Topic # 1.1
GPS: 1a, 4b
Basic Atomic Structure
Part I: Subatomic Particles
 subatomic particle = a particle found _________ the atom.
There are ___ types of subatomic particles:
Name
Charge Symbol
Location
Date: _____/_____/_____
SPS1. Students will investigate our current understanding of the atom. a. Examine
the structure of the atom in terms of proton, electron, and neutron locations,
atomic mass and atomic number, atoms with different numbers of neutrons
(isotopes), and explain the relationship of the proton number to the element’s
identity. SPS4. Students will investigate the arrangement of the Periodic Table
b. Use the Periodic Table to predict properties for representative elements.
Mass
proton
approx. __ amu (1.007 amu)
neutron
approx. __ amu (1.008 amu)
electron
0.000 549 amu (_________)
 all atoms of all the different types of elements contain these same ______ _____
 what makes one element ___________ from another? The _______ number.
 all atoms of the _____ element have the _____ proton number, and atoms of different
elements have __________ proton numbers.
 ex: all gold (Au) atoms have ___ protons.
79 __ 47, so
all silver (Ag) atoms have ___ protons.
gold __ silver
 ________ number varies with the type of _________ (more on this later)
 ________ number is the same as ________ number for uncharged (________) atoms
(also, more on this later)
What makes one element different from another? ________________________________________________
What does negligible mean? _________________________________________________________________
Part II: Atomic Structure
 the atom has two distinct ______: the nucleus and the electron cloud.
 nucleus = ________ of the atom (like the _____ of the earth) where the ________ and
________ are found.
 the nucleus is ________ charged. Why? Because of the presence of
_______ (see table in Part I above).
D=
 the nucleus is the area of the atom with the most _________
 remember, density = ______ ________
 look at the ________ in the table in Part I above
 protons and neutrons are very ______ in relation to ________ (high mass)
 the _____ itself is very ______ (low volume)
 high mass  low volume = ______ density
What two subatomic particles are found in the nucleus? _______________________
The nucleus is a very (small, large) area inside the atom.
 electron cloud = area _____________ the nucleus where the
________ are found, _________ very fast around the nucleus.
 the ______ ________ of any particular electron cannot be known
because of their high ______, but we do know that…
 electrons spin a ______, confined _______ from the nucleus
(like ______ have distinct _____ around the sun). We call these
distinct distances from the nucleus “______ ______.”
 energy level = a distinct distance from the nucleus where an
electron can be found, _________.
m
V
 each energy level holds a different ________ of electrons:
 1st energy level holds ___ (total)
 2nd energy level holds ___ (total)
 3rd energy level holds ____ (8 outer, 10 inner)
 4th energy level holds ____ (8 outer, 24 inner)
 the ____ - ____ energy levels hold even more than that
 in an _________ ____ diagram (AKA _______ _____ diagram), only the outer
electrons are shown.
 notice how the energy levels always contain _______, evenly _____________
electrons.
Mg
S
N
The high speed at which electrons spin prevents us from knowing the exact _______________ of any electron.
What do the “rings” on an electron dot diagram represent? _________________________________________
Electrons on the second energy level are drawn (N/S/E/W, diagonally). Why? _________________________
________________________________________________________________________________________
Part III: Atom Symbols & Numbers
 all elements are represented by either 1- or 2-letter ________.
 most match the ______ of the element, others come from ____ names or other
_____________.
 all symbols must either be one ______ letter, or one capital and one _________.
 atomic number = number of ___ . Written in ______-____
-hand corner of symbol. Identifies the ________.
 mass number = number of p+ & n0 . Identifies the ________.
Written in ___-____-hand corner.
 average atomic mass = weighted _________ of all the _____
numbers of all the isotopes of an element. ____ written on
Carbon 6
symbol, but is found on ___.
 another number you can find on a symbol of an element
is the charge.
12.01
 it will be located in the ___ ____-hand corner of the symbol.
 we will discuss charge in more detail later.
C
14
6
+2
C
Name an element whose symbol and name do not “match.” _________________________________________
96
42
Mo What is this element’s atomic number? _____ What is its mass number? _____ Name? ___________
True or False? The mass number and the average atomic mass of an element are the same. _____________
The mass number identifies the (element, isotope). The atomic number identifies the (element, isotope).
Part IV: Isotopic Notation
 isotope = atoms of the same element that have the different numbers of ________.
 this means their _______ number (______ number) is the same, but because the
number of neutrons ______, the result is different ____ numbers for each isotope.
 ex: the isotope shown above is carbon-___. The other isotopes
mass number
of carbon are carbon-___ and carbon-___.
– atomic number
neutron number
Topic # 1.1
GPS: 1a, 4b
 to find the _______ number of different isotopes, simply _________ the atomic number
from the mass number.
