Download Study Guide 1-3

Study Guide 1-3
Test 1-3 will consist of multiple choice & short answer questions over the following information.
1) Be able to determine the atomic number, mass number, name, oxidation number and isotopic
notation given a drawing of an atom or isotopic notation. You must also be able to determine
number of protons, neutrons, and electrons present.
a)
Draw the isotopic notation for an atom that has 14 protons, 20 neutrons, and 19 electrons
b)
Draw the isotopic notation for an atom that has 2 neutrons, 1 protons, and 0 electron
c)
Draw the isotopic notation for an atom that has 47 protons, 59 neutrons, and 50 electrons
Give the name, number of protons, neutrons, and electrons for each of the atoms below:
55
+3
Cu
29
2)
89
38
+1
Sr
130
52
-3
Te
Be able to determine the atomic number, mass number, name, oxidation number and
isotopic notation given a drawing of an atom or isotopic notation. You must also be able
to determine number of protons, neutrons, and electrons present.
A)
Draw the isotopic notation for an element that contains 30 protons, 38 neutrons,
and 27 electrons.
B)
Draw the isotopic notation for a neutral atom that has an atomic number of 55 and
a mass 117.
3)
4)
Understand how to find the electron configuration for a specific atom and what the parts
of the configuration designate. Give the electron configuration for each of the following:
A)
Calcium
B)
Bromine
C)
Yttrium
D)
Potassium
E)
Zinc
F)
Neon
Isotopes and Average Atomic Mass
A)
What do isotopes of the same element have in common? (4 facts)
B)
What do isotopes of the same element have that are different? (2 facts)
C)
Why does the atomic mass of an element contain a decimal?
D)
Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of
Rubidium-85 is 72.20% with an atomic mass of 84.91g, and the abundance of
Rubidium-87 is 27.80% with an atomic mass of 86.91 g, what is the average
atomic mass of Rubidium?
E)
Uranium has three common isotopes. Calculate the average atomic mass given
the following information:
234
U
U
238
U
235
F)
Atomic mass
% abundance
234.041 g
235.043 g
238.051 g
0.01500 %
0.715 %
99.27%
An element has an average atomic mass of 145.098 g. One isotope has a mass of
143.098 g and is found 41.09% in nature. A second isotope has a mass of
146.087 g and is found 0.5000% in nature. What is the mass of the third isotope?
5)
Lab safety:
Please know all 55 lab guidelines. Also, please know the location of all
the safety equipment in our lab & the uses for each piece.
6)
Please be able to identify & know the use for all the lab equipment.
7)
What is the difference between an observation & an inference? Please give an example
of an observation & an inference about the this classroom.
8)
Please list & describe the steps in the scientific method. Give a real life example that
illustrates the scientific method.
9)
Measuring
A)
Balance
B)
Ruler
C)
Thermometer
D)
Graduated cylinder
Please record each measurement correctly from these meter sticks. Assume you are
measuring in cm.
A)
50
40
7
8
B)