Name ____________________ Date _______________ Period ________ # _____
Ch. 19 Atomic Structure Note Guide
1.
Parts of an Atom Concept Map (pgs. 579 - 583)
Electrons (found
outside the nucleus
in orbitals)
Protons
Positively
(+) charged
Neutral (have
no charge)
2.
Fill in the missing parts to the subatomic particle table.
Particle
Symbol
Charge
Electron
e
Negative ( - )
Proton
p+
Positive ( + )
o
Neutron
n
Zero (neutral = 0)
Relative Mass
0 amu
1 amu
1 amu
3.
Where are the protons located in an atom?
4.
Where are the neutrons located in an atom?
5.
Where are the electrons located in an atom?
6.
Label the electrons, protons, neutrons, orbitals, and nucleus in the atom below.
Name ____________________ Date _______________ Period ________ # _____
(See pgs. 584-587)
7.
What does the atomic number of an element tell you?
the number of ________________
8.
Where is the atomic number located on each of the squares of the periodic table?
9.
What does the mass number (average atomic mass) of an element tell you?
the sum of ______________ and ________________
10.
Where is the mass number (average atomic mass) located on each of the squares
of the periodic table?
11.
Write down the formula we use for determining the number of neutrons that are in
a specific element (atom).
Number of neutrons = Atomic number (top number) - Mass Number (bottom
number made into a whole number)
12.
If an element is electrically neutral (it has not lost or gained any electrons), the
number of ______________ is the same as the number of protons or the atomic number.
13.
Testing Your Knowledge (so far): Determine the number of protons, electrons,
and neutrons in each of the following elements.
8
15
30
O
P
Zn
16
31
65
p+ =
p+ =
p+ =
o
o
n =
n =
no =
e- =
e- =
e- =
Drawing Atomic Models See pgs. 587 and 592. Look at the diagrams closely.)
14.
What is the number sequence I taught you for remembering the maximum number
of electrons you can place in the orbitals (rings) of an atom?
15.
Draw the Bohr Model for Sodium (Na)
Step 1: Determine the number of protons, electrons, and neutrons by looking at the
Periodic Table.
p+ =
no =
e- =
Step 2: Draw the model using the rules for proper placement of subatomic particles and
the maximum number of electrons you can put in each orbital (ring).
Name ____________________ Date _______________ Period ________ # _____
Lewis Dot Structures
16. According to Mrs. Mohan, we use Lewis Dot Structures to represent the valence
electrons only. These are important because they are the electrons in the outermost
orbital/ring/shell that will do the reacting with other elements to form compounds.
17.
How do you figure out the number of valence electrons for Carbon?
Step 1: Determine the number of protons, electrons, and neutrons in the atom.
p+ =
no =
e- =
Step 2: Draw the correct Bohr model of the atom.
Step 3: Look at the outermost orbital/shell/ring and see how many electrons are located
in it. This is the number of valence electrons for that element.
18.
What is the easier way of doing this that Mrs. Mohan taught you?
19.
Try the following to see if you can use the short cut.
Lithium
Nitrogen
Calcium
Oxygen
Fluorine
1.
2.
3.
4.
5.
20.
Which elements will not react with anything because they have full outermost
orbitals/shells/rings?
21.
What element is the lone exception to the short cut? How many valence electrons
does it have?
22.
What is an isotope?
23.
Complete the following chart of isotopes for Carbon. (See p. 586.)
Type of Carbon
Number of protons Number of
Number of
isotope
neutrons
electrons
Carbon-12
Carbon-13
Carbon-14