Atomic Models
and Subatomic Particles:
1. Complete the following table
Symbol
Atomic Mass
52
-
P
j3Ec_
Atomic
Number
24
Number of
Protons
Number of
Neutrons
15
15
62..
17
2
30
21
I ‘LI
47
43
127
Ca
2
Hg
ç
Bf
3
Ga
3
N
52
26
10
201
36
‘33
3 j
1-
70
7
Number of
Electrons
24
15
54
23
20
f
,
:39
36
36
28
7
to
2. An element is analyzed by a mass spectrometer and the following spectrum resulted for the
naturally occurring isotopes.
75
76
LI
77
I
T
% Abundance
20.5
27.4 7.8
36.5
7.8
a) Calculate the average atomic mass for this element.
FOc cDzo5 45
\
F2 x 0 2J9
B
1? cc*1-
C99
=
O4-E
b) ‘What element was analyzed?
Cl
c
c) Write the symbol for the most abundant isotope of this element, including the atomic mass,
and the atomic number.
C-)
I
4?
I
C,
I
V
—
2
0
9LJ
I-)
-r
a
r
3
0
Lc
&)
1
C
a
0
0
CD
0
C)
CD
o
C
CD
I
N
CD
g
-
7_
CD’’
n fln
I.
\J
I’
v
CD
a
—
1—JrCD
b
1
CD
Elements and the Periodic Table:
Cl o cc’4&
1. What is a period of the periodic table?
2. What is a group or family of the periodic table?
—
çz
D
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
Li, Na, K, Rb, Cs, Fr
Family Name
\ka
ck
Number of
Valence Electrons
Charge on the Ions
Usually Formed
j
B,Al,Ga,In,Tl
k3
F, Cl. Br, I, At
—
Be, Mg, Ca, Sr, Ba, Ra
1
2
5
N, P, As, Sb, Bi
He, Ne, Ar, Kr, Xe, Rn
C)
—2
O,S,SeTe,Po
4. Defme the following terms:
a) Atomic Radius:
*c
R
CCfl S
0
b) Ionization Energy:
-
c_)
\
Cre
(n
c) Electronegativity:
e
e lcJcn
n
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
ç..Q$EE
1(
\ ccecs
b) As you move down the periodic table:
Atomic radius
Ionization Energy
LI’
cej?’
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
,S
3
, CF
2
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, 2
Mg Al
,
3
ii) Na, Mg, Al, Si
v) P
,S
3
, CF
2
iii) Mg, Os, Cl
P
P\
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
N
t%cAJe
Chemical Bonding:
l.a) Define valence electrons:
ccec
—
4
VCc
b) How many valence electrons does each of the following families contain?
i. Alkali metals:
v. The Nitrogen family:
ii. Alkaline earth metals:
2
vi. The Oxygen family:
iii. The Boron family:
vii. The Halogens:
iv. The Carbon family:
viii. The Noble gases:
3
4cc-
5
2. Describe what is happening to the electrons involved in a:
a) Covalent bond:
cccflm
b) Polar-covalent bond:
—
Ca esQ
cLN
2
(Q.
cce.
hc
e
&
cs
c) Ionic bond:
cc-t c
3. Name the two types of intermolecular bonds:
and
C4ccN
b
cv1 nq
&c-kax
ecc\-\
Lcñccm
CQS
4. Draw the electron dot diagrams and Lewis structures for each of the following:
a) Al
SO
g) 3
3..
Lj
b)Ca
5
h) H
0
2
0
c)F
c;-_
i) C
H
2
—
1-:C
cc
j) C0
2
3
d) S
2
0
L
c
-
s_,
L_.-’
e) 3
CH
O
H
k) N
2
3
f)BF
1) C
3
H
2
Br
‘
U
0
-i
C°
c’
1
‘1_