Download IPS Unit 2 Worksheet Packet

1
IPS Unit 2 Worksheet Packet
STUDYING THE ATOM
Match the following picture or sentence with the scientist who discovered it:
D: Dalton
R: Rutherford
T: Thomson
B: Bohr
1.________________
2.______________ 3.______________ 4.________________
____ 5. Atoms are small, hard particles.
____ 6. Atoms of the same element are exactly alike.
____ 7. In an atom, electrons move in definite orbits around the nucleus, much like planets
circle the sun.
____ 8. An atom is the smallest piece of matter.
____ 9. An atom is mostly empty space with a dense, positively charged nucleus in the center.
____ 10. Atoms are indivisible.
____ 11. An atom has a small, positively charged nucleus surrounded by a large region in
which scientists can predict where an electron is likely to be found.
____ 12. An atom is made of positively charged, pudding like material through which
negatively charged particles are scattered.
____ 13. In an atom, electrons are located in energy levels that are a certain distance from the
nucleus.
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THE ATOMIC NUCLEUS
 After much observation and
questioning, Democritus concluded
that matter could not be divided into
smaller and smaller pieces forever.
Eventually the smallest possible
piece would be obtained.
 All elements are composed of atoms.
Atoms are indivisible and
indestructible particles.
 Atoms of the same element are
exactly alike.
 Atoms of different elements are
different.
 Compounds are formed by the
joining of atoms of two or more
elements.
 According to Thomson’s atomic
model, the atom was made of a
puddinglike positively charged
material throughout which
negatively charged electrons were
scattered, like plums in a pudding.



Rutherford reasoned that all of an
atom’s positively charged particles
were contained in the nucleus. The
negatively charged electrons were
scattered outside the nucleus around
the atom’s edge.
According to Bohr’s atomic model,
electrons move in definite orbits
around the nucleus, much like
planets circle the sun. These orbits,
or energy levels, are located at
certain distances from the nucleus.
According to the modern atomic
model, an atom has a small
positively charged nucleus
surrounded by a large region in
which there are enough electrons to
make the atom neutral.
Write five facts about the term nucleus, using the following words as clues.
1. Size
2. Location
3. Rutherford
4. Charge
5. Density
3
THE STRUCTURE OF AN ATOM
Using your periodic table, complete the following table.
Substance
Symbol
Helium
Bromine
Atomic
Number
Mass
Number
2
4
Mg
12
Zn
30
Br
Number of
Protons
65
80
35
13
U
Na
Ca
Silver
Ag
14
146
11
92
12
Kr
Calcium
Number of
Electrons
12
Aluminum
Sodium
Number of
Neutrons
48
40
20
47
61
36
4
Identify each element and choose whether the pair are isotopes to each other or different
elements.
Element Name
Isotope?
1. Element D has 6 protons and 7 neutrons
____________
____________
Element F has 7 prortons and 7 neutrons
2. Element J has 27 protons and 32 neutrons
____________
____________
____________
Element L has 27 prortons and 33 neutrons ____________
3. Element X has 17 protons and 18 neutrons ____________
____________
Element F has 18 prortons and 17 neutrons ____________
4. Element Q has 56 protons and 81 neutrons ____________
____________
Element R has 56 prortons and 82 neutrons ____________
5. Element T has an atomic number of 20 and
an atomic mass of 40.
____________
____________
Element Z has an atomic number of 20 and
an atomic mass of 41.
____________
6. Element W has 8 protons and 8 neutrons
____________
Element V has 7 prortons and 8 neutrons
____________
____________
7. Element P has an atomic number of 92 and
an atomic mass of 238.
____________
____________
Element S has 92 prortons and 143 neutrons ____________
Complete the following table.
Particle
Location
Proton
Electron
Neutron
Mass (amu)
Charge
5
Draw a model of the following atoms.
Li
C
B
He
Si
H
N
F
6
THE PERIODIC TABLE
Use different colored pencils to show each of the following items on the periodic table. Make a
key to indicate which color you are using for each item
group
period
metals
nonmetals
metalloids
The diagrams below show three squares from three different periodic tablse. On each diagram,
label the following items:
element name
mass number
chemical symbol
190
51
Sb
Antimony
122
Os
Osmium
76
atomic number
82
207
Lead
Pb
7
THE PERIODIC TABLE
Examine part of the periodic table shown below. Use this periodic table to answer the following
questions relating elements D, F, J, K, and R.
K
J
F
D
R
1. Which pair of elements has the same number of valence electrons?
2. Which pair of elements is in the same period?
3. Which pair of elements is in the same family?
4. Which element has the smallest atomic number?
5. Which elements would be classified as metals?
6. If the atomic number of Element D is 20, then what is the atomic number of element R?
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REPRESENTATIVE GROUPS
On the periodic table below, label each of the following:
actinoid series
alkali metals
alkaline earth metals
boron family
carbon family
halogen family
lantanoid series
nitrogen family
noble gases
oxygen family
rare-earth elements
transition metals
_______________________
IPS Unit 3 Worksheet Packet
Page 9
Using the periodic table, identify the elements described in the statements below.
1.
This element is in the same family as lead, and it has fewer protons than
sodium.
2.
This element has an atomic number that is one greater than platinum.
3.
This element has the most protons of any element in group 15.
4.
This element has more than 50 but less than 75 protons, and it is in group 17.
5.
This group 2 element has fewer protons than bromine, but more protons than
sulfur.
6.
This element has the lowest atomic number of any group 16 element.
7.
This element has an atomic number that is double the atomic number of
silicon.
8.
This element has more valence electrons, than oxygen, fewer valence
electrons than neon, more protons than sodium, but fewer protons than argon.
9.
This element has an atomic number lower than that of aluminum and one less
valence electron than the group 16 elements.
10.
This element is in group 1 and has a higher atomic number than chlorine, but a
lower atomic number than bromine.
IPS Unit 3 Worksheet Packet
Page 10
Draw the electron dot diagram for the following atoms
a. Hydrogen
f. Carbon
b. Helium
g. Nitrogen
c. Lithium
h. Oxygen
d. Beryllium
i. Fluorine
e. Boron
j. Neon
For the atoms above, predict whether they will gain electrons, lose electrons, or neither
gain nor lose electrons in a chemical reaction. Write “G” for gain, “L” for lose, and “N”
for neither.
a. ___
f. ___
b. ___
g. ___
c. ___
h. ___
d. ___
i. ___
e. ___
j. ___
IPS Unit 3 Worksheet Packet
Page 11
Draw both the electron dot diagrams for the following atoms and then draw the most
likely ion that these atoms will form. Make sure to show the charge for each ion and the
electrons if necessary.
a. Na
e. P
b. Mg
f. S
c. Al
g. Cl
d. Si
h. Ar
For the ions above, which are considered cations, and which are considered anions?
a. _____________
e. _____________
b. _____________
f. _____________
c. _____________
g. _____________
d. _____________
h. _____________
Name the ions above.
a. _____________
e. _____________
b. _____________
f. _____________
c. _____________
g. _____________
d. _____________
h. _____________
IPS Unit 3 Worksheet Packet
Page 12
Predict the ionic compound resulting between the following elements. Make sure to take
into account the charges on each ion and balance the charges with the correct number of
each ion.
a. Na and Cl
f. Li and N
b. Na and O
g. K and O
c. Mg and S
h. Ca and F
d. Ca and Br
i. Ba and N
e. Al and F
j. Sr and P
Name the above compounds:
a. ____________________
b. ____________________
c. ____________________
g. ____________________
h. ____________________
i. ____________________
d. ____________________
j. ____________________
e. ____________________
f. ____________________