Chemistry 1 1
Review Package #3
Atomic Models and Subatomic Particles
The Periodic Table
Chemical Bonding
1. Atomic Models and Subatomic Particles:
A. Subatomic Particles and Average Atomic Mass:
-
Subatomic particles: protons, neutrons and electrons properties and how to
—
calculate numbers of each
-
Atomic mass and atomic number
-
Ions
-
Isotopes and calculations of average atomic mass
B. Quantum Molecular Model
-
Electron orbitals
-
Electron configurations of neutral atoms and ions
-
Significant figures (multiplication, division, adding and subtracting)
C. History of the Atomic Models
-
Identifying which scientists made which discoveries
2. Elements and the Periodic Table:
A. Organization of the Periodic Table
-
The history of the periodic table
-
metals, non-metals, and semi-metals
-
chemical families; Alkali metals, Alkaline Earth metals, Halogens, Noble Gases
B. Periodic Trends
-
Atomic radius, and ionic radius (sizes of atoms versus their ions)
-
Ionization energy
-
Electronegativity
3. Chemical Bondin2:
A. Electrons, Electronegativity and Bonding (text pgs. 225-231)
-
valence, bonding, lone-pair electrons
-
types of chemical bonds; ionic, covalent, polar-covalent
-
predicting bond formation based on electronegativity differences
-
electron dot diagrams for elements
B. Lewis Structures to Represent Bonding (text pgs. 236-243)
-
Rules for drawing Lewis structures (Octet rule)
-
Single, double and triple bonds (bonding capacity)
-
Lewis structures for simple ions, polyatomic ions and simple molecules
Atomic Models and Subatomic Particles:
Symbol the following table.
1 Complete
.
Atomic Mass Atomic Number of Number of Number of
52 Number Protons Neutrons Electrons
24 24
15 17 15
127 52 54
26 30 23
Ca 21
2
Hg 201
36 47 36
Bf 43 36
3
Ga 70 28
3
N 7 7
2. An element is analyzed by a mass spectrometer and the following spectrum resulted for the
naturally occurring isotopes.
Mass 75 76 77
I I I
a)
% Abundance
I 20.5 27.4 7.8
Calculate the average atomic mass for this element.
36.5
I
7.8
b) What element was analyzed?
c) Write the symbol for the most abundant isotope ofthis element, including the atomic mass,
and the atomic number.
3. Write the core-notation electron configuration for the elements listed below.
Be Ar
C V
N Cu
Na Ge
S Br
4. Complete the following table.
Symbol Number of Number of Number of Electron
Protons Neutrons Electrons Configuration
70 3+
1’LJa
,-
3
37 -
17
39 Tr+
1 91
65 ,— 2+
uu
29
32 2-
16
30 3-
15
87 c 2+
,r
38
59 ‘—i 2+
27’O
5. Tn the table below briefly summarize the MAJOR contribution(s) the scientist made to our
understanding of the atom.
Scientist Major Contribution(s)
Dalton
Bohr
Thompson
Chadwick
Rutherford
Elements and the Periodic Table:
1 What is a period of the periodic table?
.
2. What is a group or family ofthe periodic table?
3 Complete the following table, stating the name of the family (if we named it), the number of
.
valence electrons and the charge on the ions that are usually produced from the elements in the
group.
Family Members Family Name Number of Charge on the Ions
Valence Electrons Usually Formed
Li, Na, K, Rb, Cs, Fr
B, Al, Ga, In, Tl
F, Cl. Br, I, At
Be, Mg, Ca, Sr, Ba, Ra
N, P, As, Sb, Bi
He, Ne, Ar, Kr, Xe, Rn
0, S, Se Te, Po
4. Define the following terms:
a) Atomic Radius:
b) Ionization Energy:
c) Electronegativity:
5. Correctly fill in the blanks below with either “increases” or “decreases”
a) As you move from left to right across the periodic table:
Atomic radius
Ionization Energy
Electronegativity
b) As you move down the periodic table:
Atomic
radius
Ionization Energy
Electronegativity
6. a) Which of the following has the LARGEST atomic radius?
i) Li, Na, K, Rb iv) Na, Mg
, Al
2 3
ii) Na, Mg, Al, Si v) P
,
3 2,
cr
iii) Mg, Os, Cl vi) N, 0, F, Cl
b) Which of the following has the LARGEST ionization energy?
i) Li, Na, K, Rb iv) Na, Mg
, Al
2 3
2,
ii) Na, Mg, Al, Si v) P
,
3 C1
iii) Mg, Os, Cl vi) N, 0, F, Cl
c) Which of the following has the SMALLEST electronegativity value?
i) Li, Na, K, Rb iii) Mg, Os, Cl
ii) Na, Mg, Al, Si vi) N, 0, F, Cl
Chemical Bonding:
1 .a) Define valence electrons:
b) How many valence electrons does each ofthe following families contain?
i. Alkali metals: v. The Nitrogen family:
ii. Alkaline earth metals: vi. The Oxygen family:
iii. The Boron family: vii. The Halogens:
iv. The Carbon family: viii. The Noble gases:
2. Describe what is happening to the electrons involved in a:
a) Covalent bond:
b) Polar-covalent bond:
c) Ionic bond:
3. Name the two types ofintennolecular bonds:
and
4. Draw the electron dot diagrams and Lewis structures for each of the following:
a) Al g) 3
SO
b)Ca 0
2
h)H
c) V i) C
H
2
2
d) j) CO
2
3
e) CH
OH
3 k) N
2
0 BF
3 1) 3
HBr
2
C
