here)
22) What is “The periodic law?”
- - - - - - - - - - - - - - - - - Short Answer – give a brief response, sketch or calculation with units.
23) How does the energy of an electron change when the electron moves farther from the nucleus?
24) What is the shape of any one of the 3p atomic orbitals?
25) How many f-orbitals can there be in an allowed (by nature) energy level?
26) What is the maximum number of electrons in the third principal energy level? Fourth? Second?
27) What is the probability of finding an electron within the region indicated by the drawn electron cloud?
28) What types of atomic orbitals does nature permit in the third principal energy level?
29) How many unpaired electrons are there in a sulfur atom (Z = 16)?
30) Arrange the following colors of light in order from highest energy to lowest: orange, green, violet, yellow, blue
31) The lowest energy state of an atom is called the
state.
32) Find the wavelength of an electromagnetic wave that travels at 3.00 x 108 m/s and has a frequency of 60 Hz?
33) Which type of electromagnetic radiation includes the wavelength 10 -7 m?
34) Calculate the energy of a photon having a frequency of 4.0 x 107 Hz? (h = 6.62 x 10-34 J s)
35) Determine the frequency of a photon with0 an energy of 5.16 x 10-24 J? (h = 6.62 x 10-34 J s)
36) Why is there no such thing as a 2d set of orbitals?
37) What is the electron configuration for vanadium? (Give long form and Noble gas form)
38) What is the element with electron configuration 1s2 2s2 2p6 3s2 3p2 ?
39) What is the electron configuration for arsenic? (Give long form and Noble gas form)
40) How many electrons are in the highest energy level of the xenon atom (atomic number 54)?
41) The as yet undiscovered element with atomic number = 118 would be a member of which Group ? Give the group’s special
name as well as number.
42) Which elements are represented by the following electron configurations? What groups?
m. 1s22s22p63s23p64s2
n. 1s22s22p63s23p64s1
o. 1s12s22p63s2
p. 1s22s22p1
43) What orbital would the 20th electron of titanium, Ti, be in?
44) In order to occupy the same orbital, two electrons must have
.
45) The U.S. Air Force uses radio waves with an extremely high frequency (called EHF) for communicating with satellites. What
is the wavelength in meters for a signal with a frequency of 3.35 x 1017 s-1 ?
46) A helium-neon laser emits light of wavelength 232.8 nm. Which region of the electromagnetic spectrum is this light?
47) Which is the higher energy photon: orange, (A) or yellow, (B)?
48) Place the following types of radiation in order of decreasing energy per photon:
i. green light, ii. radio waves, iii. gamma rays, iv. infrared radiation,
v. ultraviolet radiation
49) What is the subatomic particle that plays the greatest role in determining the physical and chemical properties of an element?
50) Name three atoms in the third period that have a partially filled d-sublevel?
51) What class of element most readily loses electrons?
52) How does the number of valence electrons change going down a group in the periodic table?
53) How does atomic radius change from left to right across a period in the periodic table?
54) How do we explain why atomic sizes decrease going left to right across a period?
55) Why does atomic size increase going down a group in the periodic table?
56) Why is the radius of a positive ion always less than the radius of its neutral atom?
57) How does the radius of a neutral atom compare to that of its anion form?
58) Define ionization energy. Give a synonym (see Sargent Welch PTOE). What units is it measured in?
59) How does ionization energy change left-to-right across the periodic table? What causes this behavior?
60) Why does ionization energy decrease going down a group of elements in the periodic table?
61) Define electronegativity.
62) Which element has the lowest electronegativity? Which has the highest?
63) What is the group trend regarding electronegativity? What is the trend going left-to-right across a period?
64) What three factors are responsible for these trends in size, ionization energy and electronegativity?
65) Metallic character is characterized as the ability to lose electrons easily. Which one of the following atoms is the most
metallic: Mg, Ba, Sn, and Pb? Which one has the lowest ionization energy?
66) How many valence electrons does lead have? Xenon? Magnesium?
67) Who is the “father” of the periodic table?
68) Use your knowledge of periodic trends to determine which of the following elements, when chemically bound to sulfur, attracts
electrons less strongly than the sulfur: cesium, oxygen, fluorine, or chlorine?
Blast from the Past: Show all steps and units in the manner used in class.
I)
Convert 17.2 g to grams. Use dimensional analysis
II)
Convert 1.36 m2 to cm2. Use dimensional analysis.
III)
Light travels at 3.00x108 m/s. How many kilometers will it travel in two (2.0) hours. Use dimensional analysis
IV)
Write balanced nuclear equations showing:
Alpha Decay, Beta minus, Beta plus and Electron Capture for
V)
119Te.
The density of aluminum is 2.70 g/cm 3. What volume would a rod of aluminum with a mass of 0.750 kg have?