Name of Isotope
Atomic
Number
Symbol
Mass
Number
# of
Neutrons
9
# of
Protons
10
66
Zn
sodium-23
40
20
16
Periods
________-32
1
2
3
4
5
6
7
Groups 1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
IA
VIIIA
hydrogen
helium
1
H
1.01
IIA
lithium
beryllium
3
Li
6.94
The Periodic Table
of the Elements
4
Be
9.01
___ = metals
___ = metalloids
sodium
magnesium
12
Mg
24.31
IIIB
IVB
VB
potassium
calcium
scandium
titanium
vanadium
chromium manganese
rubidium
strontium
yttrium
zirconium
niobium
molybdenum technetium
cesium
barium
lutetium
hafnium
tantalum
11
Na
22.99
19
K
39.10
37
Rb
85.47
20
Ca
40.08
38
Sr
87.62
55
Cs
132.91
56
Ba
137.33
francium
radium
87
Fr
(223)
88
Ra
(226)
21
Sc
44.96
39
Y
88.91
71
Lu
174.97
22
Ti
47.87
40
Zr
91.22
72
Hf
178.49
lawrencium rutherfordium
103
104
(260)
(261)
lanthanum
23
V
50.94
41
Nb
92.91
VIB
24
Cr
52.00
42
Mo
95.94
tungsten
VIIB
25
Mn
54.94
nickel
6
C
12.01
7
N
14.01
8
O
16.00
9
F
19.00
neon
10
Ne
20.18
aluminum
argon
IB
IIB
zinc
gallium
29
Cu
63.55
30
Zn
65.41
31
Ga
69.72
ruthenium
indium
silicon
14
Si
28.09
phosphorus
15
P
30.97
sulfur
16
S
32.07
chlorine
17
Cl
35.45
18
Ar
39.95
germanium
32
Ge
72.61
arsenic
33
As
74.92
selenium
bromine
krypton
iodine
xenon
34
Se
78.96
35
Br
79.90
36
Kr
83.80
rhodium
45
Rh
102.91
palladium
46
Pd
106.42
silver
47
Ag
107.87
cadmium
48
Cd
112.41
49
In
114.82
tin
50
Sn
118.71
antimony
tellurium
97.91
44
Ru
101.07
52
Te
127.60
53
I
126.90
54
Xe
131.29
rhenium
osmium
iridium
platinum
gold
mercury
thallium
lead
bismuth
polonium
astatine
radon
43
76
Os
190.23
dubnium
seaborgium
bohrium
hassium
(262)
(263)
(262)
107
108
77
Ir
192.22
78
Pt
195.08
79
Au
196.97
110
111
112
113
(265)
(268)
(272)
(273)
(285)
(284)
samarium
europium
gadolinium
64
Gd
157.25
terbium
65
Tb
158.93
dysprosium
holmium
59
Pr
140.91
60
Nd
144.24
144.91
62
Sm
150.36
actinium
thorium
protactinium
uranium
neptunium
plutonium
americium
curium
berkelium
(237)
(244)
(243)
(247)
(247)
93
81
Tl
204.38
109
praseodymium neodymium promethium
61
80
Hg
200.59
meitnerium darmstadtium roentgenium copernicium ununtrium
58
Ce
140.12
92
U
238.03
5
B
10.81
fluorine
28
Ni
58.69
75
Re
186.21
91
Pa
231.04
VIIA
oxygen
copper
cerium
90
Th
232.04
VIA
nitrogen
13
Al
26.98
57
La
138.91
89
Ac
(227)
VA
carbon
27
Co
58.93
74
W
183.84
106
cobalt
IVA
boron
26
Fe
55.85
73
Ta
180.95
105
___ = nonmetals
|---------- VIIIB ----------|
iron
metalloid
line 
IIIA
2
He
4.00
94
63
Eu
151.96
95
96
97
66
Dy
162.50
67
Ho
164.93
californium einsteinium
98
99
(251)
(252)
82
Pb
207.20
flerovium
114
51
Sb
121.76
83
Bi
208.98
84
Po
(209)
85
At
(210)
86
Rn
(222)
ununpentium livermorium ununseptium ununoctium
115
116
117
118
(289)
(288)
(293)
(294)
(294)
erbium
thulium
ytterbium
68
Er
167.26
fermium
100
(257)
69
Tm
168.93
70
Yb
173.04
mendelevium nobelium
101
102
(258)
(259)
SPS1. Students will investigate our current understanding of the atom. a. Examine the structure of the atom in terms of proton, electron, and neutron locations, atomic mass and atomic number, atoms with different numbers of neutrons
(isotopes), and explain the relationship of the proton number to the element’s identity. SPS4. Students will investigate the arrangement of the Periodic Table. b. Use the Periodic Table to predict properties for representative elements.