Atoms, the Periodic Table, Electron Configuration, and Orbital Notation
Chapter 4
1) What are the 4 parts of the Atomic Theory?
A.
B. Atoms of the
element are
.
C. Atoms form compounds by combining in
.
D. Atoms can be combined, separated or rearranged – they never
into atoms of another
.
2) Where are p+, n0, and e- located?
3) How do the masses of p+, n0, and e- compare to one another?
4) Due to Rutherford’s Gold Foil Experiment, we can conclude that:
A. The nucleus is
and has a
charge.
B. Atoms are mostly
.
5. Isotopes are atoms of the same element with a different number of
, thus a different
number.
6. Draw two examples of isotopes using chemical symbols.
7. What is the mass of carbon-12?
Of carbon-14?
8. What is the average atomic mass of an element with isotopes X-130, X-145, X-160 is percent abundances 9%, 32%, 59%, respectively.
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Chapter 5
Write the electron configuration and orbital notations for the following Atoms:
Element
1) # of p+
1) At. #
2) # of e2) Ma #
3 # of n0
Electron Configuration and orbital notation
Li
F
Mg
Si
Cr
Ga
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Electron Configuration Practice
Directions: Write and draw the electron configurations of each of the following atoms.
Example:
Co : 27 e- 1s2 2s2 2p6 3s2 3p6 4s2 3d7
1. Scandium:
2. Gallium:
3. Silver:
4. Argon:
5. Nitrogen:
6. Lithium:
7. Sulfur:
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Name:____________________________
Date____________
Per:_________
Electron Configuration Practice - Homework
In the space below, write the expanded electron configurations (ex. = 1s22s1) of the following elements:
1)
Sodium
________________________________________________
2)
potassium
________________________________________________
3)
chlorine
________________________________________________
4)
bromine
________________________________________________
5)
oxygen
________________________________________________
In the space below, write the abbreviated electron configurations (ex. Li= [He]2s1) of the following
elements:
6)
manganese
________________________________________________
7)
silver
________________________________________________
8)
nitrogen
________________________________________________
9)
sulfur
________________________________________________
10)
argon
________________________________________________
In the space below, write the orbital notation (arrows) of the following elements:
11)
manganese
_______________________________________________
12)
silver
________________________________________________
13)
nitrogen
________________________________________________
14)
sulfur
15)
argon
________________________________________________
________________________________________________
Determine what elements are denoted by the following electron configurations:
16)
1s22s22p63s23p4 ____________________
17)
1s22s22p63s23p64s23d104p65s1 ____________________
18)
[Kr] 5s24d105p3 ____________________
19)
[Xe] 6s24f145d6 ____________________
20)
[Rn] 7s25f11 ____________________
Determine which of the following electron configurations are not valid:
21)
1s22s22p63s23p64s24d104p5 __________________ 22) 1s22s22p63s33d5 ____________________
23)
[Ra] 7s25f8 ____________________
24) [Kr] 5s24d105p5 ____________________
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Name:____________________________
Date____________
Electrons, Valence, and Lewis Dot Structures
Chem 544/545 Dr. Brielmann
Per:_________
Name______________________
Period___________________
1. How many electrons are present in:
Helium (He)_____ Carbon (C)_____
Neon (Ne)_____ Sodium (Na)_____
Zinc (Zn)____
2. How many valence electrons are present in:
Helium (He)_____ Carbon (C)_____
Neon (Ne)_____ Sodium (Na)_____
Potassium (K)_____ Fluorine (F)_____
Chlorine _____
Bromine_____
3. Draw Lewis Dot Structures for the following elements:
Helium (He)
Carbon (C)
Neon (Ne)
Sodium (Na)
Ne
4. Correct the following Lewis Dot Structures:
Oxygen
Nitrogen
O
Beryllium
Be
N
Fluorine
F
5. Fill in the following table:
Carbon
Carbon anion
C-
Carbon cation
+
C
number of electrons:
number of valence electrons
Lewis structure
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Name:____________________________
Date____________
Per:_________
Law of Conservation of Matter and Electron Configuration Review
1. a. Define the term valence shell.
b. Why is the valence shell so important in studying chemical reactions?
2. Given an element with atomic number 11, provide the following information:
a. How many electrons will fill each of the following shells:
1st shell:
2nd shell:
3rd shell:
b. Is this element likely to form a cation or anion?
c. What charge will the ion formed by this element have?
3. Roman numerals are needed when naming many of the transition metals because
_________________________________________________________________________________
_________________________________________________________________________________
4. a. A molecule with an overall positive or negative charge is called a _________________________.
b. An example of one is _______________________
5. Explain, based on electron configuration, why the noble gases are so unreactive. Use helium and
neon as examples to illustrate your explanation.
6.
Each of the following chemical formulas and names are written incorrectly. Rewrite them correctly.
a.
b.
c.
d.
e.
Cl2Mg
NaP
Iron Sulfur
NH4Cl3
Cesium (I) bromide
7. a. What does the Law of Conservation of Matter state?
____________________________________________________________________________________
______________________________________________________________________________
b. Explain the reason for balancing equations based on this law.
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